Chemistry Exam 1 Things To Memorize

Front 1

A pure substance that can't be broken down into simpler unique substances by ordinary chemical means

Back 1

Element

Front 2

A particle composed of two of more atoms, in which the atoms are chemically combined by sharing electrons

Back 2

Molecule

Front 3

Nitrogen is a gas at room temperature, with a density of 1.024 g/L. These are examples of ____ properties

Back 3

Physical

Front 4

A _____ mixture has a composition that varies within a particular sample of the mixture

Back 4

Heterogeneous

Front 5

Properties that depend upon the sample size of a substance are called _____ properties

Back 5

Extensive

Front 6

The ____ _____ of an object depends upon its position in a field.

Back 6

Potential Energy

Front 7

A ____ is an attraction or repulsion affecting matter.

Back 7

Force

Front 8

____ changes to a substance result in the production of a new substance

Back 8

Chemical

Front 9

The SI unit for temperature is the ____.

Back 9

kelvin (K)

Front 10

Protons and neutrons are called ____, due to their location in an atom.

Back 10

Nucleons

Front 11

The ____ Number specifies the number of protons and neutrons in a specific atom of an element.

Back 11

Mass (A)

Front 12

A/An ____ is a fundamental particle with the mass of an electron, but with a positive charge.

Back 12

Positron (β+)

Front 13

A law is a summary of a pattern of behavior or phenomena, with no explanation of that
behavior or phenomenon offered

Back 13

A Law

Front 14

How a law differs from a theory

Back 14

Theories explain, laws declare cause-and-effect. Both can be
used for predicting unobserved behavior or phenomena

Front 15

A theory is a tested, generally-accepted explanation for
behavior or phenomena

Back 15

A Theory

Front 16

A stable combination of two or more atoms, in which the atoms are chemically combined

Back 16

Molecule

Front 17

A pure substance composed of two or more atoms of different elements

Back 17

Compound

Front 18

Distinguish between Molecule and Compound

Back 18

A molecule is a particle, a tiny piece of matter. A compound is substance, a specific
type of matter. The smallest particle of some compounds (but not all!) is a molecule, and
there are molecules of the other type of matter, elements. The two terms are NOT
interchangeable.

Front 19

Matter that consists of two or more substances in variable amounts
(ex: salt and table sugar)

Back 19

Mixture

Front 20

Distinguish between Compound and Mixture

Back 20

A compound is a pure substance composed of two or more elements, with a fixed or
constant ratio (by mass and by number of atoms), in which the atoms are chemically
combined (bonded). A mixture is composed of two or more different substances (elements
and/or compounds), with a variable composition: the ratio of substances can be changed.
Also, the forces holding the particles together in a mixture are rarely chemical bonds.


Compound: two or more atoms made of different elements
Mixture: two or more substances in variable amounts (ex: salt and table sugar)

Front 21

Intensive properties are independent of the sample size; they are properties intrinsic
to the substance. Examples are density, melting point, and temperature

Back 21

Intensive Properties

Front 22

Extensive
properties depend upon the amount of the substance in the sample. Examples include
mass, volume, and heat content

Back 22

Extensive Properties

Front 23

Distinguish between Intensive and Extensive Properties

Back 23

Intensive properties don't change based on the amount of substance- smaller amount to bigger amount is still ≈ to smaller mass to bigger mass and volume.
Extensive properties do change based on the amount of substance, a smaller amount of stuff=smaller mass and affects the amount (density) of the substance.

Front 24

Round 0.2001576 cm to 4 significant figures

Back 24

0.2002 cm

Front 25

Round 1.332099 mL to 4 significant figures

Back 25

1.332mL

Front 26

Write 0.000997355 kg in proper scientific notation to 3 sig. figs.

Back 26

9.97×10^-4 kg

Front 27

Write 273.155 K in proper scientific notation to 3 sig. figs.

