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chem 101 > ch 7 > Flashcards

ch 7 Flashcards

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1
Q

kinetic energy

A

energy from particle motion

  • disruptive forces
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2
Q

potential energy

A

stored from position, condition, composition

  • cohesive forces
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3
Q

electrostatic interaction

A

attractions/repulsions from charged particles

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4
Q

kinetic molecular theory of matter

A
  1. matter has def sizes that don’t change
  2. matter/particles in constant random motion containing KE
  3. particles interact thru attractions/repulsions and have potential energy
  4. KE INC as temp. INC
  5. energy transferred thru elastic collisions
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5
Q

compressibility

A

changes in volume from PRESSURE change

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6
Q

thermal expansion

A

changes in volume from TEMP change

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7
Q

KMT - solid

A

PE > KE

  • reg pattern
  • close packing
  • small expansion
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8
Q

KMT - liquid

A

PE = KE

  • random irreg pattern
  • close packing
  • small expansion
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9
Q

KMT - gas

A

PE < KE

  • irreg. pattern
  • widely separated, high compression
  • medium expansion
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10
Q

gas law units

A

atm, moles, L/mL, K

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11
Q

gas law

A

pressure = force/area

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12
Q

1 mm Hg =

A

1 torr

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13
Q

1 atm = ? mm Hg/torr

A

760 mm Hg, torr

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14
Q

1 atm = ? psi

A

14.7 psi

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15
Q

boyle’s law

A

p1 x v1 = p2 x v2

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16
Q

boyle’s law - volume decreases…

A

less room for molecules, more collisions, MORE pressure

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17
Q

boyle’s law - volume increases…

A

more room for molecules, less collisions, LOWER pressure

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18
Q

charles’s law

A

v1/t1 = v2/t2

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19
Q

charles’s law - temp increases…

A

KE of gas molecules INC., hit container walls more, volume INC

20
Q

charles’s law - temp decreases…

A

KE of gas molecules DEC., hit container walls less, volume DEC.

21
Q

combined gas law

A

p1v1 p2v2
____ = ______
t1 t2

22
Q

ideal gas law

A

NO CHANGES OCCUR

PV = nRT

23
Q

R =

A

0.0821 atm

24
Q

dalton’s law of partial pressures

A

Ptotal = P1 + P2 + P3…

25
Q

partial pressure

A

pressure a gas in a mixture would exert, if it were alone

26
Q

endothermic

A

heat absorbed

  • evaporation, melting, sublimation (S–>G)
27
Q

exothermic

A

heat released

  • condensation, freezing, deposition (G–>S)
28
Q

evaporation increases as …

A

temp inc. –> gas inc –> pressure inc

29
Q

ext pressure inc. –> …

A

higher BP –> harder to evap –> lower evap rate

30
Q

boiling

A

form of evap. occuring within L as bubbles, requires heat

31
Q

boiling point

A

temp where vapor pressure = ext. pressure

32
Q

normal BP

A

760 mm Hg

33
Q

higher altitude –> BP?

A

air pressure diminished, BP dec.

34
Q

lower altitude –> BP?

A

air pressure inc., BP inc.

35
Q

physical equilibrium

A

when 2 opposing phys. proccesses occur at same rate

  • vapor exerts vapor pressure onto L and surroundings
36
Q

vapor pressure for Ls w/ STRONG attractive forces

A

low vapor pressure

37
Q

vapor pressure for Ls w/ WEAK attractive forces

A

high vapor pressure

38
Q

vapor pressure of liquids

A
  1. evap starts bc little to no vapor
  2. evap. rate INCREASES
  3. evap and condensation rate become =, both phases (L and vapor) remain constant
39
Q

volatile substance

A

readily evaps. at room temp. b/c high vapor pressure

40
Q

dipole-dipole interactions

A

btwn POLAR molecules

+ and - ends interact w/ eachother

stronger polarity –> stronger DD interaction –> higher BP

41
Q

hydrogen bonds

A

special dipole-diple interaction where hydrogen is bonded to v. electroneg atoms (v strong)

  • not cov. bonding, INTERACTION
42
Q

electroneg atoms for hydrogen bonding

A

FON

43
Q

density-temp relationship

A

lower temp –> lower density

44
Q

london forces

A
  • polar AND non polar
  • induced dipole-induced dipole
  • results from momentary uneven e- dist.
  • temp. polarity –> chain reaction of pol. to surrounding molecules
45
Q

what kind of atoms have stronger london forces

A

LARGER

e- farther from nucleus

chem 101 (12 decks)

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