wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

AP Chem The Whole Enchilada Units 1-3

Total questions: 187

Worksheet time: 3hrs 14mins

Name
Class
Date
1.

Unit 1: When an electron is in a higher energy level, it is farther away from the nucleus and has less Coulombic attraction to the nucleus and is therefore easier to remove

a)

True

b)

False

2.

Unit 1: When reading a PES graph, the higher the peak, the less electrons there are in that sublevel, and a larger binding energy means that the electrons are closer to the nucleus.

a)

True

b)

False

3.

Unit 1: Isotopes of an element have the same number of protons, but different numbers of electrons.

a)

True

b)

False

4.

Unit 1: 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

5.

Unit 1: The greater the electronegativity difference between 2 atoms, the more polar the bond becomes.

a)

True

b)

False

6.

Unit 1: % error= (experimental - theoretical)/experimental

a)

True

b)

False

7.

Unit 1: Filtering separates mixtures based on differences in what property?

a)

Chemical

b)

Solubility

c)

Particle size

d)

Density

8.

Unit 1: What is the equation for calculating the density of a substance?

a)

D=m/v

b)

m=D/v

c)

D=v*m

d)

D=v/m

9.

Unit 1: When an electron is in a lower energy level, it is ________________ away from the nucleus

a)

Closer

b)

Farther

10.

Unit 1: When reading a PES (Photoelectric Spectroscopy) graph, what does the height of a peak represent?

a)

The number of electrons

b)

The number of protons

c)

The mass or the isotope

d)

The amount of energy the electron has

11.

Unit 1: Isotopes of an element have the same number of __________, but different number of __________.

a)

protons, neutrons

b)

neutrons, protons

c)

protons, electrons

d)

electrons, protons

12.

Unit 1: When reading a PES (Photoelectron Spectroscopy) graph, a larger binding energy means that the electrons are _________________ the nucleus?

a)

Closer to

b)

Farther from

13.

Unit 1: Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

14.

Unit 1: What type of change conserves mass?

a)

none

b)

chemical

c)

physical

d)

chemical and physical

15.

Unit 1: When an electron is in a higher energy level, it has ___________ Coulombic attraction to the nucleus

a)

More

b)

Less

16.

Unit 1: What is the measurement of the burette? (in mL)

a)

6.6mL

b)

6.64mL

c)

7.36mL

d)

7.3mL

17.

Unit 1: Which orbital comes after 4s?

a)

3d

b)

5s

c)

4p

d)

4d

18.

Unit 1: Are cations larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

19.

Unit 1: Which piece of glassware is the most precise

a)

beaker

b)

graduated cylinder

c)

burette

d)

test tube

20.

Unit 1: Moving across a row (L to R) on the periodic table, Zeff _________________

a)

Increases

b)

Decreases

c)

Stays the same

21.

Unit 1: What type of change separates a compound into elements?

a)

physical

b)

chemical

c)

chemical and physical

22.

Unit 1: Why do atoms get smaller moving across a period (L to R) on the periodic table?

a)

More protons (q) to attract the electrons

b)

Fewer protons (q) to attract the electrons

c)

More energy shells (r) so it can't attract the electrons

d)

Fewer energy shells (r) so it attracts the electrons closer

23.

Unit 1: Why are anions larger than their neutral atoms?

a)

More shielding that repels the other electrons

b)

Fewer protons to attract electrons

c)

More electrons to attract protons

d)

More Zeff to attract electrons

24.

Unit 1: Which piece of glassware is the least precise?

a)

graduated cylinder

b)

beaker

c)

burette

25.

Unit 1: When an electron is in a lower energy level, it has a ________________ 1st ionization energy

a)

Higher

b)

Lower

c)

Same

26.

Unit 1: Which electrons are removed first when making a cation?

a)

s

b)

p

c)

d

d)

f

27.

Unit 1: What do mass spectroscopy graphs measure?

a)

Mass of isotopes

b)

Mass of protons

c)

Energy of electrons

d)

Number of electrons

28.

Unit 1: When reading a PES graph, a larger binding energy means that the electrons are ____________ from the nucleus?

a)

closer

b)

farther

c)

the same distance

29.

Unit 1: Which orbital comes after 4p?

a)

5s

b)

4s

c)

3d

d)

4p

30.

Unit 1: germanium is a ________________, hydrogen is a _________________ and uranium is a ________________

a)

metal, non-metal, metalloid

b)

metalloid, non-metal, metal

c)

non-metal, metal, metalloid

31.

