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AP Chemistry Cumulative Units 1-3

Total questions: 130

Worksheet time: 32hrs 16mins

Name
Class
Date
1.

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

a)

12

b)

6

c)

4

d)

8

2.

What is the bond angle in BF3?

a)

90

b)

120

c)

109.5

d)

180

3.

Which orbital is filled after 4p?

a)

5s

b)

4s

c)

3d

d)

4p

4.

What is the bond angle in H2O? (Hint: It is a bent structure at 109.5, but 2 sets of lone pairs push the bonds.)

a)

120

b)

90

c)

180

d)

104.5

5.

Fill in the blanks: silicon is a ________________, hydrogen is a _________________ and uranium is a ________________

a)

metal, non-metal, metalloid

b)

metalloid, non-metal, metal

c)

non-metal, metal, metalloid

6.

Are asymmetrical molecules polar or nonpolar?

a)

Polar

b)

non-polar

c)

neither

7.

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

8.

“More polarizable” refers to which intermolecular force? (Hint: Think about polarizable being temporary dipoles.)

a)

hydrogen bonding

b)

london dispersion

c)

dipole dipole

9.

What is an example of a covalent network solid?

a)

Salt

b)

Diamond

c)

Sugar

d)

Water

10.

Scarlett, Noah, and Lily are studying the properties of different substances. They noticed that as the intermolecular forces of a substance increase, a certain property decreases. Can you name this property?

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

11.

Noah, Grace, and Maya are planning a trip to the mountains. They are packing a bag of chips for the journey. They know that as they ascend, the atmospheric pressure decreases. How would this change in pressure affect the volume of the chips bag?

a)

The bag would inflate (increase in volume)

b)

The bag would deflate (decrease in volume)

12.

Anika, Zoe, and Jackson are in a science class learning about gases. They learned that the greater the molar mass of a gas, the _________________ it moves. If they were to release helium and argon into the air, which one would move slower?

a)

slower; Helium

b)

slower; Argon

c)

faster; Helium

d)

faster; Argon

13.

Average kinetic energy (KE) is proportional to _____________.

a)

Heat

b)

Temperature

c)

Pressure

d)

Activation energy

14.

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

15.

What is the hybridization of carbon in CH4?

a)

sp3

b)

sp

c)

sp2

16.

What is the hybridization for carbon in CO2

a)

sp3

b)

sp

c)

sp2

17.

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

18.

Why are symmetrical molecules nonpolar?

a)

If they have dipoles, they do not cancel.

b)

If they have dipoles, they cancel.

19.

Name a property that increases as intermolecular forces increase.

a)

Vapor pressure

b)

Conductivity

c)

Melting point

d)

Solubility

20.

Zoe, Avery, and Maya are conducting a science experiment where they are melting a salt crystal. According to their observations, what breaks when the salt crystal melts?

a)

Intermolecular forces

b)

Intramolecular bonds

21.

Imagine Grace is studying the structure of an atom in her science class. She learns that when an electron is at a higher energy level, it is farther away from the nucleus. This means it has less Coulombic attraction to the nucleus and is therefore easier to remove and has a lower first ionization energy. Is this statement true or false?

a)

True

b)

False

22.

Elijah, Lily, and Jackson are studying chemistry. They come across the concept of isotopes. Elijah says that isotopes of an element have the same number of protons, but different numbers of electrons. Is Elijah's statement correct?

a)

Yes

b)

No

23.

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

24.

James and Evelyn are studying chemistry together. James says that the greater the electronegativity difference between 2 atoms in a molecule, the more polar the bond becomes. Evelyn is unsure about this. Is James correct?

a)

Yes

b)

No

25.

Anika, Benjamin, and Isla were having a debate. Anika said that when discussing gas laws, if Benjamin heats his birthday balloon, it will expand because temperature and volume are directly related. Is this statement true?

a)

Yes

b)

No

26.

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

27.

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

28.

Which is the strongest IMF?

a)

LDF

b)

Dipole dipole

c)

Hydrogen bonding

d)

Ion-dipole

29.

Mia, Harper, and Noah are studying chemistry and discussing about Intermolecular Forces (IMFs). They are comparing different compounds and wondering which one would have the strongest IMFs. Can you help them identify the compound with the strongest IMFs from the following options?

a)

CH4

b)

C2H2

c)

C4H8

d)

C8H14

30.

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

a)

covalent network solids

b)

ionic solids

c)

molecular solids

d)

interstitial alloys

31.

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

a)

Interstitial

b)

Substituitonal

32.

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

a)

interstitial

b)

substitutional

33.

