Download Fall Final Review Honors

CHEMISTRY I HONORS – 1st SEMESTER EXAM REVIEW – Fall 2010
STRATEGY: Start by reading through your notes to refresh your memory on these topics. Then, use this review sheet as a starting
point to identify the areas on which you need to spend more study time. For those areas, go back to homework assignments, quizzes,
and reviews to practice more problems. I would also recommend going through all of your tests since these questions are only samples
and do not include specific examples of how vocabulary and other conceptual information might appear in a multiple-choice or other
format. Remember you can access notes and reviews on Mrs. J’s Chemistry page at: www.nisd.net/comartww/pages/chem/notes.
FORMAT:
 Questions will include multiple-choice and matching.
 A formula bank will be provided in addition to any values that you might need (electronegativity, etc.), but you will NOT be given
“formulas” for items listed in the VOCAB sections (average atomic mass, % error, etc.).
Measurement – Ch. 1.3,1.5-1.8,5.1
1. 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.
2. How many sig figs are in the following numbers?
a. 2.35
c. 89.70
b. 34,000
d. 0.0052
3. Convert the following numbers into or out of scientific
notation.
a. 548,000
c. 1.200 × 10-3
b. 0.0000770
d. 9.25 × 107
4. Osmium is the densest element with a density of 22.57
g/cm3. Find the mass of a 56.2 cm3 sample of osmium.
Matter – Ch. 1.9
10. Classify the following substances as solid, liquid, gas, or
plasma based on their properties.
a. flexible volume, high KE, particles can disperse freely.
b. flexible volume, very high KE, particles are charged.
c. fixed volume, very low KE, orderly particles.
d. fixed volume, low KE, particles can move past each other.
11. Compare and contrast a solution, colloid, and suspension.
12. Classify the following as element, compound,
heterogeneous mixture, or solution.
a. graphite (carbon)
b. grape juice
c. table salt (NaCl)
d. pepper
Atomic Structure – Ch. 2.3-2.6,7.2,7.4-7.9,7.11
15. Identify the scientists who made the following discoveries.
a. Atoms contain negative particles called electrons.
b. The mass of an electron is 9.11  10-28 g.
c. Atoms contain neutral particles called neutrons.
d. Atoms contain a dense, positive nucleus.
e. Atoms are indivisible and resemble billiard balls.
16. Describe the evolution of the atomic model from the
billiard ball model to the electron cloud model.
17. Write the isotope symbol, including atomic number & mass
number, for the following isotopes.
a. carbon-14
c. nickel-63
b. chromium-53
d. 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
5.
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
6. How many milliliters are in a 2.0 quart jug of milk?
7. Mrs. J. spent last weekend grading lab notebooks. If she
spent 5.5 min on each notebook, how many hours did it
take her to grade all 95 notebooks?
8. Calculate the density from the slope of a "Mass vs.
Volume" graph.
9. Record the appropriate # of SigFigs when measuring.
VOCAB: accuracy vs. precision
13. Classify the following as chemical or physical changes.
a. cutting wire
b. ripening tomato
c. apple slices turning brown
d. compressing a gas
14. Classify the following properties as physical or chemical.
a. melts at 68.0C
b. corrosive
c. reacts violently with water
d. decomposes in air
e. magnetic
VOCAB: kinetic molecular theory
law of definite composition
law of multiple proportions
19. Calculate the wavelength if the frequency is 2.5 x 105 Hz.
20. Find the energy of a photon if frequency is 7.31 x 1014 Hz.
21. Describe how Bohr’s model explains the bright lines (red,
green, violet, violet) in the emission spectrum of hydrogen.
22. What is the primary difference between the modern model
of the atom and Bohr’s model?
23. Draw orbital diagrams for the following elements.
Symbol
Atomic #
Orbital Diagram
F
V
24. Explain why chromium’s electron configuration is [Ar]
4s13d5 instead of the expected configuration of [Ar] 4s23d4.
