Download semester two review sheet

FUNDAMENTALS
Name: ___________________ Period: ____
SEMESTER TWO FINAL REVIEW SHEET
Below are the types of questions you can expect to see on your final for Fundamentals. The topics are
arranged in the order that we learned the concepts. If there are problems you do not understand, or need
additional practice on, please revisit that unit’s review sheet from my website.
In addition to a periodic table, scientific calculator and ion chart, you may also use this HANDWRITTEN
review sheet. You may choose to answer directly on this sheet or on a separate sheet of paper and attach it.
UNIT 5: CHEMICAL REACTIONS
BALANCING AND TYPES OF REACTIONS
1. Definitions to know: chemical reaction, conservation of mass, endothermic, exothermic, subscript,
coefficient, reactants, and products.
2. Calculate the number of atoms of each element shown in each of the following:
a. Na2SO4
c. Cu(NO3)2
b. 2 MgCl 2
d. Al2(CO3)3
3. Balance each of the following equations:
a. ____ Na2CO3 + ____ HCl  ____ NaCl + ____ H2O + ___ CO2
b. ____ Fe + ____ HCl  ____ FeCl2 + ____ H2
c. ____ F2 + ____ KCl  ____ KF + ____ Cl2
4. What is an exothermic reaction? How could you tell if a reaction was exothermic?
5. What is an endothermic reaction? How could you tell if a reaction was endothermic?
6. Name four factors that can affect the rate of a chemical reaction? Be able to explain each one. As an
example: What would happen to the rate of reaction if: a catalyst was added, a sugar cube was
crushed or 6M HCl was used instead of 2M HCl?
7. What are the seven indicators of a chemical reaction occurred.
8. Identify the types of reactions shown in each of the following equations:
a. CaO + H2O  Ca(OH)2
c. Mg(NO3)2 + KCl  MgCl2 + KNO3
b. 2 Al + NiBr2  AlBr3 + Ni
d. PbO2  Pb + O2
9. Balance the following reactions with polyatomic ions and state which type of reaction it is.
a. ___ AlCl3 + ___ LiOH  ___ Al(OH)3 + ___LiCl
b. ___ Ba(CN)2 + ___ H2SO4  ___ BaSO4 + ___HCN
CARBON BASED MOLECULES (Macromolecules)
1. Definitions to know: monomer, polymer, biochemistry, hydrocarbon, carbohydrate, protein, lipids, and
nucleic acids.
2. What is organic chemistry?
3. What properties of carbon make it the building block of life?
4. What are three examples of pure carbon?
5. How many valence electrons does carbon have and what would the Lewis Dot Diagram look like?
6. Be able to fill in a chart like the one shown below:
MACROMOLECULE
FOOD EXAMPLE
MONOMER
FUNCTION IN BODY
CARBOHYDRATES
BUILD MUSCLE
NUCLEIC ACIDS
NUCLEOTIDES
BUTTER, OIL
ACIDS AND BASES
1. Definitions: acid, base, neutral, amphoteric, and pH scale.
2. Know the chemical formulas for the five common acids (ex. Nitric, phosphoric, etc.)
3. What are three characteristics of acids? What are three characteristics of bases?
4. What is the pH for a substance that is neutral? What is an example of a neutral substance?
5. Know the definition of Bronsted-Lowry acids and know how it is different from an Arrhenius acid.
6. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
NH3 (g) + HOH (l) ⇄ NH4+(aq) + OH-(aq)
7. Identify the acid, the base, the conjugate acid and the conjugate base in the reaction:
HCO3 -(aq) + HOH (l) ⇄
CO3 2-(aq) + H3O+ (aq)
8. Rank these substances from most acidic to most basic: milk of magnesia, water, vinegar, soda, blood,
hydrochloric acid and lye.
UNIT 6: MOLE CONVERSIONS, MOLE RATIOS, EMPIRICAL/MOLECULAR FORMULA
1. Definitions: mole, Avogadro’s number, molar mass, molar volume, molecules (atoms/particles),
empirical formula, molecular formula, and percent composition.
FORMULA MASS, MOLAR MASSES, MOLE CONVERSIONS
1. Calculate the formula mass in a.m.u. of the following:
a. CaSO4
c. H2O
b. RbNO3
d. NaCl
2. Calculate the gram formula mass (molar mass in grams) of the following:
a. Li2CO3
c. CF4
b. AlPO4
d. Mg(OH)2
3. Make the following conversions.
a. What is the number of moles of CaS in 250 grams of the compound?
b. How many moles is 18.06×1023 molecules of SO2?
c. How many molecules of CO2 are in .75 moles?
d. How many moles are in 800 g of HCl?
e. How many moles are in 50 g Fe2O3?
f. How many moles are in 44.8 L of CO2 gas at S.T.P.?
g. What is the volume of 5.6 moles of Cl2 gas at S.T.P.?
h. How many ions of Al=3 are present in one mole of AlCl3?