Ava, Emma, and Sophia are studying chemistry together. They come across a molecule of Hydrogen Fluoride (HF). Sophia asks, 'Which atom has the negative dipole in this molecule?'

a)

Hydrogen

b)

Fluorine

c)

Neither

34.

What type of bond forms between hydrogen and chlorine?

a)

polar covalent

b)

non-polar covalent

c)

ionic

d)

hydrogen bond

35.

What type of alloy is this?

a)

Interstitial

b)

Substitutional

36.
Choose the correct shape for this molecule:
a)
Trigonal planar
b)
Trigonal pyramidal
c)
Tetrahedral
d)
Linear
37.

Which statement is correct according to the Kinetic Molecular Theory of gases?

a)

Gas particles are stationary.

b)

Gas particles have significant volumes.

c)

Gas particles move in a random, straight-line motion.

d)

Gas particles have strong intermolecular forces.

38.

When particles in real gases are in close proximity, they are ___

a)

repelled from each other

b)

attracted to each other

c)

without mass

d)

transformed into mystical vapors

39.

What happens to a real gas at high pressure that makes it become less ideal?

a)

particles lose energy and so exert less pressure

b)

particles gain energy and so exert more pressure

c)

container volume decreases so particles occupy significant volume

d)

container volume increases so particles occupy significant volume

40.

During a science experiment at school, Nora, Scarlett, and Maya are testing the velocity of different gases at 25°C. Which gas will they observe to have the greatest velocity?

a)

He

b)

CO2

c)

CH4

d)

N2

41.

What is the term for the substance that does the dissolving in a solution?

a)

Solute

b)

Solvent

c)

Solution

d)

Miscibility

42.

During a science experiment, Harper, Scarlett, and Daniel were given three different gases: CH4, CO2, and NH3. They were asked to determine which gas would be the MOST soluble in water. Which gas should they conclude as the most soluble?

a)

CH4

b)

CO2

c)

NH3

43.

1.85 mole of NaCl is dissolved to make a 1.250 L of solution. What is the molarity?

a)

1.48 M

b)

0.675 M

c)

0.025 M

44.

How many grams of NaCl are required to make 200 ml of a 0.750 M solution?

a)

8.75 g

b)

9375 g

c)

9.38 g

45.

Ethan is working in a lab and he has 3.0 L of a 0.23 M NH3. Mia asked him how many moles of NH3 are in that solution. What should Ethan tell Mia?

a)

0.69 mol

b)

13 mol

c)

0.077 mol

46.

This is a representation of a hydrogen bond.

a)

True

b)

False

47.

This is a representation of a hydrogen bond.

a)

True

b)

False

48.

What formula do we use for dilution calculations?

a)

M1V1=M2V2

b)

D=m/V

c)

V1=M2

d)

Total Volume/Partial Volume

49.

What is the electron configuration of Phosphorus?

a)

1s2 2s2 2p6 3s2 3p3

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 4p3

d)

1s2 2s2 2p6 3s2 3p5

50.

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

51.

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

52.

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

53.

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

a)

Closer to

b)

Farther from

54.

Distillation separates mixtures based on differences in what property?

a)

Solubility

b)

Boiling Point

c)

Particle Size

d)

State of Matter

55.

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

56.

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

a)

Higher

b)

Lower

c)

Same

57.

Chromatography separates mixtures based on what property?

a)

particle size

b)

intermolecular forces

c)

boiling points

d)

state of matter

58.

Zoe & David are conducting a paper chromatography experiment in their chemistry class. They use hexane, a nonpolar substance, as the solvent. Which type of substance will travel the farthest up the paper?

a)

polar substance

b)

non polar substance

59.

List the 4 Intermolecular forces from weakest to strongest

a)

hydrogen bonding, ion-dipole, london dispersion, dipole dipole

b)

london dispersion, hydrogen bonding, ion-dipole, dipole dipole

c)

london dispersion, dipole dipole, hydrogen bonding, ion-dipole

d)

dipole dipole, hydrogen bonding, ion-dipole, london dispersion

60.

What type of solid will not conduct electricity until it is liquid or aqueous?

a)

Ionic Solid

b)

Covalent Network Solid

c)

Molecular Solid

d)

Metallic Solid

61.

