Transcript Electron Configuration - stroh

Catalyst – September 6+ 81 , 2.010x 103
1.
2.
3.
Draw the Bohr model for
Aluminum.
Draw the Bohr model for Boron.
What similarities do these two
Bohr Models have?
HOMEWORK OUT PLEASE!
Today’s Agenda
Catalyst
 HW Review
 Electron Configuration!!
 Practice, Practice, Practice
 Work Time!
 Exit Question

HOMEWORK: e- Config. Wksht.
Today’s Objectives
SWBAT compare and contrast the Bohr
model with the Quantum Model (the
modern atom).
 SWBAT write electron configurations for
elements.

HOMEWORK REVIEW!
How? Schrödinger Equation
Key Point #1: The Schrödinger
Equation predicts the location of
an electron in an atom.
 It tells us that electrons hang out in
atomic orbitals.
 Imagine electrons filing into hotels…
Schrödinger Equation and Atomic
Orbitals
Key Point #2: There are 4 atomic
orbitals…
s
p
d
f
A Saying to Remember the Four
Atomic Orbitals
some pirates die fiercely!
The s Orbital
One s orbital in each energy level
The s orbital is shaped like a sphere
Can hold 2 electrons total
So how many electron fit in the
FIRST energy level???
2
The p Orbital
Three p orbitals in each energy level
(starting in the 2nd energy level!)
Shape looks like dumbells or bowties
Can hold 6 electrons total
So how many electron fit in the
SECOND energy level???
8
2
The d orbital
-Five d orbitals in
each energy level
(starting in the 3rd
energy level!)
-Shape looks like
eggs or flowers
-Can hold 10
electrons
So how many electron fit in the
THIRD energy level???
18
8
2
The f orbital


Seven f orbitals (starting in 4th energy level!)
Can hold 14 electrons
So how many electron fit in the
THIRD energy level???
32
18
8
2
Electron Configuration
Review: Where do electrons hang out?
 Now, we have to know how many electrons
can fit into each atomic orbital
 Think of each orbital as a type of house

 Some
houses are big, some small
 Some houses have more bedrooms than
others
Electron Configuration
Review
Fill in the table below on your notes.
Orbital Type
(s, p, d, or f)
Energy Level
# of Orbitals
Maximum #
of Electrons
1,2,3,4…
1
2
2,3,4…
3
6
d
3,4…
5
10
f
4…
7
14
s
p
Electron Configuration


Key Point #3: Electron configuration
shows how the electrons are
distributed among the various
atomic orbitals and energy levels.
The format consists of a series of numbers, letters,
and superscripts as shown below:
1s2
The Code
Small superscript number = Number of electrons
2
1s
Large number = energy level
Letter = orbital
Figure it out yourself!! (15 mins)






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
Look at the table that has 1s, 2s, 2p on your notes sheet.
Here I have put a couple electron configurations. See if you
can figure out how to do the last two.
Mg-1s22s22p63s2
Ne- 1s22s22p6
Si- 1s22s22p63s23p2
K- 1s22s22p63s23p64s1
SB-
N–
Electron Configuration
2
1s
N–
Electron Configuration
2
2
1s 2s
N–
Electron Configuration
2
2
3
1s 2s 2p
N–
Electron Configuration
2
2
3
1s 2s 2p
= 7 e-
Na –
Electron Configuration
2
1s
Na –
Electron Configuration
2
2
1s 2s
Na –
Electron Configuration
2
2
6
1s 2s 2p
Na –
Electron Configuration
2
2
6
1
1s 2s 2p 3s
= 11 e-
Electron Configuration
Be:
Ne:
Br:
Electron Configuration
Be:
2
2
1s 2s
Ne:
2
2
6
1s 2s 2p
Br: 1s22s22p63s23p64s23d104p5
Noble Gas Configuration
Scientists are WAY too
lazy to write all that
mess!
Electron Configuration
FIGURE IT OUT YOURSELF!!! (10 mins)
2
14
10
[Xe]6s 4f 5d
Hg –
2
4
S – [Ne]3s 3p
2
5
Sm – [Xe]6s 4f
SiRb-
Noble Gas Configuration

Key Point #4: Noble Gas
configuration starts with noble gas
BEFORE the atom you are going to.
Exit Question

Write the electron configuration for the following 2
elements:

Manganese

Fluorine