PERCENT COMPOSITION, EMPIRICAL, AND MOLECULAR FORMULAS
1. What is the percentage composition of all elements in the compound calcium carbonate, Na2CO3?
2. What is the percentage composition of oxygen in ammonium nitrate, Sr(NO3)2?
3. Calculate the percent composition of each element in C6H12O6.
4. Calculate the percent composition of oxygen in N2O.
5. How are empirical and molecular formula related?
6. Determine the empirical formulas for each of the following molecular formulas.
a. C10H20…..
d. C6H12……
b. H2O2……
e. Na2C2O4...
c. Hg2Cl4…..
7. The empirical formula for ethylene is CH. The empirical formula mass is 13 g/mole. Find the molecular
formula if the molecular mass is 78 g/mol.
8. A compound has an empirical formula of OCNCl and an empirical mass that is equal to 77.5 grams. The
molecular mass is 232.41 grams. What is the molecular formula?
MOLE RATIOS
1. Given this equation: N2 + 3 H2 ---> 2 NH3, write the following molar ratios:
a. N2 / H2
b. N2 / NH3
c. H2 / NH3
2. Answer the following questions for this UNBALANCED equation: ___ H2 + ___O2 --> ___ H2O
a. Balance the equation: ___ H2 + ___O2 --> ___ H2O
b. What is the H2 / H2O molar ratio?
c. What is the O2 / H2O molar ratio?
UNIT 7: KINETIC MOLECULAR THEORY AND GAS LAWS
KINETIC THEORY, STATES OF MATTER, TEMP CONVERSION
1. Definitions to Know: Solid, Liquid, Gas, Phase change, temperature, heat, pressure, and absolute zero.
2. What does STP stand for and what are its numerical values?
3. What are the three assumptions of the Kinetic Theory?
4. What are the two temperature scales?
5. Convert the following temperatures from Celsius to Kelvin and Kelvin to Celsius:
a. 25°C
d. 130 K
b. 333°C
e. 40 K
c. -75°C
f. 289 K
PHASE CHANGES AND PHASE DIAGRAMS
1. Be able to label the phases/phase changes on a diagram. As practice, fill in the chart below:
PHASE CHANGE
FROM______ TO _______
ENERGY RELEASED/GAINED
EXO/ENDOTHERMIC
EX: Melting
From Solid to Liquid
Energy gained
Endothermic
2. Know the boiling point and freezing point of water.
3. If given a heating curve like the one below, be able to identify when melting and freezing occur and
answer the following the questions.
a. What is the melting temperature of the
substance?
b. What is the boiling temperature of the substance?
c. What is happening to the temperature at 1, 3,
and 5?
d. What is happening at point 2 and point 4?
e. Label solid, liquid and gas on the curve.
f. On which point of the curve are the particles
moving the least?
g. Where on the curve is ONLY a liquid present?
h. Based on the melting point and boiling point,
could this substance be water?
MIXED GAS LAW PROBLEMS
“R” Constants: 0.0821 L•atm/M•K (For atm)
8.315 L•KPa/M•K (For kPa)
62.4 L•mmHg/M•K (For mmHg)
1. Equations to Know: Dalton’s Law, Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, and Ideal Gas Law,
2. Calculate the temperature of a gas if 6.5 moles of it occupies a volume of 1.5 L at 2.4 atm
3. There is a mixture of three gases in a closed container. Gas A exerts a pressure of 10 psi, Gas B a
pressure of 5.5 psi, and the total pressure is 34.7 psi. What is the partial pressure of Gas C?
4. A gas occupies a volume of 300 cm3 at 200 kPa. What volume will it occupy at 101.3 kPa if the
temperature remains constant?
5. The pressure of a sample of helium in a 4.00 L container is 5.5 atm. What is the new pressure if the
sample is placed in a 2.00 L container?
6. A gas occupies a volume of 4440 cm3 at a temperature of 35°C. Calculate the volume that this gas will
occupy at 74°C if the pressure is held constant (must convert to Kelvin first).
7. A balloon full of air has a volume of 5.0 L at a temperature of 30°C. What is the balloon's volume at
65°C?
