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FINAL REVIEW PACKET
Nomenclature
1. Polyatomics
2. An ionic compound is made up of a __cation_______ and a _anion_______. The first element is ALWAYS the
_cation______, which forms a _ion______ with a _positive______ charge. The second element is the
__anion______, which forms an _ion_________ with a __negative________ charge.
a. Give three examples (name and formula)
MgO magnesium oxice
FeCl3 iron (III) chloride
AlBr3 aluminum bromide
3. A covalent compound is made up of ___neutral atoms usually two nonmetals__________________.
a. Give three examples (name and formula)
PO2 phosphorous dioxide
N2Cl6 dinitrogen hexachloride
CO2 carbon monoxide
b. To name covalent molecular compound, use __prefixes to show _subscripts_______________________.
4. Differentiate between a binary and ternary compound
a. Binary, two elements, ternary three of more elements
b. Give three examples of ternary compounds (name and formula)
KNO3 potassium nitrate
NH4OH ammonium hydroxide
MgSO3 magnesium sulfite
5. When is the Stock Naming system used.
a. Why? To show the oxidation number a transition element used.
b. Give three examples (name and formula)
FeCl2 iron (II) chloride
FeCl3 iron (III) chloride
FeO iron(II) oxide
6. Name the following
a. CaCr2O7 calcuim dichromate
b. Pb(SO3)2 lead (IV) sulfite
c. N3O6 trinitrogen hexoxide
d. Na3N sodium nitride
e. H3PO4 phosphoric acid
f. HF hydrofluoric acid
7. Give formula for
a. Hydroselenic acid H2Se
b. Hydrocyanic acid HCN
c. Perchloric acid HClO5
d. Sulfurous acid H2SO3
e. Hypomanganic acid H3MnO4
f. Barium chloride BaCl2
g. Vanadium (V) sulfide V2S5
h. Tetraphosphorous decaoxide P4O10
i. Nitrogen heptasulfide NS7
j. Aluminum phosphate AlPO4
k. Ammonia NH3
l. Hydrogen peroxide H2O2
m. Methane CH4
Chemical reactions
8. List five indicators of a chemical change
a. Bubbling
b. Temperature change
c. Precipitate
d. Color change
e. Mass change
9. What is the only way to determine that a chemical reaction has taken place? Can not be undone
10. Give the general format for a chemical reaction. Reactants  products
11. Identify the following symbol.
a.  yield
b. Δ change in heat
c.
Mn On
catalyst
d. + and
e. (s) solid
f. (g) gas
g. (aq) aqueous, in solution, dissolved in water
h. (l) liquid
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12. A) Predict products and B) Write a complete balanced chemical equation for the following equations. C) Indicate
whether reaction will or will not occur. D) Indicate WHY. E) Indicate type of reaction.
a. Ammonium hydroxide rapidly decomposes in the presence heat to form ammonia and water
heat
NH4OH  NH3 + H2O decomposition, will occur due to increased entropy
b. Carbon dioxide and water are formed as a result of the combustion of methane gas.
CH4(g) + 2O2  CO2 + 2 H2O combustion, will occur
c. A barium sulfate precipitate and aqueous sodium chloride are formed from the metathesis reaction
between barium chloride and sodium sulfate solutions.
BaCl2(aq) + Na2SO4(aq)  BaSO4(s) + NaCl(aq) double replacement will occur forms a precipitate
d. Zinc and dissolved copper II chloride react to form copper metal and zinc chloride.
Zn + CuCl2(aq)  ZnCl2 + Cu will occur, sincle replacement, zinc is more active than
copper
e. The dissolution of sulfur trioxide in water is a major source of acid rain through the formation of sulfuric
acid.
H2O + SO3
f.
 H2SO4 will occur synthesis reaction
Propane burns in air
C3H8 + 5O2  3CO2 + 4H2O combustion will occur
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Final Review Packet_Honors/Academy Chemistry
g. Magnesium reacts with nitrogen.
3Mg + N2  Mg3N2 synthesis will occur
h. Calcium carbonate is heated
heat
CaCO3(s)  CaO + O2(g) decomposition
i.
Zn metal is placed in a solution of Copper sulfate
Zn(s) + CuSO4  ZnSO4 + Cu(s) will occur, single replacement, zinc is more reactive than copper
j.
