Chemistry Review Assignment 1. Complete the table:
Element Element Symbol Protons Electrons Neutrons
Calcium Flourine Uranium
2. What would be the molecular difference between C-12 and C-14? 3. List 3 physical properties of:
a. francium b. lead c. iodine
4. Use periodic trends to determine which element, potassium or selenium, has the following:
a. larger radius _____________
b. larger electronegativity _____________ c. larger electron affinity _____________ d. larger ionization energy _____________
5. Use the periodic trends to determine which element, fluorine or chlorine, has the following:
a. larger radius _____________
b. larger electronegativity _____________ c. larger electron affinity _____________ d. larger ionization energy _____________ 6. Name the following compounds
a. P3F6
b. Ca3N2
c. H2SO4
d. Ba(OH)2
7. Write the formula for the following a. sodium bromide
b. dinitrogen pentoxide c. iron (II) sulfide
e. SCl3
f. K3PO4
e. carbon triflouride
5. Calculate the density of an object with a mass of 5 grams and a volume of 20 cm3.
6. How many grams of KNO3 can be dissolved into 100mL of water at 20C?
7. What type of solution is formed with 25g of NaNO3 is placed in 100g of water at 10C?
8. Identify the following as soluble or insoluble using the solubility rules: a. calcium sulfate
b. ammonium carbonate c. potassium nitrate d. strontium hydroxide 9. Complete the table on bonding:
Compound Formula Ionic/Covalent Dot Structure
Shape Molecular
Polarity
Diatomic nitrogen
Calcium chloride
Carbon tetrachloride
Sulfur triflouride
Fluorine trihydride
10. Which of the compounds above would have high electrical conductivity? 11. Which of the compounds above would have low melting points?
12. Convert:
a. 6 moles of calcium bromide to grams b. 25 grams of sodium carbonate to moles c. 0.02 moles of water to atoms of hydrogen
d. 56 grams of magnesium phosphate to formula units
13. Calculate the empirical and molecular formula for a compound with a molar mass of 180 grams, and is composed of 40% carbon, 6% hydrogen, and 53% oxygen.
14. Calculate the percent composition for the following: a. calcium sulfate
b. ammonium carbonate c. potassium nitrate d. strontium hydroxide
15. Predict the products, balance each equation, and write net ionic equations for DR reactions: a. potassium chlorate →
b. methane (CH4) + oxygen →
c. aluminum + oxygen → d. benzene (C6H6) + oxygen →
e. Mg(ClO3)2 →
f. magnesium bromide + chlorine g. aluminum + iron (III) oxide h. silver nitrate + zinc chloride i. sulfuric acid + sodium hydroxide j. zinc + hydrochloric acid
l. H2SO4 + Ba(OH)2
16. Solve:
a. A sample of air has a volume of 550.0mL at 106oC. At what temperature will its volume
be 700.0mL at constant pressure?
b. A sample of gas at 104oC and 0.870 atm occupies a volume of 3.0L. What volume
would this gas occupy at 60oC and 1.7 atm?
c. A mixture of three gases A, B and C is at a total pressure of 8.15 atm. The partial pressure of gas A is 300kPa ; that of gas B is 2100mmHg. What is the partial pressure of gas C?
d. What is the volume in liters of 2.30 mol of N2 at STP?
e. What is the volume in liters of 2.00 mol of F2 at 100 K and 150 atm?
f. Calculate the number of moles of gas contained in 1.0L at 273K and 1.5 atm.
17. What happens to the temperature of a substance as it undergoes a phase change? 18. What phase does water exist in at 1 atm and 90C?
19. What phase does water exist as at 0.5 atm and 40C? 20. Solve:
a. find the molality when 75.0 grams of MgCl2 is dissolved in 500.0 g of solvent.
b. how many moles of HCl are in 2 L of 6 M HCl
c. Determine the molar concentration of a solution in which 320 grams of glucose C6H12O6 are dissolved
in 4000 grams of water
21. Solve:
a. How much heat will be absorbed by 130g of Mercury (0.14J/gC) when its temperature started at 24.0°C and after it was 78.0°C?
b. If an 83.00 g sample of Iron (0.46J/gC) has a starting temperature of 297K and an ending temperature of 329K, how much heat will be lost from the iron sample?
c. The heat absorbed by a sample of 55.00 g is 3908.3J and its starting temperature is 78.0°C and its ending temperature was 95.0°C. What is the specific heat of this sample and what is the sample? d. A sample of silver with a mass of 63.3 g is heated to a temperature of 111.3C and placed in a container of water at 16.85C. The final temperature of the silver (0.23J/gC) and water is 19.25C. Assuming no heat loss, what mass of water was in the container?
22. Identify the driving force behind each reaction (entropy or enthalpy) a. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g) + 890 kJ
b. 2 NaF(s) + energy 2 Na(s) + F2(g)
23. Exothermic reactions have values of H that are which, negative or positive? __________ What is the sign of H for endothermic reactions? _________
24. How long does it take a 180g sample of Au-198 (Au-198 = 2.69 days) to decay to 1/8 its original mass? 25. Fill in the following table with the correct values:
Solution pH pOH [OH-] [H+]
0.5M NaOH
2.1M HCl
0.24M HNO3
1.2M Ba(OH)2
26. Which of the solutions above would feel slippery?
a. HCl + NaOH --> NaCl + HOH
28. Predict the products of the following neutralization and hydrolysis reactions. a. H2SO4 + 2 NH4OH -
b. NaOH + H2CO3
c. MgCl2 + HOH
d. CaCO3 + HOH
28. The molarity of a HCl solution can be determined by titrating a known volume of the solution with a sodium hydroxide solution of know concentration. If 14.7 mL of 0.102 M NaOH is required to titrate 25.00 mL of a HCl solution, what is the molarity of the HCl solution?
