Download UNIT 1—Water AB

Chem Regular First Semester Final Exam Review
This review is simply a guide. Anything we’ve covered is considered “fair game” on the final. However, we did try to
give example problems from all the topics we’ve studied. So if you run across something during your studying that is not
found on this sheet, please bring it to our attention. The material we cover the week after break is not on this review
sheet, but it will definitely be covered on the final exam.
We’ll let you know about extra final exam review sessions after break.
The resources you will be using for the final exam will include the periodic table, your polyatomic ion list, an activity series, a solubility chart, and a
calculator.
Good luck studying! If you’ve kept up all along, you’ll do fine with this review sheet. If you’ve had trouble, I suggest you find a study buddy to reteach you the things you’re still confused with. Plan your study time NOW so that you’ll leave enough time for each class. Also, make your study
session calendars with classmates now so that your schedule works out for you!
UNIT 1—Water AB
Pp 4-44
1. Review the Foul Water Lab (Procedure and calculations)
Calculating % of water purified
Vocab:

Filtration

Filtrate

Sand filtration

Decanting

Charcoal Adsorption

Distillation

Conductivity
2. Make sure you’re familiar with the water cycle (hydrologic cycle).

What is an example of direct water use? What is an example of indirect water use?
3. Where is the majority of the Earth’s water? Be familiar with the three main physical states that water can be found in.
Vocab

Surface Water

Ground Water

Aquifer

glacier
4. What is density?
a. What is the density of a substance whose mass is 5.7 g and volume is 2 cm x 3 cm x 4 cm?
b. Would the substance in “a” float or sink on water? Explain.
c. What’s the mass of a 50.0 L sample of mercury? (Hg density = 13.6 g/mL)
5. The following data is gathered in the lab to determine the density of water. An empty, dry graduated cylinder is found to
have a mass of 28.45 grams. When the cylinder is filled with 12.5 mL of water, the mass of the cylinder and the water is
found to be 40.65 grams.
a. Determine the density of water according to this data.
b. Compare the value found in this experiment to the text value for the density of water. What is the %
error of this experiment?
6. How many significant digits are in the following numbers?
a. 2.75
b. 2.750 c. 0.00768
d. 1.00768
e. 100
f. 4.70 x 106
7. Calculate each of the following to the correct number of significant figures.
a. 2.80 x 13 b. 45.68 / 0.25
c. 5.86 + 98
d. 400 / 25.0
e. 16.8900 x 3.000
8. Be able to use dimensional analysis to solve problems. Identify the conversion factors. Practice both with these problems.
a. How many seconds are there in 5 days?
b. 250 grams = ? pounds
9. What’s the difference between a physical and chemical property? A physical and chemical change? Give 3 examples
of each.
10. take a break
11. The Metric System!!! Know units for mass, distance, volume. Know prefixes and how to convert.
a. 25.0 grams = ? kg
b. 0.0087 L = ? mL
c. 4,286 cm = ? km
12. Convert each of the following between scientific notation and regular notation
a. 2.5 x 10-3 = ? b. 7.54 x 106 = ? c. 457,800 = ?
d. 0.0000925 = ?
13. Vocab

Element

Compound

Mixture (Homogeneous and Heterogeneous)

Aqueous Solution

Be familiar with the Matter Pyramid developed in class
1
14. Writing formulas of ionic compounds and naming ionic compounds.

Name the following ionic compounds
a. CaCl2
b. CuSO4
c. Ba(NO3)2
d. Fe2(SO4)3

Write the formulas of the following compounds
a. Lithium Oxide
b. Silver Nitrate c. Tin (IV) Phosphate
15. Review properties of ionic compounds.
Vocab:

Ion

Anion

Cation

Polyatomic Ion

Proton

Electron

Neutron
d. Chromium (III) Sulfate
UNIT I—Water CD
Pp. 45-84
1. Review Solubility curves. Especially problems in the Water packet on pages 55-56.
a. How is solubility of an ionic compound in water generally affected by an increase in temperature?
b. How is the solubility of a gas in water generally affected by an increase in tempterature?
c. Using figure 20 on page 46 of your book….

