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8 GRADE PHYSICAL SCIENCE: 2 SEMESTER TEST OUTLINE
WAVES & SOUND
1) frequency: the number of waves produce in a given amount of time
a) SI unit hertz
2) Draw, label, and give an example of a transverse wave. (label: amplitude, wavelength, crest,
trough, rest position) light waves
crest
amplitude
------------------------------------------------------------------------ Rest Position
wavelength
trough
3) Draw, label, and give an example of a longitudinal wave. (label: wavelength, compression,
rarefaction) sound waves
compression
rarefaction
wavelength
4) mechanical wave: a wave that requires a medium
5) electromagnetic wave: the process by which an electric current is produced by a changing
magnetic field does not require a medium
6) sonar: the use of reflected sound waves to locate underwater objects
LIGHT
1) Light is an electromagnetic wave.
Does it need a medium to travel on? no
2) Draw, label and give one example for each section of the electromagnetic spectrum:
Frequency Increases
Wavelength Decreases
Radio
Microwave
AM/FM
Microwave
Oven
Infrared
Ultraviolet
Light in restaurants
keep food warm
Tanning
bed
X-ray
X-ray machine for
broken bones
Gamma Ray
Nuclear

Visible light spectrum
3) As wavelength decreases, frequency increases.
4) reflection:
occurs when light or any other wave bounces off an object.
5) refraction:
the bending of a wave as it passes at an angle from one medium to another.
6) diffraction:
the bending of waves around barriers or through openings.
7) lens: a curved transparent object that forms an image by refracting.
8) What is the difference between a convex and concave lens? A convex lens is wider in the
middle and makes the images appear larger and the concave lens is thinner in the middle
and makes the image appear smaller.
9) Draw and label the law of reflection.
CHEMICAL & PHYSICAL PROPERTIES/CHANGES
1) physical property: Matter can be observed or measured without changing the identity of
the matter. Example: color, state, odor, volume, mass
2) solubility: the amount of that substance that will dissolve in a given amount of solvent
3) chemical property: Describe a substance based on its ability to change into a new
substance with different properties. Example: flammable, reacts with oxygen
4) physical change: Change that affects one or more physical properties. It maintains its
original self. Example: breaking chalk, freezing water, cutting your hair
5) chemical change: Occurs when one or more substances are changed into entirely new
substances with different properties. Example: baking a cake, soured milk
THERMAL ENERGY
1) temperature: measure of the average kinetic energy of the particles of an object.
a) relationship between temperature and how fast the particles of an object are moving – the
faster the particles of an object are moving, the higher the temperature of the object.
b) Water boils at 100 0C
Water freezes at 0 0C
2) thermal expansion: increase in the volume of a substance due to an increase in
temperature.
3) Kelvin: the official SI unit of temperature
4) absolute zero: the lowest temperature on the Kelvin scale – 0 Kelvin
5) heat: the transfer of energy between objects that are different temperatures
6) thermal energy: the total kinetic energy of the particles that makes up an object.
a) What unit is thermal energy measured in? joules
7) thermal equilibrium: energy is transferred from the higher temperature object to the
lower temperature object until both objects reach the same temperature.
8) conduction:
contact.
transfer of the thermal energy from one substance to another through direct
a) give an example spoon touching bowl of soup & getting hot
9) conductor:
10) insulator:
11) convection:
substances that conduct thermal energy very well.
substances that do not conduct thermal energy very well.
the transfer of thermal energy by the movement of a liquid or gas.
b) give an example one heater located in deep end of pool warms entire swimming pool
12) radiation:
the transfer of energy through matter or space as waves.
c) give an example sunlight shines directly through window
13) thermal conductivity:
conducts thermal energy well
14) specific heat capacity: the amount of energy it takes to raise the temperature of
1 kg of the material 1o C
15) Use the table on page 256 to answer the following questions about specific heat:
d) list the 3 substances that heat the fastest: lead, gold and mercury
e) does copper or aluminum heat the slowest? Aluminum 899 because copper is 387
THE ATOM
1) atom: The smallest particle into which an element can be divided and still be the same
substance.
a) What charge does an atom have? (positive, negative, or neutral?) neutral
2) Which takes up more space in an atom? (nucleus or empty space) empty space
3) Define, give the charge, and location for the following:
a) protons: positively charged particles of the nucleus (+)
b) neutrons:
the particles of the nucleus that have no charge/neutral
c) electrons:
the negatively charged particles in atoms (-)
4) quarks: the smaller particles that make up protons and neutrons
5) nucleus: the tiny, extremely dense, positively charged region in the center of an atom –
made up of protons and neutrons
What is the charge of the nucleus? Positive
6) electron energy levels: any of several different regions in which electrons travel about the
nucleus.
a) maximum # of electrons on the first 3 energy levels:
st
1
2
nd
2
8
rd
3
18
b) Draw a Bohr diagram for an atom that has 11 electrons:
c) List the valence electrons for the Bohr model you drew 1
7) valence shell:
the outermost energy level of an atom
8) valence electrons:
electrons in the valence shell
9) atomic number:
the number of protons in the nucleus of an atom
10) mass number:
the sum of the protons and neutrons in an atom
11) isotope: atoms that have the same number of protons but have different numbers of
neutrons
12) Find the following:
a) mass number
11
11
3+
B
b) protons
5
c) neutrons
6
5
d) electrons (with the charge) 2
ATOMIC SCIENTISTS
What is the theory of each atomic scientist:
1) John Dalton: all substances are made of atoms & elements combine
2) JJ Thomson: theory of “plum-pudding” models-small particles are inside the atom.
3) Ernest Rutherford:
empty space
4) Neils Bohr:
there is a small positively charged nucleus & atoms have mostly
electrons travel in definite paths
5) Schrodinger & Heisenberg:
electrons are found in electron clouds
PERIODIC TABLE
1) The Periodic Law:
the law that states that the chemical and physical properties of
elements are periodic functions of their atomic numbers
2) Sections of the periodic table
a) groups: (have the most properties in common)
i) name 1 element in group 16: sulfur
b) periods:
horizontal row of elements (from left to right) on the periodic table
i) name 1 element in period 4: calcium
c) metals:
found to the left of the zigzag line, solid at room temperature, good
conductors, shiny and malleable
i) name 1 element that is a metal: iron
d) nonmetals:
found to the right of the zigzag line, most gases at room temperature, not
malleable or shiny, poor conductors
i) name 1 element that is a nonmetal: carbon
e) metalloids:
also called semiconductors, found at the border of the zigzag line, have
properties of both metals and nonmetals
i) name 1 element that is a metalloid: boron
3) Use the periodic table on pages 304 – 305 to complete the following:
a) The name for Na is
sodium
b) Mercury has an atomic mass of
200
c) The chemical symbol for gold is
Au.
d) Halogens require how many electrons to fill their outer shell? 1 What group? 17
e) Group 18 is non-reactive… Why? outer shell is completely full (has 8)
f) Groups 1 and 2 are non or very reactive?
Very reactive
4) The current periodic table is arranged by atomic number
5) Draw dot diagrams for elements 1-10:
H
He

