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Worksheets

Saturday Prep

Total questions: 72

Worksheet time: 1hrs 8mins

Name
Class
Date
1.
Which phrase describes the charge and mass of a neutron?
a)
a charge of +1 and no mass
b)
a charge of +1 and an approximate mass of 1 u.
c)
no charge and no mass
d)
no charge and an approximate mass of 1 u.
2.
What is the number of electrons in a potassium atom?
a)
18
b)
19
c)
20
d)
3
3.
The number of valence electrons in each atom of an element affects the element's
a)
chemical properties
b)
number of isotopes
c)
decay mode
d)
half-life
4.
The nuclides I-131 and I-133 are classified as
a)
isomers of the same element
b)
isomers of Xe-131 and Cs-133
c)
isotopes of the same element
d)
isotopes of Xe-131 and Cs-133
5.
The elements on the Periodic Table are arranged in order of increasing
a)
mass number
b)
atomic number
c)
number of isotopes
d)
number of valence electrons
6.
Compared to a 1.0-gram sample of chlorine gas at standard pressure, a 1.0-gram sample of solid aluminum at standard pressure has
a)
a lower melting point
b)
a higher boiling point
c)
a lower density
d)
a greater volume
7.
Which processes represent one chemical change and one physical change?
a)
freezing and melting
b)
freezing and vaporization
c)
decomposition and melting
d)
decomposition and combustion
8.
In the ground state, an atom of each of the elements in Group 2 has a different
a)
oxidation state
b)
first ionization energy
c)
number of valence electrons
d)
number of electrons in the first shell
9.
Which statement explains why water is classified as a compound?
a)
Water can be broken down by chemical means.
b)
Water is a liquid at room temperature.
c)
Water has a heat of fusion of 334 J/g,
d)
Water is a poor conductor of electricity.
10.

Which formula is an empirical formula?

a)

CH4

b)

C2H6

c)

C3H6

d)

С4Н10

11.

Which compound contains both ionic and covalent bonds?

a)

KI

b)

CaCl2

c)

CH2Br2

d)

NaCN

12.

Given the balanced equation representing a reaction: H2 --> H + H What occurs during this reaction?

a)

Energy is absorbed as bonds are formed.

b)

Energy is absorbed as bonds are broken.

c)

Energy is released as bonds are formed.

d)

Energy is released as bonds are broken.

13.
Parts per million is used to express the
a)
atomic mass of an element
b)
concentration of a solution
c)
volume of a substance
d)
rate of heat transfer
14.

According to Table F, which ions combine with chloride ions to form an insoluble compound?

a)

Fe2+ ions

b)

Ca2+ ions

c)

Li+ ions

d)

Ag+ ions

15.

At 1 atm, equal masses of H2O(s), H2O(l), and H2O(g) have

a)

the same density

b)

the same distance between molecules

c)

different volumes

d)

different percent compositions

16.
Which list includes three forms of energy?
a)
chemical, mechanical, electromagnetic
b)
chemical, mechanical, temperature
c)
thermal, pressure, electromagnetic
d)
thermal, pressure, temperature
17.
At STP a 1-liter sample of Ne(g) and a 1-liter sample of Kr(g) have the same
a)
mass
b)
density
c)
number of atoms
d)
number of electrons
18.
A reaction will most likely occur if the colliding particles have the proper
a)
mass, only
b)
mass and volume
c)
orientation, only
d)
orientation and energy
19.

Which factors have the greatest effect on the rate of a chemical reaction between AgNO3(aq) and Cu(s)?

a)

solution concentration and temperature

b)

solution concentration and pressure

c)

molar mass and temperature

d)

molar mass and pressure

20.
Which expression represents the heat of reaction for a chemical change in terms of potential energy, PE?
a)
(PEproducts) + (PEreactants)
b)
(PEproducts) - (PEreactants)
c)
(PEproducts) × (PEreactants)
d)
(PEproducts) / (PEreactants)
21.
When a chemical reaction is at equilibrium, the concentration of each reactant and the concentration of each product must be
a)
constant
b)
variable
c)
equal
d)
zero
22.
Which element is present in all organic compounds?
a)
nitrogen 
b)
oxygen   
c)
carbon
d)
sulfur
23.
Two types of organic reactions are
a)
deposition and saponification
b)
deposition and transmutation
c)
polymerization and saponification
d)
polymerization and transmutation
24.

Given the balanced equation representing a reaction:


2Al(s) + 3Cu2+(aq) –> 2Al3+(aq) + 3Cu(s)


Which particles are transferred in this reaction?

a)

electrons

b)

neutrons

c)

positrons

d)

protons

25.
In an operating voltaic cell, reduction occurs
a)
at the anode
b)
at the cathode
c)
in the salt bridge
d)
in the wire
26.

