Chemistry 11 Exam Review

v In most cases the emphasis is on ability to apply principles to problem solving not to regurgitation of information.

v Tests, quizzes, labs and all classroom assignments/work can help guide you in preparing for this exam.

Ø Differentiate between the following terms:

· Solid, liquid and gas See your notes

· Physical properties and chemical properties Make a chart to show these

· Physical change and chemical change See your notes

· Atoms, elements and compounds See your notes

Ø Describe the Law of conservation of mass and the Law of conservation of energy

§ Law of conservation of mass - the mass of substances produced (products) by a chemical reaction is always equal to the mass of the reacting substances (reactants).

§ Law of conservation of energy - energy can be transformed (changed from one form to another), but cannot be created or destroyed.

Ø Development of the theory of the atom

· Gas discharge tubes, Dalton, J.J. Thompson, Rutherford, Bohr – go over how each developed their theories, main points of each theory and each model of the atom.

· Determination of atomic number, mass number, electrons, protons, neutrons and the element symbol for both atoms and ions. Refer to charts that we have done for practice.

Name / Symbol / Atomic Mass / Atomic Number / Number of Protons / Number of Neutrons / Number of Electrons
Calcium / Ca / 40 / 20 / 20 / 20 / 20
Neon / Ne / 20 / 10 / 10 / 10 / 10
Krypton / Kr / 84 / 36 / 36 / 48 / 36
Bromine / Br / 80 / 35 / 35 / 45 / 35
Iodine ion / I- / 127 / 53 / 53 / 74 / 54
Cadmium ion / Cd2+ / 112 / 48 / 48 / 64 / 46

· Isotopes and estimating average atomic masses

§ Isotopes are atoms that have the same number of protons but have different numbers of neutrons and therefore differing masses.

§ Nitrogen has two isotopes – N14 and N15 . Nitrogen-14 exists with 99.632% abundance and Nitrogen-15 occurs with 0.369% abundance. Find the average atomic mass of nitrogen

14 x 0.99 = 13.86

15 x 0.01 = 0.15 .

14.01

· Draw Bohr diagrams 7+

· Draw energy level diagrams, and electron configuration diagrams

1s22s22p3

1 ______

s px py pz

Ø The Periodic Table and it’s trends

· Explain the concept of families and relate to oxidation numbers

· Give the names of the families for groups 1, 2, 7, and 8

1-alkali metals, 2-alkaline earth metals, 7-halogens, 8-noble gasses

· Characteristics of metals, nonmetals and metalloids

· Describe the periodic trends in electron configurations

# of electons on valence orbital increase

# of orbitals increases

· Draw electron dot diagrams for various elements

· Give valence electrons for various elements and describe how the valence # is related to the reactivity of elements.

S – 2s23p4 Li – 2s1 Kr – 4s24p6

Tends to gain 2e- Tends to lose 1e- Does not tend to react

· Describe the periodic trends of

a) Atomic size decreases

increases

b) Ionization energy increases

decreases

c) Electron affinity increases

decreases

d) Ionic Size decreases but cations are smaller than anions

increases

Ø Chemical Bonding

· Ionic bonding – dot diagrams and equations

· Covalent bonding types

· Bond polarity

· Molecular polarity

· Molecular geometry

1. Draw the dot notation, and show the equations for ionic bonding for the following combinations **I was unable to do the dot diagrams on here…sorry.

a) Sr & I b) Al & S c) K & P

Sr + energy Sr+2 + 2e- 2Al + energy 2Al+3 + 6e- 3K + energy 3K+ + 3e-

2I + 2e- 2I- + energy 3S + 6e- 3S-2 + energy P + 3e- P-3 + energy

Sr+2 + 2I- SrI2 + energy 2Al+3 + 3S-2 Al2S3 + energy 3K+ + P-3 K3P + energy

2. List some of the differences between ionic and covalent compounds

Ionic / Covalent
Hard / Relatively Soft
High melting point / Low melting point
Conduct electricity in molten and water solution form / Poor conductors
Soluble in water / Limited solubility in water
Strong forces of attraction / Weak forces of attraction
Have regular structures / Irregular structures
Relatively simple compounds / Can create complex compound formulae

