Semester I Review Questions

Matter

1.Classify the following substances as solid, liquid, gas, or plasma based on their properties.

  1. flexible volume, high KE, particles can disperse freely.
  2. flexible volume, very high KE, particles are charged.
  3. fixed volume, very low KE, orderly particles.
  4. fixed volume, low KE, particles can move past each other.

2.Compare and contrast a solution, colloid, and suspension.

3.Classify the following as element, compound, heterogeneous mixture, or solution.

  1. graphite (carbon)
  2. grape juice
  3. table salt (NaCl)
  4. pepper

4.Classify the following as chemical or physical changes.

  1. cutting wire
  2. ripening tomato
  3. apple slices turning brown
  4. compressing a gas

5.Classify the following properties as physical or chemical.

  1. melts at 68.0C
  2. corrosive
  3. reacts violently with water
  4. decomposes in air
  5. magnetic

6.Calculate the specific heat of a metal when 25.0 g of the metal changes 20oC, and releases 6700 J of energy.

7.How much energy is lost when 50.0 g of steam changes from 150oC to 100oC? (2.04J/goC)

Measurement

8.In a lab, the average measured density for Pre-1982 pennies was 7.98 g/cm3. Given that the literature value for the density is 8.92 g/cm3, calculate the percent error.

9.How many sig figs are in the following numbers? Round each value to 3 sig figs.

  1. 2.2500
  2. 34,0100
/
  1. 89.70157
  2. 0.0052001

10.Convert the following numbers into or out of scientific notation. How many sig figs are in each value?

  1. 548,000
  2. 0.0000770
/
  1. 1.200 × 10-3
  2. 9.25 × 107

11.Osmium is the densest element with a density of 22.57 g/cm3. Find the mass of a 56.2 cm3 sample of osmium.

12.Perform the following SI prefix conversions.

a. 65.2 mm = ? dm / c. 65,000 L = ? mL
b. 2.3 kg = ?g / d. 0.502 km = ? cm

13.Mr. B spent last weekend grading lab reports. If he spent 5.5 min on each notebook, how many hours did it take he to grade 95 notebooks?

14. Calculate the total number of years 2.65x1023 seconds would represent.

Atomic Structure

15.Identify the scientists who made the following discoveries.

  1. Atoms contain negative particles called electrons.
  2. The mass of an electron is 9.11  10-28 g.
  3. Atoms contain neutral particles called neutrons.
  4. Atoms contain a dense, positive nucleus.
  5. Atoms are indivisible and resemble BB’s.

16.Describe the evolution of the atomic model from the BB model to the electron cloud model.

17.Write the isotope symbol, including atomic number & mass number, for the following isotopes.

  1. carbon-14c.nickel-63
  2. chromium-53d.zirconium-92

18.Complete the table for the following isotopes.

Symbol

/ Zn
Atomic # / 20
Mass # / 65 / 74 / 40
# of protons / 34
# of neutrons / 21
# of electrons / 18

19.Calculate the average atomic mass of copper if 69.17% of the copper atoms occurring in nature are 63Cu and 30.83% are 65Cu.

20.Determine the half-life of a radioactive isotope if 100 grams decayed into 6.25 grams in two hours.

21.If the half-life of an isotope is 525 years, how long will it take for 64 g to become 1.0g?

22.Uranium -238 decays by emitting an alpha particle. Finish and Balance the equation.

23.Carbon – 14 emits a beta particle. Finish and Balance the equation.

Naming and Writing Formulas

24. Name the following compounds:

  1. KI
  2. Mn2(SO3)7
  3. SnBr4
  4. Mg3P2
  5. NaF
  6. Sr(MnO4)2
  7. Cr(PO4)2
  8. Al2Se3
  9. HNO3
  10. HCl
  11. HClO2
  12. H3PO4
  13. N2O2
  14. P4S9
  15. CBr4
  16. Se2F8
  17. BCl3
  18. P3I7
  19. N2O
  20. Si2F4

25.Write the formula for the following compounds

  1. cobalt (III) chromate
  2. ammonium oxide
  3. potassium hydroxide
  4. lead (IV) sulfate
  5. silver cyanide
  6. vanadium (V) nitride
  7. strontium acetate
  8. molybdenum (III) chloride
  9. platinum (II) sulfide
  10. ammonium phosphate
  11. trisulfur hexafluoride
  12. tetrasulfur hexachloride
  13. hexanitrogen decoxide
  14. pentanitrogen decoxide
  15. disilicon nonoxide
  16. silicon dioxide
  17. disulfur pentoxide
  18. carbon tetrachloride
  19. hypochlorous acid
  20. nitrous acid
  21. acetic acid
  22. hydrosulfuric acid

Writing and Balancing Equations

26. For the following reactions, balance them and indicate whether the following are examples of synthesis, decomposition, combustion, single replacement, double replacement

___Na3PO4 + ___KOH  ___NaOH + ___K3PO4 ______

___MgCl2 + ___Li2CO3___MgCO3 + ___ LiCl ______

___C6H12 + ___ O2___ CO2 + ___ H2O ______

___Pb + ___FeSO4___PbSO4 + ___Fe ______

___CaCO3___CaO + ___CO2 ______

___P4 + ___ O2___ P2O3 ______

___ RbNO3 + ___BeF2___Be(NO3)2 + ___ RbF ______

___ AgNO3 + ___Cu ___Cu(NO3)2 + ___ Ag ______

___C3H6O + ___ O2 ___ CO2 + ___ H2O ______

___ C5H5 + ___Fe ___Fe(C5H5)2 ______

___C6H6 + __ O2 __ H2O + __ CO2______

___NaI + __ Pb(SO4)2 __ PbI4 + __ Na2SO4______

___NH3 + __ O2__ NO + __ H2O______

___Fe(OH)3 __ Fe2O3 + __ H2O______

___HNO3 + __ Mg(OH)2 __H2O + __ Mg(NO3)2______

___H3PO4 + __ NaBr  __ HBr + __ Na3PO4______

___C + __ H2 __ C3H8______

___CaO + __ MnI4 __ MnO2 + __ CaI2______

___Fe2O3 + __ H2O  __ Fe(OH)3______

___C2H2 + __ H2 __ C2H6______

27. Classify and Balance the following Reactions

Rubidium and nitrogen react to form rubidium nitride

Potassium chlorate when heated produces potassium chloride and oxygen gas

Cesium reacts with aluminum chloride to produce cesium chloride and aluminum

Solutions of iron (III) nitrate and sodium phosphate are mixed to yield sodium nitrate and iron (III) phosphate

Tetracarbon decahydride reacts with oxygen to produce carbon dioxide and water.