NAME________________________________
TEST: BONDING AND NOMENCLATURE
Multiple Choice
Directions: Each set of lettered choices below refers to the numbered statements immediately
following it. Select the one lettered choice that best fits each statement. A choice may be used once,
more than once, or not at all in each set.
Questions 1-5 refer to the following molecules.
(A)
CO2
(B)
H2O
(C)
CH4
(D)
C2H4
(E)
PH3
1.
2.
3.
4.
5.
This molecule has exactly one double bond.
This molecule contains the most polar bond.
This molecule has an atom with trigonal pyramidal geometry.
This molecule is commonly known as methane.
This molecule contains an atom with a hybridization of sp.
Questions 6-8
(A)
F
(B)
N
(C)
Mg
(D)
Cr
(E)
Mn
6. Only forms monatomic ions with 2+ charge in solutions.
7. Forms a compound having the formula K2XO4
8. Forms oxides that are common air pollutants and that yield acidic solution in water.
Questions 9-12
(A) SO32(B) NO31(C) PO43(D) SCN1(E) H3O+
9. This molecule forms a trigonal planar geometry.
10. This molecule does not require resonance to accurately describe its bonding.
11. When this molecule bonds with hydrogen, it forms an acid which is named phosphoric acid.
12. The central atom of this molecule has sp type hybridization.
Directions: Each of the questions or incomplete statements below is followed by five suggested
answers or compilations. Select the one that is best in each case and then blacken the corresponding
space on the answer sheet.
13. Which of the following correctly identifies the formula for copper (II) dichromate
(A)
(B)
(C)
(D)
(E)
Cu2Cr2O7
Cu(CrO4)2
CoCr2O7
CuCr2O7
Co2(CrO4)2
14. Of the following compounds, which is the most ionic?
(A)
(B)
(C)
(D)
(E)
SiCl4
BrCl
PCl3
Cl2O
CaCl2
15. According to the VSEPR model, the progressive decrease in the bond angles in the series of
molecules CH4, NH3, and H2O is best accounted for by the
(A)
(B)
(C)
(D)
(E)
increasing strength of the bonds.
decreasing size of the central atom.
increasing electronegativity of the central atom.
increasing number of unshared pairs of electrons.
decreasing repulsion between hydrogen atoms.
16. Types of hybridization exhibited by the C atoms in propene, CH3CHCH2, include which of the
following?
I. sp
II. sp2
III. sp3
(A) I only
(B) III only
(C) I and II only
(D) II and III only
(E) I, II, and III
17. The SbCl5 molecule has trigonal bipyramid structure. Therefore, the hybridization of Sb
orbitals should be
(A) sp2
(C) sp2d
(E) sp3d2
(B) sp3
(D) sp3d
18. CCl4, CO2, PCl3, PCl5, SF6
Which of the following does NOT describe any of the molecules above?
(A) Linear
(D) Tetrahedral
(B) Octahedral
(E) Trigonal pyramidal
(C) Square planar
19. Which of the following compounds is ionic and contains both sigma and pi covalent bonds?
(A) Fe(OH)3
(C) H2S
(E) NaCN
(B) HClO
(D) NO2
20. The most correct name for FeSO3 is:
(A) Iron sulfate
(C) Iron sulfite
(B) Iron (II) sulfate
(D) Iron (III) sulfite
(E) Iron (II) sulfite
21. The geometry of the SO3 molecule is best described as
(A) trigonal planar
(D) bent
(B) trigonal pyramidal
(E) tetrahedral
(C) square pyramidal
22. Which of the following molecules has the shortest bond length?
(A) N2
(C) Cl2
(E) I2
(B) O2
(D) Br2
23. Pi (π) bonding occurs in each of the following species EXCEPT.
(A) CO2
(C) CN(E) CH4
(B) C2H4
(D) C6H6
24. Which of the following has a zero dipole moment?
(A) HCN
(C) SO2
(E) PF5
(B) NH3
(D) NO2
25. For which of the following molecules are resonance structures necessary to describe the
bonding satisfactorily?
(A) H2S
(C) CO2
(E) PF3
(B) SO2
(D) OF2
Free Response:
Directions: Using the paper provided, answer each of the following questions clearly showing the
methods you use and the steps involved at arriving at the answers.
1. Answer the following questions using principles of chemical bonding and molecular structure.
a. Consider the carbon dioxide molecule, CO2, and the carbonate ion, CO32–.
i. Draw the complete Lewis electron-dot structure for each species.
ii. Account for the fact at the carbon-oxygen bond length in CO32– is greater than
the carbon-oxygen bond length in CO2.
b. Now consider the sulfate ion SO42- and the iodine trifluoride molecule IF3.
i. Draw the complete Lewis electron-dot structure for each ion/molecule.
ii. In terms of molecular geometry, account for the fact that the SO42- ion is
nonpolar, whereas the IF3 molecule is polar.
2. Using dot structures and words completely compare and contrast ionic bonds and covalent
bonds.
3. Completely fill in the table below. (Hint: For Ca(SCN)2 do not include the Ca when
considering the shape, hybridization or polarity.)
Name
Chemical
formula
Lewis structure
Hybridization
Ammonia
Ca(SCN)2
Nitrous Acid
ClBr3
sp3d2
Molecular
shape
Polar?