Chemistry Semester Test Practice
January 2012
Use the following choices to answer questions 1 – 3.
A. Solids only.
B. Liquids only.
C. Gases only.
D. Both solids and liquids.
E. Both liquids and gases.
____
1.
This phase (or state) of matter has definite shape and definite volume.
____
2.
This phase (or state) of matter does not have a definite shape and does not have a
definite volume.
____
3.
This phase (or state) of matter does not have a definite shape, but does
have a
definite volume.
----------------------------------------------------------------------------------------------------------------------------____
4.
Dalton's theory essentially agreed with modern atomic theory EXCEPT for the
statement that
A. all atoms of the same element have the same mass.
B. all matter is made up of small particles called atoms.
C. atoms of the same element are chemically alike.
____
5.
According to Dalton's atomic theory, atoms
A. Can be created or destroyed in chemical reactions.
B. of a given element are identical in size, mass, and other properties.
C. can be divided in smaller parts.
____
6.
Dalton's atomic theory helped to explain the law of conservation of mass
because it stated that atoms
A. Could not combine to form compounds.
B. All have the same mass.
C. Cannot be created or destroyed.
____
7.
Using the octet rule, how many electrons will nitrogen attempt to gain when
combined with another atom.
A. 2
B. 3
C. 5
D. 8
____
8.
Describe the octet rule in terms of noble gas configurations.
A. Atoms do not lose or gain electrons.
B. Elements will gain or lose electrons to form a noble gas configuration.
C. Atoms can gain up to ten electrons.
_____
9. Describe the octet rule in terms of potential energy
A. The 9 outer electrons are referred to as an octet
B. Atoms that meet the octet rule are stable because their valence electrons have a
relatively low potential energy
C. Atoms that meet the octet rule are stable because their valence electrons have a
relatively high potential energy.
____
10.
The three types of nuclear radiation in increasing order of penetrating power
are ____.
A. alpha, gamma, beta
B. alpha, beta, gamma
C. X-ray, beta, gamma
____
11.
Identify the alpha particle
A.
____
12.
13.
14.
47
C.
6
15.
He
B. γ
0
-1 β
C.
210
106
14
Po --> 82206Pb +
Ag +
C
7
0
-1 e
14
N+
2
4
He
 46106Pd
0
--1 β
The electrons involved in the formation of a chemical bond are called
Dipoles.
valence electrons.
s electrons.
Inner shell electrons.
What is the name of the compound with the formula NaCl?
A.
B.
C.
D.
____
84
B.
A.
B.
C.
D.
_____
4
Identify the beta decay emission.
A.
_____
2
sodium chloride
chlorine sodiate
sodium chlorate
monosodium chloride
A group of covalently bonded atoms that acts together as one charged atom is a ___.
A. crystal
B. polyatomic ion
C. negative ion
D. molecule
16. Define the ionic charge for the following elements:
Li = ____
____
Mg = ____
B = ____
Si = ____
N = ____
Cl = ____.
17. What is the electron configuration for nitrogen?
A. 1s2 2s2 2p3
B. 1s2 2s3 2p1
C. 1s2 2s3 2p2
____
18. The element with electron configuration 1s2 2s2 2p6 3s2 3p2 is
A. Si
B. S
C. Mg
D. Se
19. Write the electron configuration for Manganese.
_______________________________________________
20. Which element has the following electron configuration: [Kr] 5s2 4d10 5p3?
__________
____
A.
B.
C.
D.
E.
____
A.
B.
C.
D.
E.
21. Which of the following elements is a noble gas?
Gold
Oxygen
Krypton
Chlorine
Radium
22. Which of the following elements is an alkaline earth metal?
Gold
Chlorine
Krypton
Radium
Oxygen
____
23. The elements with the smallest atomic radii are found in the:
A.
B.
C.
D.
____
24. The elements with the largest first ionization energy are found in the:
A.
B.
C.
D.
____
lower right-hand corner of the periodic table
upper right-hand corner of the periodic table
lower left-hand corner of the periodic table
upper left-hand corner of the periodic table
lower right-hand corner of the periodic table
upper right-hand corner of the periodic table
lower left-hand corner of the periodic table
upper left-hand corner of the periodic table
25. The elements in which group have only 1 electron in the s sublevel?
A. Halogens
B. Noble gases
C. Alkali Metals
D. Transition Metals
