Name ____________________Answer Key__________________
Period _________
Date ______________
Physical Science – 2nd Semester – Final Exam Study Guide – (2012-2013)
1. Physical Science Basics
a. What tool(s) would you want to use to find the:
i.
Mass of an object? ________Triple Beam Balance______________________ Basic SI Unit? _____g____
ii.
Volume of an object? ________Graduated Cylinder or Ruler_____________ Basic SI Unit? __L –or- cm³_
iii.
Length of an object? ________Ruler or Meterstick____________________ Basic SI Unit? ____m_____
iv.
Density of an object? ________Triple Beam Balance & Ruler________
Basic SI Unit?_g/L –or- g/cm³
b. What is the formula for calculating density? _________Density = mass / volume or D=m/v_______________
i.
What is the density of a cube that is 15 g and has a volume of 3 cm3? __15g / 3cm³ = 5 g/cm³_____
ii.
Compare the density of solid H2O to liquid H2O, and explain what observable effect this has.
Solid water has a lower density than liquid water, and so solid water (ice) floats in liquid water!
2. Chemistry Basics
a.
b.
c.
d.
Element (def.) The building block of all matter; made up of only one type of atom
Atom (def.) The smallest part of an element that still has the properties of that element
Compound (def.) A substance made up of two or more DIFFERENT atoms bonded together
Molecule (def.) A substance made up of two or more atoms bonded together
3. Model of the Atom: Evolution of the Atomic Theory
Atoms are so small that many scientists throughout history have created _____models_______ to describe them.
Why have atomic theories changed over time? _____The advancement of new technologies________
Scientist
Year
John Dalton
(1)
J.J. Thomson
(2)
Niels Bohr
(4)
Ernest Rutherford
(3)
Major Discovery/Contribution
The Atomic Theory: Provided evidence
that atoms were the smallest thing in
the universe; atoms of the same
element were the same, while atoms of
different elements were different
Cathode Ray Gun:
Discovered the electron
Discovered that elements gave off light
energy when electrons jumped from
orbital to orbital
Gold Foil Experiment: Discovered the
dense, positively charged nucleus
surrounded by empty space
Name of atomic model
Billiard Ball Model
Plum Pudding Model
Bohr Model
Planetary Model
4. Periodic Table
a. The current periodic table is arranged by increasing ________Atomic Number_______.
b. Reading the Periodic Table
i.
An element’s ___Physical and chemical properties____ can be predicted from its location in the
periodic table.
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ii.
iii.
iv.
v.
vi.
vii.
The atomic number represents the number of ___protons____.
The atomic mass represents the number of _____protons and neutrons in the nucleus____.
The atomic symbol represents ____the name of the element______.
The group/family number represents ____the number of valence electrons______.
The row/period number represents _____the number of orbitals____.
This group contains the most elements: ___Transition Metals____.
c. Matching Word Bank: Metalloid, transition element, metal, non-metal, group 18- noble gases, group, group 1
The most stable elements are found here. They are colorless tasteless gases that glow when
Group 18 – Noble
an electrical current passes through them.
Gases
Elements that share some properties with metals, and some with non-metals.
Column of elements in the periodic table that have similar physical or chemical properties.
The most reactive elements in the periodic table, and are soft enough to be cut with a knife.
An element that has a shiny luster, is a good conductor of heat and electricity, is malleable
and ductile.
Elements in groups 3-12
Element that is usually a gas or brittle, solid at room temperature, and does not conduct
heat and electricity well.
Metalloids
Group
Group 1 – Alkali
Metals
Metal
Transition Metal
Non-metal
5. Parts of an Atom
Valence Electron
Neutron
Proton
Charge
Location in the
atom
Proton
Positive
Nucleus
Electron
Negative
Electron
Cloud/Orbital
Neutron
Neutral
Nucleus
Nucleus
Positive
Center of Atom
Subatomic Particle
The atom shows to the left has __7__ valence electrons.
This atom has __7__ electrons that would be involved in bonding.
