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Chem Sem 2 > Midterm > Flashcards

Midterm Flashcards

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
de Broglie
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
26
electroscope
proved there are two charges
27
isotopes
same element, but different masses (different number of nuetrons)
28
atomic mass
of neutrons + protons
29
atomic number
of protons
30
chemical formulae
a symbolic system of letters and numbers that precisely and accurately tells the chemical makeup of a compound
31
formula mass
sum of the atomic masses of every atom in the compound
32
molar mass
the formula mass, but each amu is a gram
33
number of moles
mass given ------------------- molar mass
34
percent mass
mass of what you want ------------------------------------- x100% total mass
35
atomic structure
hard, dense, + nucleus in the center surrounded by energy levels of subshells or a set number of orbitals, which contain 2 electrons each
36
electron configuration
coordinates for the electrons of an element in its ground state
37
molecular formula
C6H12O6 formula mass ------------------------------ x empirical formula empirical formula mass
38
empirical formula
the whole # ratio of the atoms in the compound
39
polarity
uneven electron distribution (either in a bond or a compound)
40
dipole
polar
41
Intramolecular Forces
forces inside molecules (Bonds)
42
Intermolecular Forces
attractive forces between molecules (IMF) that hold substances together (+ attracted to -)
43
Ion-Dipole Forces (IMF)
polar molcules attracted to an ion (the ion is atracted to the oppositely charged side of the polar molecule)
44
Hydrogen Bond
(not really a bond) hydrogen bonded to an electronegative element (F, Cl, O, S)
45
Dipole-Dipole Forces
2 or more polar molecules with IMF (+ attracted to -)
46
Dispersion
2 or more nonpolar molecules bump occasionally, which causes a momentary polarity. (the bigger the molecule and more surface areas means more IMF)
47
metallic bonding
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
isomers
2 or more structures with the same formula, but different structures
49
bond
association between 2 or more atoms that stabilizes both atoms, which causes them to stick together
50
ionic
transter of electrons from the least electronegative atom to the more electronegative atom EN \> 1.7 w/ metal
51
electronegativity
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
covalent
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
formal charge
valence electrons - assigned electrons you want it to be 0
54
Lewis Dot Structure
drawings that represent molecules 1) element symbol represents the atom w/o valence electrons 2) dots represent the valence electrons
55
VSEPR Theory
Valence Shell Electron Pair Repulsion electron shells will orbit themselves in such a way as to minimize repulsion shapes
56
NH4+1
ammounium
57
OH-1
hydroxide
58
CO3-2
carbonate
59
PO4-3
phosphate
60
SO4-2
sulfate
61
NO3-1
nitrate
62
C2H3O2-1
acetate
63
ammounium
NH4+1
64
hydroxide
OH-1
65
carbonate
CO3-2
66
phosphate
PO4-3
67
sulfate
SO4-2
68
nitrate
NO3-1
69
acetate
C2H3O2-1
70
Binary Ionic Compounds Naming
1) write the + ion 2) write the - ion, drop the last syllable and write "-ide"
71
2 nonmetals bond naming
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
limiting reactant
reactant that will run out first
73
Crystallization
heat separate by melting/boiling point solid-liquid, liquid-liquid solutions
74
Centrifuge/Separatory Funnel
separate by density
75
Filtration
separate by size solid-liquid
76
Attraction/Mechanical
separate by force-experiencing mixtures solid-liquid, solid-solid, solid-gas
77
Distillation
heat until one part changes state, condense then separate gas-gas, liquid-liquid solution
78
Chromatography
separate by adhesion/solubility
79
octet rule
atoms want 8 electrons (full s and p)
80
valence electrons
highest n value
81
quantum numbers
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
excited state
an electron in a higher shell than it should be
83
UV transition
to and from n = 1
84
Visible transition
to and from n = 2
85
IR transition
any other transition
86
Blackbody Radiation
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
Zeff/ENC
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
atomic radius
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
ionization energy
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
ionic radi
size of the atom as its most stable ion + ions = smaller b/c you lose electrons - ions = bigger b/c you add electrons
91
Net Ionic Equations
equation showing the ions involved in the chemical reaction
92
# stoichiometry Synthesis
element + element ---\> compound
93
# stoichiometry Decomposition
compound ----\> element + element
94
# stoichiometry Single Replacement
A+B- + C+ -----\> C+B- + A+
95
# stoichiometry Combustion
H?C? + O2 -----\> CO2 + H2O
96
# stoichiometry Double Replacement
A+B- + C+D- -----\> A+D- + C+B-
97
Mega
x106
98
Micro
x10-6
99
Nano
x10-9
100
Pico
x10-12
101
Quantum Mechanical Model
explains orbits based on the electron wave interference
102
metallic character
ability to lose electrons decrease right: close to noble gas configuration increase down: pull of protons is less because more energy levels
103
metals
lower electronegativity lose electrons easily conduct electricity and heat bendy/malleable
104
nonmetals
gain or share electrons easily higher electronegativities brittle
105
metalloids
have properties of metals and nonmetals

Chem Sem 2 (6 decks)

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