25. Give the shorthand electron configuration for the following.
Symbol
# eShorthand e- Configuration
Pd
At
26. Predict the ions that will form from the following atoms and
give the shorthand configuration of the ion.
Atom
Ion
Noble Gas
Shorthand e- Configuration
Rb
Te
27. How did Mendeleev and Mosely arrange the elements in
the periodic table?
28. Circle the atom with the LARGER radius.
a. Ra
N
b. Ne
Xe
29. Circle the particle with the LARGER radius.
a. Cl
Cl –
b. Mg
Mg2+
Nuclear Chemistry – Ch. 2.5,3.1,18.1-18.4,18.5
34. Calculate the average atomic mass of Br, if the nuclides
are Br-158(25.34%), Br-160(50%), and Br-162(24.66%).
35. Calculate the relative abundance of sodium nuclides. If the
average atomic mass is 22.99 and the nuclides are Na-23
(mass is 22.985amu) and Na-24 (mass is 23.789 amu).
36. Find the mass defect of Pu. If the average atomic mass of
Pu is 244. (1 p= 1.007276 amu, 1 n = 1.008665 amu, 1 e= 0.0005486 amu)
37. __________ + 4He  243Bk + 1n
38. 238U + 12C  ________ + 6 1n
Chemical Bonding – Ch. 2.8, 4.8, 8.1-8.2,8.4-8.8
41. Based on their electronegativities (p353), are the bonds in
the following substances IONIC, POLAR, or NONPOLAR?
a. MgO
c. LiCl
b. H2O
d. Br2
42. Are the following properties characteristics of ionic,
covalent, or metallic bonding?
a. These bonds are formed by delocalized electrons in
an “electron sea.”
b. These bonds involve a transfer of electrons.
c. Substances containing these bonds are malleable
and have very high melting points.
d. Substances containing these bonds do not conduct
electricity and have low melting points.
e. Compounds containing these bonds have a crystal
lattice structure.
f. These bonds are formed by sharing electrons.
43. Use Lewis Diagrams to show the formation of MgO.
44. Use Lewis Diagrams to show the formation of H2O.
30. Circle the atom with the HIGHER first ionization energy.
a. Li
Cs
b. Ba
As
31. Circle the atom with the HIGHER melting point.
a. Cl
Si
b. Cs
W
32. Why are there small jumps in the 1st ionization energies of
the elements as you move across a period?
33. Why is there a large increase in ionization energy when
the 4th electron is removed from aluminum?
VOCAB: ionization energy
periodic law
metals/nonmetals/metalloids
shielding
excited state/ground state
quark
wave-particle duality
isotope
valence/core ephoton
Pauli Exculsion Principle
Hund’s Rule
Heisenberg Uncertainty Principle Aufbau Principle
average atomic mass
39. Find the nuclear binding energy of Pu, using the
information from question 36.
40. Na-24 has a half life of 14.8 hours. If you have 5.6g left of
this substance after 7.4 days, how much of this substance
did you have originally (in kg)?
VOCAB: fission
fusion
alpha particles
Beta particles
isotope
half life
Chain reaction
critical mass
mass defect
Gamma rays
positron
avg. atomic mass
45. Explain the relationship between potential energy and
stability.
46. Write formulas for the following compounds (HINT: First
determine ionic/acid/covalent).
a. calcium bromide
d. silicon dioxide
b. iron(III) sulfate
e. dinitrogen tetroxide
c. hydrofluoric acid
f. sulfurous acid
47. Write names for the following compounds (HINT: First
determine ionic/acid/covalent).
a. CrCl3
d. MgSO4
b. Cu2CO3
e. P4O6
c. AsCl5
f. HClO3
48. Explain the difference between nonpolar covalent, polar
covalent, and ionic bonds in terms of sharing of electrons
and electric charge.
VOCAB: bond energy (bond length)
electronegativity
chemical bond
potential energy
dipole
Molecular Structure – Ch. 8.9-8.13
49. Explain the main idea of the VSEPR Theory.
50. For each of the following molecules, draw the Lewis electron dot diagram, give the shape and bond angle(s), and state
whether the molecule is polar or nonpolar. Show your work in the spaces provided for counting valence e - and e- pairs.
