Chemistry Honors II – some stuff you should already know and/or be able to do
but may not remember
Atomic structure
1. How many protons, electrons, and neutrons are in each atom or ion? If no mass number is given the atom is the most common isotope of the element.
(a) copper-64(e)
(b) hydrogen-3 (aka tritium)(f)
(c) sulfur(g) Pb 4+
(d) (h) K 1+
Periodic table & periodic trends
2. Identify the element or an element that the statement describes.
(a) the noble gas in period 4(h) an alkali metal with lower ionization energy
(b) the alkali metal is period 2 than potassium
(c) a transition element in period 6(i) a period 2 element with higher
(d) the halogen in period 3 electronegativity than nitrogen
(e) atransuranium element (j) a nonmetal element that typically forms two
(f) a period 3 element with a covalent bonds in molecules
larger radius than Si(k) an element with the same number of valence
(g) an alkaline earth metal with electrons as nitrogen
a larger radius than Sr(l) a period 3 element that forms a 3+ ion
Chemical nomenclature
3. Give the correct formula of each element or compound.
(a) gold(e) sodium sulfide(i) copper(II) oxide
(b) fluorine(f) magnesium nitride(j) iron(III) chloride
(c) dinitrogen trioxide(g) barium hydroxide(k) tin(IV) carbonate
(d) sulfurhexachloride(h) zinc phosphate(l) ammonia
4. Give the correct IUPAC or STOCK system name for each compound.
(a) KNO3(d) CuC2H3O2(g) H2S
(b) Al2O3(e) KMnO4(h) BF3
(c) Cr2O3(f) W(CO3)2(i) N2O5
Chemical reaction equations
5. Balance the following reaction equations with the smallest whole-number coefficients. Identify the type of reaction as one of the five types of simple reactions.
(a) Na + H2O NaOH + H2(d) C2H6 + O2 CO2 + H2O
(b) KClO3 KCl + O2(e) Fe + O2 Fe2O3
(c) H3PO4 + Ba(OH)2 Ba3(PO4)2 + H2O
6. Complete and balance the following reactions. Reactions a & b are single-replacement reactions. Reactions c & d are double-replacement reactions.
(a) Mg + AgNO3 (d) CaCl2 + Na2CO3
(b) NaBr + Cl2 (e) H2SO4 + KOH
(c) HCl + Pb(NO3)2
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descriptive gas properties
7. Whatword or words in parentheses will make the statement correct according to the kinetic-molecular theory of gases you learned in Hon. Chem.
(a) The particles of a gas are (far apart or close together).
(b) The particles of a gas have (strong or weak or no) attractive forces for each other.
(c) As the temperature of a sample of gas increases the average speed of the particles of
the gas will (increase or decrease or stay the same).
(d) The Kelvin temperature of two samples of different gases is equal. The (average
kinetic energy or speed) of the particles of the different gases is also the same.
(e) A gas will occupy (the entire volume or some but not all the volume) of its container.
(f) The (pressure or volume or temperature) of a gas is due to the collisions between the
gas particles and the walls of its container.
(g) If the temperature of a gas increases but the amount and pressure do not change
then the volume of the gas (must increase or must decrease or possibly not change).
(h) If the volume of a gas increases but the amount and temperature do not change
then the pressure of the gas (must increase or must decrease or possibly not
change).
(i) If the pressure on a gas increases and the temperature decreases and the amount
does not change then the volume of the gas (must increase or must decrease or
possibly not change).
(k) If the volume of a gas increases and the temperature increases and the amount does
not change then the pressure of the gas (must increase or must decrease or
possibly not change).
(l) 20 L of Ne at STP will contain (twice as many or half as many or thesame
number of) moles of atoms as 20 L of Ar at STP.
(m) 20 L of Ne at STP will contain (twice as many or half as many or the same
number of) grams of atoms as 20 L of Ar at STP.
descriptive solution properties
8. The questions below refer to these four solutions:
solution P1 L of 1 M FeCl3
solution Q2 L of 1 M CuCl2
solution R2 L of 2 M NaCl
solution S2 L of 2 M KCl
(a) Which solution, P or Q, is more concentrated?
(b) Which solution, Q or R, is more concentrated?
(c) Which solution, P or Q, contains more moles of solute?
