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Electron Configuration and Stability in Chemistry: Exercises and Questions, Study notes of Chemistry

Milwaukee Institute of Art & Design (MIAD)Chemistry

PART B – SHORTHAND ELECTRON CONFIGURATION. Use the patterns within the periodic table to write the longhand electron configuration notation.

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[Type text] [Type text] [Type text]
Electron Configuration – Ch. 4 CHEM
Electron Configurations Name ____________________________
Date ________________ Per ______
PART A – ORBITAL NOTATION
Use the patterns within the periodic table to write the orbital notation for the following atoms.
Symbol
# e-
Orbital Notation
1.
Mg
     
1s2 2s2 2p6 3s2
2.
Ar
        
1s2 2s2 2p6 3s2 3p6
3.
V
          __ __
1s2 2s2 2p6 3s2 3p6 4s2 3d3
4.
Ge
              __
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2
5.
Kr
                
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
6.
Ca
         
1s2 2s2 2p6 3s2 3p6 4s2
pf3

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[Type text] [Type text] [Type text]

Electron Configuration – Ch. 4 CHEM

Electron Configurations Name ____________________________

Date ________________ Per ______

PART A – ORBITAL NOTATION

Use the patterns within the periodic table to write the orbital notation for the following atoms.

Symbol

# e

Orbital Notation

1. Mg

1s^2 2s^2 2p^6 3s^2

2. Ar

1s^2 2s^2 2p^6 3s^2 3p^6

3. V

             __ __

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^3

4. Ge

                 __

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^2

5. Kr

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6

6. Ca

1s^2 2s^2 2p^6 3s^2 3p^6 4s^2

Stability & Electron Configuration – Ch. 4 CHEM

PART B – SHORTHAND ELECTRON CONFIGURATION Use the patterns within the periodic table to write the longhand electron configuration notation for the following elements. Symbol # e

Longhand Electron Configuration Notation

  1. S 1s^2 2s^2 2p^6 3s^2 3p^4
  2. Pb 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^2
  3. F 1s^2 2s^2 2p^5
  4. U 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^2 4d^10 5p^6 6s^2 4f^14 5d^10 6p^6 7s^2 6d^1 5f^3
  5. Ag 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^10 4p^6 5s^1 4d^10 PART B – RULES OF ELECTRON CONFIGURATIONS Which of the following “rules” is being violated in each electron configuration below? Explain your answer for each. Hund’s Rule, Pauli Exclusion Principle, Aufbau Principle
  6.    __ __ 1s 2s 2p Hunds Rule – does not have a maximum number of unpaired electrons
  7.      ___  _ _ 1s 2s 2p 3s 3p Aufbau Principle – electrons skip sublevels (not a ground state configuration)
  8.         _ 1s 2s 2p 3s 3p Pauli Exclusion Principle – 3s electrons are not paired.