What causes gas pressure?

a)

large space between the molecules

b)

random motion of particles

c)

collisions with the walls of the container & other particles

62.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
63.
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
64.
What is the mass of one mole of aluminum chloride (remember to determine the correct formula first)?
a)
62.435g
b)
116.399g
c)
133.341g
d)
97.888g
65.
How many particles are in a mole?
a)
602
b)
602 million
c)
602 moles
d)
6.02 x 1023
66.
How many moles are in 16.94g of water?
a)
16.94 mol H2O
b)
0.9401 mol H2O
c)
305.3 mol H2O
d)
1.063 mol H2O
67.
How many grams are in 3.3 mol of Potassium sulfide (K2S)?
a)
360 g
b)
454 g
c)
238 g
d)
132 g
68.
Copper (Cu) is a transition element used in the making of coins. Calculate the mass in grams of 0.0420 moles of copper.
a)
0.00697 g
b)
0.252 g
c)
2.67 g
d)
6.61 g
69.

How many molecules of AlCl3 are in 9.44 moles of AlCl3?

a)

5.68 molecules

b)

5.68x1024 molecules

c)

0.705 molecules

d)

1.25x1023 molecules

70.

Analyze the Mass Spectrum Graph. Calculate the average atomic mass of the unknown element.

a)

10.2 amu

b)

10.5 amu

c)

10.8 amu

d)

11.0 amu

71.

Analyze the Mass Spectrum Graph. What is the most likely identity of the element?

a)

Sodium

b)

Neon

c)

Carbon

d)

Boron

72.

The atomic weight of a newly discovered element is 10.600 amu. It has two naturally occurring isotopes. One has a mass of 10.000 and a natural abundance of 70.000%. What is the isotopic mass of the other isotope?

a)

12.00 amu

b)

10.60 amu

c)

11.50 amu

d)

11.00 amu

73.

What is the noble gas electron configuration for an atom of iodine in the ground state?

a)

[Kr]5s24d105p5

b)

[Xe]5s24d105p5

c)

[Kr]5s25d105p5

d)

[Xe]5s24d105p5

74.

What is the electron configuration of V2+?

a)

[Ar] 4s23d3

b)

[Ar] 4s13d4

c)

[Ar] 3d3

d)

[Ar] 4s23d1

75.

Sodium chloride is used as table salt. Select the electron configuration of the ion that would form an ionic bond with a chloride ion with a salty taste like sodium chloride.

a)

1s22s2

b)

1s22s22p5

c)

1s2

d)

1s22s1

76.

Which two particles are attracted to each other?

a)

Two neutrons

b)

A proton and an electron

c)

Two protons

d)

An electron and a neutron

77.

A repulsive force exists between which two particles?

a)

Two neutrons

b)

An electron and a neutron

c)

An electron and a proton

d)

Two protons

78.

What does  r2r^2  the stand for in this formula?

a)

Coulomb constant

b)

Electric Force

c)

Charge on object 1

d)

Charge on object 2

e)

distance between the centers of the charges of mass (squared)

79.
Calculate the volume that a 0.323-mol sample of a gas will occupy at 265 K and a pressure of 0.900 atm.
a)
7.18 L 
b)
7.81 L
c)
4.63 L
d)
4.36 L
80.
Determine the Kelvin temperature required for 0.0470 mol of gas to fill a balloon to 1.20 L under .998 atm pressure. 
a)
0 K 
b)
107 K 
c)
207 K 
d)
307 K 
81.

Elements in the same __________ have similar chemical and physical properties.

a)

group/family

b)

period

82.

In a PES graph, if two peaks are the same height, it means that they ...

a)

have the same number of electrons

b)

are in the same energy level

c)

have the same amount of binding energy

d)

are isotopes of the same element

83.

In a PES graph, 1s electrons will have a _______ binding energy than 2s electrons.

a)

higher

b)

lower

c)

same

84.

In this PES graph, which electrons are closest to the nucleus?

a)

A

b)

B

c)

C

d)

They are all at an equal distance

85.
As you move down a group, atomic radius increases because - 
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
86.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
87.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
88.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
89.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
90.
An atom that has gained or lost electrons is called ...
a)
a winner
b)
an isotope
c)
an ion
d)
a loser
91.
Atoms that gain electrons become...
a)
negatively charged
b)
positively charged
c)
remain neutrally charged
d)
21
92.
If an aluminum atom has 13 protons (+) and 10 electrons (-), what is it's charge?
a)
Al3+
b)
Al13+
c)
Al10+
d)
Al10-
93.
If an oxygen atom has 8 protons (+) and 10 electrons (-), what is it's charge?
a)
O10-
b)
O8+
c)
O2-
d)
O10+
94.
What type of elements will form an ionic bond?
a)
Metals + Metals
b)
Nonmetals + Nonmetals
c)
Metals + Nonmetals
d)
None of the above
95.
An ionic bond involves two elements...
a)
Transferring electrons
b)
Sharing electrons
96.
Which is the correct name for CaBr2?
a)
Calcium Bromine
b)
Bromine Calcium
c)
Calcium Bromide
d)
Carbon and Bromine
97.
What is the formula of calcium oxide?
a)
CaO2
b)
CaO
c)
Ca2O
d)
CO
98.

