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Chemistry Regents Quick Facts

Total questions: 140

Worksheet time: 1hrs 14mins

Name
Class
Date
1.

Charge of an electron

a)

Positive

b)

Negative

c)

Neutral

2.

Charge of an proton

a)

Positive

b)

Negative

c)

Neutral

3.

Charge of a neutron

a)

Positive

b)

Negative

c)

Neutral

4.

How do you know the number of protons

a)

Atomic Number

b)

Mass Number

5.

Overall charge of an atom

a)

Positive

b)

Negative

c)

Neutral

6.

An atom with a charge.

a)

Ion

b)

Electrolyte

c)

Neutral

7.

How do you find the number of electrons in an atom

a)

Same as Mass

b)

8

c)

0

d)

Same as Atomic #

8.

How do you find the number of neutrons?

a)

0

b)

Same as protons

c)

Mass-Protons

d)

Protons - Electrons

9.

Isotopes have... (CHECK ALL THAT APPLY)

a)

Same number of protons

b)

Different number of neutrons

c)

Different number of electrons

d)

Different Masses

e)

Different Atomic Numbers

10.

Rutherford's Gold Foil...(Check all the apply)

a)

Atom is mostly empty space

b)

Small, dense, positively charged nucleus

c)

Electrons are surrounding the nucleus

d)

Some particles deflected (bounced back)

e)

Most particles passed through

11.

Have a mass of 1 amu... (check all that apply)

a)

Protons

b)

Neutrons

c)

Electrons

12.

Area of probability of finding an electron

a)

Orbit

b)

Orbital

c)

Nucleus

d)

Core

13.

Modern model of atom with electrons in orbitals

a)

Hard Sphere

b)

Rutherford

c)

Bohr

d)

Wave-Mechanical

14.

Which electrons have more energy?

a)

Shells closer to nucleus

b)

Shells further from nucleus

15.

Ground State --> Excited State

a)

Absorb Energy

b)

Release Energy

16.

Excited State --> Ground State

a)

Absorb Energy

b)

Release Energy (Light)

17.

Periodic Table organized in order of increasing...

a)

Atomic Mass

b)

Electronegativity

c)

Atomic Number

d)

Oxidation States

18.

Affinity (attraction) towards electron

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

19.

Size of the atom

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

20.

Amount of energy required to remove an electron

a)

Electronegativity

b)

Ionization Energy

c)

Atomic Radius

d)

Atomic Mass

21.

Where can you look up trends in Electronegativity, Ionization Energy, and Atomic Radius?

a)

Table A

b)

Table S

c)

Periodic Table

d)

Table I

22.

Left of Staircase (not H)

a)

Metal

b)

Nonmetal

c)

Metalloid

23.

Staircase

a)

Metal

b)

Nonmetal

c)

Metalloid

24.

Rightt of Staircase (plus H)

a)

Metal

b)

Nonmetal

c)

Metalloid

25.

Liquid at STP... (check all that apply)

a)

Hg

b)

H

c)

Si

d)

Br

e)

O

26.

Noble Gas

a)

Group 1

b)

Group 2

c)

Group 17

d)

Group 18

27.

Noble Gases have _____ valence electrons so they are ______.

a)

0, reactive

b)

8, reactive

c)

0, unreactive

d)

8, unreactive

28.

The # of Electrons SHARED in a single bond

a)

1

b)

2

c)

4

d)

6

29.

The # of Electrons SHARED in a double bond

a)

1

b)

2

c)

4

d)

6

30.

The # of Electrons SHARED in a triple bond

a)

1

b)

2

c)

4

d)

6

31.

The # of PAIRS of Electrons in a single bond

a)

1

b)

2

c)

4

d)

6

32.

Break Bonds...

a)

Absorb Energy

b)

Release Energy

33.

Form Bonds...

a)

Absorb Energy

b)

Release Energy

34.

Shows # of atoms

a)

Structural Formula

b)

Molecular Formula

c)

Empirical Formula

35.

Shows arrangement of atoms

a)

Structural Formula

b)

Molecular Formula

c)

Empirical Formula

36.

Reduced/simplified version of the formula

a)

Structural Formula

b)

Molecular Formula

c)

Empirical Formula

37.

CANNOT be broken down by a chemical change

a)

Element

b)

Compound

c)

Mixture

d)

Solution

38.

