Question

Fill in the blanks:

1. The H−O−H bond angle in H₂O is ______ the H−C−H bond angle in CH₄.
2. The O−S−O bond angle in SO₂ is ______ the F−B−F bond angle in BF₃. the F−B−F bond angle in BF₃.
3. The F−S−F bond angle in SF₆ is greater thanThe F−S−F bond angle in SF₆ is _____ the F−Br−F bond angle in BrF₅.

Answer 1

The H-O-H bond angle in H₂O is smaller than the H-C-H bond angle in CH₄ due to the presence of lone pairs. The O-S-O bond angle in SO₂ is greater than the F-B-F bond angle in BF₃ due to the presence of a lone pair. The F-S-F bond angle in SF₆ is greater than the F-Br-F bond angle in BrF₅ due to the increased electronegativity of fluorine atoms.

Step-by-step explanation:

The H-O-H bond angle in H₂O is smaller than the H-C-H bond angle in CH₄. This is because the oxygen atom in water is sp³ hybridized, which means it has two lone pairs and two bonding pairs of electrons. The presence of lone pairs in the water molecule causes the bonding pairs to be pushed closer together, resulting in a smaller bond angle.

The O-S-O bond angle in SO₂ is greater than the F-B-F bond angle in BF₃. This is because sulfur in SO₂ is sp² hybridized, which means it has one lone pair and two bonding pairs of electrons. The presence of a lone pair in the sulfur atom causes the bonding pairs to spread out more, resulting in a larger bond angle.

The F-S-F bond angle in SF₆ is greater than the F-Br-F bond angle in BrF₅. This is because the fluorine atoms in SF₆ are more electronegative than the bromine atoms in BrF₅. The increased electronegativity of the fluorine atoms pulls the bonding pairs closer together, resulting in a larger bond angle.

Answer 2

1. smaller. 2. smaller. 3. greater

Step-by-step explanation:

1. H−O−H angle is 104.45 and H−C−H angle is 109.5

2. O−S−O angle is 119 and F−B−F angle is 120

3. The F−S−F bond angle in SF₆ is 90 and F−Br−F bond angle in BrF₅ is 84.8