Final Review Trimester 1 – MURPHY
Name___________________________
Summer Work – Chapters 1-2
1. Write the following numbers in scientific notation. Be sure to show the correct number of significant digits.
12,000 __________________________
.00012 __________________________
56.7000 __________________________
100000 __________________________
2. Circle all digits that are significant in the numbers listed below.
100 .2030
.003040 1,000.0
3. Name each of the compounds below.
a.CaCl2_______________________ b. LiNO3_____________________________
c. Cu2(CrO4)_____________________ d. NH4Br_____________________________
4. Write the formula for each of the following compounds using the ions table provided.
a. strontium fluoride_______________ b. ammonium sulfide____________________
c. potassium carbonate_____________ d. tin(III) sulfate________________________
5. Determine the density of a substance that has a mass of 4.56 kg and a volume of 5,460 mL.
You answer should be in grams per cubic centimeters.
6. Explain how an atom turns into a positive ion.
7. Explain how an atom turns into a negative ion.
8. In the list of reactions, circle any that are chemical.
Melting of ice, burning paper, heating cement, evaporating water, burning gasoline, baking cookies, mowing lawn, breaking a test tube.
9. In the list of properties below, circle all chemical properties and underline any physical properties.
Melting point, mass, reacts with air, fades, burns, boiling point, density, reacts with water, specific heat capacity, shape
10. For each of the following substances, determine if the substance is a mixture, compound or element.
Silver carbonate Potassium Kool-Aid
Chocolate chip cookies
11. Determine the number of protons, neutrons and electrons in at atom of titanium with a mass number of 49.
12. For the following data collected in a lab for the density of gold samples, determine if each group is accurate, precise, both or neither. The accepted value for density of gold is 19.30 g/ml.
Remember to find the average to help determine the correct answer.
a. 19.30 g/ml - 19.28 g/ml - 19.31 g/ml - 19.29 g/ml - 19.33 g/ml - 19.31 g/ml b. 19.3 g/ml - 19.2 g/ml - 19.9 g/ml - 19.4 g/ml - 19.0 g/ml - 19.2 g/ml c. 18.90 g/ml - 18.91 g/ml - 18.89 g/ml - 18.91 g/ml - 18.89 g/ml - 18.90 g/ml
13. On the following periodic table label the Noble Gases, the Alkali Metals, the Alkaline Earth Metals, the Halogens, the Transition Metals and the Inner Transition Metals, also list the charge for each group.
14. Name the following acids or bases by name.
LiOH (aq) __________________ H2CO3 (aq) _________________
HBr (aq) ___________________ H3PO3 (aq) ___________________
15. Write the formulas for the following acids or bases.
Ammonium hydroxide _________________ Sulfuric Acid _________________
Hydrophosphoric Acid _________________ Chloric Acid ___________________
Mass Relationships in Chemical Reactions – Chapter 3
16. Calculate the molar mass of (NH4)3PO4.
17. Calculate the percent composition of BaSO4.
18. How many atoms in 23 grams of zinc?
19. Determine the empirical formula for a compound with 32.38% sodium, 22.65% sulfur, and 44.99% oxygen.
20. The empirical formula of a compound is P2O5. The molar mass of the molecular compound is 283.89 g. What is the molecular formula?
21. Calcium chloride forms a hexahydrate. Calculate the percent by mass of anhydrous salt.
22. Balance the equations below.
a) KClO3 KCl + O2
b) Na + HCl H2 + NaCl
c) Al2(CO3)3 + Ca(OH)2 CaCO3 + Al(OH)3
d) H2C2O4 + NaOH → Na2C2O4 + H2O
e) FeCl3 + NaOH → Fe(OH)3 + NaCl
f) S8 + O2 → SO3
23. How many moles of oxygen are produced by the decomposition of 4.87 moles of KClO3?
2 KClO3 → 2 KCl + 3 O2
24. If 4.6 moles of sodium carbonate react with excess calcium hydroxide, how many grams of sodium hydroxide will be produced? BALANCE THE EQUATION FIRST!!!!
Na2CO3 + Ca(OH)2 → NaOH + CaCO3
25. Urea, (NH2)2CO is prepared by reacting ammonia with carbon dioxide in the following equation:
2NH3 (g) + CO2 (g) (NH2)2CO (aq) + H2O (l)
If 637.2 g of NH3 are treated with 1142 g of CO2, which is the limiting reactant? Calculate the mass of (NH2)2CO formed. What is the percent yield if you produced 1081 g in the experiment?