(d) Which solution, Q or R, contains more moles of solute?
(e) Which solution, R or S, contains more moles of solute?
(f) Which solution, R or S, contains more grams of solute?
(g) Which of the solutions will conduct electricity?
(h) In which solution is the concentration of chloride ions highest?
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problems You may need a periodic table and/or information from a reference book or
from the internet.
1. Convert the given quantity into the new unit.
(a) 427 mL to liters(c) 0.871atm to kPa(e) 52 J to kJ
(b) -47oC to K(d) 1000. mmHg to atm(f) 891 μg to grams
2. A piece of metal has a mass of 47 g. A graduated cylinder contains 29.6 mL of water. When the metal is put into the water, the water level in the graduated cylinder rises to 32.0 mL. What is the density and what is the identity of the metal?
3. Copper has two primary isotopes, with a mass of 62.93 amu and with a mass of 64.93 amu. The relative abundance of Cu-63 is 69.09 % and the relative abundance of Cu-65 is 30.91%. What is the average atomic mass of copper?
4. What is the molar mass of each substance to three significant figures?
(a) Ge(b) VF3(c) Au2(SO3)3
5. Convert the given quantity to the requested quantity.
(a) 0.87 mol Ne to atoms(c) 43.5 g Ne to mol
(b) 0.87 mol Ne to grams(d) 8.66 X 10 22 atoms Ne to grams
6. What is the percent nitrogen by mass in each compound?
(a) NH4ClO3(b) Ba(NO3)2(c) Ba(NO3)2●2H2O
7. How many grams CuSO4●5H2O must I mass to have 1.50 g CuSO4 ?
8. What is the empirical formula of each ionic compound?
(a) The compound is 86.7% lead and 13.3% oxygen.
(b) The compound is 36% aluminum and 64% sulfur.
9. The compound caffeine is 49.48% carbon, 5.19% hydrogen, 28.85% nitrogen, and
16.48% oxygen. The molar mass of the compound is 97.0 g/mol. What is the molecular formula of the compound?
10. The questions refer to the reaction:2Na + 2H2O 2NaOH + H2
(a) How many moles H2 are produced when 4.8 mol Na react?
(b) How many grams water are required to react with 4.8 moles Na?
(c) How many grams NaOH are produced when 4.8 g Na react?
(d) How many liters of H2 are produced at 1.4 atm and 300 K when 4.8 g Na react?
(e) When 4.8 g Na react, only 5.3 g NaOH are actually produced. What is the percent
yield of the reaction?
(f) I have 40 g Na and 60 g H2O available to react. Which is the limiting reactant?
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11. I have 450. mL of 0.239 M CaBr2 solution. This is the “original solution.”
(a) Write the dissociation equation for solid CaBr2 dissolved in water.
(b) What are the concentrations of Ca 2+ and Br 1- in the original solution?
(c) How many moles and how many grams CaBr2 are in the original solution?
(d) I dilute 300. ml of the original solution to a volume of 1.28 L. What is [CaBr2] in
this dilute solution?
(e) I add 0.100 M AgNO3 to 25.0 mL of the original solution. How many mL of the
AgNO3 solution are needed to completely precipitate AgBr from this sample of the
original solution?
12. Calculate the volume of Ne gas present in each situation described below.
(a) 1.25 mol Ne at STP
(b) 1.25 mol Ne at 750 mmHg and 127oC
(c) A fixed amount of Ne at 87.8 kPa and a volume of 1.44 L ischanged to 127 kPa at
constant temperature.
(d) A fixed amount of Ne at 2.88 atm, 27oC, and a volume of 40.0 L is changed to
1.44 atm and -73oC.
13. A compound contains only calcium and bromine.
Analysis of the compound gives the amounts
of calcium and bromine in a sample. Different
samples were analyzed and the results are
shown on the graph.
(a) How many grams calcium are in a sample
that contains 30. g bromine?
(b) What was the mass of a sample that
contained 15 g calcium?
(c) What is the % calcium in the compound?
(d) What is the empirical formula of the compound?
14. The drawing below represents two samples of gas in separate
containers. The right container has twice the volume of the left container. The two gases are at the same temperature. The gas in the left container is neon and the gas in the right container is argon. The two containers are kept isolated by a partition. The balls represent relative numbers of atoms of the two gases. The volume of the connecting tube is negligible.