Krypton is located in group 18. It has __8__
valence electrons, which is the most that any element can have.
Krypton’s atomic number is 36 and its atomic mass is 84. It has _36_ protons, _48_ neutrons, and _36_ electrons.
6. Properties of Atoms Gaining or Losing Electrons
a. An atom that has gained or lost an electron is called a(n) ___ion____
b. Group (# and name) ___Group 1 – Alkali Metals____ loses electrons most easily.
c. Group (# and name) ___Group 17 - Halogens___ gains electrons most easily.
i.
Elements in group 17 want to bond with elements in group _1 (Alkali Metals)_
ii.
Elements in group 16 want to bond with elements in group _2 (Alkaline Earth Metals)_
d. The charge becomes positive when what has happened? _atoms lose electrons_
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i.
What do we call a positively charged ion? _cation_
e. The charge becomes negative when what has happened? _an atom gains electron_
i.
What do we call a negatively charged ion? _anion_
f. An ionic bond is an attraction between what charges? _Oppositely charged ions_
7. DNA
a. TRUE / False. All things, living and non-living are made up of atoms.
b. Macromolecule (def.) _A large molecule made up of thousands of atoms_
c. List the 5 elements that make up the DNA macromolecule: *REMEMBER TO “CHONP” 
1). _Carbon_; 2). _ Hydrogen _; 3). _ Oxygen _; 4). _ Nitrogen _; 5). _ Phosphorous_
8. Chemical Bonding
a. Ionic bond
i.
Metal / non-metal and metal / non-metal bonded together
ii.
Protons / neutrons / electrons are shared / transferred
iii.
Draw how Aluminum and Oxygen would ionically bond (using arrows). 
b. Covalent bond
i.
Metal / non-metal and metal / non-metal bonded together
Al2+3O3-2
ii.
Protons / neutrons / electrons are shared / transferred
iii.
Draw the structural and Lewis structure for Carbon tetrachloride. 
c. Classify the following compounds as ionic or covalent, then name them accordingly:
i.
KCl
_ Ionic_
_ Potassium chloride__
ii.
CO2
_ Covalent_ _ Carbon dioxide_
iii.
CaF2
_ Ionic__
_ Calcium fluoride_
CH4 or
iv.
P2O5
_ Covalent_ _ Diphosphorous pentoxide_
Methane
9. Naming Chemical Formulas
a. H2O is the molecular formula for _water_. The 2 means _2 atoms of hydrogen__; no number after the O
indicates _there is only one atom of oxygen_.
b. The molecular formula for oxygen gas is O2_.
i.
Oxygen is a diatomic molecule because _it is made up of 2 atoms_.
c. C6H12O6 is the chemical formula for _sugar_.
d. The chemical formula for methane is _CH4_.
10. Physical and Chemical Properties and Changes
a. Identify the following as either being a physical property or a chemical property:
i.
Flammability _Chemical property (Irreversible; DEF: the ability for something to catch on fire)_
ii.
Melting point _Physical property (Reversible; DEF: the point at which something melts)_
iii.
Color _Physical property (observe with the senses)_
b. Name a property that would describe salt. _Small, white, crystalline, salty_; Name a property that would
identify salt. _salty taste_
c. A chemical / physical change occurs when bonds are broken.
d. A chemical / physical change occurs when no new substance is formed.
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e. Physical change (def.) _Occurs when one or more physical properties of a substance are changed, is reversible_
i.
Name 3 examples of a physical change:
1. _melting_ 2. _ dissolving_ 3. _ boiling_
f. Chemical change (def.) _An irreversible change that occurs when chemical bonds break and new bonds form,
producing a new substance with new properties_
i.
Name examples of a chemical change:
1. _ Change in color_ 2. _ Change in odor_ 3. _ Production of light_ 4._ Emission of a gas_
5. _ Formation of precipitate_ 6. _ Release energy (Exothermic)_ 7. _ Absorb energy (Endothermic)_
ii.