Li 
Be


B


C

 
N
 

 

 
  O   F   Ne 
6) What family is neon in? Noble Gases Give one fact about the family.
Their atoms have 8 electrons in their outer valence shell
7) Name one element in the alkali metals:
Li
Lithium
ELEMENTS, COMPOUND & MIXTURES
1) element: a pure substance that cannot be separated or broken down into simpler
substances by physical or chemical means.
a) give an example
2) compound:
combined.
Carbon
is a pure substance composed of two or more elements that are chemically
a) give an example NaCl = Sodium + Chlorine = Sodium Chloride
3) mixture:
is a combination of two or more substances that are not chemically combined
b) give an example
pizza
4) How are elements and compounds similar? Each has its own physical properties such as
boiling point, melting point, density and color
5) How are compounds and mixtures similar? 2 or more elements join together
CHEMICAL BONDS & COMPOUNDS
1) Atoms bond by _________, ___________, or ______electrons.
sharing
2) ionic bond:
gaining, losing, or
the force of attraction between oppositely charged ions.
3) ions: charged particles that form during chemical changes when one or more valence
electrons transfer from one atom to another.
4) covalent bond: the force of attraction between the nuclei of atoms and the electrons
SHARED BY THE ATOMS.
5) molecule:
a NEUTRAL group of atoms held together by covalent bonds
6) binary compounds:
a combination of two elements
a) give one example of using the criss-cross method to make a binary formula
Fe 2+
O 3-
2+
3-
2+
3-
Fe
O
Fe
O
Equals: Fe3O2
CHEMICAL REACTIONS & EQUATIONS
1) How many atoms of each element are in the following chemical formula?
2H2SO4 = 4 hydrogen atoms, 2 sulfur atoms, and 8 oxygen atoms
2) Is the following equation balanced or unbalanced? (show work)
potassium
chlorine
oxygen
2KCl + 3O2 ----------- 2KClO3
2
2
2
2
6
6
= a balanced equation
a) Label your reactants and products reactants – potassium (K), chlorine (Cl),
and oxygen (O); products – 2KClO
3) Law of Conservation of Mass:
In a chemical reaction, no mass is lost or gained
a) How does a balanced equation illustrate this law? Even though a chemical reaction
has taken place, both sides of the equation retain the same number of atoms.
TYPES OF REACTIONS
1) synthesis:
compound
a reaction in which two or more substances combine to form a single
2) decomposition:
A reaction in which a single compound breaks down to form two or
more simpler substances
3) single replacement: A reaction in which an element takes the place of another element
that is part of a compound.
4) double replacement: A reaction in which ions in two compounds switch places.
5) endothermic:
A chemical reaction in which energy is absorbed.
6) exothermic:
A chemical reaction in which energy is released or removed
7) List the 4 clues that a chemical reaction is taking place.
1) The formation of gas bubbles
2) The formation of a solid in a solution
3) Color change of the substance
4) The release of energy in any form (light, thermal, etc.)
ACIDS & BASES
1) Acid: any compound that increases the number of hydrogen ions which dissolved in
water (pH scale: 0 – 6.9)
a) example: lemon
2) Base: any compound that increases the number of hydroxide ions when dissolved in
water (pH scale: 7.1 – 14)
a) example: baking soda
3) Neutralization:
3) Indicator:
a chemical reaction between an acid and a base. (PH scale: 7)
an organic compound that changes color in an acid or base
a) give an example of one indicator and how it indicates an acid
or a base: red cabbage juice turns litmus paper pink or red if
an acid and blue/green or yellow if a base
4) pH Scale:
A scale that ranges from 0 to 14 to determine pH
ACIDS 0 – 6.9
NEUTRAL 7
BASES 7.1 – 14
a) draw and label (3 acids/3 bases)
0

1 2
 
stomach
acid
(1)
3
4
5
6
7
8
9
10


   
  
lemon coffee
water
baking
juice
(5)
(7)
soda
(3)
(9)
b) What is the pH of a neutral compound?
7
11

12

bleach
(12)
13
14


oven
cleaner
(13)