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2014-2015 HONORS Chemistry Midterm Review
This review sheet is a list of topics and sample practice problems only. The practice problems
are good representation of what to expect on the midterm, but it is not enough to just study from
the review. You need to look over your notes, old review sheets, tests and quizzes, homework,
etc. Ask questions!!!! You may check your answers online and I am available Tuesday,
Wednesday, and Fridays for extra help.
Chapter 1 & 2: Intro to Chemistry
Key Topics:
 What is chemistry
 Uncertainty in Measurement –sig figs
 Physical and chemical properties
 Physical and chemical changes
1. Determine the number of significant figures in the following values:
a. 6.70
3
c. 15,300
3
b. 0.03260
4
d. 4.68
3
2. Perform the following calculations and express your answer with the correct number
of significant figures:
a. 34.0 x 45.62 =
1550
b. 45 – 95.24 =
-50.
Chapter 3: Atomic Structure
Key Topics:
 Models of the atom (Modern atomic theory)
 Isotopic Notation, Subatomic particles
 Atomic Orbitals – s, p, d shapes
 Electron configurations
 Valence electrons
 Periodic Law
3. Describe the basic structure of the atom in the modern atomic theory
(be able to label protons, neutrons, electrons, and the nucleus) (Ch. 3):
Protons, neutrons – in nucleus (densely packed)
Electrons – surrounding nucleus in orbitals/clouds
Protons: +
Electrons: Neutrons: neutral
4.
14
6
C protons = 6
neutrons = 8
electrons = 6
5. Sketch s and p orbitals (Ch 3):
Electron clouds where there is a probability of finding electrons
6. Write the electron configuration for Bromine.
1s22s22p63s33p64s23d104p5
7. What element has the following electron configuration:
1s22s22p63s33p64s23d5 Manganese
Chapter 4: The Periodic Table
Key Topics:
 Organization of the Periodic Table (Periodic Law)
 Periodic Trends: Electronegativity
 Recognize properties of main groups
8. State the periodic law (Ch 4):
Elements are grouped on periodic table by their physical and chemical
properties (atomic number increases). “The physical and chemical
properties of the elements are periodic functions of their atomic
numbers” (pg 116).
9. Label the following areas on your periodic table (some may overlap) (Ch 4):
Chapter 5: Ionic Compounds
Key Topics:



Octet Rule
Naming and writing formulas
Properties of ionic versus covalent compounds
10. Compare and contrast ionic and covalent bonds (Ch 5 and 6, essay):
Ionic
Both
Covalent
Metal & nonmetal
Giving/taking electrons
(transferring)
High MP and BP
Conducts electricity
when molten or
dissolved in water
Both form stable octets Nonmetal & nonmetal
(8 valence electrons)
Sharing of electrons
Low MP and BP
Both do not conduct
Poor conductors of
electricity as solids
electricity
11. Name the following ionic formulas (Ch 5):
a. NH4Cl
Ammonium chloride
b. CuO
Copper(II) oxide
c. NaF
Sodium fluoride
d. Mg(NO3)2
Magnesium nitrate
12. Write formulas for the following ionic compounds (Ch 5):
a. Magnesium Hydroxide
Mg(OH)2
b. Copper(II) Chloride
CuCl2
c. Calcium Hydroxide
Ca(OH)2
d. Sodium Phosphate
Na3PO4
Chapter 6: Covalent Compounds
Topics:
 Naming and writing formulas
 Properties
 Lewis Dot structures
 Polar vs. Non-polar covalent bonds
 VSEPR
Be able to…
 Sketch lewis structures and predict molecular geometries (VSEPR)
11. Name the following covalent compounds (Ch 6):
a.
b.
c.
d.
CO2
SiF4
SnO4
CCl4
Carbon dioxide
Silicon tetrafluoride
Tin tetraoxide
Carbon tetrachloride
12. Write formulas for the following covalent compounds (Ch 6):
a.
b.
c.
d.
dinitrogen pentoxide
phosphorus trichloride
carbon monoxide
selenium hexachloride
N 2O 5
PCl3
CO
SeCl6
13. Write the dipole moment and bond character of each (Ch 6):
a. C-H
b. C-S
c. Na-Cl
d. Si-O
e. Cl-N
2.6-22.2=.4
2.6-2.6=0
0.9-3.2=2.3
1.9-3.4=1.5
3.2-3.0=.2
nonpolar covalent
nonpolar covalent
ionic
polar covalent
nonpolar covalent
14. Draw Lewis Structures (Ch 6):
CH3Cl
OF2
Check answers during class.
SO3
15.
Identify the shape and bond angle of molecular compounds (Ch 6):
Lewis Structure
Shape
Bond angles
NH3
Trigonal pyramidal
<109.5
SO2
Linear
180
CCl4
Tetrahedral
109.5
Chapter 7: Organic Chemistry
Topics:
 Organic bonding
 Hydrocarbons
 Alkanes, alkenes, alkynes
 Naming and drawing formulas
 Functional groups
 Practical applications
16. Define hydrocarbon: compounds containing carbon and hydrogen atoms
17. Compare/Contrast Alkanes, Alkenes, Alkynes:
Type of Bonds
Alkane
Single
Alkene
Double
Alkyne
Triple
Name
-ane
-ene
-yne
18. List and describe 3 uses of organic compounds (Ch 7, organic presentations)
Soap, perfumes, synthetic fabrics, polymers, medicine, PLASTIC
petroleum (energy)
19. Drawing and naming organic structures and naming (Ch 7):
Recognize how to draw/name structures for alkanes, alkenes, and alcohols.
3-octene
Pentane
1-butanol
2-pentene
Chapter 8: The Mole
Topics:
 Mole
 Avogadro’s number
 Percent composition
 Empirical formulas
 Molecular formulas
Be able to…
 Calculate molar mass
 Convert between grams and moles
 Convert between number of particles and moles
 Perform multi-step conversions
 Calculate percent composition
 Determine empirical formula
 Determine molecular formula
20. Determine the molar mass of the following compounds (Ch 8):
Al2(SO4)3 2(26.98) + 3(32.06) + 12(16.00) = 342.14
KBr
39.10 + 79.90 = 119.00g/mol
Li2O
2(6.94) + 16.00 = 29.88g/mol
21. Find the percent composition of each element (Ch 8):
%Mg in MgSO4?
Total mass MgSO4: 24.31 + 32.06 + 4(16.00) = 120.37 g/mol
Mg: 24.31/120.37 x 100% = 20.20% Mg
S: 32.06/120.37 x 100% = 26.63% S
O: 64.00/120.37 x 100% = 53.17% O
%H in C2H5O?
Total mass C2H5O: 2(12.01) + 5(1.01) + 16.00 = 45.07 g/mol
C: 24.02/45.07x 100% = 53.29% C
H: 5.05/45.07x 100% = 1.11% H
O: 64.00/45.07x 100% = 35.50% O
22. Mole conversions (Ch 8):
# of moles in 2.5g of Aluminum Oxide?
2.5 g x 1 mol = .025mol
101.96g
# of moles in 15g of Neon?
15 g x 1 mol = .74mol
20.18g
# of atoms in 0.5mol of Gold?
.5 mol x 6.02 x 1023 atoms = 3 x 1023 atoms
1mol
# of atoms in 1.5 grams of Zinc (II) Chloride?
1.5g x 1 mol x 6.02 x 1023 atoms = 6.6 x 1022 atoms
136.29g
1mol
Chapter 9: Chemical Reactions and Equations
Key Topics:
 Chemical reaction
 Reactant
 Product
 Chemical equation
 Coefficient
 Reaction Types
Be able to…
 Write and balance equations
 Identify types of reactions
23. Balancing equations (Ch 9):
4 Fe + 3 O2  2 Fe2O3
synthesis
3 Fe + 4 H2O  1 Fe3O4 + 4 H2
single replacement
3 Mg + 1 N2  1 Mg3N2
synthesis