Bonding,
Chemical
Reactions, and
Nomenclature
Reactions in
Aqueous
Solutions
Measurements,
Units, and the
Mole
Stiochiometry
Energy and
Thermochemistry
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Question 1 - 10
What is the name for HNO3?
Answer 1 – 10
Nitric Acid
Question 1 - 20
What type of bond represents a sea of electrons?
Answer 1 – 20
• Metallic Bonding
Question 1 - 30
The electrons in a nonpolar covalent bond are:
a)Unequally shared between atoms
b)Just exist and do not interact
c) Shared equally between atoms
Answer 1 – 30
C) Shared equally between atoms
Question 1 - 40
Balance this equation:
__ HF(aq)+__Ca(OH)2(aq) → __ H2O(aq)+__ CaF2 (aq)
Answer 1 – 40
2 HF(aq)+Ca(OH)2(aq) → 2 H2O(aq)+ CaF2 (aq)
Question 1 - 50
Name 6 polyatomic ions
Answer 1 – 50
NH4+
NO2NO3SO32OHCN-
Question 2 - 10
1. What are the products in this double
displacement reaction?
NaOH (aq) + MgCl2 (aq) → ??
2. Does a precipitate form?
Answer 2 – 10
1. 2NaOH (aq) + MgCl2(aq) → 2NaCl + Mg(OH)2
2. Yes! Mg2+(aq) + 2OH-(aq) → Mg(OH)2(s)
Question 2 - 20
What is a spectator ion?
Answer 2 – 20
• its an ion that is present in
solution but does not
participate in the reaction
Question 2 - 30
• What is the difference between a
strong base and a strong acid?
Answer 2 – 30
• Strong Acid completely
dissociates into H+ and anion in
water
• Strong Base completely
dissociates into OH and cation in
water
Question 2 - 40
• Explain how to distinguish between the
following types of reactions:
•
•
•
•
Single replacement
Double displacement (precipitation)
Synthesis
Acid-Base
Answer 2 – 40
• Single Replacement: element a + compound
BC → element B + compound AC
• Double Displacement/precipitation: a solid
forms after mixing solutions of 2 ionic
compounds
• Synthesis: 2 reactants → 1 Product
• Acid-Base: form H2O from H+ and OH- ions
Question 2 - 50
• How do you recognize the
correct chemical formula
for an ionic compound?
Answer 2 – 50
• When the (+) cation(s) combine with the (-)
anion(s) in a ratio that results in a net charge
of 0
Question 3 - 10
• How many zeros does Avogadro's Number
have?
Answer 3 – 10
• 24 zeros
– 6.02 x 10-23
Question 3 - 20
• What is the molar mass of
CO2 expressed with 3 sig
figs?
Answer 3 – 20
• 44.0 g/mol
– Carbon = 12.01 g/mol
– Oxygen = 16.00 g/mol (2x)
– Add all together = 44.01 g/mol
– 3 sig figs!
Question 3 - 30
• How many sig figs are in the
measurement 0.003540 kg?
Answer 3 – 30
• 4 sig figs
Question 3 - 40
• If the reactants areNa₂S and Cu(NO₃)₂, what
will the products be?
Answer 3 – 40
• NaNO₃ and CuS
Question 3 - 50
Determine the:
1.Empirical Formula
2.Molecular Formula
3.Percent Composition
Of a substance with the molar mass of 78 g/ mol
• Percent of C: 92.3 %
• Percent of H: 7.7 %
Answer 3 – 50
Question 4 - 10
• Stoichiometry heavily relies on _____ ratios.
Answer 4 – 10
• Mole
Question 4 - 20
• A sample contains 27.1 g of calcium
oxide. How many moles of calcium oxide are
in the sample?
Answer 4 – 20
• 0.483 mol
Question 4 - 30
• A 2.00 g sample of ammonia is mixed with
4.00 g of oxygen. Which is the limiting
reactant and how much excess reactant
remains after the reaction has stopped?
4 NH3(g) + 5 O2(g)  4 NO(g) + 6 H2O(g)
Answer 4 – 30
• Limiting Reactant:
• Excess Reactant:
Question 4 - 40
• Define limiting reactant and excess reactant.
Answer 4 – 40
• Limiting Reactant - The reactant in a chemical reaction that limits the
amount of product that can be formed. The reaction will stop when all
of the limiting reactant is consumed.
• Excess Reactant - The reactant in a chemical reaction that remains when
a reaction stops when the limiting reactant is completely consumed. The
excess reactant remains because there is nothing with which it can react.
Question 4 - 50
• 90.0 g of FeCl3 reacts with 52.0 g of H2S. What
is the limiting reactant? What is the mass of
HCl produced? What mass of excess reactant
remains after the reaction?
Answer 4 – 50
•Grams of HCL: 60.8 g
•Limiting Reactant: FeCl3
•Excess reactant: 23.6 g H2S
Question 5 - 10
• Is burning coal an exothermic or an
endothermic reaction?
Answer 5 – 10
•Exothermic; heat is
leaving the system.
Question 5 - 20
• A 450 g piece of iron (specific
heat: 0.449 J/g°C ) is heated
from 22°C to 87°C. How much
heat was necessary to cause this
change?
Answer 5 – 20
• 13,000 J
Question 5 - 30
• Which of the following is not a state function?
Distance, energy, or temperature?
Answer 5 – 30
• Distance
Question 5 - 40
• How much energy is required to heat 7.40 mL
of water from 25°C to 46°C?
Answer 5 – 40
• q = mc delta T
• q = (7.40 g) (4.184 J/gC) (21 C)
– 7.40 mL X 1g/1mL = 7.40 g water
• q = 650. J
• 7.40 mL X 1g/1mL = 7.40 g water
Question 5 - 50
• 2O3  3O2
• O2  2 O
• NO + O3  NO2 + O2
∆H = - 427 kilojoules
∆H = + 459 kilojoules
∆H = - 199 kilojoules
• Calculate the Enthalpy (∆H) for the overall
reaction:
NO + O  NO2
Answer 5 – 50
•
•
•
•
Reverse reaction 1
Reverse reaction 2
Multiply reaction 3 by 2
Add the reactions, then divide by 2
•
delta H = +427 KJ – 459 KJ – 2 (199 KJ) = -430 KJ / 2 = -215 KJ