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Chemistry > Chapter 1 and 2 > Flashcards

Chapter 1 and 2 Flashcards

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1
Q

Definition of Chemistry

A

the science that deals with the materials of the universe and the changes these materials undergo

  • seeks to understand what matter does by studying what atoms and molecules do
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2
Q

The world is made up of________ and _________.

A

matter and energy

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3
Q

Matter

A

anything that occupies space and has mass

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4
Q

Mass

A

the number of atoms in an object

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5
Q

Matter is composed of a lot of tiny little pieces we call _________ and _________.

A

atoms

molecules

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6
Q

Atoms

A

the tiny particles that make up all matter

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7
Q

In most substances, the atoms are ________ together in units called_________.

A

bonded

molecules

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8
Q

Molecules

A

2 or more atoms that are chemically joined

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9
Q

_______ is used to understand mass

A

weight

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10
Q

Compound

A

a molecule that is made up of 2 or more different types of elements chemically joined.

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11
Q

Element

A

matter composed of only one type of atom.

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12
Q

States of matter differ by how much ______ they carry.

A

energy

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13
Q

Why do the properties of liquids, gases, and solids differ?

A

because the atoms or molecules have different structures in each state.

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14
Q

All chemicals have some form of _______.

A

motion

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15
Q

State changes are called ___________.

A

physical changes; chemical formula stays the same

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16
Q

Chemical change

A

aka. chemical rxn, physical appearance may change but most importantly chemical formula changes.

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17
Q

The particles of a solid are _________ and are in a ______ position.

A

packed close together
fixed

-although they may vibrate

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18
Q

The close packing of the particles results in solids being _________.

A

incompressible

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19
Q

the inability of the particles to move around results in solids retaining their _______ and ________ when placed in a new container; prevents the particles from _________.

A

shape
volume
flowing

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20
Q

Au is an ___________

A

atomic element because it is made up of one type of atom

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21
Q

O2 is a___________.

A

molecular element because it is often found in O2 form

and is made up of 2 atoms (same) in one molecule

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22
Q

H2O is a ___________

A

molecular compound because water molecules are made up of 2 different types of atoms

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23
Q

The particles in a liquid are closely _______ but they have some ability to move around.

A

packed

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24
Q

Why are liquids incompressible?

A

because molecules in a liquid are closely packed

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25
Q

Why are liquids able to take the shape of a container?

A

the ability of particles to move in a liquid allows liquids to take the shape of the container in which they are placed and to flow. However, they don’t have enough freedom to escape and expand to fill the container.

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26
Q

In which state do particles have complete freedom from each other?

A

the gas state; the particles are constantly flying around, bumping into each other and the container.

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27
Q

In the gas state, there is a lot of ________ between particles.

A

empty space

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28
Q

are gases compressible?

A

yes; because there is a lot of empty space, the particles can be squeezed closer together.

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29
Q

Why do gases flow and expand to take the shape of their container?

A

because the particles are not held in close contact and are moving freely.

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30
Q

Volume

A

the amount of space something occupies

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31
Q

Solid

A

Shape: fixed
Volume: fixed
Compress: no
Flow: no

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32
Q

Liquid

A

Shape: Indefinite
Volume: fixed
Compress: no
Flow: yes

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33
Q

Gas

A

Shape: Indefinite
Volume: Indefinite
Compress: yes
Flow: yes

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34
Q

fixed

A

keeps shape when placed in a container

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35
Q

indefinite

A

takes shape of the container

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36
Q

How are pure substances classified

A

Element

Compound; 2 or more chemical elements joined

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37
Q

How are mixtures classified?

A

Homogenous

Heterogeneous

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38
Q

Matter can be divided into ______ and _______.

A

Pure substances

Mixtures

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39
Q

Pure substance

A

composed of only one type of atom or molecule

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40
Q

Mixture

A

composed of 2 or more different pure substances that are not chemically united, but simply mixed together.

