Physical Science Final Review
Earth Science
Chapter 28: Earthquakes
Fault: break in the earth’s crust along a
transform boundary
Plate Boundaries: boundaries along
which plates collide
Transform: plates boundaries slide past
Convergent: plate boundaries collide
Divergent boundaries: plate boundaries
separate
Relative dating: a way to put events in
order of which they happened: crosscutting, inclusions, original
horizontality, lateral continuity,
fossils(faunal succession), superposition
Fossil: remains of prehistoric life
Tsunami: underwater earthquakes,
volcanic eruptions or landslides cause
violent displacement of the sea floor
Kinetic energy: energy of motion
(movement)
Potential energy: stored energy
Epicenter: the point on the surface
directly above the focus
Focus: exact point below the surface
where the earthquake started
Richter Scale: measures the amount of
energy released using a scale of 1-10
P-waves: are the first waves to arrive at a
seismograph station. Are the fastest form
of wave, sometimes called compression
waves
S-waves: arrive after the primary waves
at the seismograph station. Can travel
through solids but not liquids
Plate Tectonics: theory of plate
movement that explains the formations
of mountains, ridges, earthquakes,
volcanoes, trenches, etc
Trench: feature where oceanic and
continental crust converge
Mid-ocean Ridge: largest ridge in our
lab created by divergent plate boundaries
Geological time scale: Earth’s history
divided into eras
What is Pangaea & evidence for Pangaea?
 Pangaea is the theory that all continents were once part of a single land mass
o Ocean ridge rocks are younger than the surrounding ocean rock
o The continents appear to fit together
o Rock & fossil correlation is found where the continents appear to fit
together
What feature is found where oceanic and continental crust converge?
• Subduction: oceanic plate dives below the continental crust
• A deep oceanic trench marks the boundary between a subducting and an
overriding plate at a convergent boundary.
What feature is found where continental plates converge?
 Mountains or mountain chains
How many seismograph stations are needed to locate an epicenter?
 3
A 436g sample of a radioisotope has a half-life of 3.4 days. How much of the sample
will remain after 17.0 days?
 5 half lives
 436g  218g 109 g  54.5 g  27.25 g  13.625g = 14g
How much of a 352g sample of a radioisotope will remain after 4 half-lives?
 352g  176g 88 g  44 g  22g = 22.0g
After 18 days the radioactivity of a sample decreases from 2500 counts to 625 counts.
What is the half-life of this sample?
 2500c  1250c 625c = 2 half lives
 18days / 2 half lives = 9days / 1 half life
The half-life of a radioisotope is 2.6 days. What time must elapse for the radiation to be
reduced to 12.5% of its original level?
 100%  50% 25%  12.5% = 3 half lives
 3 half lives x 2.6 days
_______ = 7.8 days
1 half life
Chapter 29.3: Rocks & Minerals:
Relative Dating
Concepts:
Understand how to identify a mineral, igneous rock, sedimentary rock, or metamorphic
rock.
Igneous rock – may be frothy, glassy, show conchoidal fracture, formed from lava
or magma cooling
Sedimentary – formed by cementation and compaction, may have fossils or clasts
Metamorphic – formed by heat and pressure, may have foliations
Mineral – “pure” inorganic substance, building blocks of rocks
What is the difference between a mineral and a rock?
Mineral is a solid, naturally-occurring object with a defined chemical
composition, inorganic and has a crystalline structure.
Rock is a naturally formed consolidated solid mixture containing minerals, rock
fragments, or volcanic glass
What do you use to identify a mineral?
Physical Properties:
 Cleavage
◦ Minerals break along planes that cut across relatively weak chemical
bonds, a smooth, flat surface is created.
◦ Most minerals (except metals) have one or more cleavage planes that also
help in determining their identity.
 Fracture
◦ irregular break
◦ Some minerals do not split along well-defined flat surfaces.
◦ In such cases, a mineral will break unevenly.
 Hardness
◦ The physical property that measures resistance to scratching
◦ Mohs Hardness Scale
◦ developed in 1812 by Friedrick Mohs (an Austrian mineral expert) as a
method to identify minerals.
◦ Identify a mineral’s place on the hardness scale by whether it can scratch
another mineral
 Luster
◦ The way a mineral reflects light is the physical property known as luster.
◦ Metallic and nonmetallic.
◦ Metallic luster minerals reflect light in a way that a metal surface might.
◦ Nonmetallic luster, includes minerals that shine like glass or appear earthy
or waxy.
 Streak
◦ The color of mineral in powdered form is called streak.
 Crystal Shape
◦ The orderly internal arrangement of atoms in a mineral often is indicated
by its external crystal shape.
