Semester 1 Final
Chemistry
Scientific Method
Scientific Measurement
Density and Buoyancy
Chapter 6
Study Guide
Chemical
Reactions
1. You should know how to write
a chemical formula using your valence sheet.
Example: Sodium
chloride Na +1 Cl -1 = NaCl
2. A chemical
change is when two or more substances react, or one substance
decomposes. In both cases
something new is formed. Evidence
of a chemical
change:
- Temperature change
(exothermic or endothermic)
- Color change
- Precipitate forms
- Gas produced (bubbles)
- Fire/Explosion
3. A physical change is a change in matter that does not produce
a new substance like cutting paper or mixing salt and pepper.
4. You should know the
structure of a chemical formula.
Be able to label reactants,
products, yields sign, subscripts and coefficients.
5. Know that subscripts tell us
the number of atoms of an element and coefficients tell us the number of
molecules of a substance.
6. Law of Conservation of Mass: Matter is not created nor destroyed.
7. You should know how to
balance chemical equations.
8. You should be able to
identify the four major types of chemical reactions: Synthesis, Decomposition,
Single Replacement, and Double Displacement.
9. A catalyst is a substance that speeds up a reaction but is not
involved in the chemical reaction.
Be able to identify the catalyst in a reaction.
Chapter 5
Study Guide
Chemical
Bonding
1.
Using the Periodic Table,
you should be able to draw the electron dot diagram for all of the elements
covered in class.
2.
Ionic Bonds
A.
Know that an ion is a
charged atom or group of atoms
B.
A polyatomic ion is what we
call a charged group of atoms
C.
Atoms become charged when
the gain or lose electrons.
D.
Atoms have positive charges
when the lose electrons (mostly metals) and negative charges when they gain
electrons (mostly nonmetals).
E.
Ionic Bonds form when
electrons are transferred from one atom to another resulting in ions. The opposite charges of the ions
attract each other. This is a very
strong bond.
F.
You should know how to write
chemical formulas using ion charges.
You should know how to name compounds using the chemical formula. I will give you an ion list to use on
the test.
G.
You should know the
characteristics of ionic compounds:
1)
Ionic compounds form
crystals because of the regular repeating pattern of ions.
2)
Conduct electricity when
dissolved in water.
3)
High melting points
4)
Not flammable
5)
Almost all ionic compounds
(salts) are formed from
a metal and a nonmetal bonding.
3.
Covalent Bonds
A.
Know that covalent bonds
form when atoms share electrons.
B.
Usually form when nonmetals
bond to other nonmetals.
C.
Sometimes atoms have to
share lots of electrons when they bond (example: Nitrogen gas forms with a
triple bond).
D.
Covalent molecules often
have low melting points and burn easily (more flammable).
E.
Most covalent compounds do
not conduct electricity in water like ionic compounds do.
Study Guide
Chapter 4 – The Periodic
Table
Atomic Number if given the name, symbol,
# of protons, or # of electrons
Number of Protons if given the name, symbol,
atomic #, or # of electrons
Number of Electrons if given the name, symbol,
atomic #, or #of protons
Atomic Mass (weight) if given the name or symbol
Element Symbol if given the element name
Element Name if given the symbol, atomic
#, # of protons, or #of electrons
Period Number if given the symbol, atomic
#, or # of protons or electrons
Number of Energy Levels if given the name, symbol,
atomic #, or period
Group/Family if given the name, symbol,
or atomic number
Number of Valence Electrons if given the name, symbol,
or group/family
Properties and Valence
Electrons
for Alkali Metals, Alkaline Earth Metals, Halogens and Noble (Inert Gases)
Dmitri Mendeleev
Know
where to find metals,
nonmetals, and synthetic elements on the Periodic Table
Know
that semimetals (metalloids)
are good semiconductors because they can conduct electricity but not as well as
metals (example: silicon)
Periods are horizontal rows that
tell us the number or energy levels
Know
major properties of metals and
nonmetals
Bohr Models: Be able to draw Bohr models for all elements up to 20.
Chapter
3 Study Guide
Chemistry
– Properties of Matter
Solids,
Liquids, and Gases
Study all Labs, Homework Sheets, Handouts,
Graphic Organizers, and Notes. You
may also refer to Chapter 3 in your book.
Know
definitions for the following terms:
Amorphous solid Crystalline Solid Solid
Fluid
Gas
Liquid
Surface Tension Temperature
Thermal Energy Viscosity
Evaporation
Vaporization
Boiling
Know the definitions, molecular
movement, and processes involved for each of the following:
(Example: Melting – Solid
to Liquid – Increase in Molecular Motion)
Melting
Evaporation Sublimation
Freezing
Condensation
Resublimation
Know that TEMPERATURE and PRESSURE are
two factors that can affect the phase of matter.
