Download MidtermReview2012

Name ______________________
Section A B C D
Midterm Review Packet
Date _________________
Instructions:
Step 1: Use the Course Content Meter to rank the following (page 2) topics and subtopics on a scale of 13. Write a number on the line next to each subtopic, and write the average number in the box for that
section.
IDK:
I have no idea what this is… I
need to spend a lot of time
relearning and reviewing this
information.
Course Content Meter
Not So Sure:
I remember doing this, but I don’t
remember much about it. I need
to spend some time looking over
this stuff.
No Question:
I know this for sure! I’ll just
have to review it before the
exam.
1
2
3
Step 2: Look over the entire packet and find the unit with the most 1s. Write that unit as priority #1 in the
Priorities for Studying chart (below). Then find the unit with the second most 1s. That’s your second
priority. Continue filling out the chart with each unit.
Step 3: Start with the unit that is your top priority. Follow these guidelines for studying:
(a)
Assemble your resources – find your notes and important handouts, labs, and other
assignments from that unit. Use your Objective mastery tracking sheets to fill out the
‘High’ column on the next page with your highest score on that objective. This will help
you determine how effective your old tests will be as a resource.
(b)
Create a page in your notebook labeled “Midterm Review: Unit ___”. On that page
rewrite the key vocabulary from the unit. You may want to create charts, flashcards, etc.
(c)
Solve problems – Start working on practice problems from this packet to help you practice
the think skills required to accurately answer questions. If you need more practice
problems for an objective, start by reviewing your old tests! Ask for more!
Why Study Like This? This packet will guide you to spend the MOST amount of your time focusing on
the 1s. Once you understand that stuff, move on to the 2s. Lastly, review the 3s before the midterm.
*****DO NOT start on page one, problem one and work in chronological order to the last problemt on
the last page; there is a very good chance that you will not make it that far.*****
You are also more likely to spend a bunch of time studying stuff you already know and less time studying
the stuff you don’t, simply because you didn’t get to it.
PRIORITY #1: Unit ___________
PRIORITY #2: Unit ___________
PRIORITY #3: Unit ___________
Page 1 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Unit 1: Matter and the Scientific Method
Meter #
Objective
1.1
list and describe, and identify examples of each part of the scientific method
1.2
write a testable hypothesis for a research question
1.3
explain the difference between, and identify from an experiment, independent and
dependent variables
1.6
convert between standard and scientific notation
1.7
correctly use and convert between units of mass, length and volume
1.8
make and interpret density calculations
1.10 determine the number of significant figures in a measurement
1.11 round a calculation to the correct number of significant figures
1.12 differentiate between and identify physical and chemical changes and properties
1.13 describe and define characteristics of the three states of matter and changes
between states of matter
1.14 classify substances and give examples of matter, non-matter, pure substances,
atoms, elements, compounds and mixtures
Unit 2: The Atom and the Electron
Meter #
Objective
2.2
Name the 3 subatomic particles and identify their charge, mass and location
2.3
Model number and location of subatomic particle in elements 1-20.
2.5
Relate atomic number to the number of each subatomic particle.
2.7
Draw orbital diagrams for the first 86 elements
2.8
Write the electron configuration notation for the first 86 elements
2.9
Identify the number of and location of valence electrons present in any neutral
atom and relate to groups on the periodic table
2.10 Draw an electron dot diagram for any neutral element
2.11 Differentiate between neutral atoms and ions
2.13 Write ECN and draw diagrams for ions
High
High
Unit 3: Periodicity, Bonding, & Chemical Nomenclature
Meter #
Objective
High
3.1
Predict the ion formed, and write ion symbols and names for elements in groups 1,