Back 27

2.73 × 10² K

Front 28

pico-(p)

Back 28

one-trillionth (10 ‾¹²)

Front 29

nano-(n)

Back 29

one-billionth (10^ -9)

Front 30

micro-(µ)

Back 30

one-millionth (10^-6)

Front 31

milli-(m)

Back 31

one-thousandth (.001 or 10‾³)

Front 32

centi-(c)

Back 32

one-hundredth (.01 or 10‾²)

Front 33

deci-(d)

Back 33

one-tenth (.1 or 10‾¹)

Front 34

kilo-(k)

Back 34

one thousand (1,000 or 10³)

Front 35

mega-(M)

Back 35

one million (10^6)

Front 36

giga-(G)

Back 36

one billion (10^9)

Front 37

Temperature Conversion °F ⇒ °C

Back 37

°F=32+ 9/5×° C

Front 38

Temperature Conversion °C ⇒ °F

Back 38

°C=5/9×(°F−32)

Front 39

Temperature Conversion K ⇒ °C

Back 39

K=°C+273.15

Front 40

carbon
symbol & atomic number

Back 40

C
Atomic number: 6

Front 41

fluorine
symbol & atomic number

Back 41

F
Atomic number: 9

Front 42

gold
symbol & atomic number

Back 42

Au
Atomic number: 79

Front 43

iodine
symbol & atomic number

Back 43

I
Atomic number: 53

Front 44

phosphorus
symbol & atomic number

Back 44

P
Atomic number: 15

Front 45

helium
symbol & atomic number

Back 45

He
Atomic number: 2

Front 46

tin
symbol & atomic number

Back 46

Sn
Atomic number: 50

Front 47

oxygen
symbol & atomic number

Back 47

O
Atomic number: 8

Front 48

iron
symbol & atomic number

Back 48

Fe
Atomic number: 26

Front 49

hydrogen
symbol & atomic number

Back 49

H
Atomic number: 1

Front 50

lead
symbol & atomic number

Back 50

Pb
Atomic number: 82

Front 51

nitrogen
symbol & atomic number

Back 51

N
Atomic number: 7

Front 52

sodium
symbol & atomic number

Back 52

Na
Atomic number: 11

Front 53

magnesium
symbol & atomic number

Back 53

Mg
Atomic number: 12

Front 54

aluminum
symbol & atomic number

Back 54

Al
Atomic number: 13

Front 55

silicon
symbol & atomic number

Back 55

Si
Atomic number: 14

Front 56

sulfur
symbol & atomic number

Back 56

S
Atomic number: 16

Front 57

chlorine
symbol & atomic number

Back 57

Cl
Atomic number: 17

Front 58

potassium
symbol & atomic number

Back 58

K
Atomic number: 19

Front 59

calcium
symbol & atomic number

Back 59

Ca
Atomic number: 20

Front 60

bromine
symbol & atomic number

Back 60

Br
Atomic number: 35

Front 61

silver
symbol & atomic number

Back 61

Ag
Atomic number: 47

Front 62

mercury
symbol & atomic number

Back 62

Hg
Atomic number: 80

Front 63

Radioactivity

Back 63

Radioactivity is a property of certain unstable nuclei, in which the unstable nucleus
spontaneously disintegrates, giving off radiation in the form of particles, energy or both

Front 64

Ionization

Back 64

The formation of ions

Front 65

Cations

Back 65

Positive ions, formed by loss of electrons

Front 66

Anions

Back 66

Negative ions, formed by gain of electrons

Front 67

Radioactive Decay

Back 67

The process in which a nucleus spontaneously disintegrates, giving off (nuclear) radiation

Front 68

Radiation

Back 68

Energy that flows from a source
ex: energy, heat, light

Front 69

John Dalton's explanation of Lavoisier's "Law of Conservation of Mass"
(Law of Conservation of Matter)

Back 69

The Law of Conservation of Mass states that in any process mass is conserved: the mass of
the products (the final mass) equals the mass of the reactants (the initial mass). Dalton explained this relationship by postulating that atoms, the fundamental particles making up
all matter, can neither be created nor destroyed, nor could atoms of one element be
transformed into atoms of another element. Dalton also stated that chemical reactions
simply involved a reorganization of atoms. Together these statements explain Lavoisier’s
law.

When a chemical reaction takes place, matter is neither created nor destroyed.

Front 70

Intensive vs. Extensive Properties

Back 70

Intensive properties do not depend
upon the size of the sample
measured
Extensive properties do depend upon
the amount of stuff

Front 71

The difference between the terms Atomic Mass and Mass Number

Back 71

The mass number is a number of particles: the total number of protons and neutrons
(together, the nucleons) in the nucleus of a specific isotope. The atomic mass of an atom is
the actual mass of (amount of matter in) an atom, which takes into account the mass of the
nucleons, the electrons, and the mass defect due to the binding energy. The average atomic
mass found on the periodic table is an average of the masses of all the known isotopes of
an element, the average being “weighted” by the relative abundance of those isotopes in
nature. The mass of each isotope is determined by comparing it to the mass of a carbon-12
atom, which mass is defined to be exactly 12 atomic mass units (amu).