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Chemistry 11 > CH.1 > Flashcards

CH.1 Flashcards

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1
Q

What are we studying?

A

Matter and the changes it undergoes

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2
Q

What are the fundamental concepts of chemistry?

A
  1. Matter is composed of various types of atoms
  2. One substance changes to another by reorganizing the way atoms are attached to each other
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3
Q

Who created the scientific method?

A

Louis Pasteur, who developed germ theory, pasteurization, rabies vaccination

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4
Q

What are the steps in the scientific method?

A
  1. Making observations.
    -Observations may be qualitative or quantitative.
  2. Formulating hypotheses.
    - A possible explanation for an observation
  3. Performing experiments.
    - An experiment is carried out to test a hypothesis. Involves gathering new information that enables a scientist to decide whether the hypothesis is valid. Experiments always produce new observations, and brings the process back to the beginning again.
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5
Q

What are the limitations of the Scientific Method?

A
  • By what can be observed with the five senses
  • To the present
  • How, not why a process works
  • In that it cannot make moral judgments
  • Cannot deal with the unique
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6
Q

What are the scientific models?

A

Law
- Summarizes what happens

Hypothesis
- A possible explanation for an observation

Theory
- an attempt to explain why it happens
- set of tested hypotheses that gives an overall explanation of some phenomenon

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7
Q

What are the classifications of matter?

A

Solid, liquid, gas

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8
Q

Solids are…

A
  • The particles in a solid are packed close together and are fixed in a position
    -Though they may vibrate
  • The close packing of the particles results in solids being incompressible
  • The inability of the particles to move around results in solids retaining their shape and volume when placed in a new container, and prevents the particles from flowing
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9
Q

Crystalline Solids…

A
  • Some solids have their particles arranged in an orderly geometric pattern - we call these crystalline solids
    - Salt and diamonds
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10
Q

Amorphous Solids…

A
  • Some solids have their particles randomly distributed without any long-range pattern - we call these amorphous solids
    -Plastic
    -Glass
    - Charcoal
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11
Q

Liquids…

A
  • The particles in a liquid are closely packed,
  • Have some ability to move around
  • Incompressible
  • Take the shape of their container and to flow
  • Don’t have enough freedom to escape or expand to fill the container
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12
Q

Gases…

A
  • Particles do not interact with each other
  • The particles are constantly moving, bumping into each other and the container
  • There is a lot of empty space between the particles
  • Compressible
  • Expand to fill and take the shape of their container
  • Will flow
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13
Q

Pure Substances

A

1) made of one type of particle
2) all samples shows the same intensive (independent of amount) properties

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14
Q

Mixtures

A

1) made of multiple types of particles
2) samples may show different intensive properties

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15
Q

Element (pure substances)

A

1) made of one type of atom (some elements found as multi-atom molecules in nature)
2) combine together to make compounds

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16
Q

Compounds (pure substances)

A

1) made of one type of molecule, or array of ions
2) molecules contain 2 or more different kinds of atoms

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17
Q

Heterogenous

A

1) made of multiple substances, whose presence can be seen
2) portions of a sample have different composition and properties

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18
Q

Homogenous

A

1) made of multiple substances, but appears to be one substance
2) all portions of a sample have the same composition and properties

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19
Q

Physical Properties

A
  • the characteristics of matter that can be changed without changing its composition
  • Characteristics that are directly observable
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20
Q

Chemical Properties

A
  • the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy
  • Characteristics that describe the behavior of matter
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21
Q

Common Physical Changes

A
  • Processes that cause changes in the matter that do not change its composition
  • State changes
    Boiling / condensing
    Melting / freezing
    Subliming /deposition
    Dissolving
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22
Q

Common Chemical Changes

A
  • Processes that cause changes in the matter that change its composition
        Rusting
  • The rusting of iron is a chemical change. The iron atoms in the nail combine with oxygen atoms from O2 in the air to make a new substance, rust, with a different composition
  • Processes that releases lots of energy
    Burning
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23
Q

Separation of Mixtures

A

Different Physical Property/ Technique

Boiling Point = distillation

state of matter (solid/liquid/gas) = filtration / decanting

Adherence to a Surface = chromatography

Volatility = evaporation

density = centrifugation & decanting

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24
Q

Chromatography

A
  • Separation based upon adherence to a surface
    -Stationary phase
    -Moving phase
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25
Q

Evaporation

A

Liquid vaporizes leaving less volatile liquid or solid

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26
Q

Centrifugation

A
  • Separation based density
  • Centrifugal motions causes more dense materials to go to the bottom of the tube
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27
Q

Decanting

A
  • Separation based state
    -carefully pour liquid leaving precipitation
  • Separation based density
    -carefully pour less dense liquid
28
Q

