Shell Game

1
Shell Game

• Sub-shells and electrons

2
ChemCatalyst

• The two drawings show two ways of representing
  the electron arrangement of the element calcium,
  Ca.
• Name at least two differences.
• Name at least two similarities.

Unit 1 Investigation III
3
Discussion results

• Similarities

• Differences

4
The Big Question

• How do electron subshells relate to the periodic
  table?

Unit 1 Investigation III
5
You will be able to

• Identify an element based on its electron
  configuration.

Unit 1 Investigation III
6
Notes

• Electron shells are divided into electron
  subshells.
• Subshells are determined by amount of electrons
  and energy level of those electrons

Unit 1 Investigation III
7
Reason for the configuration

• Electrons groups are placed in different rows
  based on the amount of energy they possess
• Electrons can only possess certain amounts of
  energy and achieve even a temporary amount of
  stability
• Amount of energy correlates to position. The
  positions nearest the nucleus require the least
  energy

8
Activity

• Purpose This lesson introduces you to electron
  subshells. You will explore how they are related
  to the periodic table.

(cont.)
Unit 1 Investigation III
9
S-P-D-F

• S(ome) P(eople) D(ont) F(orget)
• S subshells hold the fewest electrons at the
  lowest energy levels
• F subshells hold the most electrons with the
  highest energy levels

10
The difference between orbitals and subshells
Sublevel of orbitals it contains (1st 4 odd s) Total of electrons it can hold (2 x the of orbitals)
S 1 2
p 3 6
d 5 10
f 7 14
11

Notes

• An electron configuration is a list of all the
  subshells that have electrons for a given
  element.
• The number of electrons in a subshell is
  specified as a superscripted number.

Unit 1 Investigation III
12
Writing the electron configuration for an element

• The subshells are filled according to the amount
  of energy required for each electron
• 1s requires the lowest, 2s follows
• Partial list, 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s,
  4d, 5p

13
(No Transcript)
14
Configuration for different elements

• Hydrogen 1s1
• Oxygen 1s2 2s2 2p4
• Aluminum 1s2 2s2 2p6 3s2 3p1

• Argon
• Calcium
• Chromium
• Selenium

15
Arrow diagram for order of filling sublevels

• Color your copy
• 4 blocks where you will be adding electrons to
  different sub-shells, one block for each
  sub-shell letter (s, p, d, f)

16
(cont.)
Unit 1 Investigation III
17
(cont.)
Unit 1 Investigation III
18
Another way to determine the order that subshells
are filled
19
Shorthand configuration for larger elements

• The configuration can shortened by writing the
  symbol of the nearest noble gas with a smaller
  atomic number
• Example
• The configuration for Magnesium is
• 1s2 2s2 2p6 3s2
• Or it can be written as Ne 3s2

20
In class questions
21
(cont.)
Electron configuration Element
1s22s1
1s22s22p3 nitrogen, N
1s22s22p63s23p5
1s22s22p63s23p64s23d6
1s22s22p63s23p64s23d104p2
1s22s22p63s23p64s23d104p65s24d105p4 tellurium,Te
Unit 1 Investigation III
22
Making Sense

• How is the organization and structure of the
  periodic table related to electron subshells?

(cont.)
Unit 1 Investigation III
23
Check-In

• Identify the element with the following electron
  configuration.
• 1s22s22p63s23p64s23d104p3

Unit 1 Investigation III
24
Wrap-Up

• Electron shells can be divided further into
  subshells, referred to as s, p, d, f.
• Each subshell can hold a specific maximum number
  of electrons. The s subshell can hold 2
  electrons, the p subshell can hold 6, the d
  subshell can hold 10 electrons, and the f
  subshell can hold 14.

(cont.)
Unit 1 Investigation III
25
(cont.)

• The periodic table can assist us in figuring out
  the sequence of filling the subshells with
  electrons.
• Chemists keep track of electrons and the
  subshells they are in by writing electron
  configurations.

Unit 1 Investigation III