____
26. An element with the electron configuration 1s22s22p5 belongs to the:
A.
B.
C.
D.
E.
____
27. Low ionization energies are most characteristic of:
A.
B.
C.
D.
____
halogen group
alkali metal group
nobel gas group
transition metal group
alkaline earth metal group
Noble gases
Metalloids
Halogens
Metals
28. Which of the following if the correct compound formula for iron(II) phosphide?
A.
B.
C.
D.
Fe2P3
Fe3P2
FeP
Fe2P
29. Write the correct formula for the following compounds:
ammonium phosphate
potassium sulfide
________________________
________________________
carbon tetrachloride
________________________
magnesium nitrate
________________________
lead (III) chloride
________________________
____
30. What is the formula for dinitrogen trioxide?
A.
Ni2O3
B. N2O6
C. N2O3
D. N3O2
____ 31. What is the name of the compound Fe2O3?
A. iron oxide
B. Diiron trioxide
C. Iron (II) oxide
D. Iron (III) oxide
____
32. What is the name of the compound NH4C2H3O2?
A. Ammonium acetate
B. Diammonium diacetate
C. Nitroge tetrahydride dicarbide trihydride dioxide
D. Ammonium penta-acetate
____
33. What is the name of the compound AlCl3?
A. Aluminum trichloride
B. Aluminum (III) chloride
C. Aluminum chloride
D. Aluminum chlorate
34. Which is the electron dot formula for water?
______________
35. Which is the electron dot formula for CH4?
______________
36. Which is the electron dot formula for nitrogen trifluoride?
_______________
____
37. Which of the following is an intensive property?
A. Mass
____
D. Length
B. Chemical Composition
C. Color
D. Mass
B. Chemical Composition
C. Color
D. Mass
40. Which of the following is NOT an extensive property?
A. Mass
____
Density
39. Which of the following is NOT an intensive property?
A. Density
____
C.
38. Which of the following is an extensive property?
A. Density
____
B. Volume
B. Volume
C. Density
D. Length
41. What is the frequency (λ) of a light that has an energy (E) of 3.14 x 10 -12 J?
A. 2.08 x 10-45
B. 4.74 X 1021
C. 4.74 x 10-47
D. 1.05 x 10-20
____
42. What is the frequency (λ) of a light that has a wavelength of 3.25 X 10-8 m?
A. 9.23 x 1015
B. 9.75
C. 1.08 X 10-16
D. 2.15 x 10-41
____
43. What is the wavelength (ν) in meters of a light that has energy (E) of 2.62 x 10-13?
A. 6.626 x 10-34
B. 1.19 X 1029
C. 7.86 x 10-5
D. 1.73 x 1054
____
44. Balance the following chemical reaction: HCl + Zn  ZnCl + H2
A. 2 HCl + Zn  2 ZnCl + H2
B. 2 HCl + Zn  ZnCl + 2 H2
C. HCl + 3 Zn  3 ZnCl + H2
D. 2 HCl + 2 Zn  2 ZnCl + H2
____
45. Balance the following chemical reaction: Ag(NO 3) + AlCl3  AgCl + Al(NO3)3
A. 3 Ag(NO3) + AlCl3  AgCl + 3 Al(NO3)3
B. 2 Ag(NO3) + 3 AlCl3  3 AgCl + 2 Al(NO3)3
C. Ag(NO3) + 2 AlCl3  AgCl + 2 Al(NO3)3
D. Ag(NO3) + 3 AlCl3  2 AgCl + 3 Al(NO3)3
____
46. Balance the following chemical reaction: CH 4 + O2  CO2 + H2O
A. CH4 + 3 O2  CO2 + 2 H2O
B. CH4 + 2 O2  CO2 + 2 H2O
C. 3 CH4 + O2  CO2 + 2 H2O
D. 2 CH4 + O2  CO2 + 2 H2O
Define each type of radioactive decay, describe what type of particle each type of decay gives off
and if any energy is given off, then complete the following reactions based on their type of
radioactive decay.
47. Alpha decay:
251
98Cf

48. Beta decay:
198
79Au

49. Neutron decay:
242
94Pu

50. Gamma:
Using VSEPR, draw the lewis dot structure and name the molecular geometry of the following
compounds
51. NF3
52. CH4
53. Se02
54. BF3
55.
A contains three different solutions with various densities. Solution A has a density
of 5 g/ml, Solution B has a density of 10 g/ml, and Solution C has a density of 28 g/ml. How
will the solutions be arranged within a graduated cylinder?
56.
What would happen if you poured two liquids into a container at the same time, one
density of 2.5g/mL and one with a density of 3.4g/mL?
____
57.
This method for separating mixtures will separate the undissolved solid
particles by pouring the liquid through porous paper.
A. Filtration
B. Crystallization
C. Chromotography
____
58.
This method will separate a mixture of liquids based on their boiling
temperatures, like getting gasoline and diesel out of crude oil .
A. Distillation
B. Crystallization
C. Chromatography
59. Define fusion and give one example.
60. Define fission and give one example.
61. What are four basic ways to separate mixtures?
with a