Molecular Geometry And Hybridization Quiz #3

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  • 1/10 Questions
    For molecules of the general formula AB, n can be greater than four ________. - ProProfs

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

    • For any element A
    • Only when A is an element from the third period or below
    • Only when A is boron or beryllium
    • Only when A is carbon
    • Only when A is Xe
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Molecular Geometry And Hybridization Quiz #3 - Quiz
About This Quiz

Molecular Geometry and Hybridization Quiz #3 assesses understanding of molecular polarity, hybridization, and geometry. It focuses on the properties of molecules based on their structural attributes, crucial for students in advanced chemistry courses.

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  • 2. 
    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 - ProProfs

    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

    • (i) and (ii) only

    • (iii) only

    • (i) and (v) only

    • (iii), (iv), and (v) only

    • (v) only

    Correct Answer
    A. (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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  • 3. 
    The molecular geometry of the BeCl molecule is ____________, and this molecule is _________. - ProProfs

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

    • Linear, nonpolar

    • Linear, polar

    • Bent, nonpolar

    • Bent, polar

    • 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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  • 4. 
    The spd atomic hybrid orbital set accommodates ______ electron domains. - ProProfs

    The spd atomic hybrid orbital set accommodates ______ electron domains.

    • Two

    • Three

    • Four

    • Five

    • Six

    Correct Answer
    A. 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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  • 5. 
    The hybridization of iodine in IF and IF are __________ and __________, respectively. - ProProfs

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

    • Sp^3, sp^3d

    • Sp^3d, sp^3d^2

    • Sp^3d, sp^3

    • Sp^3d^2, sp^3d

    • Sp^3d^2, sp^3d^2

    Correct Answer
    A. 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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  • 6. 
    __________ hybrid orbitals are used for bonding by Xe in the XeF molecule. - ProProfs

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

    • Sp^2

    • Sp^3

    • Sp^3d

    • Sp^3d^2

    • Sp

    Correct Answer
    A. 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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  • 7. 

    Of the molecules below, only _________ is nonpolar.

    • BF3

    • NF3

    • IF3

    • PBr3

    • 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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  • 8. 

    Of the molecules below, only ________ is polar.

    • SbF5

    • AsH3

    • I2

    • SF6

    • CH4

    Correct Answer
    A. 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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  • 9. 
    Of the following, only ___________ has sp hybridization of the central atom. - ProProfs

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

    • PH3

    • CO3^-2

    • ICl3

    • I3^-1

    • PF5

    Correct Answer
    A. 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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  • 10. 
    Three monosulfur fluorides are observed: SF, SF, and SF. Of these, _____________ is/are nonpolar. - ProProfs

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

    • SF2 only

    • SF2 and SF4 only

    • SF4 only

    • SF6 only

    • SF2, SF4, and SF6

    Correct Answer
    A. 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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  • Current Version
  • Mar 20, 2023
    Quiz Edited by
    ProProfs Editorial Team
  • Nov 12, 2014
    Quiz Created by
    Ashley Vickers
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