Barium hydroxide and Lithium sulfate are mixed
Ba(OH)2(aq) + Li2SO4(aq)  BaSO4(s) + 2LiOH (aq) double replacement, will occur precipitate formed
k. Sodium hydroxide and Phosphoric acid are mixed.
3NaOH (aq) + H3PO4(aq)  Na3PO4(aq) + 3H2O(l) double replacement, neutralization, will not
occur, strong base, weak acid
l.
Calcium oxide in water.
CaO + H2O  Ca(OH)2 synthesis, will occur
m. Sodium in water
2Na(s) + 2H2O(l)  2NaOH + H2(g) single replacement, sodium replaces hydrogen in water will occur
)
13. What is the activity series? Why is it useful?
Identifies what elements will replace another in a compound, predicts if a reaction will occur
a. Know how to use it to predict whether a reaction will occur.
14. Determine solubility of each of the following.
a. Magnesium sulfate soluble
b. Sodium carbonate soluble
c. Calcium hydroxide soluble
d. Calcium sulfate insoluble
e. Silver nitrate soluble
f. Silver iodide insoluble
g. Lead (II) chloride insoluble
h. Lead (IV) bromide insoluble
i. Aluminum oxide insoluble
j.
15. Know difference in solubility rules for reactants vs. products.
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Final Review Packet_Honors/Academy Chemistry
Mole Quantities
16. Define mole 6.02x1024 particles
17. Convert the following
a. 4.58 mol to particles of Al = 2.76x1024
b. 4.58 mol to grams of Al = 124g
c. 901.49 g to particles of Carbon dioxide = 1.23x 1025
d. 901.49 g to L of carbon dioxide = 458.9
18. Define molar mass. The mass of a mole of a substance, equal to the atomic mass in grams
19. Give molar mass of
a. Vanadium = 50.94g
b. Vanadium IV oxide =82.94
c. Glucose =180
20. Define percent composition the percent of the total mass that each component contributes.
21. Give percent composition of
a. Aluminum carbonate = 23% Al 15% C 61%
b. Potassium phosphate = 55% K 14.6% P 30% O
22. Distinguish between empirical and molecular formula empirical is the simplest ratio of atoms in a compound,
the molecular is the actual number of atoms in a compound.
23. Solve the following
a. What is the percent composition of Nickel (II) oxide , if a sample with a mass of 41.9 g contains
33.1 g Ni and 8.8 g O? = 79% Ni 21% O
b. Calculate the molecular formulas of the compounds having the following empirical formulas and
molar masses:
i. C H , 58 g/mol; =C4H10
ii. CH, 78 g/mol; and =C6H6
iii. HgCl, 236.1 g/mol. = HgCl
c.
The percentage composition of acetic acid is found to be 39.9% C, 6.7% H, and 53.4% O. Determine
the empirical formula of acetic acid. If the molar mass is 60 g/mol, determine the molecular
formula for acetic acid. Empirical= CH2O molecular C2H6O2
24. STOICHIOMETRY (basic, Limiting Reactant, Excess Reactant, %Yield)
a. How many moles of oxygen are consumed when 96.7 moles of hydrogen sulfide gas are burned,
producing sulfur dioxide and water vapor in the process? =14.4 moles
b. If 3.70 x 1023 molecules of oxygen react with excess benzene (C6H6), how many grams of water can be
produced? =27g H2O
c. 25.0 g Calcium reacts with 40.0 g Oxygen. Determine mass of product formed. = 35.0g CaO (find limiting
reactant)
d. 500.0 L of Nitrogen gas and 600.0 L of Hydrogen gas are available and react to form Ammonia.
Determine mass of Ammonia that can be formed. How many Liters of Ammonia is produced? What is
the identity and amount of excess reactant left over. =303.5g NH3 357g of N2 is left over
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Final Review Packet_Honors/Academy Chemistry
e. 30.0 grams of acetic acid reacts with excess methanol (CH3OH) to produce 30.0 grams of methyl acetate
(CH3COOCH3) and water. Determine the percent yield of the reaction.
81% yield
f.
A chemist reacts 2.00 grams of vanadium (II) oxide with 5.75 grams of iron (III )oxide to produce
vanadium (V) oxide and iron (II) oxide. The reaction goes to 67.0% completion. How many grams of the
iron (II) oxide are produced?
(balance oxidation reduction)
Limiting reactant iron (III) oxide
Theoretical yield 5.175g
67% of that is 3.47g produced.
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Final Review Packet_Honors/Academy Chemistry