Unit 1: Are anions larger or smaller than their neutral atoms?

a)

Larger

b)

Smaller

c)

Same size

32.

Unit 1: When an electron is in a lower energy level, it has a ___________ 1st ionization energy

a)

Higher

b)

Lower

33.

What is the molar mass of Cl2?

a)

17 g/mol

b)

35.5 g/mo;

c)

71.0 g/mol

d)

89 g/mol

34.

Calculate the molar mass of KOH.

a)

28 g/mol

b)

56 g/mol

c)

84 g/mol

d)

112 g/mol

35.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

36.

What is the molar mass of the diatomic element nitrogen?

a)

7 g/mol

b)

14 g/mol

c)

28 g/mol

37.
CO2
a)
Ionic
b)
Covalent
c)
Polyatomic Ion 
d)
Metallic 
38.
What two types of atoms make a covalent bond?
a)
2 Nonmetals
b)
1 Nonmetal and 1 Metal
c)
2 Metals
d)
2 Noble Gases
39.
Ionic bonds form between metals and ____.
a)
metalloids
b)
metals
c)
nonmetals
40.

Beryllium and sulfur will form a ______ bond

a)

ionic

b)

covalent

c)

metalloid

41.

MgO

a)

ionic

b)

covalent

c)

metallic

42.

Which concept is Avogadro's number related to?

a)

Mole

b)

Atomic number

c)

Chemical equation

d)

Molar mass

43.

What does Avogadro's number allow scientists to determine?

a)

The temperature of atoms or molecules in a given amount of substance.

b)

The color of atoms or molecules in a given amount of substance.

c)

The weight of atoms or molecules in a given amount of substance.

d)

The number of atoms or molecules in a given amount of substance.

44.

Avogadro's number is approximately equal to:

a)

3.141 x 10^23

b)

9.999 x 10^22

c)

1.234 x 10^24

d)

6.022 x 10^23

45.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
46.

How do you solve the following problem: How many grams are there in 7.5 moles of H2SO4?

a)

Convert liters to moles then moles to grams

b)

Convert particles to moles then moles to grams

c)

Convert moles to grams

d)

Convert grams to moles

47.

Match the following...

a)

You convert moles to grams by...

1.

multiplying by the molar mass

b)

You convert liters to moles by...

2.

dividing by 22.4L

c)

You convert moles to particles by...

3.

multiplying my avagadro's constant

d)

You convert grams to moles by...

4.

dividing by the molar mass

e)

You convert moles to liters by...

5.

multiplying by 22.4L

48.

How many grams are in 9.28x1023 molecules9.28x10^{23}\ molecules  of NaCl?

Choose the correct setup.

a)

9.28x1023 molecules ×6.02x1023 grams1 mole9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ grams}{1\ mole}  

b)

9.28x1023 molecules ×6.02x1023 mc1 mole×58.44 g1 mole9.28x10^{23}\ molecules\ \times\frac{6.02x10^{23}\ mc}{1\ mole}\times\frac{58.44\ g}{1\ mole}  

c)

9.28x1023 molecules ×1 mole6.02x1023 mc×58.44 g1 mole9.28x10^{23}\ molecules\ \times\frac{1\ mole}{6.02x10^{23}\ mc}\times\frac{58.44\ g}{1\ mole}  

d)

9.28x1023 molecules ×58.44 g1 mole9.28x10^{23}\ molecules\ \times\frac{58.44\ g}{1\ mole}  

49.

How many moles are in 2.67x1024 molecules of H2O?

What is the missing piece?

2.67x1024 molecules×???????????6.02x1023 mc2.67x10^{24}\ molecules\times\frac{???????????}{6.02x10^{23}\ mc}  

a)

6.02x1023 mc

b)

1 mole

c)

18.016 grams

d)

2.67x1024 mc

50.

What element is this?

a)

Chlorine

b)

Lithium

c)

Boron

d)

Phosphate

e)

Phosphite

51.

If you had 192.9 atoms of silver, 100 would be Ag-107 and 92.9 would be Ag-109. What would the Average Atomic Mass be? (You have time to answer... do your work...)

