Magnesium in biology(Redirected from Dietary magnesium)
Magnesium is an essential element in biological systems. Magnesium occurs typically as the Mg2+ ion. It is an essential mineral nutrient (i.e., element) for life and is present in every cell type in every organism. For example, ATP (adenosine triphosphate), the main source of energy in cells, must bind to a magnesium ion in order to be biologically active. What is called ATP is often actually Mg-ATP. As such, magnesium plays a role in the stability of all polyphosphate compounds in the cells, including those associated with the synthesis of DNA and RNA.
Over 300 enzymes require the presence of magnesium ions for their catalytic action, including all enzymes utilizing or synthesizing ATP, or those that use other nucleotides to synthesize DNA and RNA. [cite needed]
A balance of magnesium is vital to the well-being of all organisms. Magnesium is a relatively abundant ion in Earth's crust and mantle and is highly bioavailable in the hydrosphere. This availability, in combination with a useful and very unusual chemistry, may have led to its utilization in evolution as an ion for signaling, enzyme activation, and catalysis. However, the unusual nature of ionic magnesium has also led to a major challenge in the use of the ion in biological systems. Biological membranes are impermeable to magnesium (and other ions), so transport proteins must facilitate the flow of magnesium, both into and out of cells and intracellular compartments.
Chlorophyll in plants converts water to oxygen as O2. Hemoglobin in vertebrate animals transports oxygen as O2 in the blood. Chlorophyll is very similar to hemoglobin, except magnesium is at the center of the chlorophyll molecule and iron is at the center of the hemoglobin molecule, with other variations. This process keeps living cells on earth alive and maintains baseline levels of CO2 and O2 in our atmosphere.
Inadequate magnesium intake frequently causes muscle spasms, and has been associated with cardiovascular disease, diabetes, high blood pressure, anxiety disorders, migraines, osteoporosis, and cerebral infarction. Acute deficiency (see hypomagnesemia) is rare, and is more common as a drug side-effect (such as chronic alcohol or diuretic use) than from low food intake per se, but it can occur in people fed intravenously for extended periods of time.
The most common symptom of excess oral magnesium intake is diarrhea. Supplements based on amino acid chelates (such as glycinate, lysinate etc.) are much better-tolerated by the digestive system and do not have the side-effects of the older compounds used, while sustained-release dietary supplements prevent the occurrence of diarrhea. Since the kidneys of adult humans excrete excess magnesium efficiently, oral magnesium poisoning in adults with normal renal function is very rare. Infants, which have less ability to excrete excess magnesium even when healthy, should not be given magnesium supplements, except under a physician's care.
Pharmaceutical preparations with magnesium are used to treat conditions including magnesium deficiency and hypomagnesemia, as well as eclampsia. Such preparations are usually in the form of magnesium sulfate or chloride when given parenterally. Magnesium is absorbed with reasonable efficiency (30% to 40%) by the body from any soluble magnesium salt, such as the chloride or citrate. Magnesium is similarly absorbed from Epsom salts, although the sulfate in these salts adds to their laxative effect at higher doses. Magnesium absorption from the insoluble oxide and hydroxide salts (milk of magnesia) is erratic and of poorer efficiency, since it depends on the neutralization and solution of the salt by the acid of the stomach, which may not be (and usually is not) complete.
Magnesium orotate may be used as adjuvant therapy in patients on optimal treatment for severe congestive heart failure, increasing survival rate and improving clinical symptoms and patient's quality of life.
Magnesium can affect muscle relaxation through direct action on cell membranes. Mg2+ ions close certain types of calcium channels, which conduct positively charged calcium ions into neurons. With an excess of magnesium, more channels will be blocked and nerve cells activity will decrease.
Intravenous magnesium sulphate is used in treating pre-eclampsia. For other than pregnancy-related hypertension, a meta-analysis of 22 clinical trials with dose ranges of 120 to 973 mg/day and a mean dose of 410 mg, concluded that magnesium supplementation had a small but statistically significant effect, lowering systolic blood pressure by 3–4 mm Hg and diastolic blood pressure by 2–3 mm Hg. The effect was larger when the dose was more than 370 mg/day.
Diabetes and glucose toleranceEdit
The U.S. Institute of Medicine (IOM) updated Estimated Average Requirements (EARs) and Recommended Dietary Allowances (RDAs) for magnesium in 1997. If there is not sufficient information to establish EARs and RDAs, an estimate designated Adequate Intake (AI) is used instead. The current EARs for magnesium for women and men ages 31 and up are 265 mg/day and 350 mg/day, respectively. The RDAs are 320 and 420 mg/day. RDAs are higher than EARs so as to identify amounts that will cover people with higher than average requirements. RDA for pregnancy is 350 to 400 mg/day depending on age of the woman. RDA for lactation ranges 310 to 360 mg/day for same reason. For children ages 1–13 years the RDA increases with age from 65 to 200 mg/day. As for safety, the IOM also sets Tolerable upper intake levels (ULs) for vitamins and minerals when evidence is sufficient. In the case of magnesium the UL is set at 350 mg/day. The UL is specific to magnesium consumed as a dietary supplement, the reason being that too much magnesium consumed at one time can cause diarrhea. The UL does not apply to food-sourced magnasium. Collectively the EARs, RDAs and ULs are referred to as Dietary Reference Intakes.
The European Food Safety Authority (EFSA) refers to the collective set of information as Dietary Reference Values, with Population Reference Intake (PRI) instead of RDA, and Average Requirement instead of EAR. AI and UL defined the same as in United States. For women and men ages 18 and older the AIs are set at 300 and 350 mg/day, respectively. AIs for pregnancy and lactation are also 300 mg/day. For children ages 1–17 years the AIs increase with age from 170 to 250 mg/day. These AIs are lower than the U.S. RDAs. The European Food Safety Authority reviewed the same safety question and set its UL at 250 mg/day - lower than the U.S. value. The magnesium UL is unique in that it is lower than some of the RDAs. It applies to intake from a pharmacological agent or dietary supplement only, and does not include intake from food and water.
For U.S. food and dietary supplement labeling purposes the amount in a serving is expressed as a percent of daily value (%DV). For magnesium labeling purposes 100% of the daily value was 400 mg, but as of May 27, 2016, it was revised to 420 mg to bring it into agreement with the RDA. A table of the old and new adult Daily Values is provided at Reference Daily Intake. Food and supplement companies have until January 1, 2020 to comply with the change.
Green vegetables such as spinach provide magnesium because of the abundance of chlorophyll molecules, which contain the ion. Nuts (especially Brazil nuts, cashews and almonds), seeds (e.g., pumpkin seeds), dark chocolate, roasted soybeans, bran, and some whole grains are also good sources of magnesium.
Although many foods contain magnesium, it is usually found in low levels. As with most nutrients, daily needs for magnesium are unlikely to be met by one serving of any single food. Eating a wide variety of fruits, vegetables, and grains will help ensure adequate intake of magnesium.
Because magnesium readily dissolves in water, refined foods, which are often processed or cooked in water and dried, in general, are poor sources of the nutrient. For example, whole-wheat bread has twice as much magnesium as white bread because the magnesium-rich germ and bran are removed when white flour is processed. The table of food sources of magnesium suggests many dietary sources of magnesium.
"Hard" water can also provide magnesium, but "soft" water contains less of the ion. Dietary surveys do not assess magnesium intake from water, which may lead to underestimating total magnesium intake and its variability.
Too much magnesium may make it difficult for the body to absorb calcium. Not enough magnesium can lead to hypomagnesemia as described above, with irregular heartbeats, high blood pressure (a sign in humans but not some experimental animals such as rodents), insomnia, and muscle spasms (fasciculation). However, as noted, symptoms of low magnesium from pure dietary deficiency are thought to be rarely encountered.
