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Chemistry Baseline Test

Total questions: 90

Worksheet time: 2hrs 12mins

Name
Class
Date
1.

Which subatomic particle carries a positive charge?

a)

Proton

b)

Neutron

c)

Neutrino

d)

Electron

2.

Which subatomic particle carries a negative charge?

a)

Proton

b)

Neutron

c)

Neutrino

d)

Electron

3.

Which subatomic particle has no charge?

a)

Proton

b)

Neutron

c)

Neutrino

d)

Electron

4.

_________ and __________ are located in the nucleus.

a)

Protons

b)

Neutrons

c)

Electrons

d)

Muons

5.

According to the modern atomic model, electrons are found...

a)

in circular orbits of different sizes

b)

in the nucleus

c)

in the electron cloud

d)

in circular orbits of the same size

6.

This atom is an isotope of boron known as:

a)

boron-8

b)

boron-9

c)

boron-10

d)

boron-11

7.

The mass number of this atom is (a)   .

8.

The atomic number of this atom is (a)   .

9.

The atomic number of oxygen is 8. This means that an atom of oxygen-18 has ____ neutrons.

a)

2

b)

8

c)

10

d)

18

10.

Which two individuals described the atom as an indivisible particle?

a)

Bohr and Rutherford

b)

Thomson and Dalton

c)

Dalton and Democritus

d)

Schrodinger and Thomson

11.

Who discovered the electron and developed this model of the atom?

a)

Thomson

b)

Schrodinger

c)

Bohr

d)

Rutherford

12.

This model was developed after _______ bombarded very thin gold foil with alpha particles.

a)

Democritus

b)

Dalton

c)

Thomson

d)

Rutherford

13.

This is a Bohr model. Bohr was the first to indicate that electrons in an atom are found in different ___________.

a)

energy levels

b)

nuclei

c)

electron clouds

d)

plum puddings

14.

Schrödinger's model is the most complicated. He called the places where electrons are most likely to be found _________.

a)

nuclei

b)

orbitals

c)

energy levels

d)

karaoke bars

15.

Which of the following is a nonmetallic element?

a)

Calcium (Ca)

b)

Carbon (C)

c)

Cobalt (Co)

d)

Copper (Cu)

16.

Which of the following represents the correct number of atoms in water (H2O)?

a)

One atom of hydrogen (H) and one atom of oxygen (O)

b)

One atom of hydrogen (H) and two atoms of oxygen (O)

c)

Two atoms of hydrogen (H) and one atom of oxygen (O)

d)

Two atoms of hydrogen (H) and two atoms of oxygen (O)

17.

Which term refers to the amount of energy required to remove one electron from a gaseous atom or ion?

a)

First ionization energy

b)

Second ionization energy

c)

Third ionization energy

d)

Electron affinity

18.

Which explains why noble gases have the highest first ionization energy?

a)

Noble gases have stable atoms.

b)

Noble gases have unstable atoms.

c)

Noble gases are reactive.

d)

Noble gases are nonreactive.

19.

Which property generally decreases across a period?

a)

Atomic number

b)

Atomic radius

c)

Electronegativity

d)

Ionization energy

20.

Rows of elements are called ____.

a)

periods

b)

groups

c)

clusters

d)

levels

21.

Vertical columns in the periodic table are called ___.

a)

periods

b)

metals

c)

metalloids

d)

groups

22.

What is special about Mendeleev's table?

a)

Elements are in groups

b)

Elements are in alphabetical order

c)

Undiscovered elements can be predicted

d)

Radioactive elements are at the bottom

23.

How many electrons are in the outer shell of a carbon (C) atom?

a)

1

b)

2

c)

3

d)

4

24.

How many energy shells does krypton (Kr) have?

a)

1

b)

2

c)

3

d)

4

25.
Which of the following compounds is formed by ionic bonding?
a)
HF
b)
PCl5
c)
MgCl2
d)
CH4
26.

Predict the type of bond that is formed between phosphorus and chlorine.

a)

Ionic

b)

Covalent

c)

Metallic

d)

H-bond

27.

Which pair of elements forms an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

28.

How many valence electrons are shown in the diagram?

a)

16

b)

7

c)

6

d)

2

29.

TRUE OR FALSE: Ionic compounds have high boiling points because they consist of strong ionic bonds.

a)

TRUE

b)

FALSE

30.

Which of the following is NOT an alloy?

a)

bronze

b)

copper

c)

brass

d)

stainless steel

31.

How are covalent bonds formed?

a)

Donating & receiving valence e- between atoms.

b)

Opposite slight charges attract each other between compounds.

c)

Scientists are still not sure how they form.

d)

Sharing valence e- between atoms.

32.

What is the basis of a metallic bond?

a)

the attraction of neutral metal atoms.

b)

the attraction between protons and neutrons.

c)

the attraction between positive metal ions and interlocking electrons.

d)

the attraction between positive metal ions and free-floating electrons.

33.

Examine the image: How many bonds are formed in the model of the compound? Also, identify what type of bond is formed.

a)

2 bonds; covalent

b)

4 bonds; metallic

c)

2 bonds; ionic

d)

4 bonds; covalent

34.

