Chemistry
Study guide Fall Final
CH 1 Matter & Changes
Classify the following:
1. Grain alcohol
2. Pumpkin
3. Salt
4. Salt water
5. Gasoline
6. Air
A. Heterogeneous
B. Solution
C. Compound
D. Element
Classify the following:
7.
8.
9.
10.
11.
12.
Odor
Reacts with air
Rusting
Solubility
Expansion
Flammable
A. Intensive Property
B. Extensive Property
C. Chemical Property
Classify the following:
13.
14.
15.
16.
17.
Growth of a plant
A. Physical Change
Dissolving carbon dioxide in coke
B. Chemical Change
Mixing two clear solutions and getting a cloudy solution
Formation of clouds
Evaporation of salt water
CH 2 Measurement & Calculations
Tell how many significant figures are in the following:
18. 200.0 m
19. 150 L
20. 0.00505 dL
21. 25,000 g
Calculate the following using proper sig figs and scientific notation.
22. 0.00287 m + 47.55 m + .027 m + 1.8645 m
23. (0.0350cm)(2.00cm)(0.050cm)
24.
25.
25,000g – 10,250.50g
(2.20 x 10-5 g)(0.0034 x 103 g)(5.0 x 10-3 K)
(1.550 x 10-2 cm3)(1.50 x103 g)(0.0350 x 10-2 K)
26. 23.655 s – 0.09553 s
27. 10,000.0 m2
25.0 m
28. (2.55 x 10-5 cm)(5.00 x 103 cm)(1.5 x 10-2)
(9.11 x 105 cm)(6.023 x 1023 cm)
29. 0.02255 s + 75.600 s + 3.0 s + 750. S
Density- Calculate the following density problems.
30. Calculate the volume (cm3) given 25.6 mg and 2.55 dag/L.
31. Calculate the mass (g) given 550 m3 and 0.110 hg/mm3
32. Calculate the density (g/cm3) given 0.020 pg and 500.0 L
Honors Chemistry
Convert the following temperatures: Show work and put all answers into scientific notation.
1.
78.6 K to F
2.
- 45.3 C to K
3.
50.0 F to C
4.
– 10.0 C to F
CH 3 Atoms: Building Blocks of Matter
Calculate the following:
Nuclear Symbol Atomic Number Mass Number
79
Se
Protons
Neutrons
Electrons
34
50
38
30
28
65
119
Sn+4
50
15
1.
16
18
Calculate the mass of the second isotope given the following information: Average atomic mass of the two
isotopes is 25.3345 amu, the mass of the first isotope is 26.2525 amu with an abundance of 67.35%.
2.
Calculate the average atomic mass given the following information.
Isotope Relative Abundance
65
X 65.34%
23
66
X 23.78%
23
68
X 10.00%
23
69
X 0.88%
23
3.
Calculate the relative abundance given the following information. Average atomic mass of two isotopes is
55.3238 amu. The mass of one of the isotopes is 56.2500 amu and the mass of the second isotope is
54.3434amu.
4.
A sample of C6H4Cl2 contains 5.25 moles . (C=12.0 H=1.0 Cl=35.5)
a. How many molecules are in this sample.
b.
What is the mass of this sample.
c.
How many total atoms are in this sample.
d. How many carbon atoms are in this sample.
5.
A sample of Ba(ClO3)2 has a mass of 0.0500 grams.
(Ba=137.3 Cl=35.5 O= 16.0)
a. How many moles are in this sample.
b.
How many formula units are in this sample.
c.
How many oxygen atoms are in this sample.
d. How many ClO3-1 ions are in this sample.
6.
How many moles are in 50.0 g of oxygen. (O=16.0)
CH 21 Nuclear Chemistry
Complete each of the following equations.
1. 22688Ra = 22286Rn +______
2. 94Be + 42He = 126C + ______
3. 23490Th = 23491Pa + ______
4. 18775Re + ___________ = 18875Re + 11H
In the space provided, identify each of the following nuclear reactions as an a. alpha decay, b. beta decay, c. positron emission, or d.
electron capture.
