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Chem > Midterm > Flashcards

Midterm Flashcards

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1
Q

Kilo

A

x103

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2
Q

Hecta

A

x102

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3
Q

Deca

A

x10

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4
Q

Deci

A

x10-1

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5
Q

Centi

A

x10-2

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6
Q

Mili

A

x10-3

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7
Q

element

A

the simplest form of matter that has unique properties (a kind of atom)

pure substance

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8
Q

compound

A

2 or more elements chemically bonded together in a fixed proportion (can be broken)

pure substance

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9
Q

mixture

A

2 or more substances combined physically, not chemically

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10
Q

homogenous mix/solution

A

a mixture that has uniformly distributed components where every sample is the same

can be solid, liquid, gas, aqueous

impure substance

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11
Q

heterogeneous mix

A

a mixture with distinct phases or layers (good for separation of mixtures)

impure substance

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12
Q

Experimental Errors

A

Leaks/Spills

“System”: the way the reaction is conducted

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13
Q

Systematic Error

A

design flaw

not cleaning out beaker/flask/container thoroughly

uncalibrated scale

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14
Q

sig figs

A

way to measure precision of your tools

the # of digits that are not placeholder zeros/the #s recovered from your measurement

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15
Q

precision

A

represents the repeatability of a measurement

recorded in sig figs

technique impacts precision

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16
Q

accuracy

A

how representative the measurement is of what you actually want

measured by % error: |actual - accepted|

——————- x100%

accepted

tools and estimation impact accuracy

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17
Q

adding/subtracting sig figs

A

1) count sig figs to the right of the decimal in each measurement
2) use the lowest number

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18
Q

multiplying/dividing sig figs

A

1) count sig figs in each measurement
2) use lowest number

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19
Q

Aristotle

A

thought: things can be split indefinitely

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20
Q

Democritus

A

thought: there is a limit to the amount something can be split

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21
Q

Dalton

A

found that gases react in multiples of 22.4 L

found that everything reacts in simple whole # ratios (Law of Multiple Proportions)

found that compounds combine in non-varying ratios, a different ratio means a difference compound (Law of Simple Proportions)

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22
Q

Thompson

A

plum pudding model

no nucleus or empty space

neg particles can move around freely (Crookes Tube) ===> permiable, squishy outer layer

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23
Q

Rutherford

A

found the nucleus and empty space in the atom

fixed the electrons into orbits (that forced them to go faster than the speed of light)

shot alpha particles at a piece of thin gold leaf and some of the alpha particles deflected elsewhere ===> there is a hard, dense, positive nucleus, but mostly empty space

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24
Q

Bohr

A

thought that electrons existed in different energy levels (if they couldn’t possibly orbit as Rutherford suggested), but still orbit in those energy shells

he had no reason why this would happen

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25
Q

de Broglie

A

found out that electron are waves, so they have to exist in different energy levels

thought that all materials are wavelike

things like baseballs are too large to be wavelike

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26
Q

electroscope

A

proved there are two charges

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27
Q

isotopes

A

same element, but different masses (different number of nuetrons)

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28
Q

atomic mass

A

of neutrons + protons

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29
Q

atomic number

A

of protons

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30
Q

chemical formulae

A

a symbolic system of letters and numbers that precisely and accurately tells the chemical makeup of a compound

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31
Q

formula mass

A

sum of the atomic masses of every atom in the compound

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32
Q

molar mass

A

the formula mass, but each amu is a gram

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33
Q

number of moles

A

mass given

molar mass

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34
Q

percent mass

A

mass of what you want

————————————- x100%

total mass

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35
Q

atomic structure

A

hard, dense, + nucleus in the center surrounded by energy levels of subshells or a set number of orbitals, which contain 2 electrons each

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36
Q

electron configuration

A

coordinates for the electrons of an element in its ground state

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37
Q

molecular formula

A

C6H12O6

formula mass

—————————— x empirical formula

empirical formula mass

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38
Q

empirical formula

A

the whole # ratio of the atoms in the compound

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39
Q

polarity

A

uneven electron distribution (either in a bond or a compound)

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40
Q

dipole

A

polar

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41
Q

Intramolecular Forces

A

forces inside molecules (Bonds)

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42
Q

Intermolecular Forces

A

attractive forces between molecules (IMF) that hold substances together (+ attracted to -)

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43
Q

Ion-Dipole Forces (IMF)

A

polar molcules attracted to an ion (the ion is atracted to the oppositely charged side of the polar molecule)

44
Q

Hydrogen Bond

A

(not really a bond) hydrogen bonded to an electronegative element (F, Cl, O, S)

45
Q

Dipole-Dipole Forces

A

2 or more polar molecules with IMF (+ attracted to -)

46
Q

Dispersion

A

2 or more nonpolar molecules bump occasionally, which causes a momentary polarity. (the bigger the molecule and more surface areas means more IMF)

47
Q

metallic bonding

A

metal + metal

a group of metal atoms self-ionizes and loses its electrons into a general delocalized pool or bonding electrons

bendy and conducts heat

48
Q

isomers

A

2 or more structures with the same formula, but different structures

49
Q

bond

A

association between 2 or more atoms that stabilizes both atoms, which causes them to stick together

