Question 1

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

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Question 2

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SF₆.

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Question 3

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO₃.

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Question 4

Determine the electron geometry (eg), molecular geometry (mg), and polarity of TeCl₆.

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Question 5

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF₃ OF₂ PF₄⁺

Accepted Answer

All three molecules have a trigonal bipyramidal geometry. The F-A-F bond angle depends on the number of lone pairs on the central atom A. The more lone pairs, the greater the repulsion and the smaller the bond angle. In OF₂, there is one lone pair on the central atom, resulting in the smallest F-A-F bond angle. In PF₃, there are two lone pairs on the central atom, resulting in a larger F-A-F bond angle than in OF₂. In PF₄⁺, there are three lone pairs on the central atom, resulting in the largest F-A-F bond angle. Therefore, the correct order from smallest to largest F-A-F bond angle is: OF₂ < PF₃ < PF₄⁺. This matches option B.

Question 6

How many of the following molecules are polar? XeCl₂ COF₂ PCl₄F SF₆

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Question 7

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS₂ CF₄ SCl₂

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Question 8

How many of the following molecules are polar? PCl₅ COS XeO₃ SeBr₂

Accepted Answer

PCl₅, COS, and SeBr₂ are polar molecules as they have polar bonds and an overall net dipole moment. XeO₃ is not polar as it has symmetrical geometry and no net dipole moment.

Question 9

How many of the following molecules are polar? BrCl₃ CS₂ SiF₄ SO₃

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Question 10

Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H₂O H₃O⁺

Accepted Answer

The X-A-X bond angle is determined by the repulsion between the outer atoms X, which pushes them away from each other and leads to a wider bond angle. In H₂O, the central atom S has two outer atoms (H and O), while in H₃O⁺, it has three outer atoms (H, O, and an extra proton). In HCN, the central atom C has only two outer atoms (H and N). Based on this, we can predict that the X-A-X bond angle will be widest in H₃O⁺ (due to three outer atoms), narrower in H₂O (due to two outer atoms and a lone pair on the sulfur atom), and narrowest in HCN (due to two outer atoms and a small size of the N atom in comparison to S or O). Therefore, the correct order of increasing X-A-X bond angle is H₂O < H₃O⁺ < HCN, which is option E.

Question 11

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N₂O NCl₃ NO₂⁻

Accepted Answer

In general, the X-A-X bond angle decreases as the size of the central atom A increases. For N₂O, the central atom is S and it has a bond angle of approximately 109.5 degrees (tetrahedral geometry). For NCl₃, the central atom is Cl and it has a bond angle slightly less than 109.5 degrees. For NO₂⁻, the central atom is O and it has a bond angle less than 109.5 degrees (approx. 104.5 degrees due to bent geometry caused by the lone pair of electrons on O). Therefore, the order of decreasing bond angle is: N₂O > NO₂⁻ > NCl₃. Choice C correctly reflects this order.

Question 12

How many of the following molecules are polar? XeO₂ SiCl₂Br₂ C₂Br₂ SeCl₆

Accepted Answer

The two polar molecules are XeOS and SeCl. This is because they have an electronegativity difference between their central atom and their surrounding atoms, creating a dipole moment. None of the other molecules have a significant electronegativity difference, so they are nonpolar.

Question 13

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO₂.

Accepted Answer

The molecule has one central sulfur atom (S) bonded to two oxygen atoms (O) and one boron atom (B). The electron geometry is trigonal planar because there are three electron groups around the central sulfur atom. The molecular geometry is bent because the two oxygen atoms are not symmetrically arranged around the central sulfur atom. The molecule is polar because the two O-S bonds are polar and do not cancel each other out. Therefore, the best choice is B (eg = trigonal planar, mg = bent, polar).

Question 14

Determine the electron geometry (eg), molecular geometry (mg), and polarity of HBrO₂.

Accepted Answer

The electron geometry of the molecule can be determined by counting the number of electron groups around the central atom, which is sulfur. There are three electron groups (one bond to H, one bond to Br, and one lone pair), so the electron geometry is tetrahedral.

The molecular geometry, on the other hand, takes into account only the positions of the atoms and not the lone pairs. In this case, there are two bonded atoms and one lone pair. This results in a bent molecular geometry.

Finally, the molecule is polar because the dipole moments of the two S-O bonds do not cancel each other out due to the bent shape of the molecule.

Question 15

Determine the electron geometry (eg), molecular geometry (mg), and polarity of XeO₃.

Accepted Answer

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Question 16

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO₂ SeCl₆SeF₂

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Question 17

A pilot checks for water in the gas before flying a small airplane. How does she do it?

Accepted Answer

The pilot drains a small amount of fuel from the bottom of the fuel tank or fuel system using a fuel drain valve or sump. Water, being denser than fuel, will settle at the bottom, allowing the pilot to visually inspect for any separation into two layers, indicating the presence of water.

Question 18

Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms.

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Question 19

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SF₆.

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Question 20

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Accepted Answer

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Quiz 10: Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF₆.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO₃.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of TeCl₆.

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF₃ OF₂ PF₄⁺

How many of the following molecules are polar? XeCl₂ COF₂ PCl₄F SF₆

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS₂ CF₄ SCl₂

How many of the following molecules are polar? PCl₅ COS XeO₃ SeBr₂

How many of the following molecules are polar? BrCl₃ CS₂ SiF₄ SO₃

Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H₂O H₃O⁺

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N₂O NCl₃ NO₂⁻

How many of the following molecules are polar? XeO₂ SiCl₂Br₂ C₂Br₂ SeCl₆

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO₂.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of HBrO₂.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of XeO₃.

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO₂ SeCl₆SeF₂

A pilot checks for water in the gas before flying a small airplane. How does she do it?

Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF₆.

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Quiz 10: Chemical Bonding Ii: Molecular Shapes, Valence Bond Theory, and Molecular Orbital Theory

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF6.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO3.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of TeCl6.

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4⁺

How many of the following molecules are polar? XeCl2 COF2 PCl4F SF6

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS2 CF4 SCl2

How many of the following molecules are polar? PCl5 COS XeO3 SeBr2

How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3

Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H2O H3O⁺

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N2O NCl3 NO2⁻

How many of the following molecules are polar? XeO2 SiCl2Br2 C2Br2 SeCl6

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO2.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of HBrO2.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of XeO3.

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO2 SeCl6 SeF2

A pilot checks for water in the gas before flying a small airplane. How does she do it?

Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF6.

Choose the compound below that contains at least one polar covalent bond but is nonpolar.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF₆.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO₃.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of TeCl₆.

Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF₃ OF₂ PF₄⁺

How many of the following molecules are polar? XeCl₂ COF₂ PCl₄F SF₆

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. CS₂ CF₄ SCl₂

How many of the following molecules are polar? PCl₅ COS XeO₃ SeBr₂

How many of the following molecules are polar? BrCl₃ CS₂ SiF₄ SO₃

Place the following in order of increasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. HCN H₂O H₃O⁺

Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the outer atoms in each molecule. N₂O NCl₃ NO₂⁻

How many of the following molecules are polar? XeO₂ SiCl₂Br₂ C₂Br₂ SeCl₆

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SO₂.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of HBrO₂.

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of XeO₃.

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO₂ SeCl₆SeF₂

Determine the electron geometry (eg) , molecular geometry (mg) , and polarity of SF₆.