S.O.L. Review

Down to the wire!

What do you need to do now?

Eat a good dinner, go to bed at a decent hour.

Be on time for school tomorrow. Eat a good breakfast and avoid

excess caffeine. I will be serving snacks in my room

from 8:15-8:50 Your SOL is in the library at 9:05

What do I need to study?

Review with your flashcards, but remember they do not cover everything

Review the chapter summaries in your textbook

Look over your notes and old tests Look at the ppt on my website USA Test Preps & J-Labs ARE NOT

ENOUGH!!!!!

Gas Laws

P, V?P, T?V, T?What law does this graph

represent?

Chemical or Physical Change?

A banana turns brown Water boils Licking a lollipop Baking bread Soda explodes when you shake it up

Safety

What do you do with waste chemicals? Where do you find information on a

chemical? What equipment protects you from

toxic vapors? Where does broken glass go? What do you do when you get splashed

with a chemical?

Name these chemicals! NaF

sodium fluoride

K2CO3 potassium

carbonate

MgCl2 magnesium

chloride

Be(OH)2 beryllium hydroxide

Ca3(PO4)2 calcium phosphate

(NH4)2SO4

ammonium sulfate

Mn(NO3)3 manganese (III)

nitrate

FePO4 iron (III) phosphate

Write these formulas! potassium fluoride

KF ammonium nitrate

NH4NO3

magnesium iodide MgI2

copper (II) sulfate CuSO4

aluminum phosphate AlPO4

lead (II) nitrate Pb(NO3)2

cobalt (II) selenide CoSe

silver cyanide AgCN

copper (II) carbonate CuCO3

iron (II) oxide FeO

These are covalent, why?

SiF4 silicon tetrafluoride

N2S3 dinitrogen trisulfide

HBr hydrogen bromide (or hydrobromic

acid) Br2

bromine

Write these covalent compounds?

diboron hexahydride B2H6

nitrogen tribromide NBr3

sulfur hexafluoride SF6

diphosphorus pentoxide P2O5

What is the empirical formula?

C2H4O2 CH2O

methane CH4

C6H12O6 CH2O

What do these look like?

carbon disulfide CS2 is linear and non-polar

boron trifluoride BF3 is trigonal planar and non-polar

difluoromethane CH2F2 is tetrahedral and polar

Conversions . . . YEA!

30 grams of H3PO4 0.31 moles

25 grams of HF 1.25 moles

110 grams of NaHCO3 1.31 moles

1.1 grams of FeCl3 0.0068 moles

Moles to mass . . .

4 moles of Cu(CN)2 462 grams

5.6 moles of C6H6 436.8 grams

21.3 moles of BaCO3 4202.5 grams

1.2 moles of (NH4)3PO3 159.6 grams

Moles gas volume . . .

25 Liters of O2

1.12 moles

10 moles of N2

224 L

1.0 x 105 Liters NH3

4460 moles

2.35 x 10-2 moles H2O(g) 0.527 L

Percent Error

If you measured 23 out of 90 74.4% error

If you measured 78 out of 85 8.23% error

If you start with 100g but only recover 43%. 57% error

Balancing Equations

Balance equations because of the Law of Conservation of Matter: the mass of the reactants = mass of products

__N2 + __H2 __NH3

__C6H12O6 + __O2 __H2O + __CO2

__Ca3(PO4)2 + __ZnCl2 __CaCl2 + __Zn3(PO4)2

Percent Yield

My theoretical yield is 500g but actual recovery was only 327g 65.4% recovery

If the recipe is written to yield 24 muffins, but you only got 21 out of them, 87.5% recovery

Molarity!!!!!!!!!!!!!!!!!!!!!!!!

What is the formula for molarity? Molarity = moles solute/L of solution

How do you find moles if you are given mass? Moles = mass / molar mass (periodic chart)

What is the formula for a dilution? M1V1 = M2V2

Calculate it You have 4.5L of a solution that you

added 3.15 moles of NaCl to. 0.7M

How many moles of CuBr do you need to make 10.0L of a 3M solution? 30 moles

What is the volume of a 6.3M solution made from 3.22moles of AgNO3 0.511 L or 511 mL

What are these?

