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Physical Science: Semester 2 > Chapter 19 > Flashcards

Chapter 19 Flashcards

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1
Q

a change in which one or more reactants are converted to a new product/substance

A

chemical reaction

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2
Q

initial substances in a chemical reaction

A

reactants

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3
Q

new substances produced as a result of chemical reaction

A

products

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4
Q

a shorthand form of expressing chemical reactions using chemical formulas and other symbols

A

chemical equation

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5
Q

balanced chemical equation

A

a chemical equation with the same number of atoms on both sides

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6
Q

why do chemists use elements in grams instead of amu

A

it’s virtually impossible to select individual atoms of an element. so, the ratios remain the same, but the elements involved are measured in grams.

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7
Q

the amount of a substance containing 6.02 × 10^23 particles of said substance

A

mole

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8
Q

why are moles measured calculated with the number 6.02 × 10^23?

A

sizing up atom portions but keeping the ratios intact causes all elements to be multiplied by the same amount; in this case, by 6.02 x 10^23

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9
Q

the mass in grams of one mole of a substance

A

molar mass

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10
Q

what is true about amu and molar mass

A

they will have the same numeric measurement, but their units will be different

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11
Q

what can you use molar mass to calculate

A

number of moles and mass

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12
Q

a reaction that occurs when a substance reacts with oxygen to produce thermal and light energy

A

combustion reaction

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13
Q

a reaction where two or more substances combine to form another substance

A

synthesis reaction

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14
Q

what is the generalized formula for synthesis reactions

A

A + B = AB

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15
Q

reactions that occur when one substance breaks down, or decomposes, into two or more substances

A

decomposition reactions

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16
Q

what is the general formula for decomposition reactions

A

AB => A + B

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17
Q

c/c decomposition reactions and synthesis reactions

A

they are complete opposites of each other

18
Q

the chemical reaction in which one element replaces another element in a compound

A

single-displacement reaction

19
Q

generalized equation for single-displacement reactions

A

A + BC => AC + B

20
Q

a reaction where the positive ion of one compounds replaces the positive ion of the other to form two new compounds

A

double-displacement reaction

21
Q

generalized equation for double-displacement reaction

A

AB + CD => AD + CB

22
Q

c/c single-displacement and double-displacement reactions

A

single-displacement: one element displaced by another element (AB + C = AC + B)
double-displacement: ions replace each other and one element of each compound is displaced
(AB + CD = AD + CB)

23
Q

an insoluble compound that comes out of a solution from a double-displacement reaction

A

precipitate

24
Q

the loss of electrons during a chemical reaction

A

oxidation

25
Q

the gain of electrons during a chemical reaction

A

reduction

26
Q

c/c oxidation and reduction

A

oxidation: lose electrons
reduction: gain electrons

always come as a pair

27
Q

nickname for the pair that is reduction and oxidation

A

redox

28
Q

chemical reactions that release energy

A

exergonic reaction

29
Q

the rate at which chemical reactions take place

A

reaction rate

30
Q

a ‘commonsense’ idea that explains why reaction rates depend upon external factors; states that atoms, ions, and molecules must collide in order to react

A

collision model

31
Q

why does the collision model matter (in terms of its relations to reaction rate)

A

it explains why reaction rates may change according to external factors, including temperature, concentration, volume and pressure, and surface area.

32
Q

a substance that speeds up a chemical reaction

A

catalyst

33
Q

a substance that slows the rates of chemical reactions

A

inhibitor

34
Q

a reaction that can occur in both the forward and reverse directions (product => reactant => product)

A

reversible reaction

35
Q

equilibrium

A

a state in which forward and reverse reactions/processes proceed at equal rates

36
Q

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

A

Le Châtelier’s principle

37
Q

exergonic reaction that primarily releases thermal energy

A

exothermic reaction

38
Q

chemical reaction where energy is absorbed; such reactions require more energy to break bonds than is released from formation of new bonds

A

endergonic reaction

39
Q

endergonic reaction that primarily requires/absorbs thermal energy in order to continue

A

endothermic reaction

40
Q

c/c endothermic and exothermic reactions

A

exothermic: release thermal energy
endothermic: absorb thermal energy

41
Q

c/c endergonic and exergonic reactions

A

exergonic: energy released from bonding > energy required to break bonds; energy released

endergonic: energy required to break bonds > energy released from bonding; energy absorbed

Physical Science: Semester 2 (11 decks)

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