Vsper Quiz#2 Identify Molecular Shape And Angle
- 1.
Name the shape of this molecule:
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
C. LinearExplanation
The molecule is linear because it has two bonded atoms and no lone pairs of electrons. In a linear molecule, the bonded atoms are arranged in a straight line, with a bond angle of 180 degrees.Rate this question:
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- 2.
Name the shape of this molecule:
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
A. Trigonal planarExplanation
The molecule is named trigonal planar because it has a central atom bonded to three other atoms in a flat, triangular arrangement. This arrangement results in a planar shape for the molecule.Rate this question:
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- 3.
Name the shape of this molecule: The bond angle is about 120 in this molecule
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
B. Bent (from trigonal planar)Explanation
The molecule has a bond angle of about 120 degrees, which suggests that the central atom is surrounded by three bonded atoms in a trigonal planar arrangement. However, the molecule is described as "bent," which means that the bonded atoms are not in a straight line. This indicates that there is an additional lone pair of electrons on the central atom, causing the bonded atoms to be slightly pushed closer together. Therefore, the correct answer is "bent (from trigonal planar)."Rate this question:
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- 4.
Name the shape of this molecule:
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
D. TetrahedralExplanation
The molecule is tetrahedral because it has four bonded atoms and no lone pairs on the central atom. A tetrahedral molecule has a central atom surrounded by four other atoms, forming a three-dimensional shape with bond angles of approximately 109.5 degrees.Rate this question:
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- 5.
Name the shape of this molecule:
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
F. Trigonal pyramidal -
- 6.
Name the shape of this molecule: The bond angle in this molecule is 105 degrees
- A.
Trigonal planar
- B.
Bent (from trigonal planar)
- C.
Linear
- D.
Tetrahedral
- E.
Bent (from tetrahedral)
- F.
Trigonal pyramidal
Correct Answer
E. Bent (from tetrahedral)Explanation
The molecule has a bond angle of 105 degrees, which suggests that it is not a trigonal planar or linear molecule. The only options left are tetrahedral, bent (from trigonal planar), and trigonal pyramidal. Since the bond angle is less than the ideal tetrahedral angle of 109.5 degrees, the molecule must be bent. This means that it started as a tetrahedral molecule but has undergone distortion or bending, resulting in a bond angle of 105 degrees.Rate this question:
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- 7.
What is the bond angle of this molecule:
- A.
180
- B.
120
- C.
109.5
- D.
107
- E.
105
Correct Answer
C. 109.5Explanation
The bond angle of 109.5 degrees is commonly found in molecules with a tetrahedral shape. This shape occurs when a central atom is bonded to four other atoms and has no lone pairs of electrons. One example of a molecule with this bond angle is methane (CH4), where the central carbon atom is bonded to four hydrogen atoms. The bond angle of 109.5 degrees is a result of the repulsion between the electron pairs in the molecule, which causes them to arrange themselves as far apart as possible, leading to a tetrahedral shape.Rate this question:
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- 8.
Find the correct number of bonding regions (single, double or triple bonds) and lone pairs of electrons that makes the shape of this molecule:
- A.
4 bonding regions and 0 lone pairs
- B.
3 bonding regions and 1 lone pair
- C.
2 bonding regions and 2 lone pairs
- D.
3 bonding regions and 0 lone pair
- E.
2 bonding regions and 1 lone pair
Correct Answer
A. 4 bonding regions and 0 lone pairsExplanation
This molecule has four bonding regions and zero lone pairs. The number of bonding regions is determined by the number of bonds formed between atoms. In this case, there are four bonds, indicating four bonding regions. Lone pairs are non-bonding electrons that are not involved in bonding. Since there are no lone pairs mentioned in the question, the molecule has zero lone pairs.Rate this question:
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- 9.
What is the bond angle of this molecule:
- A.
180
- B.
120
- C.
109.5
- D.
107
- E.
105
Correct Answer
A. 180Explanation
The bond angle of 180 degrees suggests that the molecule is linear. In a linear molecule, the atoms are arranged in a straight line with a bond angle of 180 degrees between them. This means that the atoms are directly opposite each other and there is no bending or distortion in the molecular structure.Rate this question:
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- 10.
What is the bond angle of this molecule:
- A.
180
- B.
120
- C.
109.5
- D.
107
- E.
