Phosphorus Mass Number

Exact Mass: 30.973762 g/mol: Computed by PubChem 2.1 (PubChem release 2019.06.18) Monoisotopic Mass: 30.973762 g/mol: Computed by PubChem 2.1 (PubChem release 2019.06.18) Topological Polar Surface Area: 0 Å²: Computed by Cactvs 3.4.6.11 (PubChem release 2019.06.18) Heavy Atom Count: 1: Computed by PubChem: Formal Charge: 0: Computed by PubChem: Complexity: 0. Phosphorus is a chemical element with an atomic number of 15, which means that the atomic structure includes 15 protons and 15 electrons. For Phosphorus, the chemical symbol is P. Atomic Mass of Phosphorus The atomic mass of phosphorus is 30.973762 u. The mass number of phosphorus is 31. This means that there are a total of 31 protons and neutrons in the nucleus of the most common isotope of. See full answer below.

Mass Number Of Phosphorus 31
What Is Phosphorus Mass Number
Phosphorus Atomic Mass And Number

Chemical properties of phosphorus - Health effects of phosphorus - Environmental effects of phosphorus

Atomic number	15
Atomic mass	30,9738 g.mol^-1
Oxidation states	± 3, 4, 5
Electronegativity according to Pauling	2,1
Density	1,82 g/ml at 20°C
Melting point	44,2 °C
Boiling point	280 °C
Vanderwaals radius	1,04 Å
Ionic radius	0,34 Å
Atomic radius	1,28 Å
Electronic shell	[Ne]3s23p3
Energy of first ionisation	10,118 eV
Energy of second ionisation	19,725 eV
Energy of third ionisation	29,141 eV
Discovered by	Hennig Brandt in 1669

Properties

Phosphorous is a multivalent nonmetal of the nitrogen group. It is found in nature in several allotropic forms, and is an essential element for the life of organisms.

There are several forms of phosphorous, called white, red and black phosphorous, although the their colours are more likely to be slightly different. White phosphorous is the one manufactured industrial; it glows in the dark, is spontaneously flammable when exposed to air and is deadly poison. Red phosphorous can vary in colour from orange to purple, due to slight variations in its chemical structure. The third form, black phosphorous, is made under high pressure, looks like graphite and, like graphite, has the ability to conduct electricity.

Applications

Concentrated phosphoric acids are used in fertilizers for agriculture and farm production. Phosphates are used for special glasses, sodium lamps, in steel production, in military applications (incendiary bombs, smoke screenings etc.), and in other applications as: pyrotechnics, pesticides, toothpaste, detergents.

Phosphorous in the environment

In the natural world phosphorous is never encountered in its pure form, but only as phosphates, which consists of a phosphorous atom bonded to four oxygen atoms. This can exists as the negatively charged phosphate ion (PO₄^3-), which is how it occurs in minerals, or as organophosphates in which there are organic molecules attached to one, two or three of the oxygen atoms.

The amount of phosphorous that is naturally present in food varies considerably but can be as high as 370 mg/100 g in liver, or can be low, as in vegetable oils. Foods rich in phosphorous include tuna, salmon, sardines, liver, turkey, chicken, eggs and cheese (200 g/100 g).

There are many phosphate minerals, the most abundant being forms of apatite. Fluoroapatite provides the most extensively mined deposits. The chief mining areas are Russia, USA, Morocco, Tunisia, Togo and Nauru. World production is 153 million tones per year. There are concerns over how long these phosphorous deposits will last. In case of depletion there could be a serious problem for the worlds food production since phosphorus is such an essential ingredient in fertilizers.

In the oceans, the concentration of phosphates is very low, particularly at the surface. The reason lies partly within the insolubility of aluminum and calcium phosphates, but in any case in the oceans phosphate is quickly used up and falls into the deep as organic debris. There can be more phosphate in rivers and lakes, resulting in excessive algae growth. For further details go to environmental effects of phosphorous.

Health effects of phosphorus

Phosphorus can be found in the environment most commonly as phosphates. Phosphates are important substances in the human body, because they are a part of DNA materials and they take part in energy distribution. Phosphates can also be found commonly in plants.
Phosphate is a dietary requirement, the recommended intake is 800 mg/day, a normal diet provides between 1000 and 2000 mg/day, depending on the extent to which phosphate rich foods are consumed.

Humans have changed the natural phosphate supply radically by addition of phosphate-rich manures to the soil and by the use of phosphate-containing detergents. Phosphates were also added to a number of foodstuffs, such as cheese, sausages and hams.
Too much phosphate can cause health problems, such as kidney damage and osteoporosis. Phosphate shortages can also occur. These are caused by extensive use of medicine. Too little phosphate can cause health problems.
Phosphorus in its pure form has a white colour. White phosphorus is the most dangerous form of phosphorus that is known to us. When white phosphorus occurs in nature this can be a serious danger to our health. White phosphorus is extremely poisonous and in many cases exposure to it will be fatal.
In most cases people that died of white phosphorus exposure had been accidentally swallowing rat poison. Before people die from white phosphorus exposure they often experience nausea, stomach cramps and drowsiness.
White phosphorus can cause skin burns. While burning, white phosphorus may cause damage to the liver, the heart or the kidneys.