Fundamental SI Units

A

length = meter^2 = m

mass = kilogram = kg

time = second = s

temperature = kelvin = K

amount of substance = mole = mol

electric current = ampere = A

luminous intensity = candela = cd

29
Q

exa / E

A

10^18

30
Q

peta / P

A

10^15

31
Q

tera / T

A

10^12

32
Q

giga / G

A

10^9

33
Q

mega / M

A

10^6

34
Q

kilo / k

A

10^3

35
Q

hecto / h

A

10^2

36
Q

deka / da

A

10^2

37
Q

deci / d

A

10^1

38
Q

centi / c

A

10^2

39
Q

milli / m

A

10^3

40
Q

micro /

A

10^6

41
Q

nano / n

A

10^9

42
Q

pico / p

A

10^12

43
Q

femto / f

A

10^15

44
Q

atto / a

A

10^18

45
Q

zepto / z

A

10^21

46
Q

yocto / y

A

10^24

47
Q

Length

A

Commonly use centimeters
- 1 m = 100 cm
- 1 cm = 0.01 m = 10 mm
- 1 inch = 2.54 cm

48
Q

Mass

A

Measure of the resistance of an object to a change in its state of motion

  • Measured by the force necessary to give an object a certain acceleration
49
Q

Weight

A

Force exerted by gravity on an object

50
Q

Time

A

Measure of the duration of an event

51
Q

Temperature Scales

A
  • Fahrenheit Scale
  • Celsius Scale
  • Kelvin scale
    - absolutely scale
    - No negative numbers
    - directly proportional to average amount of kinetic energy
    • 0 K = absolute zero
52
Q

Fahrenheit vs. Celsius

A

C = (F -32) / 1.8

53
Q

Kelvin vs. Celsius

A

K = C + 273.15

54
Q

Volume

A

Commonly measured solid volume in cubic centimeters (cm^3)
- 1 m^3 = 10^6 cm^3
- 1 cm^3 = 10^-6 cm^3

Commonly measure liquid or gas volume in millimeters (mL)
- 1 L is slightly larger than 1 quart
- 1 L = 1 dm^3 = 1000 mL = 10^3 mL
- 1 mL = 0.001 L = 10^-3 mL
- 1 mL = cm^3

55
Q

Non-SI Units

A

Length = Angstrom, 10^-8 cm

Volume = Liter, L, 10^-3 m^3

Energy = Calorie, cal, 4.184 J

Pressure
- 1 atm = 1.064 x 10^2 kPa
- 1 atm = 760 mmHg

56
Q

Mass & Volume

A
  • are extensive properties
  • the value depends on the quantity of matter
  • extensive properties cannot be used to identify what type of matter something is
57
Q

Density

A

Solids = g/cm^3

Liquids = g/mL

Gases = g/L

p = m /v v = m/p m = p x v

58
Q

Uncertainties in Scientific Measurements

A

Systematic Errors
- thermometer constantly 2 C too low

Random errors
- limitation in reading a scale

Precision
- reproducibility of a measurement

Accuracy
- How close to the real value

59
Q

Precision

A
  • caused by random errors
  • determine the precision of a set of measurement by evaluating how far they are from the actual value and each other
  • should average out
60
Q

Accuracy

A
  • caused by systematic errors
    • caused by limitations in the instruments, better technique, or experimental design
    • can be reduced by using more accurate inst…
  • Determine the accuracy by evaluating how far it is from the actual value
  • Do not average out b/c the measurements can be either too high or too low
61
Q

Significant Figures

A

The non-place-holding digits in a reported measurement

The range of values to expect for repeated measurements

62
Q

Counting Significant Figure

A

1) All non-zero digits are significant
a) 1.5 has 2 sig figs

2) Interior zero are significant
3) Leading zeros are NOT significant
4) Trailing zeros may or may not be significant
a) trailing zeros after a decimal point are significant
b) zeros at the end of a number without a written decimal point and ambiguous and should be avoided by using scientific notation

63
Q

Multiplication and Division with Sig Figs

A

When multiplying or dividing, the results has the same sig figs as the measurements with the fewest number of sig figs

64
Q

Additions and subtraction with Sig Figs

A

When adding or subtracting, the result has the same number of decimal places

65
Q

Problem Solving and Dimensional Analysis

A

Arrange conversion factors so give unit cancels

given unit x (desired unit / given uni) = desired unit

66
Q

Percent as a Conversion Factor

A
  • Gives the ratio of the parts to the hole
    - % = parts/ whole x 100
  • Uses the same unit in the numerator and denominator
    -Uses the value of 100
  • Can be written as two factors

Chemistry 11 (3 decks)

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