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chemistry > unit 4 - matter & energy > Flashcards

unit 4 - matter & energy Flashcards

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1
Q

matter

A
  • anything that takes up space (volume) and has mass
  • matter can exist in 3 phases
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2
Q

at certain temp or pressure, the matter can be…

A

a solid, liquid, or a gas

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3
Q

solid phase

A
  • orderly arrangement
  • particles are in fixed positions / tightly packed
  • crystalline
  • particles vibrate/slight movement
  • definite volume
  • definite shape
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4
Q

all molecular movement is said to stop at

A

0 degrees Kelvin

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5
Q

properties of gas phase

A
  • total disorder
  • much Empty Space
  • particles have complete freedom of motion/move fastest
  • particles are far apart
  • no definite volume & no definite shape
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6
Q

properties of liquid phase

A
  • some disorder
  • particles are free to move relative to eachother
  • move faster and more than a liquid/less than gas
  • definite volume
  • no definite shape (indefinite, negligible = synonymous)
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7
Q

changes in what result in changes of phases

A

temperature and/or pressure

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8
Q

temperature affects what

A

how fast particles move

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9
Q

pressure affects what

A

how packed the particles are

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10
Q

phase changes are…

A

physical changes which can be endothermic or exothermic

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11
Q

endothermic

A

process that requires absorption of heat (heating process)

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12
Q

exothermic

A

process that involves the release of heat (cooling process)

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13
Q

melting

A
  • Endothermic Change
    (Heat is Absorbed)

● Solid (s) → Liquid (l)
Phase Change

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14
Q

evaporation/vaporization

A
  • Endothermic
    (Heat is Absorbed)

● Liquid (l) → Gas (g)
Phase Change

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15
Q

sublimation

A
  • Endothermic
    (Heat is Absorbed)

● Solid (s) → Gas (g)
● Skips the Liquid Phase
● Ex. Dry Ice & Iodine
CO2 (s) → CO2 (g)
I2 (s) → I2 (g)

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16
Q

condensation

A
  • Exothermic
    (Release of Heat)

● Gas (g) → Liquid (l)
Phase Change

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17
Q

freezing

A
  • Exothermic
    (Release of Heat)

● Liquid (l) → Solid (s)

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18
Q

deposition

A
  • Exothermic
    (Release of Heat)

● Gas (g) → Solid (s)
Phase Change

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19
Q

in chemical reactions, what is conserved

A

mass, charge, and energy of matter

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20
Q

pure substance

A
  • a type of matter.
  • has definite composition and the properties are the same throughout

Ex. Elements & Compounds (No Mixtures)

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21
Q

elements

A
  • made of one kind of atom.
  • all atoms that make up an element have the same atomic number.
  • CAN NOT be broken down by ordinary means.
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22
Q

compound

A
  • a substance made of two or more
    elements that are chemically combined.
  • It has a definite Composition
    -mass ratio (formula) never changes
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23
Q

binary compound

A
  • simplest compouds
  • made up of only 2 kinds of elements
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24
Q

properties of a compound

A

Properties of the compound are drastically
different from the original elements.

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25
Q

can a compound be broken down by ordinary chemical means

A

YES (decomposition)

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26
Q

mixture

A

– a combination of two or more pure substances that can be separated by physical means
- combination of two or more distinct substances
- composition ALWAYS VARIES!
- parts are only Physically combined

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27
Q

(aq)

A
  • aqueous
  • dissolved in water = solution
  • mixture
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28
Q

properties of a mixture

A

1) Formed by a physical combination
2) Parts of a mixture retain their original properties.
3) Parts are separated by physical properties.
Ex. Magnetism, density, size, boiling point
4) Parts of a mixture are in any proportion- VARY!
- No Definite Formula; composition varies
Ex. NaCl (aq)- can be made with various amounts of water and salt.

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29
Q

two types of mixtures

A

homogeneous and heterogeneous

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30
Q

homogeneuos

A
  • all parts look the same
    -particles evenly distributed
    Ex. Air, Milk, NaCl (aq)
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31
Q

heterogeneous

A
  • you can see the parts
  • particles unevenly distrib.
    Ex. Rocks, Soil, & Sand
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32
Q

physical properties

A

characteristic which can be
observed without producing a new substance.

