Nitrogen has different oxidation states in the following compounds: nitrite ion, nitrous oxide, nitrate ion, ammonia, and nitrogen gas. Arrange these species in order of increasing nitrogen oxidation state. Select the correct answer below: A. ammonia, nitrogen gas, nitrite, nitrous oxide, nitrate B. nitrogen gas, ammonia, nitrous oxide, nitrite, nitrate C. ammonia, nitrogen gas, nitrous oxide, nitrite, nitrate D. ammonia, nitrogen gas, nitrate, nitrite, nitrous oxide

C. ammonia, nitrogen gas, nitrous oxide, nitrite, nitrate

Explanation:

To establish the oxidation number of nitrogen in each compound, we know that the sum of the oxidation numbers of the elements is equal to the charge of the species.

Nitrite ion (NO₂⁻)

1 × N + 2 × O = -1

1 × N + 2 × (-2) = -1

N = +3

Nitrous oxide (NO)

1 × N + 1 × O = 0

1 × N + 1 × (-2) = 0

N = +2

Nitrate ion (NO₃⁻)

1 × N + 3 × O = -1

1 × N + 3 × (-2) = -1

N = +5

Ammonia (NH₃)

1 × N + 3 × H = 0

1 × N + 3 × (+1) = 0

N = -3

Nitrogen gas (N₂)

2 × N = 0

N = 0

The order of increasing nitrogen oxidation state is:

C. ammonia, nitrogen gas, nitrous oxide, nitrite, nitrate

intermolecular forces are the forces between molecules or particles.

there are two kinds of van der waals forces: weak london dispersion forces and stronger dipole-dipole forces.

in molecule of water there are dipole-dipole forces between negatively charged oxygen from one molecule of water and positively charger hydrogen of another molecule of water.

hydrogen bond is an electrostatic attraction between two polar groups that occurs when a hydrogen atom (h), covalently bound to a highly electronegative atom such as flourine (f), oxygen (o) and nitrogen (n) atoms.