8. Calculate the pressure in kPa exerted by a gas if .40 mole occupies 2.5 L at 298 K.
9. A gas has a pressure of 2 atm and a temperature of 289 K. If the temperature increases to 400 K, what is
the new pressure if the volume remains constant?
10. At 315K a gas exerts a pressure on its container of 101.67 kPa. The temperature suddenly drops to 280K,
what pressure does the gas now exert?
11. If I have an unknown quantity of gas at a pressure of 2.4 atm, a volume of 27 liters, and a temperature
of 78°C, how many moles of gas do I have?
UNIT 8: WATER, SOLUTIONS, UNITS OF CONCENTRATION
PROPERTIES OF WATER
1. Define the following terms: polarity, surface tension, vapor pressure, specific heat, and capillary
action.
2. Draw four water molecules. Label the types of bonds (covalent vs. hydrogen), oxygen atoms,
hydrogen atoms, and respective charges on the atoms.
3. Is water polar or nonpolar? Explain.
4. Why is water considered the universal solvent?
5. What are the special properties of water and why do they occur?
6. Explain why solid ice is less than liquid water with regard to particle arrangement.
7. Why does a substance like sugar dissolve in water, but oil does not?
SOLUTIONS
1. Define the following terms: solution, solvent, solute, dilute, concentrated, dissociate, immiscible,
solubility, saturated, supersaturated, and unsaturated.
2. Give an example of solid, liquid, and gas solution. Identify the solute and solvent.
3. What are the factors that affect the solubility of a gas?
4. A glass of water has 10g of sugar dissolved in it. If more sugar can be added to dissolve in the
water, is the solution unsaturated, saturated, or supersaturated?
COLLIGATIVE PROPERTIES
1. What are colligative properties
2. What are four examples of colligative properties and how are they affected (do they
increase/decrease)?
3. Give an example of a colligative property in real-life and explain why/how it is used?
CALCULATING CONCENTRATION
Common Conversion Factors:
1000 g = 1 kg
1000 mL = 1 L
For water 1 g = 1 mL
For water 1 kg = 1 L
1. Definitions: molarity, molality, concentration, ppm,
2. If 4.7 g of Na2CO3 is dissolved in 1000 mL of water, what is the molarity of the solution?
3. How many moles of NaCl would be needed to make 12.5 L of a 1.50 M solution?
4. What is the molarity of a bleach solution containing 6 moles of NaOCl per liter of bleach?
5. What is the concentration in ppm of ethanol in a solution that contains 0.005 g of ethanol dissolved in
11500 kg of water (1 kg = 1g)?
6. Calculate the molarity of a 1.60 L solution containing 0.05 moles of dissolved KBr.
7. If .5g of blood are added to 10.0 kg of water what is the concentration in PPM? (1 kg = 1g)
8. A solution is made up of 120 g NaOH and 440 g water. The total volume is 200.0 mL. Determine the
following:
a. Moles of NaOH
d. PPM
b. Moles of H2O
e. Molarity
c. Molality
9. What is the molality of a solution that contains 2 moles of HNO3 in 5.500 kg H2O?
10. What mass of water in kg is required to dissolve 3.5 moles of NaCl to prepare a 3.75m solution?
SOLUBILITY AND SOLUBILITY CURVES
1. What does like dissolves like mean?
2. Why doesn’t pressure affect solids and liquids?
3. How many grams of NaCl can dissolve in 100 g
of water at 50oC?
4. For most substances, solubility increases as
temperature increases. What are the
exceptions on the graph below?
5. What mass of solute will dissolve in 100g of
water at the following temperatures?
a. KNO3 at 30°C ____________
b. NaCl at 30°C ____________
c. NH4Cl at 70°C ____________
d. Which of the above three substances is
most soluble in water at 15°C.
6. On a solubility curve, the lines indicate the
concentration of a __________________ solution
- the maximum amount of solute that will
dissolve at that specific temperature.
7. Values on the graph ____________ (below,
above, on) a curve represent unsaturated
solutions - more solute could be dissolved at
that temperature.
8. Values on the graph ____________ (below,
above, on) a curve represent supersaturated
solutions – no more solute could be dissolved
at that temperature.
9. Using the solubility graph, determine if the
following solutions are saturated, unsaturated
or supersaturated. If they are anything but
saturated, list two things you can do to make
them saturated (include numbers).
Solution (in 100g
H2O)
10 g of KClO3 at 20oC
o
40 g NaCl at 40 C
o
60 g KNO3 at 40 C
40 g KClO3 at 80oC
Sat, Unsat,
Supersat
+/- how many °C to
make saturated?
+/- how many g to
make saturated?