Name: Nihal Ahmed
Class:3B
1. The force between two bodies having identical electric charges
A) is a force of repulsion
B) is a force of repulsion if the charges are negative, and one of attraction if they are
positive
C) increases as the bodies are moved further apart
D) is independent of the distance between them
E) is directly proportional to the distance between them
2. Which of the following groups contains no ionic compounds?
A) HCN, NO2, Ca(NO3)2
B) PCl5, LiBr, Zn(OH)2
C) KOH, CCl4, SF4
D) NaH, CaF2, NaNH2
E) CH2O, H2S, NH3
3. In which pair do both compounds exhibit predominantly ionic bonding?
A) SCl6 and HF
B) Na2SO3 and NH3
C) KI and O3
D) LiF and H2O
E) LiBr and MgO
4. When a metal reacts with a nonmetal a covalent bond is formed.
5. A nonpolar covalent bond results from the unequal sharing of a pair of electrons between
atoms in a molecule.
6.
Atoms having equal or nearly equal electronegativities are expected to form
A) no bonds
B) polar covalent bonds
C) nonpolar covalent bonds
D) ionic bonds
E) covalent bonds
7. Choose the compound with the most ionic bond.
A) LiCl
B) KF
C) NaCl
D) LiF
E) KCl
8. Atoms with greatly different electronegativity values are expected to form
A) no bonds
B) covalent bonds
C) triple bonds
D) ionic bonds
E) none of these
9. Which of the following bonds is least polar?
A) C—O
B) H—C
C) S—Cl
D) Br—Br
E) They are all nonpolar.
10. For the elements Cs, F, and P, the order of increasing electronegativity is:
A) Cs < F < P
B) Cs < P < F
C) P < F < Cs
D) F < Cs < P
E) none of these
11. For the elements Cs, F, and Cl, the order of increasing electronegativity is:
A)
B)
C)
D)
E)
F < Cl < Cs
Cs < Cl < F
Cl < Cs < F
F < Cs < Cl
none of these
12. In the gaseous phase, which of the following diatomic molecules would be the most polar?
A) CsF
B) CsCl
C) NaCl
D) NaF
E) LiF
13. Based on electronegativities, which of the following would you expect to be most ionic?
A) N2
B) CaF2
C) CO2
D) CH4
E) CF4
14. In which case is the bond polarity incorrect?
A) +H–F–
B) +K–O–
C) +Mg–H–
D) +Cl–I–
E) +Si–S–
15. Metals typically have
A) high
B) low
C) negative
D) no
E) two of these
electronegativity values.
16. The electron pair in a C-F bond could be considered
A) closer to C because carbon has a larger radius and thus exerts greater control over
the shared electron pair
B) closer to F because fluorine has a higher electronegativity than carbon
C) closer to C because carbon has a lower electronegativity than fluorine
D) an inadequate model since the bond is ionic
E) centrally located directly between the C and F
17. Based on electronegativity differences, which of the following is most likely to be ionic?
A) CaF2
B) Br2
C) BH3
D) NO
E) CF4
18. What is the correct order of the following bonds in terms of decreasing polarity?
A) N-Cl, P-Cl, As-Cl
B) P-Cl, N-Cl, As-Cl
C) As-Cl, N-Cl, P-Cl
D) P-Cl, As-Cl, N-Cl
E) As-Cl, P-Cl, N-Cl
19. Which of the following bonds would be the most polar without being considered ionic?
A) Mg-O
B) C-O
C) O-O
D) Si-O
E) N-O
20. Which of the following bonds would be the least polar, yet still be considered polar
covalent?
A) Mg-O
B)
C)
D)
E)
C-O
O-O
Si-O
N-O
21. In which of the following compounds does the bond between the central
atom and bromine have the greatest ionic character?
A) LiBr
B) KBr
C) SeBr2
D) AsBr3
E) CaBr2
22. Which of the following statements is incorrect?
A) Ionic bonding results from the transfer of electrons from one atom to another.
B) Dipole moments result from the unequal distribution of electrons in a molecule.
C) The electrons in a polar bond are found nearer to the more electronegative element.
D) A molecule with very polar bonds can be nonpolar.
E) Linear molecules cannot have a net dipole moment.
23. Which of the following molecules has no dipole moment?
A) CO2
B) NH3
C) H2O
D) all
E) none