0: Honors Chemistry Name: Review for Midterm Class

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0: Honors Chemistry
Review for Midterm
Name:
Class:
Date:
BONDING
1. Consider the following chemical formulas: NaCl, H2O, and N2. For each formula,
a. Draw the Lewis dot structure.
b. Label each Lewis dot structure as polar covalent bond, nonpolar covalent bond, or
ionic bond. Include evidence for each label.
c. Identify the VSEPR shape of any covalent molecules.
2. Complete the table below about bonding theories.
Bonding Type
Types of Atoms in Bond
Behavior of Electrons
Metal and a nonmetal (or a
polyatomic ion)
Metallic
Electrons are shared EQUALLY in a single,
double, or triple bond.
Nonmetals
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3. Using the chart below, identify the bonding type of each substance. Justify your answer.
Physical Properties of Substances A, B, and C
Solubility in a…
Substance
Nonpolar
Conductivity
Polar Solvent
Melting Point Boiling Point
(solids)
Solvent
(as a solid)
A
Yes
No
No
High
High
B
No
Yes
No
Low
Low
C
No
No
Yes
High
High
A:
B:
C:
4. Use the electronegativity difference to determine if the bond type.
Element A
Element B
Electroneg. A Electroneg. B
Difference
Ca
Cl
C
H
O
O
Bond Type
5. Based on the types of atoms, predict if each pair of atoms will form an ionic, metallic, or
covalent bond.
Element A
Element B
Atom Type A
Atom Type B
Bond Type
Fe
O
Na
Mg
O
O
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6. Use the electron sea to explain the properties of metals.
7. Explain what happens to a metal when it combines with a nonmetal, in terms of
electrons.
8. Why do ionic compounds conduct when dissolved in water, but not as solids? Draw a
picture to explain and provide an example of such a compound.
9. What is meant by the phrase “like dissolves like”?
10.Determine the VSEPR shape of the following:
a. CH4
b. H2S
11.What do the “dots” in a Lewis dot structure represent?
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NAMING AND FORMULA WRITING
12.Complete the table below by writing in the bonding type, and the name or formula as
needed.
Ionic, Covalent,
Name
Formula
or Acid?
A
Sodium Carbonate
B
C
P4O10
Phosphorous Acid
D
E
FeSO4
Perchloric Acid
F
G
H2CrO4
Cobalt (II) bromide
H
I
LiC2H3O2
Copper (III) sulfate
J
K
L
HCN
Aluminum hydroxide
Cu3PO4
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13.For each of the following, determine if the formula is correct or incorrect. If incorrect,
change the formula so that it is correct.
a. CaCl
b. NH4NO3
c. H2CN
d. NaCrO4
e. Ca(OH)2
f. BaHCO3
14.The following name/ formula pairs are incorrect. Change the formula so that the pair is
correct.
a. CaBr, Calcium bromide
b. BaSO4, barium nitrate
c. FeCl2, Iron (III) chloride
d. CS, carbon disulfide
e. KNO2, Potassium nitrate
f. H2SO4, hydrosulfuric acid
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CHEMICAL REACTIONS
15.Explain the law of conservation of mass. How does a balanced chemical equation
illustrate this principle?
16.Identify the number of each type of atom in the following formulas.
a. Ca3(PO4)2
b. C3H5(OH)3
c. (NH4)2CrO4
17.Write the balanced chemical equation and indicate the type of reaction.
a. ___ N2 + ___O2  ___NO
b. Solid baking soda (sodium bicarbonate) is heated, forming carbon dioxide gas and
solid sodium oxide.
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c. ___ FeCl3 + ___ NaOH  ___ Fe(OH)3 + ___NaCl
d. Sodium phosphate and calcium chloride react to form calcium phosphate and
sodium chloride.
e. ___C3H8 + ___O2  ___CO2 + ___H2O
18.Use the experimental data below to construct an activity series.
A(NO3)2 B(NO3)2 C(NO3)2 D(NO3)2
A
-NR
Reaction Reaction
B
Reaction -Reaction Reaction
C
NR
NR
-NR
D
NR
NR
Reaction --
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19.Based on the activity series you constructed, which metals (X) will replace metal D in the
chemical reaction below?
X + DCl2  XCl2 + D
20.Complete the table below about the different types of reactions.
Type of Reaction
General Equation
Explanation
A + B  AB
Decomposition
A lone element replaces a less reactive
element in a compound
Double Replacement
CxHyOz + O2  CO2 + H2O
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PERIODIC TRENDS
21.Color code the table of elements below to show metals (blue), nonmetals (green), and
metalloids (red).
22.Which elements are diatomic?
23.Summarize the properties of metals, nonmetals, and metalloids.
Conductivity
Malleability
Appearance
Metal
Nonmetal
Metalloid
24.Give examples of elements in the same…
a. Family:
b. Series:
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25.Complete the table about family names on the periodic table.
Family Name Column
26.Halogens have very high ionization energy. Explain why.
Alkali Metals
18
Halogens
2
27.Explain how and why each of the periodic trends change as you move across a series or
down a group.
Trend
Across a Series
Down a Group
Electronegativity
Atomic
Size/
Radius
First
ionization
energy
Shielding
Effect
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SUBATOMIC PARTICLES
28.Complete the table about subatomic particles.
Particle
Charge
Location
Proton
Mass (heavy or light)
Neutron
Electron
29.Which subatomic particle is responsible for the chemical properties of an atom?
30.Complete the following table.
Symbol
Atomic #
Protons
23 +1
A
Na
11
B
20
C
20
D
11
Neutrons
Electrons
21
20
20
12
Mass #
40
11
a. What is an isotope? Circle the isotopes in the table above.
b. Which has more electrons Fe0, Fe+2, Fe+3, or Fe+5?
31.Complete the picture showing the results of Rutherford’s experiment, then write a brief
explanation of what is happening.
32.Describe what happens when an electron absorbs and reemits energy.
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EXPERIMENTAL METHODS
33.Students wanted to determine how the amount of sodium affected the amount of
energy given off during the reaction of sodium with water. They measured out 1 gram, 2
grams, 3grams, and 4 grams of sodium metal, and added each to 500 mL of water. The
amount of energy given off was then recorded into the table below.
The Effect of Mass of Sodium on the Amount of Energy Released
Amount of water (mL)
Mass of sodium (g)
Energy released (kilojoules)
500
1
12.6
500
2
25.2
500
3
38.1
500
4
48.9
a. What is the independent variable?
b. What is the dependent variable?
c. What is a constant in the experiment above?
d. What is a possible question the students were trying to answer during this
experiment?
e. What did the students use to measure out the sodium?
f. What did the students use to measure out the water?
g. Which reactant contained only one type of atom?
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INTERMOLECULAR FORCES
34.Consider the two molecules below.
a. Identify which IMFs are present in each molecule.
b. The boiling point of H2O is 100°C, while the boiling point of H2S is -60°C. Use IMFs
to explain the difference in boiling points for these otherwise similar molecules.
35.Which molecule is more likely to have a strong odor? Explain.
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MOLE CALCULATIONS
36.Explain what Avogadro’s number is – what do we use it for?
37. Setup and solve the following mole conversions.
a. How many moles are in a 35 gram sample of sodium chloride?
b. How many molecules are present in 15 L of carbon dioxide?
c. How many grams are in 2 moles of sodium atoms?
d. How many grams are present in 1.204x1024 atoms of iron?
38.Explain why a mole of silver and a mole of gold have the same number of atoms, but
different molar masses.
39.Find the percent by mass of oxygen in each of the following.
a. KMnO4
b. H2O
c. CaO