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ILCC General Chemistry > Module 1: Introduction - Matter and Measurement > Flashcards

Module 1: Introduction - Matter and Measurement Flashcards

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1
Q

Define chemistry

A

Chemistry is the study of the properties and behavior of matter

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2
Q

Define matter

A

Anything that takes up space and has mass

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3
Q

Define atoms

A

Building blocks of matter; each element is made of a unique kind of atom

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4
Q

How many kinds of atoms does an element have?

A

1

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5
Q

What is a compound?

A

A substance made of 2 or more types of elements (2 or more types of atoms)

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6
Q

What are the 2 ways to classify matter?

A

States of matter; composition of matter

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7
Q

What are the states of matter?

A

Solid, liquid, gas

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8
Q

What are the states of matter for water?

A

Solid=ice, liquid=water, gas=water vapor

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9
Q

How do you classify matter based on its composition?

A

Follow the schema to determine what type of mixture the matter is

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10
Q

What are the classifications of matter based on composition?

A

Element, compound, homogenous mixture, heterogenous mixture

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11
Q

Define substance

A

Something that has distinct properties and does not vary from sample to sample

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12
Q

What are the 2 types of substances?

A

elements and compounds

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13
Q

Can an element be broken down further?

A

No: it can not be decomposed to simpler substances

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14
Q

Can a compound be broken down further?

A

Yes: it can be broken down into simpler substances

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15
Q

What does it mean that compounds have a definite composition?

A

The relative number of each atom that makes up the compound is the same in any sample

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16
Q

What is the law of constant composition?

A

Law that compounds have a definite composition: relative number of atoms of each element are the same in any sample

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17
Q

What is another name for the Law of Constant Composition?

A

Law of Definite Proportions

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18
Q

What does the Law of Constant Composition mean for water?

A

Water is composed of hydrogen atoms and oxygen atoms, always in a 2:1 ratio. Water is H2O

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19
Q

What properties do mixtures exhibit?

A

The properties of the substances that make them up

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20
Q

What are the types of mixtures?

A

Homogenous and heterogenous

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21
Q

What is a heterogenous mixture?

A

Varies in composition throughout a sample

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22
Q

What is a homogenous mixture?

A

same composition throughout a sample

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23
Q

What is another name for a homogenous mixture?

A

solution

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24
Q

What types of properties can we observe about a substance?

A

physical properties and chemical properties

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25
Q

What are physical properties of a substance?

A

properties that can be observed without changing a substance into another substance

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26
Q

What are some examples of physical properties?

A

boiling point, density, mass, volume

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27
Q

What are chemical properties of a substance?

A

Properties that can ONLY be observed when a substance is changed into another substance

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28
Q

Examples of chemical properties

A

flammability, corrosiveness, reactivity with acid

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29
Q

What types of properties can we observe about a substance (regarding its quantity)

A

Intensive and extensive properties

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30
Q

What is an intensive property of a substance?

A

A property that is independent of the amount of the substance that is present

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31
Q

Examples of intensive properties

A

density, boiling point, color

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32
Q

What are extensive properties of a substance?

A

Properties that depend upon the amount of the substance present

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33
Q

What are some examples of extensive properties?

A

mass, volume, energy

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34
Q

What are physical changes?

A

Changes in matter that do not change the composition of a substance

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35
Q

Examples of physical changes

A

changes of state, temperature, and volume

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36
Q

What are chemical changes?

A

changes to a substance that result in new substances

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37
Q

Examples of chemical changes

A

combustion, oxidation, and decomposition

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38
Q

Converting between the 3 states of matter is what type of change?

A

a physical change
(Ex: when ice melts or water evaporates, there are still 2 H atoms and 1 O atom in each molecule)

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39
Q

What are 3 methods used to separate mixtures?

A

filtration, distillation, chromatography

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40
Q

What are mixtures separated based on?

A

The physical properties of the components of the mixture

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41
Q

What is filtration?

A

Solid substances are separated from liquids and solutions

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42
Q

What is distillation?

A

Distillation uses differences in boiling points of substances to separate a homogenous mixture into its components

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43
Q

What is chromatography?

A

Separates substances on the basis of differences in the ability of substances to adhere to the solid surface (Ex: dyes to paper)

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44
Q

What units do we use in chemistry?

A

SI units

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45
Q

What is the SI?

A

The International System of Units (Systeme International d’Unites)

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46
Q

SI unit of mass

A

Kilogram (kg)

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47
Q

SI unit for length

A

meter (m)

48
Q

SI unit for time

A

second (s or sec)

49
Q

SI unit for temperature

A

Kelvin (K)

50
Q

SI unit for an amount of substance

A

Mole (mol)

51
Q

SI unit for electric current

A

ampere (A or amp)

52
Q

SI unit for luminous intensity

A

candela (cd)

53
Q

What is the metric system based on?