Following are some foods and the amount of magnesium in them:
- Pumpkin seeds, no hulls (1/4 cup) = 303 mg
- Chia seeds, (1/4 cup) = 162 mg
- Buckwheat flour (1/2 cup) = 151 mg
- Brazil nuts (1/4 cup) = 125 mg
- Oat bran, raw (1/2 cup) = 110 mg
- Cocoa powder (1/4 cup) = 107 mg
- Halibut (3 oz) = 103 mg
- Almonds (1/4 cup) = 99 mg
- Cashews (1/4 cup) = 89 mg
- Whole wheat flour (1/2 cup) = 83 mg
- Spinach, boiled (1/2 cup) = 79 mg
- Swiss Chard, boiled (1/2 cup) = 75 mg
- Chocolate, 70% cocoa (1 oz) = 73 mg
- Tofu, firm (1/2 cup) = 73 mg
- Black Beans, boiled (1/2 cup) = 60 mg
- Quinoa, cooked (1/2 cup) = 59 mg
- Peanut butter (2 tablespoons) = 50 mg
- Walnuts (1/4 cup) = 46 mg
- Sunflower seeds, hulled (1/4 cup) = 41 mg
- Chickpeas, boiled (1/2 cup) = 39 mg
- Kale, boiled (1/2 cup) = 37 mg
- Lentils, boiled (1/2 cup) = 36 mg
- Oatmeal, cooked (1/2 cup) = 32 mg
- Fish Sauce (1 Tbsp) = 32 mg
- Milk, non fat (1 cup) = 27 mg
- Coffee, espresso (1 oz) = 24 mg
- Whole wheat bread (1 slice) = 23 mg
Biological range, distribution, and regulationEdit
In animals, it has been shown that different cell types maintain different concentrations of magnesium. It seems likely that the same is true for plants. This suggests that different cell types may regulate influx and efflux of magnesium in different ways based on their unique metabolic needs. Interstitial and systemic concentrations of free magnesium must be delicately maintained by the combined processes of buffering (binding of ions to proteins and other molecules) and muffling (the transport of ions to storage or extracellular spaces).
In plants, and more recently in animals, magnesium has been recognized as an important signaling ion, both activating and mediating many biochemical reactions. The best example of this is perhaps the regulation of carbon fixation in chloroplasts in the Calvin cycle.
Magnesium is very important in cellular function. Deficiency of the nutrient causes disease of the affected organism. In single-cell organisms such as bacteria and yeast, low levels of magnesium manifests in greatly reduced growth rates. In magnesium transport knockout strains of bacteria, healthy rates are maintained only with exposure to very high external concentrations of the ion. In yeast, mitochondrial magnesium deficiency also leads to disease.
Plants deficient in magnesium show stress responses. The first observable signs of both magnesium starvation and overexposure in plants is a decrease in the rate of photosynthesis. This is due to the central position of the Mg2+ ion in the chlorophyll molecule. The later effects of magnesium deficiency on plants are a significant reduction in growth and reproductive viability. Magnesium can also be toxic to plants, although this is typically seen only in drought conditions.
In animals, magnesium deficiency (hypomagnesemia) is seen when the environmental availability of magnesium is low. In ruminant animals, particularly vulnerable to magnesium availability in pasture grasses, the condition is known as ‘grass tetany’. Hypomagnesemia is identified by a loss of balance due to muscle weakness. A number of genetically attributable hypomagnesemia disorders have also been identified in humans.
Overexposure to magnesium may be toxic to individual cells, though these effects have been difficult to show experimentally. Hypermagnesemia, an overabundance of magnesium in the blood, is usually caused by loss of kidney function. Healthy animals rapidly excrete excess magnesium in the urine and stool. Urinary magnesium is called magnesuria. Characteristic concentrations of magnesium in model organisms are: in E. coli 30-100mM (bound), 0.01-1mM (free), in budding yeast 50mM, in mammalian cell 10mM (bound), 0.5mM (free) and in blood plasma 1mM.
Mg2+ is the fourth-most-abundant metal ion in cells (per moles) and the most abundant free divalent cation — as a result, it is deeply and intrinsically woven into cellular metabolism. Indeed, Mg2+-dependent enzymes appear in virtually every metabolic pathway: Specific binding of Mg2+ to biological membranes is frequently observed, Mg2+ is also used as a signalling molecule, and much of nucleic acid biochemistry requires Mg2+, including all reactions that require release of energy from ATP. In nucleotides, the triple-phosphate moiety of the compound is invariably stabilized by association with Mg2+ in all enzymatic processes.
In photosynthetic organisms, Mg2+ has the additional vital role of being the coordinating ion in the chlorophyll molecule. This role was discovered by Richard Willstätter, who received the Nobel Prize in Chemistry 1915 for the purification and structure of chlorophyll.
The chemistry of the Mg2+ ion, as applied to enzymes, uses the full range of this ion’s unusual reaction chemistry to fulfill a range of functions. Mg2+ interacts with substrates, enzymes, and occasionally both (Mg2+ may form part of the active site). In general, Mg2+ interacts with substrates through inner sphere coordination, stabilising anions or reactive intermediates, also including binding to ATP and activating the molecule to nucleophilic attack. When interacting with enzymes and other proteins, Mg2+ may bind using inner or outer sphere coordination, to either alter the conformation of the enzyme or take part in the chemistry of the catalytic reaction. In either case, because Mg2+ is only rarely fully dehydrated during ligand binding, it may be a water molecule associated with the Mg2+ that is important rather than the ion itself. The Lewis acidity of Mg2+ (pKa 11.4) is used to allow both hydrolysis and condensation reactions (most common ones being phosphate ester hydrolysis and phosphoryl transfer) that would otherwise require pH values greatly removed from physiological values.
Essential role in the biological activity of ATPEdit
Nucleic acids have an important range of interactions with Mg2+. The binding of Mg2+ to DNA and RNA stabilises structure; this can be observed in the increased melting temperature (Tm) of double-stranded DNA in the presence of Mg2+. In addition, ribosomes contain large amounts of Mg2+ and the stabilisation provided is essential to the complexation of this ribo-protein. A large number of enzymes involved in the biochemistry of nucleic acids bind Mg2+ for activity, using the ion for both activation and catalysis. Finally, the autocatalysis of many ribozymes (enzymes containing only RNA) is Mg2+ dependent (e.g. the yeast mitochondrial group II self splicing introns).
Magnesium ions can be critical in maintaining the positional integrity of closely clustered phosphate groups. These clusters appear in numerous and distinct parts of the cell nucleus and cytoplasm. For instance, hexahydrated Mg2+ ions bind in the deep major groove and at the outer mouth of A-form nucleic acid duplexes.
Cell membranes and wallsEdit
Biological cell membranes and cell walls are polyanionic surfaces. This has important implications for the transport of ions, in particular because it has been shown that different membranes preferentially bind different ions. Both Mg2+ and Ca2+ regularly stabilize membranes by the cross-linking of carboxylated and phosphorylated head groups of lipids. However, the envelope membrane of E. coli has also been shown to bind Na+, K+, Mn2+ and Fe3+. The transport of ions is dependent on both the concentration gradient of the ion and the electric potential (ΔΨ) across the membrane, which will be affected by the charge on the membrane surface. For example, the specific binding of Mg2+ to the chloroplast envelope has been implicated in a loss of photosynthetic efficiency by the blockage of K+ uptake and the subsequent acidification of the chloroplast stroma.
