Question

1. list these diatomic molecular compounds in order of weakest (1) to strongest (3) bonds: _n₂ _cl₂ _o₂ 21. describe the differences between ionic bonds, metallic bonds, and covalent bonds. be specific.

Explanation:

Question 20

Step1: Consider bond orders

Bond order is related to bond strength. For \(N_2\), the bond order is \(3\) (using molecular orbital theory, \(\sigma_{2s}^2\sigma_{2s}^*2\sigma_{2p}^2\pi_{2p}^4\), bond order \(=\frac{1}{2}(8 - 2)=3\)). For \(O_2\), the bond order is \(2\) (\(\sigma_{2s}^2\sigma_{2s}^*2\sigma_{2p}^2\pi_{2p}^4\pi_{2p}^*2\), bond order \(=\frac{1}{2}(8 - 4)=2\)). For \(Cl_2\), it has a single covalent bond (bond order \( = 1\)) as it is formed by sharing one pair of electrons (\(Cl - Cl\)).

• Ionic bonds: Formed by the transfer of electrons from a metal to a non - metal. There is a strong electrostatic attraction between cations (positive ions) and anions (negative ions). For example, in \(NaCl\), \(Na\) donates an electron to \(Cl\).
• Metallic bonds: Occur in metals. The electrons are delocalized (not associated with a single atom). The metal cations are surrounded by a “sea of electrons”. This allows metals to conduct electricity (mobile electrons) and be malleable (layers of cations can slide over each other).
• Covalent bonds: Formed by the sharing of electrons between non - metals. Can be polar (unequal sharing, e.g., \(H - Cl\)) or non - polar (equal sharing, e.g., \(H - H\)).

Answer:

\(Cl_2\) (1), \(O_2\) (2), \(N_2\) (3)

Question 21