Chemistry Marking Period 1 Nrhs

Front 1

Length

Back 1

In science, we measure
length using the mete

Front 2

Mass

Back 2

Mass is a quantity of
matter

Front 3

Volume

Back 3

Volume measures the amount of space an object
occupies

Front 4

Temperature

Back 4

Temperature should be recorded using Kelvin (K)

Front 5

Conversion Factor

Back 5

When a measurement is multiplied by a
conversion factor, the numerical value is generally
changed, but the actual size of the quantity
measured remains the same

Front 6

Dimensional Analysis

Back 6

a way to analyze and solve problems using the
units of the measurement

Front 7

Error

Back 7

There is a difference between accepted and
experimental values.

– Accepted value: correct value based on reliable references

– Experimental value: value measured in lab

Front 8

% Error

Back 8

Is the absolute value, positive value, of the
error divided by the accepted value and then
multiplied by 100%

Front 9

Accuracy

Back 9

Accuracy is a measure of how close a
measurement comes to the actual or
true value of whatever is measured

Front 10

Precision

Back 10

Precision is a measure of how close a
series of measurements are to one
another

Front 11

Standard Notation

Back 11

A given number which is written with decimal
values and without a (x10) value

Front 12

Scientific Notation

Back 12

A given number which is written as the
product of two numbers:

– A coefficient and

– 10 raised to a power

Front 13

Matter

Back 13

PURE
SUBSTANCES and

Mixtures Made of 2+
substances

Front 14

Pure Substance

Back 14

Element & Compound

Front 15

Element

Back 15

Can NOT be separated by chemical means

Front 16

Compound

Back 16

Separated by chemical means ONLY Made up of 2+ elements chemically combined

Front 17

MIXTURES

Back 17

Homogeneous Mixture (solution) & Heterogeneous Mixture

Front 18

Homogeneous Mixture (solution)

Back 18

Same composition throughout
“UNIFORM”

Front 19

Heterogeneous Mixture

Back 19

Different composition throughout
“NOT UNIFORM”

Front 20

Annotation of Matter

Back 20

Chemists use chemical symbols to represent elements.

Front 21

Properties of Matter

Back 21

To understand matter, we begin by using observations and listing properties. Physical and Chemical

Front 22

Extensive Property

Back 22

A property that depends on how much material you are dealing with

Front 23

Intensive Properties

Back 23

A property that does not depend on how much material you are dealing with but helps identify matter (a constant about that particular type of matter)

Front 24

Chemical Property

Back 24

A property or behavior of a substance when it undergoes a chemical change or reaction

Front 25

Changes in Matter

Back 25

Matter can be altered by physical or chemical means

Front 26

Physical Change

Back 26

A change that does NOT alter the chemical properties in a substance

Front 27

Chemical Change

Back 27

Any change that results in the formation of new chemical substances. At the molecular level,chemical change involves making or breaking of bonds between atoms.

Front 28

States of Matter

Back 28

a solid, liquid, or gas.

Front 29

Solids

Back 29

a form of matter that has definite shape and volume.

Front 30

Liquids

Back 30

a form of matter that has indefinite shape, flows, but has a fixed volume.

Front 31

Gases

Back 31

a form of matter that has indefinite shape and indefinite volume.

Front 32

Plasma

Back 32

When air or gas is charged, plasma forms with conductive properties similar to those of metals.

Front 33

Separation of Matter

Back 33

In a chemical reaction, COMPOUNDS can be
CHEMICALLY separated into the elements that make it up.

Front 34

Filtration

Back 34

Filtrate flows through filter paper, undissolved particles remain on filter paper.

Front 35

Watch Glass Evaporation

Back 35

Separate the dissolved solid (solute) from the liquid (solvent) by boiling the solution

Front 36

Crucible Evaporation

Back 36

Removes any liquid captured inside the crystals of a solid by heating until boiling point has been reached.

Front 37

Distillation

Back 37

Will separate 2 or more liquids by there different boiling points.

Front 38

Chromatography

Back 38

Will separate particles based on their size and solubility

Front 39

The atom

Back 39

The ATOM is the smallest particle of an element that retains its identity in a chemical reaction.

Front 40

Parts of any atom

Back 40

Electrons – Protons – Neutrons

Front 41

Protons (p+)

Back 41

Have a mass of approx. 1 atomic mass unit
(a.m.u.)

Positively charged

Front 42

Neutrons (n0)

Back 42

Have a mass of approx. 1 a.m.u.

Neutral charge

Front 43

Electrons (e-)

Back 43

Have a mass of approx 1/1840 a.m.u.

Negative charge

Front 44

Democritus

Back 44

A Greek philosopher that believed
that atoms were indestructible and
indivisible

Front 45

John Dalton

Back 45

In the 1700s, John Dalton
transformed Democritus’s ideas on
atoms into a scientific theory by
using experimental methods.

Front 46

Dalton’s Atomic Theory

Back 46

All elements are composed of
indivisible atoms.

Front 47

The Nucleus

Back 47

The first, Dalton’s theory a solid
indivisible, indestructible particle
The second, J.J. Thompson and others
supposed the atom was filled with
positively charged material and the
electrons were evenly distributed
throughout.
And then came Ernest Rutherford and
his Gold Foil Experiment

Front 48

Gold-Foil Experiment

Back 48

In 1911, Rutherford and his coworkers
at the University of Manchester,
England, directed a narrow beam of
alpha particles at a very thin sheet
of gold foil.

Front 49

Rutherford’s Atomic Theory

Back 49

Rutherford concluded that the atom
is mostly empty space. All the
positive charge and almost all of the
mass are concentrated in a small
region called the nucleus.

Front 50

Physical Property

Back 50

A quality or condition of a substance that can be observed or measured without changing the substance’s composition.