Number of
Lewis Diagram
Counting
Molecular Shape
Molecular
& Bond Angle(s)
Polarity
valence e
e pairs
SiO2
AsF5
51. Draw the dipole moments for each bond in the following molecules and circle whether the molecule is polar or nonpolar.
TeCl2
bent BCl3
trigonal planar CH2Cl2
tetrahedral
Te
Cl
Cl
Cl
Cl
B
C
Cl
polar
nonpolar
VOCAB: octet rule
bond angle
expanded octet
dipole moment
Cl
polar
nonpolar
lone pairs
bonding pairs
Chemical Reactions – Ch. 3.6-3.7,4.5-4.6,4.8-4.10
52. Write a word equation for the following reaction (incl. how
many? of what? what state?).

 BaCl2(s) + 3O2(g)
Ba(ClO3)2(s) 
53. Rewrite and balance the following word equation using
chemical formulas, physical states, and energy. – When
solid sodium chlorate absorbs energy, it produces solid
sodium chloride and oxygen gas.
Predict the products and balance (54-57). Write N.R. if no
reaction will occur. Include physical states .
54. Cu(s) + MgSO4(aq) 
55. C5H12(l) + O2(g) 
Chemical Composition – Ch. 3.2-3.5
62. How many magnesium sulfate molecules are in 25.0 g?
63. Find the molarity of a 750 mL solution containing 346 g of
potassium nitrate.
64. Calculate the number of grams required to make a 50.0
mL solution of 6.0M NaOH.
65. Find the % composition of copper(II) chloride.
H
polar
Cl
H
nonpolar
56. NH4Cl(aq) + Pb(NO3)2(aq) 
57. Fe2O3(s) 
58. For each of the reactions in #54-57, specify whether it is
combustion, synthesis, decomposition, single
replacement, or precipitate.
State whether the following species are being oxidized or reduced
59. Cr2+  Cr3+
60. Cr  Cr2O72Solve this redox reaction using half reaction method(acid)
61. CH4(g) + O2(g)  CO2(g) + H2O(g)
66. The percent composition of a compound is 40.0% C, 6.7%
H, and 53.7% O. The molecular mass of the compound is
180.0 g/mol. Find its empirical and molecular formulas.
VOCAB: Avogadro’s number
empirical formula
percent composition
molecular formula
molarity
CHEMISTRY I HONORS – 1st SEMESTER EXAM REVIEW – Fall 2010
ANSWER KEY
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
10.5%
a. 3, b. 2, c. 4, d. 2
a. 5.48 × 105, b. 7.70 × 10-5, c. 0.001200, d. 92,500,000
1270 g
a. 0.652 dm, b. 2,300 kg, c. 65 mL, d. 50,200 cm
1900 mL
8.7 hours
slope = (mass)  (volume) = density
always record one estimate digit
a. gas, b. plasma, c. solid , d. liquid
Solution and colloid do not settle. Colloid and suspension are heterogeneous mixtures and scatter light.
a. element, b. solution, c. compound, d. heterogeneous mixture
a. physical, b. chemical, c. chemical, d. physical
a. physical, b. chemical, c. chemical, d. chemical, e. physical
a. Thomson, b. Millikan, c. Chadwick, d. Rutherford, e. Dalton
Dalton’s billiard ball model-sphere of uniform density. Thomson’s plum pudding model-negative electrons dispersed in positive
atom. Rutherford’s nuclear model-dense, positive nucleus surrounded by negative electrons. Bohr’s planetary model-electrons
move in circular orbits in specific energy levels. Schrödinger’s electron cloud model-electrons move within orbitals not in specific
orbits. (Chadwick then added neutrons to the nucleus.)