Atoms are chemically combined in a fixed proportion that cannot be changed.

a)

Element

b)

Compound

c)

Mixture

d)

Solution

39.

Heterogeneous mixture

a)

Evenly mixed

b)

Unevenly mixed (has layers)

40.

Homogeneous mixture

a)

Evenly mixed

b)

Unevenly mixed (has layers)

41.

Solutions are...

a)

homogeneous mixtures

b)

heterogeneous mixtures

42.

Similar chemical properties

a)

Same number of neutrons

b)

Same number of valence electrons

c)

Same mass

d)

Same color

43.

Phase (solid/liquid/gas), Melting/Boiling point, Density

a)

Physical Properties

b)

Chemical Properties

44.

Phase Changes are...

a)

Physical Changes

b)

Chemical Changes

45.

Rusting, Oxidized, Reacts, Synthesized, Decomposed, Combusts

a)

Physical Changes

b)

Chemical Changes

46.

Metal/Nonmetal

a)

Ionic Bond

b)

Covalent Bond

47.

Two Nonmetals

a)

Ionic Bond

b)

Covalent Bond

48.

Electrons Shared

a)

Ionic Bond

b)

Covalent Bond

49.

Electrons Transfered

a)

Ionic Bond

b)

Covalent Bond

50.

Electrons shared equally

a)

Ionic Bond

b)

Nonpolar Covalent Bond

c)

Polar Covalent Bond

d)

Hydrogen Bond

51.

Electrons shared unequally

a)

Ionic Bond

b)

Nonpolar Covalent Bond

c)

Polar Covalent Bond

d)

Hydrogen Bond

52.

Bond polarity is determined by difference in...

a)

Ionization Energy

b)

Electronegativity

c)

Atomic Number

d)

Atomic Mass

53.

X --> Y + Z

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

e)

Combustion

54.

A + B --> C

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

e)

Combustion

55.

Element + Compound --> Element + Compound

(A + BC --> B + AC)

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

e)

Combustion

56.

Compound + Compound --> Compound + Compound

(WX + YZ --> WZ + YX)

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

e)

Combustion

57.

Hydrocarbon + O2 --> CO2 + H2O

a)

Synthesis

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

e)

Combustion

58.

Acid + Base --> Salt + Water

a)

Synthesis

b)

Neutralization

c)

Decomposition

d)

Combustion

59.

What happens when you increase the concentration of ions in a solution? (CHECK ALL THAT APPLY)

a)

Lower Freezing Point

b)

Higher Freezing Point

c)

Lower Boiling Point

d)

Higher Boiling Point

60.

Which are forms of ENERGY? (CHECK ALL THAT APPLY!)

a)

Nuclear

b)

Electromagentic

c)

Thermal

d)

Temperature

e)

Chemical

61.

Real Gases are most like Ideal Gases at...

a)

Low Temperature & Low Pressure

b)

Low Temperature & High Pressure

c)

High Temperature & Low Pressure

d)

High Temperature & High Pressure

62.

Effective Collisions have proper...

a)

energy and charge

b)

orientation and charge

c)

energy and orientation

d)

charge and mass

63.

At Equilibrium... (CHECK ALL THAT APPLY)

a)

Rates are Equal

b)

Rates are Constant

c)

Concentrations are Equal

d)

Concentrations are Constant

64.

Which phase is a mixture?

a)

s

b)

l

c)

g

d)

aq

65.

Temperature

a)

Average Potential Energy

b)

Average Kinetic Energy

c)

Average Atomic Mass

d)

Average Ionization Energy

66.

Systems in nature favor...

a)

Low Energy & Low Entropy

b)

Low Energy & High Entropy

c)

High Energy & Low Entropy

d)

High Energy & High Entropy

67.

All C-C Single Bonds

a)

Alkane

b)

Alkene

c)

Alkyne

68.

Have a C-C Double Bond

a)

Alkane

b)

Alkene

c)

Alkyne

69.

Have a C-C Triple Bond

a)

Alkane

b)

Alkene

c)

Alkyne

70.

Saturated Hydrocarbons (Check all that apply)

a)

Alkane

b)

Alkene

c)

Alkyne

71.

