Mastering Chemistry Tro Chapter 10
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
CS2 > CF4 > SCl2
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: PF5
Trigonal bipyramidal
Determine the molecular geometry about each interior atom and make a sketch: C2H4 (skeletal structure: H2CCH2)
Trigonal planar
Draw the Lewis structure for BrCl3. What is the hybridization on the Br atom?
sp3d
Draw the Lewis structure for BrF5. What is the hybridization on the Br atom?
sp3d2
Draw the Lewis structure for SF6. What is the hybridization on the S atom?
sp3d2
How many of the following molecules are polar? PCl5 COS XeO3 SeBr2
3
Determine the molecular geometry about each interior atom and make a sketch: C2H6 (skeletal structure: H3CCH3)
Tetrahedral
Place the following in order of increasing X-Se-X bond angle, where X represents the outer atoms in each molecule. SeO2 SeCl6 SeF2
SeCl6 < SeF2 < SeO2
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: [IF4]+
Seesaw
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: [IBr4]-
Square planar
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: BrF5
Square pyramidal
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: ClF3
T-shape
Determine the electron geometry, molecular geometry and polarity of N2O (N central).
eg= linear, mg=linear, polar
A molecule containing a central atom with sp3 hybridization has a(n) __________ electron geometry.
tetrahedral
A molecule containing a central atom with sp3d hybridization has a(n) __________ electron geometry.
trigonal bipyramidal
Identify the shape that goes with sp3d.
trigonal bipyramidal
According to the electronegativity difference between the atoms in water, it would be appropriate to label hydrogen with the symbol ____ and oxygen with the symbol ____.
hydrogen δ+ ; oxygen δ−
According to the electronegativity difference between the atoms in methane, it would be appropriate to label hydrogen with the symbol ____, and carbon with the symbol ____.
hydrogen δ0 ; carbon δ0
The H−O−H bond angle in H2O is _________ the H−C−H bond angle in CH4
less than
The O−S−O bond angle in SO2 is _________ the F−B−F bond angle in BF3.
less than
For the water molecule, oxygen is _______ electronegative than hydrogen.
more
According to the electronegativity difference between the atoms in carbon dioxide, it would be appropriate to label oxygen with the symbol ____, and carbon with the symbol ____.
oxygen δ− ; carbon δ+
Consider the molecule below. Determine the hybridization at each of the 3 labeled atoms.
1=sp2, 2=sp3, 3=sp3
Consider the molecule below. Determine the molecular geometry at each of the 3 labeled atoms.
1=trigonal planar, 2=tetrahedral, 3=trigonal pyramidal
How many of the following molecules are polar? XeO2 SiCl2Br2 C2Br2 SeCl6
2
How many of the following molecules have sp hybridization on the central atom? C2Cl2 CO2 O3 H2O
2
How many of the following molecules have sp3d hybridization on the central atom? SiCl4 BrF5 AsF5 BrF3
2
Choose the compound below that contains at least one polar covalent bond, but is nonpolar.
AsCl5
Consider the molecule below. Determine the molecular geometry at each of the 2 labeled carbons.
C1 = bent, C2 = trigonal planar
Consider the molecule below. Determine the hybridization at each of the 2 labeled carbons.
C1 = sp2, C2 = sp3
Choose the compound below that contains at least one polar covalent bond, but is nonpolar.
CF4
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⁺
H2O < H3O⁺ < HCN
Place the following in order of increasing dipole moment. I. BCl3 II. BIF2 III. BClF2
I < III < II
Place the following in order of decreasing dipole moment. I. cis-CHCl=CHCl II. trans-CHCl=CHCI III. cis-CHF=CHF
III > I > II
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⁻
N2O > NO2⁻ > NCl3
Place the following in order of increasing F-A-F bond angle, where A represents the central atom in each molecule. PF3 OF2 PF4⁺
OF2 < PF3 < PF4⁺
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: SCl6
Octahedral
Determine the electron geometry, molecular geometry and polarity of SF6 .
eg=octahedral, mg=octahedral, nonpolar
Determine the electron geometry, molecular geometry and polarity of TeCl6.
eg=octahedral, mg=octahedral, nonpolar
Determine the electron geometry (eg) and molecular geometry (mg) of XeF4.