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41
Q

The smallest piece of an element is called a(n) _______.

A

atom

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42
Q

The smallest piece of a compound is called a _________.

A

molecule

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43
Q

all molecules of a compound are __________.

A

identical

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44
Q

each molecule has the same ______ and _______ of atoms.

A

number

type

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45
Q

Homogeneous

A

matter that is uniform throughout

  • appears to be one thing
  • solutions (homogeneous mixtures)
  • i.e. salt water
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46
Q

Heterogeneous

A

matter that is non-uniform throughout

-i.e. oil and water

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47
Q

Physical properties

A

the characteristics of matter that can be changed without changing its composition

  • characteristics that are directly observable.
  • i.e. characteristic odor of gasoline
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48
Q

Name the 17 physical properties.

A
  1. mass
  2. solid
  3. melting point
  4. taste
  5. texture
  6. malleability
  7. volume
  8. liquid
  9. boiling point
  10. odor
  11. shape
  12. ductility
  13. density
  14. gas
  15. volatility
  16. color
  17. solubility
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49
Q

Ductility

A

can be drawn into a wire

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50
Q

Volatility

A

tendency to convert from liquid to gas readily compared to water

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51
Q

Name the 6 chemical properties

A
  1. acidity
  2. flammability
  3. oxidizing ability
  4. basicity (aka alkalinity)
  5. corrosiveness
  6. Reducing ability
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52
Q

How do you perform a calculation involving both multiplication/division and addition/subtraction with sig figs?

A
  1. follow order of operations
  2. keep track of sig figs through each step and only round at the end

6.78 x 5.903 x (5.489 -5.01)
6.78 x 5.903 x 0.4790 (only 2 sig figs)
19.1707
~19

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53
Q

G

A

giga

Basex10^9

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54
Q

M

A

mega

Basex10^6

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55
Q

k

A

kilo

Basex10^3

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56
Q

d

A

deci

Basex10^-1

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57
Q

c

A

centi

Basex10^-2

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58
Q

m

A

milli

Basex10^-3

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59
Q

u

A

micro

Basex10^-6

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60
Q

n

A

nano

Basex10^-9

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61
Q

p

A

pico

Basex10^-12

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62
Q

1 inch = _______cm

A

2.54 cm exactly

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63
Q

1 liter = ______mL

A

1000mL

64
Q

1 liter = _________cc

A

1000 cc

65
Q

Formula for the volume of a rectangular block

A

V = l x w x h

66
Q

Formula for Density

A

D = m/v

67
Q

Formula to convert Celsius to Kelvins

A

K = C +273

68
Q

Formula to convert Fahrenheit to Celsius

A

C = (F-32)/1.8

69
Q

1 calorie (cal) = _________joules (J)

A

4.184 J

70
Q

1 Calorie (Cal) = _________calories (cal)

A

1000 cal

71
Q

What is the heat capacity of liquid water?

A

4.184 J/g degrees celsius

72
Q

Formula for heat capacity

A

Q = m x Cs x Change in T in Celsius

Q = energy required
m = mass in grams of sample
Cs = specific heat capacity
73
Q

What is the formula for change in temperature?

A

Change in temp =Tf - Ti

74
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 the matter
  • i.e. the susceptibility of iron to rust
75
Q

When any Hydrocarbon is burned it produces what 2 things?

A

CO2 (carbon dioxide) and H2O (water)

76
Q

Physical changes

A

changes in the properties of matter that do not affect its composition.

  • the kinds of molecules don’t change
  • i.e. heating water (raises temp but it is still water)
  • evaporating butane from a lighter
  • dissolving sugar in water (sugar can still be separated from water.
77
Q

Chemical changes

A

involve a change in the properties of matter that change its composition

  • a chem rxn
  • the new substances have different molecules than the original substances
  • rusting is iron combining with oxygen to make iron (III) oxide
  • burning butane from a lighter changes it into carbon dioxide and water.
78
Q

Phase changes are ___________.

