Free Printable CH. 19 Definitions and Reaction Types

1.

A change in which one or more substances are converted into new substances.

a)

Chemical Equation

b)

Chemical Reaction

c)

Chemical Formula

d)

Products

2.

The starting substances that react

a)

Reactants

b)

Products

c)

Catalysts

d)

Inhibitor

3.

The new substances produced

a)

Reactants

b)

Products

c)

Catalysts

d)

Inhibitor

4.

A way to describe a chemical reaction using chemical formulas and other symbols.

a)

Chemical Formula

b)

Chemical Reaction

c)

Chemical Equation

d)

Chemical Symbols

5.

Represents the number of units of each substance taking part in a reaction.

a)

Susbscript

b)

Superscript

c)

Coefficient

d)

Exponent

6.

A chemical equation with the same number of atoms of each element on both sides of the arrow.

a)

Balanced Chemical Equation

b)

Symmetrical Equation

c)

Equilibrium

d)

LeChatelier's Principle

7.

The mass in grams of one mole of a substance.

a)

Mole

b)

Avogadro's Number

c)

Molar Mass

d)

Coefficients

8.

The amount of a substance that contains 6.02 x 10²³ particles of that substance.

a)

Mole

b)

Molar Mass

c)

Avogadro's Number

d)

Coefficient/s

9.

Occurs when a substance reacts with oxygen to produce energy in the form of heat and light.

a)

Synthesis Reaction

b)

Decomposition Reaction

c)

Double Replacement Reaction

d)

Combustion Reaction

10.

Two or more substances combine to form another substance.

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

11.

Occurs when one substance breaks down, or decomposes, into two or more substances.

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Combustion

12.

The chemical reaction in which one element replaces another element in a compound.

a)

Combustion

b)

Double Replacement

c)

Single Replacement

d)

Decomposition

13.

The positive ion of one compound replaces the positive ion of the other to to form two new compounds.

a)

Combustion

b)

Single Replacement

c)

Double Replacement

d)

Decomposition

14.

An insoluble compound that comes out of solution during a double replacement reaction.

a)

Solid

b)

Aqueous

c)

Liquid

d)

Precipitate

15.

The loss of electrons.

a)

Reduction

b)

Cation

c)

Anion

d)

Oxidation

16.

The gain of electrons.

a)

Reduction

b)

Anion

c)

Cation

d)

Oxidation

17.

Chemical Reactions that release energy.

a)

Exothermic Reactions

b)

Exergonic Reactions

c)

Endothermic Reactions

d)

Endergonic Reactions

18.

When the energy given off is primarily in the form of thermal energy.

a)

Exothermic Reactions

b)

Exergonic Reactions

c)

Endothermic Reactions

d)

Endergonic Reactions

19.

Chemical Reaction that requires energy input in the form of light, thermal energy or electricity in order to proceed.

a)

Exothermic Reaction

b)

Exergonic Reaction

c)

Endothermic Reaction

d)

Endergonic Reaction

20.

When the energy needed to keep a reaction going is in the form of thermal energy.

a)

Exothermic Reaction

b)

Exergonic Reaction

c)

Endothermic Reaction

d)

Endergonic Reaction

21.

The rate at which reactants change into products.

a)

Collision Model

b)

Reaction Rate

c)

Reversible Reaction

d)

Equilibrium

22.

States that atoms, ions, and molecules must collide in order to react.

a)

Inhibitor

b)

Catalyst

c)

Collision Model

d)

LeChatelier's Principle

23.

Substance that speeds up a reaction without being permanently changed itself.

a)

Catalyst

b)

Inhibitor

c)

Reaction Rate

d)

Coefficient

24.

Are used to slow down the rates of chemical reactions or prevent a reaction from happening.

a)

Catalyst

b)

Inhibitor

c)

Reaction Rate

d)

Coefficient

25.

A reaction that can occur in both the forward and reverse directions.

a)

LeChatelier's Principle

b)

Reversible Reaction

c)

Equilibrium

d)

Synthesis

26.

A state in which forward and reverse reactions or processes proceed at equal rates.

a)

LeChatelier's Principle

b)

Reversible Reaction

c)

Synthesis

d)

Equilibrium

27.

States that if a stress is applied to a system at equilibrium, the equilibrium shifts in the direction that opposes the stress.

a)

LeChatelier's Principle

b)

Equilibrium

c)

Reversible Reaction

d)

Inhibitors

28.

K (s) + AuNO3 $\rightarrow$

Will this single replacement reaction take place?

a)

Yes

b)

No

29.

Will this reaction take place?

Cu (s) + H2O $\rightarrow$

a)

Yes

b)

No

30.

Will this reaction take place?
Ag (s) + ZnNO3 $\rightarrow$

a)

Yes

b)

No

31.

Classify the following reaction: $Na_2SO_4\ +Pb\left(NO_3\right)_{2\ }\rightarrow\ NaNO_{3\ }+\ PbSO_4$

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

e)

Combustion

32.

Classify the following reaction: $C_6H_{14}+\ O_2\rightarrow\ CO_2\ +\ H_2O$

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

e)

Combustion

33.

Classify the following reaction: $Ni\left(ClO_{3\ }\right)_2\rightarrow\ NiCl_2+O_2$

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

e)

Combustion

34.

Classify the following reaction: $S_8+F_2\rightarrow\ SF_6$

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

e)

Combustion

35.

Classify the following reaction: $Zn\ +\ HCl\rightarrow\ ZnCl_2+H_2$

a)

Synthesis

b)

Decomposition

c)

Double Replacement

d)

Single Replacement

e)

Combustion

CH. 19 Definitions and Reaction Types

Total questions: 35

Worksheet time: 18mins

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