Question

which of the following bonds would be the most polar based on the given en values?
n-h
o-h
c-o
c-h
what is the lewis diagram for sodium chloride?
na :cl:
na+ :cl:-
na+ cl-
na+ :cl:
b
a
c
d

Explanation:

First Question (Most Polar Bond)

Step1: Recall Electronegativity Difference

Polarity of a bond depends on the electronegativity (EN) difference between atoms. Larger EN difference → more polar.

Step2: Analyze Each Bond

• N - H: EN of N ≈ 3.0, H ≈ 2.1 → Difference = \( 3.0 - 2.1 = 0.9 \)
• O - H: EN of O ≈ 3.5, H ≈ 2.1 → Difference = \( 3.5 - 2.1 = 1.4 \)
• C - O: EN of C ≈ 2.5, O ≈ 3.5 → Difference = \( 3.5 - 2.5 = 1.0 \)
• C - H: EN of C ≈ 2.5, H ≈ 2.1 → Difference = \( 2.5 - 2.1 = 0.4 \)

Step3: Compare Differences

The largest difference is for O - H (1.4), so it's the most polar.

Sodium chloride (NaCl) is an ionic compound. Na loses an electron to form \( \text{Na}^+ \), Cl gains an electron to form \( \text{Cl}^- \) (with 8 valence electrons, shown as \( [: \ddot{\text{Cl}} :]^- \)). The Lewis diagram should show the cation \( \text{Na}^+ \) and anion \( [: \ddot{\text{Cl}} :]^- \) with proper charge notation. Option d has \( [\text{Na}^+] [: \ddot{\text{Cl}} :]^- \) (correct charge on Na⁺ and Cl⁻ with Cl's octet). Option b has incorrect Na notation (should be \( \text{Na}^+ \), not \( \text{Na}^* \)), option a has Na (not ion), option c has [Cl]⁻ (incorrect Lewis structure for Cl⁻).

Answer:

O-H

Second Question (Lewis Diagram for NaCl)