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Chemistry 11 > CH.1 > Flashcards

CH.1 Flashcards

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
Evaporation
Liquid vaporizes leaving less volatile liquid or solid
26
Centrifugation
- Separation based density - Centrifugal motions causes more dense materials to go to the bottom of the tube
27
Decanting
- Separation based state -carefully pour liquid leaving precipitation - Separation based density -carefully pour less dense liquid
28
Fundamental SI Units
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
exa / E
10^18
30
peta / P
10^15
31
tera / T
10^12
32
giga / G
10^9
33
mega / M
10^6
34
kilo / k
10^3
35
hecto / h
10^2
36
deka / da
10^2
37
deci / d
10^1
38
centi / c
10^2
39
milli / m
10^3
40
micro /
10^6
41
nano / n
10^9
42
pico / p
10^12
43
femto / f
10^15
44
atto / a
10^18
45
zepto / z
10^21
46
yocto / y
10^24
47
Length
Commonly use centimeters - 1 m = 100 cm - 1 cm = 0.01 m = 10 mm - 1 inch = 2.54 cm
48
Mass
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
Weight
Force exerted by gravity on an object
50
Time
Measure of the duration of an event
51
Temperature Scales
- Fahrenheit Scale - Celsius Scale - Kelvin scale - absolutely scale - No negative numbers - directly proportional to average amount of kinetic energy - 0 K = absolute zero
52
Fahrenheit vs. Celsius
C = (F -32) / 1.8
53
Kelvin vs. Celsius
K = C + 273.15
54
Volume
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
Non-SI Units
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
Mass & Volume
- 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
Density
Solids = g/cm^3 Liquids = g/mL Gases = g/L p = m /v v = m/p m = p x v
58
Uncertainties in Scientific Measurements
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
Precision
- 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
Accuracy
- 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
Significant Figures
The non-place-holding digits in a reported measurement The range of values to expect for repeated measurements
62
Counting Significant Figure
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
Multiplication and Division with Sig Figs
When multiplying or dividing, the results has the same sig figs as the measurements with the fewest number of sig figs
64
Additions and subtraction with Sig Figs
When adding or subtracting, the result has the same number of decimal places
65
Problem Solving and Dimensional Analysis
Arrange conversion factors so give unit cancels given unit x (desired unit / given uni) = desired unit
66
Percent as a Conversion Factor
- 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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