Chemical Bonding - Ions and Metals: Valence Electrons

Question 1

valence electrons

Answer 1

• electrons in outermost energy level
• Cl: 1s^2 2s^2 2p^6 3s^2 3p^5
• Li: 1s^2 2s^1

Question 2

low energy states

Answer 2

• noble gases
• ms^2mp^6
• eight valence electrons-octet
• atoms
• compounds

Question 3

octet rule

Answer 3

• most representative elements react to form compounds through a process whereby their atoms gain, lose, or share valence electrons in order to achieve the highly stable (octet) electron configuration

Question 4

isoelectronic

Answer 4

• octet rule: representative elements
• duet rule: Li, Be
• consider hydrogen

Question 5

metals lose electrons

Answer 5

• low ionization energy: easy to remove
• cation: a positive ion
• magnitude of charge = group number
• electronic configuration
• Na atom —> Na+ ion

Question 6

predicting electron loss

Answer 6

• Li - 1s^2 2s^1 - 1s^2
• Li ^1+ - 1s^2
• Mg - 1s^2 2s^2 2p^6 3s^2
• Mg^2+ - 1s^2 2s^2 2p^6
• Al - 1s^2 2s^2 2p^6 3s^2 3p^1
• Al^3+ - 1s^2 2s^2 2p^6 (isoelectronic with Ne)

Question 7

nonmetals gain electrons

Answer 7

• high ionization energy - difficult to remove
• high electron(s) affinity - addition is stable
• anion - a negative charge
• Cl 1s^2 2s^2 2p^6 3s^2 3p^5
• Cl^1- 2s^2 2s^2 2p^6 3s^2 3p^6 (isoelectronic with Argon)

Question 8

predicting electron gain

Answer 8

• representative “A” group nonmetals gain electrons equal to the difference between eight and the group number
• magnitude of charge = 8-group #

Question 9

predicting electron gain

Answer 9

• F - 1s^2 2s^2 2p^5
• F^- - 1s^2 2s^2 2p^6 (isoelectronic with Ne)
• O - 1s^2 2s^2 2p^4
• O^2- - 2s^2 2s^2 2p^6 (isoelectronic with Ne)
• P - 1s^2 2s^2 2p^6 3s^2 3p^3
• P^3- - 1s^2 2s^2 2p^6 3s^2 3p^6 (isoelectronic with Ar)

Question 10

general rules for “A” gorup

Answer 10

• metals lose electrons: loss equals group number
• nonmetals gain electrons: gaine equals 8 - group number
• total lost = total gained: attain noble-gas configuration