Download Objectives for Third Exam

Concept Areas for CHE 170 Third Exam (all fair game on final exam)
Chapter 7: Atomic Structure
Concept Area I: Terminology
• quantum mechanics
• quantum-mechanical
model
• electromagnetic radiation
• waves
• amplitude
• wavelength, λ
• frequency, ν
• Hertz, hz
• electromagnetic spectrum
• gamma rays
• X-rays
• ultraviolet or UV
• visible light
• infrared or IR
• microwaves
• radio waves
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
interference (constructive
or destructive)
diffraction
photoelectric effect
Planck’s constant
Rydberg constant
photon or quantum
quantized
spectra, spectrum
continuous spectra
line spectra
emission spectrum
absorption spectrum
de Broglie’s theory and
equation
Heisenberg uncertainty
principle
Bohr model of the atom
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
ground state
atomic orbitals
s, p, d, f
degenerate orbitals
quantum numbers
principal quantum number,
n
angular momentum
quantum number, ℓ
magnetic quantum number,
mℓ
spin
Pauli exclusion principle
spin quantum number, ms
principal level or shell
sublevel or subshell
probability density cloud
node
Concept Area II: Light
a. You need to understand that light is a form of energy.
b. You should know and be able to apply the terms wavelength, frequency, amplitude, node and
electromagnetic spectrum.
c. You should be able to list different kinds of light in increasing or decreasing energy,
frequency or wavelength.
d. You need to know and be able to use the equation that relates frequency and wavelength: c =
λν.
Concept Area III: Atomic Line Spectra
a. You should understand that all light can be split to show that it contains multiple kinds of
waves.
b. You should be able to describe how the unique spectrum absorbed or emitted by an atom can
be used to identify the element.
c. You need to understand the difference between absorption and emission spectra and be able
to describe what each would look like for an element.
Concept Area IV: Electrons and Atomic Line Spectra
a. You should be familiar with the photoelectric effect (learn from book) and how it supports
Planck’s equation.
b. You need to understand that light consists of quantized particles called photons.
c. You should know that electrons can also be described as waves and that this is why atoms
give off unique line spectrums.
d. You should be familiar with the Bohr model of the atom.
e. You should know and be able to use Planck’s equation to find frequency and energy: E = hν.
Note, this means you must memorize Planck’s constant: 6.626×10–34 Js.
Che 170 Objectives for Third Exam.docx
Page 1 of 3
Concept Areas for CHE 170 Third Exam (all fair game on final exam)
f. You should be able to combine Planck’s equation with c = λν to relate energy and
wavelength: E = hc/λ.
g. You should be able to use de Broglie’s equation, λ = h÷(mv), to calculate the wavelength of
a particle.
Concept Area V: Atomic Orbitals
a. You should understand the Heisenberg uncertainty principle.
b. You should understand what is meant by probability density and the significance of quantum
mechanics how it relates to orbital shapes and the structure of an atom.
c. You should be able to differentiate between s, p, and d orbitals and be able to draw s and p
orbitals.
d. You should know that atomic orbitals have different amounts of energy based on which
energy level they are at.
Concept Area VI: Quantum Numbers
a. You need to know what the four quantum numbers are and what they represent: principal
quantum number, n; angular momentum quantum number, ℓ; magnetic quantum number, mℓ;
and electron spin, ms.
b. You need to understand the Pauli Exclusion Principle and why only two electrons can be put
into any given orbital.
Che 170 Objectives for Third Exam.docx
Page 2 of 3
Concept Areas for CHE 170 Third Exam (all fair game on final exam)
Chapter 8 – Periodic Properties of the Elements
Concept Area I: New Terms
• atomic orbital energy
diagram
• Aufbau principle
• degenerate
• diamagnetic
• effective nuclear charge,
Z*
• electron affinity
•
•
•
•
•
•
•
•
electronic configuration
ferromagnetic
filled subshell
ground state
half-filled subshell
Hund’s rule
inner-shell/core electrons
ionization energy
•
•
•
•
•
•
•
•
Noble gas notation
octet rule
orbital
paramagnetic
shell
shields, shielding
subshell
valence electrons
Concept Area II: Magnetism and Atomic Structure
a. You should know how to determine if a substance is paramagnetic or diamagnetic.
b. You should understand how magnets can be formed from ferromagnetic elements.
Concept Area III: Atomic Orbital Energy Level Diagrams
a. You need to remember what the four quantum numbers tell you (names of orbitals, how
many degenerate orbitals).
b. You need to know how many orbitals of each type are present in a shell or subshell of
specific energy.
c. You need to know how many electrons can go into each orbital, subshell and shell.
d. You should know that the different energies of atomic orbitals control the order in which
they fill up with electrons.
e. You should be able to use the Aufbau Principle and know when and why to break it for
certain elements.
f. You must be able to draw an atomic orbital energy level diagram or write an electron
configuration for any atom or ion.
g. You need to know where the valence electrons are located and how many of them there are.
Concept Area IV: Applications
a. You should remember that the periodic table is arranged so that elements with similar
properties are by each other.
b. You need to be able to calculate an approximation of the effective nuclear charge of an atom
or ion and use it along with atomic theory to explain some of trends on the periodic table.
c. You need to recognize the role that ionization energy and electron affinity play in the
chemistry of the elements and be able to explain the observed trends.
d. You should be able to predict whether an atom becomes larger or smaller when it becomes an
ion.
e. You should be able to explain why we can use the periodic table to predict the most
commonly formed ion for main group elements.
Che 170 Objectives for Third Exam.docx
Page 3 of 3