The Mg2+ ion tends to bind only weakly to proteins (Ka ≤ 105) and this can be exploited by the cell to switch enzymatic activity on and off by changes in the local concentration of Mg2+. Although the concentration of free cytoplasmic Mg2+ is on the order of 1 mmol/L, the total Mg2+ content of animal cells is 30 mmol/L and in plants the content of leaf endodermal cells has been measured at values as high as 100 mmol/L (Stelzer et al., 1990), much of which buffered in storage compartments. The cytoplasmic concentration of free Mg2+ is buffered by binding to chelators (e.g., ATP), but also, what is more important, by storage of Mg2+ in intracellular compartments. The transport of Mg2+ between intracellular compartments may be a major part of regulating enzyme activity. The interaction of Mg2+ with proteins must also be considered for the transport of the ion across biological membranes.
In biological systems, only manganese (Mn2+) is readily capable of replacing Mg2+, but only in a limited set of circumstances. Mn2+ is very similar to Mg2+ in terms of its chemical properties, including inner and outer shell complexation. Mn2+ effectively binds ATP and allows hydrolysis of the energy molecule by most ATPases. Mn2+ can also replace Mg2+ as the activating ion for a number of Mg2+-dependent enzymes, although some enzyme activity is usually lost. Sometimes such enzyme metal preferences vary among closely related species: For example, the reverse transcriptase enzyme of lentiviruses like HIV, SIV and FIV is typically dependent on Mg2+, whereas the analogous enzyme for other retroviruses prefers Mn2+.
Importance in drug bindingEdit
An article investigating the structural basis of interactions between clinically relevant antibiotics and the 50S ribosome appeared in Nature in October 2001. High-resolution X-ray crystallography established that these antibiotics associate only with the 23S rRNA of a ribosomal subunit, and no interactions are formed with a subunit's protein portion. The article stresses that the results show "the importance of putative Mg2+ ions for the binding of some drugs".
Measuring magnesium in biological samplesEdit
By radioactive isotopesEdit
The use of radioactive tracer elements in ion uptake assays allows the calculation of km, Ki and Vmax and determines the initial change in the ion content of the cells. 28Mg decays by the emission of a high-energy beta or gamma particle, which can be measured using a scintillation counter. However, the radioactive half-life of 28Mg, the most stable of the radioactive magnesium isotopes, is only 21 hours. This severely restricts the experiments involving the nuclide. Also, since 1990, no facility has routinely produced 28Mg, and the price per mCi is now predicted to be approximately US$30,000. The chemical nature of Mg2+ is such that it is closely approximated by few other cations. However, Co2+, Mn2+ and Ni2+ have been used successfully to mimic the properties of Mg2+ in some enzyme reactions, and radioactive forms of these elements have been employed successfully in cation transport studies. The difficulty of using metal ion replacement in the study of enzyme function is that the relationship between the enzyme activities with the replacement ion compared to the original is very difficult to ascertain.
By fluorescent indicatorsEdit
A number of chelators of divalent cations have different fluorescence spectra in the bound and unbound states. Chelators for Ca2+ are well established, have high affinity for the cation, and low interference from other ions. Mg2+ chelators lag behind and the major fluorescence dye for Mg2+ (mag-fura 2) actually has a higher affinity for Ca2+. This limits the application of this dye to cell types where the resting level of Ca2+ is < 1 μM and does not vary with the experimental conditions under which Mg2+ is to be measured. Recently, Otten et al. (2001) have described work into a new class of compounds that may prove more useful, having significantly better binding affinities for Mg2+. The use of the fluorescent dyes is limited to measuring the free Mg2+. If the ion concentration is buffered by the cell by chelation or removal to subcellular compartments, the measured rate of uptake will give only minimum values of km and Vmax.
First, ion-specific microelectrodes can be used to measure the internal free ion concentration of cells and organelles. The major advantages are that readings can be made from cells over relatively long periods of time, and that unlike dyes very little extra ion buffering capacity is added to the cells.
Second, the technique of two-electrode voltage-clamp allows the direct measurement of the ion flux across the membrane of a cell. The membrane is held at an electric potential and the responding current is measured. All ions passing across the membrane contribute to the measured current.
Third, the technique of patch-clamp uses isolated sections of natural or artificial membrane in much the same manner as voltage-clamp but without the secondary effects of a cellular system. Under ideal conditions the conductance of individual channels can be quantified. This methodology gives the most direct measurement of the action of ion channels.
By absorption spectroscopyEdit
Flame atomic absorption spectroscopy (AAS) determines the total magnesium content of a biological sample. This method is destructive; biological samples must be broken down in concentrated acids to avoid clogging the fine nebulising apparatus. Beyond this, the only limitation is that samples must be in a volume of approximately 2 mL and at a concentration range of 0.1 – 0.4 µmol/L for optimum accuracy. As this technique cannot distinguish between Mg2+ already present in the cell and that taken up during the experiment, only content not uptaken can be quantified.
Inductively coupled plasma (ICP) using either the mass spectrometry (MS) or atomic emission spectroscopy (AES) modifications also allows the determination of the total ion content of biological samples. These techniques are more sensitive than flame AAS and are capable of measuring the quantities of multiple ions simultaneously. However, they are also significantly more expensive.
The chemical and biochemical properties of Mg2+ present the cellular system with a significant challenge when transporting the ion across biological membranes. The dogma of ion transport states that the transporter recognises the ion then progressively removes the water of hydration, removing most or all of the water at a selective pore before releasing the ion on the far side of the membrane. Due to the properties of Mg2+, large volume change from hydrated to bare ion, high energy of hydration and very low rate of ligand exchange in the inner coordination sphere, these steps are probably more difficult than for most other ions. To date, only the ZntA protein of Paramecium has been shown to be a Mg2+ channel. The mechanisms of Mg2+ transport by the remaining proteins are beginning to be uncovered with the first three-dimensional structure of a Mg2+ transport complex being solved in 2004.
The hydration shell of the Mg2+ ion has a very tightly bound inner shell of six water molecules and a relatively tightly bound second shell containing 12–14 water molecules (Markham et al., 2002). Thus, it is presumed that recognition of the Mg2+ ion requires some mechanism to interact initially with the hydration shell of Mg2+, followed by a direct recognition/binding of the ion to the protein. Due to the strength of the inner sphere complexation between Mg2+ and any ligand, multiple simultaneous interactions with the transport protein at this level might significantly retard the ion in the transport pore. Hence, it is possible that much of the hydration water is retained during transport, allowing the weaker (but still specific) outer sphere coordination.
In spite of the mechanistic difficulty, Mg2+ must be transported across membranes, and a large number of Mg2+ fluxes across membranes from a variety of systems have been described. However, only a small selection of Mg2+ transporters have been characterised at the molecular level.
Ligand ion channel blockadeEdit
Magnesium ions (Mg2+) in cellular biology are usually in almost all senses opposite to Ca2+ ions, because they are bivalent too, but have greater electronegativity and thus exert greater pull on water molecules, preventing passage through the channel (even though the magnesium itself is smaller). Thus, Mg2+ ions block Ca2+ channels such as (NMDA channels) and have been shown to affect gap junction channels forming electrical synapses.
Plant physiology of magnesiumEdit
The previous sections have dealt in detail with the chemical and biochemical aspects of Mg2+ and its transport across cellular membranes. This section will apply this knowledge to aspects of whole plant physiology, in an attempt to show how these processes interact with the larger and more complex environment of the multicellular organism.
Nutritional requirements and interactionsEdit
Mg2+ is essential for plant growth and is present in higher plants in amounts on the order of 80 μmol g−1 dry weight. The amounts of Mg2+ vary in different parts of the plant and are dependent upon nutritional status. In times of plenty, excess Mg2+ may be stored in vascular cells (Stelzer et al., 1990; and in times of starvation Mg2+ is redistributed, in many plants, from older to newer leaves.
