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CP Chemistry Review Unit 1: Atomic Structure, Periodic Properties and Nuclear Chemistry
Chapter 4 Section 1-2
Explain the significance each person had on our understanding of the atom:
1. Democritus/Aristotle
2. Lavoisier
3. Dalton
4. Proust
5. Thomson
6. Millikan
7. Rutherford
8. Bohr
Chapter 4 Section 3
Select the choice that best answers each question or completes each statement.
1. Which of these descriptions in incorrect?
a. proton: positive charge, in nucleus, mass of 1 amu
b. electron: negative charge, mass of about 0 amu, in nucleus
c. neutron: mass of about 1 amu, no charge
2. Thallium has two isotopes, thallium-203 and thallium-205. Thallium’s atomic number is 81 and its atomic mass is
204.38 amu. Which statement about the thallium isotopes is true?
a. There is more thallium-203 in nature.
b. Atoms of both isotopes have 81 protons.
c. Thallium-205 atoms have fewer neutrons.
d. The most common atom of thallium has a mass of 204.38 amu.
3. T/F Every aluminum-27 atom has 27 protons and 27 electrons, because the mass number of aluminum-27 is 27.
4. T/F Isotopes of an element have different atomic masses, because the nuclei of an element’s isotopes contain different
numbers of protons.
5. T/F An electron is repelled by a negatively charged particle, because an electron has a negative charge.
Identify the # of protons, neutrons, and electrons in the following atoms:
6. 31P
p= ____ n= ____ e= ____
7. 39Ca
p= ____ n= ____ e= ____
8. 128Te
p= ____ n= ____ e= ____
Write the complete symbol for the atoms which have the following # of p, n, & e's:
9. p= 26 n= 30 e= 26
__________
10. p= 23 n= 28 e= 23
__________
11. p= 80 n= 120 e= 80 __________
12. Complete the table, using the periodic table as a guide: (first one is done as an example):
Name
# of protons, neutrons, and
Complete Symbol
electrons
66
Zinc-66
p= 30, n= 36, e=30
30Zn
Magnesium-20
p= 12, n= 14, e= 12
61 Fe
26
Iodine-132
p= 82, n= 110, e= 82
185 W
74
13. Lithium has 2 naturally occurring isotopes: Li-6 with an atomic mass of 6.015 amu, and Li-7 with an atomic mass of
7.016 amu. What is the percent abundance of Li-7?
Chapter 5 Section 1 & 2
1. What causes an atom to emit light?
2. What was wrong with Rutherford’s model of the atom, and how did Bohr account for this in his view of the atom?
3. Why did Bohr’s model not work for all elements?
4. What did Heisenberg propose about the movement of electrons around the nucleus?
5. How did Schroedinger explain where the electron is inside the atom?
6. For each quantum number, list the symbol and give a brief description.
Quantum #
Symbol
Description
Principal
Angular
Momentum
Magnetic
Spin
7. Draw the shapes of the following types of orbitals:
s-orbital
p-orbital
8. Complete the following table to indicate the total number of orbitals in each energy level (n). In the remaining columns,
specify how many of those orbitals are s, p, d, and f.
Level n
Total # of
orbitals
# of
s-orbitals
# of
p-orbitals
# of
d-orbitals
# of
f-orbitals
1
2
3
4
9. Follow the instructions for the following element: Fe
a. Draw the orbital diagram (this is the diagram like the one on page 133).
b. Write out the complete electron configuration.
c. Write out the short hand configuration.
d. Identify the highest energy level and sublevels; how many valence electrons are present?