2, 13-18
3.4
Predict the type of bond that will form between any two elements
3.5
Write names and formulas for ionic compounds, including those requiring the
stock system and those including polyatomic ions
3.6
Write names and formulas for covalent compounds
3.7
Write the names and formulas for the first ten hydrocarbons
3.8
Draw Lewis structures for covalent compounds
3.9
Use the VSEPR theory to predict the molecule shape and bond angle
Page 2 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Unit 4: The Mole
Meter #
Objective
4.1
Define the mole as a number of representative particles
4.2
Make calculations to convert between atoms/molecules, number of moles and
mass of a sample of an element or compound
Unit 5: Chemical Reactions
Meter #
Objective
5.1
Identify the four indications of a chemical change
5.2
Write a chemical equation from a word equation
5.3
Balance a chemical equation
5.4
Identify a reaction as one of the five types of chemical reactions
High
High
Objective 1.1
1. List all of the parts of the scientific method.
2. List at least 5 sources of error that might have occurred during the candium lab.
Objective 1.2
1. List the 3 key words that should be included in every hypothesis.
2. Write a hypothesis for the following problem statement: “What is the relationship between the
height of a person and their weight?”
3. Explain what the biggest problem is with the following hypothesis: “If I change the amount of
water I give my plants, then the amount they grow will also change, because plants need water
to grow.”
Objective 1.3
1. Explain the difference between an independent and dependent variable.
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Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
2. Given the following problem statement, label the independent and dependent variables: “How
is the speed of a reaction affected by temperature?”
3. Given an experiment that involves testing the acidity of water from different sources, label the
independent and dependent variable.
Objective 1.6
1. Write the following numbers in standard form
a. 2.02 x 1012
b. 5.014 x 10-4
2. Write the following numbers using scientific notation
a. 3,000
b. 0.00009950
3. Which of the following numbers is larger? Explain how you arrived at that answer.
a. 6.11 x 10-7
b. 6.22 x 10-8
4. Convert the following numbers into scientific notation
a. 970
b. 0.000402
5.
Convert the following numbers into standard notation
a. 1.12 x 103
b. 9.1 x 10-7
Objective 1.7
1. Match each unit to the corresponding type of dimension.
cm
volume
ml
length
week
mass
kg
time
2. a. Convert 5.8 miles to meters. (1 mile = 5280 feet, 1 foot = 12 inches, 1 inch = 2.54 centimeters)
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Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
b. Convert 3.85 gallons into milliliters (1 gallon = 3.79 liters)
Objective 1.8
1. Calculate the density of an object that is 4.94g and occupies a space of 1.2cm3
2. Rank the following 4 objects from most (1) to least (4) dense.
_____ mass = 4.2g, volume = 3.1ml
_____ density = 1.2g/cm3
_____ mass = 8.4g, volume = 32cm3
_____ volume = 1.2ml, mass = 15.6g
Objective 1.10
1. Identify the number of significant figures in the following measurements:
a. 7.21
b. 11.123
c. 61
2. Identify the number of significant figures in the following measurements:
a. 101
b. 0.09500
c. 0.0003009
Objective 1.11
1. Round the following calculations to the correct number of significant figures:
a. 42 x 13 =
b. 10.1 – 3.1 =
c. 12.00 + 4.10 =
d. 8.0 / 1.0 =
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Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
2. If Joelle masses out a penny at 2.89grams and measures the volume to be 0.4ml, calculate the
density of the penny by dividing the mass by the volume.
3. Make the following calculations and round your answers to the correct number of significant
figures.
a. 900 x 1 =
b. 8.2 / 1.3 =
c. 435.5 x 27.1 =
d. 5000/200 =
4. Calculate the density of an object that is 12.62 grams in mass and 4.31ml in volume.
Objective 1.12
1. Identify the following changes as physical or chemical:
a. Smashing a brick against a wall
b. Acid rain dissolving a statue
c. An explosion from dynamite
d. The freezing of water
2. List 3 action words that might be used to describe a chemical change.
3. When a small amount of carbon is mixed in with molten iron, the cooled resulting alloy is
called steel. Would you consider the iron to be changed physically or chemically? Explain.
Objective 1.13
1. List the 3 main states of matter (phases)
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Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
2. Which state of matter tends to occupy the largest amount of space? The smallest? In other words,
which state of matter is the densest? Which is the least dense?
