23 ccc energy and matter identify the dominant intermolecular force in ammonia (nh₃). given that ammonia is a gas at room temperature, what can you infer about the relative strengths of the intermolecular forces between ammonia molecules and between water molecules?

Question

Accepted Answer

# Explanation:
## Step1: Analyze NH₃'s structure
Ammonia ($NH_3$) has a trigonal pyramidal structure with a lone pair on nitrogen. Nitrogen is highly electronegative, so $NH_3$ is a polar molecule and can form hydrogen bonds (since $N - H$ bonds are present, and $N$ is electronegative enough to participate in H - bonding). So the dominant intermolecular force in $NH_3$ is hydrogen bonding.
## Step2: Compare with $H_2O$
Water ($H_2O$) is a liquid at room temperature, while $NH_3$ is a gas. The state of matter depends on intermolecular force strength: stronger forces hold molecules closer (liquid/solid), weaker forces allow more separation (gas). Since $NH_3$ is gas and $H_2O$ is liquid at room temp, intermolecular forces in $NH_3$ (hydrogen bonds) are weaker than in $H_2O$ (also hydrogen bonds, but $H_2O$ has two lone pairs on O and two H atoms, leading to more extensive H - bonding).
# Answer:
Dominant intermolecular force in $NH_3$: Hydrogen Bonding. Intermolecular forces in $NH_3$ are weaker than in $H_2O$ (since $NH_3$ is gas, $H_2O$ is liquid at room temp, so $H_2O$’s intermolecular forces (hydrogen bonds) are stronger).

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Question

Explanation:

Step1: Analyze NH₃'s structure

Step2: Compare with \(H_2O\)

Answer: