Download Physical Science – 2nd Semester – Final Exam Study

Name ____________________________________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? kg
ii.
Volume of an object? ruler or water displacement method
Basic SI Unit? cm³ or mL
iii.
Length of an object? Ruler
Basic SI Unit? meter
iv.
Density of an object? graduated cylinder
Basic SI Unit? mL
b. What is the formula for calculating density? mass/volume
i.
What is the density of a cube that is 15 g and has a volume of 3 cm3? 5g/cm³
ii.
Compare the density of solid H2O to liquid H2O, and explain what observable effect this has.
_________solid H2Ois less dense than liquid H2O_____________________________________
2. Chemistry Basics
a.
b.
c.
d.
Element (def.) ___substance made up of one kind of atom____________________________________
Atom (def.) __basic building block of matter_____________________________________________________
Compound (def.) __a molecule that contains atoms or molecules of two or more different elements________
Molecule (def.) a combination of two or more of the same or different atoms that are 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? Better technology came around.
Scientist
Year
Major Discovery/ Contribution
Name of atomic model
1802
Each element is made up of small,
Billiard Ball Model
indivisible particles called atoms.
John Dalton
Different elements have atoms of
different masses.
1897
Negatively charged electron
Plum Pudding Model
J.J. Thomson
1913
Niels Bohr
1909
Ernest Rutherford
Electrons move fixed orbits around the
atom’s nucleus in specific layers, or
electron shells; Atoms absorb or give off
energy when the electrons move from
one shell (energy level) to another
1909 (Based on idea that positive
reflects positive) atom mostly empty
space; electrons orbit randomly around
positively charged nucleus
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 properties can be predicted from its location in the periodic table.
ii.
The atomic number represents the number of protons.
iii.
The atomic mass represents the number of neutrons and protons.
1
iv.
The atomic symbol represents the name of the element.
v.
The group/family number represents how many valence electrons it has.
vi.
The row/period number represents how many shells it has.
vii.
This group contains the most elements: 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.
Metalloid
Column of elements in the periodic table that have similar physical or chemical properties.
Group
The most reactive elements in the periodic table, and are soft enough to be cut with a knife.
Group 1
An element that has a shiny luster, is a good conductor of heat and electricity, is malleable
Metal
and ductile.
Elements in groups 3-12
Transition Elements
Element that is usually a gas or brittle, solid at room temperature, and does not conduct
Non-Metals
heat and electricity well.
5. Parts of an Atom
Charge
Location in the
atom
Proton
+
In the Nucleus
Electron
-
Electron Cloud or
Valence Shell
Neutron
Neutral
In the Nucleus
Nucleus
Positive
Middle
Subatomic Particle
The atom shown 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, 18 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 lose 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.
ii.
Elements in group 16 want to bond with elements in group 2.
d. The charge becomes positive when what has happened? When an atom has lost an electron.
i.
What do we call a positively charged ion? Cation.
e. The charge becomes negative when what has happened? When an atom gains and electron.
i.
What do we call a negatively charged ion? Anion.
f. An ionic bond is an attraction between what charges? Positive and Negative.
7. DNA
a. True / False. All things, living and non-living are made up of atoms. True
2
b. Macromolecule (def.) A molecule containing a lot of atoms (100).
c. List the 5 elements that make up the DNA macromolecule:
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
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 Potassium and Chlorine Ionic Bond
ii.
CO2 Carbon and Oxygen Covalent Bond
iii.
CaF2 Calcium and Fluorine Ionic Bond
iv.
P2O5 Phosphorous and Oxygen Covalent Bond
9. Naming Chemical Formulas
a. H2O is the molecular formula for water. The 2 means 2 hydrogen atoms; no number after the O indicates 1
oxygen atom.
b. The molecular formula for oxygen gas is _____O2________.
i.
Oxygen is a diatomic molecule because it has 2 oxygen atoms.
c. C6H12O6 is the chemical formula for Glucose.
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
ii.
Melting point Physical
iii.
Color Physical
b. Name a property that would describe salt.__white__; Name a property that would identify salt __taste
c. A chemical / physical change occurs when bonds are broken.
d. A chemical / physical change occurs when no new substance is formed.
e. Physical change (def.) A change that alters the form or appearance, but does not change the substance.
i.
