Models
Name: ____________________________________________________ Period: ___________
Chapter 5 Section 3 Guided Reading: Electron Configuration
Electron Configurations Reading:
1. The orbit that an electron follows is described in terms of ___________________,
______________ and ___________________. It can also be described in terms of
_______________and _______________.
2. Electron configuration describes how an atom’s ___________________ orbit it’s
________________.
3. How is the electron configuration for Hydrogen written? ___________
4. The _________________ indicates that hydrogen’s one electron orbits the nucleus in
an orbital that has a ________________________ (___) shape and is in the
_____________ (___) energy level.
5. The first energy level can hold only _____ electrons.
6. What is the electron configuration for lithium? ______________________ How many
energy levels does lithium occupy? ___________
7. What is the electron configuration for silver? __________________________________
8. How many energy levels do silver’s electrons occupy? ____ How many different orbital
types are there in silver’s electron configuration? __________ What are they?
_____________________
9. The first rule of electron configuration states that “An electron MUST occupy the
______________ energy level available”.
10. The second rule of electron configuration states that “Each orbital can hold only a
certain number of electrons. The ____ orbital can hold a maximum of ____ electrons,
while the ____ orbital can hold ____ electrons, and the _____ orbital can hold as many
as ______ electrons. Another orbital, known as that __________________, can hold a
maximum of ________ electrons.”
11. The third rule of electron configuration states that “electrons fill __________________
that have the ______________ energy first.”
12. An electron that occupies a higher energy level although a lower energy level is available
is said to in an __________________________.
13. When all the electrons occupy the lowest energy levels available, they are said to be in a
____________________________.
Chapter 5.3 - Ground-State Electron Configuration
1. Why do electrons in an atom tend to assume the arrangement that gives the atom the
lowest energy possible?
______________________________________________________________
2. What are the names of the three rules, or principles, of electron configuration?
a. _________________________
b. _________________________
c. _________________________
3. The ____________________________________ states that each electron occupies the
lowest energy orbital available.
4. Electrons in orbitals can be represented by _____________. Each electron has an
associated ____________. An arrow pointing _______(____) represents a spin in one
direction, while an arrow pointing ____________ (_____) represents a spin in the
____________ direction. An empty box, or line, represents an
__________________________ orbital, while a box, or line, containing a single
___________________ (___) represents an orbital with _____ electron, and a box, or
line, containing both an _______ and a __________ down arrow (_______) represents a
______________ orbital.
5. The ______________________________________________________ states that a
maximum of _________ electrons can occupy a single atomic orbital, but only if the
electrons have __________________________ spins. According to this principle, an
atomic orbital containing paired electrons with ___________________ spins is written
________.
6. What type of charged electrons repel each other? _____________________________
7. _____________________________ states that single electrons with the same spin much
occupy each equal-energy orbital before additional electrons with opposite spins can
occupy the same orbitals.
8. Draw Hund’s Rule according to the 2p orbitals:
a. _____ _____ _____
b. _____ ______ ______
c. _____ ______ ______
d. _____ ______ ______ e. _____ ______ ______
f. _____ ______ ______
Chapter 5.3 - Electron Arrangement:
1. What are the boxes, or lines, in the orbital notation labeled with?
_________________________ and ______________________________________.
2. Show carbon’s orbital electron configuration (make sure to label each line):
a. ______ _______
_______ _______ ______
3. The electron configuration notation designates the
________________________________ and __________________________ associated
with each of the atom’s orbitals and includes a _____________________________
representing the number of electrons in the ______________.
4. Electron configuration notation does not usually show the _________________
distributions of electrons related to a sublevel.
5. Noble gases are found in the last __________________ of the periodic table. They have
_____ electrons in their outermost orbital, and are very _________________.
6. How is noble gas configuration beneficial when writing out electron configurations?
________________________________________________________________________
Chapter 5.3 - Valence Electrons:
1. Only _______________ electrons determine the _____________________ properties of
an element. They are defined as the electrons in the atom’s __________________
orbitals, the level typically associated with the atom’s ____________________ principle
energy level.