Important numbers: Atomic Mass of Ag-107 is 106.905 and Atomic Mass of Ag-109 is 108.904.

a)

107.87

b)

108.85

c)

107.44

d)

108.26

e)

107.94

52.
What are isotopes?
a)
charged atoms
b)
radioactive elements
c)
elements with different numbers of neutrons
53.
What are the steps of operation in the mass spectrometer?
a)
Accelerate, Deflect,Ionize, Detect
b)
Deflect,Ionize, Accelerate, Detect
c)
Ionize, Accelerate, Deflect, Detect
d)
Detect, Accelerate, Deflect, Ionize
54.
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
55.
Which element does this mass spectrum most likely represent?
a)
neon
b)
scandium
c)
boron
d)
sodium
56.
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
57.
How many isotopes are shown in this mass spectrum?
a)
1
b)
84
c)
86
d)
4
58.
Based on the mass spectrum, which isotope of chlorine is most abundant?
a)
35Cl
b)
37Cl
c)
70Cl
d)
72Cl
59.
Carbon has three known isotopes. Which is the most abundant?
a)
carbon-12.011
b)
carbon-12
c)
carbon-13
d)
carbon-14
60.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
61.

Molecular Formula = C2F6

Choose the correct empirical formula.

a)

CF

b)

C2F6

c)

C3F

d)

CF3

62.

Empirical Formula = CF2

Molecular formula mass = 192 g/mol

Molecular Formula = ?

a)

C4F8

b)

C8F4

c)

C3F6

d)

C2F4

63.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
64.

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

a)

29%

b)

43%

c)

57%

d)

73%

65.

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

a)

29%

b)

43%

c)

57%

d)

73%

66.

which one defines percent composition?

a)

the percent by mass of each element in a compound

b)

when elements join together

c)

when water dries up

d)

elements split

67.

How do you calculate the percent composition by mass of an element in a compound?

(​ (a)   ) ÷\div (​ (b)   ) ×\times 100

Choose from the below words
Total Molar Mass of Element in Compound
Total Molar Mass of Compound
Molar Mass of a Single Element
100
68.

% to Mass; Mass to Moles; Divide by Small; Multiply Till Whole

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find % Composition

69.

Weight of the Molecular Formula Divided by the Weight of the Empirical Formula x 100

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find Percent Composition

70.

Individual divided by total x 100

a)

Steps to find an Empirical Formula

b)

Steps to find a Molecular Formula

c)

Steps to find Percent Composition

71.

Click the hotspot for the box that represents an element.

A
B
C
D
72.

Click the hotspot that represents a mixture

A
B
C
D
73.

Identify the substance in box Y.

a)

element

b)

compound

c)

mixture

74.

Identify this substance.

a)

element

b)

compound

c)

mixture

75.

Identify this substance.

a)

element

b)

compound

c)

mixture

76.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
77.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)

Zinc (Zn)

b)

Copper (Cu)

c)

Nickel (Ni)

d)

Germanium (Ge)

78.

The PES spectrum below is for the element _______________.

a)

O

b)

Ne

c)

N

d)

F

79.

Examine the spectrum below. Where would you expect the 2p peak for F be if it were on the same spectrum?

a)

To the left of the peak at 3.04

b)

To the right of the peak at 3.04

c)

To the left of the peak at 1.31

d)

To the right of the peak at 1.31

80.

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

81.

Which electrons would be ejected with the most kinetic energy according to the spectrum below?

a)

The ones in the peak at 151

b)

The ones in the peak at 7.9

c)

The ones in the peak at 1.09

d)

The ones in the peak at 0.58

82.

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

83.

How many valence electrons does the element pictured in the PES spectrum below have?

a)

1

b)

2

c)

3

d)

4

84.

As the energy level goes higher, the electrons

a)

have lower in energy

b)

are more stable

c)

are weaker

d)

are farther from the nucleus

85.

Click on the hotspot that represents an energy level.

A
B
C
D
E
F
86.

The lowest available energy state of an electron is called the:

a)

the lowest state

b)

the ground state

c)

the entry state

d)

the fixed state

87.
What is the label for energy?
a)
J
b)
m
c)
Hz
d)
nm
88.
Valence electrons are found in the ______ energy level.
a)
Farthest in
b)
Middle
c)
Outermost
89.

Select the hotspot that shows the most EN element

A
B
C
D
E
F
90.

Select the hotspot that shows the smallest element

A
B
C
D
E
F
91.

Select the hotspot that shows the largest element

A
B
C
D
E
F
92.

Select the hotspot that shows the largest 1st ionization energy

A
B
C
D
E
93.

Reorder the following in order of increasing atomic radius

a)

F

b)

Cl

c)

Br

d)

I

e)

At

1)
2)
3)
4)
5)
94.