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33
Q

malleabilitiy

A

ability to be hammered into a sheet and not fall a part

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34
Q

ductility

A

ability to be drawn into a wire

35
Q

conductivity

A

ability to carry a current or heat

36
Q

tenacity

A

ability to resist being pulled apart

37
Q

sublimation

A

can change from a solid to a gas without melting at certain temperature

38
Q

boiling point

A

temperature at which liquid turns to gas

39
Q

solubility

A

ability to dissolve

40
Q

brittleness

A

ability to shatter when struck

41
Q

magnetism

A

ability to be attracted to a magnet

42
Q

melting point

A

temperature at which solid turns to a liquid

43
Q

chemical properties

A

characteristics which describe how a substance reacts or fails to react with other substances

44
Q

physical change

A

a change in the appearance but NOT in major properties or composition

45
Q

chemical change

A

a change in which one or more substances form with totally new properties and compounds
ex: burning, digestion, rusting/corrosion, souring of milk, decaying

46
Q

parts of a mixture can be separated based on their…

A

density, charge, boiling point, size, magnatism

47
Q

filtration

A
  • Is used to separate mixture components based on SIZE.
    (Heterogeneous Mixture).

*Small particles (filtrate)
pass through the filter paper.

*Large particles (residue)
remains on the filter paper.

48
Q

density

A

A separatory funnel is used
to separate parts of a mixture
based on differences in DENSITY

49
Q

paper chromatography (charge/polarity)

A

● Separates a mixture based on
different attractions to the
paper.
- Molecules have a difference
in CHARGE/POLARITY
● Components of the mixture
move up the paper, BUT at
different rates separate from each other.

50
Q

distillation (boiling point)

A
  • Used to seprate Homogenous Mixtures based on Boiling Point
  • Separation between liquids
    ex: alcohol and H2O
  • solid dissolved in liquid
    ex: NaCl dissolved in H2O
51
Q

temperature

A

The measure of the average kinetic
energy (energy of motion) of a substance’s particles.
- measured in Fahrenheit, Celsius, and Kelvins

52
Q

Heat

A

The amount of energy transferred from one substance to another.
- measured in units of Joules or calories

53
Q

heat moves from…

A

a higher temp to a lower temp

54
Q

boiling point of H2O

A

100°C & 373 K

55
Q

freezing point of H2O

A

0°C & 273 K

56
Q

body temp

A

37°C & 310 K

57
Q

room temp

A

20-25°C & 293-298 K

58
Q

absolute zero

A

temperature at which all molecular motion stops
- 0K or -273°C

59
Q

to find kelvin from celcius…

A

°C + 273

60
Q

to find celcius from kelvin

A

K - 273

61
Q

a 1° change on the Celcius scale equals a 1° change on the Kelvin scale

A
62
Q

heating and cooling curves

A

are diagrams that represent a substance being heated or cooled at a constant rate
- they illustrate melting point and boiling point

63
Q

melting point

A

temp. at which solid and liquid phases exist in equilibrium (same as the freezing point)

64
Q

boiling point

A

temp. at which liquid and gas phases exist in equilibrium (same as the condensation point)

65
Q

kinetic energy

A

energy of motion; increases as temp increases

66
Q

potential energy

A

stored energy in bonds; increases as the distance between the molecules increases

67
Q

heat of fusion

A

amount of heat required to melt 1 gram of a substance; S -> L

68
Q

heat of vaporization

A

amount of heat to vaporize a substance; L -> G

69
Q

table s: solid

A

phase below its freezing or melting point

70
Q

table s: liquid

A

phase between its freezing point and boiling point

71
Q

gas

A

phase above its boiling point/condensation point

72
Q

calorimetry

A
  • study of heat and its measurement
  • measurement of heat absorbed or released by a substance
  • unit for heat (Q) is Joules
73
Q

specific heat

A

amount of heat energy in joules required to change the temperature of 1 gram of a particular substance by 1 degree (J/g * °C)

74
Q

specific heat of water

A

4.18 J/g * °C

75
Q

1 kJ = 1000 J

A
76
Q

equation to calculate the amount of heat in joules

A

Q = mc (ΔT)

77
Q

Q

A

Heat gained or lost (Joules or J)

78
Q

m

A

Mass in grams of the substance

79
Q

c

A

Specific Heat of a Substance

80
Q

ΔT

A

Change in Temp. (Final - Initial)

81
Q

heat of fusion is equal to

A

amount of heat released when freezing

82
Q

heat of vaporization is equal to

A

amount of heat released to condense

83
Q

heat of fusion formula

A

Q = m x Hf

84
Q

heat of vaporization formula

A

Q = m x Hv

chemistry (11 decks)

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