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AP Chemistry Unit 1 Test

Total questions: 100

Worksheet time: 2hrs 23mins

Name
Class
Date
1.

Mass spectroscopy graphs measure ______________

a)

boiling points of hydrocarbons

b)

ionization energies of electrons

c)

atomic masses of isotopes

d)

numbers of electrons in each sublevel

2.

2) What is the physical state in which matter has no specific shape but does have a specific volume?

a)

A) gas

b)

B) solid

c)

C) liquid

d)

D) salts

e)

E) ice

3.

9) Which one of the following is a pure substance?

a)

A) concrete

b)

B) wood

c)

C) salt water

d)

D) elemental copper

e)

E) milk

4.

Isotopes of an element have the same number of _______, but different numbers of _________.

a)

neutrons

protons

b)

protons

neutrons

c)

protons

electrons

d)

electrons

protons

5.

14) An element cannot __________.

a)

A) be part of a heterogeneous mixture

b)

B) be part of a homogeneous mixture

c)

C) be separated into other substances by chemical means

d)

D) interact with other elements to form compounds

e)

E) be a pure substance

6.
How many sig. fig. are in the number below:
0.056
a)
1
b)
2
c)
3
d)
4
7.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of carbon?

a)

29%

b)

43%

c)

57%

d)

73%

8.

What percentage of the total atomic mass of carbon monoxide (CO) is composed of oxygen?

a)

29%

b)

43%

c)

57%

d)

73%

9.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of bromine? Hint - consider the mass of both atoms of bromine in your calculation.

a)

13%

b)

43%

c)

63%

d)

87%

10.

Cations (+) are smaller than their atoms since you are removing valence electrons that are farther from the nucleus and anions (−) are larger than their atoms since adding extra electrons increases electron-electron repulsions.

a)

True

b)

False

11.

The greater the electronegativity difference between 2 atoms, the more polar the bond becomes.

a)

True

b)

False

12.

How many peaks would be expected for a PES spectum for Calcium?

a)

2

b)

3

c)

4

d)

5

13.

Which of these elements would have the same number of PES peaks as Fluorine?

a)

Neon

b)

Beryllium

c)

Sodium

d)

Chlorine

14.

Which peak (or peaks) correspond to the valence electrons?

a)

The peak at 1

b)

The peaks at 1 and 2.05

c)

The peak at 239

d)

The peaks at 239 and 22.7

15.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

16.

How many significant figures are in 127.500?

(a)  

17.

How many significant figures are in 670?

(a)  

18.

What does the 4th peak from the left represent?

a)

The 2s electrons

b)

The 3d electrons

c)

The 2p electrons

d)

The 3s electrons

19.

How many significant figures are in 0.0730?

(a)  

20.

Give the answer to the correct number of significant figures to

3.419 + 3.912 + 7.0518 + 0.00013

a)

14.383

b)

14.382

c)

14.3829

d)

14.38293

21.

How many significant figures are in 300900?

(a)  

22.

Give the answer to the correct number of significant figures to

17.3 x 6.2

(a)  

23.

Give the answer to the correct number of significant figures to

247.89 ÷ 43.5

a)

5.70

b)

5.7

c)

5.699

d)

5.69

24.

The symbol M stands for

a)

molality

b)

moles

c)

molar mass

d)

molarity

25.

Give the answer to the correct number of significant figures to

109.3758 ÷ 5.813

(a)  

26.

In the expression “like dissolves like,” the word “like” refers to similarity in what?

a)

size

b)

polarity

c)

energy

d)

mass

27.

Molarity is expressed as

a)

mols solute/grams solution

b)

mols solute/L solution

c)

mols solute/mL solution

d)

mass solute/mass of solute + solution

28.

Which gas is the most soluble at 20 oC?

a)

Helium

b)

Nitrogen

c)

Carbon dioxide

d)

oxygen

e)

methane

29.

Concentrated hydrochloric acid has a concentration of 12 M.  You are given 10 mL of this acid.  If you dilute this amount of HCl to 600 mL, what is the new molarity of the solution?

a)

2 M

b)

0.2 M

c)

1.2 M

d)

0.0002M

30.