Mg2+ is taken up into plants via the roots. Interactions with other cations in the rhizosphere can have a significant effect on the uptake of the ion.(Kurvits and Kirkby, 1980; The structure of root cell walls is highly permeable to water and ions, and hence ion uptake into root cells can occur anywhere from the root hairs to cells located almost in the centre of the root (limited only by the Casparian strip). Plant cell walls and membranes carry a great number of negative charges, and the interactions of cations with these charges is key to the uptake of cations by root cells allowing a local concentrating effect. Mg2+ binds relatively weakly to these charges, and can be displaced by other cations, impeding uptake and causing deficiency in the plant.
Within individual plant cells, the Mg2+ requirements are largely the same as for all cellular life; Mg2+ is used to stabilise membranes, is vital to the utilisation of ATP, is extensively involved in the nucleic acid biochemistry, and is a cofactor for many enzymes (including the ribosome). Also, Mg2+ is the coordinating ion in the chlorophyll molecule. It is the intracellular compartmentalisation of Mg2+ in plant cells that leads to additional complexity. Four compartments within the plant cell have reported interactions with Mg2+. Initially, Mg2+ will enter the cell into the cytoplasm (by an as yet unidentified system), but free Mg2+ concentrations in this compartment are tightly regulated at relatively low levels (≈2 mmol/L) and so any excess Mg2+ is either quickly exported or stored in the second intracellular compartment, the vacuole. The requirement for Mg2+ in mitochondria has been demonstrated in yeast and it seems highly likely that the same will apply in plants. The chloroplasts also require significant amounts of internal Mg2+, and low concentrations of cytoplasmic Mg2+. In addition, it seems likely that the other subcellular organelles (e.g., Golgi, endoplasmic reticulum, etc.) also require Mg2+.
Distributing magnesium ions within the plantEdit
Once in the cytoplasmic space of root cells Mg2+, along with the other cations, is probably transported radially into the stele and the vascular tissue. From the cells surrounding the xylem the ions are released or pumped into the xylem and carried up through the plant. In the case of Mg2+, which is highly mobile in both the xylem and phloem, the ions will be transported to the top of the plant and back down again in a continuous cycle of replenishment. Hence, uptake and release from vascular cells is probably a key part of whole plant Mg2+ homeostasis. Figure 1 shows how few processes have been connected to their molecular mechanisms (only vacuolar uptake has been associated with a transport protein, AtMHX).
The diagram shows a schematic of a plant and the putative processes of Mg2+ transport at the root and leaf where Mg2+ is loaded and unloaded from the vascular tissues. Mg2+ is taken up into the root cell wall space (1) and interacts with the negative charges associated with the cell walls and membranes. Mg2+ may be taken up into cells immediately (symplastic pathway) or may travel as far as the Casparian band (4) before being absorbed into cells (apoplastic pathway; 2). The concentration of Mg2+ in the root cells is probably buffered by storage in root cell vacuoles (3). Note that cells in the root tip do not contain vacuoles. Once in the root cell cytoplasm, Mg2+ travels toward the centre of the root by plasmodesmata, where it is loaded into the xylem (5) for transport to the upper parts of the plant. When the Mg2+ reaches the leaves it is unloaded from the xylem into cells (6) and again is buffered in vacuoles (7). Whether cycling of Mg2+ into the phloem occurs via general cells in the leaf (8) or directly from xylem to phloem via transfer cells (9) is unknown. Mg2+ may return to the roots in the phloem sap.
When a Mg2+ ion has been absorbed by a cell requiring it for metabolic processes, it is generally assumed that the ion stays in that cell for as long as the cell is active. In vascular cells, this is not always the case; in times of plenty, Mg2+ is stored in the vacuole, takes no part in the day-to-day metabolic processes of the cell (Stelzer et al., 1990), and is released at need. But for most cells it is death by senescence or injury that releases Mg2+ and many of the other ionic constituents, recycling them into healthy parts of the plant. In addition, when Mg2+ in the environment is limiting, some species are able to mobilise Mg2+ from older tissues. These processes involve the release of Mg2+ from its bound and stored states and its transport back into the vascular tissue, where it can be distributed to the rest of the plant. In times of growth and development, Mg2+ is also remobilised within the plant as source and sink relationships change.
The homeostasis of Mg2+ within single plant cells is maintained by processes occurring at the plasma membrane and at the vacuole membrane (see Figure 2). The major driving force for the translocation of ions in plant cells is ΔpH. H+-ATPases pump H+ ions against their concentration gradient to maintain the pH differential that can be used for the transport of other ions and molecules. H+ ions are pumped out of the cytoplasm into the extracellular space or into the vacuole. The entry of Mg2+ into cells may occur through one of two pathways, via channels using the ΔΨ (negative inside) across this membrane or by symport with H+ ions. To transport the Mg2+ ion into the vacuole requires a Mg2+/H+ antiport transporter (such as AtMHX). The H+-ATPases are dependent on Mg2+ (bound to ATP) for activity, so that Mg2+ is required to maintain its own homeostasis.
A schematic of a plant cell is shown including the four major compartments currently recognised as interacting with Mg2+. H+-ATPases maintain a constant ΔpH across the plasma membrane and the vacuole membrane. Mg2+ is transported into the vacuole using the energy of ΔpH (in A. thaliana by AtMHX). Transport of Mg2+ into cells may use either the negative ΔΨ or the ΔpH. The transport of Mg2+ into mitochondria probably uses ΔΨ as in the mitochondria of yeast, and it is likely that chloroplasts take Mg2+ by a similar system. The mechanism and the molecular basis for the release of Mg2+ from vacuoles and from the cell is not known. Likewise, the light-regulated Mg2+ concentration changes in chloroplasts are not fully understood, but do require the transport of H+ ions across the thylakoid membrane.
Magnesium, chloroplasts and photosynthesisEdit
Mg2+ is the coordinating metal ion in the chlorophyll molecule, and in plants where the ion is in high supply about 6% of the total Mg2+ is bound to chlorophyll. Thylakoid stacking is stabilised by Mg2+ and is important for the efficiency of photosynthesis, allowing phase transitions to occur.
Mg2+ is probably taken up into chloroplasts to the greatest extent during the light-induced development from proplastid to chloroplast or etioplast to chloroplast. At these times, the synthesis of chlorophyll and the biogenesis of the thylakoid membrane stacks absolutely require the divalent cation.
Whether Mg2+ is able to move into and out of chloroplasts after this initial developmental phase has been the subject of several conflicting reports. Deshaies et al. (1984) found that Mg2+ did move in and out of isolated chloroplasts from young pea plants, but Gupta and Berkowitz (1989) were unable to reproduce the result using older spinach chloroplasts. Deshaies et al. had stated in their paper that older pea chloroplasts showed less significant changes in Mg2+ content than those used to form their conclusions. The relative proportion of immature chloroplasts present in the preparations may explain these observations.
The metabolic state of the chloroplast changes considerably between night and day. During the day, the chloroplast is actively harvesting the energy of light and converting it into chemical energy. The activation of the metabolic pathways involved comes from the changes in the chemical nature of the stroma on the addition of light. H+ is pumped out of the stroma (into both the cytoplasm and the lumen) leading to an alkaline pH. Mg2+ (along with K+) is released from the lumen into the stroma, in an electroneutralisation process to balance the flow of H+. Finally, thiol groups on enzymes are reduced by a change in the redox state of the stroma. Examples of enzymes activated in response to these changes are fructose 1,6-bisphosphatase, sedoheptulose bisphosphatase and ribulose-1,5-bisphosphate carboxylase. During the dark period, if these enzymes were active a wasteful cycling of products and substrates would occur.