Front 51

Isotopes

Back 51

ISOTOPES are atoms that have the same
number of protons but different numbers of
neutrons.

Front 52

Atomic Mass

Back 52

The ATOMIC MASS of an element is a
weighted average mass of the atoms in a
naturally occurring sample of the element

Front 53

How to Calculate
Average Atomic Mass

Back 53

1. multiply each of the element’s isotopes to their %
abundance
2. Divide each product by 100 (to remove the %)
3. Add up all the values together
(isotope’s mass x it’s % abundance) + …
100

Front 54

Isotopes

Back 54

ISOTOPES are atoms that have the
same number of protons but
different numbers of neutrons.

Front 55

Naming Isotopes &
Isotope Notation

Back 55

Remember that isotopes have the same # of protons and electrons. They also have the same atomic number.

Front 56

Atomic Orbitals

Back 56

An PRINCIPLE ENERGY LEVEL is
often thought of as a region of
space in which there is a high
probability of finding an electron.

Front 57

Energy Sublevels

Back 57

There are four energy sublevels: – s – p – d – f

Front 58

Electron Configurations

Back 58

The ways in which electrons are arranged
in various orbitals around the nuclei of
atoms

Front 59

Expanded Configurations

Back 59

An expanded e- configuration gives us
more information than a short-hand
configuration

Front 60

Filling the sub-orbitals:

Back 60

1s2s2p63s23p64s23d10...

Front 61

Orbital Electron Notations

Back 61

These notations give us a clearer idea
of what the expanded notation looks
like.

Front 62

e- Configuration Rules

Back 62

Electrons MUST occupy the orbitals of
lowest energy first

Front 63

Filling the sub-orbitals

Back 63

There are many locations that
electrons might fill in an atom, the most
stable condition exists when they fill
the lowest available energy orbitals
first.

Front 64

Abbreviated Expanded
Configurations

Back 64

Using an abbreviated notation allows us to
add on extra electrons to an already
perfectly filled expanded notation.

Front 65

Quantum Numbers

Back 65

n, L, m, s

Front 66

The first: “principle quantum number” = “n”

Back 66

It is the same as the number of the energy level that contains the electrons

Front 67

The second: “sublevels” = “L”

Back 67

Sublevels are described by using the number of the principal energy level together with the letter designation of each sublevel.

Front 68

The third: “sublevel orientations” = “m”

Back 68

Relates to the orbitals in the sublevels and their
orientations (orbitals)

Front 69

The fourth: “spin of an electron” = “s”

Back 69

This number indicates that each orbital
can contain two electrons spinning in
opposite directions.

Front 70

Lewis Dot Structures

Back 70

Lewis Dot Structure, or Electron Dot
Diagrams, are drawn using the
valence number of electrons.

Front 71

Light

Back 71

An electromagnetic wave is depicted as a
sine wave that has an amplitude,
wavelength, and frequency.

3.00 x 108 ms-1

Front 72

Electromagnetic Spectrum

Back 72

Electromagnetic radiation comes in a broad range of frequencies call the electromagnetic spectrum.

Front 73

Planck’s Constant

Back 73

Energy of a photon = E= hν
h is Planck’s constant (6.626 x 10-34 J s)

Front 74

History of Atomic Emission

Back 74

Bohr found that electrons, in atoms, exist in
different levels (orbitals) – Energy increased the farther the energy
level is from the nucleus

Front 75

Ground State

Back 75

When the electron has its lowest
possible energy

Front 76

Excited State

Back 76

Excitation of the electron by absorbing energy raises the atom from the ground state to an excited state

Front 77

RADIOACTIVITY

Back 77

the process by which nuclei emit particles and rays

Front 78

RADIATION

Back 78

the penetrating rays and particles emitted by a radioactive source

Front 79

Radioactive Decay

Back 79

An unstable nucleus releases energy by emitting radiation

Front 80

Nuclear Stability and Decay

Back 80

The nuclear force is an attractive force that acts between all nuclear particles that are extremely close together, such as protons and neutrons in a nucleus.

Front 81

Band of Stability

Back 81

A nucleus with too many neutrons relative to the number of protons will undergo Beta Decay.

Front 82

Alpha Radiation

Back 82

Consists of helium nuclei that have been emitted from a radioactive source. These emitted particles, called alpha particles. they least penetrating.

Front 83

Beta Radiation

Back 83

An electron resulting from the breaking apart of a neutron in an atom

Front 84

Gamma Radiation

Back 84

High energy photon emitted by a radioisotope They are the most penetrating

Front 85

Positron Decay

Back 85

A particle with the same mass as the electron but opposite charge

Front 86

Transmutation Reactions

Back 86

The conversion of an atom of one element to an atom of another element

Front 87

Natural Transmutation

Back 87

When radioactive elements spontaneously decay over a long period of time and transform into other more stable elements

Front 88

Artificial Transmutation

Back 88

Human made reactions in which a nucleus is bombarded with a high speed particle which causes the nucleus to emit a proton or neutron

Front 89

Half-Life

Back 89

The time required for one-half of the nuclei of a radioisotope sample to decay to products.

Front 90

Nuclear Reactors

Back 90

Use fission to produce useful energy Much of energy generated is in the form of heat A coolant fluid, usually liquid sodium or water, removes the heat from the reactor core. The heat is used to generate steam, which drives a turbine that in turn generates electricity.

Front 91

Nuclear Waste

Back 91

Fuel rods from nuclear power plants are one major source of nuclear waste

Front 92

Nuclear Fusion

Back 92

FUSION occurs when nuclei combine to produce a nucleus of greater mass. In solar fusion, hydrogen nuclei (protons) fuse to make helium nuclei and two positrons.