For molecules of the general formula AB, n can be greater than four ________.

only when A is an element from the third period or below

only when A is boron or beryllium

Molecular Geometry And Hybridization Quiz #3

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Quizzes Created: 7 | Total Attempts: 5,369

Questions: 10 | Attempts: 192 | Updated: Mar 20, 2023

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Molecular Geometry And Hybridization Quiz #3 - Quiz

Questions and Answers

1.

For molecules of the general formula AB, n can be greater than four ________.
- A.
  
  For any element A
- B.
  
  Only when A is an element from the third period or below
- C.
  
  Only when A is boron or beryllium
- D.
  
  Only when A is carbon
- E.
  
  Only when A is Xe
Correct Answer
B. Only when A is an element from the third period or below

Explanation
Molecules of the general formula AB can have n greater than four only when A is an element from the third period or below. This means that if A is an element from the third period or below in the periodic table, the molecule AB can have more than four atoms. If A is an element from a higher period, the molecule AB will not have more than four atoms.

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2.

Of the molecules below, only ________ is polar.
- A.
  
  SbF5
- B.
  
  AsH3
- C.
  
  I2
- D.
  
  SF6
- E.
  
  CH4
Correct Answer
B. AsH3

Explanation
AsH3 (arsine) is the only polar molecule among the given options. This is because it has a trigonal pyramidal molecular geometry with a lone pair of electrons on the central atom (arsenic). The asymmetry in the molecule leads to an uneven distribution of charge, resulting in a polar molecule. The other molecules listed (SbF5, I2, SF6, CH4) have symmetrical molecular geometries or no lone pairs, making them nonpolar.

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3.

Of the molecules below, only _________ is nonpolar.
- A.
  
  BF3
- B.
  
  NF3
- C.
  
  IF3
- D.
  
  PBr3
- E.
  
  BrCl3
Correct Answer
A. BF3

Explanation
BF3 is the only nonpolar molecule among the given options. This is because BF3 has a trigonal planar molecular geometry with the boron atom in the center and three fluorine atoms surrounding it. The fluorine atoms are all identical and have the same electronegativity, resulting in a symmetrical distribution of charge around the boron atom. Since there are no lone pairs of electrons on the central atom and the bond dipoles cancel out each other, BF3 is nonpolar. In contrast, NF3, IF3, PBr3, and BrCl3 have polar bonds or lone pairs, leading to an overall dipole moment and making them polar molecules.

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4.

Three monosulfur fluorides are observed: SF, SF, and SF. Of these, _____________ is/are nonpolar.
- A.
  
  SF2 only
- B.
  
  SF2 and SF4 only
- C.
  
  SF4 only
- D.
  
  SF6 only
- E.
  
  SF2, SF4, and SF6
Correct Answer
D. SF6 only

Explanation
SF6 only is the correct answer because SF6 is an octahedral molecule with six fluorine atoms surrounding the central sulfur atom. The fluorine atoms are arranged symmetrically around the sulfur atom, resulting in a symmetrical distribution of electron density. As a result, SF6 is a nonpolar molecule. On the other hand, SF2 and SF4 have a bent and seesaw molecular geometry respectively, which leads to an asymmetrical distribution of electron density and makes them polar molecules.

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5.

The molecular geometry of the BeCl molecule is ____________, and this molecule is _________.
- A.
  
  Linear, nonpolar
- B.
  
  Linear, polar
- C.
  
  Bent, nonpolar
- D.
  
  Bent, polar
- E.
  
  Trigonal planar, polar
Correct Answer
A. Linear, nonpolar

Explanation
The BeCl molecule consists of two atoms, Be and Cl, with a linear arrangement. Since there are no lone pairs on the central atom (Be), the molecule is symmetrical and the dipole moments of the two Be-Cl bonds cancel each other out, resulting in a nonpolar molecule.

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6.

Of the following, only ___________ has sp hybridization of the central atom.
- A.
  
  PH3
- B.
  
  CO3^-2
- C.
  
  ICl3
- D.
  
  I3^-1
- E.
  
  PF5
Correct Answer
B. CO3^-2

Explanation
CO3^-2 is the only molecule among the given options that has sp hybridization of the central atom. In CO3^-2, the central atom is carbon, which forms three sigma bonds with three oxygen atoms. To accommodate these bonds, carbon undergoes sp hybridization, where one s orbital and two p orbitals hybridize to form three sp hybrid orbitals. These orbitals are then used to form sigma bonds with the oxygen atoms, resulting in a trigonal planar geometry around the carbon atom. The other molecules in the options do not have sp hybridization of the central atom.

