REVIEW
CHEMISTRY MID-TERM
2012 – 2013
(200 points)
Mr. Chuba
(4 points) 1. Express the following numbers in scientific notation to three significant figures:
a. 0.000000027
b. 356
c. 0.096
d. 802.6
(4 points) 2. Convert the following numbers to regular form:
a. 1.52 x 104
b. 7.78 x 10-8
c. 3.256 x 10-5
d. 6.03 x 106
( 6 points) 3. Determine the number of significant figures in each of the following numbers:
a. 4867 miles
b. 56 mL
c. 60104 tons
d. 2900.0 g
e. 0.0000003 cm
f. 4.6 x 1019 atoms
(10 points) 4. Express each answer in the correct number of significant figures:
a. 7.310 ÷ 5.70
b. 3.26 x 10-3 – 7.88 x 10-5
c. 4.02 x 106 + 7.74 x 107
d. 4.51 x 3.6666
e. 3.70 – 2.9133
(2 points) 5. A lead sphere has a mass of 1.20 x 104g and its volume is 1.05 x 103 cm3. Calculate the density of lead.
(2 points) 6. Mercury is the only metal that is a liquid at room temperature. Its density is 13.6 g/cm3. How many grams of mercury will occupy a volume of 95.8 cm3?
(2 points) 7. The price of gold on a certain day in 2004 was $315 per ounce. Determine the price of 1.00g of gold on that day.
1 oz = 31.03g
(3 points) 8. The speed of sound in air at room temperature is 343 m/s. Determine the speed in mi/hr.
1 mi = 1.609 km
(4 points) 9. The human stomach can expand to hold up to 4.20 quarts of food. A pistachio nut has a volume of 0.900 mL. Determine the number of pistachio nuts that the stomach can hold.
1 gallon = 3.79 L 1 gallon = 4 quarts 1 L = 1000 mL
(7 points) 10. Determine whether these statements describe either a physical (P) or chemical (C) property:
a. _____ oxygen gas supports combustion.
b. _____ fertilizers help increase agricultural production.
c. _____ water boils below 1000C on top of a mountain.
d. _____ lead is denser than aluminum.
e. _____ uranium is a radioactive element.
f. _____ iron has a tendency to rust.
g. _____ rainwater in industrialized regions tends to be acidic.
(7 points) 11. Determine whether each of the following is either a physical change (P) or a chemical change (C):
a. _____ when a glass of water is left out in the sun, the water gradually disappears.
b. _____ carbon dioxide in air is converted to more to more complex molecules by plants during photosynthesis.
c. _____ the helium gas in a balloon tends to leak out after a few hours.
d. _____ rocks are ground into sand.
e. _____ frozen orange juice is liquefied by adding water to it.
f. _____ digesting a pizza.
g. _____ a spoonful of table salt dissolves in a bowl of soup.
(8 points) 12. Which of these properties are intensive (I) and which are extensive (E)?
a. ______area
b. _____ color
c. _____ density
d. _____ length
e. _____ volume
f. _____ temperature
g. _____ mass
h. _____ ductility
(10 points) 13. Classify each of these substances as an element (E), compound (C), homogeneous mixture (hom), or heterogeneous mixture (het):
a. _____ water
b. _____ gold
c. _____ raisin bran cereal
d. _____ orange soda
e. _____ rubbing alcohol (C3H7OH)
f. _____ sugar
g. _____ cellulose
h. _____ uranium
i. _____ sand on the beach
j. _____ brass
(5 points) 13. List the major contributions of each of the following scientists:
a. Dalton
b. Thomson
c. Milliken
d. Rutherford
e. Chadwick
(3 points) 14. Define the following:
a. atomic number
b. mass number
c. average atomic mass
(1 point) 15. Why does a knowledge of atomic number enable us to deduce the number of electrons present in an atom?
(1 point) 16. Why do all atoms of an element have the same atomic number, although they may have different mass numbers?
(1 point) 17. What do we call atoms of the same element with different mass numbers?
(1 point) 18. Explain the meaning of each term in the symbol AX.
Z
(3points) 19. Write the isotopic symbol for each of the following:
a. platinum-195
b. copper-63
c. tungsten-186
(4 points) 20. Write the name for each of the following isotopes:
a. 33S
16
b. 201Hg
80
c. 23Na
11
d. 64Ni
28
(16 points) 21. Complete the following table:
SYMBOL / PROTONS / NEUTRONS / ELECTRONS / MASS NUMBER25 / 56
262Bh
107
288Uup
115 / 115 / 173
204Hg
80 / 124
26 / 57
(2 points) 22. What are allotropes? How are allotropes different from isotopes?
