1. Ch. 8 Clicker Review

2. Transferring of electrons between atoms would describe a(n)
A. splitting bond
B. ionic bond
C. covalent bond
D. molecular bond ☺

3. Intermolecular forces are ___ than ionic or covalent bonds
A. stronger
B. weaker
C. narrower
D. shorter ☺

4. When a metal and a nonmetal form a bond you would expect what type of bond?☺
A. ionic
B. covalent
C. metallic
D. molecular

5. Dipole interactions are weak attractions between
A. non polar molecules
B. ions
C. neutrons
D. polar molecules ☺

6. When two nonmetals form a bond, you would expect
A. transfer of electrons for a covalent bond
B. sharing of electrons for an ionic bond
C. sharing of electrons for a covalent bond
D. transfer of electrons for an ionic bond ☺

7. Electrons can be lost, shared or ____ during bonding processes.☺
A. gained
B. demoted
C. emitted
D. spun off

8. Which of the following would contain an ionic bond?
A. HCl
B. MgCl2
C. N2
D. SiH4 ☺

9. What is the shape of NH3? ☺ A. bent B. trigonal planar C. tetrahedral
D. pyramidal ☺

10. What is the shape of H2O? ☺ A. Bent B. Linear C. trigonal planar
D. pyramidal

11. What is the shape of CH4? ☺ A. pyramidal B. tetrahedral
C. trigonal planar
D. bent ☺

12. What is the shape of SiO2? ☺ A. Linear B. Bent C. trigonal planar
D. pyramidal

13. Which element will form a covalent bond with oxygen?
A. neon
B. phosphorus
C. potassium
D. magnesium ☺

14. Ionic compounds generally have __ melting points than covalent compounds?
A. lower
B. higher
C. less predictable
D. less consistant ☺

15. Van der Waals forces include
A. dipole interactions only
B. dipole interactions and dispersion forces only
C. dipole interactions and hydrogen bonding only
D. hydrogen bonding and dispersion forces only ☺

16. When nitrogen triple bonds with another nitrogen atom, there are/is
A. no lone pairs of electrons on either nitrogen atom
B. two lone pairs of electrons on each nitrogen atom
C. one lone pair of electrons on each nitrogen atom
D. one lone pair of electrons on only one of the nitrogen atoms ☺

17. What types of bonds can be found in a solid sample of H2S?
A. covalent bonding only
B. both ionic and covalent bonding
C. hydrogen bonding only
D. both covalent and hydrogen bonding ☺

18. Which structure is nonpolar?B. C. D. ☺

19. Which element does not naturally occur as a diatomic molecule?
A. H
B. Br
C. N
D. C ☺

20. The reason a water skimmer/strider can walk on water is because of
A. dispersion forces
B. hydrogen bonds
C. electric fields
D. van der Waals forces ☺

21. What is the shape of SiO32-?☺
A. trigonal planar
B. bent
C. pyramidal
D. tetrahedral

22. Hydrogen bonding always involves
A. non polar molecules
B. hydrogen
C. neutrons
D. dispersion forces ☺

23. Which of the following would be nonpolar?
A NF3
B. H2Se
C. SiH4
D. H2S ☺

24. What type of bonds are in ethanol?
A. ionic
B. nuclear
C. metallic
D. covalent ☺

25. Which of the following would be polar?
A. He
B. N2
C. SiO2
D. SeO2 ☺

26. The lewis dot structure for a molecule of SiO32- would have
A. 3 single bonds
B. 2 single bonds and two double bonds
C. 1 single bonds and two double bonds
D. 2 single bonds and 1 double bond ☺

27. What type of bond forms in N2, Br2 and O2
A. an ionic bond formed by the gain of electrons
B. a covalent bond formed by the sharing of electrons
C. a metallic bond formed by the transfer of electrons
D. a nuclear bond formed by the sharing of electrons ☺

28. If all of the electrons are distributed ____ in a molecule, the molecule is non-polar.☺
A. equally
B. within p orbitals
C. unequally
D. randomly

29. Hydrogen bonding is the ___ intermolecular force
A. evasive
B. strongest
C. least polar
D. weakest ☺

30. Which compound would have a covalent bond?
A. CaBr2
B. KCl
C. PO
D. NaBr ☺

31. This shows the formation of a _____ bond.☺
A. non polar covalent
B. polar covalent
C. metallic
D. non polar ionic

32. How many bonds are shown in the structural formula below?
A. 1 covalent, 8 ionic
B. one double covalent, 8 ionic
C. 8 double covalent, 1 single covalent
D. 1 double covalent, 8 single covalent ☺

33. When a molecule is polar, it behaves as if one end of the molecule is ___ and the other end of the molecule is ___. ☺
A. negative, positive
B. magnetic, nonmagnetic
C. ionic, nonionic
D. neutral, positive