5._____ 146C = 147N + 0-1β
6._____ 10647Ag + 0-1e = 10646Pd
7._____ 21084Po = 20682Pb + 42He
8._____ 3819K = 3818Ar + 0+1β
Write the nuclear equations for the following reactions:
a. Carbon-12 combines with hydrogen-1 to form nitrogen-13.
b. Curium-246 combines with carbon-12 to form nobelium-254 and ___ neutrons.
c.
d.
e.
f.
Hydrogen-2 combines with hydrogen-3 to form helium-4 and a something else
91
42Mo undergoes positron emission.
6
2He undergoes beta decay.
129
55Cs undergoes electron capture
9. Phosphorus-32 has a half-life of 14.3 days. How many days will it take for a radioactive sample to
decay to one-eighth its original size?
10. Iodine-131 has a half-life of 8.0 days. How many milligrams of an original 160 mg sample will
remain in 40 days?
11. . Iodine-131 has a half-life of 8.0 days; it is used in medical treatments for thyroid conditions.
Determine how many days must elapse for a 0.80 mg sample of iodine-131 in the thyroid to decay
to 0.10 mg
CH 4 Arrangement of Electrons in Atoms
a.
write the electron configuration or noble, b. Lewis dot structure, and c. ionic charge for the following: (3
pts each)
Cu
Sb
Ar
CH 5 Periodic Law
Order the following groups of elements from smallest to greatest atomic radius.
1. 1. Na, 2. K, 3. Li
2. 1. Al, 2. P, 3. Cl
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
Order the following groups of elements from smallest to greatest 1st ionization energy.
3. 1. Li, 2. Na, 3. K
4. 1. Si, 2. S, 3. Na
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
Order the following groups from smallest to greatest electronegativity.
5. 1. Mg, 2. Si, 3. Cl
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
6. 1. Be, 2. Mg, 3. Sr
a. 1-2-3 b. 3-2-1 c. 2-1-3 d. 1-3-2 e. 2-3-1 ab. 3-1-2
ac. none
CH 6 Chemical Bonding & CH 7 Chemical Formulas and Compounds (Ionic and Acids)
Draw the following Lewis Structures for the following ionic compounds.
KP3 __________________________________________________
AlCl3 __________________________________________________
Write the chemical formula for the following compounds.
1. perchloric acid
2. iron III oxlate
3. sulfuric acid
4. chromic acid
5. ammonia arsenate
6. hydrofluoric acid
Write the names for the following.
7. HBr
8. Zn3(PO4)2
9. HClO
10. Al(MnO4)3
11. H3PO3
12. Calculate the molar mass of the following hydrate MgSO4 · 8H2O (Mg=24.3 S=32.1 O=16.0 H=1.0)
13. Find the percent composition of the elements Mg, S, O and H2O in the above hydrate.
14. Calculate the percent of water in Sn(NO3)2 7 H2O. (Sn=118.7 N=14.0 O=16.0
H=1.0)
15. Find the molecular formula when the empirical formula is C7H9O if the molecular mass is
327g/n.(C = 12.0, H = 1.0, O = 16.0)
16. Find the molecular formula of a compound with the following masses;
59.0g of C, 7.1g of H, and 26.2 g of O and 7.7g of N. The formula mass of the compound
is 549 amu.(C=12.0 H = 1.0 O=16.0 N=14.0)
17. A 16.50 g sample of a compound contains 6.64 g of potassium, 4.42 g of chromium, and the rest of
the compound is oxygen. Find the empirical formula. (K=39.1 Cr=52.0 O=16.0)
18. What is the empirical formula for a compound made up of 3.24 g calcium, 1.67 g phosphorus and
3.44 g oxygen. (Ca= 40.1 P= 31.0 O=16.0)