A

physical changes

79
Q

Boiling

A

liquid to gas

80
Q

Melting

A

solid to liquid

81
Q

Subliming

A

solid to gas (dry ice CO2(s))

82
Q

Condensing

A

gas to liquid

83
Q

Freezing

A

liquid to solid

84
Q

Deposition

A

gas to solid

85
Q

State changes require _________ or _________ the substance.

A

heating
cooling
(occurs by changing the temp)

86
Q

Separation of mixtures by different physical properties- Distillation

A

taking advantage of different boiling points of chemicals involved.

87
Q

Separation of mixtures by different physical properties-Filtration

A

taking advantage of the different states of matter

Gravity filtration allows for the separation of heterogeneous mixtures

88
Q

Scientific method

A

a way that scientists learn about the natural world

89
Q

Observation

A

to measure or describe something about the physical world

90
Q

Qualitative observation

A

A qualitative observation would be one describing the quality of a thing (e.g. round, blue, hot) without expressing numerical values

91
Q

Quantitative observation

A

a quantitative observation, such as the weight or length of an object. Quantitative observations have numbers, such as 3 pounds or 5 meters.

92
Q

Scientific law

A

a statement that summarizes past observations and predicts future ones

  • usually formulated from a series of related observations
  • just states things does not give why.
93
Q

Hypothesis

A

a tentative explanation for an observation or scientific problem that can be tested by further investigation.

94
Q

Experiment

A

procedures designed to test scientific laws, hypotheses, or theories

95
Q

Theory

A

a proposed explanation for observations and laws

-based on one or more well established hypotheses

96
Q

Precision

A

the reproducibility of multiple measurements, it is how close the experimental values for different trials are to each other

97
Q

Accuracy

A

has to do with how close the experimental results are to the true value.

98
Q

The last digit of a number is always a _________ the first place of ____________.

A

guess

uncertainty

99
Q

Energy

A

anything that has the capacity to do work

100
Q

Even though chemistry is the study of matter, matter is affected ____________.

A

energy

-it can cause physical and/or chemical changes in matter

101
Q

What are the kinds of Energy?

A

Kinetic

Potential

102
Q

Kinetic energy

A

energy of motion, or energy that is being transferred from one object to another.

103
Q

Potential energy

A

energy that is stored; aka energy of postion- can be transformed into kinetic energy

104
Q

What are the forms of energy?

A
  1. Electrical
  2. Heat/thermal
  3. Light/radiant
  4. Chemical
105
Q

Electrical energy

A

kinetic energy associated with the flow of electrical charge

106
Q

Heat/Thermal energy

A

kinetic energy associated with molecular motion

107
Q

Light/Radiant energy

A

kinetic energy associated with energy transitions in an atom.

108
Q

Chemical energy

A

potential energy in the attachment of atoms or because of their position.

109
Q

Heat

A

(verb) is the exchange of thermal energy between samples of matter

110
Q

Heat flows from matter that has _____ thermal energy to matter that has ____ thermal energy.

A

high
low

-until they reach the same temperature

111
Q

How is heat exchanged?

A

heat is exchanged through molecular collisions between two samples.

112
Q

When a process results in the evolution of heat, it is said to be what?

A

exothermic

-i.e. the burning of a match releases heat (energy)

113
Q

A process that absorbs energy is said to be what?

A

endothermic

-i.e. melting ice to form liquid water (requires energy source)

114
Q

Scientific notation

A

a system used to write very big or very small numbers in a more compact and precise way.

115
Q

A number written in scientific notaion consists of a _____ part and an __________ part.

