Answers to Monster Review:

SECTION 1

1. A

2. C (assuming it's straight from a cow or goat---you get the idea)

3. B Remember H₂ is still an element because it consists of just one type of atom.

4. D

5. D

6. D ( There are many substances that are liquids at room temperature)

7. C

8. A ( That's a characteristic property of hydrogen.)

9. D ( Treat sulfur as a non-metal to answer this question.)

10. C

11. C

12. D

13. A ( Rutherford discovered this with his gold-foil experiment.)

14. C

15. A

16. B

17. A

18. B

19. B

20. D

21. C

22. B

23. A

24. D

25. C

Section 2

1. Yes. The indicators of chemical change in this experiment are the following:

· There is a change of colour: from white to grey.

· There is a gas released too, suggesting that a compound decomposed

· A change in chemical properties occurred since, unlike the original, the new substance is flammable

2. Any four of the following properties of metals will suffice:

Physical group characteristic properties	Chemical group characteristic
Malleable	React with acid
Ductile	React with non-metals
Higher melting points than non-metals	Form alloys with themselves but don't react with other metals
Good conductors of heat and electricity	Lose electrons in chemical reactions
With a couple of exceptions, usually solid at room temperature

3. Draw an electron configuration (shell-diagram; Bohr-Rutherford diagram) for each of the following:

a. O 8p 2e) 6e

b. K⁺¹ 19p 2e)8e)8e (notice it lost an electron)

4. By referring to their atomic structure, explain why the alkali metals are highly reactive.

Each alkali metal (Li, Na, K etc) has one valence electron. By losing one electron, they will end up with noble gas electron arrangements, which are very stable. So anything that comes along that is willing to accept an electron like a halogen, other non-metal, acid or water will react with members of this family or group.

5. Complete the following table:

Neutral element/ion	Atomic #	# of protons	# of electrons	# of neutrons	Mass #
Fe^+2				29
C			6	8
^19F^-1
^197Au
		4	2	5

Neutral element/ion	Atomic #	# of protons	# of electrons = protons - charge	# of neutrons = mass - protons	Mass # = Protons + neutrons
Fe^+2	26	26	26-2 = 24	29	26 + 29 = 55
C	6	6	6	8	6 + 8 = 14
^19F^-1	9	9	9-(-1) = 10	19 - 9 = 10	19
^197Au	79	79	79	197 - 79 = 118	197
^9Be^+2	4	4	2	5	4 + 5 = 9

6. Hydrogen's spectrum will not be tested. Other classes are too wimpy to do this stuff!

7. a. Ge or Sb

b. Ne

c. O

d. Be

8. a. Na

b. Br

9. a. sodium oxide

b. calcium sulfate

c. iron (III) hydroxide ( 430 only)

10. a. CO

b. N₂O₄

11. a. Draw one dot around Li and seven around Cl; then use an arrow to show that Li loses its electron to Cl.

b. C shares three of its electrons with N and one with hydrogen.

c. you need one ring and three double bonds or 4 double bonds and no rings. Other possibilities also exist.

12. a. Li

b. F

c. Si

d. He

e. B

f. Fr

g. Br

13. 0.10(268) + 0.40(269) + 0.50(270) = 269.4 u

14. The mass increased because we had not originally weighed the amount of oxygen that reacted.

15. a. Mg + 2 HCl à MgCl₂ + H₂

b. 2 Mg + O₂ à 2 MgO

c. already balanced

d. 3 Cl₂ + 2 CrBr₃à 3 Br₂ + 2 CrCl₃

e. already balanced

f. already balanced

g. Zn + 2 AgNO₃ à Zn(NO₃)₂ + 2 Ag

h. KClO₃ + 3 Na₂SnO₂ à KCl + 3 Na₂SnO₃

i. 4Al + 3 O₂ à 2 Al₂O₃

16. a. 4 moles

b. 194 g

c. 0.0133 moles

d. 0.05 moles

e. 70.56 g

f. 0.0129 moles

g. multiply by 6.02 X 10²³ = 6.62 X 10²³ molecules.

17. 3/x =2/0.123

x = 0.0185 moles.

Review #2

1. A

2. C

3. C

4. C N₂ + 3 H₂ --> 2 NH₃

28 + 3*2 = 34 g

5. C

6. D

7. A

8. D

9. D

10. D 2*18 = 36 g

11. B 440/44 =10 moles

12. D

13. C 153/102 = 1.5 moles

ratio : 1.5 moles (4 moles Al / 2 moles AlCl₃)

x = 3 moles of Al

3 *27 = 81 g

14. D

15. B 4 Fe + 3 O₂ --> 2 Fe₂O₃

1000g/(2*56 + 3*16) = 6.25 moles of Fe₂O₃

3/x = 2/6.25

x = 9.4 moles of O₂

16. B 50/(40 + 12 + 48) = 0.50 moles

ratio is 1:1 so 0.50 mole of water is produced

0.5 mole*18g/mole = 9 g

17. D They meant sodium chloride is produced. 100/(23+16+1) = 2.5 moles of NaOH

ratio is 1:1 so 2.5 mole of sodium chloride (NaCl) is produced = 58.5 g/mole*2.5 = 146 g

18. C 219/36.5 = 6 moles of HCl

2/6 = 1/x

x = 3 moles of H₂ = 3 *2 g/mole = 6 g

19. B

20. A

21. B

22. A 12g/(100 + 3*100)ml =12/400 = 0.3g/mL

23. C C₁V₁ = C₁V₂

1 V₁ = 3(0.2) = 0.6 L

24. D 0.5/.050 = 10 moles/L

25. 2.5*6.02 X 10²³ = 1.5 X 10²⁴ molecules

26. 10*2.5 *6.02 X 10²³ =1.5 X 10²⁵ molecules

27. C₁V₁ = C₁V₂

20 V₁ = 12(0.050)

V₁ = 0.030L

Pipette 30 ml of the original.

Transfer to a 50 ml volumetric flask.

Add water to the mark and mix.

28. 2 HCl + Mg(OH)₂ --> 2 H₂O + MgCl₂

29. 10/63.5 = 0.157 moles of Cu

2 Cu + O₂ à 2 CuO

2/0.157 = 1/x

x = 0.0787 moles of O₂

0.0787 moles of O₂ *32 g/mole = 2.5 g.

30. Surround each K+ with a few water molecules, making sure that each ion faces the oxygen atoms, which have a partial negative charge. Do the same for the Cl^- ions, but make sure that the ions face the water’s hydrogen atoms, which have a partial positive charge.

31. The positive sodium ions attract electrons from the power source and the negative chloride ions return electrons to the circuit.

32. Electrolytes, which are composed of ions, conduct electricity and react more quickly. Non-electrolytes are slower to react, and they do not conduct electricity.

33. (1) Acids produce H+ ions in solution; bases produce OH^-.

(2) Acids are sour-tasting; bases are bitter.

(3) Acids turn blue litmus red; bases turn red litmus blue.

(4) Acids release hydrogen gas when in contact with many metals; bases do not;

(5) Acids feel wet before burning; bases fell slippery.

Stoichiometry Review

1. 289.5 g/mole or amu(atomic mass units)

2. 20.2 moles

3. 6.35 g

4. 3.34 X10²² molecules

5. a. 15 moles

b. 0.30 moles

c. 33 g

d. 250 g

Want even more practice? Do Review 1 to R12, where it says “sample questions”. Where? Go here.