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10th grade > Chem printed notes unit > Flashcards

Chem printed notes unit Flashcards

1
Q

The Kinetic Theory of Matter

A

all particles of matter are in motion

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2
Q

Kinetic theory of gases

A
  1. gases are tiny
  2. no definite volume and are independent
  3. move fast in a straight line and change direction in collision
  4. are elastic and don’t stick together
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3
Q

Kinetic energy are…

A

transferred but not lost

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4
Q

Gas pressure

A

collision of gas particles with each other and their container.

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5
Q

as collision increases

A

pressure increases

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6
Q

as temperature increases

A

pressure increases

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7
Q

altitude increases

A

atmospheric pressure decreases

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8
Q

As volume increases,

A

pressure decreases.

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9
Q

standard pressure

A

average pressure at sea level.

  • 1 atm
  • 760 mmHg
  • 101.3 kPa
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10
Q

Kelvin
(temperatureis the amt of kenetic energy)
KE is proportional to Kelvin

A

Celsius + 273

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11
Q

Kinetic Molecular theory about gases

A
  1. movement is straight
  2. motion is constant and random
  3. no attractive/repulsive forces among particles
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12
Q

Factors Affecting Gas Pressure

A
  1. as the amt of gas increases, pressure increases
  2. as volume decreases, pressure increases
  3. as temp increases, pressure increases
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13
Q

Boyle’s law

A

PV=PV

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14
Q

Charles’ law

A

v/t=v/t

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15
Q

Gay-Lussac’s Law

A

p/t=p/t

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16
Q

the combined gas law

A

pv/t=pv/t

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17
Q

Ideal gases

A

gases that follow the kinetic molecular theory/gas laws (ATM IS AT A CONSTANT)

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18
Q

Ideal Gas Law

A

PV=nRT

R= .0821, pressure is in atm

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19
Q

Dalton

A

Ptotal=P1+P2+P3

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20
Q

Diffusion

A

gas particles spread

21
Q

Effusion

Graham

A

gas escape through a small hole

22
Q

When will real gas deviate from ideal gas behavior

A
  • high pressure
  • low temp
  • high molar mass
  • polar molecules
23
Q

Intermolecular Forces (IM)

A

forces of attraction btw particles (more in solids)

24
Q

Flow

A

particles can slide past eachother (only gas and liquids)

25
Compressible
liquid and gas but gas is more
26
KE
gas has more and solid has least
27
Viscosity:
inability to flow
28
Evaporation
liquid to gas below boiling point. Particles must have enough KE to beat IM. Highest KE at surface. cools overall
29
Evaporation in a closed container
after evaporation, particles will lose energy and become a liquid.
30
Equilibrium
reaction ocuring at the same rate, dynamic process bc looks likes nothing is happening
31
Vapor Pressure
pressure caused by evaporated particles in closed container. vapor can b measure in container
32
As temp increases
pressure increases
33
as im forces increases
vp decreases
34
boiling
conversion throughout substance. In order to boil, vapor pressure=atm pressure. Temp remains constant. also occurs by lowering atm pressure
35
normal boiling point
boiling at standard pressure (sea level)
36
high atm
bp increases
37
low atm
bp decreases
38
Crystaline
solid particles arranged in a pattern
39
Amorphous
no order in particle
40
Ionic (metal and nonmetal)
positive and negative, stronger higher normal boiling point
41
Molescular (nonmetal)
covalent bond, weaker IM
42
Sublimation
solid to gas without liquid. occurs when vapor pressure is greater/equal to atm
43
deposition
gas to solid without liquid
44
VP of soild
is lower than vp of a liquid
45
phase diagram
shows temp and pressurre
46
liquid state more dense than solid
slant left
47
Molarity (M)
Liters of solution on bottom
47
Molarity
Liters of solution on bottom
48
Molality (m)
Kg

10th grade (45 decks)

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