Isotopes? Atomic Number? Ions? Trend in electronegativity? Trend in ionization energy? Trend in atomic mass?

Random Formula for density?

D = m/V Kelvin conversion?

K = C + 273 Ideal Gas Law?

PV = nRT Specific Heat?

cp= q / m x T pH

-log10[H3O+]

What is . . .

Standard temperature and pressure? Oxidation? Reduction? Arrhenius Acid/Base? Bronsted-Lowry Acid/Base?

Who is?

Thomsson? Rutherford? Bohr? Mendeleev? Moseley?

What type of reaction is this? Na + Cl = NaCl

Synthesis

H2O = H2 + O2

Decomposition

CxHyOz + O2 = H2O + CO2

Combustion

A + BX = AX + B Single Replacement

AX + BY = AY + BX Double Replacement

What are these rules?

Aufbau Hund’s Rule Heisenberg Uncertainty Principle Periodic Law Pauli’s Exclusion Principle

Which forces hold these atoms and molecules together?

H2O Intramolecular: Covalent Bond Intermolecular: Hydrogen Bonding

NaCl Intramolecular: Ionic Intermolecular: Ionic

NH3 Intramolecular: Covalent Intermolecular: Dipole-dipole

Organic Compounds

Men Meth- Eat Eth- Popcorn & Prop- Butter But-

Single is –ane Double is –ene Triple is -yne

SOL Review

Speed Round

1. The average kinetic energy of a sample of water molecules is

A. Increased as the temperature is increased

B. Increased as the temperature is decreased

C. Unaffected by temperature changes

D. Always equal to zero

Read each question carefully and choose the best answer.

2. The element chlorine exists as two naturally occurring isotopes. Cl-35 occurs 75% of the time and Cl-37 occurs 25% of the time. Which of the following calculations should be used to calculate the correct average atomic mass of chlorine?

A. (35 amu x .75) + (37 amu x .25)

B. (35 amu x 3) + 37 amu

2

C. (35 amu x 3) + 37 amu

3

D. 35 amu + 37 amu

2

3. The mass of an object was recorded as 9.93 g, 9.90 g, and 10.02 g, using an electronic analytical balance. What is the average of these three masses expressed to the correct number of significant figures?

A. 9.9 g B. 9.95 g C. 10.0 g D. 10.00 g

4. Which of these shows a volume of 1.25 liters expressed in milliliters?

A. 125 mL B. 12.5 x 101 mLC. 1.25 x 102 mLD. 1.25 x 103 mL

5. How does the radioactive isotope C-14 differ from its

stable counterpart C-12?

A. It has a different number of protons and two less neutrons than C-12

B. It has the same number of protons and two more electrons than C-12

C. It has the same number of protons but two more neutrons than C-12

D. It has a different number of protons and two more neutrons than C-12

6. What is the first step that should be taken when a caustic chemical gets into a person’s eyes?

A. Identify the chemical

B. Call for an ambulance

C. Flush the affected area with water

D. Apply a neutralizing agent

7. Which of these conclusions can be drawn from Rutherford’s experiment?

A. Each atom contains electrons.

B. The nucleus of an atom can be split.

C. Each atom contains protons.

D. Atoms are mostly empty space.

8. Group Mass Data forSample X (g)

DisplacementData for Sample

X (mL)

1 2.7 3.4

2 1.20 1.5

3 6.2 7.40

According to the above data, which of the following represents the average density for sample X using the correct number of significant figures?

A. 1 g/mL B. 0.8 g/mL C. 0.81 g/mL D. 0.821 g/mL

1. Which is the correct formula for iron (III) sulfate?

A. Fe3(SO4)2 B. FeSO4

C. Fe2(SO4)3 D. Fe2(SO3)3

2. Which of these represents the empirical formula and the molecular formula, respectively, for a given organic compound?

a) CH and C2H2 b) CH and CH4c) CH2 and C2H2 d) CH3 and C3H12

3. Which of these describes a tendency for atomic radii as displayed on the periodic chart?

A. Atomic radii decrease left to right across a period.

B. Atomic radii increase left to right across a period.

C. Atomic radii decrease top to bottom down a group.

D. Atomic radii increase, then decrease from top to bottom down a group.

4. Chlorine forms a 1- ion. How many electrons does

a chloride ion have?