Be
able to explain the Gas Laws
and give examples of each (Charles’s Law, Boyle’s Law, and
Temperature/Pressure)
Know
the effects of changing temperature, pressure, and volume of a gas.
Know
that water freezes at 0 degrees C and boils at 100 degrees C.
Know your labs – why we did the labs and what they
showed. Labs to know: Freezing
point lab, Marshmallow Madness Lab, Endothermic and Exothermic Lab, and all gas
demos.
FROM CHAPTER 2 KNOW
THE FOLLOWING:
Be able to define,
describe, and identify chemical changes, physical changes, endothermic
reactions and changes, and exothermic reactions and changes.
Know that
electricity can be used to break molecules apart. This is called electrolysis. We used electrolysis to break bonds in water. We saw gas bubbles produced and acids
and bases produced. That was the
evidence that new substances had been formed – a chemical change.
Chapter 2 Test Study Guide
Properties of
Matter
Concepts to Know:
1.
Everything is either energy
or matter.
2.
Properties of matter are
characteristics of a substance that help to identify that substance. Physical properties are characteristics
that can be observed and measured without breaking bonds or changing the substance
chemically.
Examples: Color, shape, density, boiling point
Chemical properties can only
be observed when a substance is changes chemically.
Examples: Reactivity with
other chemicals, flammability
3.
An element is a pure
substance that cannot be broken down into any other substance. There are 92 naturally occurring
elements in the universe. Elements
are organized on the Periodic Table of the Elements.
4.
Atoms are the smallest
particle of an element.
5.
Molecule – Two or more atoms
chemically bonded. Examples: NaCl, CaCl2, O2,
H2O, H2
6.
Compound – Two or more
DIFFERENT types of atoms chemically bonded. Example: All of
the examples for molecules BUT H2. H2 is only made of one thing, Hydrogen.
7.
A mixture is two or more
things combined together that have not been chemically bonded. Solutions are a type of mixture where
one thing dissolves into another. Examples: trail mix, salt water
8.
Heterogeneous Mixture – You
can see the parts of the mixture
9.
Homogeneous Mixture – You
can’t see the parts of the mixture.
10. A physical change is a change in a substance that does not alter a
substance chemically. It’s still
the same substance.
11. A chemical change is a change where bonds are broken and new substances
are formed. Example: Burning wood,
reacting Sulfuric Acid and Sugar.
12. Law of Conservation of Matter says that whatever matter goes into a
chemical reaction has to come out.
13. Thermal Energy is the measure of the amount of movement of molecules in
a substance. The more movement,
the more thermal energy, the higher the temperature. Temperature is a measure of the thermal energy of an
object. We measure thermal energy
(temperature) with a thermometer.
14. Chemical Energy is energy stored in chemical bonds.
15. Know the indicators of a chemical change and that a precipitate is a
solid formed from a chemical reaction between two or more substances.
Study Guide –
8th Grade Physical Science
Chapter 1 Test
To
prepare for this test you will need to use your notes, labs, homework, and
class work as well as your textbook.
Scientific Inquiry (pages 6-15)
1. Know what an inference
is. Be prepared to make inferences
about a picture similar to the class and homework examples.
2. Know what a hypothesis is.
3. What are parameters in a
scientific investigation?
4. Know the definitions for
manipulated and responding variable and be able to identify each in a given
example.
5. What is a controlled
experiment? Why is it important
for experiments to be controlled?
6. What is a scientific
theory? Know how theories and
hypotheses are different.
Measurement and Equipment (pages 16 – 26)
1. What is length? What units do we use to measure length
in science?
2. What is weight?
3. What is mass? What units do we use to measure mass?
4. How are weight and mass
different?
5. What happens to weight as
gravity increases or decreases?
6. What is volume? What units do we use to measure volume?
7. What is density? What are the units for density? What is the formula used to measure
density?
8. Be ready to compare the
relative densities of common objects discussed in class.
9. Know graduated cylinder,
beaker, balance, ruler, and Erlenmeyer flask.
Graphing in Science (pages 34 – 41)
1. Know how to identify
manipulated and responding variables in an experiment.
2. Know how to take the data
from a data table and graph the data putting the manipulated data on the horizontal
axis and the responding variable on the vertical axis. Label each axis.
3. Know how to read a line
graph.
