Name ___________________
Reading Guide: Atomic Structure 2/Periodicity
(Chapters 4 and 5)
Section 4.1: Development of a New Atomic Model
Define the following terms:
electromagnetic radiation
quantum
photon
line emission spectrum
Answer the following questions:
Describe the photoelectric effect.
What is meant by the dual wave-particle nature of electromagnetic radiation?
What does the energy of a photon depend upon?
How does the Bohr model explain the emission spectrum of a hydrogen atom?
Section 4.2: Quantum Model of the Atom
Define the following terms:
quantum theory
orbital
quantum number
principal quantum number
Principle energy level
Honors Chemistry
Carpenito/Dinota
Answer the following questions:
What are some specific examples of the wave nature of electrons?
What is the fundamental difference between the Bohr model of the atom and the wave-mechanical model of the
atom?
Explain why the location of an electron in an atom is uncertain using the Heisenberg uncertainty principle and de
Broglie’s wave-particle duality.
How is the distance of an electron from the nucleus related to the principal energy level?
What is the relationship between n and the number of sublevels in an energy level? the number of orbitals in an
energy level?
What do the s, p, d, and f sublevel designations (angular momentum quantum number) tell us about an atom’s
orbitals?
Section 4.3: Electron Configurations
Define the following terms:
Electron configuration
Aufbau principle
Pauli exclusion principle
Hund’s Rule
Answer the following questions:
What must be true of two electrons that occupy the same orbital?
Write ground state electron configurations, using the noble gas notation, for the following elements:
a. Bromine (Br)
b. Strontium (Sr)
c.
Antimony (Sb)
d. Rhenium (Re)
e. Titanium (Ti)
Draw the orbital notation for each of the following elements:
a. Silicon (Si)
b. Fluorine (F)
c.
Calcium (Ca)
d. Krypton (Kr)
A chlorine atom in the ground state has a total of 7 electrons in orbitals related to the atom’s third energy level.
How many of the 7 electrons occupy p orbitals? How many of the 17 electrons in a chlorine atom occupy p
orbitals?
When a sulfur atom reacts with other atoms, electrons in orbitals related to the atom’s third energy level are
involved. How many such electrons does a sulfur atom have?
What element is represented by each electron configuration?
a. [Kr]5s24d105p1
b. 1s22s22p5
c.
[Xe]6s24f4
d. [Ar]4s2
e. 1s22s22p63s23p64s23d104p5
Section 5.2: Electron Configuration and the Periodic Table
Define the following terms:
s block
p block
d block
transition elements
main group elements
Answer the following questions:
How is an elements electron configuration related to the period it occupies on the periodic table?
What determines the length of each period in the periodic table?
What information is provided by the specific block location of an element?
Why are hydrogen and helium separated from the other elements in the same group (groups 1 and 18,
respectively)?
Section 5.3: Electron Configuration and Periodic Properties
Define the following terms:
Atomic radius
Ion
Ionization energy
cation
anion
valence electrons
electronegativity
Answer the following questions:
What are the period and group trends for atomic radius? Explain the trends.
What are the period and group trends for ionization energy? Explain the trends.
What is meant by electron affinity?
How the does the ionic radius of a nonmetal compare with its atomic radius? Explain the change in radius.
How does the ionic radius of a metal compare with its atomic radius? Explain the change in radius.
In what sublevels are valence electrons always located?
What element has the highest value for electronegativity? Where on the periodic table are the elements with
relatively high electronegativity values found?
Explain why the d block elements have little variation in periodic properties (atomic radius, ionization energy,
etc).
Why aren’t electronegativity values listed for noble gases?