Chem 1405 Test 1
The following questions are a mixture of multiple choice, True or False and
short answer type questions.
Each question carries 1 points. The Test is for 40 points.
This is not an open book, so try to answer this test in the time limit given.
1. Which of the following is an example of a physical property?
A) corrosiveness of sulfuric acid
B) toxicity of cyanide
C) flammability of gasoline
D) neutralization of stomach acid with an antacid
E) lead becomes a liquid when heated to 601oC
2. Dry ice (carbon dioxide) changes from a solid to a gas at –78.5°C. What is this temperature in °F?
A) –173°F
B) –12.6°F
C) –109°F
D) –75.6°F
E)
none of them are within 2°F of the right answer
3. The SI prefixes micro and milli represent, respectively:
A) 106 and 10–6.
D) 10–3 and 109.
–3
6
B) 10 and 10 .
E) 10–6 and 10–3.
C)
103 and 10–6.
4. Which of the following objects will sink when dropped into a bucket of water?
(Given: density of water = 1.00 g/cm3)
A) a cube of aluminum (density = 2.702 g/cm3)
B) a diamond (density = 3.51 g/cm3)
C) a chunk of dry ice (density = 1.56 g/cm3)
D) a chunk of sodium (density = 0.91 g/cm3)
E) a sphere of magnesium (density = 1.74 g/cm3)
5. Give the correct number of significant figures and units to the problem below.
56 mm + 4.5 m =
A) 61 mm B) 61 m C) 61 m2 D) 4.6 m E) 4.56 m
6. Radio waves travel at the speed of light, which is 3.00 × 108 m/s. How many kilometers will radio
messages travel in exactly one year?
A) 9.46 × 1015 km
D) 9.46 × 1012 km
8
B) 7.30 × 10 km
E) 3.33 × 10–3 km
C)
7.10 × 1010 km
7. Which of the following speeds is the greatest? (1 mile = 1609 m)
A) 40 mi/h
D) 0.74 km/min
B) 2.0 × 105 mm/min
E) 400 m/min
C)
40 km/h
8. 1.572 × 108 troy oz of silver were used in the United States in 1980. How many kilograms is this? (1 troy
oz = 31.1 g)
A) 4.89 × 106 kg
D) 4.89 x 1012 kg
B) 4.89 kg
E) 5.05 × 10 3 kg
6
C)
5.05 × 10 kg
9. Atoms of the same element with different mass numbers are called
A) ions. B) neutrons. C) allotropes. D) chemical families.
E) isotopes.
10. A cation is defined as
A) a charged atom or group of atoms with a net negative charge.
B) a stable atom.
C) a group of stable atoms.
D) an atom or group of atoms with a net positive charge.
11. Which one of the following elements is most likely to form a 2+ ion?
A) calcium B) carbon C) fluorine D) oxygen E) sodium
12. Although mercury is a metal, it is a liquid.
A. True
B.False
13. Which of the following statements regarding conversion factors is NOT true?
a.
They don’t change the intrinsic value of a measurement.
b.
They do change the scale (units) of a measurement.
c.
They don’t change the number of significant figures in a measurement.
d.
They are equivalent to multiplying a measurement by one.
14. Which element is a nonmetal?
a. a. sodium (Na)
b. iron (Fe)
c. europium (Eu)
d. sulfur (S)
15. Which statement best describes the octet rule?
a.
Atoms will lose a maximum number of electrons during a chemical reaction.
b.
Atoms react in order to obtain eight electrons in their valence shell.
c.
Atoms will react until they have a total of eight electrons.
d.
Atoms will react in order to obtain the electron configuration of the nearest noble gas.
16. An atom can either lose or gain electrons to attain the electronic configuration of a noble element. This
statement is
A. True
B. False
17. The electronic configuration of Ca is :
18. The electronic configuration of O2- is :
19. Which of the following is the correct name of Mg3N2?
a.
magnesium nitrogen
b.
magnesium nitride
c.
magnesium (II) nitride
d.
trimagnesium dinitride
20. How many bonds will nitrogen form in a Lewis structure?
a.
1
b.
2
c.
3
d.
4
21. The elcetronegativity of elements changes from the left to right of the periodic table in this way:
a. Increase
b. Decreases
c. Does not change
22. In writing the chemical formula of a compound such as Al2O3, the following statement is a true
relationship between the Al and O atoms:
a. Al and O share equal number of electrons
b. Al donates 3 electrons and O donates 2 electrons
c. Each Al donates 3 electrons and each O accepts 2 electrons
d. Al accepts 4 electrons and O accepts 6 electrons
23. An example of a compound formed by covalent bonding is:
a. H2CO3
b. CH4
c. NaCl
d. O2
24. An example of a compound formed by molecular bonding is:
a. H2CO3
b. CH4
c. NaCl
d. O2
25. An example of a compound formed by inoic bonding is:
a. H2CO3
b. CH4
c. NaCl
d. O2
26. The reason some elements have multiple valencies is because-
27. Write the Lewis structure of
A. CHCl3
2
1X3
B. H2O
C.
28. The dipole moment of a compound depends on the resultant partial charges based on the
electronegativities of the individual constituents present in the compound.
Based on this definition, write the resulting dipole moment in the following compounds:
A. CO
B. SrF
1X3
C. CH3OH
29. C is unique in its ability to form single , double and triple bonds with another C atom. Predict the structure
of the following compounds 1X3
A. CH4
B. C2H4
30. Classify the following as ionic, polar covalent or nonpolar covalent:
1X4
A. CH3OH
B. C2H4
C. BaCl2
D. PCl5
C. C2H2