How many grams of silver nitrate would you need to make a 1.0 molar aqueous solution of silver nitrate in 710 mL of water?

a)

1.4

b)

238

c)

240

d)

0.7

31.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
32.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
33.

Which gas is the least soluble at 20 oC?

a)

Helium

b)

Nitrogen

c)

Carbon dioxide

d)

oxygen

e)

methane

34.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

35.
Molar mass is in units of ________.
a)
grams
b)
grams/mole
c)
mole
d)
moles/gram
36.

A sample contains 36.95 g of mercury (Hg) and 13.05 g of chlorine (Cl). What is the chemical formula for this compound?

a)

HgCl2

b)

Hg3Cl

c)

Hg17Cl36

d)

HgCl

37.

What is the chemical formula of a compound, if a sample containts 81.82 grams of carbon and 18.18 grams of hydrogen?

a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
38.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
39.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

40.

You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.

a)

SO

b)

SO2

c)

SO3

d)

SO4

41.
4.0 moles of H2O would have what mass?
a)
72 g
b)
23 g
c)
68 g
d)
4.5 g
42.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

43.

Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

NaPO4

44.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
45.

A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

46.

Do the diagrams have the same molecular formula?

a)

Yes

b)

No

47.

Do the diagrams have the same empirical formula?

a)

Yes

b)

No

48.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
49.

Based on the mass spec data, which Iron isotope is the most abundant?

a)

Fe-54

b)

Fe-56

c)

Fe-57

d)

Fe-58

50.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
51.

The empirical formula of a substance is CH2O. The molar mass is 180g/mol. What is the molecular formula?

a)

CH2O

b)

C3H6O3

c)

C6H12O6

d)

C12H6O12

52.

An unlabeled bottle of alcohol produces the following composition: 

C = 59.94% H = 13.44% O = 26.62%.

Which alcohol was analyzed?

a)

ethanol (C2H6O)

b)

propanol (C3H8O)

c)

butanol (C4H10O) 

d)

pentanol (C5H12O)

53.

The mass of each element per 100 mass unit of compound is called __________.

a)

percent composition

b)

molar mass

c)

mole ratio

d)

molecular formula

54.
What do the heights of the peaks represent in the mass spectrum?
a)
number of isotopes
b)
relative abundance of each isotope
c)
average atomic mass
d)
charge:mass ratio
55.

If black ball represents carbon (C) atom and white balls represent hydrogen (H) atoms. What is the molecular formula of the diagram shown?

a)

CH

b)

CH4

c)

C4H

d)

C4H4

56.
What do the peaks on the mass spectrum represent?
a)
anions
b)
different isotopes
c)
atoms with differing numbers of electrons
d)
numbers of electrons
57.

Element X has 2 isotopes. X-125 and X-126. For every 100 atoms of X, 30 of them have a mass of 125.0 amu and 70 have a mass of 126.0 amu. What is the average atomic mass of X?

a)

125.3 amu

b)

125.7 amu

c)

126.3 amu

d)

126.7 amu

58.

What element has the following mass spec data?

a)

Sulfur

b)

Nitrogen

c)

Oxygen

d)

Carbon

59.

How many isotopes are shown in this mass spec?

a)

1

b)

2

c)

6

d)

7

60.

What element has the following mass spec data?

a)

Tin

b)

Tellurium

c)

Chromium

d)

Polonium

61.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
62.

The second shell from the center of an atom can hold how many electrons?

a)

2

b)

6

c)

8

d)

18

63.

Valence electrons are located...

a)

inside the nucleus

b)

in outer space

c)

on the outermost orbit of an atom

64.
a)

10

b)

2

c)

8

d)

18

65.

How many electrons can the d sublevel hold?

a)
8
b)
10
c)
2
d)
4
66.

Calculate the average atomic mass from the mass spec.

a)

85.56 amu

b)

85.75 amu

c)

86.44 amu

d)

86.74

67.
There are 4 different types of subshells s,p,d,f
a)
true
b)
false
68.

What is the maximum number of electrons that an s orbital can have?

a)

1 electron

b)

2 electrons

c)

3 electrons

d)

4 electrons

69.

How many electrons can the p sublevel hold?

a)
8
b)

6

c)
2
d)
4
70.

