Name ____________________________________________________
Unit 5: Bonding – Covalent & Intermolecular
Date ________________________________
Multiple Choice Questions
1. Which pair of atoms is held together by a covalent bond?
(1) HCl
(2) LiCl
(3) NaCl
(4) KCl
2. As a bond between a hydrogen atom and a sulfur atom is formed, electrons are
(1) shared to form an ionic bond
(2) shared to form a covalent bond
(3) transferred to form an ionic bond (4) transferred to form a covalent bond
3. Which statement describes a multiple covalent bond?
(1) Two electrons are shared.
(2) Four electrons are shared.
(3) Two electrons are transferred.
(4) Four electrons are transferred.
4. What is the total number of electrons shared in a triple covalent bond?
(1) 2
(2) 4
(3) 3
(4) 6
5. Which terms describe a substance that has a low melting point and poor electrical
conductivity?
(1) covalent and metallic
(2) covalent and molecular
(3) ionic and molecular
(4) ionic and metallic
6. Which compound contains both ionic and covalent bonds?
(1) KI
(2) CaCl2
(3) CH2Br2
(4) NaCN
7. Which substance contains nonpolar covalent bonds?
(1) H2
(2) H2O
(3) Ca(OH)2
(4) CaO
8. The electrons in a bond between two chlorine atoms are shared
(1) unequally, and the resulting bond is polar
(2) unequally, and the resulting bond is nonpolar
(3) equally, and the resulting bond is nonpolar
(4) equally, and the resulting bond is polar
9. What type of bond exists in a molecule of hydrogen iodide?
(1) a polar covalent bond with an electronegativity difference of zero
(2) a polar covalent bond with an electronegativity difference between zero and 1.7
(3) a nonpolar covalent bond with an electronegativity difference of zero
(4) a nonpolar covalent bond with an electronegativity difference between zero and 1.7
10. Which substance is correctly paired with its type of bonding?
(1) NaBr – nonpolar covalent
(2) HCl – nonpolar covalent
(3) NH3 – polar covalent
(4) Br2 – polar covalent
11. Which of these formulas contains the most polar bond?
(1) HBr
(2) HCl
(3) HF
(4) HI
12. Which statement explains why a C-O bond is more polar than a F-O bond?
(1) At STP, carbon has a greater density than fluorine.
(2) A carbon atom has more valence electrons than a fluorine atom.
(3) The difference in electronegativity between carbon and oxygen is greater than that
between fluorine and oxygen.
(4) The difference in first ionization energy between carbon and oxygen is greater than
that between fluorine and oxygen.
13. Which statement explains why a CO2 molecule is nonpolar?
(1) Carbon and oxygen are both nonmetals.
(2) Carbon and oxygen have different electronegativities.
(3) The molecule has a symmetrical distribution of charge.
(4) The molecule has an asymmetrical distribution of charge.
14. Which formula represents a nonpolar molecule containing polar covalent bonds?
(1) H2O
(2) CH4
(3) NH3
(4) H2
15. Which formula represents a polar molecule?
(1) O2
(2) CO2
(3) NH3
(4) CH4
16. Which structural formula represents a linear nonpolar molecule containing two polar
bonds?
(1)
(2)
(3)
(4)
17. Which formula represents a tetrahedral molecule?
(1) CH4
(2) CaCl2
(3) HBr
(4) Br2
18. Which molecules are held together by dipole-dipole forces?
(1) H2
(2) N2
(3) CH4
(4) HCl
19. At 25C, iodine exists as a solid and bromine exists as a liquid. This difference in
phase is due to the presence of stronger
(1) covalent bonds in iodine
(2) covalent bonds in bromine
(3) van der Waals forces in iodine
(4) van der Waals forces in bromine
20. Van der Waals forces of attraction between molecules always decreases with
(1) increasing molecular size and increasing distance between the molecules
(2) increasing molecular size and decreasing distance between the molecules
(3) decreasing molecular size and increasing distance between the molecules
(4) decreasing molecular size and decreasing distance between the molecules
21. When the atoms of the elements in Group 17 are compared in order from top to
bottom, the attractions between the atoms of each successive element
(1) increase and the boiling point decreases
(2) decrease and the boiling point increases
(3) increase and the boiling point increases
(4) decrease and the boiling point decreases
22. The table below shows the normal boiling point of four compounds.
Which compound has the strongest intermolecular forces?
(1) HF
(2) CH3Cl
(3) CH3F
(4) HCl
23. When compared to H2S, H2O has a higher boiling point because it contains stronger
(1) metallic bonds (2) covalent bonds (3) ionic bonds
(4) hydrogen bonds
24. Which compound has the strongest hydrogen bonding at STP?
(1) H2O
(2) H2S
(3) H2Se
(4) H2Te
25. In an aqueous solution of an ionic salt, the oxygen atom of the water molecule is
attracted to the
(1) negative ion of the salt, due to oxygen’s partial positive charge
(2) negative ion of the salt, due to oxygen’s partial negative charge
(3) positive ion of the salt, due to oxygen’s partial positive charge
(4) positive ion of the salt, due to oxygen’s partial negative charge
26. Molecule-ion attractions are present in
(1) NaCl (aq)
(2) HCl (g)
(3) CCl4 ()
(4) KClO3 (s)