10. How do exceptional electron configurations differ?
Chapter 5 Section 3
1. What is the classical view of light?
2. What visible light has the highest energy?
3. What visible light has the longest wavelength?
4. What is the relationship of wavelength to frequency?
5. What is the wavelength of light with a frequency of 2.36 x 1014 Hz?
6. What is the frequency of light with a wavelength of 455 nm?
7. What is the quantum view of light?
8. What is a quantum?
9. What is the photoelectric effect?
10. How are energy and frequency related?
11. What is the frequency of light with an energy of 5.45 x 10-26 J?
12. What is the energy of light with a frequency of 2.36 x 1014 Hz?
13. What is the energy of light with a wavelength of 565 nm?
Chapter 6 Section 1
1. Outline the development of the modern periodic table from Newlands to Glenn Seaborg? Include the theorists and
explain what their contributions to the development of the periodic table were.
2. Name the three broad classes of elements. What are some chemical or physical properties of each class?
3. Which of these sets of elements have similar physical and chemical properties? Explain.
a. O, N, C, B
b. Sr, Mg, Ca, Be
c. N, Ne, Ni, Nb
4. Identify each element as a metal, metalloid, or nonmetal.
a. Au
b. Si
c. S
d. Ba
5. Name two elements that have properties similar to those of the element Na. Why are they similar?
Chapter 6 Section 2
1. What information can be included in a periodic table?
2. Into what four classes can elements be sorted based on their electron configurations?
3. Why do the elements potassium and sodium have similar chemical properties? Explain
4. Classify each element as a representative element, transition metal, or noble gas.
a. 1s22s22p63s23p6
b. 1s22s22p63s23p64s23d1
c. 1s22s22p63s23p2
5. Which of the following elements are transition metals: Cu, Sr, Cd, Au, Al, Ge, Co?
6. How many electrons are in the highest occupied energy level of Group 5A elements?
Chapter 6 Section 3
1. How does atomic size, first ionization energy, ionic size, and electronegativity change within a group and across a
period?
2. Which element in each pair has the larger first ionization energy?
a. Na, K
b. Mg, P
3. Explain each of the following comparisons in the terms of nuclear charge and atomic structure.
a. Calcium has a smaller second ionization energy than potassium.
b. Lithium has a larger first ionization energy than cesium.
c. Magnesium has a larger third ionization energy than aluminum.
2. Explain why it takes more energy to remove a 4s electron from zinc than from calcium.
3. Use nuclear charge and shielding to explain why electronegativity increases as first ionization energy increases across
a period.
4. The Mg2+ and Na+ ions each have 10 electrons. Which ion would you expect to have the smaller radius? Explain.
5. Electron affinity is a measure of an atom’s ability to gain electrons. Predict the trend for electron affinity across a
period in terms of nuclear charge and shielding effect.
6. Arrange these elements in order of decreasing atomic size: S, Cl, Al, and Na. Does your arrangement demonstrate a
periodic trend or a group trend?
7. Arrange these elements in order of increasing metallic character: Fr, Hf, Mo, Fe, Zn.
Chapter 25 Section 1-3
1. If a radioisotope undergoes beta emission,
a. the atomic number changes.
b. the number of neutrons remains constant.
c. the isotope loses a proton.
d. the mass number changes.
Determine the missing particle, and label the following as: natural decay, electron capture, induced decay, fission, or
fusion.
2. 24397Bk + 11p ---> 9640Zr + 5022Ti + __________
3. __________+ 0-1e ---> 2614Si
4. 10847Ag + 10n ---> __________+ 10944Ru
5. A francium-224 atom gets hit by a deuteron (21H).
What type of reaction is it? ______________What isotope is produced? _______________
6. A Pa-235 undergoes a series of alpha and/or beta decays to eventually become a Fr-227.
How many alpha decays? ______ beta decays? ______
7. Zn-65 has a half-life of 244 days. What percent will decay in 1year?
8. If a newly cut piece of wood gives a C-14 Geiger tube reading of 150 cpm, and a wooden artifact gives reading of 65
cpm, how old is the artifact?
9. Calculate the nuclear binding energy for Iron-56. Its mass is 55.845 amu.
electron mass = 0.000548579867 atomic mass units
proton mass = 1.00727638 atomic mass units
neutron mass = 1.0086654 atomic mass units
1 amu = 1.660538782 x 10-27 kg
10. Compare and contrast fission and fusion?