Question 1

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃. A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar

Accepted Answer

The central atom (C) has four electron groups (two single bonds and two lone pairs), giving it a tetrahedral electron geometry. However, since two of the groups are lone pairs, they repel more strongly than bonds and push the two bonded atoms closer together, resulting in a bent molecular geometry. Therefore, the correct answer is C (tetrahedral eg, bent mg).

Question 2

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

Accepted Answer

In PF₃ and PF₄⁺, the central atom (P) has five surrounding atoms which creates trigonal bipyramidal geometry. In OF₂, the central atom (O) has four surrounding atoms which creates tetrahedral geometry. The F-A-F bond angle in tetrahedral geometry is ~109.5°, while the F-A-F bond angle in trigonal bipyramidal geometry is ~90° and ~120°. Therefore, OF₂ has the smallest bond angle, followed by PF₃, and finally PF₄⁺ has the largest bond angle. Therefore, the correct order from smallest to largest bond angle is OF₂ < PF₃ < PF₄⁺, which matches answer choice B.

Question 3

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₄. A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar

Accepted Answer

The answer of Determine the electron geometry (eg) and molecular...

Question 4

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⁻ A) NCl₃ > NO₂⁻ > N₂O B) NO₂⁻ > N₂O > NCl₃ C) N₂O > NO₂⁻ > NCl₃ D) NCl₃ > N₂O > NO₂⁻ E) N₂O > NCl₃ > NO₂⁻

Accepted Answer

The X-A-X bond angle is determined by the repulsion between the outer atoms and lone pairs on the central atom. In this case, N, O, Cl are the central atoms and S, O, Cl are the outer atoms. The largest X-A-X bond angle will be in the molecule where the central atom has the least number of lone pairs. Therefore, the X-A-X bond angle will be largest in N₂O, followed by NO₂⁻ and then NCl₃. Thus, the correct choice is C.

Question 5

Determine the electron geometry (eg) and molecular geometry (mg) of IBr₄^-. A) eg = tetrahedral, mg = tetrahedral B) eg = octahedral, mg = square planar C) eg = trigonal planar, mg = bent D) eg = tetrahedral, mg = trigonal pyramidal E) eg = trigonal bipyramidal, mg = linear

Accepted Answer

IBr4^- has 6 regions of electron density around the central iodine atom, leading to an octahedral electron geometry. With 4 bonded atoms and 2 lone pairs, the molecular geometry is square planar.

Question 6

Consider the molecule below. Determine the molecular geometry at each of the two labelled carbons. 
A) C1 = tetrahedral, C2 = linear
B) C1 = trigonal planar, C2 = bent
C) C1 = bent, C2 = trigonal planar
D) C1 = trigonal planar, C2 = tetrahedral
E) C1 = trigonal pyramidal, C2 = seesaw

Accepted Answer

The answer of Consider the molecule below. Determine the molecular...

Question 7

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂NH₂. A) mg = tetrahedral B) mg = trigonal pyramidal C) mg = trigonal planar D) mg = trigonal bipyramidal E) mg = bent

Accepted Answer

The bolded and underlined atom is nitrogen in CH3CH2NH2. It has three bonds and one lone pair, resulting in a trigonal pyramidal molecular geometry.

Question 8

Determine the electron geometry (eg) and molecular geometry (mg) of ICl₂⁻. A) eg = tetrahedral, mg = bent B) eg = tetrahedral, mg = trigonal pyramidal C) eg = trigonal bipyramidal, mg = linear D) eg = trigonal bipyramidal, mg = trigonal planar E) eg = octahedral, mg = linear

Accepted Answer

ICl₂⁻ has 5 regions of electron density (3 lone pairs and 2 bonds), giving it a trigonal bipyramidal electron geometry. The lone pairs occupy equatorial positions, resulting in a linear molecular geometry.

Question 9

Consider the molecule below. Determine the molecular geometry at each of the three labelled atoms. 
A) 1 = trigonal planar, 2 = tetrahedral, 3 = trigonal pyramidal
B) 1 = tetrahedral, 2 = tetrahedral, 3 = tetrahedral
C) 1 = trigonal planar, 2 = tetrahedral, 3 = tetrahedral
D) 1 = tetrahedral, 2 = tetrahedral, 3 = trigonal planar
E) 1 = trigonal planar, 2 = trigonal pyramidal, 3 = trigonal pyramidal

Accepted Answer

The answer of Consider the molecule below. Determine the molecular...

Question 10

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃. A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = linear C) eg = tetrahedral, mg = bent D) eg = trigonal bipyramidal, mg = tetrahedral E) eg = octahedral, mg = square planar

Accepted Answer

The bolded and underlined atom is the central carbon atom in CH3OCH3. This carbon atom has four electron groups around it, which gives it a tetrahedral electron geometry. The molecular geometry is also tetrahedral because there are no lone pairs of electrons on the central carbon atom.

Question 11

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH. A) mg = tetrahedral B) mg = trigonal pyramidal C) mg = trigonal planar D) mg = trigonal bipyramidal E) mg = bent

Accepted Answer

The answer of Determine the molecular geometry (mg) of the...