Reorder the following in order of increasing atomic radius.

a)

Cl

b)

S

c)

P

d)

Si

e)

Al

1)
2)
3)
4)
5)
95.

Reorder the following in order of increasing EN

a)

Ni

b)

Cu

c)

N

d)

O

e)

F

1)
2)
3)
4)
5)
96.

Unit 2: A single bond is composed of

a)

1 sigma bond

b)

1 pi bond

c)

1 sigma and 1 pi bond

d)

no sigma or pi bonds

97.

Unit 2: A triple bond is composed of

a)

1 sigma bond

b)

1 pi bond

c)

2 pi bonds

d)

1 sigma and 2 pi bonds

98.

Unit 2: Lattice energy is the energy to break an ionic bond in a compound. Lattice energy increases as the ion’s charge increases. Lattice energy decreases as the radii of the ions increase.

a)

True

b)

False

99.

Unit 2: SiO2 (quartz) and diamonds are ____________________, and they have very high boiling/melting points.

a)

covalent network solids

b)

ionic solids

c)

molecular solids

d)

interstitial alloys

100.

Unit 2: ______________ alloys are made when a smaller atom fits into the gaps between larger atoms of a metallic crystal.

a)

Interstitial

b)

Substituitonal

101.

Unit 2: What type of alloy is made when the radii of the atoms are similar in size?

a)

interstitial

b)

substitutional

102.

Unit 2: In this molecule, Carbon has a formal charge of ____ and Nitrogen has a formal charge of _____.

a)

0, 0

b)

1, 0

c)

0, -1

d)

-1, 0

103.

Unit 2: What type of alloy is this?

a)

Interstitial

b)

Substitutional

104.

Unit 2: What is the total # of covalent bonds carbon can form when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

105.

Unit 2: What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

106.

Unit 2: What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

104.5

107.

Unit 2: Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

108.

Unit 2: What is the bond angle in NH3

a)

120

b)

107.3

c)

180

d)

90

109.

Unit 2: What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

110.

Unit 2: What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

111.

Unit 2: Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

112.

Unit 2: What is the hybridization for an oxygen in CO2

a)

sp3

b)

sp

c)

sp2

113.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
114.

Unit 2: What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

115.

Unit 2: What is the the shape of this molecule according to VSPER theory?

a)
Linear
b)
Tetrahedral
c)
Trigonal Planar
d)
Trigonal pyramidal
116.

Unit 2: What compound could this be?

a)

CO2

b)

NH3

c)

H2S

d)

CH4

117.

Unit 2: Draw the Lewis Dot structure for PCl5 and determine the predicted molecular geometry

a)

octahedral

b)

trigonal pyramidal

c)

seesaw

d)

trigonal bipyramidal

118.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
119.

Unit 2: Choose the correct shape for this molecule:

a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
120.

Unit 2: How many sigma and pi bonds does this have?

a)
1 sigma and 1 pi
b)
2 sigma and 1 pi
c)
1 sigma and 2 pi
d)
2 sigma and 2 pi
121.

Unit 2: How many sigma and pi bonds does this have? 

a)
3 sigma and 2 pi
b)
5 sigma and 5 pi
c)
5 sigma and 0 pi
d)
0 sigma and 5 pi
122.

Unit 2: Carbon atom undergo

a)
sp hybridization
b)
sp2 hybridization
c)
sp3 hybridization
d)
dsp3 hybridization
123.

Unit 2: What is the total # of covalent bonds carbon has to make when drawing a Lewis structure?

a)

12

b)

6

c)

4

d)

8

124.

Unit 2: What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

125.

Unit 2: What is the bond angle in H2O?

a)

120

b)

90

c)

180

d)

109.5

126.

Unit 2: Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

127.

Unit 2: What is the bond angle in NH3

a)

120

b)

109.5

c)

180

d)

90

128.

Unit 2: What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

129.

Unit 2: What is the hybrid orbital used in CH4?

a)

sp3

b)

sp

c)

sp2

130.

Unit 2: What is the hybrid orbital used in CO2

a)

sp3

b)

sp

c)

sp2

131.

Unit 2: Count the number of sigma and pi bonds in this molecule:

a)

13 sigma, 1 pi

b)

14 sigma, 2 pi

c)

1 sigma, 14 pi

d)

2 sigma, 13 pi

132.

Unit 2: Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

133.

