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Final Exam Review #1
Supplemental Instruction
Iowa State University
Allison
Chem 163
Dr. Appy
12/09/14
1. Classify each of the following substances as an elemental substance, a compound,
a homogenous mixture, or a heterogeneous mixture.
a. Water
compound
b. Air
homogeneous mixture
c. Iron nail
elemental substance
d. Diamond
elemental substance
e. Salt
compound
f. Mud
heterogeneous mixture
2. Classify each of the following as either a physical change or a chemical change.
a. Boiling water
physical
b. Burning paper
physical
c. Photosynthesis
chemical
d. Melting ICE
physical
e. Changing color
chemical
3. Define:
a. Law: a statement that describes the way things are consistently observed
to be have under a given set of circumstances
b. Theory: a tentative explanation for a set of observations. A theory must be
consistent with every one of the observations and is tested through
experiments
c. Hypothesis: what a theory is called the first time it is postulated, and
before it is well enough tested to be accepted as a theory.
4. Describe the difference between accuracy and precision.
Accuracy: the degree to which a measured value is close to the true value.
Precision: the degree to which a set of measured values of the same quantity agree
with each other.
5. Two teams of students take a series of 5 measurements of the mass of a 18 oz
beaker of water.
Team A (in oz): 15.9, 15.9, 15.8, 16.0, 15.9
Team B (in oz): 17.4, 17.6, 18.1, 18.2, 17.7
a. Which team is more accurate? Team B
b. Which team is more precise? Team A
6. Determine how many significant figures are in the following:
a. 0.0987 ----- 3 sig figs
b. 100,030 ----- 5 sig figs
c. 0.000975 ----- 3 sig figs
d. 9.00 ----- 3 sig figs
7. Carry out the following operations. Express the answers with the appropriate
number of significant figures.
a. (5.678 – 1.56) x 0.00987 = 0.0406
b. 4.67 + 0.98 = 5.65
c. 3.4567 x 2300 = 8.0 x 10^3
8. The speed of light is 3.00 x 108 m/s. Express the speed of light in mi/hr.
9. Express each of the following measured quantities in either standard notation of
scientific notation (whichever form it is not already in).
a. 1.234 x 104 m --- 12,340 m
b. 1.900 x 103 m ---- 1900
c. 0.00078 cm ---- 7.8 x 10^-4
d. 0.00000009 ft ----- 9 x 10^-8
10. Express absolute zero in both Celsius and Fahrenheit to the nearest degree.
K = ºC + 273.15
ºF = 32 + (9/5)ºC
ºC = K – 273.15
ºF = 32 + (9/5)(-273.15)
ºC = 0 – 273.15
ºF = 32 - 491.67
= -273.15 ºC  -273 ºC
= -459.67 ºF  -460. ºF or -4.60 x 102 ºF
11. What volume, in mL, is occupied by 8.87 grams of solid gold (density = 19.3
g/ml) at 25.0 degrees Celsius?
d= m/v
v= m/d
8.87 g / (19.3 g/mL) = 0.460 mL
12. How much energy (in J) is required to heat 1.89 x 105 g of water from 25.7 ºC to
67.8ºC?
ΔT = 67.8 – 25.7 = 42.1 ºC
q= mCsΔT = (1.89 x 105 g)(4.184J/gºC)(42.1ºC) = 3.33 x 10^7
13. Write the correct charge for each subatomic particles:
a. Protons
+
b. Neutrons
No Charge
c. Electrons
-
14. Fill in the table:
Protons
Neutrons
Electrons
Net Charge
19
21
18
+1
Fe
26
30
26
0
Na+
11
12
10
+1
31
15
16
15
0
40
K+
56
23
P
15. Which of the following is not part of Dalton’s atomic theory?
a. All matter is made up of atoms.
b. Atoms can be neither created nor destroyed.
c. Atoms of a particular element are alike.
d. Atoms of different elements differ.
e. Most of the mass of an atom is contained in the nucleus
f. Chemical reactions involve the union or separation of atoms
16. List the following elements in order of increasing first ionization energy (from
lowest to highest): Ne, O, Mg, Ca, K, P
K, Ca, Mg, P, O, Ne
17. What color of light is emitted by a hydrogen atom who’s electron transfers from
n=3 to the n=1 energy state? Use the energy level diagram and visible spectrum.
n=3
n=1
12.1 eV
1.0 eV
11.1 eV
E= hc/wavelength
wavelength = hc/E
= (6.626 x 10^ -34 J*s)(3.00x10^8 m/s)
11.1 eV
___(1 ev)__
___(10^9 nm)___
(1.602x10^-19 J)
1m
= 102.5 nm --- Ultraviolet
18. Write the full AND abbreviated electron configurations for a silver atom in the
ground state.
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6, 5s2, 4d9
[Kr]5s2, 4d9
19. Predict which of the follow ionic compounds will have the highest melting point.
NaCl, CaCl2, MgS
20. Place the following atoms in order of increasing atomic size (smallest to largest).
Cl, Ne, Na, Rb
Ne, Cl, Na, Rb
21. Define electronegativity.
22. Name the following compounds:
a. LiCl
Lithium chloride
b. MgCl2
Magnesium chloride
c. SF6
Sulfur hexafluoride
d. N2O4
Dinitrogen tetroxide
e. NaNO2
Sodium nitrite
f. HF
Hydrofluoric acid
g. H2S
Hydrosulfuric acid
h. CoCl2
Cobalt (II) chloride or Cobaltous chloride
i. HNO3
Nitric acid
j. CuCl
Copper (I) Chloride or Cuprous chloride
23. Fill out the following chart:
Compound
H2O
SO2
Electronic
Geometry
Molecular
Geometry
Bond Angle
Tetrahedral
Bent
<109.5
Trigonal planar
Bent
<120
AsF3
Trigonal
Tetrahedral
<109.5
pyramidal
CF4
Tetrahedral
Tetrahedral
109.5
For Hydrogen:
Useful Equations and Conversions:
E = hc/λ
c = 3.00 x 108 m/s
h = 6.626 x 10-34 J*s
1 eV = 1.602 x 10-19 J
1 m = 109 nm
F = kq1q2/r2