Question 12

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CO₂H. A) mg = tetrahedral B) mg = trigonal pyramidal C) mg = trigonal planar D) mg = trigonal bipyramidal E) mg = bent

Accepted Answer

The bolded and underlined atom is the central carbon in the carboxylic acid group (COOH). This carbon is bonded to three atoms (two oxygens and one carbon) and has no lone pairs, resulting in a trigonal planar geometry.

Question 13

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH. A) mg = tetrahedral B) mg = trigonal pyramidal C) mg = trigonal planar D) mg = trigonal bipyramidal E) mg = bent

Accepted Answer

The answer of Determine the molecular geometry (mg) of the...

Question 14

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₂. A) eg = trigonal bipyramidal, mg = bent B) eg = linear, mg = linear C) eg = tetrahedral, mg = linear D) eg = trigonal bipyramidal, mg = linear E) eg = tetrahedral, mg = bent

Accepted Answer

The electron geometry of XeF₂ is trigonal bipyramidal because Xe has six electron domains around it (one lone pair, two axial F atoms, and three equatorial B12S1U1 atoms). However, the molecular geometry is linear because the lone pair on Xe occupies one of the equatorial positions, causing the two axial F atoms to move closer together and giving a linear shape. Choice D is the only option that correctly matches the electron and molecular geometries.

Question 15

Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO₃. A) eg = tetrahedral, mg = trigonal pyramidal, polar B) eg = tetrahedral, mg = tetrahedral, nonpolar C) eg = trigonal planar, mg = trigonal planar, nonpolar D) eg = trigonal bipyramidal, mg = trigonal planar, polar E) eg = trigonal pyramidal, mg = bent, nonpolar

Accepted Answer

The answer of Determine the electron geometry (eg), molecular geometry...

Question 16

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 A) CS₂ > SCl₂ > CF₄ B) SCl₂ > CF₄ > CS₂ C) CF₄ > SCl₂> CS₂ D) CS₂ > CF₄> SCl₂ E) CF₄> CS₂ > SCl₂

Accepted Answer

The answer of Place the following in order of decreasing...

Question 17

Determine the electron geometry (eg) and molecular geometry (mg) of ClF₃. A) eg = tetrahedral, mg = tetrahedral B) eg = linear, mg = trigonal planar C) eg = trigonal planar, mg = bent D) eg = tetrahedral, mg = trigonal pyramidal E) eg = trigonal bipyramidal, mg = T-shaped

Accepted Answer

ClF3 has 5 regions of electron density (3 bonds and 2 lone pairs), giving it a trigonal bipyramidal electron geometry. The lone pairs occupy equatorial positions, resulting in a T-shaped molecular geometry.

Question 18

How many of the following molecules are polar? BrCl₃ CS₂ SiF₄ SO₃ A) 1 B) 2 C) 3 D) 4 E) 0

Accepted Answer

The answer of How many of the following molecules are...

Question 19

Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO₂ SeCl₆SeF₂ A) SeCl₆ < SeF₂ < SeO₂ B) SeF₂ < SeO₂< SeCl₆ C) SeF₂ < SeCl₆< SeO₂ D) SeO₂ < SeF₂< SeCl₆ E) SeCl₆ < SeO₂< SeF₂

Accepted Answer

The answer of Place the following in order of increasing...

Question 20

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⁺ A) H₃O⁺ < HCN < H₂O B) H₃O⁺ < H₂O < HCN C) HCN < H₃O⁺ < H₂O D) H₂O < HCN < H₃O⁺ E) H₂O < H₃O⁺ < HCN

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.

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

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃.

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

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₄.

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⁻

Determine the electron geometry (eg) and molecular geometry (mg) of IBr₄^-.

Consider the molecule below. Determine the molecular geometry at each of the two labelled carbons.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂NH₂.

Determine the electron geometry (eg) and molecular geometry (mg) of ICl₂⁻.

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

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CO₂H.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₂.

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

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

Determine the electron geometry (eg) and molecular geometry (mg) of ClF₃.

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

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

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⁺

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

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH3OCH3.

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

Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.

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⁻

Determine the electron geometry (eg) and molecular geometry (mg) of IBr4-.

Consider the molecule below. Determine the molecular geometry at each of the two labelled carbons.

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CH2NH2.

Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻.

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

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH3OCH3.

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CH2OH.

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CO2H.

Determine the molecular geometry (mg) of the bolded and underlined atom CH3CH2OH.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.

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

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

Determine the electron geometry (eg) and molecular geometry (mg) of ClF3.

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

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

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⁺

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃.

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

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₄.

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⁻

Determine the electron geometry (eg) and molecular geometry (mg) of IBr₄^-.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂NH₂.

Determine the electron geometry (eg) and molecular geometry (mg) of ICl₂⁻.

Determine the electron geometry (eg) and molecular geometry (mg) of the bolded and underlined atom CH₃OCH₃.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CO₂H.

Determine the molecular geometry (mg) of the bolded and underlined atom CH₃CH₂OH.

Determine the electron geometry (eg) and molecular geometry (mg) of XeF₂.

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

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

Determine the electron geometry (eg) and molecular geometry (mg) of ClF₃.

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

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

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⁺