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Chemistry Flashcards

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AP® Biology flashcards Biology 101 flashcards
1
Q

horizontal rows

A

periods

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2
Q

vertical columns

A

groups

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3
Q

alkali metals

A

group 1/1a

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4
Q

alkaline earth metals

A

group 2/2a

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5
Q

transition metals

A

group b/3-12

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6
Q

inner transition metals

rare earth elements

A

lanthanides and actinides

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7
Q

atoms of an element with different number of neutrons

A

isotopes

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8
Q

average of the mass numbers of all known isotopes weighted by their percent abundance

A

molar mass

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9
Q

a technique to determine the mass of various isotopes

A

mass spectrometry

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10
Q

avogadro’s number

A

6.02`

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11
Q

one mole of gas always occupies…

A

22.4 liters

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12
Q

expresses the concentration of a solution in terms of volume

A

molarity

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13
Q

percent by mass of each element that makes up a compound

A

percent composition

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14
Q

represents the simplest ratio of one element to another in a compound

A

empirical formula

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15
Q

represents the actual formula for the substance

A

molecular formula

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16
Q

what states that when building up the electron configuration of an atom, electrons are placed in orbitals, subshells, shells, etc

A

aufbau principle

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17
Q

two electrons which share an orbital cannot have the same spin

A

pauli exclusion principle

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18
Q

when an electron is added to a subshell, it will always occupy an empty orbital if one is available

A

hund’s rule

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19
Q

amount of energy that an electron has depends on its distance from the nucleus of the atom

A

coulomb’s law

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20
Q

experimnetal technique that measures the relative energies of electrons in atoms and molecules

A

photoelectron spectroscopy

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21
Q

it is impossible to know both the position and momentum of an electron at a particular instant

A

heisenberg’s uncertainty principle

22
Q

the approximate distance from the nucleus of an atom to its valence electrons

A

atomic radius

23
Q

positively charged ions

A

cations

24
Q

negatively charge ions

A

anions

25
Q

energy required to remove an electron from an atom

A

first ionization energy

26
Q

energy required to remove an electron from the next electron from the ion

A

second ionization energy

27
Q

refers to how strongly the nucleus of an atom attracts the electrons of other atoms in a bond

A

electronegativity

28
Q

the transferring or sharing of electrons

A

bonds

29
Q

occurs between metals and nonmetals

give up electrons

A

ionic bond

30
Q

two atoms share an electron

A

covalent bonds

31
Q

network solids are held together in a lattice of covalent bonds

A

network covalent bonds

32
Q

process which an impurity is added to an existing lattice

A

doping

33
Q

theory that states that kinetic energy of an ideal gas is directly proportional to its absolute temperature

A

kinetic molecular theory

34
Q

rate at which a gas will escape from a container through microscopic holes in the surface of the container

A

effusion

35
Q

the total pressure of a mixture of gases is just the sum of all the partial pressures of the individual gases in the mixture

A

dalton’s law

36
Q

measure of mass per unit of volume

A

density

37
Q

elements + simple compounds = more complex compunds

A

synthesis reactions

38
Q

single compound is split into two or more elements or simple compounds

A

decomposition

39
Q

acid + base = water and a salt

A

acid-base reaction

40
Q

reaction that results in the change of the oxidation states

A

oxidation reduction reaction

41
Q

carbon + hydrogen (presence of oxygen) = co2 and h2o

A

hydrocarbon combustion

42
Q

two aquaeous solutions that mix and create an insoluble salt

A

precipitation

43
Q

used to determine which reactants are gaining or losing electrons

A

oxidations states

44
Q

energy flow between two substances at different temperatures

A

heat

45
Q

average amount of kinetic energy in a substance

A

temperature

46
Q

energy that must be put into a solid to melt it

A

heat of fusion

47
Q

energy that must be put into liquid to turn it into a gas

A

heat of vaporization

48
Q

measurement of heat changes during chemic reactions

A

calorimetry

49
Q

shows what happens to the temperature of a substance as heat is added

A

heating curve

50
Q

a number that expresses the relationship between the amounts of products and reactants present at equilibrium in a reversible chemical reaction at a give temp

A

equilibrium constant

51
Q

these never reach equilibrium

dissociates completely in water

A

strong acids

52
Q

small fraction of its molecules will dissociate in hydrogen ions and conjugate base ions

A

weak acids

Biology (6 decks)

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