Honors Chemistry 1
Fall, 2014
Mr. Cunnings
Chapter 3 Test Review Sheet and Practice Problems
Problems & Questions:
1) Write the electron configuration AND create an orbital diagram for each of the following atoms. I
expect you to know all of the symbols studied from chapter 1, although I will give you the symbols for
elements that we haven’t already studied on your test.
a. Lithium
b. Oxygen
c. Sodium
d. Magnesium
e. Silicon
Honors Chemistry 1
f. Neon
g. Zinc
h. Nickel
i. Vanadium (V)
j. Germanium (Ge)
k. Selenium (Se)
Fall, 2014
Mr. Cunnings
Honors Chemistry 1
l. Barium (Ba)
m. Iridium (Ir)
n. Tellurium (Te)
o. Mercury
p. Uranium
Fall, 2014
Mr. Cunnings
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
2) Perform the following conversions, given either mass, moles, or particles. You must include the correct
number of significant figures and the correct unit in your final answer!
a. How many moles of iron are present in 79.0 grams of iron?
b. If you have a sample of 3.20 moles of Neon atoms, what is the mass (in grams) of the neon
sample?
c. You have a sample of copper wire that has a mass of 128.71 grams. How many copper atoms are
in this sample?
d. 1.834 x 1022 atoms of oxygen have a mass of _______ grams
e. If you have a sample of 5.43 x 1025 atoms of silver, how many mols of silver do you have?
f. What is the mass of silver given in part e above?
g. You obtain a chromium sample that contains 0.799 mol of chromium atoms. How many
chromium atoms are in the sample?
h. What is the mass of the chromium sample described in part g above?
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
i. If you have a 3.0 kg bag of sodium chloride for icing your driveway during the winter, how
many molecules of NaCl are in the bag? Be sure you start by converting the given mass into
grams!!
j. Glucose is the fuel our brains use, and it has a molecular formula of C6H12O6. You go to lunch
and consume 100.0 grams of glucose. How many mols of glucose did you consume?
k. How many glucose atoms are present in the amount of glucose described in part J?
l. How many moles of nitrogen dioxide gas (NO2) are present in a sample of nitrogen dioxide that
has a mass of 0.090 grams?
m. A sample of arsenic has a mass of 44.91 grams. How many atoms of arsenic are present in the
sample?
n. How many atoms are in 0.340 mol of sodium?
o. How many molecules of carbon monoxide (CO) are present in 2.09 mol of CO?
p. How many molecules of magnesium chloride (MgCl2) are present in a sample of pure
magnesium chloride that has a mass of 132.0 grams?
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
3) Create a picture for each of the orbital shapes below, and name the shape:
a. s orbital
b. p orbital
c. d orbital (should contain two different types of shape)
4) Draw the electron cloud for the neon atom using the shapes from problem 3. I know this is hard to do
on paper, but try your best to show the p-orbitals in three different dimensions.
5) List all of the key features of Dalton’s atomic theory.
6) Describe the cathode ray experiment described in section 3.1. Create a diagram of this experiment. This
experiment led to the discovery of which subatomic particle?
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
7) What did the gold foil experiment tell us about the structure and composition of the atom? Who
famously conducted this experiment?
8) The VAST MAJORITY of the alpha particles shot at the gold foil did what?
a. Bounced back at the source
b. Went straight through the foil
c. Were absorbed by the foil
d. Melted the foil
9) Describe Rutherford’s atomic model, and create a diagram of his atomic model.
10) Describe all of the subatomic particles below in terms of their electric charge and location within an
atom:
a. Proton
b. Electron
c. Neutron
11) Define an isotope and give examples of THREE DIFFERENT CARBON ISOTOPES
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
12) Solve the following isotope problems:
a. An oxygen atom has an atomic mass of 18 amu. How many neutrons does the atom contain?
b. How many neutrons does Iodine-130 contain?
c. A sodium isotope contains 11 protons, 12 neutrons, and 11 electrons. What is the mass number
of this sodium atom?
d. List the protons, neutrons, and electrons in a silver-109 atom. An atom has a mass number of 41,
and it contains 20 protons. Write the name of the isotope in both notations shown: (e.g., Carbon12) AND (e.g., 126𝐶 )
e. Considering the atom 235
92𝑈
i. How many protons does the atom contain?
ii. How many neutrons does the atom contain?
iii. How many electrons does a Uranium-235 atom contain?
f. Considering the atom Lead-208
i. How many protons does the atom contain?
ii. How many neutrons does the atom contain?
iii. How many electrons does a lead-208 atom contain?
g. A potassium atom has a mass number of 40.
i. How many neutrons does this potassium isotope contain?
ii. How many protons does this potassium isotope contain?
iii. How many electrons does this potassium isotope contain?
Honors Chemistry 1
Fall, 2014
Mr. Cunnings
13) Describe Bohr’s model of the atom. Draw a picture describing this model. List the key features of
Bohr’s atomic model.
14) What is the difference between “ground state” and “excited state” for an electron? How does an
electron go from ground state to excited state within an atom?
15) The bigger the energy level jump within an atom for an electron (e.g., from 1s all the way to 5s), the
(longer / shorter) the wavelength of energy that was (absorbed / released) by the atom, and the (higher /
lower) the frequency of the electromagnetic energy (absorbed / released) by the atom.
16) For an electron to drop from excited state back to ground state, it must (absorb / release) energy.
17) Most of the volume of an atom is occupied by which of the following?
a. The nucleus
b. The protons
c. The electron cloud
18) Describe briefly each of the quantum numbers below. What information do they provide us about the
electrons?
a. The principal quantum number
b. The angular momentum quantum number
c. The magnetic quantum number
d. The spin quantum number
Honors Chemistry 1
Fall, 2014
19) How many orbitals does each sublevel below contain?
a. s
b. p
c. d
d. f
20) How many electrons (at most) can fit into each sublevel?
21) Define the following, and know the Chem2 poster analogy for each:
a. Hund’s Rule
b. Aufbau Principal
c. Pauli Exclusion Principal
22) Where is an electrons location within an electron cloud?
23) What is the abbreviation for the atomic mass unit?
24) What is the relative molar mass for each element or compound listed below?
a. Fe
b. O2
c. Fe2O3
d. NaCl
e. H2SO4
Mr. Cunnings