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CH141 > Important vocab and concepts > Flashcards

Important vocab and concepts Flashcards

1
Q

element

A

substance that is composed of a single type of atom; cannot be decomposed by a chemical change

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2
Q

extensive property

A

property of a substance that depends on the amount of the substance

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3
Q

heterogeneous mixture

A

combination of substances with a composition that varies from point to point

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4
Q

homogeneous mixture (solution)

A

combination of substances with a composition that is uniform throughout

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5
Q

intensive property

A

property of a substance that is independent of the amount of that substance

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6
Q

law of conservation of matter

A

when matter converts from one type to another or changes form, there is no detectable change in the total amount of matter present

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7
Q

mixture

A

matter that can be separated into its components by physical means

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8
Q

compound

A

pure substance that can be decomposed into two or more elements

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9
Q

pure substance

A

homogenous substance that has a constant composition

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10
Q

atomic mass

A

average mass of atoms of an element (amu)

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11
Q

atomic mass unit (amu)

A

unit of mass = to 1/12 of the mass of a 12C atom

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12
Q

binary acid

A

compound that contains hydrogen and one other element, bonded in a way that imparts acidic properties to the compound

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13
Q

binary compound

A

compound containing two different elements

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14
Q

covalent bond

A

attractive force between the nuclei of a molecule’s atoms and pairs of electrons between atoms

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15
Q

covalent/molecular compound

A

composed of molecules formed buy atoms of two or more different elements

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16
Q

dalton’s atomic theory

A

set of postulates that
established the fundamental properties of atoms

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17
Q

isomers

A

compounds with the same chemical formula but different chemical structures

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18
Q

law of constant composition/definite proportions

A

all samples of a pure compound contain the same elements in the same proportions by mass

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19
Q

law of multiple proportions

A

when two elements react to form more than one compound, a fixed mass of one element will react with masses of the other element in a ratio of small whole numbers

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20
Q

Avogadro’s Number

A

6.022x10^23 mol

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21
Q

solute

A

solution component present in a concentration less than that of the solvent

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22
Q

solvent

A

solution component present in a concentration that is higher relative to other components

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23
Q

acid

A

substance that produces H3O+ when dissolved in water

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24
Q

complete ionic equation

A

chemical equation in which all dissolved ionic reactants and products, including spectator ions, are explicitly represented by formulas for their dissociated ions

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25
Q

end point

A

measured volume of titrant solution that yields the change in sample solution appearance or other property expected for stoichiometric equivalence

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26
Q

equivalence point

A

volume of titrant solution required to react completely with the analyte in a titration analysis; provides a stoichiometric amount of titrant for the sample’s analyte according to the titration reaction

27
Q

insoluble

A

of relatively low solubility; dissolving
only to a slight extent

28
Q

net ionic equation

A

chemical equation in which only those dissolved ionic reactants and products that undergo a chemical or physical change are represented (excludes spectator ions)

29
Q

neutralization reaction

A

reaction between an acid and a base to produce salt and water

30
Q

precipitate

A

insoluble product that forms from reaction of soluble reactants

31
Q

single-displacement reaction

A

(also, replacement) redox reaction involving the oxidation of an elemental substance by an ionic species

32
Q

soluble

A

of relatively high solubility; dissolving to a relatively large extent

33
Q

spectator ion

A

ion that does not undergo a chemical or physical change during a reaction, but its presence is required to maintain charge neutrality

34
Q

stoichiometric factor

A

ratio of coefficients in a balanced chemical equation, used in computations relating amounts of reactants and products

35
Q

strong acid

A

acid that reacts completely when
dissolved in water to yield hydronium ions

36
Q

strong base

A

base that reacts completely when dissolved in water to yield hydroxide ions

37
Q

titrant

A

solution containing a known concentration of substance that will react with the analyte in a titration analysis

38
Q

titration analysis

A

quantitative chemical analysis method that involves measuring the volume of a reactant solution required to completely react with the analyte in a sample

39
Q

weak acid

A

acid that reacts only to a slight extent when dissolved in water to yield hydronium ions

40
Q

weak base

A

base that reacts only to a slight extent when dissolved in water to yield hydroxide ions

41
Q

Amonton’s law (Gay-Lussac’s law)

A

pressure
of a given number of moles of gas is directly proportional to its kelvin temperature when the volume is held constant

42
Q

Avogadro’s law

A

volume of a gas at constant temperature and pressure is proportional to the number of gas molecules

43
Q

Boyle’s law

A

volume of a given number of moles of gas held at constant temperature is inversely proportional to the pressure under which it is measured

44
Q

Charles’s law

A

volume of a given number of moles of gas is directly proportional to its kelvin temperature when the pressure is held constant

45
Q

compressibility factor (Z)

A

ratio of the experimentally measured molar volume for a gas to its molar volume as computed from the ideal gas equation

46
Q

Dalton’s Law of partial pressures

A

total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the component gases

47
Q

ideal gas constant (R)

A

constant derived from the ideal gas equation R = 0.08206 L atm mol–1 K–1 or 8.314 L kPa mol–1 K–1

48
Q

ideal gas law

A

relation between the pressure, volume, amount, and temperature of a gas under conditions derived by combination of the simple gas laws

49
Q

STP

A

273.15 K (0 °C) and 1 atm (101.325 kPa)

50
Q

bomb calorimeter

A

device designed to measure the energy change for processes occurring under conditions of constant volume; commonly used for reactions involving solid and gaseous reactants or products

51
Q

calorie (cal)

A

unit of heat or other energy; the amount of energy required to raise 1 gram of water by 1 degree Celsius; 1 cal is defined as 4.184 J

52
Q

calorimeter

A

device used to measure the amount of heat absorbed or released in a chemical or physical process

53
Q

calorimetry

A

process of measuring the amount of heat involved in a chemical or physical process

54
Q

chemical thermodynamics

A

area of science that deals with the relationships between heat, work, and all forms of energy associated with chemical and physical processes

55
Q

endothermic process

A

chemical reaction or physical change that absorbs heat

56
Q

enthalpy

A

sum of a system’s internal energy and
the mathematical product of its pressure and volume

57
Q

enthalpy change

A

heat released or absorbed
by a system under constant pressure during a
chemical or physical process

58
Q

exothermic process

A

chemical reaction or physical
change that releases heat

59
Q

first law of thermodynamics

A

internal energy of a
system changes due to heat flow in or out of the system or work done on or by the system

60
Q

Hess’s law

A

if a process can be represented as the sum of several steps, the enthalpy change of the process equals the sum of the enthalpy changes of the steps

61
Q

standard enthalpy of combustion

A

heat released when one mole of a compound undergoes complete combustion under standard conditions

62
Q

standard enthalpy of formation

A

enthalpy change of a chemical reaction in which 1 mole of
a pure substance is formed from its elements in their most stable states under standard state conditions

63
Q

standard state

A

set of physical conditions as accepted as common reference conditions for reporting thermodynamic properties; 1 bar of pressure, and solutions at 1 molar concentrations, usually at a temperature of 298.15 K

64
Q

work

A

energy transfer due to changes in
external, macroscopic variables such as pressure and volume; or causing matter to move against an opposing force

CH141 (7 decks)

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