Integrated Science Midterm(Chem/sci. Method) 9Th Grade

Front 1

Metals

Back 1

Have1-3 e- in their valence shell. they give away electrons

Front 2

Isotope

Back 2

Atoms of the same element that have diff. mass# and the sme chemical properties

Front 3

Octet Rule

Back 3

All atoms except (H and He) 8 Electrons in valence shell H and He prefer 2.

Front 4

Ionic Bond

Back 4

Attractive force between two ions with opposite charge

Front 5

Fission

Back 5

splitting of an atomic nucleus into 2 smaller nuclei w/2 release of energy

Front 6

Fusion

Back 6

When 2 atoms are combined to form one larger atom W/energy released. Heat & pressure increase. H Bomb/stars

Front 7

Formula for fusion

Back 7

Hydrogen combines
H1 + H1 = He2

Front 8

Formula for fission

Back 8

235 U + 1/on--- 92Kr Ba+ 3 1/0 n + energy

Front 9

Uses for fission

Back 9

Nuclear Power Plants
Atomic Bomb

Front 10

Uses for fusion

Back 10

H Bomb Sun

Front 11

Nuclear power plant

Back 11

Uses Uranium and fission to create electrical energy

Front 12

Isotope

Back 12

Atoms of the same element that have diff. mass # and the same chemical properties.

Front 13

Uses of radioactive isotopes

Back 13

Study living organisms to diagnose and Treat disease- sterilize

Front 14

Alpha particle

Back 14

4He
2

Front 15

Beta Particle

Back 15

A high speed electron is shot out of the nucleus changing the atomic # to 1 higher(indicating radiation)

Front 16

Example of Beta Decay

Back 16

14 14
C N
6 9 Stable 7P 7N

Front 17

Half Life

Back 17

Time it takes for 1/3 of a sample of radioactive material to decay to another nuclide

Front 18

Radioactive fallout

Back 18

Clouds of fine dust radioactive particles from bomb debris that falls back to earth.

Front 19

Nuclide

Back 19

Naced nucleus- Nucleus with no electron

Front 20

Decay Series

Back 20

Steps it takes to become
non-radioactive- Stable 83 and below

Front 21

Binding energy or

Back 21

The huge amount of energy that holds protons together in nucleus

Front 22

Transmutation

Back 22

Change across

Front 23

Gamma Radiation

Back 23

y- waves of pure energy that travel at the speed of light. Electromagnetic energy

Front 24

Time Distance and shielding

Back 24

Speed of light

Concrete or lead shelilding

Front 25

What materials stop which radiation Particles?

Back 25

Alph-Paper
Beta-Aluminum 1 centimeter thick
Gamnma-concrete or lead

Front 26

Scientific method

Back 26

Planned organized approach of solving a problem

Front 27

Indeptndent varialbe

Back 27

in an experiment is the factor that is the manipulated by the experimentor.

Front 28

Dependent variable

Back 28

Is a factor that can change if the independent variable is changed

Front 29

Control Group

Back 29

It does not receive the independent variable

Front 30

Experimental group

Back 30

The group affected by the independent variable. the group receiving a different treatment

Front 31

Metals

Back 31

have 1-3 e- in thir valence shell. They give away electrons

Front 32

Metalloid

Back 32

Resembling or alike a metal. the elements towards the right of the the periodic table.

Front 33

Neutral atom

Back 33

Atom w/no charge because it has the same # of protons

Front 34

Inert Element

Back 34

An atom of an element that has as many valence electrons as its outer most shell can hold.

Front 35

Radioactive elements

Back 35

Elements that are chemically unstable and give off radiation.

Front 36

Non-metals

Back 36

Elements that don't have most of the properties of metals

Front 37

Period

Back 37

The horizontal rows on the periodic table.

Front 38

Group or family

Back 38

The verticle rosw on the periodic table with atoms that have a similer physical and chemical characteristics.

Front 39

Atomic Mass

Back 39

The average number of protons and neutrons of the isotopes of an element.

Front 40

Atomic Number

Back 40

The number of protons in the nucleus of an atom.

Front 41

Proton

Back 41

A tiny atomic particle in the nucleus of an atom with mass and a positive charge.

Front 42

Neutron

Back 42

A tiny atomic particle in the nucleus of an atom that is electricaly neutral and has about the same mass as a proton.

Front 43

Electron

Back 43

A tiny atomic particle in the energy levels of an atom with little mass and a negative electral charge.

Front 44

Ion

Back 44

An electricaly charged atom or group of atoms with an uneven number of protons and neurons.

Front 45

Neutral atom

Back 45

An atom without a net charge and an equal number of protons and neutrons.

Front 46

Chemical Reaction

Back 46

The change of one or more substances into other substances.

Front 47

four ways you can tell a chemical reation is occurring

Back 47

Energy is released, a new substance is formes, light is released, or a chnge of color.

Front 48

As you go down the periodic talbe what is added

Back 48

Energy levels

Front 49

Atom

Back 49

The smallest particle of an element that has all of the characteristics of an element.

Front 50

Compound

Back 50

A sustance composed of two or more molecules.

Front 51

Diatomic molecule

Back 51

2 or more atoms of the same element that combine naturally.

Front 52

Particles in the nucleus

Back 52

protons and neutrons exist in one nucleus of an atom.

Front 53

Particles in the orgitals or shells

Back 53

Electrons are in the orbitals or shells of an atom

Front 54

Reactant

Back 54

The molecules to the left of the arrow when balancing equations.

Front 55

Product

Back 55

The molecules to the right of the arrow when balancing equations

Front 56

Subscript

Back 56

The number to the lower right of an element that tells how many atoms there are of that element.

Front 57

Coefficient

Back 57

The number in front of a molecule that tells the number of molecules that you have.

Front 58

Ionic bonds usually form between

Back 58

2 ions of opposite charge

Front 59

Covalent bonds

Back 59

Bonds formed when 2 or more atoms share electrons with each other, forming a molecule.

Front 60

covalent bonds usually form between

Back 60

2 or more atoms that need to become inert

Front 61

Bohr model

Back 61

Draw a bohr model for carbon

Front 62

Lewis Dot

Back 62

Draw a lewis dot for carbon

Front 63

Valence Electrons

Back 63

the electrons in the outer enery level of an atom that participate in a chemical bonding.

Front 64

Positive Ion

Back 64

An ion with more protons then eletrons because it lost some electrons to become an ion

Front 65

Negative ion

Back 65

an ion with more electrons then protons becuase it gained some electrons to become an ion.

Front 66

Control factors

Back 66

the variable that do not change

Front 67

continuous data

Back 67

Used in a line graph

Front 68

Discontinuous Data

Back 68

Used in a bar or pie graph.

Front 69

Raw Data

Back 69

The numbers without being put into graphs/ can be measured

Front 70

Derived dat

Back 70

Mathmatically calculated not measured

Front 71

Bar graph (when used)

Back 71

For discontinous data when x and y are the same

Front 72

Line graph ( when used)

Back 72

Discontinous data relative . Shows how part is relative to the whole.

Front 73

Advantages of using a data table

Back 73

1.Can see the numbers froe easily
2. Organization

Front 74

Column

Back 74

Vertical

Front 75

Row

Back 75

Horizontal

Front 76

Hypothesis

Back 76

an educated guess; neither right or wrong

Front 77

Interpolation

Back 77

prediction using info/ measurements from existing points

Front 78

Extrapolation

Back 78

predictions of info/measurements from beyond the exiting points.