A.P. Chemistry – Chapter 7 and 8 – Atomic Structure and Electron Configurations– Fall 2012
When explaining trends it is not sufficient to state a rule. You do need to consider the structure of the atoms and their electrons to explain the behaviors, the properties of these atoms. (Form determines behavior)
Describe the properties of electromagnetic radiation


Use the terms
Use c = λ/ν, speed of light.

Recognize the relative wavelength (or frequency) of the various types of electromagnetic radiation
(Figure 7.3) wavelength, frequency, amplitude, and node . Section 7.1 the relationship between wavelength and frequency of electromagnetic radiation and the

Understand that the energy of a photon, a massless particle of radiation, is proportional to its frequency.
(Planck’s equation, Eqn 7.2). This is an extension of Planck’s idea that energy at the atomic level is quantized. Section 7.2
Understand the origin of light from excited atoms and its relationship to atomic structure

Describe the Bohr model of the atom, its ability to account for the emission line spectra of excited hydrogen atoms, and the limitations of the model. (Section 7.3)

Understand that, in the Bohr model of the H atom, the electron can occupy only certain energy levels, each with an energy proportional to 1/ n 2 ( E=-Rhc/n 2 ), where n is the principal quantum number. If an electron moves from one energy state to another, the amount of energy absorbed or emitted in the process is equal to the difference in energy between the two states. Eqns 7.4 and 7.5, Section 7.3
Homework
(possibly done over the summer)
Ch. 7
3
1
5,12,14,54,56,61,62,
76
Ch 7
Problems
18,22,58
Got
It
Describe the experimental evidence for wave-particle duality
Understand that in the modern view of the atom, electrons are described by the physics of waves. The wavelength of an electron or any subatomic particle is given by de Broglie’s equation (eqn 7.6) Section 7.4
Describe the basic ideas of quantum mechanics

Recognize the significance of quantum mechanics in describing the modern view of atomic structure.
Section 7.5

Understand that an orbital for an electron in an atom corresponds to the allowed energy of that electron.

Understand that the position of the electron is not known with certainty; only the probability of the electron being at a given point of space can be calculated. This is the interpretation of the quantum mechanical model and embodies the postulated called the Heisenberg uncertainty principle.
Ch 7
24

Define the three quantum numbers ( n,l,and m l
) and their relationship to atomic structure.

Describe the allowed energy states of the electron in an atom using three quantum numbers, ( n,l,and m l
). Section 7.5

Describe the shapes of the orbitals. Section 7.6
Understand the role magnetism plays in determining and revealing atomic structure

Classify substances as paramagnetic (attracted to a magnetic field; characterized by unpaired electron spins) or diamagnetic (repelled by a magnetic field). Section 8.1

Recognize that each electron in an atom has a different set of four quantum numbers. Section 8.2

Understand that the Pauli exclusion principle leads to the conclusion that no atomic orbital can be assigned more than two electrons and that the two electrons in an orbital must have opposite spins
(different values of m s
) Section 8.2
Understand effective nuclear charge and its role in determining atomic properties.
Understand effective nuclear charge, Z, and its ability to explain why different subshells in the same shell have different energies. Also understand the role of Z in determining the properties of atoms.
Section 8.3 and 8.6
Write the electron configuration for elements and monatomic ions

Using the periodic table as a guide, depict electron configurations of the elements and monatomic ions using orbital box or the spdf notation. Section 8.3 and 8.4

Recognize that electrons are assigned to the subshells of an atom in order of increasing subshell energy.
In the H atom the subshell energies increase with increasing n , but in a many-electron atom, the energies depend on both n and l.
 When assigning electrons to atomic orbitals, apply the Pauli exclusion principle and Hund’s rule.
Sections 8.3 and 8.4
Understand the fundamental physical properties of the elements and their periodic trends.
1.
Predict how properties of atoms – size, ionization energy (IE), and electron affinity (EA) – change on moving down a group or across aperiod of the periodic table. The general trends for these properties are as follows:

Atomic size decreases across a period and increases down a group.

IE increases across a period and decreases down a group.

The affinity for an electron generally increases across a period (the value of EA becomes more negative) and decreases down a group (Sec. 8.6)
2.
Recognize the role that ionization energy and electron affinity play in the chemistry of the elements (Sec.
8.7)
Ch 7
28,30,36,38,40,
74
44,51,65
Ch. 8
18, 19
Ch. 8
2.3.6.12.14.21,
37.38.39.48
Ch 8
26,28,30,33,45,4
6,50,53
62,67

Date What We Will Do In Class
9/24 Test on Gravimetric Analysis Labs. Receive Bohr Energy levels handout from Ebbing. Receive Atomic Spectroscopy and Energy
Levels Activity #18. Receive Why Every English Classroom Should
Have a Periodic Table. Receive Focus Questions for this unit.
9/25 Do Atomic Spectroscopy and Energy Levels Activity #18. WC review of answers. Receive Relationships Among Values HO.
9/27 Review focus Qtns and receive Unit Take Home Test. This test is due Oct 3rd. Receive Patterns in IE handout
9/28 Do Periodic Trends in Atomic Structure
10/1 Complete the Periodic Trends in Atomic Structure and review responses.
10/2 Work on take home test. If you are caught up on this do homework questions listed on this activity sheet that you might not have done this summer.
10/3 Hand in Take Home test. WC board work on Ch 7 homework qtns.
Receive AP CoTest Bank qtns.
10/4 WC board work on Ch 8 homework qtns
Do Focus Questions.
Assignments
Complete Activity #18. Do the Focus Questions. You can extend this homework through the 27 th
.
Read Patterns in IE Hand out. Work on Take Home Test.
Remember that a rule is not an explanation.
Same as 9/27
Same as 9/27
Same as 9/27. Work on homework qtns listed on this activity sheet.
Work on homework qtns listed on this activity sheet and AP Co Test
Bank qtns
Prep for unit test
10/5 AP Company Test Bank qtns.
10/9 Unit Test
Prep for unit test