Which type of reaction has the general formula:

AB + CD → AD + CB

a)

Double Replacement

b)

Single Replacement

c)

Synthesis

d)

Decomposition

e)

Combustion

35.

What type of reaction is this?

Cl2 + 2KI → I2 + 2KCl

a)

Synthesis

b)

Single replacement

c)

Double replacement

d)

Decomposition

e)

Combustion

36.

What type of reaction is this?

2C5H10 + 15O2 → 10CO2 + 10H2O

a)

Synthesis

b)

Decomposition

c)

Single replacement

d)

Double replacement

e)

Combustion

37.

What type of reaction is this?

2AgNO3 + Cu → Cu(NO3)2 + 2Ag

a)

Synthesis

b)

Decomposition

c)

Double replacement

d)

Single replacement

e)

Combustion

38.

Which of the following is the general formula for a decomposition reaction?

a)

A + B → AB

b)

AB → A + B

c)

AB + C → AC + B

d)

AB + CD → AC + BD

39.

Using the balanced equation in question 1,
Mg(s) + HCl(aq) → MgCl2(aq) + H2(g)
How many grams of HCl are consumed by the reaction of 2.50 moles of magnesium?

a)

5.00 g

b)

7.29

c)

182 g

d)

218 g

40.

What is the first thing you must do to solve a stoichiometry problem?

a)

Write a balanced equation

b)

Panic

c)

Write an unbalanced equation

d)

Ask for help

41.

For the balanced reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe, what is the ratio of moles of Mg to moles of Fe?

a)

3 mol Mg / 2 mol Fe

b)

2 mol Mg / 3 mol Fe

c)

1 mol Fe / 2 mol Fe

d)

3 mol MgO / 2 mol Fe

42.

2CO + O2 → 2CO2
How many liters of carbon dioxide are produced from 10 L of carbon monoxide?

a)

10

b)

20

c)

1

d)

5

43.

Using the balanced equation in question 5,
CaC₂(s) + H₂O(l) → C₂H₂(g) + Ca(OH)₂(aq)
How many grams of Ca(OH)₂ would be formed from 3.20 moles of CaC₂?

a)

119 g

b)

21.2 g

c)

114 g

d)

237 g

44.

Using the balanced equation from question 9:

C₂H₂(g) + O₂(g) → CO₂(g) + H₂O(g)

How many moles of water (H₂O) are produced when 25.0 grams of C₂H₂ are consumed?

a)

0.960 moles

b)

0.480 moles

c)

1.92 moles

d)

3.84 moles

45.

What state of matter is shown?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

46.

What is the state of matter shown in the image?

a)

Solid

b)

Liquid

c)

Gas

47.

What state of matter is shown in the image?

a)

Solid

b)

Liquid

c)

Gas

48.

Which is not true about the liquid state of matter?

a)

The liquid state has a definite volume and a definite shape.

b)

The liquid state takes the shape of its container.

c)

The liquid state has a definite volume and an indefinite shape.

d)

The particles in a liquid can easily move past each other.

49.

A gas typically consists of:

a)

Low energy particles that experience high attractive forces between them.

b)

Low energy particles that experience no attractive forces between them.

c)

High energy particles that experience high attractive forces between them.

d)

High energy particles that experience little attractive force between them.

50.

Which of the following statements is true regarding the particle structure of liquids? The particles of a liquid are:

a)

very close together, so the liquid cannot easily change its shape.

b)

fast-moving, so they fill the volume of their container.

c)

relatively close together, so they cannot be easily compressed.

d)

very far apart, so they have plenty of room to move around.

51.

The state of matter in which a material has a definite volume and a definite shape is the:

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

52.

Which process could cause a material to change state from gas to liquid?

a)

Adding heat

b)

Adding energy

c)

Removing particles

d)

Removing energy

53.

The substance being dissolved is called the ________

a)

solvent

b)

solid

c)

solute

d)

solvate

54.

A non-electrolyte is composed of __________in solution

a)

molecules

b)

molecules and ions

c)

ions

d)

none of the above

55.

What does "like dissolves like" mean?

a)

polar solvents dissolve in polar solutes

b)

polar solutes dissolve in polar solvents

c)

non-polar solvents dissolve in polar solutes

d)

non-polar solutes dissolve in polar solvents

56.

Gases are more soluble at ______temps and _____pressures

a)

high, low

b)

low , high

c)

high, high

d)

low, low

57.

Molarity concentration is abbreviated as _________

a)

MM.

b)

m.

c)

Mol.

d)

M.

58.

Molarity is defined as _________ divided by ___________

a)

mol, liters

b)

mol, kg

c)

kg, liters

d)

liters, kg

59.

How many mols of HCl are in 3 liters of 2.0M HCl solution?

a)

2.0

b)

1.5

c)

6.0

d)

0.66

60.

A hydrogen ion, H+, is the same as a(n):

a)

neutron

b)

electron

c)

proton

d)

hydroxide ion

61.

OH- is called the:

a)

hydrate ion

b)

hydrogen ion

c)

hydronium ion

d)

hydroxide ion

62.

