Write the chemical formula for iridium(III) nitride?

Answer: The correct selection is (b).

Explanation:

The energy required to detach an electron from an atom or ion in its gaseous state is termed ionization energy.

This indicates that a smaller atom necessitates a greater amount of energy to remove its valence electron. The reason for this is that there exists a strong attraction between the nucleus and the electrons in smaller atoms or elements.

Therefore, a significant amount of energy is needed to dislodge the valence electrons.

The electronic configuration for helium is . Hence, due to its fully occupied valence shell, it exhibits greater stability.

Consequently, a large amount of energy is needed to remove an electron from a helium atom.

In conclusion, from the choices provided, the ionization energy of helium will be greater than that of the diatomic molecule.

Answer:

1219.5 kJ/mol

Explanation:

The calculation for this value requires using the following equation:

ΔHºrxn = Σn * (BE of reactants) - Σn * (BE of products)

ΔHºrxn = [1 * (BE C = C) + 2 * (BE C-H) + 5/2 * (BE O = O)] - [4 * (BE C = O) + 2 * (BE O-H)].

The bond energy (BE) values are:

BE C = C: 839 kJ/mol

BE C-H: 413 kJ/mol

BE O = O: 495 kJ/mol

BE C = O: 799 kJ/mol

BE O-H: 463 kJ/mol

By substituting these values into the equation, you will get:

ΔHºrxn = [1 * 839 + 2 * (413) + 5/2 * (495)] - [4 * (799) + 2 * (463)] = 1219.5 kJ/mol