Question

Explain the X-S-X bond angles for the series of compounds SF₄, SCl₄, and SBr₄.

a) SF₄: 109.5°, SCl₄: <109.5°, SBr₄: >109.5°
b) SF₄: <109.5°, SCl₄: 109.5°, SBr₄: >109.5°
c) SF₄: >109.5°, SCl₄: <109.5°, SBr₄: 109.5°
d) SF₄: >109.5°, SCl₄: >109.5°, SBr₄: >109.5°

Answer 1

Answer: The X-S-X bond angles for the series of compounds SF₄, SCl₄, and SBr₄ are as follows:

- SF₄: 109.5°

- SCl₄: &lt;109.5°

- SBr₄: &gt;109.5°

Step-by-step explanation:

In SF₄, the molecule adopts a tetrahedral geometry with a central sulfur atom bonded to four fluorine atoms. The bond angles between the sulfur atom and the fluorine atoms are all equal and measure approximately 109.5°. This is due to the repulsion between the electron pairs in the sulfur atom's valence shell, which results in the arrangement of the fluorine atoms as far apart from each other as possible.

In SCl₄, the molecule also adopts a tetrahedral geometry with a central sulfur atom bonded to four chlorine atoms. However, the bond angles in SCl₄ are less than 109.5°. This is because chlorine is larger than fluorine, resulting in increased repulsion between the electron pairs in the sulfur atom's valence shell and a compression of the bond angles.

In SBr₄, the molecule adopts a distorted tetrahedral geometry with a central sulfur atom bonded to four bromine atoms. The bond angles in SBr₄ are greater than 109.5°. This is because bromine is larger than fluorine, resulting in decreased repulsion between the electron pairs in the sulfur atom's valence shell and an expansion of the bond angles.

To summarize:

- SF₄: 109.5° - Tetrahedral geometry, all bond angles equal

- SCl₄: &lt;109.5° - Tetrahedral geometry, bond angles compressed due to larger chlorine atoms

- SBr₄: &gt;109.5° - Distorted tetrahedral geometry, bond angles expanded due to larger bromine atoms

Remember, the bond angles depend on the size and repulsion between the atoms bonded to the central atom.

Answer 2

The X-S-X bond angles for the compounds SF₄, SCl₄, and SBr₄ are: SF₄: 109.5°, SCl₄: <109.5°, SBr₄: >109.5°.

Step-by-step explanation:

The X-S-X bond angles for the series of compounds SF₄, SCl₄, and SBr₄ are as follows:

• SF₄: 109.5°
• SCl₄: <109.5°
• SBr₄: >109.5°

These bond angles can be explained by considering the electron pair repulsion theory, known as VSEPR theory. According to VSEPR theory, the electron pairs around a central atom will arrange themselves in a way that minimizes electron pair repulsion. In the case of SF₄, the molecule has a tetrahedral shape, resulting in bond angles of 109.5°. However, in SCl₄, one of the chlorine atoms is replaced by a lone pair of electrons, which repels the bonding pairs more strongly, resulting in a decrease in the bond angle. Similarly, in SBr₄, the larger size of the bromine atom causes the bond angle to increase.