Name 3 signs that a chemical change has occurred:
1. _ Burning_ 2. _ Cooking_ 3. _ Rusting_
g. Balancing Chemical Equations
i.
_2_ H2 + ____ O2  _2_ H2O
ii.
How does the Law of Conservation of Mass apply to the equation you balanced above? _Atoms are not
created or destroyed in the reaction. You must have the same number of atoms in the beginning of the
reaction as you do in the final product._
h. What forms of energy could be transferred in a chemical reaction? _ Radiant (Light)_ _ Heat_ _ (All others) _
i.
A change that gives off energy is called _Exothermic (think “EXit”)_ Ex. _Fireworks exploding_
ii.
A change that absorbs energy is called _Endothermic (think “ENter”)_ Ex. _Baking cookies_
iii.
True / False. Every chemical reaction involves a change in energy.
11. Mixtures
a. Heterogeneous (def.) _A mixture that is unevenly mixed; can see the different parts of the mixture_
i.
Name an example of a heterogeneous mixture: _Salad, concrete, M&M’s_
b. Homogeneous (def.) _A mixture that is evenly mixed; looks like the same substance_
i.
Name an example of a homogeneous mixture: _Kool-Aid, Salt-water_
c. Separating Mixtures: Name & give a brief description of the 5 physical methods to separate mixtures:
1. Magnetism _Separates objects with magnetic properties (those with Fe, Ni, Co)_
2. Filtration _Separates substances based on size_
3. Dissolving _Breaks down a substance and surrounds it_
4. Evaporation _Separates dissolved solute from a solution (Anything from water!)_
5. Chromatography _Separates different colored pigments and dyes based on filtration_
d. Solutions
i.
Solute (def.) _The substance found in the lesser amount; the substance that IS dissolved_
ii.
Solvent (def.) _The substance found in the greater amount; substance that DOES the dissolving_
iii.
Solubility (def.) _The ability for a substance to be dissolved_
iv.
In Kool-Aid, identify the solute _Kool-Aid Powder_ and the solvent _Water_
v.
True / False. Typically there is more solute than solvent in a solution.
vi.
True / False. Solutes and solvents can be solids, liquids, or gases.
vii.
True / False. When a salt dissolves in water, each of its particles is surrounded by water molecules. This
is why the freezing point of salt water is lower than the freezing point of fresh water.
12. Acids and Bases
a. Acidic solutions pH levels from _0_ to _6_; Taste _Sour_; Ex. _Lemon juice_
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i.
What can a substance do if it has a warning of “corrosive”? _It can eat away at other materials_
b. Basic solutions pH levels from _8_ to _14_; Taste _Bitter_; Ex. _Shampoo, soap, other cleaning supplies_
13. Phase Changes
a. The three main states of matter are:
b. Draw the molecular arrangement of each:
_ Solid_
_Liquid_
_Gas_
c. Label the Phase Change Diagram. Use arrows where necessary (phase transitions).
Solid (A)
Gas (E)
Liquid and Gas (D)
Melting (B)
Condensing (D)
Liquid (C)
Solid and Liquid (B)
Freezing (B)
Evaporating (D)
d. The average kinetic energy of the particles of a substance going through a phase transition can be described as
(circle all that apply): increasing / decreasing / staying the same.
e. Compare the amount of kinetic energy (motion) of the particles in a solid to a gas. _Atoms of a gas have more
kinetic energy than the atoms in a solid_
14. Types of Energy
a. Energy (def.) _The ability to do work or to cause change_
b. What does it mean if something has potential energy? _Energy is stored in an object_
i.
Example: _A stretched rubber band, a roller coaster on top of a hill_
c. When does an object possess kinetic energy? _An object in motion_
i.
Example: _A roller coaster moving down a hill_
d. Chemical PE (def.) _Energy stored in chemical bonds, that can only be released during a chemical reaction_
i.
Example: _ Fossil fuels (natural gas, coal, oil), food, batteries_
15. Energy Transformations
a. The law of conservation of energy states that when one form of energy is converted into another, _ energy
cannot be created or destroyed_
i.