Objective 1.14
1. Of the following options below, circle all of the options that are matter.
a. Communism
b. dust
c. protons
d. fear
e. the sun
2. What small particle is the basic piece of all matter?
3. If fire is made from gas particles that are ionized, should fire be considered matter or nonmatter? Explain.
Objective 2.2
1. Name the 3 subatomic particles.
2. Calculate the total mass number of an atom of sodium with 11 neutrons. Write your answer in
atomic mass units (amu).
3. Fill in the table below:
Particle
Mass
Proton
Charge
Location
Electron
Neutron
4. In order for an atom to be considered electrically neutral, what two subatomic particles must be
present in equal amounts? Explain why.
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Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 2.3
Given the model of neutral nitrogen-14 to the right:
1. Place the correct number of protons in the correct location.
2. Place the 7 neutrons in the correct location.
3. Place the correct number of electrons in the correct location.
4. How many electrons are in a neutral atom of potassium?
5. Draw a picture of a magnesium atom and label each of the 3 types of subatomic particles.
Objective 2.5
1. In a neutral atom, how are the number of protons and the number of electrons related?
a. There are more protons. b. There are more electrons. c. The numbers are equal.
2. Fill out the table below by relating the atomic number to number of each subatomic particle.
Assume all atoms are neutral.
Atomic number Atomic mass
# of protons
#of neutrons
# of electrons
14
7
11
23
19
39
3. How is the atomic number usually related to the number of protons in an atom?
a. # of protons > atomic #
b. They are equal
c. # of protons < atomic #
4. How is the atomic mass number usually related to the number of protons in an atom?
a. # of protons > atomic mass b. They are equal
c. # of protons <atomic mass
Objective 2.7
1. Draw an orbital diagram for nitrogen below. Label each orbital.
2. Which of the following orbitals will be filled first (lowest energy)?
a. 4s
b. 3d
c. 2p
d. 5f
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Date _________________
Name ______________________
Section A B C D
Midterm Review Packet
3. Draw the orbital diagram for phosphorus below. Make sure to label each orbital.
4. Draw the orbital diagram for Uranium.
Objective 2.8
1. Rewrite the following electron orbitals in order of increasing energy state (2p, 3s, 4p, 3d)
2. Write the full electron configuration notation (ECN) for phosphorus.
3. Which of the following is an incorrect ECN?
a. 1s22s1
b. 1s21p62s1 c. 1s22s22p63s1
d. 1s22s22p63s23p64s23d3
4. Write the ECN for iron below:
5. The ECN for transition metals can be different than expected. Try to explain why the ECN for
Chromium would be [Ar]3d54s1 instead of [Ar]3d44s2 as expected.
Objective 2.9
1. How many valence electrons are present in an atom with the ECN of: 1s22s22p3?
a. 2.
b. 3
c. 4
d. 5
e. 6
f. 7
2. How many valence electrons are present in a neutral atom of oxygen?
3. How many valence electrons are present in a neutral atom of lead?
4. For each of the following elements, write the number of valence electrons that a neutral atom
of that element will have.
a. Sodium
b. Barium
c. Fluorine
d. Aluminum
5. Write the ECN for phosphorus and circle the valence electrons
Page 9 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 2.10
1. In an electron/Lewis dot diagram, what do the dots represent?
2. Draw an electron dot diagram for chlorine:
3. Draw an electron dot diagram for Scandium:
4. What is the maximum number of dots that can be around a symbol in a correctly drawn
electron dot diagram?
