Docsity
Docsity

Prepare for your exams
Prepare for your exams

Study with the several resources on Docsity


Earn points to download
Earn points to download

Earn points by helping other students or get them with a premium plan


Guidelines and tips
Guidelines and tips

Understanding Atomic Electron Configurations and Inert Gases, Lecture notes of Molecular biology

The concept of inert gases and noble gas configuration in atoms. It discusses the division of electrons into core and outer groups, the significance of looking isoelectronic to a noble gas, and the importance of having full or half-full orbitals for stability. It also includes examples of various elements and their electron configurations in the ground and excited states.

What you will learn

  • Which noble gas is S2- isoelectronic to?
  • What is the most stable electron configuration for Chromium?
  • Which element has a noble gas configuration with 3 valence electrons?
  • Which transition metal will lose its electrons in the order p before s before d?
  • What is the most stable electron configuration for Copper?

Typology: Lecture notes

2021/2022

Uploaded on 09/27/2022

anandit
anandit 🇺🇸

4.8

(19)

255 documents

1 / 18

Toggle sidebar

This page cannot be seen from the preview

Don't miss anything!

bg1
What are inert Gases again??
NOBLE GASES!!
pf3
pf4
pf5
pf8
pf9
pfa
pfd
pfe
pff
pf12

Partial preview of the text

Download Understanding Atomic Electron Configurations and Inert Gases and more Lecture notes Molecular biology in PDF only on Docsity!

What are inert Gases again??

NOBLE GASES!!

Hebden Pg 156 #27 ( odds only)

  1. This means “having the same number of electrons / the same electron configuration as a noble gas” but not the same number of protons or the same properties.
  2. Recall …Mg vs. Mg 2+ Mg 1s 2 2s 2 2p 6 3s 2 Mg 2 +  1s 2 2s 2 2p 6 *loses two electrons to be isoelectronic with Neon (Ne) The e- in Mg 2 + are the same as Neon, and the configuration is the same, but they are still different elements – most elements want to do this - be Isoelectronic (look-alikes) with Noble gases.

Ne 1s

2

2s

2

2p

6

Titanium Ion…Ti

Ti

 [Ne] 3s

3p

You can’t just write [Ar]!!

  1. Br 1 -
  2. Sc 3 +
  3. N 3 -
  4. Sb 3+ Br 1 - :[Ar]3d 10 4s 2 4p 6 Mn 2 + : [Ne] 3s 2 3 p 6 N 3 - : [He]2s 2 2p 6 Sb 3+ : [Kr]4d 10 5 s 2
  1. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2
  2. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 1
  3. 1s 2 2s 2 2p 4 3s 1
  4. 1s 2 2s 2 2p 6 3s 1
  5. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 (20 e-) = Calcium GS
  6. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 1 (20e-) = Calcium ES!!!
  7. 1s 2 2s 2 2p 4 3s 1 (9 e-) = Fluorine ES!!!
  8. 1s 2 2s 2 2p 6 3s 1 (11e-) = Sodium GS
  1. The most stable orbitals are completely full (all paired electrons) or half full (no paired electrons). a. These types of orbitals are lower in energy (more stable) than those which are partially filled. b. This is especially important for p, d, and f orbitals
  2. Atoms will sometimes rearrange their electrons between orbitals close in energy in order to obtain one of these above conditions.
  1. The transition metals (d-orbitals) will lose electrons from their outer orbitals (highest n value) first, and then the d-orbitals to form stable ions. (p before s before d ) e.g. Sn [Kr] 36 4d 10 5s 2 5p 2 Sn 2 + [Kr] 36 4d 10 5s 2 5p 0 Sn 4 + [Kr] 36 4d 10 5s 0 5p 0

“Those electrons in an atom, that are not in an

inert Gas formation core, or are not in a full d or f

subshell” ….

Al  [Ne] 3s

2

3p

1

Ga  [Ar] 3d

10

4s

2

4p

1

Pb  [Xe] 4f

14

5d

10

6s

2

6p

2

Xe  [Kr] 4d

105

s

2

5p

6

= 3 valence e-

= 3 valence e-

= 4 valence e-

= 0 valence e-

(noble gas)