Two major classes of the enzymes that interact with Mg2+ in the stroma during the light phase can be identified. Firstly, enzymes in the glycolytic pathway most often interact with two atoms of Mg2+. The first atom is as an allosteric modulator of the enzymes’ activity, while the second forms part of the active site and is directly involved in the catalytic reaction. The second class of enzymes includes those where the Mg2+ is complexed to nucleotide di- and tri-phosphates (ADP and ATP), and the chemical change involves phosphoryl transfer. Mg2+ may also serve in a structural maintenance role in these enzymes (e.g., enolase).
Plant stress responses can be observed in plants that are under- or over-supplied with Mg2+. The first observable signs of Mg2+ stress in plants for both starvation and toxicity is a depression of the rate of photosynthesis, it is presumed because of the strong relationships between Mg2+ and chloroplasts/chlorophyll. In pine trees, even before the visible appearance of yellowing and necrotic spots, the photosynthetic efficiency of the needles drops markedly. In Mg2+ deficiency, reported secondary effects include carbohydrate immobility, loss of RNA transcription and loss of protein synthesis. However, due to the mobility of Mg2+ within the plant, the deficiency phenotype may be present only in the older parts of the plant. For example, in Pinus radiata starved of Mg2+, one of the earliest identifying signs is the chlorosis in the needles on the lower branches of the tree. This is because Mg2+ has been recovered from these tissues and moved to growing (green) needles higher in the tree.
A Mg2+ deficit can be caused by the lack of the ion in the media (soil), but more commonly comes from inhibition of its uptake. Mg2+ binds quite weakly to the negatively charged groups in the root cell walls, so that excesses of other cations such as K+, NH4+, Ca2+, and Mn2+ can all impede uptake.(Kurvits and Kirkby, 1980; In acid soils Al3+ is a particularly strong inhibitor of Mg2+ uptake. The inhibition by Al3+ and Mn2+ is more severe than can be explained by simple displacement, hence it is possible that these ions bind to the Mg2+ uptake system directly. In bacteria and yeast, such binding by Mn2+ has already been observed. Stress responses in the plant develop as cellular processes halt due to a lack of Mg2+ (e.g. maintenance of ΔpH across the plasma and vacuole membranes). In Mg2+-starved plants under low light conditions, the percentage of Mg2+ bound to chlorophyll has been recorded at 50%. Presumably, this imbalance has detrimental effects on other cellular processes.
Mg2+ toxicity stress is more difficult to develop. When Mg2+ is plentiful, in general the plants take up the ion and store it (Stelzer et al., 1990). However, if this is followed by drought then ionic concentrations within the cell can increase dramatically. High cytoplasmic Mg2+ concentrations block a K+ channel in the inner envelope membrane of the chloroplast, in turn inhibiting the removal of H+ ions from the chloroplast stroma. This leads to an acidification of the stroma that inactivates key enzymes in carbon fixation, which all leads to the production of oxygen free radicals in the chloroplast that then cause oxidative damage.
- "Magnesium (In Biological Systems)". Van Nostrand's Scientific Encyclopedia. 2006. doi:10.1002/0471743984.vse4741.
- Leroy, J. (1926). "Necessite du magnesium pour la croissance de la souris". Comptes Rendus des Séances de la Société de Biologie. 94: 431–433.
- Lusk, J.E.; Williams, R.J.P.; Kennedy, E.P. (1968). "Magnesium and the growth of Escherichia coli". Journal of Biological Chemistry. 243 (10): 2618–2624. PMID 4968384.
- Marschner, H. (1995). Mineral Nutrition in Higher Plants. San Diego: Academic Press. ISBN 0-12-473542-8.
- "Definition: magnesium from Online Medical Dictionary". Archive.org. 25 December 2007. Retrieved 17 January 2018.
- Granick S, Evolution of Heme and Chlorophyll in book, Bryson V, HJ Vogel, ed., Evolving Genes and Proteins. Academic Press, NY and London, 1965, pp. 67-88.
- Romani, Andrea, M.P. (2013). "Chapter 3. Magnesium in Health and Disease". In Astrid Sigel; Helmut Sigel; Roland K. O. Sigel. Interrelations between Essential Metal Ions and Human Diseases. Metal Ions in Life Sciences. 13. Springer. pp. 49–79. doi:10.1007/978-94-007-7500-8_3.
- Larsson S. C.; Virtanen M. J.; Mars M.; et al. (March 2008). "Magnesium, calcium, potassium, and sodium intakes and risk of stroke in male smokers". Arch. Intern. Med. 168 (5): 459–65. doi:10.1001/archinte.168.5.459. PMID 18332289.
- Euser, A. G.; Cipolla, M. J. (2009). "Magnesium Sulfate for the Treatment of Eclampsia: A Brief Review". Stroke. 40 (4): 1169–1175. doi:10.1161/STROKEAHA.108.527788. PMC . PMID 19211496.
- Stepura OB, Martynow AI (February 2008). "Magnesium orotate in severe congestive heart failure (MACH)". Int. J. Cardiol. 131 (2): 293–5. doi:10.1016/j.ijcard.2007.11.022. PMID 18281113.
- Slutsky, I.; Sadeghpour, S.; Li, B.; Liu, G. (2004). "Enhancement of Synaptic Plasticity through Chronically Reduced Ca2+ Flux during Uncorrelated Activity". Neuron. 44 (5): 835–49. doi:10.1016/j.neuron.2004.11.013. PMID 15572114.Full Text
- Slutsky, I.; Abumaria, N.; Wu, L. J.; Huang, C.; Zhang, L.; Li, B.; Zhao, X.; Govindarajan, A.; Zhao, M. G.; Zhuo, M.; Tonegawa, S.; Liu, G. (2010). "Enhancement of Learning and Memory by Elevating Brain Magnesium". Neuron. 65 (2): 165–77. doi:10.1016/j.neuron.2009.12.026. PMID 20152124.Full Text
- Duley L, Gülmezoglu AM, Henderson-Smart DJ, Chou D (2010). "Magnesium sulphate and other anticonvulsants for women with pre-eclampsia". Cochrane Database Syst Rev (11): CD000025. doi:10.1002/14651858.CD000025.pub2. PMID 21069663.
- Kass L, Weekes J, Carpenter L (2012). "Effect of magnesium supplementation on blood pressure: a meta-analysis". Eur J Clin Nutr. 66 (4): 411–8. doi:10.1038/ejcn.2012.4. PMID 22318649.
- Fang X, Han H, Li M, Liang C, Fan Z, Aaseth J, He J, Montgomery S, Cao Y (2016). "Dose-Response Relationship between Dietary Magnesium Intake and Risk of Type 2 Diabetes Mellitus: A Systematic Review and Meta-Regression Analysis of Prospective Cohort Studies". Nutrients. 8 (11). doi:10.3390/nu8110739. PMC . PMID 27869762.
- Veronese N, Watutantrige-Fernando S, Luchini C, Solmi M, Sartore G, Sergi G, Manzato E, Barbagallo M, Maggi S, Stubbs B (2016). "Effect of magnesium supplementation on glucose metabolism in people with or at risk of diabetes: a systematic review and meta-analysis of double-blind randomized controlled trials". Eur J Clin Nutr. 70 (12): 1354–1359. doi:10.1038/ejcn.2016.154. PMID 27530471.
- "Magnesium", pp.190-249 in "Dietary Reference Intakes for Calcium, Phosphorus, Magnesium, Vitamin D, and Fluoride". National Academy Press. 1997.
