Part 1: Complete the chart below using a periodic table



Chemistry: Semester 1 Final Exam Review Name: _________________________

The chemistry final exam is on Wednesday, January 21 (hours 1-3) and Thursday, January 22 (hours 4-6). It consists of 38 multiple choice questions and 8 short answer questions.

Clickers – What do I need to study in order to be ready for the final?

|Clicker |Concept |Check if INCORRECT |Review Packet |Book Pages to Read |Book Practice Problems |

| | | |Problems | | |

|1 |models of the atom | |1-3 |p. 102-108, p. 127-130 |p. 108: 14; p. 132: 1-3 |

|2 |protons, neutrons, and electrons | |4-8 |p. 110 |p. 111: 15, 16 |

|3 |protons, neutrons, and electrons | |4-8 |p. 111 |p. 122: 50 |

|4 |isotopes | |9 |p. 112 |p. 113: 20; p. 116: 21 |

|5 |nuclear reactions | |10 |p. 800-802 |p. 808: 12 |

|6 |valence electrons | |11-13 |p. 187-188 |p. 193: 7 |

|7 |ion charge | |11-13 |p. 188- 192 |p. 193: 5, 6, 9 |

|8 |electron configuration | |14-15 |p.133-135 |p. 135: 8; p. 151: 70 |

|9 |naming ionic compounds | |16 |p. 261, 266 |p. 282: 67 |

|10 |naming covalent compounds | |16 |p. 268-269 |p. 270: 22 |

|11 |writing formulas of compounds | |17 |p. 262-265, 270 |p. 263: 11; p. 265: 13; p. 270: 24|

|12 |types of reactions | |19 |p. 330-336 |p. 339: 24 |

|13 |predicting products of reactions | |20 |p. 337-339 |p. 339: 26 |

|14 |predicting products of reactions | |20 |p. 337-339 |p. 339: 26 |

|15 |balancing equations | |21-22 |p. 324-327 |p. 327: 3; p. 328: 5 |

|16 |balancing equations | |23 |p. 324-327 |p. 327: 3; p. 328: 5 |

|17 |molar mass | |24 |p. 293-296 |p. 315: 53 |

|18 |mole conversions | |25-26 |p. 297-299 |p. 315: 58a-c, 59a-c |

|19 |stoichiometry | |27-30 |p. 359-362 |p. 361: 13 |

|20 |rate of reactions | |31-33 |p. 545-547 |p. 547: 2, 4, 5 |

Unit 1: Atomic Structure and the Periodic Table

Models of the Atom

1. Complete the chart below about the five different models of the atom:

|Model |Drawing |What does this model tell us about the structure of the atom? |

|Dalton | | |

| | | |

|Thomson | | |

| | | |

|Rutherford | | |

| | | |

|Bohr | | |

| | | |

|Quantum | | |

| | | |

2. Explain one similarity and one difference between Thomson’s model of the atom and Rutherford’s model of the atom.

3. Explain one similarity and one difference between Rutherford’s model of the atom and Bohr’s model of the atom.

Protons, Neutrons, and Electrons

4. How do you determine the number of protons in an atom?

5. How do you determine the number of electrons in an atom?

6. How do you determine the number of neutrons in an atom?

7. Because atoms are electrically neutral, the number of _______________ must equal the number of _______________.

8. Use a periodic table to complete the chart below:

| |Element |Atomic Symbol |Atomic Number |# of Protons |# of Electrons |# of Neutrons |Mass Number |

|b |Potassium | | | | | |39 |

|a |Lithium | | | | | | |

|b |Oxygen | | | | | | |

|c |Potassium | | | | | | |

|d |Chlorine | | | | | | |

|e |Aluminum | | | | | | |

9. List two elements that have similar chemical and physical properties to barium.

10. Why do the elements you chose have similar chemical and physical properties to barium?

Electron Configurations

11. How many electrons can the following subshells hold?

s subshell: __________ p subshell: __________

d subshell: __________ f subshell: __________

12. Use a periodic table to complete the chart below:

| |Electron Configuration |Element |# of Valence Electrons |Shorthand Electron |

| | | | |Configuration |

|a |1s22s22p63s23p64s23d2 | | | |

|b |1s22s22p63s23p64s1 | | | |

|c | |phosphorous | | |

|d | |fluorine | | |

|e | |calcium | | |

Unit 2: Ionic and Covalent Compounds

Naming Ionic and Covalent Compounds

13. Circle whether the following compounds are ionic or covalent and then name the compounds:

a) MgBr2 Ionic/Covalent ___________________________________

b) SnF4 Ionic/Covalent ___________________________________

c) Ca(NO3)2 Ionic/Covalent ___________________________________

d) (NH4)2O Ionic/Covalent ___________________________________

e) Fe3(PO4)2 Ionic/Covalent ___________________________________

f) SiF4 Ionic/Covalent ___________________________________

g) KCl Ionic/Covalent ___________________________________

h) BaSO4 Ionic/Covalent ___________________________________

i) PbI2 Ionic/Covalent ___________________________________

j) N2S3 Ionic/Covalent ___________________________________

Writing Formulas for Ionic and Covalent Compounds

14. Fill in the chart below to show the transfer of electrons when calcium and phosphorous form an ionic bond. Then write the resulting chemical formula.

