Download Name: Period:______ PHYSICAL SCIENCE 1st Semester Final

Name:___________________________________
Period:_________
PHYSICAL SCIENCE
1st Semester Final Exam Study Guide
Chapter 1
Vocabulary:
science, technology, scientific method, observation, hypothesis, independent variable, dependent
variable, scientific theory, scientific law, model, scientific notation, mass, volume, density,
precision, accuracy
Key Ideas:
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Science and technology are interdependent. Advances in one lead to advances in the
other.
Natural science is generally divided into three branches: Physical Science, Earth and
Space Science, and Life Science.
The goal of the scientific method is to solve a problem or better understand an observed
event.
The independent (manipulated) variable is the variable in an experiment that you are
changing deliberately. It is what you are testing.
The dependent (responding) variable is what changes as a result of the independent
variable. It is what you are measuring.
Scientific models make it easier to study things that are difficult to observe directly.
There are many safety precautions that scientists must make prior to carrying out
investigations.
Scientific notation makes really large or really small numbers easier to work with.
Precision is the exactness of a measurement, while accuracy is the closeness to the true
value.
Scientists must communicate results in order for the knowledge base of the scientific
community to grow.
Be able to:
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Identify the vocabulary words
List the steps of the scientific method
Identify independent and dependent variables in a given experiment.
Write numbers using scientific notation
Calculate density
Name:___________________________________
Period:_________
Practice:
1. What is the goal of the scientific method?
2. Write the following terms using scientific notation.
a. 120,000 km =
b. 745,00000 mL =
c. 0.0046 g =
3. Convert the following terms from scientific notation.
a. 6.2 x 104 =
b. 3.7 x 102 =
c. 4.1 x 10-3 =
4. Ms. McNeice wanted to see how different types of music affected students’ pulse rate.
She played country, rap, classical, alternative, and pop.
a. What is the independent variable?
b. What is the dependent variable?
5. Homer notices that his shower is covered in a strange green slime. His friend Barney tells
him that coconut juice will get rid of the green slime. Homer decides to check this out by
spraying half of the shower with coconut juice. He sprays the other half of the shower
with water. After 3 days of "treatment" there is no change in the appearance of the green
slime on either side of the shower.
a. What is the independent variable?
b. What is the dependent variable?
c. What should Homer’s conclusion be?
6. An unknown liquid has a volume of 30 mL and a mass of 90 g. What is the density of
this liquid?
Name:___________________________________
Period:_________
Chapter 2
Vocabulary:
Pure substance, element, atom, compound, heterogeneous mixture, homogeneous mixture,
solution, suspension, colloid, physical property, viscosity, conductivity, malleability, melting
point, boiling point, filtration, distillation, physical change, chemical change, reactivity,
flammability, chemical change, precipitate
Key Ideas:
 Every sample of a given substance has the same properties because a substance has a
fixed, uniform composition.
 An element has a fixed composition because it contains only one type of atom.
 A compound always contains two or more elements joined in a fixed proportion.
 The properties of a mixture can vary because the composition is not fixed.
 Homo = same ; hetero = different
 Based on the size of its largest particles, a mixture can be classified as a solution,
suspension, or a colloid.
 Viscosity, conductivity, malleability, hardness, melting point, boiling point, and density
are examples of physical properties.
 Viscosity decreases as the temperature of a liquid increases.
 Properties of matter are used to choose materials for specific uses.
 Properties of mater can be used to separate substances; Filtration and distillation are two
common separation methods.
 A physical change does not change the composition of matter.
 A chemical change forms one or more new substances.
 Three common types of evidence for a chemical change: change in color, production of a
precipitate, and production of a gas.
Be able to:
 Identify vocabulary words
 Identify whether a change is physical or chemical
 Determine whether a mixture is homogeneous or heterogeneous
 Describe the physical properties of a substance
 Determine the state of matter given the melting point and boiling point
Practice:
1. Identify each as either a substance or mixture. If it is a substance, state whether it is an
element or compound. If it is a mixture, state whether it is homogeneous or
heterogeneous.
a. Water =
b. Iron =
Name:___________________________________
Period:_________
c. Carbon dioxide =
d. Ice cream sundae =
e. Coffee =
2. Why is copper used for electrical wiring?
3. Substance “A” has the following properties. Melting point = 10°C ; Boiling point = 92°C
Identify the state of substance “A” at the following temperatures.
a. 8°C =
b. = 122°C =
c. 13°C =
4. Explain why the properties of a pure substance do not vary from sample to sample.
5. What is the difference between a compound and an element?
6. What allows a mixture to be separated by filtration?
7. List one chemical change and one physical change that occur when a candle burns.
8. Describe the difference between a compound and a mixture.
Name:___________________________________
Period:_________
Chapter 3
Vocabulary:
Solid, liquid, gas, kinetic energy, pressure, phase change, endothermic, exothermic, sublimation,
deposition, vaporization, evaporation,
Key Ideas:
 Matter is classified as a solid, liquid, or gas based on whether their shapes and volumes
are definite or variable.
 Kinetic theory states that all particles of matter are in constant motion.