Name the following compound - (NH4)2SO4

a)

ammonium (I)

sulfate

b)

ammonium (II)

sulfate

c)

ammonium sulfate

d)

hydronium sulfate

99.

Determine the formula for the compound - nickel (III) sulfide

a)

Ni3S2

b)

NiS

c)

Ni2S3

d)

Ni2(SO4)3

100.

Determine the formula for the compound - phosphorus trichloride

a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
101.

Determine the formula for the compound - dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

102.

Is the following molecule polar or non-polar?

a)

polar

b)

non-polar

103.

Polar molecules can have non-polar covalent bonds.

a)

True

b)

False

104.

More electronegative atoms in covalent compounds are likely to have:

a)

Partial positive charge

b)

Partial negative charge

105.

In a polar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

106.

In a nonpolar covalent bond, the electrons gather around...

a)

The atom with the Greatest Electronegativity

b)

The atom with the Lowest Electronegativity

c)

Each atom Equally

d)

None of the Above

107.

The polarity of a bond is determined by...

a)

The sum of the electronegativities of the two atoms

b)

The difference in the electronegativities of the two atoms

c)

The charges of the atoms

d)

None of the Above

108.

A diatomic molecule like O2 is always _____ because electrons are shared _____

a)

nonpolar; unequally

b)

polar; equally

c)

nonpolar; equally

d)

polar; unequally

109.

Order the types of bonds based on the charge of their molecules. (lowest amount of charge to greatest)

a)

Polar Covalent --> Ionic --> Nonpolar Covalent

b)

Ionic --> Nonpolar Covalent --> Polar Covalent

c)

Ionic --> Polar Covalent --> Nonpolar Covalent

d)

Nonpolar Covalent --> Polar Covalent --> Ionic

110.
Does HCl have hydrogen bonding?
a)
yes
b)
no
111.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
112.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

113.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

114.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

115.

Which intramolecular force has the greatest strength?

a)

ionic bond

b)

nonpolar covalent

c)

polar covalent

116.
The strength of temporary dipoles:
a)
increases with the size of molecules
b)
is greater than intremolecular forces
c)
is the strongest intermolecular force
117.

How is a supersaturated solution made?

a)

Heat to high temperature, saturate, then slowly cool.

b)

Saturate, slowly heat to high temperature, then rapidly cool.

c)

Cool to a low temperature, saturate, then slowly heat.

d)

Slowly heat to high temperature, saturate, then rapidly cool.

118.
Which of the following is the solute of a 0.5M NaOH solution?
a)
water
b)
Na
c)
OH
d)
NaOH
119.

As you put in more solute in the solution, the concentration of the solution will...

a)

increase

b)

decrease

c)

stay the same

120.

Which of the following ONLY has the effect on the solubility of 'gas'?

a)

Pressure

b)

Temperature

c)

Molarity

d)

Volume

121.

Two liquids or gases that will not dissolve in each other are called

a)

miscible

b)

immiscible

c)

suspension

d)

emulsion

122.

Which of these is NOT a factor that affects solvation?

a)

agitation/stirring

b)

increasing temperature

c)

increasing surface area

d)

adding dye

123.
What is the molarity of 3 mole of hydrochloric acid in 3 L of water. 
a)
3
b)
1
c)
6
d)
9
124.

Saltwater is a 

a)
compound
b)
element
c)
heterogeneous mixture
d)
solution
125.

If I have 18 M H2SO4 and I want to make 500 mL of a 1 M H2SO4 solution, what do I do?

4 lines
126.

What volume, in milliliters, of 10.0 M NaOH is needed to prepare 300.0 mL of 2.00 M NaOH by dilution?

a)

0.067 mL

b)

100 mL

c)

60.0 mL

d)

125 mL

127.

What percentage of the total atomic mass of magnesium bromide (MgBr2) is composed of magnesium?

a)

13%

b)

43%

c)

63%

d)

87%

128.

What is the empirical formula of a compound that is 63.52% iron and 36.48% Sulfur?

a)

Fe2S

b)

FeS2

c)

FeS

d)

Fe3O2

129.

Determine the empirical formula of a compound containing 63.50 % silver, 8.25 % nitrogen, and the remainder oxygen.

a)

AgNO3

b)

Ag2NO3

c)

AgNO2

d)

Ag2N2O5

130.
What is the name of the atom pictured here?
a)
Nitrogen-15
b)
Nitrogen-7
c)
Nitrogen-8

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