A 
decimal (a # usually between 1 and 10)
exponential part (10 raised to some exponent)
116
Q

Write the following number in scientific notation; 3,456,700

A

3.4567x10^6

117
Q

Write the following number in scientific notation; 0.00000012

A

1.2x10^-7

118
Q

10^0

A

1

119
Q

10^1

A

10

120
Q

10^2

A

100

121
Q

10^-1

A

0.1

122
Q

10^-2

A

0.01

123
Q

sig fig rule A

A

All non-zero digits are significant; 3.14

124
Q

sig fig rule B

A

Interior zeros are significant; 3.004

125
Q

sig fig rule C

A

trailing zeros are significant when a decimal is present; 300.00

126
Q

sig fig rule D

A

leading zeros are NOT significant; 0.0000012

127
Q

sig fig rule E

A

exact numbers have infinite sig figs; this includes accurate counting of discrete numbers, defined quantities, and integral numbers

128
Q

how many sig figs? 8 atoms

A

according to sig fig rule E1 discrete numbers that are counted accurately have an infinite amount of sig figs
8.00000000…..

129
Q

how many sig figs? 100cm = 1 m

A

according to sig fig rule E2 defined quantities have an infinite number of sig figs

look for equal sign

100.00000….cm = 1.0000….m

130
Q

how many sig figs? D = r/2

A

according to sig fig rule E3 integral numbers (formulas) have an infinite number of sig figs

the 2 is exact, otherwise formula is false

131
Q

How do you round using sig figs when multiplying or dividing?

A

the product or quotient has the same number of sig figs as the number with the lowest number of sig figs

132
Q

How do you round using sig figs when adding or subtracting?

A

the sum or the difference has the same number of decimal places as the quantity carrying the fewest decimal places.

133
Q

How do you round using sig figs when you encounter calculations involving multiplication/division and addition/subtraction?

A
  1. follow order of operations

2. keep track of significant figures through each step and only round at the end

134
Q

Units

A

previously agreed on quantities used to report experimental measurements

135
Q

What are the two common unit systems?

A

English system and Metric system (SI/ International system of units)

136
Q

What is the SI unit for length?

A

meter; m

137
Q

What is the SI unit for mass?

A

kilograms; kg

138
Q

What is the SI unit for Time?

A

seconds; s

139
Q

What is the SI unit for temperature?

A

Kelvins; K

140
Q

Conversion factors

A

relationships between 2 units; conversion factors are generated from equivalence statements 1 in = 2.54 cm

141
Q

dimensional analysis

A

using units as a guide to problem-solving

142
Q

Derived units

A

a unit formed from the combination of other units

ex. volume is the measure of 3D space occupied; V is derived from length
ex. Density is mass divided by volume

143
Q

meniscus

A

lowest point of concave or highest point of convex

144
Q

Density

A

units of mass divided by volume (most commonly expressed as g/cm^3, g/mL, or g/L

145
Q

Temperature

A

the measure of the average kinetic energy of the molecules in a sample

146
Q

Do all molecules in a sample have the same amount of kinetic energy?

A

No, that is why temperature gives us an average of the kinetic energy of molecules in a sample

147
Q

a higher temperature means a ______________

A

larger average kinetic energy

148
Q

The Kelvin scale has no _________

A

negative values; real things are always in positive amounts.

149
Q

What two reference points does the Fahrenheit scale use?

A

the freezing point of concentrated salt water (0 degrees F) and the supposed average body temp (100 degrees F)

150
Q

What is room temp in Fahrenheit?

A

75 degrees F

151
Q

What are the two reference points for Celsius scale?

A

the freezing point of DI water (0 degrees C) and the boiling point of DI water (100 degrees C)

152
Q

What temperature scale is commonly used in science?

A

Celsius; because they have more reproducible standards

153
Q

What is room temperature in Celsius?

A

25 degrees C

154
Q

Specific heat capacity

A

(specific heat) the amount of energy needed to change one gram of a substance by 1 degree Celsius.

155
Q

What is the specific heat capacity of liquid water?

A

4.184 J/g degrees C

Chemistry (5 decks)

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