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Test 1 Flashcards

1
Q

Molecular geometry w/ 2

A

linear

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2
Q

Molecular geometry w/ 3

A

trigonal planar

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3
Q

Molecular geometry w/ 4

A

tetrahedral

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4
Q

Molecular geometry w/ 5

A

trigonal bipyramidal

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5
Q

Molecular geometry w/ 6

A

octahedral

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6
Q

Avogadro’s number

A

6.022*10^23

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7
Q

Boyle’s Law

A

P1V1 = P2V2

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8
Q

Amontons’ Law

A

P1/T1 = P2/T2

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9
Q

Charles’ Law

A

V1/T2 = V2/T2

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10
Q

0K (absolute zero) =

A

-273.15 C

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11
Q

Combined Gas Law

A

(P1V1)/T1 = (P2V2)/T2

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12
Q

Dalton’s law

A

Plot = P1 + P2 + P3 +…

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13
Q

Avogadro’s Law

A

V1/n1 = V2/n2

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14
Q

Mole Fractions

A

Ptot/ntot = P1/n1 = P2/n2 = P3/n3 = …

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15
Q

Ideal Gas Law

A

PV = nRT

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16
Q

who found the ideal gas law?

A

Clapeyron

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17
Q

diffusion

A

the spread of one substance into another on its own

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18
Q

effusion

A

the process of moving thru an opening from a higher pressure region to a lower pressure region

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19
Q

Graham’s Law

A

rate of effusion, measured by the root mean squared speed, is inversely proportional to the root of the molar mass

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20
Q

Who discovered KMT?

A

Rudolph Clausius

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21
Q

What does KMT do?

A

It explains the gas laws and how they connect to the kinetic motion of particles

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22
Q

KMT law 1

A

Ideal gas molecules are infinitely small; take up no space; are separated by relatively long distances

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23
Q

KMT law 2

A

Idea gas molecules move constantly and randomly

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24
Q

KMT law 3

A

Ideal gases are not attracted or repelled by other gases, they collide elasticly

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25
KMT law 4
Average kinetic energy of an ideal gas is proportional to speed/temp
26
equation from KMT law 4
Urms = square root of (3RT/Mw)
27
Two discoveries about real gases (between gas and liquid)
atoms in real gases attract and occupy space; ideal equations must be modified to account.
28
VanderWaals Equation
(Preal + (an^2/Videal^2))(Videal - nb) = nRT
29
traits of ionic molecules
E.N. difference > 2.0, discrete charges, metal + nonmetal
30
traits of polar covalent molecules
nonmetals, E.N. difference between 0.5 and 2.0, shape yields dipole
31
traits of non polar covalent molecules
nonmetals, not much E.N. difference
32
Ion-dipole =
ionic + polar, homogenous bc ions fully dissociate, IMF #1
33
H-bond =
dipole-dipole w/ O-H, N-H, or F-H, IMF #2
34
dipole-dipole =
polar + polar, homogenous but polar don't dissociate, IMF #3
35
induced dipole-dipole =
non polar + polar, non polar molecule experiences temporary dipole
36
dispersion =
non polar + non polar, "sharing" of e's across molecules, lower frequency of exchange than in covalent bond
37
what causes surface tension?
discrepancy between number of interactions a molecule can have between interior and exterior molecules
38
surface tension
energy needed to separate molecules at the surface of a liquid
39
cohesion
interactions between like particles
40
adhesion
interactions between unlike particles
41
meniscus
adhesion > cohesion
42
reverse meniscus
cohesion > adhesion
43
capillary action
process of a liquid flowing in a narrow space without the assistance of, or even in opposition to, any external forces like gravity.
44
viscosity
resistance of a liquid to flow due to IMFs, results in a thick, sticky semifluid
45
volatility
a measure of how easily a liquid evaporates as a function of pressure and temp
46
vapor pressure
the pressure of a gas directly over the surface of its liquid or solid form. "how much liquid is naturally escaping into the gaseous state?"
47
amorphous solids
disordered array of atoms, ions, or molecules (cooled too quickly)
48
crystalline solids
ordered array of atoms, ions, or molecules, cooled slowly
49
elemental solids
atomic, covalent, or metallic. All are crystalline, all generally 1 element type
50
atomic solids
type of elemental solid made of nonmetallic atoms held together strictly by IMFs. PROPERTIES: fairly soft, lower melting points, poor conductivity
51
covalent solids
type of elemental solid made of nonmetallic atoms held together by an extended 3D network of covalent bonds. PROPERTIES: brittle, higher melting points, poor conductivity.
52
metallic solids
type of elemental solid made of metallic atoms held together by metal-metal bonds, which are ductile and malleable. metallic characteristics arise due to delocalized e's in bonds.
53
compound solids
crystalline solids generally made of 2+ elements in fixed proportions
54
ionic solids
compound solids made of metal + nonmetal molecules. alternating cations and anions held by ionic bonds. PROPERTIES: hard and brittle, moderate melting point, poor conductivity but decent when molten.
55
molecular solids
compound solids made of nonmetal nonmetal covalent molecules held by IMFs. PROPERTIES: fairly soft, low to mod melting point, poor conductivity. GRAPHITE!!!
56
Solution solids
category of crystalline solid
57
alloy
a metal + another element, which may or may not be a metal, mixed in unfixed proportion
58
substitutional alloy
solute atoms replace solvent atoms, occurs when approx same size, eg. Fe + Ni, no IMFs
59
interstitial alloy
occurs when non-host material is much smaller than host material and can occupy existing spaces within the crystal lattice of the host metal. E.G. Fe + C
60
simple cubic
SC 1 atom
61
body centered cubic
BC 2 atoms
62
cubic closest packed
FCC 3 atoms

CHM 202 (1 decks)

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