Download Chapter 13 Review

Chapter 13 Review
Atomic Models
The
first model of the atom
showing electrons was
developed by JJ Thomson.
What did he call his model?
The Plum Pudding Model
Atomic Models
Rutherford’s
model of the
atom included a ________.
nucleus
Atomic Models
The
Bohr Model was the
first model that showed the
electrons located in
________ ________.
energy levels
Atomic Models
Energy
levels on a Bohr
model are like _______ of a
__________.
steps of a ladder
Atomic Energy
A
___________ is the
amount of energy required
to move from one energy
level to the next.
quantum
Atomic Energy
What
do electrons usually
release when going from
the excited state back to the
ground state?
photons
Atomic Models
What
is the most current
model of the atom called?
Quantum Mechanical Model
Atomic Models
The
Quantum Mechanical
Model is based on who’s
equations?
Erwin Schrodinger
Atomic Sublevels
How
many sublevels are in
energy level 1?
1 sublevel (s)
Atomic Sublevels
How
many sublevels are in
energy level 2?
2 sublevels (s,p)
Atomic Sublevels
How
many sublevels are in
energy level 3?
3 sublevels (s,p,d)
Atomic Sublevels
How
many sublevels are in
energy level 4?
4 sublevels (s,p,d,f)
Atomic Orbitals
List
the 4 sublevels in order
of lowest energy to highest
energy.
s, p, d & f
Atomic Orbitals
How
many orbitals are in
the “s” sublevel?
1 orbital
Atomic Orbitals
How
many electrons are in
the “s” sublevel?
2 electrons
each orbital holds 2
electrons
Atomic Orbitals
How
many orbitals are in
the “p” sublevel?
3 orbitals
Atomic Orbitals
How
many electrons are in
the “p” sublevel?
6 electrons
Atomic Orbitals
How
many orbitals are in
the “d” sublevel?
5 orbitals
Atomic Orbitals
How
many electrons are in
the “d” sublevel?
10 electrons
Atomic Orbitals
How
many orbitals are in
the “f” sublevel?
7 orbital
Atomic Orbitals
How
many electrons are in
the “f” sublevel?
14 electrons
Atomic Orbitals
What
is the shape of the “s”
orbital?
sphere
Atomic Orbitals
What
is the shape of the “p”
orbital?
dumb bell
Atomic Orbitals
What
is the shape of the “d”
orbital?
cloverleaf
Energy Levels
How
many electrons can go
in energy level 1?
2 electrons (s)
Energy Levels
How
many electrons can go
in energy level 2?
8 electrons (s,p)
Energy Levels
How
many electrons can go
in energy level 3?
18 electrons (s,p,d)
Energy Levels
How
many electrons can go
in energy level 4?
32 electrons (s,p,d,f)
Electron Configurations
__________
___________
states that electrons enter
orbitals of lowest energy
first.
Aufbau Principle
Electron Configurations
 __________
_________
__________ states that only 2
electrons can occupy an
orbital and they must have
opposite spins.
 Pauli’s Exclusion Principle
Electron Configurations
 ___________
__________
states that electrons fill all
orbitals of the same energy
before putting 2 electrons in
the same orbital.
 Hund’s Rule
Electron Configurations
What
does the “3” in
tell you?
the energy level
10
3d
Electron Configurations
What
does the “d” in
tell you?
the sublevel
10
3d
Electron Configurations
What
10
3d
does the “10” in
tell you?
the number of electrons
Electron Configurations
An
atom is said to have an
________ when it has 8
electrons in its last energy
level.
octet
Electron Configurations
Write
the electron
configuration for
phosphorus.
1s22s22p63s23p3
Electron Configurations
Write
the electron
configuration for Iron.
2
2
6
2
6
2
6
1s 2s 2p 3s 3p 4s 3d
Electron Configurations
Write
the electron
configuration for bromine.
2
2
6
2
6
2
10
5
1s 2s 2p 3s 3p 4s 3d 4p
Electron Configurations
What
are the 2 exceptions
when writing electron
configurations?
Chromium and Copper
Electron Configurations
Write
the electron
configuration for chromium.
2
2
6
2
6
1
5
1s 2s 2p 3s 3p 4s 3d
Electron Configurations
Write
the electron
configuration for copper.
2
2
6
2
6
1
10
1s 2s 2p 3s 3p 4s 3d
Energy Levels
What
is the highest energy
level for Chlorine?
rd
3 (its in period 3)
Energy Levels
What
is the highest energy
level for Gold?
th
6 (its in period 6)
Orbital Notation
Draw
the orbital notation for
Iron.
see additional diagram