AP Chemistry Homework
Due Date: _________
Chapter 7 – Atomic Structure and Periodicity
Remember from Chemistry last year: families of the periodic table, quantum theory, Bohr
model, photoelectric effect, Electron Configurations, describing the location of the electron
Assignment:

Read the chapter

Complete problems 1, 12, 33, 39, 41, 45, 49, 53, 57, 63, 69, 73, 79, 81, 85, 91, 95, 105, 107,
117, 127, 137
Chapter 8 – Bonding: General Concepts
Remember from Chemistry last year: ionic and covalent bonds, electronegativity, drawing Lewis
dot structures, VSEPR Theory, molecular geometry
Assignment:

Read the chapter

Complete problems 27, 29, 41, 47, 53, 59, 63, 65, 67, 71, 72, 83, 84, 89, 91, 98, 109, 115,
119, 125, 157
Chapter 9 – Covalent Bonding: Orbitals
New: localized electron model, molecular orbital model, hybrid orbitals, sigma (ϭ) bonds, pi (π)
bonds, bond energy, bond order, paramagnetism, diamagnetism, resonance
Assignment:

Read the chapter

Complete problems 8, 19, 23, 29, 31, 38, 43, 45, 46, 51, 61, 63, 68
Chapters 7, 8, 9
Review questions:
(Answers can be found on the Student website accessible from www.cengagebrain.com)
Chapter 7: pp. 340-341
© Cengage learning 2014
7.1 Four types of Electromagnetic Radiation (EMR) are ultraviolet, microwaves, gamma rays and
visible. All of those types of EMR can be characterized by wavelength, frequency, photon energy
and speed of travel. Define these terms and rank the four types of electromagnetic radiation in
order of increasing wavelength, frequency, photon energy and speed.
Date:_______
Define:
Wavelength:
Frequency:
Photon energy:
Speed of travel:
Rank:
increasing wavelength:
increasing frequency:
increasing photon energy
speed:
7.2 Characterize the Bohr model of the atom. In the Bohr model, what do we mean when we say
that something is quantized? How does the Bohr model of the hydrogen atom explain the hydrogen
emission spectrum? Why is the Bohr model fundamentally incorrect?
Date:_______
7.3 What experimental evidence supports the quantum theory of light? Explain the wave-particle
duality of all matter. For what size particles must one consider both the wave and particle
properties?
Date:_______
7.4 List the most important ideas of the quantum mechanical model of the atom. Include in your
discussion the terms or names wave function, orbital, Heisenberg uncertainty principle, de Broglie,
Schrödinger, and probability distribution.
Date:_______
7.5 What are quantum numbers? What information do we get from quantum numbers, n,ℓ, and m ℓ?
We define a spin quantum number (ms), but do we know that an electron literally spins?
Date:_______
7.6 How do 2p orbitals differ from one another? How do 2p and 3p orbitals differ from one
another? What is a nodal surface in an atomic orbital? What is wrong with 1p, 1d, 2d, 1f, 2f and 3f
orbitals? Explain what we mean when we say that a 4s electron is more penetrating than a 3d
electron.
Date:_______
7.7 Four block of elements in a periodic table refer to various atomic orbital being filled. What are
the four blocks and the corresponding orbitals? How do you get the energy ordering of the atomic
orbitals from the periodic table? What is the aufbau principle? Hund’s rule? The Pauli exclusion
principle? There are two common exceptions to the ground state electron configuration for
elements 1-36 as predicted by the periodic table. What are they?
Date:_______
aufbau principle:
Hund’s rule:
Pauli exclusion principle:
7.8 What is the difference between core electrons and valence electrons? Why do we emphasize
the valence electrons in an atom when discussing the atomic properties? What is the relationship
between valence electrons and elements in the same group of the periodic table?
7.9 Using the element phosphorus as an example, write the equation for a process in which the
energy change will correspond to the ionization energy and to the electron affinity.
Explain why the first ionization energy tends to increase as one proceeds from left to right
across a period. Why is the first ionization energy of aluminum lower than that of magnesium and
the first ionization energy of sulfur lower than that of phosphorus?
Why do the successive ionization energies of an atom always increase? Not the successive
ionization energies for silicon given in Table 7.5. Would you expect to see any large jumps between
successive ionization energies of silicon as you removed all the electrons one by one, beyond those
shown in the table?
Date:_____________