Unsaturated Hydrocarbons (Check all that apply)

a)

Alkane

b)

Alkene

c)

Alkyne

72.

Reaction that occurs at the Anode

a)

Oxidation

b)

Reduction

73.

Reaction that occurs at the Cathode

a)

Oxidation

b)

Reduction

74.

Which is not an organic reaction?

a)

Substitution

b)

Combustion

c)

Addition

d)

Distillation

e)

Polymerization

75.

Organic Reaction where one atom replaces a hydrogen in an alkane.

a)

Combustion

b)

Substitution

c)

Addition

d)

Polymerization

e)

Fermentation

76.

Organic Reaction where a double or triple bond is broken and other atoms are attached to make it saturated

a)

Combustion

b)

Substitution

c)

Addition

d)

Polymerization

e)

Fermentation

77.

Organic Reaction where small subunits are linked together to make larger ones.

a)

Combustion

b)

Substitution

c)

Addition

d)

Polymerization

e)

Fermentation

78.

Spontaneous electrochemical cells

a)

Voltaic

b)

Electrolytic

79.

Nonspontaneous electrochemical cells

a)

Voltaic

b)

Electrolytic

80.

Electrochemical cells that require a battery/power source

a)

Voltaic

b)

Electrolytic

81.

Electrons flow...

a)

through the wire from anode to cathode.

b)

through the wire from anode to cathode.

c)

through the salt bridge in both directions

d)

through the salt bridge from anode to cathode.

e)

through the salt bridge from cathode to anhode.

82.

Ions flow...

a)

through the wire from anode to cathode.

b)

through the wire from anode to cathode.

c)

through the salt bridge in both directions

d)

through the salt bridge from anode to cathode.

e)

through the salt bridge from cathode to anhode.

83.

Purpose of a salt bridge (CHECK ALL THAT APPLY)

a)

Keep cell electrically neutral

b)

Allow ions to flow

c)

Allow electrons to flow

d)

Provide electrolytes to conduct electricity

84.

Oxidation

a)

Lose electrons, become negative

b)

Lose electrons, become positive

c)

Gain electrons, become negative

d)

Gain electrons, become positive

85.

Reduction

a)

Lose electrons, become negative

b)

Lose electrons, become positive

c)

Gain electrons, become negative

d)

Gain electrons, become positive

86.

Separation based on particle size

a)

Distillation

b)

Evaporation

c)

Filtration

d)

Chromatography

e)

Electrolysis

87.

Separation based on boiling points

a)

Distillation

b)

Evaporation

c)

Filtration

d)

Chromatography

e)

Electrolysis

88.

Which measure CONCENTRATION? (Check all that apply)

a)

Kelvin

b)

ppm

c)

M (Molarity)

d)

mol/L

e)

Joules

89.

Which is a property of a gas according to Kinetic Molecular Theory? (CHECK ALL THAT APPLY)

a)

Particles move in random straight line motion

b)

No attraction between gas particles

c)

Gas particles have negligible volume

d)

No loss of energy during collisions

90.

Definite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

91.

Indefinite shape and definite volume

a)

Solid

b)

Liquid

c)

Gas

92.

Indefinite shape and indefinite volume

a)

Solid

b)

Liquid

c)

Gas

93.

Adding a catalyst... (CHECK ALL THAT APPLY)

a)

Lowers activation energy

b)

Speeds up chemical reaction

c)

Lowers the heat of reaction

d)

Provides an alternate reaction pathway

e)

Makes endothermic reactions exothermic

94.

Potential Energy of Products - Potential Energy of Reactants

a)

Activation Energy

b)

Heat of Reaction

c)

Heat of Fusion

d)

Average Kinetic Energy

95.

Melting/Fusion, Vaporization/Boiling, and Sublimation

a)

Endothermic with increasing entropy.

b)

Exothermic with increasing entropy.

c)

Endothermic with decreasing entropy.

d)

Exothermic with decreasing entropy.

96.

Condensation, Freezing, and Deposition

a)

Endothermic with increasing entropy.

b)

Exothermic with increasing entropy.

c)

Endothermic with decreasing entropy.

d)

Exothermic with decreasing entropy.

97.

Disorder of molecules / Randomness

a)

Heat of Reaction

b)

Activation Energy

c)

Entropy

d)

Electronegativity

98.