A

10

54
Q

Metric base for mass

A

gram (g)

55
Q

Metric base unit for length

A

meter (m)

56
Q

Metric base unit for time

A

second (s or sec)

57
Q

Metric base unit for temperature

A

degrees celsius or Kelvins

58
Q

metric system base units for amount of substance

A

mole (mol)

59
Q

metric system base units for volume

A

cubic centimeter (cc or cm^3) or liter (l)

60
Q

What do we use prefixes for?

A

To convert the base units into units that are appropriate for common usage or appropriate measure

61
Q

Prefix petra

A

Abbreviation: P
10^15

62
Q

Prefix Tera

A

Abbreviation: T
10^12

63
Q

Prefix giga

A

Abbreviation: G
10^9

64
Q

Prefix mega

A

Abbreviation: M
10^6

65
Q

Prefix kilo

A

Abbreviation: k
10^3

66
Q

Prefix deci

A

Abbreviation: d
10^-1

67
Q

Prefix centi

A

Abbreviation: c
10^-2

68
Q

Prefix milli

A

Abbreviation: m
10^-3

69
Q

Prefix micro

A

Abbreviation: (greek letter mu)
10^-6

70
Q

Prefix nano

A

Abbreviation: n
10^-9

71
Q

Prefix pico

A

Abbreviation: p
10^-12

72
Q

Prefix femto

A

Abbreviation: f
10^-15

73
Q

Prefix atto

A

Abbreviation: a
10^-18

74
Q

Prefix zepto

A

Abbreviation: z
10^-21

75
Q

What are the basic units we measure in in science?

A

mass and length

76
Q

What is mass?

A

a measure of the amount of material in an object
(base unit is kg in SI; base unit is gram in metric)

77
Q

What is length?

A

a measure of distance (meter is the base unit)

78
Q

what is volume

A

the amount of 3D space that a substance or object occupies

79
Q

Is volume a base unit in SI?

A

No

80
Q

What is volume derived from in SI?

A

length (m * m * m = m^3)

81
Q

What are the most commonly used metric units for volume?

A

liter (L) and milliliter (mL)

82
Q

What is a liter?

A

A cube 1 decimeter long on each side

83
Q

What is a milliliter

A

A cube 1 centimeter long on each side (also called 1 cubic centimeter)
(cm * cm * cm = cm^3)

84
Q

What is temperature?

A

In general, temperature is considered the “hotness and coldness” of an object that determines the direction of heat flow

85
Q

How does heat flow?

A

Heat flows spontaneously from an object with higher temperature to an object with a higher temperature to an object with a lower temperature

86
Q

What temperature scales are used in science

A

Celsius and Kelvin

87
Q

What is the Celsius scale based on?

A

The properties of water

88
Q

What are the freezing/boiling point of water on the Celsius scale?

A

0 degrees Celsius = freezing point of water
100 degrees Celsius = boiling point of water

89
Q

What is the Kelvin temperature scale based on?

A

The properties of gases

90
Q

What is the lowest possible Kelvin temperature?

A

0 K (absolute zero)
There is no motion of molecules/no heat

91
Q

What is the conversion from Kelvin to Celsius?

A

K = degrees Celsius + 273.15

92
Q

What is the Fahrenheit scale based on?

A

Weather/people

93
Q

Is Fahrenheit used in scientific measurements

A

no

94
Q

Conversion from Fahrenheit to Celsius

A

Degrees F = 9/5 (C) + 32

95
Q

Conversion from Celsius to Fahrenheit

A

Degrees Celsius = 5/9 (F - 32)

96
Q

What type of property is density?

A

a physical property

97
Q

Where are the units from density derived from?

A

Units for mass and volume

98
Q

What are the most common units for density?

A

g/mL or g/cm

99
Q

Formula for density

A

D = m/V

100
Q

What is an exact number

A

numbers that are counted or given by definition

101
Q

Examples of exact numbers

A

12 eggs in 1 dozen, 4 people

102
Q

What is an inexact number?

A

Also called a measured number. Depends on how the number was determined because scientific instruments have limitations (different limitations on different instruments)

103
Q

All measured numbers have some degree of

A

inaccuracy

104
Q

What is accuracy

A

The proximity of a measurement to the true value of a quantity

105
Q

What is precision

A

The proximity of several measurements to each other

106
Q

What are significant figures

A

Refers to the digits that were measured

107
Q

Why do we pay attention to the significant figures

A

So we do not overstate the accuracy of our answers

108
Q

Rules for sig figs: all nonzero digits are:

A

significant

109
Q

Rules for sig figs: zeros between 2 significant figures are:

A

significant

110
Q

Rules for sig figs: zeroes at the beginning of a number are:

A

never significant

111
Q

Rules for sig figs: zeroes at the end of a number are significant only if:

A

a decimal point is written in the number

112
Q

When addition or subtraction is performed, answers are rounded to?

A

The least significant decimal place

113
Q

When multiplication or division is performed, answers are rounded to?

A

The number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation

114
Q

What do we use dimensional analysis for?

A

To convert one quantity to another unit

115
Q

What does dimensional analysis often use?

A

Conversion factors (like 1 in = 2.54 cm)

ILCC General Chemistry (2 decks)

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