50
Q

ionic

A

transter of electrons from the least electronegative atom to the more electronegative atom

EN > 1.7

w/ metal

51
Q

electronegativity

A

an atom’s pull on an electron

increases to the right: more protons

decreases down: more energy levels, so the electrons are further out

tells the polarity of a molecule

delta EN = |ENatom1 - ENatom2|

52
Q

covalent

A

2 or more atoms have overlapping orbitals, such that the electrons count for both atoms and they statisfy the octet rule (pairs of electrons are shared)

EN ≥ 0.4 polar

EN < 0.4 nonpolar

w/o metal

53
Q

formal charge

A

valence electrons - assigned electrons

you want it to be 0

54
Q

Lewis Dot Structure

A

drawings that represent molecules

1) element symbol represents the atom w/o valence electrons
2) dots represent the valence electrons

55
Q

VSEPR Theory

A

Valence Shell Electron Pair Repulsion

electron shells will orbit themselves in such a way as to minimize repulsion

shapes

56
Q

NH4+1

A

ammounium

57
Q

OH-1

A

hydroxide

58
Q

CO3-2

A

carbonate

59
Q

PO4-3

A

phosphate

60
Q

SO4-2

A

sulfate

61
Q

NO3-1

A

nitrate

62
Q

C2H3O2-1

A

acetate

63
Q

ammounium

A

NH4+1

64
Q

hydroxide

A

OH-1

65
Q

carbonate

A

CO3-2

66
Q

phosphate

A

PO4-3

67
Q

sulfate

A

SO4-2

68
Q

nitrate

A

NO3-1

69
Q

acetate

A

C2H3O2-1

70
Q

Binary Ionic Compounds Naming

A

1) write the + ion
2) write the - ion, drop the last syllable and write “-ide”

71
Q

2 nonmetals bond naming

A

1) write least electronegative
2) write most electronegative
3) add # prefix

1-mono, 2-di, 3-tri, 4-tetra, 5-penta, 6-hexa, 7-septa, 8-octa

72
Q

limiting reactant

A

reactant that will run out first

73
Q

Crystallization

A

heat

separate by melting/boiling point

solid-liquid, liquid-liquid solutions

74
Q

Centrifuge/Separatory Funnel

A

separate by density

75
Q

Filtration

A

separate by size

solid-liquid

76
Q

Attraction/Mechanical

A

separate by force-experiencing mixtures

solid-liquid, solid-solid, solid-gas

77
Q

Distillation

A

heat until one part changes state, condense then separate

gas-gas, liquid-liquid solution

78
Q

Chromatography

A

separate by adhesion/solubility

79
Q

octet rule

A

atoms want 8 electrons (full s and p)

80
Q

valence electrons

A

highest n value

81
Q

quantum numbers

A

numerical values that represent unique electrons

n = energy level

l = subshell (s=0, p=1, d=2, f=3)

m = orbitals (-l to l)

s = spin up/spin down (1/2 or -1/2)

82
Q

excited state

A

an electron in a higher shell than it should be

83
Q

UV transition

A

to and from n = 1

84
Q

Visible transition

A

to and from n = 2

85
Q

IR transition

A

any other transition

86
Q

Blackbody Radiation

A

energy given off by an object because it is heated, objects should go through the colors (ultimately get bluer) as it gets hotter, but it doesn’t

87
Q

Zeff/ENC

A

proton’s pull on electrons - nonvalence electrons

how protons are negatively effected by the nonvalence electrons

increases right: more protons

decreases down: nonvalence electrons increase faster than protons

88
Q

atomic radius

A

1/2 the distance between the center of 2 adjacent atoms

decreases right: same number of shells of electrons and more protons

increases down: more physical size is added (protons, neutrons, electrons)

89
Q

ionization energy

A

energy needed to remove one electron from a neutral atom

increase right: get closer to noble gas configuration, don’t want to get rid of their electrons

decrease down: there is more distance bewteen the electrons and protons

90
Q

ionic radi

A

size of the atom as its most stable ion

+ ions = smaller b/c you lose electrons

  • ions = bigger b/c you add electrons
91
Q

Net Ionic Equations

A

equation showing the ions involved in the chemical reaction

92
Q

stoichiometry

Synthesis

A

element + element —> compound

93
Q

stoichiometry

Decomposition

A

compound —-> element + element

94
Q

stoichiometry

Single Replacement

A

A+B- + C+ —–> C+B- + A+

95
Q

stoichiometry

Combustion

A

H?C? + O2 —–> CO2 + H2O

96
Q

stoichiometry

Double Replacement

A

A+B- + C+D- —–> A+D- + C+B-

97
Q

Mega

A

x106

98
Q

Micro

A

x10-6

99
Q

Nano

A

x10-9

100
Q

Pico

A

x10-12

101
Q

Quantum Mechanical Model

A

explains orbits based on the electron wave interference

102
Q

metallic character

A

ability to lose electrons

decrease right: close to noble gas configuration

increase down: pull of protons is less because more energy levels

103
Q

metals

A

lower electronegativity

lose electrons easily

conduct electricity and heat

bendy/malleable

104
Q

nonmetals

A

gain or share electrons easily

higher electronegativities

brittle

105
Q

metalloids

A

have properties of metals and nonmetals

Chem (8 decks)

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