True / False. Most forms of energy cannot be converted into other forms.
b. Natural gas (_ Chemical_ energy) heats (_ Thermal_ energy) water.
c. Batteries (_ Chemical_ energy) are used to turn on a flashlight (_ Radiant (light)_ energy).
d. You rub your hands together (_ Mechanical_energy) on a cold day and friction is created to produce heat (_
Thermal_ energy).
e. A microwave (_ Radiant_ energy) in a house turns on because of energy produced in a nuclear power plant
from an atom’s nucleus (_ Nuclear_ energy)?
f. A light bulb [visible light] (_ Radiant_ energy) turns on because of turning on the light switch (_ Mechanical_
energy)?
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g. Fossil fuels (_ Chemical_ energy) are burned, which is called combustion, and heat (_ Thermal_energy) is
released.
h. A spinning turbine (_ Mechanical_energy) produces usable energy to power homes (_Electrical_ energy).
16. Sources of Energy
a. Identify the following as being renewable or non-renewable:
i.
Biomass _ Renewable_
v.
Solar _ Renewable_
ii.
Coal _ Non-Renewable_
vi.
Nuclear _ Non-Renewable_
iii.
Petroleum _ Non-Renewable_
vii.
Hydroelectric _ Renewable_
iv.
Wind _ Renewable_
viii.
Geothermal _Renewable_
b. What part of the water cycle would not be possible without solar energy? _The Sun_
c. Nuclear Energy
i.
Energy stored in _the nucleus of an atom_
ii.
Nuclear Fission (def.) _When two or more smaller atoms fuse together_
iii.
Nuclear Fusion (def.) _When a large atom splits into two or more atoms_
iv.
True / False. Fusion releases 3-4 times more energy than fission.
v.
True / False. Only nuclear energy is produced in a nuclear reaction, not light or heat.
17. Heat Transfer
a. Conduction (def.) the transfer of heat energy between substances that are touching
i.
Example: molecule to molecule
b. Convection (def.) the cyclical motion of molecules in a gas or liquid caused by the transfer of heat through a
surface
i.
Example: Hot Air Balloon
c. Radiation (def.) Electromagnetic waves travel through space and transfer heat energy.
i.
Example: Microwave
d. Temperature (def.) The measure of the amount of kinetic energy in a substance.
i.
The scale to measure the amount of KE in the atoms of a substance: Celsius
e. Heat (def.) is the transfer of energy from an object with high molecular K.E., to an object with low molecular
K.E.
i.
Heat moves from a hotter object to a cooler object.
f. Insulator (def.) A substance that prevents or slows the flow of heat energy.
i.
Example: Rubber
g. Conductor (def.) substances that allow electrons to move freely across the surface of their atoms
i.
Example: _Metals_
18. Electricity
a. Static Electricity (def.) _ The build-up of charges on an object._
b. Static Discharge (def.) _Spark or shock; the loss of static electricity as electric charges move off an object in an
attempt to become neutrally charged._
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c. A _switch_turns a circuit on and off by opening or closing.
d. _Series_ circuits have one path, while
_parallel_ circuits have more than one path.
e. Circuits A & C are _Series_
f. Circuits B & E are _Parallel_
g. Electric currents always flow from the:
Negative to Positive
h. In a series circuit: finish the saying
“when one light bulb goes out…
they’ll all go out.”
i. In a series circuit: Adding another bulb will
_add resistance and make the lights dimmer_
j. True / False. In a parallel circuit, the current
from each bulb has its own path.
k. An electric current will always follow the path _of least resistance_.
19. Magnetism
Magnetism (def.) the force of attraction or repulsion of magnetic material.
Magnetism in a physical / chemical property.
Poles that attract are _opposite_; Poles that repel are _similar_
The region around the magnet is known as the magnetic field. The closer these lines are together, the stronger
the magnetic field.
e. True / False. A magnet is capable of producing an electric current.
a.
b.
c.
d.
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