5. Draw an electron dot diagram for Aluminum
Objective 2.11
1. Which has more electrons, a neutral atom of sulfur or a sulfur anion?
2. Explain the difference between an ion and a neutral atom.
3. Explain the difference between an ion and a neutral atom.
4. Explain the difference between a cation and an anion.
Objective 2.13
1. Write the ECN for Ca+
2. Draw a dot diagram for S3. Write the ECN for sulfur after it has gained 2 electrons.
4. Draw an electron dot diagram for a sodium atom that has lost an electron.
Page 10 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 3.1
1. Write the symbol of the most common ion formed from the following elements (Li, N, O, F, Ca,
Ba, Cs, I, S, B, Al, Mg, Na, H, Ne)
Objective 3.4
1. Identify each of the following compounds as ionic or covalent:
NaCl
LiOH
BaNO3
MgCO3
CO2
BrF3
SO2
PCl5
2. Write 2 examples (not listed above!) of ionic compounds, covalent compounds.
Objective 3.5 & 3.6
1. Name the following compounds
NaCl
LiOH
BaNO3
MgCO3
CO2
BrF3
SO2
PCl5
FeCl2
SnO2
2. Name the 4 compounds that you wrote in Objective 3.4, question #2.
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Midterm Review Packet
Date _________________
3. Write the formula for the following compounds
Name ______________________
Section A B C D
lithium chloride
boron trifluoride
ammonium nitrate
aluminum nitrite
barium sulfate
zinc hydroxide
sulfur dioxide
carbon monoxide
iron (III) fluoride
copper (I) phosphate
vanadium (IV) sulfide
Objective 3.7
1. Write the name and formula for the first 10 hydrocarbons.
2. Write the generic formula for alkanes given ‘n’ carbons.
Page 12 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 3.8
1. Draw Lewis structures for the following covalent compounds: PCl3, PCl5, NH3, OH-, PO43-, H2S,
Cl2, O2, N2, C2H6
Page 13 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 3.9
1. Using VSEPR theory, predict the molecule shape for the following atoms that you drew for
objective 3.8 (PCl3, PCl5, NH3, PO43-, H2S). Label the shape name and the bond angle on the
previous page.
Objective 4.1
1. Match each of the following words to the number that matches it best:
a. Dozen
2
b. Couple
12
c. Mole
6.02x1023
2. How many atoms are in 1 mole of atoms?
Objective 4.1
1. Which of the following numbers is equivalent to 1 mole of atoms?
a. 9.57 x 1032
b. 6.02 x 1023
c. 12
d. 6.02 x 10-23
2. Write the mass of one mole of calcium atoms.
Objective 4.2
1. Draw the map and conversion fractions that shows the relationship between number of
atoms/molecules, moles and mass.
2. Convert 2.00 mol of aluminum into grams.
3. Calculate the molar mass of carbon dioxide.
4. Convert 125g of carbon dioxide into molecules.
Page 14 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
Objective 4.2
1. Convert 29.3g of carbon into moles of carbon.
2. Convert 5.912x1024 atoms of calcium into grams of calcium.
Objective 5.1
1. List the 4 indications of a chemical reaction.
Objective 5.2
1. Write the chemical formula for each of the following compounds
a. Aluminum chloride
b. Methane
c. Ammonium nitrate
d. Carbon monoxide
2. Write a balanced chemical equation from the following word equation: “Solid aluminum reacts
with the oxygen in the air to form solid aluminum oxide.”
Objective 5.3
1. Use the bold and underlined words to help you determine if the following statement is TRUE or
FALSE
“Subscripts are used to help balance the charge of a compound, while coefficients are used to
balance the mass of the overall equation.”
Page 15 of 16
Date _________________
Midterm Review Packet
Name ______________________
Section A B C D
2. Write a balanced chemical equation for the following:
a. Solutions of magnesium iodide and lead (II) nitrate react to a form a solution of
magnesium nitrate and solid lead (II) iodide.
b. Nitrogen gas reacts with oxygen gas and water to produce a solution of hydrogen nitrate.
Objective 5.4
1. Which type of reaction would you consider to be the opposite of synthesis?
2. For each of the following reactions, write the type of reaction.
a. CH4 + 2O2  CO2 + 2H2O
b. P4 + 5O2  P4O10
c. NH4OH  NH3 + H2O
d. BaCl2 + Na2SO4  BaSO4 + 2NaCl
P4O10
e. Cu + AgNO3  CuNO3 + Ag
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