Reactions in Aqueous Solutions – Chapter 4
26. What types of reactions are the following: choose from: synthesis, combustion, single displacement, decomposition, double displacement, acid base
NH3 + O2 → NO + H2O
CaO + H2O → Ca(OH)2
H2SO4 + KOH → K2SO4 + H2O
H2O → H2 + O2
27. Predict the products of the following reactions:
a) AgI + Na2S → b) Na3PO4 + HCl → c) FeS + O2 → d) PCl5 + H2O → e) C2H6O + O2 →
28. Find the oxidation number of the underlined element.
a._________ Na2S b._________ MnO2 c.____________H2SO4
29. Write the half reactions for each of the following reactions and label as oxidation/reduction:
Zn(s) + 2HCl(aq) ---> ZnCl2(aq) + H2(g)
Cu(s) + 2Ag+(aq) ---> 2Ag(s) + Cu2+(aq)
SiCl4(l) + 2Mg(s) ---> 2MgCl2(s) + Si(s)
30. What is the molarity of a KCl solution whose volume is 400 mL and contains 85 g of KCl?
31. How many grams of NaCl are needed to make a .5 M solution with a volume of 100 mL?
32. In order to dilute a 1.25 M solution, what volume would you need to use to make 200 mL of a . 3 M solution?
33. In a titration experiment, a student finds that 23.48mL of a NaOH solution are needed to neutralize 0.5468g of KHP (molar mass =204.2 g/mol). What is the concentration of the NaOH solution?
Gases – Chapter 5
34. Convert 1200 mm Hg to atmospheres.
35. A sample of oxygen has a volume of 220 ml at 460 mm Hg. What will the volume be at a pressure of 750 mm Hg?
36. A gas has a volume of 750 ml at 25oC. What will the volume be at 70oC?
37. A helium balloon has a volume of 5 liters at 25oC and 1.2 atm. What will the volume be at .8 atm and 10oC?
38. What is the pressure of 1.15 mol of nitrogen gas in a 7.2 liters container at 32°C?
39. Calculate the density of CO2 in grams per liter at 0.990 atm and 55°C.
40. A chemist has synthesized a greenish-yellow gas compound of chlorine and oxygen and finds that its density is 7.71 g/L at 36°C and 2.88 atm. Calculate the molar mass of the compound.
41. Sodium azide, NaN3, is used in some car air bags. The impact in a collision triggers the decomposition of NaN3 as follows:
2NaN3 (s) 2 Na(s) + 3 N2 (g)
The nitrogen gas produced quickly inflates the bag between the driver and the windshield and dashboard. Calculate the volume of nitrogen gas generated at 80°C and 823 mmHg by the decomposition of 60.0 g of NaN3.
42. A mixture of gases contains 4.46 moles of neon, 0.74 mole of argon, and 2.15 moles of xenon.
Calculate the partial pressures of the gases if the total pressure is 2.00 atm.
Thermochemistry – Chapter 6
43. When 1 mol of Al2O3 is formed, 1669.8 kJ of heat are liberated. Determine the ΔH for the reaction between Al and Fe3O4 if the heat of formation for Fe3O4 is – 1120.9 kJ/mol.
8 Al (s) + 3 Fe3O4 (s) 4 Al2O3 (s) + 9 Fe (s)
44. How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22°C to 55°C, if the specific heat of aluminum is 0.90 J/g°C?
45. Classify each of the following as an exothermic or endothermic process.
Melting ice cubes _____________________ Baking Bread __________________
Burning a candle ____________________ Formation of snow in clouds ___________________________
Evaporation of water____________________
46. Calculate the ∆H for the following reaction:
NO + O NO2
You are given these three equations:
O2 2O ∆H = +495 kJ
2O3 3O2 ∆H = -427 kJ
NO + O3 NO2 + O2 ∆H = -199 kJ
47. A 185 gram sample of copper at 98.00C was added to 102 grams of water at 20.00C in a perfectly insulated calorimeter. The final temperature of the copper-water mixture was 31.20C. Calculate the specific heat of copper using this data.
Quantum Theory & the Electronic Structure of Atoms – Chapter 7
48. Summarize each of the following for how electrons are configured around the nucleus.
a. The Aufbau Principle
b. The Pauli Exclusion Principle
c. Hund’s Rule
49. Why do electrons enter the 4s orbital before they enter the 3d orbitals?
50. Draw the orbital diagram and write the electron configuration for each of the elements listed.
a. Mg
b. Ge
c. Cu
d. V
51. Explain what the 4 quantum numbers tell us about an atom.
52. Calculate the energy of a photon with a wavelength of 5.00 x104 nm.
53. Is hell exothermic or endothermic? Support your answer with proof.