Acids increase the concentration of what in water?

a)

H+ ions

b)

hydrate ions

c)

hydroxide ions

d)

OH- ions

63.

Bases can be referred to as:

a)

none of the choices

b)

proton acceptors

c)

proton donors

d)

protons

64.

A beaker full of acid is added to a beaker full of base. The pH of the base will:

a)

change constantly

b)

decrease

c)

increase

d)

stay the same

65.

Which substance has the lowest pH?

a)

milk

b)

NaOH

c)

pure water

d)

lemon juice

66.

Any substance that does not conduct electricity when in solution is called a(n) ―

a)

nonelectrolyte

b)

electrolyte

c)

conductor

d)

semiconductor

67.

The diagram shows what happens when zinc reacts with hydrochloric acid. Which of these best describes the energy transformation that occurs during this reaction?

a)

Thermal energy - kinetic energy

b)

Kinetic energy -potential energy

c)

Chemical energy - thermal energy

d)

Potential energy - chemical energy

68.

The diagram represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

a)

Heat energy flows from solid A to solid B. Solid A decreases in temperature

b)

Heat energy flows from solid A to solid B. Solid A increases in temperature

c)

Heat energy flows from solid B to solid A. Solid B decreases in temperature.

d)

Heat energy flows from solid B to solid A. Solid B increases in temperature.

69.
For an endothermic reaction, the heat is on the ____ side.
a)
reactant
b)
product
c)
either side
70.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
71.

A chemical reaction has reached equilibrium when,

a)

the concentrations of the reactants and products are the same

b)

the concentrations of the reactants and products become constant

c)

the forward reaction begins

d)

the reverse reaction begins

72.

When a catalyst is added to a reaction at equilibrium, the rate of the reverse reaction

a)

decreases and the rate of the forward reaction decreases

b)

decreases and the rate of the forward reaction increases

c)

increases and the rate of the forward reaction increases

d)

increases and the rate of the forward reaction decreases

73.

NaCl <-----> Na+ + Cl-

If the above reaction is reversible and reaches equilibrium, and then some Na+ added,

a)

the concentration of Na⁺ will increase

b)

the reaction rate to the right would increase

c)

more NaCl(s) will be produced

d)

the concentration of Na+ will increase and the reaction rate to the right would increase

74.

What is the difference between a voltaic cell and an electrolytic cell?

a)

An electrolytic cell needs a battery

b)

A voltaic cell needs a battery

75.

 Oxidation is the ________ of electrons

a)

Lose

b)

Gain

76.

 Reduction is the _______ of electrons

a)

Lose

b)

Gain

77.

Determine the oxidation state of the following atom: F2

a)

1

b)

2

c)

0

78.

What is the oxidation state of Oxygen in the following compound? H2O

a)

0

b)

+1

c)

-2

79.
Which molecular chemical bond found commonly in organic compounds?
a)
Hydrogen Bond
b)
Ionic Bond
c)
Van Der Waals Force 
d)
Covalent Bond
80.

If the given structure is converted to condensed structure, which will be its correct version?

a)

CH3CH2CH2CH2CH2CH3

b)

CH3(CH2)4CH3

c)

C6H14

d)

(CH3)2(CH2)4

81.

Which of these molecules has a triple covalent bond?

a)

CH4

b)

C2H6

c)

C2H4

d)

C2H2

82.

Which is the structures with IUPAC nomenclature


2,2,4-trimethylpentane

a)
b)
c)
d)
83.

Give the IUPAC name for this compound

a)

3-methyl-4-ethylhexane

b)

3-ethyl-4-methylhexane

c)

3-methyl-4-ethylheptane

d)

3-ethyl-4-methylheptane

84.

Which statement explains the energy term in this reaction?

a)

Mass is lost due to the conversion of energy to mass.

b)

Mass is gained due to the conversion of mass to energy.

c)

Mass is gained due to the conversion of energy to mass.

d)

Mass is lost due to the conversion of mass to energy.

85.

Which risk is related to the radioactive isotopes used to generate electricity?

a)

depletion of atmospheric ozone

b)

exposure to nuclear emissions

c)

depletion of fossil fuels

d)

exposure to acid rain

86.

The study of the composition, structure, and properties of matter and the changes it undergoes.

a)

Chemistry

b)

Physics

c)

Biology

d)

Social Science

87.

The study of carbon containing compounds.

a)

Organic Chemistry

b)

Inorganic Chemistry

c)

Physical Chemistry

d)

Biochemistry

88.

The study of compounds that do not contain carbon.

a)

Organic Chemistry

b)

Inorganic Chemistry

c)

Biochemistry

d)

Analytical Chemistry

89.

The study of the properties and changes in matter and their relation to energy.

a)

Physical Chemistry

b)

Biochemistry

c)

Organic Chemistry

d)

Inorganic Chemistry

90.

What is the subfield of physical chemistry that focuses on the energy changes associated with chemical and physical changes called?

a)

Thermochemistry

b)

Electrochemistry

c)

Nuclear chemistry

d)

Biochemistry

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