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Organic and Inorganic Chemistry > chemical reactions - Sheet1 > Flashcards

chemical reactions - Sheet1 Flashcards

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1
Q

Alters state without changing composition.

A

Physical Change

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2
Q

Converts one substance into another.

A

Chemical Change

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3
Q

Starting materials in a chemical reaction.

A

Reactants

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4
Q

Substances formed from a chemical reaction.

A

Products

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5
Q

Symbolic representation of a chemical reaction.

A

Chemical Equation

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6
Q

Numbers indicating molecule quantities in reactions.

A

Coefficients

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7
Q

Atoms cannot be created or destroyed.

A

Law of Conservation of Mass

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8
Q

Equal number of atoms on both sides.

A

Balanced Equation

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9
Q

Two or more reactants form a single product.

A

Combination Reaction

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10
Q

Single reactant converts to multiple products.

A

Decomposition Reaction

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11
Q

One element replaces another in a compound.

A

Single Replacement Reaction

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12
Q

Two compounds exchange parts to form new compounds.

A

Double Replacement Reaction

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13
Q

Loss of electrons from an atom.

A

Oxidation

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14
Q

Gain of electrons by an atom.

A

Reduction

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15
Q

Simultaneous oxidation and reduction processes.

A

Redox Reaction

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16
Q

Causes another compound to be reduced.

A

Reducing Agent

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17
Q

Causes another compound to be oxidized.

A

Oxidizing Agent

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18
Q

Quantity containing 6.022 x 10²³ items.

A

Mole

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19
Q

6.022 x 10²³, number of particles in a mole.

A

Avogadro’s Number

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20
Q

Sum of atomic weights in a compound.

A

Formula Weight

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21
Q

Unit for measuring atomic weights.

A

Atomic Mass Unit (amu)

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22
Q

Separate oxidation or reduction process representation.

A

Half Reaction

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23
Q

Reaction of a substance with oxygen producing heat.

A

Combustion Reaction

24
Q

Compounds composed of hydrogen and carbon.

A

Hydrocarbon

25
Q

Calculation of reactants and products in reactions.

A

Stoichiometry

26
Q

Numbers indicating atom quantities in a formula.

A

Subscripts

27
Q

Abbreviations for chemical elements.

A

Chemical Symbols

28
Q

Relating mass of substance to moles.

A

Mass to Mole Conversion

29
Q

Iron atom with atomic mass 55.85 amu.

A

Fe atom

30
Q

Sulfur atom with atomic mass 32.07 amu.

A

S atom

31
Q

Oxygen atom with atomic mass 16.00 amu.

A

O atom

32
Q

Mass of one mole, in g/mol.

A

Molar mass

33
Q

Ratio used to convert units.

A

Conversion factor

34
Q

Water’s molar mass is 18.02 g/mol.

A

H2O molar mass

35
Q

C9H8O4 with molar mass 180.2 g/mol.

A

Aspirin

36
Q

Ratio of moles from balanced equation.

A

Mole ratio

37
Q

Equation showing equal moles of reactants/products.

A

Balanced equation

38
Q

Maximum expected product from reactants.

A

Theoretical yield

39
Q

Amount of product actually obtained.

A

Actual yield

40
Q

Actual yield divided by theoretical yield.

A

Percent yield

41
Q

Reactant completely consumed in reaction.

A

Limiting reactant

42
Q

Reactant remaining after reaction completion.

A

Excess reactant

43
Q

Conversion using mole ratios from equation.

A

Mole-mole conversion

44
Q

Nitrogen’s molar mass is 28.02 g/mol.

A

Molar mass of N2

45
Q

Oxygen’s molar mass is 32.00 g/mol.

A

Molar mass of O2

46
Q

Using molar mass to find moles from grams.

A

Mass to moles conversion

47
Q

Divide grams by molar mass.

A

Grams to moles conversion

48
Q

Divide number of molecules by Avogadro’s number.

A

Molecules to moles conversion

49
Q

6.022 × 10²³ particles per mole.

A

Avogadro’s number

50
Q

Find moles in 100 g of aspirin.

A

Sample Problem 5.9

51
Q

Calculate molecules in 325 mg of aspirin.

A

Sample Problem 5.10

52
Q

Determine moles of CO from C2H6.

A

Sample Problem 5.11

53
Q

Calculate percent yield of ethanol.

A

Sample Problem 5.14

54
Q

Identify limiting reactant using moles.

A

Sample Problem 5.18

55
Q

Determine limiting reactant using grams.

A

Sample Problem 5.20

Organic and Inorganic Chemistry (3 decks)

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