A. 1 B. 16 C. 17 D. 18

5. Which of the groups below has the electron dot structure shown above?

A. Noble gases

B. Halogens

C. Alkali metals

D. Transition elements

?

6. An element has an electron configuration of

1s22s22p63s2. Which of these will be in the same group as this element?

A. 1s22s22p6

B. 1s22s22p63s23p64s2

C. 1s22s22p63s1

D. 1s22s22p63s23p6

7. Which of these elements is the most chemically active?

A. F B. Cl C. Br D. I

1. What is the percentage of aluminum in

aluminum oxide (Al2O3)?

A. 47% B. 48% C. 53% D. 54%

2. A student wanted to calculate the formula for hydrated copper sulfate. After careful massing, she heated the compound to remove the water. She calculated the formula to be CuSO4

. 4H2O.

The actual formula was CuSO4 . 5H2O. What is the

most likely source of analytical error in the student’s experiment?

A. The water was not completely evaporated from the compound.

B. The actual mass of the anhydrous CuSO4 was less than the measurement.

C. The CuSO4 reacted with elemental copper.

D. The atmospheric pressure prevented complete reaction.

5. Which is an example of a synthesis reaction?

A. HCl + KOH KCl + H2O

B. Pb(NO3)2 + 2HBr PbBr2 + 2HNO3

C. Mg + H2SO4 MgSO4 + H2

D. C + O2 CO2

6. What would be the product(s) of this reaction?

A. 2Mg3Al2O3

B. Mg3Al2 + 3O2

C. 6Mg + Al3O2

D. 3Mg + Al2O3

3MgO + 2Al ?

7. Using the chart above, which of these combinations will probably form a precipitate?

A. Ammonium chloride

B. Barium bromide

C. Calcium chromate

D. Copper (II) carbonate

8.

Very Active Metal + Water Metal hydroxide + ?

Which of these completes this reaction?

A. Oxygen

B. Hydrogen

C. Metal oxide

D. Air

9. A compound is composed of 58.8% C, 9.8% H, and 31.4% O, and the molar mass is 102 g/mol. What is the molecular formula for this compound?

A. C2H10O3

B. C5H5O3

C. C5H10O2

D. CH3O3

10. NaHCO3(s) + HCl(aq) NaCl(aq) + CO2(g) + H2O(g)

Data Table

Evaporating dish + watch glass 42.70 g

Evaporating dish + watch glass 45.20 g+ NaHCO3

Evaporating dish + watch glass 44.45 g + NaCl

A student conducted an experiment and was interested in the mass of the product of the chemical reaction. Some results of the experiment are shown above. What is the mass of the NaCl?

A. 0.75 g B. 1.75 g C. 2.25 g D. 2.50 g

11. A compound is 50% sulfur and 50% oxygen. What is the empirical formula?

A. SO4

B. S2O4

C. SO3

D. SO2

A(s) + B(s) D(g) + heat

12. The reaction shown above is –

A. An endothermic reaction

B. An exothermic reaction

C. A decomposition reaction

D. A double-replacement reaction

13. Which compound contains both ionic and covalent bonds?

A. NH4Cl

B. MgBr2

C. CH4

D. NH3

1. One of the main assumptions of the kinetic molecular theory of gases is that the particles of an ideal gas—

A. must be single atoms instead of molecules

B. are in constant motion

C. must be maintained at very high pressures

D. must be highly chemically reactive

2. A sample of oxygen gas is collected over water at 220C and 98.67 kPa pressure. If the partial pressure of the water is 2.67 kPa, the partial pressure of the oxygen is –

A. 93.3 kPa

B. 96.00 kPa

C. 98.66 kPa

D. 101.33 kPa

3. If the pressure exerted on a confined gas is doubled, then the volume of the gas --

A. increases four times

B. decreases by one-fourth

C. is doubled

D. is halved

4. Water can be made to boil above its normal boiling point of 100oC by –

a. decreasing the air pressure

b. increasing the air pressure

c. increasing the heat being applied

d. decreasing the volume of the container

5 10 15 20 25

50

25

0

-25

Time(min)