- "Overview on Dietary Reference Values for the EU population as derived by the EFSA Panel on Dietetic Products, Nutrition and Allergies" (PDF). 2017.
- Tolerable Upper Intake Levels For Vitamins And Minerals (PDF), European Food Safety Authority, 2006
- "Federal Register May 27, 2016 Food Labeling: Revision of the Nutrition and Supplement Facts Labels. FR page 33982" (PDF).
- Nutrition, Center for Food Safety and Applied. "Labeling & Nutrition - Changes to the Nutrition Facts Label". www.FDA.gov. Retrieved 17 January 2018.
- "Top 10 Foods Highest in Magnesium + Printable One Page Sheet". HealthAliciousNess. Retrieved 17 January 2018.
- Valberg, L. S.; Holt, J.M.; Paulson, E.; Szivek, J. (1965). "Spectrochemical Analysis of Sodium, Potassium, Calcium, Magnesium, Copper, and Zinc in Normal Human Erythrocytes". Journal of Clinical Investigation. 44 (3): 379–389. doi:10.1172/JCI105151. PMC . PMID 14271298.
- Seiler, R. H.; Ramirez, O.; Brest, A. N.; Moyer, J. H. (1966). "Serum and erythrocytic magnesium levels in congestive heart failure: effect of hydrochlorothiazide". American Journal of Cardiology. 17 (6): 786–791. doi:10.1016/0002-9149(66)90372-9.
- Walser, M. (1967). "Magnesium metabolism". Ergebnisse der Physiologie Biologischen Chemie und Experimentellen Pharmakologie. 59: 185–296. doi:10.1007/BF02269144.
- Iyengar, G.V.; Kollmer, W. E.; Bowen, H. J. M. (1978). The Elemental Composition of Human Tissues and Body Fluids. Weinheim, New York: Verlag Chemie. ISBN 0-89573-003-0.
- Stelzer, R.; Lehmann, H.; Krammer, D.; Luttge, U. (1990). "X-Ray microprobe analysis of vacuoles of spruce needle mesophyll, endodermis and transfusion parenchyma cells at different seasons of the year". Botanica Acta. 103: 415–423. doi:10.1111/j.1438-8677.1990.tb00183.x.
- Shaul, O.; Hilgemann, D. W.; de-Almeida-Engler, J.; Van, M.M.; Inze, D.; Galili, G. (1999). "Cloning and characterization of a novel Mg(2+)/H(+) exchanger". EMBO Journal. 18 (14): 3973–3980. doi:10.1093/emboj/18.14.3973. PMC . PMID 10406802.
- Thomas, R.C.; Coles, J. A.; Deitmer, J. W. (1991). "Homeostatic muffling". Nature. 350 (6319): 564. doi:10.1038/350564b0. PMID 2017256.
- Berkowitz, G. A.; Wu, W. (1993). "Magnesium, potassium flux and photosynthesis". Magnesium Research. 6 (3): 257–265. PMID 8292500.
- Shaul, O. (2002). "Magnesium transport and function in plants: the tip of the iceberg". BioMetals. 15 (3): 309–323. doi:10.1023/A:1016091118585. PMID 12206396.
- Hmiel, S. P.; Snavely, M. D.; Florer, J. B.; Maguire, M. E.; Miller, C. G. (1989). "Magnesium transport in Salmonella typhimurium: genetic characterization and cloning of three magnesium transport loci". Journal of Bacteriology. 171 (9): 4742–4751. PMC . PMID 2548998.
- MacDiarmid, C.W.; Gardner, R. C. (1998). "Overexpression of the Saccharomyces cerevisiae magnesium transport system confers resistance to aluminum ion". J. Biol. Chem. 273 (3): 1727–1732. doi:10.1074/jbc.273.3.1727. PMID 9430719.
- Wiesenberger, G.; Waldherr, M.; Schweyen, R. J. (1992). "The nuclear gene MRS2 is essential for the excision of group II introns from yeast mitochondrial transcripts in vivo". J. Biol. Chem. 267 (10): 6963–6969. PMID 1551905.
- Kaiser, W. M. (1987). "Effects of water deficit on photosynthetic capacity". Physiologia Plantarum. 71: 142–149. doi:10.1111/j.1399-3054.1987.tb04631.x.
- Rao, I. M.; Sharp, R. E.; Boyer, J.S. (1987). "Leaf Phosphate Status, Photosynthesis, and Carbon Partitioning in Sugar Beet: III. Diurnal Changes in Carbon Partitioning and Carbon Export". Plant Physiology. 92 (1): 29–36. doi:10.1104/pp.92.1.29. PMC . PMID 16667261.
- Grunes, D. L.; Stout, P. R.; Brownwell, J.R. (1970). "Grass tetany of ruminants". Advances in Agronomy. Advances in Agronomy. 22: 332–374. doi:10.1016/S0065-2113(08)60272-2. ISBN 978-0-12-000722-6.
- Paunier, L.; Radde, I. C.; Kooh, S.W.; Conen, P.E.; Fraser, D. (1968). "Primary hypomagnesemia with secondary hypocalcemia in an infant". Pediatrics. 41 (2): 385–402. PMID 5637791.
- Weber S, Hoffmann K, Jeck N, Saar K, Boeswald M, Kuwertz-Broeking E, Meij II, Knoers NV, Cochat P, Suláková T, Bonzel KE, Soergel M, Manz F, Schaerer K, Seyberth HW, Reis A, Konrad M (2000). "Familial hypomagnesaemia with hypercalciuria and nephrocalcinosis maps to chromosome 3q27 and is associated with mutations in the PCLN-1 gene". European Journal of Human Genetics. 8 (6): 414–422. doi:10.1038/sj.ejhg.5200475. PMID 10878661.
- Weber S, Schneider L, Peters M, Misselwitz J, Rönnefarth G, Böswald M, Bonzel KE, Seeman T, Suláková T, Kuwertz-Bröking E, Gregoric A, Palcoux JB, Tasic V, Manz F, Schärer K, Seyberth HW, Konrad M (2001). "Novel paracellin-1 mutations in 25 families with familial hypomagnesemia with hypercalciuria and nephrocalcinosis". Journal of the American Society of Nephrology. 12 (9): 1872–1881. PMID 11518780.
- Chubanov V, Waldegger S, Mederos y Schnitzler M, Vitzthum H, Sassen MC, Seyberth HW, Konrad M, Gudermann T (2004). "Disruption of TRPM6/TRPM7 complex formation by a mutation in the TRPM6 gene causes hypomagnesemia with secondary hypocalcemia". Proceedings of the National Academy of Sciences of the United States of America. 101 (9): 2894–2899. doi:10.1073/pnas.0305252101. PMC . PMID 14976260.
- Harrison’s Principles of Internal Medicine, Online Edition
- Milo, Ron; Philips, Rob. "Cell Biology by the Numbers: What are the concentrations of different ions in cells?". book.bionumbers.org. Retrieved 23 March 2017.
- Cowan, J. A. (1995). J.A. Cowan, ed. Introduction to the biological chemistry of magnesium. The Biological Chemistry of Magnesium. New York: VCH.
- Romani, A. M. P.; Maguire, M. E. (2002). "Hormonal regulation of Mg2+ transport and homeostasis in eukaryotic cells". BioMetals. 15 (3): 271–283. doi:10.1023/A:1016082900838. PMID 12206393.
- Black, C. B.; Cowan, J.A. (1995). J.A. Cowan, ed. "Magnesium-dependent enzymes in nucleic acid biochemistry". The Biological Chemistry of Magnesium. New York: VCH.