105
Correct Answer
B. 120Explanation
The bond angle of 120 degrees suggests that the molecule is trigonal planar in shape. In a trigonal planar molecule, the central atom is bonded to three other atoms, creating a flat, triangular arrangement. This type of arrangement is commonly seen in molecules with a central atom surrounded by three bonding pairs and no lone pairs of electrons. The bond angle of 120 degrees is characteristic of this arrangement, as the three bonding pairs repel each other equally, pushing the atoms as far apart as possible.Rate this question:
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- 11.
What is the bond angle of this molecule:
- A.
180
- B.
120
- C.
109.5
- D.
107
- E.
105
Correct Answer
D. 107Explanation
The bond angle of a molecule refers to the angle between two adjacent bonds. In this case, the correct answer is 107. The bond angle of 107 suggests that the molecule has a bent or V-shaped geometry. This can be seen in molecules with three atoms, where the central atom is bonded to two other atoms and has one or two lone pairs of electrons. The presence of lone pairs causes the bond angle to deviate from the ideal tetrahedral angle of 109.5 degrees.Rate this question:
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- 12.
Find the correct number of bonding regions (single, double or triple bonds) and lone pairs of electrons that makes the shape of this molecule:
- A.
4 bonding regions and 0 lone pairs
- B.
3 bonding regions and 1 lone pair
- C.
2 bonding regions and 2 lone pairs
- D.
3 bonding regions and 0 lone pair
- E.
2 bonding regions and 1 lone pair
Correct Answer
D. 3 bonding regions and 0 lone pairExplanation
The molecule in question has three bonding regions and no lone pairs of electrons. This can be determined by examining the Lewis structure of the molecule and counting the number of bonds and lone pairs. In this case, there are three lines indicating bonding regions and no dots indicating lone pairs. Therefore, the correct answer is 3 bonding regions and 0 lone pairs.Rate this question:
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- 13.
Find the correct number of bonding regions (single, double or triple bonds) and lone pairs of electrons that makes the shape of this molecule:
- A.
4 bonding regions and 0 lone pairs
- B.
3 bonding regions and 1 lone pair
- C.
2 bonding regions and 2 lone pairs
- D.
3 bonding regions and 0 lone pair
- E.
2 bonding regions and 1 lone pair
Correct Answer
B. 3 bonding regions and 1 lone pairExplanation
This molecule has three bonding regions and one lone pair of electrons. The bonding regions can be determined by counting the number of bonds between atoms, including both single, double, and triple bonds. The lone pair of electrons refers to a pair of electrons that is not involved in bonding and is localized on a specific atom. In this case, there are three bonding regions (which could be single, double, or triple bonds) and one lone pair of electrons.Rate this question:
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- 14.
Find the correct number of bonding regions (single, double or triple bonds) and lone pairs of electrons that makes the shape of this molecule: The bond angle is about 120 in this molecule
- A.
4 bonding regions and 0 lone pairs
- B.
3 bonding regions and 1 lone pair
- C.
2 bonding regions and 2 lone pairs
- D.
3 bonding regions and 0 lone pair
- E.
2 bonding regions and 1 lone pair
Correct Answer
E. 2 bonding regions and 1 lone pairExplanation
The molecule in question has a bond angle of about 120 degrees. This suggests that it has a trigonal planar shape, which is consistent with the presence of 2 bonding regions and 1 lone pair of electrons. This arrangement allows for the optimal distribution of electron density around the central atom, resulting in a stable and symmetrical structure.Rate this question:
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- 15.
Find the correct number of bonding regions (single, double or triple bonds) and lone pairs of electrons that makes the shape of this molecule: The bond angle in this molecule is 105 degrees
- A.
4 bonding regions and 0 lone pairs
- B.
3 bonding regions and 1 lone pair
- C.
2 bonding regions and 2 lone pairs
- D.
3 bonding regions and 0 lone pair
- E.
2 bonding regions and 1 lone pair
Correct Answer
C. 2 bonding regions and 2 lone pairsExplanation
The molecule in question has a bond angle of 105 degrees. This information suggests that the molecule has a bent or V-shaped geometry. In a bent molecule, there are two bonding regions and two lone pairs of electrons. The bonding regions correspond to the two chemical bonds in the molecule, while the lone pairs are non-bonding pairs of electrons that are not involved in any chemical bond. Therefore, the correct answer is 2 bonding regions and 2 lone pairs.Rate this question:
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Current Version
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Mar 20, 2023Quiz Edited by
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Nov 11, 2012Quiz Created by
Ssamreth
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