 There are forces of attraction among the particles.
 Solids have a definite volume and shape.
 Liquids have a definite volume and a variable shape.
 Gases have a variable volume and shape.
 Collisions between particles of a gas and the walls of the container cause the pressure in a
closed container of gas.
 Factors that affect the pressure of an enclosed gas are its temperature, volume, and the
number of particles.
 Raising the temperature of a gas will increase the pressure.
 Decreasing the volume of a gas will increase the pressure.
 Increasing the number of particles of a gas will increase the pressure.
 Combined gas law: P1V1/T1 = P2V2/T2
 Melting, freezing, vaporization, condensation, sublimation, and deposition are six
common phase changes.
 Temperature does not change during a phase change.
 Energy is either released (exothermic) or absorbed (endothermic) during a phase change.
 Evaporation occurs at temperatures below the substance’s boiling point and at the surface
of a liquid.
Be able to:
 Identify vocabulary words
 Describe the differences between solids, liquids, and gases
 Describe how the temperature, pressure, and volume of gases are related
 Use the combined gas law to calculate the pressure, volume, or temperature of a gas
 Identify whether a phase change was endothermic or exothermic
Practice:
1. How does the arrangement of particles differ between solids and gases?
2. A sample of gas has a volume of 283 mL at a temperature 25°C and a pressure 0.50 atm.
What is the volume of this gas at 100°C and 1.0 atm?
Name:___________________________________
Period:_________
3. A toy balloon filled with air has an internal pressure of 1.25 atm and a volume of 2.50 L.
If I take the balloon to the bottom of the ocean where the pressure is 95 atmospheres,
what will the new volume of the balloon be?
4. Identify each phase change as either endothermic or exothermic.
a. Solid  Liquid
b. Gas  Solid
c. Liquid  gas
5. Using the kinetic theory, explain why a liquid has a definite volume but a gas does not.
6. Using the kinetic theory, explain what causes gas pressure.
7. What three factors affect the pressure of a gas in a closed container?
8. If a piston moves downward in a cylinder, what happens to the volume and the pressure
of the gas in the cylinder? The temperature remains constant.
9. What happens to the speed of the particles inside an air-filled balloon if the temperature
of the balloon increases?
10. How does an exothermic phase change differ from an endothermic phase change?
11. Draw a diagram showing the process of the six common phase changes.
Name:___________________________________
Period:_________
Chapter 4
Vocabulary:
nucleus, proton, neutron, electron, atomic number, mass number, isotopes, energy levels,
electron cloud, orbital, electron configuration, ground state
Key Ideas:
 Dalton proposed the atomic theory stating that all matter is made up of particles called
atoms that cannot be divided.
 Thomson’s experiments provided the first evidence that atoms are made up of smaller
particles called subatomic particles (electrons, neutrons, protons).
 According to Rutherford’s model, all of an atom’s positive charge is located in its
nucleus.
 Protons, electrons, and neutrons can be distinguished by mass, charge, and location in an
atom.
 Isotopes of an element have the same atomic number but different mass numbers because
they have different numbers of neutrons.
 An electron can move from one energy level to another when the atom gains or loses
energy.
 Scientists use the electron cloud model to describe the possible locations of electrons
around the nucleus.
 The most stable electron configuration is one in which the electrons are in orbitals with
the lowest possible energies.
Be able to:
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Identify vocabulary words
Understand and explain why indirect evidence is used to study the structure of
atoms
Compare the subatomic particles of an atom (mass, location, charge)
Differentiate between atomic number and mass number
Calculate the number of protons, neutrons, and electrons a given atom of an
element contains
Understand the differences between isotopes of an element
Compare the modern atomic theory to past models of the atomic theory
Explain the difference between ground state and excited state
Practice:
1. Explain why indirect evidence must be used to study the atom.
2. Name the three subatomic particles.
3. Compare and contrast the three subatomic particles by mass, location, and charge.
Name:___________________________________
Period:_________
4. Describe how you could distinguish a proton from an electron.
5. Which characteristic of an atom always varies among atoms of different elements?
6. How are the isotopes of an element different from one another?
7. How can atoms be neutral if they contain charged particles?
8. What is the difference between atomic number and mass number?
9. If the atomic number of an atom is 11, how many electrons does it have? Explain.
10. If an atom has an atomic number of 6 and a mass number of 14, how many protons,
electrons, and neutrons are in the atom?
11. What is the difference between atoms of oxygen-15 and oxygen-16?
11b. If the atomic mass on the periodic table is 15.9, then which isotope is more
prevalent?
12. What is the main difference between Bohr’s model of the atom and the atomic theory that
is currently accepted?
13. What does it mean to say that an atom is in an excited state? Ground state?
14. Describe the most stable electron configuration of the electrons in an atom.
15. How many protons, neutrons and electrons to each of the following isotopes contain?
Li – 7
Si – 29
Ne – 20
I – 126
Ba – 137
B – 11
Name:___________________________________
Period:_________
Chapter 5
Vocabulary:
periodic table, period, group, periodic law, atomic mass unit (amu), metals, transitional metals,
nonmetals, metalloids, valence electron, alkali metals, alkaline earth metals, halogens, noble
gases
Key Ideas:
 Mendeleev arranged the elements into rows in order of increasing mass so that the
elements with similar properties were in the same column.