3. give examples of a) single covalent bonding

Cl-Cl

b) double covalent bonding

O=O

c) triple covalent bonding

N=N

d) polar covalent bonding

O-H

e) co-ordinate covalent bonding

H-N-H

4. Draw dot, Lewis, structural and orbital diagrams for the following compounds, indicate the bond types (single, double or triple) and the bond polarities for each.

a) C2I2 b) H2CS c) PF3 d) SF2

5. Predict the shapes of the compounds above.

Ø Chemical Naming and formula writing

· Determine the oxidation numbers for atoms of a compound

· Writing chemical formulas and naming of compounds for compounds containing

a) a metal and a nonmetal

b) hydrogen and another element

c) two nonmetals

d) compounds containing one or more polyatomic ions

e) acids

6. Name the following compounds indicating the oxidation number of the underlined elements

CuSO4- Copper II sulfate Mg2C Magnesium carbide N2O3 dinitrogen trioxide

KMnO4 Potassium permanganate AlF3 Aluminum fluoride NaC2H3O2 sodium acetate

OF2 oxygen difluoride Hg3PO4 mercury III phosphate Ni2O3 Nickel III oxide

CF4 Carbon tetrafluoride (NH4)3P ammonium phosphide Ca(ClO3)2 calciumchlorate

Au2S3 gold III sulfide Fe(OH)3 Iron III hydroxide HI Hyroiodic acid

H2SO3 sulfurous acid Sn(S2O3)2 tin II thiosulfate

7. Write formulas for the following chemicals

Silver sulfide Ag2S Barium phosphate Ba3PO4 Tin IV oxide SnO2

Mercury I acetate HgC2H3O2 Phosphoric acid H3PO4 Potassium nitride K3N

Lead II chromate PbCrO4 Dichlorine monoxide Cl2O Calcium carbide Ca2C

Aluminum fluoride AlF3 Bromine trichloride BrCl3 Copper II hydride CuH2

Ø Equations

· Balancing equations

· Chemical reaction types

8. For each of the following, complete the equation where necessary, balance the equation and state the type of reaction.

a) Silver nitrate + zinc ?

2AgNO3 + Zn 2Ag + Zn(NO3)2 single replacement

b) Magnesium chlorate Magnesium chloride + oxygen

Mg(ClO3)2 MgCl2 + O2 decomposition

c) Ammonium sulfide + gold III nitride ?

3(NH4)2S + 2AuN 2(NH4)3N + Au2S3 double replacement

d) Magnesium Nitride + water Magnesium hydroxide + ammonia

Mg3N2 + 6H2O Mg(OH)2 + NH3 double replacement

e) Strontium + Phosphorus ?

3Sr + 2P Sr3P2 Synthesis

f) Si4H10 + O2 SiO2 + H2O

2Si4H10 + 13O2 8SiO2 + 10H2O double replacement

g) C7H6O3 + oxygen water + carbon dioxide

C7H6O3 + 7O2 3H2O + 7CO2 Combustion

h) HbrO3 + HBr H2O + Br2

HbrO3 + 5HBr H2O + Br2 Double replacement

Ø The Mole Concept

· Mole mass determination

· Avogadro’s number

· Conversion between each of the following: grams – moles – molecules – atoms

· Percent composition

· Determination of empirical formula and molecular formula

9. Calculate the number of atoms of antimony in an ingot with a mass of 600.0g.

2.9655x1024 atoms

10. Calculate the mass of silver in a bar of silver that has 4.5 x 1022 atoms of silver.

8.07g

11. Determine the mass of 0.82 moles of aluminum chloride.

109.47g

12. How many molecules of benzene (C6H6) would be contained in a bottle holding 230g?

1.77x1024 molecules

13. The chemical formula for Rolaids is NaAlH2CO4. If you swallowed 8.3 x 1021 molecules of Rolaids, how many grams of Rolaids would that be? 1.77g

14. How many atoms of oxygen is in the above sample? 3.32x1022 atoms

15. The chemical stimulant caffeine has the formula C8H10N4O2. In a cup of coffee that contains 3.5g of caffeine, how many grams of nitrogen would the cup hold?