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7.

The spd atomic hybrid orbital set accommodates ______ electron domains.
- A.
  
  Two
- B.
  
  Three
- C.
  
  Four
- D.
  
  Five
- E.
  
  Six
Correct Answer
E. Six

Explanation
The spd atomic hybrid orbital set consists of three orbitals: one s orbital, three p orbitals, and five d orbitals. Each orbital can accommodate a maximum of two electrons. Therefore, when all the orbitals in the spd set are considered, a total of six electron domains can be accommodated.

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8.

The hybridization of iodine in IF and IF are __________ and __________, respectively.
- A.
  
  Sp^3, sp^3d
- B.
  
  Sp^3d, sp^3d^2
- C.
  
  Sp^3d, sp^3
- D.
  
  Sp^3d^2, sp^3d
- E.
  
  Sp^3d^2, sp^3d^2
Correct Answer
B. Sp^3d, sp^3d^2

Explanation
The hybridization of iodine in IF is sp^3d, while the hybridization of iodine in IF7 is sp^3d^2.

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9.

__________ hybrid orbitals are used for bonding by Xe in the XeF molecule.
- A.
  
  Sp^2
- B.
  
  Sp^3
- C.
  
  Sp^3d
- D.
  
  Sp^3d^2
- E.
  
  Sp
Correct Answer
D. Sp^3d^2

Explanation
The XeF molecule is formed by the bonding of xenon (Xe) and fluorine (F) atoms. In order to form bonds, Xe utilizes hybrid orbitals. The sp^3d^2 hybrid orbitals are used by Xe in the XeF molecule. This hybridization allows Xe to form six bonds, as it has six electron pairs in its valence shell. Therefore, the correct answer is sp^3d^2.

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10.

In which of the molecules does the central atom utilize d orbitals to form hybrid orbitals? i) PCl ii) CCl iii) TeCl iv) XeF v) SF
- A.
  
  (i) and (ii) only
- B.
  
  (iii) only
- C.
  
  (i) and (v) only
- D.
  
  (iii), (iv), and (v) only
- E.
  
  (v) only
Correct Answer
D. (iii), (iv), and (v) only

Explanation
The central atom utilizes d orbitals to form hybrid orbitals in molecules that have an expanded octet or have more than 8 valence electrons. In this case, (iii) TeCl, (iv) XeF, and (v) SF are the only molecules that fit this criteria. PCl and CCl do not have an expanded octet and do not require the use of d orbitals for hybridization.

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Current Version
Mar 20, 2023

Quiz Edited by
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Nov 12, 2014

Quiz Created by
Ashley Vickers

Molecular Geometry And Hybridization Quiz #3

For molecules of the general formula AB, n can be greater than four ________.

Of the molecules below, only ________ is polar.

Of the molecules below, only _________ is nonpolar.

Three monosulfur fluorides are observed: SF, SF, and SF. Of these, _____________ is/are nonpolar.

The molecular geometry of the BeCl molecule is ____, and this molecule is _.

Of the following, only ___________ has sp hybridization of the central atom.

The spd atomic hybrid orbital set accommodates ______ electron domains.

The hybridization of iodine in IF and IF are and , respectively.

__________ hybrid orbitals are used for bonding by Xe in the XeF molecule.

In which of the molecules does the central atom utilize d orbitals to form hybrid orbitals? i) PCl ii) CCl iii) TeCl iv) XeF v) SF

Molecular Geometry And Hybridization Quiz #3

For molecules of the general formula AB, n can be greater than four ________.

Of the molecules below, only ________ is polar.

Of the molecules below, only _________ is nonpolar.

Three monosulfur fluorides are observed: SF, SF, and SF. Of these, _____________ is/are nonpolar.

The molecular geometry of the BeCl molecule is ____________, and this molecule is _________.

Of the following, only ___________ has sp hybridization of the central atom.

The spd atomic hybrid orbital set accommodates ______ electron domains.

The hybridization of iodine in IF and IF are __________ and __________, respectively.

__________ hybrid orbitals are used for bonding by Xe in the XeF molecule.

In which of the molecules does the central atom utilize d orbitals to form hybrid orbitals? i) PCl ii) CCl iii) TeCl iv) XeF v) SF

The molecular geometry of the BeCl molecule is ____, and this molecule is _.

The hybridization of iodine in IF and IF are and , respectively.