Download Fall 2012 Chem106 Final Review Name: Test 1 Materials Question

Fall 2012 Chem106
Final Review
Name:
Test 1 Materials
Question 1. How Many significant figures does each of the following numbers have?
34.22
0.030345
2.0030
5.04x103
34030
Question 2. Which label on the periodic table best represents the following:
A
C
B
D
Alkali Metals
Metalloids
Halogens
F
G
E
Nonmetals
Noble Gases
Question 3. Fill in the Symbol, Atomic Number (AN), Number of Protons(NP), Number of Neutrons(NN),
Mass Number (MN) and Number of Electron (NE) for each of the following?
Symbol
AN
NP
NN
MN
NE
15
N
20
26
238
U
96
44
Question 4. What’s the half-life of a material that decays to 12.5% of its original mass in 24 days?
a)
3 days
b)
8 days
c)
16 days
d)
12 days
Question 5. The half-life for the radioactive decay of barium-137 is 2.5 minutes. If a sample of has an
initial activity of 10564.0 μCi, what is the activity of the sample after 15 minutes?
a)
82.5313μCi
b)
165.063 μCi
c)
0 μCi
d)
330.125 μCi
Question 6. If the half-life of a radioactive element is 8 years, what percentage of the original sample
would be left after 32 years?
a)
6.25%
b)
3.125%
c)
12.5%
d)
0.064%
Question 7. If Pu-238 loses an alpha particle what element is formed?
234
242
a)
U
b)
Cm
238
238
c)
U
d)
Pu
Question 8. Absorbing a neutron will have what affect on the nucleus?
a) increase atomic mass # by 2 a) increase atomic mass # by 1
a) decrease atomic mass # by 2 a) decrease atomic mass # by 1
Question 9. If the density of a liquid is 1.07g/mL, what volume does 32.4 g of it have?
a) 30.28 mL
b) 30.3 mL
c) 34.7 mL
d) 0.0330 mL
Question 10. Which element has the smallest Atomic Radius?
a) Ti
b) V
c) Mn
d) Zn
Question 11. What is the density of a liquid that has a volume of 34.6 mL and a mass of 39.67 g?
a) 1.147 g/mL
b) 1.00 g/mL
c) 1.15 g/mL
d) 0.872 g/mL
Question 12. What does the metric prefix μ mean?
a) 103
b) 10-3
c) 106
d) 10-6
Question 13. Which form of radiation is the most dangerous?
a) alpha particle
b) beta particle
c) positron
d) gamma radiation
Question 14. Given that TF= 1.8TC +32, what is 344.8◦F in Kelvin and Celsius?
Question 15. Write the long form electron configuration, abbreviated electron configuration, the
number of valence electrons, and the electron dot symbol for the following:
a) P
b) N
c) C
Question 16. Convert the following:
a) Given that 2.20 lbs. are in 1 kg, and there are 16 ounces in a lb., how many kg are in 242.3 oz?
b) Convert 5.657x105 mL to ML.
c) 4.65x107 sec to years.
Question 17. How many Cal. and kJ are in a food item that has 2.5g of fat, 8.5g of carbohydrates, and
3.5g of protein(Fat = 9Cal/g, Prot and Carb = 4 Cal/g)?
Question 18. What will the final temperature be if 237500 Joules are used to heat 685.0g of water
initially at 2.5◦C (Heat = Mass x ∆T x Specific Heat; Specific Heat of water = 4.184J/g◦C)?
Test 2 Materials
Question 1. Draw the electron dot formulas for the following:
a) NCl2H (N is central atom)
b)CO2 (1 N is central atom)
c) For the compounds in question #5, give the number of electron groups, the electronic geometry
and the molecular shape of the molecules.
Compound
Electron
Groups
Electron
Molecular
Group
Shape
Arrangement
SCl2H
CO2
Question 2. Write the molecular formula for the following names:
a) Lead (IV) Sulfide
b) Molybdenum (V) Phosphate
c) Barium Phosphide
d) Ruthenium (III) sulfide
Question 3. Name the following covalent compounds:
a) PO3
b) F2S3
Question 4. The combustion of natural gas, CH4 is very important in energy production:
a) What is the balanced chemical equation for the combustion of natural gas?
b) If 25.5g of CH4 and 65.2g of O2 are burned, what is the limiting reactant?
c) How much water is produced(in grams)?
d) What is the percent yield if only 18.5g of H2O are collected?