(3 points) 23. Determine the average atomic mass of titanium given the following information:
Titanium-46 mass = 45.95 amu relative abundance = 8.000%
Titanium-47 mass = 46.95 amu relative abundance = 7.500%
Titanium-48 mass = 48.00 amu relative abundance = 73.70%
Titanium-49 mass = 48.95 amu relative abundance = 5.500%
Titanium-50 mass = 49.94 amu relative abundance = 5.300%
(5 points) 24. Name the concept, theory, model, etc. that each of the following scientists is known for in the development of the modern atomic model:
a. Max Planck
b. Bohr
c. de Broglie
d. Heisenberg
e. Schrodinger
(4 points) 25. Write the abbreviation for and describe each of the following quantum numbers:
a. principal quantum number
b. azimuthal quantum number
c. magnetic quantum number
d. spin quantum number
(4 points) 26. Define each of the following:
a. Pauli Exclusion principle
b. Aufbau Principle
c. Hund’s Rule
d. Heisenberg’s Uncertainty principle
(16 points) 27. Complete the following table:
Value of l / Letter / Range of ml / Number of orientations / Maximum # of electrons0
1
2
3
(3 points) 28. Write the complete electron configuration for each of the following:
a. As
b. K
c. Y
(6 points) 29. Draw the orbital diagram for each of the following:
a. O
b. V
c. Al
(3 points) 30. Determine the frequency of electromagnetic radiation with a wavelength of 3.33 x 10-8 m.
(3 points) 31. Determine the minimum frequency of light needed to eject an electron from an atom of platinum if the energy required is 9.08 x 10-19 J.
(4 points) 32. The argon-fluoride laser used in some refractive eye surgeries emits a wavelength of
1.933 x 10-7m. Determine the energy of this laser.
(1 point) 33. State the periodic law.
(6 points) 34. Identify each of the following as a metal, nonmetal or metalloid
a. phosphorus b. niobium
c. arsenic d. holmium
e. krypton f. strontium
(4 points) 35. Name each of the following groups by their family name.
a. Group 17 b. Group 1
c. Group 18 d. Group 2
(6 points) 36. Classify each of the following elements as a (an) alkali metal, alkaline earth metal, halogen, or noble gas.
a. rubidium d. iodine
b. bromine e. radon
c. radium f. lithium
(1 point) 37. State the trend for atomic radius.
(1 point) 38. State the trend for ionization energy.
(1 point) 39. State the trend for electronegativity.
(1 point) 40. Arrange these elements in order of decreasing atomic radius: sulfur, tellurim, and oxygen.
(1 point) 41. Arrange these elements in order of increasing ionization energy: Tl, Ga, In, B.
(1 point) 42. Arrange these elements in order of decreasing electronegativity: O, F, C, N.
(10 points) 43. Name the following ionic compounds:
a. MgI2 f. Pb(NO2)4
b. LaP g. (NH4)3AsO4
c. Sn(O2)2 h. Al2(HPO4)3
d. Ba(Cr2O7)2 i. B2S3
e. YPO4 j. Zn(HCO3)2
(10 points) 44. Write the formula for each of the following ionic compounds:
a. osmium (III) acetate f. tin (II) permanganate
b. barium telluride g. molybdenum (III) carbonate
c. plutonium (IV) cyanide h. rhodium sulfide
d. thallium sulfite i. tantalum iodide
e. dimercury (I) arsenide j. europium (II) phophate
MID-TERM TOPIC SUMMARY
Unit 1
- rules for significant figures
- rounding rules
- SI units
- Unit conversions (railroad tracks)
- Kilo-hecto-deca-base unit-deci-centi-milli
Unit 2
- matter
- mixtures (homogeneous & heterogeneous)
- compounds
- elements
- allotropes
- physical changes
- chemical changes
- physical properties
- chemical properties
- allotropes
Unit 3
- protons, electrons, neutrons - Rutherford
- mass number - Milliken
- isotopes - Thompson
- isotopic symbol
- average atomic mass calculations
- Democritus
- Dalton
Unit 4
- c=λγ
- amplitude
- frequency
- speed of light
- Planck’s constant
- E=hγ
- ground state
- excited state
- quantum numbers: n, l, ml, ms
- electron configurations: complete and abbreviated
- Aufbau Principle
- Pauli Exclusion Principle
- Hund’s Rule
- orbital diagrams
- Planck
- Bohr
- de Broglie
- Heisenberg
- Schrodinger
Unit 5
- Mendeleev
- Moseley
- metals, nonmetals, noble gases, metalloids
- family names
- trends in atomic radius, ionization energy, electronegativity
- definitions of atomic radius, ionization energy, electronegativity
- naming ionic compounds containing monatomic ions
- writing formulas for ionic compounds containing monatomic ions
- naming ionic compounds containing polyatomic ions
- writing formulas for ionic compounds containing polyatomic ions