Chemistry Fall Final Study Guide
Unit 1: Matter, Elements & the Periodic Table
1. How many sig figs are in the following numbers?
a. 89,501
b. 0.0290
c. 5,700
d. 2,000.
e. 0.30600
2. Use the Conversion Factor Sheet in your Glossary to solve the following problems. Show your work
using bridges and correct amount of sig figs in your answer!
a. How many hours is 23,870 minutes?
c. How many mm Hg are in 3.5 atm?
b. How many seconds are in 28 hours?
3. What is matter? Name 3 things that are matter and 3 things that are NOT matter.
4. What is the different between a physical property and a chemical property?
5. Label the following properties of matter as either physical or chemical:
a. Calculating the density of gold
d. Bleaching your hair
b. Salt dissolving in water
e. Shooting off fireworks
c. Melting Ice
f. Sublimation of dry ice
6. Solve the following density problems. Round to the correct number of sig figs.
a. What is the density of a piece of wood that has a mass of 25.0 grams and a volume of 29.4 cm3?
b. Mercury metal is poured into a graduated cylinder that holds exactly 22.5 mL. The mercury used
to fill the cylinder weighs 306.0 g. From this information, calculate the density of mercury.
c. What is the weight of the ethyl alcohol that exactly fills a 200.0 mL container? The density of
ethyl alcohol is 0.789 g/mL.
d. What volume of silver metal will weigh exactly 2500.0 g. The density of silver is 10.5 g/cm3.
7. How is the periodic table organized? What are groups and periods?
a. Where are the metals found on the periodic table? Where are the nonmetals found on the periodic
table? What is Hydrogen?
b. What are the names for the groups 1A, 2A, 3B-12B, 7A and 8A?
8. On the periodic table, what are the trends for atomic mass atomic numbers, atomic radii (size), and
reactivity as you move across a period and down a group?
Unit 2: Atomic Structure
9. Which part gives the identity of the atom? Which part(s) make up most of the (atomic) mass of the
atom? Which makes up very little?
10. What does the periodic table tell us about the parts of the atom:
a. Find the following for the atoms Aluminum, Chlorine, and Magnesium:
i. Atomic #
vi. # of valence electrons
ii. # of protons
vii. # of core electrons
iii. # of electrons
viii. # of neutrons for 2 of its
iv. Average atomic mass
isotopes
v. Name of the group it is in
ix. Draw the 2 isotopes of the
(NOT the #)
atom
11. What is the atomic number and atomic mass of phosphorus and strontium?
a. What is the difference between atomic number and atomic mass?
12. What is an isotope? Name two possible isotopes for carbon and potassium. Use isotope symbol.
13. a. Write the equation for the alpha decay of astatine -213.
b. Write the equation for the beta decay of neptunium -239.
c. What is more harmful alpha particles, beta particles, or gamma rays?
14. What are valence electrons?
a. How many valence electrons do Mg, S, and Al have?
15. Answer the following for the atoms of Carbon, Barium, and Bromine:
a. How many total electrons does it have?
b. How many valence electrons are there?
c. How many core electrons are there?
d. How many shells will it have?
16. What elements with the following electron configurations of
a. 1s22s22p63s23p64s23d104p1
b. 1s22s22p63s23p4
17. Write the electron configuration for each of the following atoms: Be, Si, Tc, I and Cs.
Unit 3: Chemical Bonding
18. What are ions? What are cations and anions?
19. In ionic bonds, metals tend to lose electrons and nonmetals gain electrons. What happens to these
elements to achieve noble electron configuration? What charge will the element form?
a. oxygen
b. chlorine
c. sodium
d. barium
20. Fill in the following chart:
Group #A
# valence eIA
II A
III A
IV A
VA
VI A
VII A
VIII A
Lose/gain e-?
Oxidation #?
Type of ion?
21. a. What is the chemical formula and name of the compound formed when beryllium reacts with
fluorine?
b. What is the chemical formula and name of the compound formed when potassium reacts with sulfur?
22. What is a crystal lattice? Why do ionic compounds form a crystal lattice structure? Draw a picture of
NaCl in a crystal lattice.
23. What are the chemical formula and charge for the following polyatomic ions?
a. Sulfate
b. Hydroxide
c. Nitrate
d. Nitrite
e. Sulfite
f. Chromate
g. Carbonate
h. Ammonium
24. Write the correct name for the following compounds:
a. Fe2(SO3)3
c. Na3PO4
b. RbI
d. CuCl2
e. Ti3P2
25. What are isomers? Draw the three isomers for C3H9N.
26. What is the HONC1234 and Octet rule? Which molecules obey the Octet rule? Draw the Lewis Dot
structures for the following molecules.
a. CF3
b. PCl2
c. OCl2
d. SiI4
27. What does VSEPR mean?
28. What is the difference between lone pairs and bonded electron pairs?
29. Fill in table.
Molecule
Lewis Dot
Structure
Structural
Formula
Lone pairs
on central
atom
Bonded pairs on
central atom
Shape of
Molecule
CO2
SeCl2
NH3
CH4
CH2O
30. Write the molecular formula, structural formula, Lewis Dot structure, and ball-and-stick formula for
water, methane, and carbon dioxide.
31. What are the different characteristics between a polar vs. nonpolar molecules? (ex: dissolve in water,
attraction to a negatively charged wand, on wax paper).
32. How do you use the electronegativity values chart to determine nonpolar covalent, polar covalent, and
ionic bonds? What is happening to the electrons in these different bonds?
33. Determine type of bond between these atoms: Cl-Cl, As-H, Ca-O, P-I, K-Cl, and F-Si
34. Are the following molecules polar or nonpolar molecules? Explain
a. SiF4
b. PI3
c. SCl2
d. SiS2
35. What are intermolecular forces?
36. What are three types of intermolecular/ van der Waals forces? Which is the strongest? Weakest?
37. Explain how electronegativity can help determine the bond type in a molecule.
38. Explain how you can tell if an entire molecule will be polar or nonpolar.
39. Fill in the following chart:
Molecule
Lewis Dot
Structure
(use Octet
Rule)
Structural
Formula
(use HONC
1234)
Shape
1. sketch ball & stick model
2. Write name of shape
3. Show direction of all
dipoles (e- pull) according
to electronegativity
difference
Is the
entire
molecule
Polar or
Nonpolar?
Can we
smell
it?
Will it
dissolve
in water?
Type of
IMF?
(Intermolecular
Force)
CBr4
H2Se
CH2S
AsH3
HSiF3
Unit 4: Biochemistry
40. What are the different functional groups, the smells associated for each, and their common names
endings?
41. What are chemical reactions? Where do they take place in the molecule? What is happening in the
molecules when chemical reactions occur?
42. What are reactants? Products?
43. Explain the collision theory.
44. What is activation energy?
45. What is a catalyst? What does it do?
46. What are carbohydrates and how are they used by living organisms?
47. Complete the following chart:
Carbohydrate
Monosaccharides
Disaccharides
Polysaccharides
Examples
48. What are lipids and how are they used by living organisms?
49. What are proteins and how are they used by living organisms?
50. What is the structure of amino acids? Which functional groups are present? What does the “R” stand
for?
51. What type of bond holds proteins together?
52. What are the 2 types of nucleic acids and what are their functions?
53. What type of bond is found in alkanes? Alkenes? Alkynes?