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Gen Chem I > Ch 1: Particles of Matter > Flashcards

Ch 1: Particles of Matter Flashcards

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1
Q

Macroscopic phenomena

A

large-scale phenomena

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2
Q

particulate representations

A

show the structure of matter on the scale of atomic and subatomic particles//explain macroscopic phenomena

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3
Q

Mass

A

quantity of matter in any object

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4
Q

Matter

A

everything in the universe (or body) that has mass and occupies space

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5
Q

Chemistry

A

study of the composition, structure, and properties of matter

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6
Q

Pure substances

A
  • have a constant composition does Not vary from one sample to another [eg: water]
  • cannot be separated/broken down into simpler substances
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7
Q

Physical process

A

transformation of a sample of matter that does not alter the chemical identities of any of the substances in the sample EG; change in physical state S > L

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8
Q

Two groups of pure substances

A

Elements & compounds

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9
Q

Elements

A

pure substance cant be broken down

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10
Q

Compounds

A
  • substances whose elements can be separated from one another
  • this is accomplished through a chemical reaction
  • typically have different properties from those of the elements of which they are composed
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11
Q

Chemical reaction

A

transformation of one of more substances into one or more different substances

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12
Q

Mixture

A

Any matter that is not a pure substance composed of 2 or more that retain their own chemical identities

  • substances in mixtures CAN be separated by physical processes
  • substances not present in definite proportion
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13
Q

Homogeneous mixture (aka solutions)

A

the substance that makes up the mixture is uniformly distributed

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14
Q

Heterogeneous mixture

A

Not distributed uniformly

(can tell by boundaries), also opaqueness

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15
Q

Atom

A
  • only particle that makes up elements

- cannot be chemically or mechanically divided into smaller parts

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16
Q

Some elements exist as………

A

Molecules!!

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17
Q

Molecules

A

assembly of 2 or > atoms held together in a characteristic pattern by forces called chemical bonds

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18
Q

Energy

A

the capacity to do work

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19
Q

Diatomic molecules

A

2 atoms EG: H2, F2, CL2, Br2, I2

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20
Q

Law of constant composition

A

all samples of a particular compound contain the same elements combined in the same proportions

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21
Q

Ion

A
  • particle consisting of one or more atoms
  • positively or negatively charged
  • Electrostatically attracted to one another
  • can be single atoms or may have 2 or > atoms bonded together
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22
Q

Cations

A

Positive ions

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23
Q

Anions

A

Negative ions

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24
Q

ball and stick model

A

use spheres to represent atoms and sticks to represent chemical bonds
Adv: show correct angles between bonds
Did:size of spheres are not proportional to atoms they represent

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25
Q

Molecular models

A

3D perspective

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26
Q

Structural formula

A

uses straight lines

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27
Q

Space filling molecular models

A

spheres drawn to scale and touch one another as real molecules do.
DIS: not colored, bond space between atoms difficult to discern

28
Q

Not all compounds are ____________

A

Molecular.

some compounds are ions

29
Q

Plasma includes

A

red blood cells, white blood cells, and platelets

30
Q

Protein isolation techniques

A
  • 2D Electrophoresis
  • Filtration
  • Distillation
31
Q

2D Electrophoresis

A

proteins separated in two steps:

1) based on the fact that molecules of these proteins have different charges depending on their enviro.
2) fractions from the first step are separated by the molecules size

32
Q

Filtration

A

-Separates particles suspended in liquid

important for water

33
Q

Volatilities

A

how easily liquids are converted to gas

34
Q

Distillation

A
  • most widely used
  • desalinates water
  • converts fresh water into distilled water
35
Q

Ion exchange

A

remove all dissolved ions from water

36
Q

Intensive properties

A

Characterize matter independent of the quantity of the material present

37
Q

Extensive properties

A

varies with the quantity of the substance present

38
Q

2 categories of properties

A

Physical & chemical

39
Q

Physical properties

A

properties of a pure substance can be observed or measured w.o changing the substance into another substance

40
Q

Density

A

ratio of the mass of an object to its volume

d=m/v

41
Q

chemical reactivity includes

A

rates of reaction, identity of other substances with which it reacts, identity of the products formed
^^^ define the chemical properties of a substance

42
Q

chemical property

A

property of a substance that can be observed only by reacting it to form another substance

43
Q

3 states of matter

A

solid
liquid
gas

44
Q

solid

A

has a definite volume and shape

45
Q

liquid

A

definite volume, no shape

46
Q

gas

A

neither shape nor volume, expands to occupy entire shape and volume of its container
-compressible

47
Q

Sublimation

A

Transformation of a solid directly into a gas

48
Q

Deposition

A

Transforms gas directly into a solid

49
Q

scientific theory (model)

A

a general explanation of a widely observed phenomenon that has been extensively tested and validated

50
Q

scientific method

A

approach to acquire knowledge based on observation of phenomena, development of testable hypothesis, and additional experiment that test the validity of the hypothesis

51
Q

E=mc^2

A

E=energy
M=mass of matter
C= speed of light

52
Q

SI unit

A

volume

53
Q

density of gas expressed in

A

grams/liter (g/l)

54
Q

liquids expressed as

A

g/cm^3 = g/ml

55
Q

solids expressed as

A

g/cm^3

56
Q

Unit factor method (aka dimensional analysis)

A

used to convert a value from one unit system to another

-uses conversion factors

57
Q

Conversion factors

A

fractions in which the numerators and denominators have different units but represent equivalent quantities

58
Q

Significant figures

A
  • all the certain digits measured in a measured value plus one estimated digit
  • the greater the # of significant figures the greater the certainty about its value
59
Q

Rules about zeros and decimals

A

1) 0’s at the beginning of a value are not significant
2) 0s at the end are
3) 0s at the end w.o a decimal may or may not be
4) 0s between non 0 digits always are

60
Q

Precision

A

indicates how well results of repeated measures or analyses agree w. each other

61
Q

Accuracy

A

how close results are to the true value of a quantity

62
Q

Standard deviation

A

measure of amt of variance or dispersion in a set of values

63
Q

Confidence interval

A

range of values has a specified probability of containing the true value of measurement
[-range of values around a calculated mean]

64
Q

F & C scales differ how

A

1) diff zero points

2) size of temp change corresponding to 1 degree

65
Q

to convert f to c

A

C=5/9 (F-32)

66
Q

Kelvin

A

SI unit of temp.

0 point is the coldest temp [absolute zero approx.: -273.15C]

67
Q

Conversion from C to K

A

just 273.15 to the C value

Gen Chem I (2 decks)

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