How many grams of Potassium Nitrate will dissolve in 100 g of H2O at 40ºC?

How many grams of Potassium Nitrate will dissolve in 250 g of H2O at 60ºC?

What type of a solution will you have if 75 0grams of Potassium Nitrate is dissolved in 100 mL of
water at 50ºC?

If you want to dissolve 300 grams of Potassium Nitrate in water at 30ºC, how many grams of water
will you need to make sure that all your KNO3 will dissolve?
2. Solution vocabulary

Solute

Solvent

Saturated

Unsaturated

Supersaturated

Precipitate

Dissolve

Solubility

Solution Concentration (definition and math)

Pph, ppt, ppm (definition and math)

Green Chemistry
3. What does it mean when we say that a molecule is polar? Be able to identify whether a substance is polar or non-polar
by…. seeing how it interacts with water or by seeing its molecular structure. Is water polar or non-polar? What does the
following phrase mean… “like dissolves like”? Properties of covalent compounds (polar vs non-polar, MP, types of elements,
solubility, etc).
4. Heavy metal ions are an environmental concern. Why? What metals are considered heavy metals?
5. Acid – Base Chemistry. Determine whether each of the following are acidic, basic, or neutral.
a. pH = 3
b. pH = 7
c. pH = 10
d. Lemon juice e. HCl
f. NaOH
6. What kinds of ions are present in hard water? How is hard water softened?
7. What steps are present in a municipal water treatment plant? How are these steps similar to the steps we went through
in the “Foul Water Lab?”
UNIT II—Materials AB
Pp.94-127
1. Classify each of the following as a physical or chemical property
a. Color
b. Reactivity with an acid
c. Boiling point d. Malleability
e. Flammability
2. Classify each of the following as a physical or chemical change
a. burning of paper
b. melting of a chunk of ice
c. dissolving salt in water
d. boiling water
e. reacting CuCl2 with Al
f. Reacting a penny with nitric acid
3. What are some common properties of metals. Common properties of Metalloids? Common properties of non-metals?
Where are each of these groups found on the periodic table?
4. Woohoo! The Periodic Table!!!!! Who Told the elements where to go? How are elements organized on the table. Be
familiar with the following vocab…

Atomic number

Atomic weight

Mass number

Isotopes

Group or Family
2

Period

Alkali Metals, Noble Gases, Halogens
5. Know the location, mass, and charge of the three main subatomic particles.
6. Review the copper lab. Its steps and the location of the copper during each step.
7. Oxidation and Reduction… In the reaction below, determine which element is getting oxidized and which is getting
reduced.

Cu+2(aq) + Mg(s)  Cu(s) + Mg+2(aq)

3Li + FeCl3  3LiCl + Fe

2Al(s) + 3Zn+2(aq)  3Zn(s) + 2Al+3(aq)
8. Use the activity series (p121 in book or in packet) to predict whether the following reactions will occur.

3Li + FeCl3  3LiCl + Fe

Au + FeCl3  AuCl3 + Fe
9. Mining and Refining- What factors determine whether it is worthwhile to mine a particular metallic ore at a certain site?
Mining Vocab…

Electrometallurgy

Pyrometallurgy

Hydrometallurgy

Ore
10. Take a break
11. For each of the following, determine the mass number, atomic number, number of protons, neutrons and electrons.
a. 40Ca
b. 15N
c. Uranium-235
d. The +1 ion of 23Na
e. The -2 ion of 32S
12. What’s the difference between atomic mass and mass number?
13. What is an isotope?
14. Take a break
15. Identify the four main families(Halogens, Noble gases, Alkalai metals, Alkaline Earth Metals). Identify Metals, Non-metals,
metalloids.
16. What’s an anion? What’s a cation?
17. Fill in the chart below for the following NEUTRAL ATOMS:
ISOTOPE
SYMBOL
ATOMIC
NUMBER
8
MASS NUMBER
NUMBER OF
PROTONS
14
11
23
56
NUMBER OF
NEUTRONS
8
7
21
NUMBER OF
ELECTRONS
20
26
UNIT II—Materials CD
Pp.128-169
1. Identify the type and balance the following reactions:
a. C12H26
+
O2