What is the maximum number of electrons that an f orbital can have?

a)

11 electrons

b)

14 electrons

c)

13 electrons

d)

12 electrons

71.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
72.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
73.
What electron configuration matches an oxygen atom?
a)
1s22s22p63s2, 3p64s23d104p5
b)
1s22s22p4
c)
1s22s22p6
d)
1s22s22p63s23p64s23d1
74.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
75.
Which electron configuration belongs to Copper (Cu)?
a)
1s2 2s2 2p6 3s2 3p6 4s2 3d8
b)
1s2 2s2 2p6 3s2 3p6 4s2 3d9
c)
1s2 2s2 2p6 3s2 3p6 4s2 3d10
76.
What is the name of Group 1?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
77.
What is the name of Group 2?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
78.
What is the name of Groups 3-12?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
79.
What is the name of Groups 18?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Halogens
d)
Noble Gases
80.
What is the name of Groups 17?
a)
Alkali Metals
b)
Alkali Earth Metals
c)
Transition Metals
d)
Halogens
81.
What type of elements touch the zigzag line?
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Solids
82.
Where are the metals on the Periodic Table?
a)
To the left
b)
In the upper right hand corner
c)
On the zigzag line
d)
At the bottom
83.
How would you describe reactivity on the periodic table?
a)
Elements in the same group are most likely to react.
b)
Elements in the same Periodic are most likely to react.
c)
Elements on opposite sides of the Periodic Table are most likely to react.
d)
There is no trend of reactivity.
84.
How is the Periodic Table arranged?
a)
Increasing atomic mass
b)
Increasing atomic number
c)
Decreasing atomic mass
d)
Decreasing atomic number
85.

Why does K have a larger radius than Na?

a)

K has more mass

b)

K has more electron shells

c)

K has more valence electrons

d)

K has more protons

86.

Which element would have a smaller radius?

a)

Li

b)

Be

c)

O

d)

F

87.

Which element has the smallest ionization energy?

a)

N

b)

P

c)

As

88.

Why does iodine have a smaller electronegativity value than fluorine?

a)

Iodine has a larger radius so it is less difficult to remove electrons

b)

Iodine has a larger radius so it does not attract electrons easily

c)

Iodine has a smaller radius so it does not attract electrons easily

d)

Iodine has a smaller radius so it is less difficult to remove electrons

89.

(Select all that apply) Aluminum (compared to chlorine) would have:

a)

a smaller radius

b)

a smaller ionization energy

c)

a smaller electronegativity

d)

metallic properties

e)

13 valence electrons

90.

Why does fluorine have a larger ionization energy than chlorine?

a)

Since Fluorine has a smaller radius, it is harder to remove electrons from it

b)

Since Fluorine has a smaller radius, it attracts electrons easier

c)

Since Fluorine has a larger radius, it is easier to remove electrons from it

d)

Since Fluorine has a larger radius, it is harder to attract more electrons

91.

What is ionization energy?

a)

The size of the atom

b)

The energy needed to remove an electron

c)

The desire an atom has for another electron.

92.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
93.

Which element in period 4 has the highest electronegativity?

a)

potassium

b)

calcium

c)

copper

d)

bromine

94.

The ability of an atom to attract electrons is called __________.

a)

atomic radius

b)

ionization energy

c)

electronegativity

95.

What is the decrease in the attraction between an electron and the nucleus in an atom with more than one electron shell?

a)

shielding effect

b)

effective nuclear charge

c)

ionization energy

d)

electronegativity

96.

Order the following from smallest to largest atomic radius:

Ra, Be, Ca, Rb, H

a)

Ra, Be, Rb, H, Ca

b)

Rb, H, Ca, Be, Ra

c)

Ra, Rb, Ca, Be, H

d)

H, Be, Ca, Rb, Ra

97.

The effective nuclear charge of magnesium is

a)

+1

b)

+2

c)

+12

d)

+24

98.

Effective nuclear charge ________ across a period.

a)

increases

b)

decreases

c)

stays the same

99.

What is effective nuclear charge?

a)

The charge that effects the mass of the atom.

b)

The charge that the protons feel from the rest of the atom.

c)

The nuclear charge felt by the valence electrons.

d)

The nuclear charge felt by the core electrons.

100.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.

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