Question 5. Consider the reaction:
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
a) What type of reaction is it?
b) What species is being reduced and what is being oxidized?
Question 6. Consider the Molecule VO(H2PO4)2:
a) What is its Molar Mass?
b) How many moles are in 234.5g of it?
c) How many moles are 8.36x1022 molecules?
d) How many H atoms are in 1 molecule of it?
e) How many O atoms are in 7.35 moles?
Question 7. Write the Balanced Formulas for the following Anions and Cations:
O2CO32N3FSr2+
Mo4+
V5+
Na+
Fe3+
Question 8. What is the pressure (in mmHg) of a gas that occupies 1.345x108μL, has a temperature of
67.3◦C and contains 1.76 moles of N2?
Question 9. At standard temperature and pressure (STP), how many moles of N2 occupy 5.83x10-3ML?
Question 10. A container of Xe gas at -23◦C occupies 3.45L at a pressure of 2.45atm. What volume (in L)
does it occupy at 72◦C at a pressure of 657mmHg?
Question#11 How many moles of oxygen can be produced from one mole of KClO3 in the reaction:
2KClO3→2KCl + 3O2?
a) 1 mol
c) 2 mol
b) 1.5 mol
d) 3 mol
Question#12 The number of C atoms in 0.500 mole of C is_______.
a) 2.50 × 1023 C atoms
b) 3.01 × 1023 C atoms
c) 5.01 × 1023 C atoms
d) 6.00 × 1023 C atoms
Question#13 How many moles of O atoms are there in 2 moles of glucose: (C6H12O6)?
a) 2 moles
b) 24 moles
c) 6 moles
d) 12 moles
Question#14 What is the molar mass of S3 if the molar mass of sulfur is 32.0?
a) 64 g
b) 32 g
c) 96 g
d) 10.7 g
Question#15 What is the percent yield if 50 g of CO2 were collected and 200g were expected?
a) 50%
b) 25%
c) 75%
d) 100%
Question#16 Which of the following reactions can be classified as decomposition?
a) CuCO3 (s) → CuO (s) + CO2 (g)
b) 4Fe (s) + 3O2 (g) → 2Fe2O3 (s)
c) Mg (s) + 2AgNO3 (aq) → Mg(NO3)2 (aq) + 2Ag (s)
d) NaOH (aq) + HCl (aq) → NaCl (aq) + H2O (l)
Question#17 What is the correct name of the ionic metal compound: AuCl3?
a) gold chloride
b) gold trichloride
c) gold (III) chloride
d) gold (III) trichloride
Question#18 What is the name of the covalent compound: S3Cl5?
a) Sulfur chloride
b) Sulfur hexachloride
c) Trisulfur chloride
d) Trisulfur pentachloride
Question#19 What is the correct formula for Chromium (VI) hydroxide?
a) Cr(OH)3
b) Cr(OH)6
c) CrOH6
d) Cr6OH
Question#20 How many electrons were lost by Pb in Lead (IV) chloride?
a) 4
b) 5
c) 0
d) 6
Test 3 Materials
1. A patient receives 250 mL of a 4% (m/v) mannitol solution every hour. The number of grams
of mannitol is_______.
a) 8
b) 10
c) 15
d) 20
2. Write the balanced equation for dissociating the following solid ionic salts in water:
a) Na2CO3(s)
b) (NH4)3PO4(s)
3. (15pts) Which of the following reaction has a precipitate. Use the solubility rules and predict
the products, if there is an insoluble product then write the total ionic equation and the net ionic
equation for the reaction.
a) KNO3(aq) + Na2SO4(aq)
or
b) (NH4)2SO4(aq) + Ca(NO3)2(aq)
4. How many grams of a solution of 1.760%(m/m) Na2S can be made with a starting Na2S mass of 6.278
g?
5. How many liters of a 1.250 M HCl solution will react with 13.68g of Na?
Na(s) +2HCl(aq) → H2 (g) + 2NaCl(aq)
6. Write the balanced equation for the neutralization reaction between the following acid/base
pairs:
a) Mg(OH)2 + H2SO4
b) Al(OH)3 + H2CO3
7. Calculate the [H3O+] or the pH of the following solutions, and say wither the solution is
acidic, basic, or neutral:
a) pH= 5.352
b) [H3O+] = 0.006001 M
8. What volume of a 0.0150M HCl solution would be neutralized by 32.25 mL of a 0.020M
NaOH solution?