What do you use to identify an igneous rock?
 Igneous
◦ - crystals intersecting at angles
◦ -size of the grain
What do you use to identify a sedimentary rock?
◦ -layers of rock pieces
What do you use to identify a metamorphic rock?
◦ -pressure created results in lines
◦ -pressure and heat create grains in foliation (wavy patterns)
◦
-hardest of the 3 rocks
Know the difference between intrusive & extrusive. Include temperature, time, and grain
size.
◦ Intrusive Igneous rocks
 Formed from magma which cools and solidifies below Earth’s
surface
 Cooling and solidification take a long time resulting in large
visible crystals
 Coarse-grained like granite
 Granite is mostly found in the continents
◦ Extrusive Igneous rocks
 Formed from lava on or above Earth’s surface
 Cooling and solidification takes place relatively quickly resulting
in very small crystals
 Fine-grained like basalt
 Basalt is in the ocean floor
Identify and define the different types of relative dating techniques. (Superposition,
original horizontality, inclusions, faunal succession, intrusive relationships, lateral
continuity.)
Superposition – older layers on bottom, youngest layers on top
Original Horizontality – sediment forms horizontal layers
Inclusions – rocks (clasts) included in a rock are older than the rock around them
Faunal Succession – Fossils included in rock layers are the same age as the rocks
they are in.
Intrusive relationships – veins of rock and faults are younger than the rock they
cut through.
Lateral continuity – rock layers extend in all directions until they are disturbed by
another formation.
Chapter 24 & 26: Atmosphere & Water Cycle
Barometer: instrument to measure
pressure
Conduction: transfer of heat by direct
contact
Convection: transfer of heat through a
medium or indirectly
Transpiration: water released into the
atmosphere from plants (evaporation of
water from plants)
Evaporation: water molecules speed up
enough to break bonds and phase change
into a gas.
Run off: water that flows over land
before reaching surface water
Ground water: water that collects
underground
Clouds: place where condensation
occurs
Condensation: vapor molecules lose
kinetic energy, slow down, reform bonds
and phase change to a liquid
Energy: comes from the sun in order to
keep the water cycle going, light & heat
in the form of radiation
Know the diagrams of the water cycle. The diagram we took a quiz on & took notes on is on the
final.
Where does the majority of water come from?
 oceans
Why is the water cycle necessary?
 There is very little water that is good for drinking
What happens to pressure as you increase altitude?
 Pressure decreases
What are the most prevalent gases in the atmosphere from greatest to least?
 Nitrogen, Oxygen, Hydrogen, water vapor
What human activity has increased carbon dioxide most in the atmosphere?
 Fossil fuels (other contributors are pollution & refridgerants)
List the layers of the atmosphere from closest to the earth to outer space?
Troposphere
Tropopause- boundary
Stratosphere
Stratopause- boundary
Mesosphere
Mesopause- boundary
Thermosphere
Chapter 27: Weather
Coriolis Effect: The bending of air currents due to the Earth’s rotation
Relative Humidity: amount of water vapor in air compared to maximum amount air can hold
Sling psychrometer: measures relative humidity
- 2 thermometers
- 1 wet-bulb (wet cloth)
- 1 dry-bulb
- wet bulb: water evaporates from cloth shows ↓ cloth
- dry bulb: temperature does not change
- air is dry water evaporates quickly, difference between wet and dry bulb is large
- air has a large water amount – little water evaporates from wet bulb; difference is small
- no evaporation- same temperature
*difference indicates the amount of water vapor in air.
Absolute Humidity: - measure of amount of water vapor in air & measured in grams per cubic
meters (g/m3)
- airs ability to hold water vapor depends on temperature of air
- temperature ↑ capacity for water vapor ↑
Why does Earth have seasons?
 Earth is tilted on its axis which allows one hemisphere to get more radiation from the
sun than the other hemisphere- thus changing the weather & giving us seasons.
What happens to the sun’s radiation in our atmosphere?
 Some of the radiation is absorbed in the form of light and heat (which helps us to
thrive)
 Some is reflected (emitted) out back into space as infrared radiation or heat.
Read a relative humidity chart.
Chemistry
Atom: smallest unit of matter that cannot be
easily broken down
Electron: Tiny negatively charged particle
attracted to the positive charges in the
nucleus.- a lot of volume
Proton: protons are positively charged and
very close together in the nucleus- a lot of
mass
Neutron: Neutrons make the nucleus more
stable by adding to the strong nuclear force,
without adding positive, repulsive charges - a
lot of mass
Compound: two different atoms that are held
together by a strong or weak chemical bond
Chemical Formula:
Element: one type of atom (matter)
Molecule: two or more atoms that are held
together by a strong chemical bond
Ion: charged particle or atom (b/c lost or
gained electrons)
Reactants:chemical compounds that are
combined (left side of the arrow)
Products: the resultant chemical compounds
(right side of the arrow)
Isotope: atoms of the same element that have
different numbers of neutrons.