H2O
+
CO2
b. CuCl2
+
Al

AlCl3
+
Cu
c. H2
+
I2

HI
d. SnCl2
+
Cl2

SnCl4
e. CaCO3
+
HCl

CaCl2 +
H2CO3
f. Solid Sodium reacts with water to produce Sodium Hydroxide and Hydrogen gas
g. A double replacement reaction occurs between Iron (III) Chloride and Sodium hydroxide.
h. The combustion of decane.
2. What is the law of conservation of mater?
3. !!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!THE MOLE!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!! What is it?
4. What’s the molar mass of the following:
a. O2
b. CO2
c. Rn
d. Fe(NO3)3
e. Al2(SO4)3
5. Convert each of the following…
a. Convert 45.0 g of NaCl to moles of NaCl
b. How many atoms are in 2.35 moles of Au?
c. 3.60 x 1022 molecules of water = _____grams of water
d. 0.58 grams of Sodium Sulfate = ________particles of Sodium Sulfate
e. How many particles would there be in a 134 gram sample of HCl?
6. Determine the % of Fe in the compound Fe(NO3)3
3
7. Determine the % composition of each element in Potassium Carbonate
8. Give 3 examples of renewable resources. Give 3 examples of non-renewable resources.
9. Take a break.
10. What is an alloy?
11. What are some methods of modifying surfaces of materials?
12. Review the electroplating demo. At which electrode does oxidation take place? At which electrode does reduction
take place?
13. Vocab:

Recycling

Reuse

Electroplating

STOICHIOMETRY
1. Refer to the following reaction:
FeS + HCl  FeCl2 + H2S
a) If you react 125 moles of FeS with 212 moles of HCl, how many moles of FeCl2 can be produced?
b) Which reactant is the limiting reactant?
c) How many moles of the excess reactant will remain when the reaction has stopped?
2. Refer to the following reaction:
Cl2 + NaBr  NaCl + Br2
a) If you have 36.0 grams of Sodium Bromide and an excess of chlorine, what mass of Br 2 can be produced?
3. Refer to the following reaction:
Aluminum reacts with Hydrochloric Acid to produce Aluminum Chloride and Hydrogen Gas.
a) Write the balanced chemical equation for this reaction.
b) If you react 265.3 grams of Aluminum with 332.4 grams of HCl, how many moles of Aluminum Chloride will be
produced?
c)Which reactant is the limiting reactant?
d) How many grams of the excess reactant will remain when the reaction has stopped?
Predicting products of Chemical Reaction
1. A synthesis (combination) reaction occurs between solid Lithium and Oxygen gas. The product is Lithium Oxide.
2. A double replacement reaction occurs.
Ca(NO3)2 (aq) +
Na2CO3 (aq) ---
3. A combustion reaction occurs when Ethane (C2H6) is burned.
4. Solid Iron is placed in a solution of Cu(NO3)2 (aq).
5. Solid zinc plus aqueous sulfuric acid (H2SO4) in a single replacement reaction yields ….
6. Solid lead plus aqueous sodium nitrate in a single replacement reaction yields ….
7. Water decomposes (this will occur if an electric current is run through the water).
8. Aluminum burning in a synthesis reaction.
9. Solid Magnesium in a solution of Sodium Chloride (single replacement) …..
10. Aqueous copper (II) sulfate plus aqueous barium nitrate in a double replacement reaction yields ….
11. The combustion of the pure liquid benzene, C 6H6.
12. Lithium plus aqueous sodium fluoride in a single replacement reaction yields …
13. A double replacement reaction occurs between Lead (II) Nitrate and Potassium Iodide
14. A double replacement reaction occurs between Strontium Bromide and Ammonium Carbonate.
15. A double replacement reaction occurs between Lithium Oxide and Copper (II) Sulfate.
16. The combustion of Octane (C8H18)
4