Which phase has the greatest disorder?

a)

s

b)

l

c)

g

d)

aq

99.

Organic compounds must have...

a)

Sulfur

b)

Oxygen

c)

Nitrogen

d)

Sulfur

e)

Carbon

100.

H+ Donors

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

101.

H+ Acceptors

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

102.

Produce OH- in water

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

103.

High concentration of H+ / H3O+

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

104.

Electrolytes (CHECK ALL THAT APPLY)

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

105.

Substances that conduct electricity when dissolved in water

a)

Electrolytes

b)

Metals

c)

Nonmetals

d)

Nonelectrolytes

106.

Substances that conduct electricity in the solid phase

a)

Electrolytes

b)

Metals

c)

Nonmetals

d)

Nonelectrolytes

107.

Start with an H

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

108.

Ionic Solids

(Metal/Nonmetal)

(Metal/Polyatomic)

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

109.

Metal + OH

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

110.

End in COOH

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

111.

Carbon/Hydrogen + OH

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

112.

Carbon/Hydrogen/Oxygen in that order

a)

Acids

b)

Bases

c)

Salts

d)

Sugars

e)

Alcohols

113.

Chemical energy --> Electrical energy

a)

Voltaic Cell

b)

Electrolytic Cell

114.

Electrical energy --> Chemical energy

a)

Voltaic Cell

b)

Electrolytic Cell

115.

Table G, on the line

a)

Unsaturated

b)

Saturated

c)

Supersaturated

116.

Table G, below the line

a)

Unsaturated

b)

Saturated

c)

Supersaturated

117.

Table G, above the line

a)

Unsaturated

b)

Saturated

c)

Supersaturated

118.

Solutions are at equilibrium when they are...

a)

Unsaturated

b)

Saturated

c)

Supersaturated

119.

During a phase change, temperature...

a)

increases, always.

b)

decreases, always.

c)

remains constant.

d)

increases or decreases depending on the change.

120.

One change in pH = ____ change in acidity

a)

1x

b)

2x

c)

10x

d)

14x

121.

"Substance" refers to... (CHECK ALL THAT APPLY)

a)

Element

b)

Compound

c)

Mixture

d)

Solution

122.

Insoluble compounds in water form...

a)

Solutions

b)

Homogeneous Mixtures

c)

Heterogeneous Mixtures

123.

In a REDOX reaction, the metal higher on Table J is the one that is..

a)

Oxidized

b)

Reduced

124.

Strongest IMF

a)

van der Waals

b)

Dipole-Dipole

c)

Hydrogen Bonding

125.

Higher Boiling Point = _____ IMFs

a)

Stronger

b)

Weaker

126.

Higher Vapor Pressure = _____ IMFs

a)

Stronger

b)

Weaker

127.

Isomers have...

a)

same molecular and structural formulas.

b)

different molecular and structural formulas.

c)

same molecular formula with different structural formulas.

d)

same structural formula with different molecular formulas.

128.

Split the nucleus of a heavy atom

a)

Fission

b)

Fusion

c)

Both

129.

Combining two light nuclei to form a larger one

a)

Fission

b)

Fusion

c)

Both

130.

Small amounts of mass are converted to large amounts of energy.

a)

Fission

b)

Fusion

c)

Both

131.

In an acid..

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

132.

In a base..

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

133.

In a neutral solution..

a)

[H3O+] = [OH-]

b)

[H3O+] > [OH-]

c)

[H3O+] < [OH-]

134.

The substance being dissolved

a)

Solute

b)

Solvent

c)

Solution

135.

The substance doing the dissolving, often water.

a)

Solute

b)

Solvent

c)

Solution

136.

Symmetrical molecules are...

a)

Polar

b)

Nonpolar

137.

Asymmetrical molecules are...

a)

Polar

b)

Nonpolar

138.

Water molecules are...

a)

Polar

b)

Nonpolar

139.

Polar molecules...

a)

Dissolve polar molecules.

b)

Dissolve nonpolar molecules.

c)

Dissolve both polar and nonpolar molecules.

d)

Do not dissolve anything.

140.

Nonpolar molecules...

a)

Dissolve polar molecules.

b)

Dissolve nonpolar molecules.

c)

Dissolve both polar and nonpolar molecules.

d)

Do not dissolve anything.

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