Anion: gains electrons & negatively charged
ion
Cation: loses electrons & positively charged
ion
Ionic: metal bonds nonmetal
Covalent: nonmetal bonds nonmetal
Acid: starts with hydrogen H1+
What properties do solids, liquids, and gases have?
 Solids:
o A solid retains its volume and shape.
o Vibrate
o Least Kinetic Energy
 Liquids:
Binary Acid: hydrogen & one other element
(no oxygen)
Oxyacid: hydrogen & polyatomic
Coefficients: make the total number of atoms of
each element the same for the reactants as for the
products
Physical Change: any change that does not
affect the identity of the atoms or molecules in
the material
Chemical Change: results in the formation of
new molecules as atoms are rearranged
Mixture: contain more than one kind of
matter and can be separated by physical means
Substance: material composed of only one
type of molecule (pure) &cannot be separated
into different kinds of matter by physical
means
Homogenous: mixture is the same throughout
Heterogenous: mixture has visibly different
substances throughout.
Valence electron: outer shell electrons in “s”
& “p” columns
Octet Rule: all elements want 8 valence shell
electrons (Noble Gas Wannabe’s)
Strong Nuclear Force: Attractive force
between any two nuclear particles (protons,
neutrons), Only acts over a very short distance
& Overcomes the repulsive force between the
positive protons
Mass Number: The total number of protons
and neutrons in the nucleus
Atomic mass: Average mass of protons and
neutrons combined. atomic mass units
(amu)

o
o
o
Gases:
o
o
o
o
A liquid has a definite volume, but no definite shape.
Liquids flow to take the shape of the container.
vibrate, rotate, translate
A gas has no definite volume or shape.
Gases expand to fill their containers.
vibrate, rotate, translate
Most Kinetic Energy
List the states of matter in order of their kinetic energy from least to greatest.
 Solids  liquids  gases  plasma
Know the heating and cooling curve & Phase Diagram.
-Know how to write chemical compound names and chemical formulas.
CO carbon monoxide
calcium iodide CaI2
CO2 carbon dioxide
hydrogen chloride HCl
nitrogen dioxide NO2
HBr(aq) hydrobromic acid
N2O4 dinitrogen tetraoxide
hydrogen sulfide H2S
dinitrogen pentaoxide N2O5
Na2O sodium oxide
PbO lead (II) oxide
magnesium nitride Mg3N2
lead (IV) oxide PbO2
calcium phosphide Ca3P2
sulfur dioxide SO2
aluminum carbide Al4C3
SO3 sulfur trioxide
LiH Lithium Hydride
BCl3 boron trichloride
magnesium sulfide MgS
iron (II) chloride FeCl2
copper (I) oxide
HI(aq) hydroiodic acid
Hydronitric acid
H3PO3 phosphorous acid
Chlorous acid
H3PO4 phosphoric acid
Sulfurous acid
Cu2O
H3N(aq)
HCLO2
H2SO3
HCl(aq) hydrochloric acid
Hydrofluoric acid HF(aq)
FeCl3 iron (III) chloride
copper (II) oxide CuO
KBr potassium bromide
MnF7 manganese (VII) fluoride
-Know how to balance equations and how to identify their “type”.
_2_ZnS + _1_O2
_1_Li2O
+
_1_C3H8
+ _5_O2
→ _2_ZnO + _2_S
_1_H2O →
→
_2_H2O + _1_ CH4
_3_CaO + _2_Al
_2_LiOH
_4_H2O
Synthesis
+ _3_CO2
→ _4_H2 + _1_CO2
→
Single Replacement
_1_Al2O3 + _3_Ca
_______________
Combustion
(not one we looked at)
Single Replacement
Name indicators of a chemical change.








Formation of a Precipitate – insoluble solid
Exothermic Reaction - Increase in temperature
Formation of a gas without heating
Endothermic Reaction - Decrease in temperature
Change in color
Evolution of Light without heating
Change in smell
Change in taste
What is a physical change and give an example of one?
 Any change that does not affect the identity of the atoms or molecules in the material
o Bending, Phase changes, breaking, heating, etc
Identify the following as physical or chemical changes:
Paper tearing
Wood burning
Ice melting
Water boiling
Reheating leftover food
Digesting food
physical
chemical
physical
physical
physical
chemical
Study hard and then have a great summer!!!!!!!!!