eg=octahedral, mg=square planar
Determine the electron geometry, molecular geometry and polarity of HBrO2 .
eg=tetrahedral, mg==trigonal pyramidal, polar
Determine the electron geometry (eg) and molecular geometry (mg) of SiF4.
eg=tetrahedral, mg=tetrahedral
Determine the electron geometry (eg), molecular geometry (mg), and polarity of PCl3.
eg=tetrahedral, mg=trigonal pyramidal, polar
Determine the electron geometry (eg), molecular geometry(mg) and polarity of XeO3.
eg=tetrahedral, mg=trigonal pyramidal, polar
Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.
eg=trigonal bipyramidal, mg= T-shape
Determine the electron geometry (eg) and molecular geometry (mg) of ICl2⁻.
eg=trigonal bipyramidal, mg=linear
Determine the electron geometry (eg) and molecular geometry (mg) of XeF2.
eg=trigonal bipyramidal, mg=linear
Determine the electron geometry (eg) and molecular geometry (mg) of PF5.
eg=trigonal bipyramidal, mg=trigonal bipyramidal
Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO2.
eg=trigonal planar, mg=bent, polar
Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.
eg=trigonal planar, mg=trigonal planar
Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.
eg=trigonal planar, mg=trigonal planar
Determine the electron geometry (eg) and molecular geometry(mg) of BCl3.
eg=trigonal planar, mg=trigonal planar
Determine the electron geometry (eg), molecular geometry (mg), and polarity of SO3.
eg=trigonal planar, mg=trigonal planar, nonpolar
The F−Xe−F bond angle in XeF4 is __________ the F−S−F bond angle in SF6.
equal to
Identify the number of electron groups around a molecule with a tetrahedral shape.
four
The F−S−F T-junction bond angle in SF4 is _________ the F−Cl−F T-junction bond angle in ClF3.
greater than
The F−S−F bond angle in SF6 is__________ the F−Br−F bond angle in BrF5.
greater than
How many of the following molecules are polar? XeCl2 COF2 PCl4F SF6
3
Consider the following molecules with trigonal planar geometry. Carbonate (CO32−) and nitrate (NO3−) both exhibit resonance, whereas phosgene (COCl2) does not. Predict the bond angles for each of the molecules in accordance to whether or not they exhibit resonance.
(CO32−) 120, 120 (NO3−) 120, 120 (COCl2) 111.4, 124.3 bottom angle , right angle
Determine the electron geometry (eg) and molecular geometry (mg) of the underlined carbon in CH3CN.
...
How many of the following molecules are polar? BrCl3 CS2 SiF4 SO3
1
How many of the following molecules have sp3 hybridization on the central atom? XeCl4 CH4 SF4 C2H2
1
Give the approximate bond angle for a molecule with a tetrahedral shape.
109.5°
Give the approximate bond angle for a molecule with a trigonal planar shape.
120°
Determine the molecular geometry about each interior atom and make a sketch: C2H2 (skeletal structure: HCCH)
Linear
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: [IF2]-
Linear
Examine the three dimensional structures of each of the following molecules in the simulation, which can be found in the Real Molecules mode. Then, identify which molecules are polar and which are nonpolar. Assume that every bond in each molecule is polar covalent.
Polar: SO2, SF4, ClF3, NH3 Nonpolar: SF6, XeF2, XeF4, PCl5
Based on the electronegativity difference between carbon and hydrogen, the bonds in methane are _______.
nonpolar
A molecule containing a central atom with sp3d2 hybridization has a(n) __________ electron geometry.
octahedral
Based on the electronegativity difference between carbon and oxygen, the bonds in carbon dioxide are _______.
polar
he difference in electronegativity signifies that the hydrogen-oxygen bond is _______.
polar
Determine the molecular geometry and make a sketch of the molecule or ion using the bond conventions in Section 10.4: SF4
seesaw
Draw the Lewis structure for SO3. What is the hybridization on the S atom?
sp2
Draw the Lewis structure for BrO4⁻. What is the hybridization on the Br atom?
sp3
Draw the Lewis structure for OF2. What is the hybridization on the O atom?
sp3