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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
Molecular models
3D perspective
26
Structural formula
uses straight lines
27
Space filling molecular models
spheres drawn to scale and touch one another as real molecules do. DIS: not colored, bond space between atoms difficult to discern
28
Not all compounds are ____________
Molecular. | some compounds are ions
29
Plasma includes
red blood cells, white blood cells, and platelets
30
Protein isolation techniques
- 2D Electrophoresis - Filtration - Distillation
31
2D Electrophoresis
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
Filtration
-Separates particles suspended in liquid | important for water
33
Volatilities
how easily liquids are converted to gas
34
Distillation
- most widely used - desalinates water - converts fresh water into distilled water
35
Ion exchange
remove all dissolved ions from water
36
Intensive properties
Characterize matter independent of the quantity of the material present
37
Extensive properties
varies with the quantity of the substance present
38
2 categories of properties
Physical & chemical
39
Physical properties
properties of a pure substance can be observed or measured w.o changing the substance into another substance
40
Density
ratio of the mass of an object to its volume | d=m/v
41
chemical reactivity includes
rates of reaction, identity of other substances with which it reacts, identity of the products formed ^^^ define the chemical properties of a substance
42
chemical property
property of a substance that can be observed only by reacting it to form another substance
43
3 states of matter
solid liquid gas
44
solid
has a definite volume and shape
45
liquid
definite volume, no shape
46
gas
neither shape nor volume, expands to occupy entire shape and volume of its container -compressible
47
Sublimation
Transformation of a solid directly into a gas
48
Deposition
Transforms gas directly into a solid
49
scientific theory (model)
a general explanation of a widely observed phenomenon that has been extensively tested and validated
50
scientific method
approach to acquire knowledge based on observation of phenomena, development of testable hypothesis, and additional experiment that test the validity of the hypothesis
51
E=mc^2
E=energy M=mass of matter C= speed of light
52
SI unit
volume
53
density of gas expressed in
grams/liter (g/l)
54
liquids expressed as
g/cm^3 = g/ml
55
solids expressed as
g/cm^3
56
Unit factor method (aka dimensional analysis)
used to convert a value from one unit system to another | -uses conversion factors
57
Conversion factors
fractions in which the numerators and denominators have different units but represent equivalent quantities
58
Significant figures
- 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
Rules about zeros and decimals
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
Precision
indicates how well results of repeated measures or analyses agree w. each other
61
Accuracy
how close results are to the true value of a quantity
62
Standard deviation
measure of amt of variance or dispersion in a set of values
63
Confidence interval
range of values has a specified probability of containing the true value of measurement [-range of values around a calculated mean]
64
F & C scales differ how
1) diff zero points | 2) size of temp change corresponding to 1 degree
65
to convert f to c
C=5/9 (F-32)
66
Kelvin
SI unit of temp. | 0 point is the coldest temp [absolute zero approx.: -273.15C]
67
Conversion from C to K
just 273.15 to the C value

Gen Chem I (2 decks)

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