Question

use your previous drawing the answer the following questions. click all that apply.
(a) in hydrogen solid (below 14k), what types of bonds and interactions are present?
(b) in hydrogen gas (at room temperature), what types of bonds and interactions are present?
(c) if hydrogen is heated above 6000k, what types of bonds and interactions are present?

Explanation:

• (a) In hydrogen solid (at 14K), hydrogen molecules are closely packed. Covalent bonds exist within hydrogen molecules ($H - H$). Since it is a solid, London dispersion forces (weak intermolecular forces between non - polar molecules) are also present.
• (b) In hydrogen gas at room temperature, hydrogen exists as $H_2$ molecules. Covalent bonds are present within the $H_2$ molecules. There are no strong intermolecular forces like hydrogen bonds (as hydrogen is bonded to itself, not a highly electronegative atom like $O$, $N$, or $F$ in a way to form hydrogen bonds) and no ionic bonds (it is a non - ionic compound). London dispersion forces are very weak but still present between the gas molecules.
• (c) When hydrogen is heated above 6000K, it dissociates into hydrogen atoms. So, there are no bonds (covalent, ionic, hydrogen) or intermolecular forces (London dispersion forces require the presence of molecules).

Answer:

(a) Covalent bonds, London dispersion forces
(b) Covalent bonds, London dispersion forces
(c) none