1.01g

16. The formula for an organic compound is C10H8O. If a person drinks 3.0 x 1021 molecules of the compound, what mass of hydrogen would that person consume? 0.040g

17. What is the % iron in the compound Fe3(PO4)2? 46.8%

18. An organic compound contains 30.3% carbon, 1.7% hydrogen, and 68% bromine. If the molar mass of the compound is 236 g/mol, what is the correct molecular formula?

C6H4Br2

19. The analysis of a 10g sample of a sodium compound shows that in addition to sodium, the compound contains 5.38g of oxygen and 2.69g of sulfur. If the molar mass is 238g/mol, calculate the correct chemical formula. Na2O8S2

20. A sample of organic compound contains 0.225 moles of carbon, 0.328g of hydrogen, and 1.50 x 1022 atoms of nitrogen per 1.5 x 1022 molecules of compound. What is the chemical formula of the compound? C9H13N

Ø Chemical Stoichiometry

· Stoichiometric calculations

· Double Reactions

· Limiter reactions

21. How many grams of hydrogen can be produced from a reaction involving 4.5g of zinc and an excess of hydrochloric acid?

Zn + 2HCl ZnCl2 + H2 Mass of H2 = 0.139g

22. How many grams of water is produced from the following reaction if 5.00g of SiF4 is reacted with 2.00g of NaOH?

SiF4 + 6 NaOH Na2SiO3 + 4NaF + 3H2O

NaOH is the limiter Mass of H2O =0.45g

23. What mass of sodium nitride can be produced form the following double reaction using

3.4 x 1022 molecules of N2O5? N2O5 N2 + O2

Na + N2 Na3N

Mass of Na3N = 9.38g

24. If 34.0g of gold III nitrate reacts with 23.7g of barium chloride, what mass of gold III chloride is formed in this reaction?

2Au(NO3)3 + 3BaCl2 2AuCl3 + 3Ba(NO3)2

BaCl2 is the limiter. Mass of AuCl3 = 23.07g

Ø Organic Chemistry

· Name and draw structural formula for the hydrocarbon families including

a) alkanes

b) alkenes

c) alkynes

d) substituent branches

e) cyclo groups

f) benzenes

g) various functional groups

· Describe and draw structural formula for isomers

· Identify and write balanced equations for hydrocarbon reactions.

25. Name the following organic compounds:

a) CH3-CH-CH2-CH3 b) CH3-CH2-CH-CH=CH2

CH3-CH-CH2-CH3 Cl

3,4-dimethylhexane 3-chloro-1-pentene

CH2- CH3

c) CH3-C=C-CH-CH-CH3 d) CH3-CH2-CH

CH3 CH2 CH2

CH2 CH2

3-ethyl-3-methyl-4-hexyne ethylcyclopentane

26. Draw structural formulas for the following:

a) 3-cloro-2,2,5-trimethylheptane

CH3

CH3-C-CH2- CH2-CH-CH2-CH3

CH3 Cl CH3

b) 4-bromo-2,3-diethyl -1nonene

CH3=C-CH- CH-CH2-CH2-CH2-CH2-CH3

CH2CH2 Br

CH3 CH3

c) Bromocyclopropane Br

CH2 CH2

d) 2,6-dimethyl-3-octyne

CH3-CH-C = C-CH2-CH-CH2-CH3

CH3 CH3

27. Draw and name three structural isomers of the compound C6H10

CH3-CH2-CH2-CH2-C=CH CH3-CH2-C=C-CH2-CH3

1-hexyne 3-hexyne

CH3

CH=C-C-CH3

CH3 2,2-dimethyl-3-butyne

28. Write balanced equations for each of the following:

a) Combustion of 2,3-dimethyl-3-ethyl-pentane

C9H20 + 14O2 9H2O + 10CO2

b) Reaction between 5-ethyl-3,3-dimethyloctane and bromine.

C12H26 + Br2 C12H25Br + HBr