| |# of valence electrons |Lewis Dot Diagram |Will it lose or gain electrons? How |

| | | |many? |

|Calcium (Ca) | | | |

|Phosphorous (P) | | | |

|Chemical Formula | | | |

15. Circle whether the following compounds are ionic or covalent and then write the formulas for the compounds:

a) lead(IV) oxide Ionic/Covalent _________________________

b) aluminum bromide Ionic/Covalent _________________________

c) nitrogen tribromide Ionic/Covalent _________________________

d) ammonium sulfate Ionic/Covalent _________________________

e) sodium phosphate Ionic/Covalent _________________________

f) copper(II) nitride Ionic/Covalent _________________________

g) lithium sulfide Ionic/Covalent _________________________

h) diphosphorus pentoxide Ionic/Covalent _________________________

i) iron(II) carbonate Ionic/Covalent _________________________

j) potassium chlorate Ionic/Covalent _________________________

Unit 3: Chemical Reactions

Types of Reactions

16. Identify the following types of reactions (synthesis, decomposition, combustion, single replacement, or double replacement):

a) C6H14 + O2 → CO2 + H2O _________________________

b) AgNO3 + Ni → Ni(NO3)2 + Ag _________________________

c) Ca(C2H3O2)2 + Na2CO3 → CaCO3 + NaC2H3O2 _________________________

d) NaClO3 → NaCl + O2 _________________________

e) Ca + HCl → CaCl2 + H2 _________________________

f) Cu + S8 → CuS _________________________

g) C3H8 + O2 → CO2 + H2O _________________________

h) BaCO3 → BaO + CO2 _________________________

i) AgNO3 + K3PO4 → Ag3PO4 + KNO3 _________________________

j) K + H2O → KOH + H2 _________________________

Predicting Reaction Products

17. Identify the type of reaction, and then predict the products:

a) HNO3 + Ni → Type of reaction: _________________________

Products: HNO3 + Ni → _________________________

b) Ca(OH)2 + HCl → Type of reaction: _________________________

Products: Ca(OH)2 + HCl → _________________________

c) Li + Cl2 → Type of reaction: _________________________

Products: Li + Cl2 → _________________________

d) Zn + H2SO4 → Type of reaction: _________________________

Products: Zn + H2SO4 → _________________________

e) LiNO3 + K3PO4 → Type of reaction: _________________________

Products: LiNO3 + K3PO4 → _________________________

Balancing Chemical Equations

18. What is the law of conservation of mass?

19. Why must equations be balanced?

20. Balance the following equations:

a) _____ Al(OH)3 + _____ H2CO3 → _____ Al2 (CO3)3 + _____ H2O

b) _____ Al + _____ S8 → _____ Al2S3

c) _____ Cs +_____ N2 →_____ Cs3N

d) _____ Mg +_____ Cl2 → _____ MgCl2

e) _____ Rb +_____ RbNO3 →_____ Rb2O +_____ N2

Unit 4: Stoichiometry (or Calculating Chemical Quantities)

Molar Mass and Mole Conversions

21. Calculate the molar mass of the following:

a) CO2 __________

b) Na2SO4 __________

c) Cu(NO3)2 __________

22. Calculate the number of moles in the following:

a) 964 g Na2SO4

b) 23.7 g Cu(NO3)2

23. Calculate the number of grams in the following:

a) 5.15 moles Na2SO4

b) 0.97 moles Cu(NO3)2

Stoichiometry

24. In the reaction below, what is the ratio of moles of iron (Fe) used to moles of iron chloride (FeCl3) produced?

___Fe + ___Cl2 ( ___FeCl3

25. How many moles of sodium carbonate (Na2CO3) are needed to react completely with 3.0 moles of calcium hydroxide (Ca(OH)2)?

___Na2CO3 + ___Ca(OH)2 ( ___NaOH + ___CaCO3

26. When 13.5 g of calcium chloride react with an excess of silver nitrate, how many grams of silver chloride are produced?

___CaCl2 + ___AgNO3 ( ___Ca(NO3)2 + ___AgCl

27. Iron (III) oxide and hydrogen gas are heated to form metallic iron and water. How many grams of iron are produced by heating 12.4 grams of iron (III) oxide?

Unit 5: Rates of Reactions

28. What effect does each of the following have on the rate of a reaction? Explain your reasoning.

a) Switching from a powder reactant to a solid block of the same reactant

b) Adding more of a reactant

c) Keeping the temperature constant using a water bath

29. A 6.0 g sample of Mg reacts with HCl in two different experiments. The reaction for both was:

Mg + 2HCl → MgCl2 + H2

In the first experiment, it took 6.2 minutes for all the Mg to react. In the second experiment, it took 10.8 minutes for all the Mg to react. What are some possible explanations for the change in rate in the second experiment?

30. Using a drawing, explain why increasing the surface area increases the rate of a reaction.

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