Chemistry A Final Exam Review Name: ______Hour: ______
Chemistry A
Final Exam Review
The final exam will include:
Matter (Density) Labs Packet
Periodic Table Packet
Atomic Structure Packet
Ionic Compounds Packet
Covalent Compounds Packet
Polyatomic Ions Packet
Acids Packet
States of Matter Packet
Nuclear Packet
Directions: Complete the following review packet in order to prepare for your upcoming Chem A Final Exam.
Part 1: Multiple Choice- Periodic Table, Atomic Structure and Density Labs
Choose the best answer from the choices listed.
1. What is the charge of an electron?
a. Positive b. Negative c. Neutral
2. What is the charge of a proton?
a. Positive b. Negative c. Neutral
3. What is the charge of a neutron
a. Positive b. Negative c. Neutral
4. What is the mass of an electron?
a. 0 amu b. 1 amu c. unknown
5. What is the mass of a proton?
a. 0 amu b. 1 amu c. unknown
6. What is the mass of a neutron?
a. 0 amu b. 1 amu c. unknown
7. What does “amu” stand for?
a. Astronomical Measurement Unit
b. Anatomical Metric Unit
c. Average Mortgage Unit
d. Atomic Mass Unit
8. Where are the electrons found inside an atom?
a. nucleus b. electron cloud c. they are outside the atom
9. Where are the protons found inside an atom?
a. nucleus b. electron cloud c. they are outside the atom
10. Where are the neutrons found inside an atom?
a. nucleus b. electron cloud c. they are outside the atom
11. Atomic number is the number of ______in an atom.
a. protons b. electrons c. protons + neutrons d. protons + electrons
12. Mass number is the number of ______in an atom.
a. protons b. electrons c. protons + neutrons d. protons + electrons
13. To calculate the number of ______in an atom you subtract the atomic number from the mass number.
a. protons b. electrons c. neutrons d. nothing
14. The majority of the space inside an atom contains ______.
a. protons b. electrons c. neutrons d. nothing
15. The majority of the mass of an atom is located in the ______.
a. protons b. electrons c. nucleus d. electron cloud
Chemistry A Final Exam Review Name: ______Hour: ______
Chemistry A Final Exam Review Name: ______Hour: ______
Part 1 CONTINUED
16. What is the basic shape of an s-orbital?
a. circle b. square c. heart d. dumbbell
17. What is the basic shape of a p-orbital?
a. circle b. square c. heart d. dumbbell
18. How many electrons can the first electron orbital (shell) hold?
a. 1 b. 2 c. 4 d. 8
19. How many electrons can the second electron orbital (shell) hold?
a. 1 b. 2 c. 4 d. 8
20. Electron configurations can only be abbreviated using ______.
a. Alkali metals
b. Alkaline earth metals
c. Halogens
d. Noble gases
21. Valence electrons are ALWAYS located in the ______of an atom.
a. nucleus b. 1st shell c. 2nd shell d. outermost shell
22. An ion is a….
a. Neutral atom
b. Charged atom
c. Positive atom
d. Negative atom
23. An isotope is a version of an atom with different numbers of…
a. protons b. electrons c. neutrons d. ions
24. All atoms want ______valence electrons in order to be stable (except H and He).
a. 2 b. 4 c. 6 d. 8
25. The two atoms that are exceptions to the above rule are ______and ______because they only want 2 electrons in order to be stable.
a. H and He b. H and Li c. d. La and Ac
26. An atom will give away electrons when forming an ion if it has less than ______valence electrons.
a. 2 b. 4 c. 6 d.
27. An atom will steal electrons when forming an ion if it has ______or more valence electrons.
a. b. 4 c. 6 d. 8
28. Uranium-235 and Uranium -238 are examples of ______.
a. isotopes b. ions c. cations d. anions
29. Uranium-238 has more ______than Uranium 235.
a. protons b. electrons c. neutrons d. valence electrons
30. Hydrogen has an average atomic mass of 1.01 amu. Which of hydrogen’s three isotopes in most abundant (common)?
a. Hydrogen-1 b. Hydrogen-2 c. Hydrogen-3
31. Elements that are found in the same ______of the periodic table have similar chemical and physical properties.
a. Block b. Group c. Period
Part 1 CONTINUED
32. Where are metals located on the periodic table?
a. Left of staircase b. Right of staircase c. Touching staircase
33. Where are nonmetals located on the periodic table?
a. Left of staircase b. Right of staircase c. Touching staircase
34. Where are metalloids located on the periodic table?
a. Left of staircase b. Right of staircase c. Touching staircase
35. Ionic compounds must be made of ______.
Chemistry A Final Exam Review Name: ______Hour: ______
a. Special Metals
b. Metal and Non-metal
c. Two metals
d. Two non-metals
Chemistry A Final Exam Review Name: ______Hour: ______
36. Covalent compounds must be made of ______.
Chemistry A Final Exam Review Name: ______Hour: ______
a. Special Metals
b. Metal and Non-metal
c. Two metals
d. Two non-metals
Chemistry A Final Exam Review Name: ______Hour: ______
37. The density of lead is 11.37 g/mL, while the density of aluminum is 2.70 g/mL. What is true about the density graphs of these two metals?
a. The slope of lead is negative (downhill) and the slope of aluminum is positive (uphill)
b. The slope of lead is positive (uphill) and the slope of aluminum is negative (downhill)
c. Aluminum’s slope is steeper than lead’s slope
d. Lead’s slope is steeper than aluminum’s slope
Chem A Final Review Packet Name: ______Hour: _____ Page 9
Part 2 Short Answer: Periodic Table, Atomic Structure and Density Labs
Refer to the following table to answer questions 1-4
1. Which substance is most dense?
2. Which substance is least dense?
3. A container contains water, aluminum, lead and wood. After shaking the container and waiting for everything to distribute based on density, what would be found on the bottom of the container?
