Honors Chemistry Midterm Exam Review
Topics: UNIT 1 – UNIT 5
Formula writing
Nomenclature
Molar mass and gram/mole conversions
Gram/mole/liter/molecule conversions
Balancing equations
Reaction types
Stoichiometry
Radioactivity
Nuclear chemistry equations
Scientists for atomic theory
Periodic Table (everything) and Trends
Quantum numbers, orbitals, electron configurations
Solutions and Solubility
Concentraion and Molarity calculations
Colligative prop calculations
Example Questions:
1.
What is the symbol for the sulfate ion?
2.
Write the formula for magnesium acetate.
3.
What is the name of Na2CO3?
4.
What is the formula for nitric acid?
5.
Name C2H6
6.
What is the formula for iron(III) chloride?
7.
Calculate the molar mass of iron(III) chloride.
8.
How many grams of hydrogen gas at STP are in 3.50L?
9.
Know how to balance equations.
10.
How many moles are in 25.0g sodium chloride?
11.
How many grams are in 0.959 moles of water?
12.
List the 5 different types of reactions and write an example of each.
13.
Define limiting reactant and % yield.
14.
Sodium reacts with water and forms sodium hydroxide and hydrogen
gas. If 24.8g of sodium is added, then how many molecules of
hydrogen are formed?
15.
Define half-life.
16.
How many protons are in C-14?
17.
How many neutrons are in U-235?
18.
Define isotope.
19.
Define radioactivity.
20.
List and define the 3 types of radioactivity.
21.
Who discovered the uncertainty principle?
22.
Who said the atom was like a solar system and the electrons transition
between energy levels?
23.
Who discovered the nucleus using a Gold Foil experiment?
24.
Define fission and fusion.
25.
What family name applies to iodine and other Group 17 non-metals?
26.
What family name applies to magnesium and other Group 2 metals?
27.
Define ionization energy and electronegativity.
28.
Define and compare/contrast energy levels, sublevels and orbitals:
29.
How many p-orbitals are there in a p-sublevel?
30.
What types of orbitals are found in the 4th energy level?
31.
Know how to write and analyze electron configurations.
32.
How many valence electrons do the alkali metals have?
33.
Define wavelength and frequency.
34.
Who created the first Periodic Table of the Elements?
35.
What happens to the size of the atom when it becomes a positive ion?
36.
Define allotrope.
37.
Know the property differences between metals and nonmetals.
38.
Calculate the molarity of 5.00g of potassium nitrate in a 250.0 mL flask.
39.
Compare and contrast the properties of solids and liquids.
40.
Define colligative property.
41.
List the various types of intermolecular forces and compare them in
terms of definitions and relative strengths:
42.
What is the molality of a non-electrolyte solution of C2H4(OH)2 in water
if the new freezing point is -5.50 ºC? Kf is -1.86 ºC/m.
43.
How do you prepare a 0.500M solution of sodium chloride in a 100.0
mL flask?
44.
Know the difference between a beaker, grad. cylinder, volumetric flask
and Erlenmeyer flask.
There will be two, 10 point open-ended questions for you to answer on the
midterm exam. The following are examples and practice to prepare for the
midterm questions. The essay topics are:
1.
Reactions and Stoichiometry
2.
Periodic Table Trends
3.
Solutions and Solubility
4.
Atomic Theory
1. Reactions and Stoichiometry
Ex. “A lab scientist combines 55.0 grams of magnesium metal with an
excess quantity of nitrogen gas”
Write the balanced chemical equation:
What type of chemical reaction is this?
Show stoichiometry work to calculate the theoretical mass (grams)
of product that will form for this reaction:
Show work to calculate percent yield if this lab scientist
experimentally collects 61.5 grams of product:
2. Periodic Table Trends
Ex. “The location of Barium on the periodic table reminds us that atoms of
Barium have very distinct properties compared to atoms of other elements”
Do atoms of Barium have larger or smaller atomic radii than most
other metals? Explain the scientific factors behind your choice:
Do atoms of Barium have large or small electronegativity values
compared to atoms of other elements? Explain the scientific factors
behind your choice:
Define ionization energy and explain why the 1st and 2nd ionization
energy values for Barium atoms would be small in comparison to the
3rd ionization energy value for Barium:
3. Solutions and Solubility
Ex. “Describe, on a molecular level, the dissolving process of sodium
chloride in a water solvent. Discuss the difference between unsaturated
and saturated solutions and describe the saturation point and define
solubility.”
4. Atomic Theory
Ex. “Our view and understanding of the atom has changed drastically
throughout recent history. Many scientists have contributed to the
understanding that we have about the atom.” Describe the role each of the
following scientist hade in the development of atomic theory: Thomson,
Rutherford and Bohr. Include a diagram to show the model of the atom
that was commonly accepted at the time each scientist did their work.