1. Give the number of significant figures in each of the following numbers:
a.) 876 b.) 832.020 c.) 0.000678 d.) 6070 e.) 1.67 x 105
2. Suppose that we need 5.00 g of a liquid that has a density of 0.664 g/cm3. What volume of the liquid will weigh 5.00 g ? Express your answer in liters.
3. Express the temperature 37.8 oC in oF and in Kelvin.
4. Give the name of each of the following elements:
a.) Na b.) C c.) Li d.) K e.) Fe f.) Ar
5. Give the symbol of each of the following elements:
a.) Silicon b.) lead c.) aluminum d.) zinc e.) silver f.) tin
6. Make the following conversions:
a.) 165 in2 to cm2 b.) 134 lbs to kg c.) 464 liters to cm3 d.) 444 gm to mg
7. Give the mass number of each of the following:
a.) sodium with 12 neutrons b.) an iron atom with 30 neutrons
8. Give the complete symbol (AZAX) for each of the following atoms:
a.) potassium with 20 neutrons b.) nitrogen with 8 neutrons c.) zinc with 34 neutrons
10. The platinum-containing cancer drug cisplatin contains 65.0% platinum. If you have 1.83 g of the compound, what mass of platinum (in grams) is contained in this sample?
11. The synthetic radioactive element technetium is used in many medical studies. Give the number of electrons, protons, and neutrons in an atom of technetium-99.
12. Verify that the atomic mass of magnesium is 24.31 amu, given the following information.
24Mg, mass = 23.985042 amu; percent abundance = 78.99%
25Mg, mass = 24.985837 amu; percent abundance = 10.00%
26Mg, mass = 25.982593 amu; percent abundance = 11.01%
13. Reviewing the periodic table:
(a) Name an element in Group 2A. (b) Name an element in the third period.
(c) What element is in the third period in Group 4A? (d) What element is in the fifth period in Group 6A?
(e) What halogen is in the fourth period? (f) What alkaline earth element is in the third period?
(g) What noble gas element is in the fifth period? (h) Name the nonmetal in Group 6A and the second period. (i) Name a metalloid in the fourth period.
1. a.) How many atoms are in 24 molecules of fructose, C6H12O6?
b.) How many moles are in 12.50 mL of liquid bromine if the density of bromine is 3.12 g/mL?
c.) How many grams of NO2 contain the same number of molecules as 15.00 grams H2O?
2. a.) What is the correct name of FeSO4 ?
b.) What is the correct name of KClO4?
c.) Give the ions present and their relative numbers in potassium sulfate.
d.) What is the formula for sodium bicarbonate?
e.) What is the formula for iron(II)oxide and iron(III)oxide?
f.) What is the name of each of the following: Hg2SO4, Co2(SO4)3, FePO4?
3. a.) What is the weight percent of carbon in oxalic acid, H2C2O4?
b.) Calculate the empirical formula of a compound which is 51.40% carbon, 8.63% hydrogen, and 39.97% nitrogen.
c.) Give the symbol and the correct charge for each of the following ions: sulfate ion, perchlorate ion, permanganate ion, hypochlorite ion, dihydrogen phosphate ion.
d.) Calculate the molar mass of each of the following compounds: Fe(C6H11O7)2, C20H24N2O2.
4. a.) How many moles of each are present if you have 2.535 g of each: C8H8O4 (aspirin) and C14H10O4 (benzoyl peroxide)
b.) Calculate the mass percent of each element in the following compounds, to the nearest 0.1%: C3H8, MgCO3.
c.) Nicotine is 74.0% C, 8.65% H, and 17.35% N and its molar mass is 162 g/mol. What is its molecular and empirical formula?
d.) Always look closely at labels. What percentage of iron is in each of the two iron supplements FeSO4 and Fe(C6H11O7)2?
5. We do an elemental analysis of a compound and determine that it only contains the elements C, H, and O. Then we combust 0.513 g of the compound and then we determine the amount of carbon dioxide and water generated in the reaction to be 0.501 g and 0.103 g respectively. What is the empirical formula of the unknown compound?
1. 3 CCl4(l) + 2 SbF3(l)--> 3 CCl2F2(l) + 2 Sb Cl3(s) is the balanced equation for making Freon. We start the reaction using 150 g of CCl4 and 100 g of SbF3.
a.) What is the limiting reagent?
b.) How many grams of Freon are produced?
2. Balance the following reactions:
a.) B4H10(s) + O2(g)--> B2O3(s) + H2O(g)
b.) C4H10(g) + O2(g) --> CO2(g) + H2O(g)
c.) Al(s) + Br2(g)--> Al2Br6(s)
d.) State the atoms that exist as diatomics.
3. Starting with 0.145 g of Mg, how much MgO is produced in the following reaction?
Mg(s) + O2(g) MgO(s)
4. Suppose that we start with 14.43 g salicylic acid (C7H6O3) and that we obtain 6.26 grams of aspirin. What is the percent yield?
2 C7H6O3(s) + C4H6O3(l) --> 2 C9H8O4(s) + H2O(l)
5. a.) What are the ion concentrations in a 0.50 M solution of (NH4)2SO4?
b.) How many grams of Na2CO3 are needed to make 2.0 L of a 1.5 M solution of Na2CO3?
c.) Your boss asks you to prepare 500. ml of a 0.200 M solution of KMnO4. How do you do it and keep your job (do it correctly)?
d.) You need 300. ml of a 1.00 M NaOH solution and your lab has a large bottle of 3.00 M NaOH. How do you obtain what you need?
e.) Define molality and mole fraction.
6. Predict whether each of the following ionic compounds is likely to be water-soluble. If a compound is soluble, list the ions that would exist in solution: a.) KCl b.) MgCO3 c.) MnO2 d.) CaI2
7. a. A precipitation reaction produces an insoluble product called a _________.
b. Ions called ________ ions are not involved in the net reaction process.
c. Write a balanced net ionic reaction for the reaction of AgNO3 and CaCl2 to yield
AgCl and Ca(NO3)2.
d. Give an example of an acidic oxide.
8. a. An acid is any substance that, when dissolved in water, increases the concentration
of _______ ions.
b. A strong acid is completely dissociated into ______ in an aqueous solution.
c. Write a balanced equation for the ionization of nitric acid in water.
9. a. A solution is a ________ mixture of two or more substances.
b. The substances in a mixture can be classified as either the ______ or the _______.
c. Compounds whose aqueous solutions conduct electricity are called ________.
d. The greater the amount of ________ of the compound, the stronger the electrolyte.