Predict the molecular structure, bond angles, and polarity (has a net dipole moment or has no net dipole moment) for each of the following compounds. a. \(\mathrm{SeCl}_{4}\) b. \(\mathrm{SF}_{2}\) c. \(\mathrm{KrF}_{4}\) d. \(C B r_{4}\) e. \(\mathrm{IF}_{3}\) f. \(\mathrm{ClF}_{5}\)

1. Determine the electron domain geometry: Se has 6 valence electrons, and each Cl atom has 7 valence electrons. Therefore, SeCl4 has a total of 34 valence electrons. Since Se is the central atom, distribute the remaining 28 electrons as 4 bonding pairs and 2 lone pairs. This results in an octahedral electron domain geometry. 2. Determine the molecular geometry: Since there are 4 bonding pairs and 2 lone pairs, the molecular geometry of SeCl4 is a seesaw shape. 3. Predict bond angles: The bond angles in a seesaw-shaped molecule are approximately 90° and 120°. 4. Determine polarity: Since Cl is more electronegative than Se, the molecule will have bond dipoles. Because of the seesaw shape, these dipoles do not cancel each other out. Therefore, SeCl4 has a net dipole moment and is polar.

1. Determine the electron domain geometry: S has 6 valence electrons, and each F atom has 7 valence electrons. SF2 has a total of 20 valence electrons. Distribute the remaining 8 electrons as 2 bonding pairs and 2 lone pairs. This results in a tetrahedral electron domain geometry. 2. Determine the molecular geometry: With 2 bonding pairs and 2 lone pairs, the molecular geometry of SF2 is bent or V-shaped. 3. Predict bond angles: The bond angles in a bent molecule are approximately 109.5°. 4. Determine polarity: The electronegativity difference between S and F results in bond dipoles. Due to the bent shape, these dipoles do not cancel each other out. Therefore, SF2 has a net dipole moment and is polar.

1. Determine the electron domain geometry: Kr has 8 valence electrons, and each F atom has 7 valence electrons. KrF4 has a total of 36 valence electrons. There are 4 bonding pairs and 2 lone pairs arranged in an octahedral electron domain geometry. 2. Determine the molecular geometry: With 4 bonding pairs and 2 lone pairs, the molecular geometry of KrF4 is square planar. 3. Predict bond angles: Bond angles in a square planar molecule are 90°. 4. Determine polarity: While there is an electronegativity difference between Kr and F, the dipoles in the molecule cancel each other out due to its symmetric square planar shape. Therefore, KrF4 has no net dipole moment and is nonpolar.

1. Determine the electron domain geometry: C has 4 valence electrons, and each Br atom has 7 valence electrons. CBr4 has a total of 32 valence electrons. With 4 bonding pairs and no lone pairs, the electron domain geometry is tetrahedral. 2. Determine the molecular geometry: Since there are 4 bonding pairs and no lone pairs, the molecular geometry of CBr4 is tetrahedral. 3. Predict bond angles: Bond angles in a tetrahedral molecule are approximately 109.5°. 4. Determine polarity: Although there is an electronegativity difference between C and Br, the symmetric tetrahedral shape causes the dipoles to cancel each other out. Therefore, CBr4 has no net dipole moment and is nonpolar.

1. Determine the electron domain geometry: I has 7 valence electrons, and each F atom has 7 valence electrons. IF3 has a total of 28 valence electrons. With 3 bonding pairs and 2 lone pairs, the electron domain geometry is trigonal bipyramidal. 2. Determine the molecular geometry: Since there are 3 bonding pairs and 2 lone pairs, the molecular geometry of IF3 is T-shaped. 3. Predict bond angles: The bond angles in a T-shaped molecule are approximately 90° and 180°. 4. Determine polarity: The electronegativity difference between I and F creates bond dipoles. The dipoles in the T-shaped molecule do not cancel each other out, resulting in a net dipole moment. Therefore, IF3 is polar.

1. Determine the electron domain geometry: Cl has 7 valence electrons, and each F atom has 7 valence electrons. ClF5 has a total of 42 valence electrons. With 5 bonding pairs and 1 lone pair, the electron domain geometry is octahedral. 2. Determine the molecular geometry: Since there are 5 bonding pairs and 1 lone pair, the molecular geometry of ClF5 is square pyramidal. 3. Predict bond angles: The bond angles in a square pyramidal molecule are approximately 90° and 180°. 4. Determine polarity: There is an electronegativity difference between Cl and F, creating bond dipoles. These dipoles in the square pyramidal geometry do not cancel each other out, so ClF5 has a net dipole moment and is polar.