Download File

Chemical Reactions Chapter 12 Study Guide (Unit 9)
Name:_________________________Hr:______












Understand and be able to explain all of the key concepts.
Define and understand all of the survival words
Memorize the names and symbols for these elements: (Ag, Al, Ar, As, Au, B, Ba, Be, Br, C, Ca, Cd, Cs,
Cl, Co Cr, Cu, F, Fe, Fr, H, He, Hg, I, K, Kr, Li, Mg, Mn, N, Na, Ne, Ni, O, P, Pb, Rn, S, Sc, Si, Sn, Sr, Ti, U, Xe,
Zn)
Know the charges (oxidations numbers) of elements found in the s & p blocks.
Know which elements are transition metals and therefore require the charge in parenthesis when being
named. [ex. Sn (II) or Co (III) ]
Know the charges of Ag+1, Zn+2, Cd+2, Al+3, and Ga+3 (exceptions to the transition area)
Know how to use the Activity Series of Metals and Halogens for single replacement reactions
Know how to use the Solubility Rules
Know how to predict the products of any reaction
Know how to balance a chemical reaction
Know how to determine the net ionic equation.
Review all classwork (including your lab notebook) and quizzes.
Key Concepts



Hydrocarbons
Because carbon has four valence electrons, carbon atoms always form four covalent bonds.
Molecules of hydrocarbons are nonpolar
Carbon atoms can form chains that are named using the following naming convention:
o




o



Prefix is determined by the number of carbons
1 = meth
 5 = pent
2 = eth
 6 = hex
3 = prop
 7 = hept
4 = but
 8 = oct
Suffix is determined by the type of bond
Alkane CnH2n+2 (all bonds are single)
Alkene CnH2n (one bond is a double)
Alkyne CnH2n-2 (one bond is a triple)


9 = non
10 = dec
12.1 The Arithmetic of Equations
 A balanced chemical equation provides the same kind of quantitative information that a recipe
does.
 Chemists use balanced chemical equations as a basis to calculate how much reactant is needed or
product is formed in the reaction.
 A balanced chemical equation can be interpreted in terms of different quantities including numbers
of atoms, molecules, or moles; mass; and volume.
 Mass and atoms are conserved in every chemical reaction.
1|Page
Chemical Reactions Chapter 12 Study Guide (Unit 9)




12.2 Chemical Calculations
In chemical calculations, mole ratios are used to convert between moles of reactant and moles of
product, or between moles of products.
In a typical stoichiometric problem, the given quantity (starting quantity) is first converted to
moles. Then the mole ratio from the balanced equation is used to calculate the moles of the
wanted substance. Finally, the moles are converted to any other unit of measurement related to
the unit mole.
12.3 Limiting Reagent and Percent Yield
In a chemical reaction, an insufficient quantity of any of the reactants will limit the amount of
product that forms.
The percent yield is a measure of the efficiency of a reaction performed in the laboratory.
Survival Words
















Actual yield (372)
Atom (101)
Balanced equation (325)
Chemical equation (353)
Coefficients (325)
Excess reagent (369)
Limiting reagent (369)
Molar mass (294)
Mole (290)
Mole ratio (359)
Molecule (214)
Percent yield (372)
Representative Particle (290)
Stoichiometry (354)
Theoretical yield (372)
Yield (323)
Key Equations
𝐏𝐞𝐫𝐜𝐞𝐧𝐭 𝐘𝐢𝐞𝐥𝐝 =
𝐀𝐜𝐭𝐮𝐚𝐥 𝐘𝐢𝐞𝐥𝐝
× 𝟏𝟎𝟎
𝐓𝐡𝐞𝐨𝐫𝐞𝐭𝐢𝐜𝐚𝐥 𝐘𝐢𝐞𝐥𝐝
NOTE: You are responsible for memorizing the
polyatomic ion list and the diatomic elements!
2|Page
Chemical Reactions Chapter 12 Study Guide (Unit 9)
Review Questions
1.
2.
3.
a.
What changes during a chemical reaction?
What remains the same during a chemical reaction?
Balance the following equations
___Ba + ___H2SO3  ___BaSO3 + ___H2
b. ___C3H8 + ___O2  ___CO2 + ___H2O
c. ___Sn(NO2)2 + ___KI  ___SnI2 + ___ KNO2
d. ___Ni + ___O2  ___Ni3O4
e. ___H2 + ___O2  ___H2O
f. ___C7H14 + ___O2  ___CO2 + ___H2O
4. 4 Al + 3 O2  2 Al2O3
a. Draw a particle diagram for the equation shown.

b. How many total molecules are on the reactant side? _____________ How many atoms? _____________
c. How many total molecules are on the product side? _____________ How many atoms? _____________
d. How many different compounds exist in the reaction? __________________
5. Mg3N2 + 3 H2O  3 MgO + 2 NH3
a. Draw a particle diagram for the equation shown.

b. How many total molecules are on the reactant side? _____________ How many atoms? _____________
c. How many total molecules are on the product side? _____________ How many atoms? _____________
d. How many different compounds exist in the reaction? _______________
e. If the mass of products is 34 grams, what was the mass of the reactants? __________________
3|Page
Chemical Reactions Chapter 12 Study Guide (Unit 9)
6. Interpret the given equation in terms of relative numbers of a) representative particles, b) numbers of
moles, and c) masses of reactants and products.
2K (s) + 2H2O (l) 2KOH (aq) +H2 (g)
7. Balance the equation: C2H5OH (l) + O2 (g)  CO2 (g) + H2O (g). Show the balanced equation obeys the law
of conservation of mass by calculating the masses of reactants and products.
8. Acetylene gas (C2H2) and Calcium hydroxide are produced by adding water to calcium carbide (CaC 2). a)
Write the balanced chemical equation. b) How many grams of acetylene are produced by adding excess
water to 5.00 grams of calcium carbide?
9. Using the equation you balanced in the problem above, determine how many moles of water are needed
to react completely with 5.00 grams of calcium carbide.
10. The last step in the production of nitric acid is the reaction of nitrogen dioxide with water.
3NO2 (g) + H2O (l)  2HNO3 (aq) + NO (g)
How many grams of nitrogen dioxide must react with water to produce 5.00 x 10 22 molecules of nitrogen
monoxide?
11. How are mole ratios used in chemical calculations?
12. Write a sequential list of steps required to solve most typical stoichiometric problems.
13. Write the 12 mole ratios that can be derived from the equation for the combustion of isopropyl alcohol.
2C3H7OH (l) + 9O2 (g)  6CO2 (g) + 8H2O (g)
14. a) Write the equation for the complete combustion of ethene.
b) If 2.7 mol of ethane is reacted with 6.3 mole of oxygen gas, identify the limiting reagent.
c) Calculate the number of moles of water produced.
15. When 84.8 grams of iron (III) oxide reacts with an excess of carbon monoxide, iron and carbon dioxide are
produced.
a) Write the balanced chemical equation.
b) What is the theoretical yield of this reaction for each product?
16. If 50.0 grams of silicon dioxide is heated with an excess of carbon, 27.9 grams of silicon carbide is
produced.
SiO2 (s) + 3C (s)  SiC (s) + 2CO (g)
What is the percent yield of this reaction?
17. If you were given 12 grams of Mg and excess amounts of 6 molar hydrochloric acid (6 mol HCl/L H2O),
exactly how much hydrochloric acid (in mL) would you need to react all of the magnesium? What is the
balanced chemical equation for this chemical reaction?
4|Page