Name 3 examples of a physical change:
1. Ice Melting 2. Chopping Wood 3. Painting a Car
f. Chemical change (def.) A change in matter that produces a new substance.
i.
Name examples of a chemical change:
1. A Burning Tree 2. Cookies 3. Rusting
ii.
Name 3 signs that a chemical change has occurred:
1. Bubbles of Gas 2.A Change in Volume 3. Light is Emitted
g. Balancing Chemical Equations
i.
2 H2 + ____ O2  2H2O
3
h. How does the Law of Conservation of Mass apply to the equation you balanced above? Matter can neither be
created nor destroyed, but can be changed in form.
i. What forms of energy could be transferred in a chemical reaction? Heat Light
i.
A change that gives off energy is called Exothermic Ex. Fireworks
ii.
A change that absorbs energy is called Endothermic Ex. Cold Pack
iii.
True / False. Every chemical reaction involves a change in energy.
11. Mixtures
a. Heterogeneous (def.) A Non-Uniform Mixture
i.
Name an example of a heterogeneous mixture: A Salad.
b. Homogeneous (def.) A Mixture in which the properties are uniform.
i.
Name an example of a homogeneous mixture: Hot Tea.
c. Separating Mixtures: Name & give a brief description of the 5 physical methods to separate mixtures:
1. Magnetism Separates objects with magnetic properties from objects with non-magnetic properties.
2. Filtration Separates a solid from a liquid.
3. Dissolving Separates a liquid from a solid.
4. Evaporation Separates a dissolved SOLUTE from a SOLUTION.
5. Chromatography Separates the different colors in dyes.
d. Solutions
i.
Solute (def.) is dissolved
ii.
Solvent (def.) does the dissolving
iii.
Solubility (def.) How much of a substance will dissolve in a liquid.
iv.
In Kool-Aid, identify the solute Sugar or the Mix 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 6.9 ; Taste Sour; Ex. Citrus Fruit
i.
What can a substance do if it has a warning of “corrosive”? Eat through materials.
b. Basic solutions pH levels from 7.1 to 14; Taste Bitter; Ex. Ammonia
13. Phase Changes
a. The three main states of matter are:
Solid Liquid Gas
b. Draw the molecular arrangement of each:
ooooooooooo
c.
o
o oo o o o o
o o oooo o o
o
o
o
o
o
o
Label the Phase Change Diagram. Use arrows where
necessary (phase transitions). See Below
Solid A
Liquid C
Gas E
Solid and Liquid B
Liquid and Gas
D
Freezing B
Melting
B
Evaporating D
Condensing D
4
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. A solid has less kinetic
energy.
14. Types of Energy
a. Energy (def.) The Ability to do Work.
b. What does it mean if something has potential energy? Capable of doing work.
i.
Example: Roller coaster as it is getting ready to take off.
c. When does an object possess kinetic energy? As it’s moving.
i.
Example: Roller Coaster.
d. Chemical PE (def.) Capable of transferring chemical energy.
i.
Example: Plants using photosynthesis to make food.
15. Energy Transformations
i.
b.
c.
d.
e.
f.
g.
h.
The law of conservation of energy states that when one form of energy is converted into another,
Energy cannot be created or destroyed, only transformed from one type to another
ii.
True / False. Most forms of energy cannot be converted into other forms.
Natural gas (Chemical energy) heats (Thermal energy) water.
Batteries (Chemical energy) are used to turn on a flashlight (Electromagnetic energy).
You rub your hands together (Thermal energy) on a cold day and friction is created to produce heat (Thermal
energy).
A microwave (Electromagnetic energy) in a house turns on because of energy produced in a nuclear power
plant from an atom’s nucleus (________nuclear____________ energy)?
A light bulb [visible light] (Electromagnetic energy) turns on because of turning on the light switch (Kinetic
energy)?
Fossil fuels (Chemical energy) are burned, which is called combustion, and heat (Thermal energy) is released.
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? Evaporation
c. Nuclear Energy
i.
Energy stored in an Atom’s Nucleus.
ii.
Nuclear Fission (def.) When a nucleus splits.
iii.
Nuclear Fusion (def.) When nuclei fuse together.
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
5
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.) 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.
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 the Positive.
h. In a series circuit: finish the saying
“when one light bulb goes out…
_____they all go out_________________”
i. In a series circuit: Adding another bulb will
add resistance and make the light 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 different; Poles that repel are the same.
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.
6