4. What would be found on the top of the container?
5. Consider the following: A student is told to find the density of gold. The mass of the object is found using a balance. The volume is found using a graduated cylinder.
Mass of the object 17.556 g
Volume of water AND gold in graduated cylinder 41.34 mL
Volume of water in graduated cylinder 32.87 mL
6. What is the volume of the gold above? SHOW WORK
7. What is the density of the gold above? SHOW WORK
8. Draw Bohr diagrams for the following elements. You must write the number of PROTONS and NEUTRONS in the nucleus (the circle). Then DRAW and LABEL appropriate number of shells and include ELECTRONS according to the Bohr model.
boron / sodium9. Write the complete electron configuration and abbreviated (noble gas) electron configuration for the following elements. You must write the symbol, atomic number, and mass number.
magnesium
chlorine
krypton
PART 2 CONTINUED
10. Draw the Lewis dot diagrams for the following atoms and their ions.
Oxygen Potassium
11. Uranium has three common isotopes. If the abundance of U-234 (234 amu) is 0.01%, the abundance of U-235 (235 amu) is 0.71%, and the abundance of U-238 (238 amu) is 99.28%. What is the average atomic mass of uranium? SHOW WORK!
12. Titanium has five common isotopes: The abundance of Ti-46 (46 amu) is 8.0%, Ti-47 (47 amu) is7.8%, Ti-48 (48 amu) is 73.4%, Ti-49(49 amu) is 5.5% and Ti-50 (50 amu) is 5.3%. What is the average atomic mass of titanium? SHOW WORK!
13. What is the density of the object graphed below?
14. What is the independent variable on the graph to the left?
15. What is the dependent variable in the graph to the left?
16. Complete the chart below.
***Mass Number may vary from the number listed on the periodic table***
Isotope / Mass Number*** / AtomicNumber / # protons / # electrons / # neutrons
K-40 / 19 / 21
Li-6 / 3
2 / 1
Part 3: Naming Compounds- Ionic, Covalent , Polyatomic AND Acids
· When should you use roman numerals? ______
· When should you use prefixes (mono, di, tri…)? ______
· How do you know there is a polyatomic ion in a compound? ______
· How do you know if a compound is an acid? ______
Formula / Name / Formula / Name1. HClO3 / 8. KMnO4
2. HNO2 / 9. HCl
3. FeBr3 / 10. Pb3(PO4)2
4. N2O / 11. H2S
5. NaHCO3 / 12. BeO
6. H2C2O4 / 13. Hg2Te
7. LiF / 14. BaSO4
Write the formulas for the following compounds.
Name / Symbol w/ ox. # / Formula / Name / Symbol w/ ox. # / Formula16. potassium nitrate / 24. ammonium chloride
17. aluminum thiosulfate / 25. zinc sulfide
18. strontium acetate / 26. dihydrogen monoxide / XXXXX
19. nitrous acid / 27. antimony(III) thiocyanate
20. carbon disulfide / XXXXX / 28. sulfur trioxide / XXXXX
21. silicic acid / 29. hydrochloric acid
22. silver arsenate / 30. potassium dichromate
23. hydroiodic acid
Part 4: All Types of Bonding and States of Matter
Match the following terms with their definition.
Chem A Final Review Packet Name: ______Hour: _____ Page 9
Molecule ______
Intermolecular Force ______
Cation ______
Ionic Bond ______
Anion ______
Ion ______
Polyatomic Ion ______
Metallic Bond ______
Intramolecular Force ______
Covalent Bond ______
a. Attraction between oppositely charged ions
b. Shared pair of valence electrons between 2 nonmetals
c. Attraction for a cation’s loosely held valence electrons
d. Positive ion (lost electrons)
e. Negative ion (gained electrons)
f. Neutral particle of 2 or more atoms bonded together
g. Charged single atom
h. Charged group of atoms
m. Force inside one molecule that holds atoms together
n. Force between multiple molecules
Chem A Final Review Packet Name: ______Hour: _____ Page 9
Fill in the blanks using the word bank provided:
Eight Electrons Cation Eight Covalent Shared Zero Metal Nonmetal
An ionic bond forms between a ______and a ______. When we draw ionic bonds, we use brackets and charges to show that a complete transfer of ______has occurred. The metal is the ______and the nonmetal is the anion. In the final picture, the metal has ______dots around it and the non-metal has ______dots around it.
A ______bond forms between 2 nonmetals. When we draw these bonds, we use bars to show the electrons are being ______between the two atoms. The goal of each atom is to have ______electrons around it, with the exception of hydrogen, which only wants 2 electrons.
Part 4 CONTINUED
Name & Formula / Is it ionic or covalent? / Draw the bond in the box (there is extra room in case you want to show your work)Dihydrogen monoxide
H2O /
Magnesium Oxide
MgO /
Ethyne
C2H2
(C’s in the middle) /
Ethane
C2H6
(C’s in the middle) /
Chlorine molecule
Cl2 /
Methane
CH4 /
Silver oxide
Ag2O /
Part 5: Nuclear Chemistry
1. Why are these reactions called nuclear reactions? ______
2. What is the difference between fission and fusion reactions? ______
______
3. Which radioactive isotope is used in nuclear power plants? ______
4. What are 4 safety precautions taken at nuclear power plants?
a. ______
b. ______
c. ______
d. ______
5. How does the US currently plan to store nuclear waste? ______
6. What is a half life? ______
7. Name 2 benefits or advantages of nuclear power:
a. ______
b. ______
8. Name 2 disadvantages of nuclear power:
a. ______
b. ______