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CHM 202 > Test 1 > Flashcards

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
Q

KMT law 4

A

Average kinetic energy of an ideal gas is proportional to speed/temp

26
Q

equation from KMT law 4

A

Urms = square root of (3RT/Mw)

27
Q

Two discoveries about real gases (between gas and liquid)

A

atoms in real gases attract and occupy space; ideal equations must be modified to account.

28
Q

VanderWaals Equation

A

(Preal + (an^2/Videal^2))(Videal - nb) = nRT

29
Q

traits of ionic molecules

A

E.N. difference > 2.0, discrete charges, metal + nonmetal

30
Q

traits of polar covalent molecules

A

nonmetals, E.N. difference between 0.5 and 2.0, shape yields dipole

31
Q

traits of non polar covalent molecules

A

nonmetals, not much E.N. difference

32
Q

Ion-dipole =

A

ionic + polar, homogenous bc ions fully dissociate, IMF #1

33
Q

H-bond =

A

dipole-dipole w/ O-H, N-H, or F-H, IMF #2

34
Q

dipole-dipole =

A

polar + polar, homogenous but polar don’t dissociate, IMF #3

35
Q

induced dipole-dipole =

A

non polar + polar, non polar molecule experiences temporary dipole

36
Q

dispersion =

A

non polar + non polar, “sharing” of e’s across molecules, lower frequency of exchange than in covalent bond

37
Q

what causes surface tension?

A

discrepancy between number of interactions a molecule can have between interior and exterior molecules

38
Q

surface tension

A

energy needed to separate molecules at the surface of a liquid

39
Q

cohesion

A

interactions between like particles

40
Q

adhesion

A

interactions between unlike particles

41
Q

meniscus

A

adhesion > cohesion

42
Q

reverse meniscus

A

cohesion > adhesion

43
Q

capillary action

A

process of a liquid flowing in a narrow space without the assistance of, or even in opposition to, any external forces like gravity.

44
Q

viscosity

A

resistance of a liquid to flow due to IMFs, results in a thick, sticky semifluid

45
Q

volatility

A

a measure of how easily a liquid evaporates as a function of pressure and temp

46
Q

vapor pressure

A

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
Q

amorphous solids

A

disordered array of atoms, ions, or molecules (cooled too quickly)

48
Q

crystalline solids

A

ordered array of atoms, ions, or molecules, cooled slowly

49
Q

elemental solids

A

atomic, covalent, or metallic. All are crystalline, all generally 1 element type

50
Q

atomic solids

A

type of elemental solid made of nonmetallic atoms held together strictly by IMFs. PROPERTIES: fairly soft, lower melting points, poor conductivity

51
Q

covalent solids

A

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
Q

metallic solids

A

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
Q

compound solids

A

crystalline solids generally made of 2+ elements in fixed proportions

54
Q

ionic solids

A

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
Q

molecular solids

A

compound solids made of nonmetal nonmetal covalent molecules held by IMFs. PROPERTIES: fairly soft, low to mod melting point, poor conductivity. GRAPHITE!!!

56
Q

Solution solids

A

category of crystalline solid

57
Q

alloy

A

a metal + another element, which may or may not be a metal, mixed in unfixed proportion

58
Q

substitutional alloy

A

solute atoms replace solvent atoms, occurs when approx same size, eg. Fe + Ni, no IMFs

59
Q

interstitial alloy

A

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
Q

simple cubic

A

SC 1 atom

61
Q

body centered cubic

A

BC 2 atoms

62
Q

cubic closest packed

A

FCC 3 atoms

CHM 202 (1 decks)

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