Question

Write the chemical properties of hydrogen with following

i. Nitrogen

ii. Metallic Oxide

iii. Molten Sulphur​

Answer 1

Answer:

Nitrogen:

• The seventh element of the periodic table between carbon and oxygen is Nitrogen.
• It’s an important part of amino acids.
• Around eighty percent of the Earth’s atmosphere comprises nitrogen gas.
• It has no colour, mostly diatomic non metal gas along with odourless and colourless in nature.
• Since it has five electrons in its outer shell, most of its compounds are trivalent.
• It is a constituent of all living tissues. Since it is a component of DNA and part of a genetic code, it is an essential element of life.
• It is found in nitrates and nitrites in soil and water.

Metallic Oxide:

• Metal oxides are crystalline solids that contain a metal cation and an oxide anion.
• They typically react with water to form bases or with acids to form salts.
• The alkali metals and alkaline earth metals form three different types of binary oxygen compounds:

1. Oxides, containing oxide ions, O²-,

2. Peroxides, containing peroxide ions, O²²−, which contain oxygen-oxygen covalent single bonds, and

3. Superoxides, containing superoxide ions, O²−, which also have oxygen-oxygen covalent bonds but with one fewer negative charge than peroxide ions.

Alkali metals (which have a +1 oxidation state) form oxides, M²O, peroxides, M²O², and superoxides, MO². (M represents a metal atom.)

• The alkaline earth metals (with a +2 oxidation state) form only oxides, MO, and peroxides, MO².
• All the alkali metal oxides can be prepared by heating the corresponding metal nitrate with the elemental metal.

2MNO³ + 10M + heat → 6M²O + N2

• A general preparation of the alkaline earth oxides involves heating the metal carbonates.

Molten Sulphur:

• Sulfur burns with a blue flame, concomitant with formation of sulfur dioxide, notable for its peculiar suffocating odor.
• Sulfur is insoluble in water but soluble in carbon disulfide and, to a lesser extent, in other nonpolar organic solvents, such as benzene and toluene.
• The first and the second ionization energies of sulfur are 999.6 and 2252 kJ/mol, respectively.
• Despite such figures, S2+ is rare, with S+4 and S6+ being more common.
• The fourth and sixth ionization energies are 4556 and 8495.8 kJ/mol.
• The magnitude of the figures is caused by electron transfer between orbitals; these states are only stable with strong oxidants such as fluorine, oxygen, and chlorine.