- Black, C.B.; Cowan, J. A. (1995). J.A. Cowan, ed. "Magnesium-dependent enzymes in general metabolism". The Biological Chemistry of Magnesium. New York: VCH.
- Cowan, J. A. (2002). "Structural and catalytic chemistry of magnesium-dependent enzymes". BioMetals. 15 (3): 225–235. doi:10.1023/A:1016022730880. PMID 12206389.
- Sperazza, J. M.; Spremulli, L. L. (1983). "Quantitation of cation binding to wheat germ ribosomes: influences on subunit association equilibria and ribosome activity". Nucleic Acids Research. 11 (9): 2665–2679. doi:10.1093/nar/11.9.2665. PMC . PMID 6856472.
- Smith, R. L.; Thompson, L.J.; Maguire, M. E. (1995). "Cloning and characterization of MgtE, a putative new class of Mg2+ transporter from Bacillus firmus OF4". Journal of Bacteriology. 177 (5): 1233–1238. PMC . PMID 7868596.
- Robinson, Howard; Gao, Yi-Gui; Sanishvili, Ruslan; Joachimiak, Andrzej; Wang, Andrew H.-J. (15 April 2000). "Hexahydrated magnesium ions bind in the deep major groove and at the outer mouth of A-form nucleic acid duplexes". Nucleic Acids Research. 28 (8): 1760–1766. doi:10.1093/nar/28.8.1760. Retrieved 17 January 2018 – via nar.OxfordJournals.org.
- Ebel, H.; Gunther, T. (1980). "Magnesium metabolism: a review". Journal of Clinical Chemistry and Clinical Biochemistry. 18: 257–270. doi:10.1515/cclm.19188.8.131.527.
- Schlünzen, Frank; Zarivach, Raz; Harms, Jörg; Bashan, Anat; Tocilj, Ante; Albrecht, Renate; Yonath, Ada; Franceschi, François (2001). "Structural basis for the interaction of antibiotics with the peptidyl transferase centre in eubacteria". Nature. 413 (6858): 814–21. doi:10.1038/35101544. PMID 11677599.
- Maguire, M.E.; Cowan, J. A. (2002). "Magnesium chemistry and biochemistry". BioMetals. 15 (3): 203–210. doi:10.1023/A:1016058229972. PMID 12206387.
- Tevelev, A.; Cowan, J. A. (1995). J.A. Cowan, ed. Metal substitution as a probe of the biological chemistry of magnesium ion. The Biological Chemistry of Magnesium. New York: VCH.
- Drakenberg, T. (1995). J. A. Cowan, ed. Physical methods for studying the biological chemistry of magnesium. The Biological Chemistry of Magnesium. New York: VCH.
- Raju, B.; Murphy, E.; Levy, L. A.; Hall, R. D.; London, R. E. (1989). "A fluorescent indicator for measuring cytosolic free magnesium". Am J Physiol Cell Physiol. 256: C540–548.
- Grubbs, R. D. (2002). "Intracellular magnesium and magnesium buffering". BioMetals. 15 (3): 251–259. doi:10.1023/A:1016026831789. PMID 12206391.
- Otten, P.A.; London, R.E.; Levy, L. A. (2001). "4-Oxo-4H-quinolizine-3-carboxylic acids as Mg2+ selective, fluorescent indicators". Bioconjugate Chemistry. 12 (2): 203–212. doi:10.1021/bc000087d. PMID 11312681.
- Gunzel, D.; Schlue, W.-R. (2002). "Determination of [Mg2+]i - an update on the use of Mg2+-selective electrodes". BioMetals. 15 (3): 237–249. doi:10.1023/A:1016074714951. PMID 12206390.
- Hille, B. (1992). "2". Ionic channels of excitable membranes. Sunderland: Sinauer Associates Inc. ISBN 0-87893-322-0.
- See Chapters 5 and 6 in Dean, J.R. (1997). Atomic Absorption and Plasma Spectroscopy. Chichester: John Wiley & Sons. ISBN 0-471-97255-X. for descriptions of the methodology as applied to analytical chemistry.
- Hille, 1992. Chapter 11
- Haynes, W. J.; Kung, C.; Saimi, Y.; Preston, R. R. (2002). "An exchanger-like protein underlies the large Mg2+ current in Paramecium". PNAS. 99 (24): 15717–15722. doi:10.1073/pnas.242603999. PMC . PMID 12422021.
- Warren, M. A.; Kucharski, L. M.; Veenstra, A.; Shi, L.; Grulich, P. F.; Maguire, M. E. (2004). "The CorA Mg2+ Transporter Is a Homotetramer". Journal of Bacteriology. 186 (14): 4605–4612. doi:10.1128/JB.186.14.4605-4612.2004. PMC . PMID 15231793.
- Gardner, R. C. (2003). "Genes for magnesium transport". Current Opinion in Plant Biology. 6 (3): 263–267. doi:10.1016/S1369-5266(03)00032-3. PMID 12753976.
- Laing, W.; Greer, D.; Sun, O.; Beets, P.; Lowe, A.; Payn, T. (2000). "Physiological impacts of Mg deficiency in Pinus radiata: growth and photosynthesis". New Phytol. 146: 47–57. doi:10.1046/j.1469-8137.2000.00616.x.
- Heenan, D.P.; Campbell, L.C. (1981). "Influence of potassium and manganese on growth and uptake of magnesium by soybeans (Glycine max (L.) Merr. cv Bragg". Plant Soil. 61 (3): 447–456. doi:10.1007/BF02182025.
- Hope, A. B.; Stevens, P. G. (1952). "Electrical potential differences in bean roots on their relation to salt uptake". Australian Journal of Scientific Research, Series B. 5: 335–343.
- Section 8.5.2 in Marschner, 1995
- Bui, D.M.; Gregan, J.; Jarosch, E.; Ragnini, A.; Schweyen, R. J. (1999). "The bacterial magnesium transporter CorA can functionally substitute for its putative homologue Mrs2p in the yeast inner mitochondrial membrane". Journal of Biological Chemistry. 274 (29): 20438–20443. doi:10.1074/jbc.274.29.20438. PMID 10400670.
- Demmig, B.; Gimmler, H. (1979). "Effect of divalent cations on cation fluxes across the chloroplast envelope and on photosynthesis of intact chloroplasts". Zeitschrift für Naturforschung. 24C: 233–241.
- Huber, S.C.; Maury, W. J. (1980). "Effects of Magnesium on Intact Chloroplasts: I. EVIDENCE FOR ACTIVATION OF (SODIUM) POTASSIUM/PROTON EXCHANGE ACROSS THE CHLOROPLAST ENVELOPE". Plant Physiology. 65 (2): 350–354. doi:10.1104/pp.65.2.350. PMC . PMID 16661188.
- Section 2.7 in Marschner, 1995
- Section 3.3 in Marschner, 1995
- Section 2.4 in Marschner, 1995
- Scott, B. J.; Robson, A. D. (1990). "Distribution of magnesium in subterranean clover (Trifolium subterranean L.) in relation to supply". Australian Journal of Agricultural Research. 41 (3): 499–510. doi:10.1071/AR9900499.
- Scott, B. J.; Robson, A. D. (1990b). "Changes in the content and form of magnesium in the first trifoliate leaf of subterranean clover under altered or constant root supply". Australian Journal of Agricultural Research. 41 (3): 511–519. doi:10.1071/AR9900511.
- Fork, D.C. (1986). "The control by state transitions of the distribution of excitation energy in photosynthesis". Annual Review of Plant Physiology and Plant Molecular Biology. 37: 335–361. doi:10.1146/annurev.arplant.37.1.335.
