Unit 3 Practice Test
1. A cation typically forms when an element has _____________________.
a. a high ionization energy and a
c. a low ionization energy and a
high electron affinity
high electron affinity
b. a high ionization energy and a
d. a low ionization energy
low electron affinity
and a low electron affinity
2. Potassium is likely to ____________________ electrons in a bond.
a. gain
d. none of the above; potassium
b. lose
is nearly stable
c. share
3. Sulfur is likely to ____________________ electrons is an ionic bond.
a. gain
c. share
b. lose
d. none of the above
4. Which of the following need Roman numerals included when writing the
name of the compound?
a. Potassium
c. Strontium
b. Tin
d. Silver
5. If the charge for a oxygen atom is –2, how many electrons are
transferred to form the ion?
a. 1
c. 3
b. 2
d. 7
6. The ionic compound, Ca(NO3)2 is named _____________________.
a. Calcium nitrite
c. Calcium nitrate
b. Calcium nitride
d. Calcium nitrogen trioxide
7. Which of the following is incorrect?
a. Na2SO4
b. KCl
c. Na2NO3
d. FeCl3
8. How many carbonate ions are in CaCO3?
a. 1
c. 3
b. 2
d. 4
9. A molecule (aka. covalent compound)has atoms bonded by ________.
a. electrostatic attraction
c. electrons being shared
between positive and negative
between two atoms who
ions
need electrons
b. electrons being gained and
d. both a and b
lost
10. CF4 is named ___________________________________________.
a. carbon fluoride
c. carbon tetrafluorine
b. carbon fluoride
d. carbon tetrafluoride
11. HI is named __________________________________________.
a. hydrogen iodide
c. hydroiodic acid
b. hydrogen hypoiodite
d. iodic acid
12. Sulfur dioxide contains _________________ double bonds.
a. 0
c. 2
b. 1
d. 3
13. The common name of SiI4 is tetraiodosilane. What is its covalent
compound name?
a. silane tetraiodide
c. silicon iodide
b. silane tetraiodine
d. silicon tetraiodide
14. HClO2 is called _________________________________________.
a. hydrogen chlorate
c. chloric acid
b. hydrogen chlorite
d. chlorous acid
15. Which of the following compounds contains the copper (I) ion?
a. CuO
c. CuS
b. CuF2
d. CuCl
16. Name the following compound: HBr
a. monohydrogen monobromide
b. hydrogen monobromide
c. bromic acid
d. hydrobromic acid
17. If a Lewis structure has 4 regions of electron density surrounding the
central atom, 3 are bonding pairs and 1 is a lone pair, what shape would
you expect the molecule to have?
a. bent
c. tetrahedral
b. trigonal pyramidal
d. trigonal planar
18. When a double covalent bond is formed, two electrons are shared.
a. True
b. False
19. Which of the following elements normally exists in the form of diatomic
molecules?
a. argon
c. nitrogen
b. iron
d. helium
20. Which of the following molecules contains a triple bond?
a. Methane (CH4)
c. carbon dioxide
b. nitrogen gas
d. oxygen
21. The suffix for an oxyacid that contains an anion ending in –ite is –ous.
a. True
b. False
22. Which of these is not an ionic compound?
a. KF
c. SiO2
b. Na2SO4
d. Na2O
23. What is the shape of a hydrosulfuric acid molecule? (HINT: Draw the
Lewis structure.)
a.
b.
c.
Linear
Trigonal planar
Trigonal pyramidal
d.
e.
Bent
Tetrahedral
Part Two: Short Answer
24. Name the following ionic compounds.
a. FeBr3
___Iron bromide_________________________
b. MgCO3
__Magnesium carbonate____________________________
25. Name the following covalent compounds.
a. P2O5
___diphosporous pentoxide_________________________
b. NO
___nitrogen monoxide__________________________
26. Name the following compounds.
a. SeCl2 ____selenium dichloride_______________________________
b. H2Se
____hydroselenic acid_________________________________
c. PCl3
____phosporous trichloride______________________________
d. LiCl
____Lithium chloride___________________________
Part Three: Discussion
27. Draw the Lewis structures for the following compounds. Then, predict
the polarity of the molecule, shape of the molecule, and type of IMF:
a. SO2
b. SO4-2
c. CI4
d. Hydroselenic acid
27. Which of the compounds in the question above will be the easiest to
boil?
The one with the weakest intermolecular forces will boil first.
Hydroselenic acid and sulfur dioxide are both polar so they have the
stronger dipole-dipolee IMF. SO42- is an ion so it only exists in a solution
with water or as part of an ionic bond with a metal (solid) therefore it itself
cannot boil. CI4 is symmetric with no lone pairs, therefore it is nonpolar
and the weak London dispersion forces are the only forces holding the
molecules together. CI4 will be the easiest to boil