Unit 2: What is the bond angle in SO2

a)

120

b)

90

c)

180

d)

109.5

134.

When two identical atoms, such as two oxygen atoms, bond, the resulting bond is​ (a)  

Choose from the below words
nonpolar covalent
polar covalent
ionic
metallic
135.

Click on the bond that shares the most electrons in this structure.

A
B
C
D
E
F
G
H
I
J
136.

Label the type of bonds seen in the structure to the right

a)

Double Bond

b)

Triple Bond

c)

Single bond

d)

Quadruple Bond

1
2
1)
2)
137.
Question Image
a)

Electronegativity difference is large enough to cause unequal sharing of electrons but not large enough to cause a transfer of electrons from one atom to another.

1.

C

b)

Compounds held together with these bonds are malleable with high thermal and electrical conductivity due to freely moving electrons

2.

A

c)

Bonded atoms share electrons without a dipole moment

3.

D

d)

Electronegativity difference between atoms is large enough to transfer electrons

4.

B

138.

Match the following

a)

One shared pair of electrons

1.

Single Bond

b)

Two shared pairs of electrons

2.

Double Bond

c)

Three shared pairs of electrons

3.

Triple Bond

139.

Match the types of elements with the correct bond formation.

a)

metal - nonmetal

1.

ionic bond

b)

metal - metal

2.

metallic bond

c)

nonmetal - nonmetal

3.

covalent bond

140.


Match the term and its diagram

a)
1.

Ionic bond

b)
2.

Covalent bond

c)
3.

Hydrogen bond

141.

​ ​ (a)   ​ compounds are usually the strongest.

Choose from the below words
Ionic
Covalent
142.

Match the following pictures to the types of bonds

a)

1.

metallic bond

b)

2.

hydrogen bond

c)

3.

ionic bond

d)

4.

covalent bond

e)

5.

polar bond

143.

A sea of electrons forms a ​ (a)  

Choose from the below words
metallic bond
ionic bond
covalent bond
144.

Match the following with their correct chemical bond type

a)

NaClNaCl

1.

Ionic

b)

H2OH_2O

2.

Covalent

c)

CoCo

3.

Metallic

145.
This is an example of a __________ bond.
a)
non-polar covalent
b)
polar covalent
c)
ionic
d)
metallic
146.
How many electrons are shared in a triple bond?
a)
6
b)
3
c)
6 pairs
d)
5
147.
What type of bond is this?
a)
ionic
b)
covalent
148.

The image above shows:

a)

covalent bonding

b)

ionic bonding

c)

metallic bonding

149.

Which best describes the bonding in the cyanide ion (CN-)?

a)

3 (sigma) bonds

b)

2 (sigma) bonds and I (pi) bond

c)

1 (sigma) bond and 2 (pi) bonds

d)

3 (pi) bonds

150.

Use your knowledge and electronegativity sheet to predict what the following compound is classified as.

a)

nonpolar covalent

b)

polar covalent

c)

ionic

d)

metallic

151.
What type of bond is illustrated above?
a)
Metallic
b)
Ionic
c)
Covalent
d)
Wiggly
152.

What is the name for the electrostatic force of attraction between the particles shown in the image?

a)

covalent bond

b)

dative covalent bond

c)

metallic bond

d)

ionic bond

153.

Unit 3: Real gases behave most like an ideal gas at high temperature and at low pressure. The more polar a gas is and the larger a gas is, the more it will deviate from ideal behavior. Consequently, small, nonpolar gases are the _______ ideal.

a)

Most

b)

Least

154.

Unit 3: Which is the strongest IMF?

a)

LDF

b)

Dipole dipole

c)

Hydrogen bonding

d)

Ion-dipole

155.

Unit 3: Which would have the strongest IMFs?

a)

CH4

b)

C2H2

c)

C4H8

d)

C8H14

156.

Unit 3: Vapor pressure and volatility decrease as IMF’s increase.

a)

True

b)

False

157.

Unit 3: Which atom has the negative dipole in this molecule?

a)

Hydrogen

b)

Fluorine

c)

Neither

158.

Unit 3: As the electronegativity difference between 2 atoms increases, the polarity of the bond ____________________

a)

increases

b)

decreases

159.

Unit 3: What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

160.

Unit 3: Why are asymmetrical molecules polar?

a)

Their dipoles do not cancel

b)

Their dipoles cancel

161.

Unit 3: When a molecular solid melts or boils, which breaks?

a)

Intermolecular forces

b)

Intramolecular bonds

162.

