CHEM. 9 week Review
Write your answers on a separate sheet of paper.
1. Define and provide 3 examples of each: physical property, chemical property, physical change, chemical change
2. Identify each of the following as physical or chemical properties
a. Liquid
b. Able to cut glass
c. Toxicity
d. Conductivity
e. Solubility Hardness
f. Shape
g. Taste
h. Rust
i. Reactivity
j. Bending
k. Burning
l. Flammability
m. Melting point
n. Solid
3. Label each of the following as an intensive property (I) or extensive property (E)
a. Metallic
b. Ductility
c. Conductivity
d. Mass
e. Density
f. Volume
g. Length
h. Melting point
i. Conductivity
j. Boiling point
k. Color
l. Malleability
m. Luster
4. Describe the experiment and contributions (what did they discover or do?) to atomic theory by the following individuals in chronological order:
a. Rutherford
b. Bohr
c. Mendeleev
d. Thomson
e. Moseley
f. Dalton
5. Group the following atoms into groups with similar reactivity: include the oxidation numbers of each atom
a. Nitrogen
b. Tin
c. Radium
d. Magnesium
e. Potassium
f. Hydrogen
g. Helium
h. Barium
i. Bromine
j. Chlorine
k. Arsenic
l. Sulfur
m. Argon
n. Radon
o. Cadmium
p. Strontium
6. Copper used in electric wires comes in two flavors (isotopes): 63Cu and 65Cu. 63Cu has an atomic mass of 62.9298 amu and an abundance of 69.09%. The other isotope, 65Cu, has an abundance of 30.91%. The average atomic mass between these two isotopes is 63.546 amu. Calculate the actual atomic mass of 65Cu.
7. Naturally occurring chlorine that is put in pools is 75.53 percent 35Cl (mass = 34.969 amu) and 24.47 percent 37Cl (mass = 36.966 amu). Calculate the average atomic mass.
8. Magnesium consists of three naturally occurring isotopes. The percent abundance of these isotopes is as follows: 24Mg (78.70%), 25Mg (10.13%), and 26Mg (11.7%). The average atomic mass of the three isotopes is 24.3050 amu. If the atomic mass of 25Mg is 24.98584 amu, and 26Mg is 25.98259 amu, calculate the actual atomic mass of 24Mg.
9. Complete the table
c= 3.0x108m/s h= 6.63x10-34Js
10. A certain source emits radiation of wavelength 660.0 nm. What is the energy, in kJ, of one mole of photons of this radiation? What color is this photon? Must Show Work
11. A red light has a wavelength of 728 nm (728x10-7m).Must Show Work
a. What is the frequency of the light?
b. What is the speed of the wave in m/s?
12. A purple light has a frequency of 7.42 x 1014 Hz. Must Show Work
a. What is its wavelength?
b. What is the energy of one quanta of light?
13. You broke your big toe! The x ray they take ofthe toe uses waves that have a length2.19 x 1010m. Must Show Work
a. What is the speed of the wave in m/s?
b. What is the wavelength in nm?
c. What is the frequency of the x ray?
14. Create a chart of the properties of metals, nonmetals, and metalloids. Provide 3 examples of each.
15. Trends: Place the following in order of
a. Increasing Atomic radius:
i. N, Sb, P, Bi, As
ii. Li, C, F
iii. Li, Na, K
iv. Ge, P, O
b. Increasing Ionic radius:
i. F-, Na+, O2-, Mg2+, N3-
ii. Mg2+, Si4-, S2-
iii. Mg2+, Ca2+, Ba2+
iv. F-, Cl-, Br-
c. Increasing Ionization Energy
i. Mg, Si, S
ii. Mg, Ca, Ba
iii. F, Cl, Br
iv. d. Ba, Cu, Ne
d. Increasing electron affinity:
i. Li, C, N
ii. C, O, Ne
iii. Si, P, O
iv. K, Mg, P
a. Increasing electronegativity:
i. F, Cl, Br
ii. Ba, Cu, Ne C, O, Ne
iii. Si, P, O
iv. K, Mg, P
16. What is the electron configuration and box notation for the following atoms:
a. Manganese
b. Selenium
c. Beryllium
d. Carbon
e. Silicon
f. Potassium
g. Vanadium
h. Yttrium
i. Silver
17. Describe the difference between ionic, covalent, and metallic bonds.
a. Describe using the classes (metal, nonmetal)
b. Describe using the oxidation numbers (+ oxidation, - oxidation)
c. Provide an example of each.
i. For the ionic bond, which atom is more electronegative?
ii. For the covalent bond, which atom is more electronegative?
18. Identify the following as an ionic, covalent or metallic bonding.
a. Copper wire (Cu2)
b. Rust (Fe203)
c. Carbon dioxide (CO2)
d. Methane (CH4)
e. Mercury (Hg2)
f. Epson salt (MgSO4)
g. Acetic Acid (CH3COOH)
h. Ammonia (NH3)
i. 2-n-propanol ((CH3)2CHOH)
19. Identify the single, double, and triple bonds found in the diagrams below
20. What is the shape, arrangement of electrons, and geometry of the following compounds?
Example: SO2 trigonal planar bent
a. SO2
b. XeF4
c. SF6
d. CF4
e. BH3
f. CH4
g. NH3
h. SF4
i. Na3P
j. O2
k. PH3
l. H202
m. N2
n. CO2
o. BF3