(a) In which container are there more
moles of gas?
(b) In which container is the gas
pressure higher?
(c) The pressure of the neon is 6 atm.
What is the pressure of the argon?
The partition is removed and the gases
thoroughly mix without changing temperature.
(d) What is the partial pressure of each gas in
the mixture?
(e) What is the total pressure in the container after mixing?
My answers to the questions on pages 1 & 2.
1.
question / protons / electrons / neutronsa / 29 / 29 / 35
b / 1 / 1 / 2
c / 16 / 16 / 16
d / 6 / 6 / 8
e / 92 / 92 / 143
f / 35 / 36 / 44
g / 82 / 78 / 126
h / 19 / 18 / 20
2. (a) Kr(e) Np-Lr(i) O, F
(b)Li(f) Na, Mg(j) C, Si
(c)La, Hf-Hg(g) Ba, Ra(k) P, As, Sb, Bi
(d)Cl(h) Na, Li(l) Al
3. (a) Au(e) Na2S(i) CuO
(b) F2(f) Mg3N2(j) FeCl3
(c) N2O3(g) Ba(OH)2(k) Sn(CO3)2
(d) SCl6(h) Zn3(PO4)2(l) NH3
4. (a) potassium nitrate(d) copper(I) acetate(g) hydrogen sulfide
(b) aluminum oxide(e) potassium permanganate(h) boron trifluoride
(c) chromium(III) oxide(f) tungsten(IV) carbonate(i) dinitrogenpentoxide
5. (a) 2Na + 2H2O 2NaOH + H2
(b) 2KClO3 2KCl + 3O2
(c) 2H3PO4 + 3Ba(OH)2 Ba3(PO4)2 + 6H2O
(d) 2C2H6 + 7O2 4CO2 + 6H2O
(e) 4Fe + 3O2 2Fe2O3
6. (a) Mg + 2AgNO3 2Ag + Mg(NO3)2
(b) 2NaBr + Cl2 Br2 + 2NaCl
(c) 2HCl + Pb(NO3)2 PbCl2 + 2HNO3
(d) CaCl2 + Na2CO3 CaCO3 + 2NaCl
(e) H2SO4 + 2KOH K2SO4 + 2H2O
7. (a)far apart(f) pressure(j) must decrease
(b)no(g) must increase(k) possibly not change
(c)increase(h) must decrease(l) the same number of
(d)average kinetic energy(i) must decrease(m) half as many as
(e) the entire volume
8. (a)same concentrstion(c) Q(e) same moles solute(g) all four
(b) R(d) R(f) S(h) P
My answers to problems on pages 3 & 4
1. (a) 0.427 L(c) 88.2 kPa(e) 0.052 kJ
(b) 226 K(d) 1.316atm(f) 0.000891 g or 8.91 X 10 -4 g
2. density = 19.6 g/cm3 and gold
3. 63.55 amu
4. (a) 72.6 g/mol(b) 146 g/mol(c) 682 g/mol
5. (a) 5.2 X 10 23 atoms(b) 18 g (c) 2.16 g(d) 2.90 g
6. (a) 13.8% N(b) 10.7% N(c) 9.42% N
7. 2.34 g CuSO4 ● 5H2O
8. (a) PbO2(b) Al2S3
9. C4H5N2O
10. (a) 2.4 mol H2(c) 8.3 g NaOH(e) 64%
(b) 8.6 g H2O(d) 1.8 L H2(f) Na is the limiting reactant.
11. (a) CaBr(s) Ca 2+ (aq) + 2Br 1- (aq)
(b) [Ca 2+ ] = 0.239 M and [Br 1- ] = 0.478 M
(c) 0.108 mol CaBr2 and 21.5 g CaBr2
(d) [CaBr2] = 0.0560 M
(e) 120. mL 0.100 M AgNO3
12. (a) 28.0 L(b) 41.5 L(c) 1.00 L(d) 40.0 L
13. (a) 7.5 g Ca(b) 75 g(c) 25% Ca(d) CaBr2
14. (a) right container(c) 4atm(e) 4.67 atm
(b) left container(d) Ne = 2 atm and Ar = 2.67atm