 The close match between Mendeleev’s predictions and the actual properties of new
elements showed how useful his periodic table could be.
 In the modern periodic table, elements are arranged by increasing atomic number
(number of protons).
 Each row on the table is a period.
 Each column on the table is a group.
 Properties of elements repeat in a predictable way when atomic numbers are used to
arrange the elements into groups.
 Atomic mass is a value that depends on the distribution of an element’s isotopes in nature
and the masses of those isotopes.
 Elements are classified as metals, nonmetals, and metalloids.
 Across a period from left to right, the elements become less metallic and more
nonmetallic in their properties.
 Elements in a group have similar properties because they have the same number of
valence electrons.
 The alkali metals (group 1A) are extremely reactive.
 Group 2A contains the alkaline earth metals.
 The halogens (group 7A) are extremely reactive nonmetals.
 The noble gases (group 8A) are colorless, odorless, and extremely unreactive.
Be able to:
 Identify vocabulary words
 Read a periodic table
 Describe how Mendeleev’s periodic table was arranged and how his table proved to be
useful
 Identify what determines the order of the elements in the modern periodic table
 Name the categories used to classify the elements in the periodic table (metal, nonmetal,
metalloid) and describe their properties
 Identify the trends that occur as you move from left to right and up and down the periodic
table
 Explain why elements in a group have similar properties
 Understand why hydrogen is located in a group with reactive metals
 Determine the reactivity of a given element
 Identify the number of valence electron a given atom of an element has
Name:___________________________________
Period:_________
Practice:
1. What information did Mendeleev have about the elements he organized into a periodic
table and why did he leave empty spaces in his table?
2. What determines the order of the elements in the modern periodic table?
3. What two factors determine the atomic mass of an element?
4. List three ways that the elements in the periodic table can be classified.
5. Why was it difficult to discover the noble gases?
6. List the two most reactive groups on the periodic table and explain why they are the most
reactive.
7. Explain why elements in a group have similar properties.
8. Which group of elements is the least reactive and why?
9. Find the correct information using the periodic table for the following elements
a. The atomic mass for carbon
b. The symbol for potassium
c. The atomic number for argon
d. The group number for aluminum
Name:___________________________________
Period:_________
Chapter 6
Vocabulary:
electron dot diagram, ion, anion, cation, chemical bond, ionic bond, chemical formula, covalent
bond, molecule, polar covalent bond
Key Ideas:
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When the highest occupied energy level of an atom is filled with electrons, the atom is
stable and not likely to react.
Some elements achieve stable electron configuration through the transfer of electrons
between atoms.
An ionic bond forms when electrons are transferred from one atom to another.
The attraction between the shared electrons and the protons in each nucleus hold the
atoms together in a covalent bond.
When atoms form a polar covalent bond, the atom with the greatest attraction for
electrons has a partial negative charge. The other atom has a partial positive charge.
The type of atoms in a molecule and its shape are factors that determine whether a
molecule is polar or nonpolar.
Attractions between polar molecules are stronger than the attractions between nonpolar
molecules.
Be able to:
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Identify vocabulary words
Determine whether or not an electron configuration is stable (when is an atom
most likely and least likely to react)
Describe what each dot in an electron dot diagram (Lewis dot diagram) represents
Describe the ways that an electron can achieve stable configuration
Understand chemical bonds
Explain what processes change atoms into ions
Cation = positive charge Anion = negative charge
Understand the characteristics of ionic bonds
Explain the properties of ionic compounds (metal bonded to nonmetal)
Use subscripts properly to write a chemical formula
Understand how covalent bonds form
Distinguish between single, double, and triple covalent bonds
Explain why the covalent bonds of elements are always nonpolar
Explain why the covalent bonds of compounds are polar (example: H2O)
Determine what type of bond a molecule/compound will form (or not form) based
on its properties-Examples: oxygen + oxygen (nonpolar covalent), chlorine +
sodium (ionic), neon(will not form bonds)
Name:___________________________________
Period:_________
Practice:
1. When an atom loses an electron, it forms a(n) ____________________.
2. When an atom gains an electron it forms a(n) ____________________.
3. The charge on a chloride ion in AlCl3 is ________________________.
4. A chemical bond that forms when atoms share electrons is always a(n)
________________ bond.
5. When two fluorine atoms share a pair of electrons, the bond that forms is a(n)
________________________________________.
6. What is a stable electron configuration? Give an example.
7. What does each dot in an electron dot diagram represent?
8. Draw an electron dot diagram for an atom of the following elements: Al, O, Ne
9. What processes change atoms into ions?
10. Explain what the subscripts in a chemical formula stand for?
11. Distinguish whether the following atoms form single, double, or triple covalent bonds.
a. Oxygen + Carbon
b. Nitrogen + Nitrogen
c. Hydrogen + Chlorine
12. Write the formula for a compound between the following elements
Na + S
Mg + O
Ca + N
F+N
O+S
P + Se