Environmental effects of phosphorus

White phosphorus
White phosphorus enters the environment when industries use it to make other chemicals and when the army uses it as ammunition. Through discharge of wastewater white phosphorus ends up in surface waters near the factories that use it.
White phosphorus is not likely to spread, because it reacts with oxygen fairly quickly. When phosphorus ends up in air through exhausts it will usually react with oxygen right away to be converted into less harmful particles. However, when phosphorus particles are in air they may have a protective coating that prevents chemical reactions.
In water, white phosphorus is not reacting with other particles that quickly and as a result it will accumulate in the bodies of aquatic organisms. In soil phosphorus will remain for several days before it is converted into less harmful substances. But in deep soils and the bottom of rivers and lakes phosphorus may remain for a thousand years or so.
Phosphates
Phosphates have many effects upon organisms. The effects are mainly consequences of emissions of large quantities of phosphate into the environment due to mining and cultivating. During water purification phosphates are often not removed properly, so that they can spread over large distances when found in surface waters.
Due to the constant addition of phosphates by humans and the exceeding of the natural concentrations, the phosphor cycle is strongly disrupted.
The increasing phosphor concentrations in surface waters raise the growth of phosphate-dependent organisms, such as algae and duckweed. These organisms use great amounts of oxygen and prevent sunlight from entering the water. This makes the water fairly unliveable for other organisms. This phenomenon is commonly known as eutrophication.

Back to the periodic table of elements.

For more information on phosphorus' place in the environment, move to the phosphorus cycle.

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››Convert moles Phosphorus to gram

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How many moles Phosphorus in 1 grams?The answer is 0.03228539149637.
We assume you are converting between moles Phosphorus and gram.
You can view more details on each measurement unit:
molecular weight of Phosphorus orgrams
The molecular formula for Phosphorus is P.
The SI base unit for amount of substance is the mole.
1 mole is equal to 1 moles Phosphorus, or 30.973761 grams.
Note that rounding errors may occur, so always check the results.
Use this page to learn how to convert between moles Phosphorus and gram.
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››Quick conversion chart of moles Phosphorus to grams

1 moles Phosphorus to grams = 30.97376 grams

2 moles Phosphorus to grams = 61.94752 grams

3 moles Phosphorus to grams = 92.92128 grams

4 moles Phosphorus to grams = 123.89504 grams

5 moles Phosphorus to grams = 154.86881 grams

6 moles Phosphorus to grams = 185.84257 grams

7 moles Phosphorus to grams = 216.81633 grams

8 moles Phosphorus to grams = 247.79009 grams

Mass Number Of Phosphorus 31

9 moles Phosphorus to grams = 278.76385 grams

10 moles Phosphorus to grams = 309.73761 grams

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moles Phosphorus to picomol
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››Details on molecular weight calculations

In chemistry, the formula weight is a quantity computed by multiplying the atomic weight (in atomic mass units) of each element in a chemical formula by the number of atoms of that element present in the formula, then adding all of these products together.

What Is Phosphorus Mass Number

Using the chemical formula of the compound and the periodic table of elements, we can add up the atomic weights and calculate molecular weight of the substance.

A common request on this site is to convert grams to moles. To complete this calculation, you have to know what substance you are trying to convert. The reason is that the molar mass of the substance affects the conversion. This site explains how to find molar mass.

The atomic weights used on this site come from NIST, the National Institute of Standards and Technology. We use the most common isotopes. This is how to calculate molar mass (average molecular weight), which is based on isotropically weighted averages. This is not the same as molecular mass, which is the mass of a single molecule of well-defined isotopes. For bulk stoichiometric calculations, we are usually determining molar mass, which may also be called standard atomic weight or average atomic mass.

Phosphorus Atomic Mass And Number

If the formula used in calculating molar mass is the molecular formula, the formula weight computed is the molecular weight. The percentage by weight of any atom or group of atoms in a compound can be computed by dividing the total weight of the atom (or group of atoms) in the formula by the formula weight and multiplying by 100.

Formula weights are especially useful in determining the relative weights of reagents and products in a chemical reaction. These relative weights computed from the chemical equation are sometimes called equation weights.

Finding molar mass starts with units of grams per mole (g/mol). When calculating molecular weight of a chemical compound, it tells us how many grams are in one mole of that substance. The formula weight is simply the weight in atomic mass units of all the atoms in a given formula.

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