- Gregory, R. P. F. (1989). Structure and function of the photosynthesising cell. Biochemistry of Photosynthesis. New York: John Wiley and Sons.
- Lu YK, Chen YR, Yang CM, Ifuku K (1995). "Influence of Fe- and Mg-deficiency on the thylakoid membranes of a chlorophyll-deficient ch5 mutant of Arabidopsis thaliana". Botanical Bulletin of Academia Sinica. 36.
- Deshaies, R. J.; Fish, L. E.; Jagendorf, A. T. (1984). "Permeability of Chloroplast Envelopes to Mg2+: Effects on Protein Synthesis". Plant Physiology. 74 (4): 956–961. doi:10.1104/pp.74.4.956. PMC . PMID 16663541.
- Gupta, A. S.; Berkowitz, G. A. (1989). "Development and Use of Chlorotetracycline Fluorescence as a Measurement Assay of Chloroplast Envelope-Bound Mg2+". Plant Physiology. 89 (3): 753–761. doi:10.1104/pp.89.3.753. PMC . PMID 16666617.
- Heldt, H.W.; Werdan, K.; Milovancev, M.; Geller, G. (1973). "Alkalization of the chloroplast stroma caused by light-dependent proton flux into the thylakoid space". Biochimica et Biophysica Acta. 314 (2): 224–241. doi:10.1016/0005-2728(73)90137-0. PMID 4747067.
- Hind, G.; Nakatani, H. Y.; Izawa, S. (1974). "Light-Dependent Redistribution of Ions in Suspensions of Chloroplast Thylakoid Membranes". Proceedings of the National Academy of Sciences of the United States of America. 71 (4): 1484–1488. doi:10.1073/pnas.71.4.1484. PMC . PMID 4524652.
- Bulychev, A. A.; Vredenberg, W. J. (1976). "Effect of ionophores A-23187 and nigericin on the light induced redistribution of magnesium potassium and hydrogen ions across the thylakoid membrane". Biochimica et Biophysica Acta. 449 (1): 48–58. doi:10.1016/0005-2728(76)90006-2. PMID 10009.
- Krause, G. H. (1977). "Light-induced movement of magnesium ions in intact chloroplasts. Spectroscopic determination with Eriochrome Blue SE". Biochimica et Biophysica Acta. 460 (3): 500–510. doi:10.1016/0005-2728(77)90088-3. PMID 880298.
- Portis, A. R. (1981). "Evidence of a Low Stromal Mg2+ Concentration in Intact Chloroplasts in the Dark: I. STUDIES WITH THE IONOPHORE A23187". Plant Physiology. 67 (5): 985–989. doi:10.1104/pp.67.5.985. PMC . PMID 16661806.
- Ishijima, S.; Uchibori, A.; Takagi, H.; Maki, R.; Ohnishi, M. (2003). "Light-induced increase in free Mg2+ concentration in spinach chloroplasts: Measurement of free Mg2+ by using a fluorescent probe and intensity of stromal alkalinization". Archives of Biochemistry and Biophysics. 412 (1): 126–132. doi:10.1016/S0003-9861(03)00038-9. PMID 12646275.
- Sharkey, T. D. (1998). A. Raghavendra, ed. "Photosynthetic carbon reduction". Photosynthesis: A Comprehensive Treatise. Cambridge: Cambridge University Press: 111–122.
- Section 8.5.6 of Marschner, 1995
- Rengel, Z.; Robinson, D. L. (1989). "Competitive Al3+ Inhibition of Net Mg2+ Uptake by Intact Lolium multiflorum Roots : I. Kinetics". Plant Physiology. 91 (4): 1407–1413. doi:10.1104/pp.91.4.1407. PMC . PMID 16667193.
- Marschner, H. (1991). Y. Waisel; A. Eshel; U. Kafikfai, eds. Root-induced changes in the availability of micronutrients in the rhizosphere. Plant Roots: The Hidden Half. New York: Marcel Dekker.
- Dorenstouter, H.; Pieters, G.A.; Findenegg, G. R. (1985). "Distribution of magnesium between chloroplhyll and other photosynthetic functions in magnesium deficient 'sun' and 'shade' leaves of poplar". Journal of Plant Nutrition. 8 (12): 1088–1101. doi:10.1080/01904168509363409.
- Wu, W.; Peters, J.; Berkowitz, G.A. (1991). "Surface Charge-Mediated Effects of Mg2+ on K+ Flux across the Chloroplast Envelope Are Associated with Regulation of Stromal pH and Photosynthesis". Plant Physiology. 97 (2): 580–587. doi:10.1104/pp.97.2.580. PMC . PMID 16668438.
- Romani, Andrea M.P. (2013). "Chapter 4 Magnesium Homeostasis in Mammalian Cells". In Banci, Lucia (Ed.). Metallomics and the Cell. Metal Ions in Life Sciences. 12. Springer. doi:10.1007/978-94-007-5561-l_4. ISBN 978-94-007-5560-4. electronic-book ISBN 978-94-007-5561-1 ISSN 1559-0836 electronic-ISSN 1868-0402
- Findling, R. L.; Maxwell, K; Scotese-Wojtila, L; Huang, J; Yamashita, T; Wiznitzer, M (1997). "High-dose pyridoxine and magnesium administration in children with autistic disorder: an absence of salutary effects in a double-blind, placebo-controlled study". J Autism Dev Disord. 27 (4): 467–478. doi:10.1023/A:1025861522935. PMID 9261669.
- Green, V.; Pituch, K.; Itchon, J.; Choi, A.; O'Reilly, M.; Sigafoos, J. (2006). "Internet Survey of Treatments Used by Parents of Children with Autism". Research in Developmental Disabilities. 27 (1): 70–84. doi:10.1016/j.ridd.2004.12.002. PMID 15919178.
- Lelord, G.; Muh, JP; Barthelemy, C; Martineau, J; Garreau, B; Callaway, E (1981). "Effects of pyridoxine and magnesium on autistic symptoms--initial observations". J Autism Dev Disord. 11 (2): 219–230. doi:10.1007/BF01531686. PMID 6765503.
- Martineau, J.; et al. (1985). "Vitamin B6, magnesium, and combined B6-Mg: therapeutic effects in childhood autism." Biol". Psychiatry. 20 (5): 467–478. doi:10.1016/0006-3223(85)90019-8.
- Tolbert, L.; Haigler, T; Waits, MM; Dennis, T (1993). "Brief report: lack of response in an autistic population to a low dose clinical trial of pyridoxine plus magnesium". J Autism Dev Disord. 23 (1): 193–199. doi:10.1007/BF01066428. PMID 8463199.
- Mousain-Bosc M, Roche M, Polge A, Pradal-Prat D, Rapin J, Bali JP (Mar 2006). "Improvement of neurobehavioral disorders in children supplemented with magnesium-vitamin B6. I. Attention deficit hyperactivity disorders". Magnes. Res. 19 (1): 46–52. PMID 16846100.
- Mousain-Bosc M, Roche M, Polge A, Pradal-Prat D, Rapin J, Bali JP (Mar 2006). "Improvement of neurobehavioral disorders in children supplemented with magnesium-vitamin B6. II. Pervasive developmental disorder-autism". Magnes. Res. 19 (1): 53–62. PMID 16846101.
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- Magnesium Deficiency
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- The Magnesium Website- Includes full text papers and textbook chapters by leading magnesium authorities Mildred Seelig, Jean Durlach, Burton M. Altura and Bella T. Altura. Links to over 300 articles discussing magnesium and magnesium deficiency.
- Dietary Reference Intake
- Healing Thresholds - description of research studies regarding supplementation with magnesium and other therapies for autism