Which type of substance yields hydrogen ions, H+ in an aqueous solution?

a)

an Arrhenius acid

b)

an Arrhenius base

c)

a saturated hydrocarbon

d)

an unsaturated hydrocarbon

27.
Phenolphthalein is pink in an aqueous solution having a pH of
a)
5
b)
2
c)
7
d)
12
28.

According to one acid-base theory, NH3 acts as a base when an NH3 molecule

a)

accepts an H+ ion

b)

donates an H+ ion

c)

accepts an OH- ion

d)

donates an OH- ion

29.
Which reaction releases the greatest amount of  energy per mole of reactant?
a)
decomposition
b)
esterfication
c)
fermentation
d)
fission
30.
Which nuclear emission is negatively charged?
a)
an alpha particle
b)
a beta particle
c)
a neutron
d)
a positron
31.

Which electron configuration represents an atom of chlorine in an excited state?

a)

2-7-7

b)

2-7-8

c)

2-8-7

d)

2-8-8

32.

Given the balanced equation representing a reaction occurring at 101.3 kilopascals and 298 K.


2H2(g) + O2(g) → 2H2O(l) + energy


What is the net amount of energy released when one mole of H2O(l) is produced? Hint: Check Table I

a)

241.8 k]

b)

285.8 k]

c)

4836kJ

d)

571.6 k]

33.

Element X reacts with copper to form the compounds CuX and CuX2. In which group on the Periodic Table is element X found?

a)

Group 1

b)

Group 2

c)

Group 13

d)

Group 17

34.

What is the mass of 1.5 moles of CO2?

a)

66g

b)

44g

c)

33g

d)

29g

35.

Given the balanced equation representing a reaction:


K2CO3(aq) + BaCl2(aq) → 2KCl(aq) + BaCO3(s)


Which type of reaction is represented by this equation?

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

36.

Which sample, when dissolved in 1.0 liter of water, produces a solution with the highest boiling point?

a)

0.1 mole KI

b)

0.2 mole KI

c)

0.1 mole MgCl2

d)

0.2 mole MgCl2

37.

Given the balanced equation representing a reaction:


4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(g)


What is the number of moles of H2O(g) formed when 2.0 moles of NH3(g) react completely?

a)

6.0 mol

b)

2.0 mol

c)

3.0 mol

d)

4.0 mol

38.

A rigid cylinder with a movable piston contains a sample of gas. At 300. K, this sample has a pressure of 240. kilopascals and a volume of 70.0 milliliters. What is the volume of this sample when the temperature is changed to 150. K and the pressure is changed to 160. kilopascals?

a)

35.0 mL

b)

52.5 mL

c)

70.0 mL

d)

105 mL

39.

A 100.-gram sample of H2O(L) at 22.0°C absorbs 8360 joules of heat. What will be the final temperature of the water?

a)

18.3°Ꮯ

b)

20.0°Ꮯ

c)

25.7°C

d)

42.0°Ꮯ

40.

Which compound has the strongest hydrogen bonding at STP?

a)

H2O

b)

H3Se

c)

H2S

d)

H3Te

41.

Which formula represents an unsaturated hydrocarbon?

a)

C2H4

b)

С4Н10

c)

C3H8

d)

С5Н12

42.
Which radioisotope is used in dating geological formations?
a)
I-131
b)
U-238
c)
Ca-37
d)
Fr-220
43.

The heating curve above represents a sample of a substance starting as a solid below its melting point and being heated over a period of time.


Which statement describes the energy of the particles in this sample during interval DE?

a)

Both potential energy and average kinetic energy increase.

b)

Both potential energy and average kinetic energy decrease.

c)

Potential energy increases and average kinetic energy remains the same.

d)

Potential energy remains the same and average kinetic energy increases.

44.

Given the potential energy diagram for a reaction:


Which intervals are affected by the addition of a catalyst?

a)

1 and 2

b)

1 and 3

c)

2 and 4

d)

3 and 4

45.

Which balanced equation represents a redox reaction?

a)

Mg + Cl2 ==> MgCl2

b)

CaO + H2O ==> Ca(OH)2

c)

HNO3 + NaOH ==> NaNO3 + H2O

d)

NaCl + AgNO3 ==> AgCl + NaNO3

46.
The pH of a solution is 7. When acid is added to the solution, the hydronium ion concentration becomes 100 times greater. What is the pH of the new solution?
a)
1
b)
5
c)
9
d)
14
47.

A chemical name for this compound is

a)

butanal

b)

butanol

c)

butanone

d)

butanoic acid

48.
What occurs in both fusion and fission reactions?
a)
Small amounts of energy are converted into large amounts of matter.
b)
Small amounts of matter are converted into large amounts of energy.
c)
Heavy nuclei are split into lighter nuclei. 
d)
Light nuclei are combined into heavier nuclei.
49.

Which particle is represented by X?

a)

2812Mg

b)

1813Al

c)

3014Si

d)

2015P

50.