14
53
63
92
6 C, 24 Cr , 28 Ni, 40 Zr
Zn
Symbol
Ca
Se
Ar
20
Atomic #
30
34
18
65
74
40
Mass #
41
34
# of protons
30
20
18
21
# of neutrons
35
40
22
18
# of electrons 30
20
34
1200 m
4.84  10-19 J
Hydrogen atoms have specific energy levels. Therefore, the atoms can only gain or lose certain amounts of energy. When atoms
lose energy, they emit photons which correspond to the lines in the emission spectrum. The more energy lost, the more energy the
photon has.
Bohr’s model stated that electrons circled the nucleus in fixed, circular paths called orbits. The modern model states that electrons
move around the nucleus in orbitals where there is a probability of finding an electron.
23.
F
9
V
23
24. In order to achieve greater stability, Cr moves one electron from the 4s-sublevel to the 3d-sublevel to make it half-full.
25.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
41.
42.
43.
Pd
At
46
85
[Kr] 5s24d8
[Xe] 6s24f145d106p5
26.
Rb
Te
Rb+
Te2-
Kr
Xe
[Ar] 4s23d104p6
[Kr] 5s24d105p6
Mendeleev arranged the elements in order of increasing atomic mass. Mosely arranged them by increasing atomic number.
a. Ra, b. Xe
a. Cl , b. Mg
a. Li, b. As
a. Si, b. W
There are small jumps in 1st ionization energy when there is an element with increased stability (full or half-full sublevel).
Removing the 4th electron from aluminum represents removing a core electron.
159.99 amu
Na-24 = 0.62% and Na-23 = 99.38%
-2.03525 amu
240Am
244Cf
-3.04x10-10 J
22.93 kg
a. ionic, b. polar, c. ionic, d. nonpolar
a. metallic, b. ionic, c. metallic, d. covalent, e. ionic, f. covalent
44.
45. The lower the potential energy, the greater the stability.
46. a. CaBr2, b. Fe2(SO4)3, c. HF, d. SiO2, e. N2O4, f. H2SO3
47. a. chromium(III) chloride, b. copper(I) carbonate, c. arsenic pentachloride, d. magnesium sulfate,
e. tetraphosphorous hexoxide, f. chloric acid.
48. nonpolar covalent – e- are shared equally, symmetrical orbital overlap, no separation of charge
polar covalent – e- are shared unequally, lopsided overlap, partial charges
ionic – e- are not shared, no overlap, complete charges
49. Electron pairs move as far apart from each other as possible in order to minimize repulsion. The number & type of electron pairs
determines the bond angles and overall shape of the molecule.
50.
51.
Number of
valence e
Lewis Diagram
Counting
e pairs
Molecular Shape
& Bond Angle(s)
Molecular
Polarity
SiO2
1(4)+2(6)=16
2B, 0L
linear, 180
nonpolar
AsF5
1(5)+5(7)=40
5B, 0L
trigonal bipyramidal,
120/90
nonpolar
TeCl2
bent
Te
BCl3
Cl
Cl
Cl
trigonal planar
CH2Cl2
Cl
C
B
Cl
Cl
H
tetrahedral
Cl
H
polar
nonpolar
polar
nonpolar
polar
nonpolar
52. One unit of solid barium chlorate when heated produces one unit of solid barium chloride and three molecules of oxygen gas.
53.
54.
55.
56.
57.
58.
59.
60.
61.
62.
63.
64.
65.
66.

 2NaCl(s) + 3O2(g)
2NaClO3(s) 
Cu(s) + MgSO4(aq)  N.R.
C5H12(l) + 8O2(g)  5CO2(g) + 6H2O(g)
2NH4Cl(aq) + Pb(NO3)2(aq)  2NH4NO3(aq) + PbCl2(s)
2Fe2O3(s)  4Fe(s) + 3O2(g)
single replacement, combustion, double replacement, decomposition
oxidized
oxidized
CH4(g) + 2O2(g)  CO2(g) + 2H2O(g)
1.25  1023 molecules MgSO4
4.6M KNO3
12 g NaOH
47.27% Cu, 52.73% Cl
empirical formula – CH2O, molecular formula – C6H12O6
I’m so proud of you! You survived a hard semester of Chem. Honors! See you next year!