Name ________________________
Chemistry Midterm Review
Chapter # 2: Matter
1. Draw the Matter Tree
2. Explain/diagram the arrangement of particles in a solid, liquid & a gas.
3. Is freezing Mercury Hg , a physical change or a chemical change? Is it reversible or
irreversible?
4. Explain why samples of gold and copper can have the same extensive properties but
not the same intensive properties?
5. Classify each of the following as homogeneous or heterogeneous:
a. food coloring _____________________
b. ice cubes floating in water ____________________
c. mouthwash ______________________
d. mashed, unpeeled potatoes _____________________
6. How is a pure substance different than a solution?
7. How is a compound different than an element?
8. Classify each of these samples of matter as a element, compound or mixture:
a. sucrose, table sugar ____________________
b. cough syrup ______________________
c. water ____________________
d. nitrogen _____________________
e. Air _____________________
9. List the elements that make up the pain reliever, acetaminophen, C8H9O2N
10. Explain the Law of Conservation of mass? What is a closed system?
11. Why are solids not as easy to compress as a gas?
12. How many grams total of magnesium and oxygen must combine to form 20g of
magnesium oxide?
13. Classify each of the following as a chemical or physical change:
a. A copper wire is bent __________________
b. Charcoal burns in a grill _________________
c. Bread dough rises when yeast is added __________________
d. Sugar dissolves in water ______________________
e. Leaves changing color in the fall ________________________
14. How does the Kinetic Energy change of the particles, as a substance changes from a
gas to a solid?
15. List 4 indicators of a chemical change that has occurred in a chemical reaction.
16. In the chromatography lab was the pen ink homogeneous or heterogeneous? Was the
separation a chemical or physical change?
Chapter # 3: Measurement
1. Why is a number put into scientific notation?
2. Put the following numbers into scientific notation:
a. 123 _____________________
b. 10,056 _____________________
c. .00708 _____________________
d. .1594 ____________________
3. Change the following into an ordinary number:
a. 4.5 X 103 _____________________
b. 3.24 X 10-2 ___________________
c. 24 X 10 2 ____________________
4. What is the % Error formula?
5. Aluminum has a density of 2.70 g / cm3 .
What is the density of a cube that measures 2.5 cm X 3.0 cm X 1.6 cm and has a mass of
36 g ? Is this cube gold? What is the % error?
6. List and describe to find volume in the lab. What are the units associated to each
method.
7. How many centimeters are in a meter? How many meters are in a kilometer? How
many kilometers are in one meter (NO, this is not a typo!)
8. Rearrange the Density equation to find:
a. D =
b. V =
c. M =
Chapter # 4: Atomic Structure
1. Draw a timeline of Atomic Structure beginning with Democritus, including Aristotle,
Dalton, Thomson, Rutherford & Bohr.
2. Describe JJ Thomson’s Experiment. What part of Atomic structure did he
contribute?
3. Describe Rutherford’s experiment. What part of atomic structure did he contribute?
4. Please fill in the following table:
ELEMENT
SYMBOL
ATOMIC
#
MASS
#
Protons
Neutrons Electrons
Ne - 22
Mercury
12
56
Br-1
36
10
Atom, Ion
or Isotope
5. Define Isotope.
6. What is the mass number of Gold? What is its Atomic mass?
7. Do the following paired examples represent isotopes or ions ? List the proton, electron
and neutron count for each.
a.
b.
6
3
7
Li
40
20
3
Ca +2
Li
40
20
Ca
8. Name 2 ways that isotopes of an element differ?
9. The 4 isotopes of lead are:
Isotope
Isotope
Isotope
Isotope
#1:
#2:
#3:
#4:
82p , 122 n
82p , 124 n
82p , 125 n
82 p, 126 n
1.4 % Abundance
24.1 % Abundance
22.1 % Abundance
52.4 % Abundance
Calculate the Atomic Mass of Lead. Remember protons and neutrons are found in the
nucleus. The nucleus accounts for the mass of the atom.
Chapter #5: Electrons
1. What did Bohr propose in his model of the Atom?
2. How do electrons in an atom move from one energy level to another?
3. What is a Quantum of Energy? What is a photon?
4. Electrons are stabilized in their beginning positions called their ___________ state.
Energy is absorbed by the electron through heat, _____________, _____________ &
__________________. This excites the electron to a higher energy level, which is
unstable. The electron will fall and in doing so gives off the captured energy in the form
of ______________________.
5. What is a principle energy level? What does n = _____ ?
6. What are the 4 types of sub orbitals? How many “rooms” does each have? How many
electrons can each of the 4 suborbitals hold? (make a chart)
7. Which of these orbital designations is considered invalid? Circle all that apply.
4s
3f
2d
3d
8. Please Explain the Aufbau Rule in writing electron configurations. Draw the Aufbau
diagram.
9. What is an orbital notation diagram? Draw a ON for the element Calcium?
10. Explain and give an example of Hund’s Rule and the Pauli Exclusion Principle.
11. Please write the electron configurations for the following elements:
a. selenium
b. nickel
c. Ga
d. Tin
12. What element is represented by:
a. . . . 2p3
b. 1s2 2s2 2p5
c.
. . . 3d7
13. Arrange the following sub orbitals in order of increasing energy: 3d, 2s, 4s, 3p
14. Draw a diagram of an Atom with the following configuration: 1s2 2s2 2p6 3s2 3p6 4s1
Chapter # 6: The Periodic Table
1. How is Mendeleev’s Periodic table arranged? How is Mosely’s?
2. Based on their locations on the periodic table, would you expect carbon and silicon to
have similar properties? Explain your answer.
3. Which of the following are symbols of the representative elements? Na, Mg, Fe, Ni, Cl
4. Which noble gas does not have 8 electrons in its outermost valence shell? _________
5. Write the electron configuration of these elements:
a. The noble gas in period 3 ____________________________________________
b. The metalloid in period 3 ____________________________________________
c. The alkali earth metal in period 2 ______________________________________
6. Please list the properties of metals, non-metals and metalloids.
7. Write the symbol of the element or elements that fit each description:
a. a non metal in group 4A __________________________
b. the inner transition element with the lowest atomic # _____________________
c. all of the non metals for which the atomic # is a multiple of 5 __________________
d. a metal in group 5A ______________________