A radioactive isotope has a half-life of 2.5 years. Which fraction of the original mass remains unchanged after 10 years?

a)

1/2

b)

1/4

c)

1/8

d)

1/16

51.
Which type of organic reaction produces both water and carbon dioxide?
a)
addition
b)
combustion
c)
esterfication
d)
fermentation
52.

Which substance is an electrolyte?

a)

O2

b)

Xe

c)

C3H8

d)

KNO3

53.
Which type of matter is represented by the particle diagram?
a)
an element
b)
a compound
c)
a homogeneous mixture
d)
a heterogeneous mixture
54.

Given the formula for an organic compound:


Name the branching group in the box.

a)

butyl

b)

ethyl

c)

methyl

d)

propyl

55.

Which volume of 0.600 M H2SO4(aq) exactly neutralizes 100. milliliters of 0.300 M Ba(OH)2(aq)?

a)

25.0 mL

b)

50.0 mL

c)

100. mL

d)

200. mL

56.

Which hydrocarbon is saturated?

a)

C2H2

b)

C3H4

c)

C3H6

d)

C4H10

57.

Given the equation representing a system at equilibrium: KNO3(s) + energy ==> K+(aq) + NO3-(aq) Which change causes the equilibrium to shift?

a)

increasing pressure

b)

increasing temperature

c)

adding a noble gas

d)

adding a catalyst

58.

Which aqueous solution has the highest boiling point at standard pressure?

a)

1.0 M KCl(aq)

b)

1.0 M CaCl2(aq)

c)

2.0 M KCl(aq)

d)

2.0 M CaCl2(aq)

59.

At standard pressure, what is the temperature at which a saturated solution of NH4Cl has a concentration of 60.g/100. g H2O?

a)

66oC

b)

57oC

c)

22oC

d)

17oC

60.

Given the balanced equation representing a reaction:


2H2O + energy ==> 2H2 + O2


Which statement describes the change in energy and bonding from the reactant?

a)

Energy is absorbed as bonds in H2O are formed.

b)

Energy is absorbed as bonds in H2O are broken.

c)

Energy is released as bonds in H2O are formed.

d)

Energy released as bonds in H2O are broken.

61.

A reaction reaches equilibrium at 100.oC.


The equation and graph representing this reaction are shown.


The graph shows that the reaction is at equilibrium after 60. seconds because the concentrations of both NO2(g) and N2O4(g) are

a)

increasing

b)

decreasing

c)

constant

d)

zero

62.

Given the balanced equation: 2KI + F2 ==> 2KF + I2 What type of chemical reaction does this equation represent?

a)

synthesis

b)

decomposition

c)

single replacement

d)

double replacement

63.
Which statement describes the general trends in electronegativity and atomic radius as the elements in Period 2 are considered in order from left to right?
a)
Both electronegativity and atomic radius increase.
b)
Both electronegativity and atomic radius decrease.
c)
Electronegativity increases and atomic radius decreases.
d)
Electronegativity decreases and atomic radius increases.
64.

What formula represents a nonpolar molecule containing polar covalent bonds?

a)

1

b)

2

c)

3

d)

4

65.

What is the percent composition by mass of nitrogen in (NH4)2CO3 (gram-formula mass =96.0 g/mol)?

a)

14.6%

b)

29.2%

c)

58.4%

d)

87.5%

66.

What is the chemical formula for lead(IV) oxide?

a)

PbO2

b)

PbO4

c)

Pb2O

d)

Pb4O

67.

In the formula XSO4, the symbol X could represent the element

a)

Al

b)

Ar

c)

Mg

d)

Na

68.

Which list of symbols represents nonmetals, only?

a)

B, Al, Ga

b)

Li, Be, B

c)

C, Si, Ge

d)

P, S, Cl

69.

Naturally occurring gallium is a mixture of isotopes that contains 60.11% Ga-69 (atomic mass = 68.93 u) and 39.89% of Ga-71 (atomic mass = 70.92 u). Which numerical setup can be used to determine the atomic mass of naturally occurring gallium?

a)

1

b)

2

c)

3

d)

4

70.

A rigid cylinder with a movable piston contains a sample of helium gas. The temperature of the gas is held constant as the piston is pulled outward. Which graph represents the relationship between the volume of the gas and the pressure of the gas?

a)

1

b)

2

c)

3

d)

4

71.

Which tests demonstrates chemical properties?

a)

1, 3 and 4

b)

1, 3 and 5

c)

2 and 4

d)

2 and 5

72.

Four statements about the development of the atomic model are shown below.


A: Electrons have wavelike properties.

B: Atoms have small, negatively charged particles.

C: The center of an atom is a small, dense nucleus.

D: Atoms are hard, indivisible spheres.

a)

C → D → A → B

b)

C → D → B → A

c)

D → B → A → C

d)

D → B → C → A

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