Tem

pera

ture

(

oC

)

5. An experiment yielded the above temperature and time information. What is the freezing point of the material in this experiment if the material is a solid at time zero?

a. –25oC

b. 0oC

c. 25oC

d. 50oC

2H2S (g) + 3O2 (g) 2H2O (g) + 2SO2 (g)

6. If 3.50 g of H2S are used in the above reaction, what will be the theoretical yield of water in grams?

A. 0.102 g

B. 0.185 g

C. 1.85 g

D. 185 g

CH4 + 2O2 CO2 +2H2O

7. The number of grams of oxygen required for the complete combustion of 4.00 grams of methane (CH4) is—

A. 4.00 g

B. 8.00 g

C. 16.0 g

D. 32.0 g

1. A solution contains 225 g of glucose, C6H12O6, dissolved in enough water to make 0.825 L of solution. What is the molarity of the solution?

A. 0.66 M B. 0.97 M C. 1.03 M D. 1.52 M

Read each question carefully and choose the best answer.

2. Which volume will be occupied by a gas containing 6.02 x 1023 atoms at STP?

A. 1.0 L

B. 11.2 L

C. 22.4 L

D. 44.8 L

3. How many milliliters of 2.00 M H2SO4 are needed to provide 0.250 mole of H2SO4?

A. 125 mL

B. 1.25 x 101 mL

C. 8.00 x 103 mL

D. 8.00 mL

4. A catalyst accelerates a chemical reaction because the –

a. catalyst decreases the number of collisions in a reaction

b. activation energy of the reaction is lowered in the presence of a catalyst

c. catalyst decreases the concentration of the reactants

d. temperature of the reaction increases due to the catalyst

5. In the reaction 2SO2 (g) + O2 (g) 2SO3 (g), which change would cause the greatest increase in the concentration of SO3?

a. Decrease the concentration of SO2

b. Decrease the concentration of O2

c. Increase the concentration of SO2

d. Increase the concentration of O2

6. The hydrogen ion concentration is 1 x 10-7. What is the pH of this solution?

a. 1

b. 7

c. 10

d. 14

7. Each beaker shown above contains 2.2 grams of iron and 1 liter of 3M H2SO4. Which reaction will go to completion first and why?

a. Beaker A because of increased surface area.

b. Beaker B because of increased surface area.

c. Beaker A because of a higher concentration level.

d. Beaker B because of a higher concentration level.

8. Four aqueous solutions and their concentrations are shown in the above illustration. Which of the solutions is most likely to be the strongest conductor of electricity?

a. I

b. II

c. III

d. IV

9. If the temperature of a reaction is increased, the reaction proceeds at a much quicker rate because the –

a. Activation energy increases

b. Energy of the products increases

c. Frequency of collisions between reactants increases

d. Energy of the activated complex increases

10. The formula H2SO4 is representative of which of the following?

a. A catalyst

b. A base

c. An acid

d. An organic compound

11. To remove the sand first and then the salt from a mixture of sand and salt water, one combination of techniques you could use would be to first—

A. evaporate and then distill

B. evaporate and then condense

C. filter and then evaporate

D. filter and then condense

12. A student must make a 3M acid solution using a 5M acid solution. Which of these is the safest way to make the solution?

a. Slowly pour the 5M acid into water.

b. Slowly add water to the 5M acid solution.

c. Mix half the acid with water; then add the remaining water.

d. Mix half the water with acid, then add the remaining acid.

First 6 Weeks SOL Answers

1. A2. A3. B4. D5. C6. C7. D8. C

Second 6 Weeks SOL Answers

1. C2. A3. A4. D5. B6. B7. A

Third 6 Weeks SOL Answers

1. C2. A3. B4. C5. D6. D7. D8. B

9. C

10. B

11. D

12. B

13. A

Fourth 6 Weeks SOL Answers

1. B

2. B

3. D

4. B

5. B

6. C

7. C

Fifth 6 Weeks SOL Answers

1. D 6. B 11. C

2. C 7. B 12. A

3. A 8. B

4. B 9. C

5. D 10. C