Unit 3: The particles under the purple curve (middle) have an average Kinetic Energy that is proportional to of 500K

a)

True

b)

False

163.

Unit 3: Which curve represents the most particles in this Maxwell-Boltzmann curve (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

They all have the same number of particles

164.

Unit 3: Which curve in this Maxwell-Boltzmann distribution represents the highest proportion of particles moving the fastest (# of particles vs. speed)?

a)

Black (peak on the left)

b)

Red (peak in the middle)

c)

Blue (peak on the right)

d)

All particles are moving at the same speed

165.

Unit 3: Why are all gas mixtures considered to be homogenous?

a)

The gas particles mix uniformly without distinct areas of concentration

b)

The gas particles mix in distinct areas of concentration

c)

The gas particles cannot be separated from each other

d)

The gas particles are in constant random motion

166.

Unit 3: Why are gases compressible?

a)

Gas particles are very small but take up large volumes of space

b)

Gas particles are very small and take up small volumes of space

c)

Gas particles are strong attracted to one another.

167.

Unit 3: How are P and V related?

a)

When Pressure increases Volume increases

b)

When Pressure increases Volume decreases

c)

When Pressure decreases Volume decreases

168.

Unit 3: What causes gas pressure?

a)

The constant collisions of gas particle on the walls of a container

b)

The decrease in temperature when gas particles move slower

c)

The collision of gas particles with each other

169.

Unit 3: How are T and V related?

a)

When Temperature increases Volume increases

b)

When Temperature increases Volume decreases

c)

When Temperature decreases Volume increases

170.

Unit 3: How are T and P related?

a)

When Temperature decreases Pressure increases

b)

When Temperature increases Pressure decreases

c)

When Temperature increases Pressure increases

171.

Unit 3: In the equation PV = nRT what are the units for T, V and P?

a)

Celcius, L, atm

b)

Kelvin, ml, torr

c)

Kelvin, L atm

172.

Unit 3: At STP what is the volume of one mole of an ideal gas?

a)

14.4 L

b)

22.4 L

c)

11.2 L

173.

Unit 3: How are gas pressure and number of moles related?

a)

When # moles decreases P increases

b)

When # moles decreases P decreases

c)

When # moles increases P increases

d)

When # of moles increases P decreases

174.

Unit 3: Which of the following gases will move the fastest if they are at the same temperature?

He Ar

a)

He will move slower because it is smaller than Ar

b)

He will move faster because it is smaller than Ar

c)

He will move faster because it is larger than Ar

175.

Unit 3: When carbon dioxide gas is collected over water, what accounts for the total pressure in the container?

a)

carbon dioxide gas only

b)

water vapor only

c)

carbon dioxide gas and water vapor

176.

Unit 3: In what conditions do real gases behave most like ideal gases?

a)

low T and high P

b)

low P and high T

c)

high T and high P

177.

Unit 3: What gases deviate the most form ideal gas behavior?

a)

polar and large gas particles

b)

nonpolar and large gas particles

c)

polar and small gas particles

178.

Unit 3: When a molecular solid melts or boils, which bonds break?

a)

Intermolecular

b)

Intramolecular

179.

Unit 3: Name a property that increases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

180.

Unit 3: List the 3 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding

d)

dipole dipole, hydrogen bonding, london dispersion

181.

Unit 3: List ALL the Intermolecular forces that exist in PCl3

a)

hydrogen bonding, london dispersion

b)

london dispersion, hydrogen bonding, dipole dipole

c)

london dispersion, dipole dipole

d)

london dispersion

182.

Unit 3: “More polarizable” refers to which Intermolecular Force?

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

183.

Unit 3: Name a property that decreases as Intermolecular Forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

184.

Unit 3: P and V are ___________________ related?

a)

inversely

b)

directly

185.

Unit 3: The more molar mass a gas has, the_________________ it moves

a)

faster

b)

slower

186.

Unit 3: Average Kinetic Energy is another term for _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

187.

Unit 3: Real gases behave most like an ideal gas at what conditions of temperature and pressure?

a)

High T, Low P

b)

High P, Low T

c)

High V, Low T

Similar Resources on Wayground

HCS Chemistry sem 2 Final Exam Review

184 questions

HCS Chemistry sem 2 Final Exam Review

quiz

Worksheet

•

9th - 12th Grade

Periodic Trends

186 questions

Periodic Trends

quiz

Worksheet

•

10th - 11th Grade