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

Module 1: Introduction - Matter and Measurement Flashcards

(115 cards)

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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
What are physical properties of a substance?
properties that can be observed without changing a substance into another substance
26
What are some examples of physical properties?
boiling point, density, mass, volume
27
What are chemical properties of a substance?
Properties that can ONLY be observed when a substance is changed into another substance
28
Examples of chemical properties
flammability, corrosiveness, reactivity with acid
29
What types of properties can we observe about a substance (regarding its quantity)
Intensive and extensive properties
30
What is an intensive property of a substance?
A property that is independent of the amount of the substance that is present
31
Examples of intensive properties
density, boiling point, color
32
What are extensive properties of a substance?
Properties that depend upon the amount of the substance present
33
What are some examples of extensive properties?
mass, volume, energy
34
What are physical changes?
Changes in matter that do not change the composition of a substance
35
Examples of physical changes
changes of state, temperature, and volume
36
What are chemical changes?
changes to a substance that result in new substances
37
Examples of chemical changes
combustion, oxidation, and decomposition
38
Converting between the 3 states of matter is what type of change?
a physical change (Ex: when ice melts or water evaporates, there are still 2 H atoms and 1 O atom in each molecule)
39
What are 3 methods used to separate mixtures?
filtration, distillation, chromatography
40
What are mixtures separated based on?
The physical properties of the components of the mixture
41
What is filtration?
Solid substances are separated from liquids and solutions
42
What is distillation?
Distillation uses differences in boiling points of substances to separate a homogenous mixture into its components
43
What is chromatography?
Separates substances on the basis of differences in the ability of substances to adhere to the solid surface (Ex: dyes to paper)
44
What units do we use in chemistry?
SI units
45
What is the SI?
The International System of Units (Systeme International d'Unites)
46
SI unit of mass
Kilogram (kg)
47
SI unit for length
meter (m)
48
SI unit for time
second (s or sec)
49
SI unit for temperature
Kelvin (K)
50
SI unit for an amount of substance
Mole (mol)
51
SI unit for electric current
ampere (A or amp)
52
SI unit for luminous intensity
candela (cd)
53
What is the metric system based on?
10
54
Metric base for mass
gram (g)
55
Metric base unit for length
meter (m)
56
Metric base unit for time
second (s or sec)
57
Metric base unit for temperature
degrees celsius or Kelvins
58
metric system base units for amount of substance
mole (mol)
59
metric system base units for volume
cubic centimeter (cc or cm^3) or liter (l)
60
What do we use prefixes for?
To convert the base units into units that are appropriate for common usage or appropriate measure
61
Prefix petra
Abbreviation: P 10^15
62
Prefix Tera
Abbreviation: T 10^12
63
Prefix giga
Abbreviation: G 10^9
64
Prefix mega
Abbreviation: M 10^6
65
Prefix kilo
Abbreviation: k 10^3
66
Prefix deci
Abbreviation: d 10^-1
67
Prefix centi
Abbreviation: c 10^-2
68
Prefix milli
Abbreviation: m 10^-3
69
Prefix micro
Abbreviation: (greek letter mu) 10^-6
70
Prefix nano
Abbreviation: n 10^-9
71
Prefix pico
Abbreviation: p 10^-12
72
Prefix femto
Abbreviation: f 10^-15
73
Prefix atto
Abbreviation: a 10^-18
74
Prefix zepto
Abbreviation: z 10^-21
75
What are the basic units we measure in in science?
mass and length
76
What is mass?
a measure of the amount of material in an object (base unit is kg in SI; base unit is gram in metric)
77
What is length?
a measure of distance (meter is the base unit)
78
what is volume
the amount of 3D space that a substance or object occupies
79
Is volume a base unit in SI?
No
80
What is volume derived from in SI?
length (m * m * m = m^3)
81
What are the most commonly used metric units for volume?
liter (L) and milliliter (mL)
82
What is a liter?
A cube 1 decimeter long on each side
83
What is a milliliter
A cube 1 centimeter long on each side (also called 1 cubic centimeter) (cm * cm * cm = cm^3)
84
What is temperature?
In general, temperature is considered the "hotness and coldness" of an object that determines the direction of heat flow
85
How does heat flow?
Heat flows spontaneously from an object with higher temperature to an object with a higher temperature to an object with a lower temperature
86
What temperature scales are used in science
Celsius and Kelvin
87
What is the Celsius scale based on?
The properties of water
88
What are the freezing/boiling point of water on the Celsius scale?
0 degrees Celsius = freezing point of water 100 degrees Celsius = boiling point of water
89
What is the Kelvin temperature scale based on?
The properties of gases
90
What is the lowest possible Kelvin temperature?
0 K (absolute zero) There is no motion of molecules/no heat
91
What is the conversion from Kelvin to Celsius?
K = degrees Celsius + 273.15
92
What is the Fahrenheit scale based on?
Weather/people
93
Is Fahrenheit used in scientific measurements
no
94
Conversion from Fahrenheit to Celsius
Degrees F = 9/5 (C) + 32
95
Conversion from Celsius to Fahrenheit
Degrees Celsius = 5/9 (F - 32)
96
What type of property is density?
a physical property
97
Where are the units from density derived from?
Units for mass and volume
98
What are the most common units for density?
g/mL or g/cm
99
Formula for density
D = m/V
100
What is an exact number
numbers that are counted or given by definition
101
Examples of exact numbers
12 eggs in 1 dozen, 4 people
102
What is an inexact number?
Also called a measured number. Depends on how the number was determined because scientific instruments have limitations (different limitations on different instruments)
103
All measured numbers have some degree of
inaccuracy
104
What is accuracy
The proximity of a measurement to the true value of a quantity
105
What is precision
The proximity of several measurements to each other
106
What are significant figures
Refers to the digits that were measured
107
Why do we pay attention to the significant figures
So we do not overstate the accuracy of our answers
108
Rules for sig figs: all nonzero digits are:
significant
109
Rules for sig figs: zeros between 2 significant figures are:
significant
110
Rules for sig figs: zeroes at the beginning of a number are:
never significant
111
Rules for sig figs: zeroes at the end of a number are significant only if:
a decimal point is written in the number
112
When addition or subtraction is performed, answers are rounded to?
The least significant decimal place
113
When multiplication or division is performed, answers are rounded to?
The number of digits that corresponds to the least number of significant figures in any of the numbers used in the calculation
114
What do we use dimensional analysis for?
To convert one quantity to another unit
115
What does dimensional analysis often use?
Conversion factors (like 1 in = 2.54 cm)

ILCC General Chemistry (2 decks)

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