Unit 1: Principles of Chemistry Chp 7. Ionic bonding Chp 8 Covalent bonding, Chp 9 Metallic bonding

OBJQ

The state relation of group numbers and their ion patterns

Group 1 → (1)+ ions

Group 2 → 2+ ions 

Group 3 → 3+ ions 

Group 5 → 3- ions 

Group 6 → 2- ions 

Group 7 → (1)- ions

OBJQ

State Ag, Cu, Pb, Zn, and Fe ion patterns

Ag^+, Cu^2+, Pb^2+, Zn^2+, Fe^2+, Fe^3+,

OBJQ

State hydrogen, hydroxide, ammonium, carbonate, nitrate and sulphate ion patterns

Hydrogen (H⁺), hydroxide (OH⁻), Ammonium (NH₄⁺), Carbonate (CO₃⁻), Nitrate (NO₃⁻), Sulfate (SO₄²⁻)

OBJQ

Define 'ionic bond' in terms of electrostatic attraction. 

Strong electrostatic attraction between positive and negative ions.

FAQ

Explain how metals form metal ions.

A metal atom has (...) electrons in its outer shell. It loses (...) electrons to form (...) ions (depending on electrons lost to get a stable electronic structure)

FAQ
Explain how non-metals form negative ions.

A non-metal atom has (...) electrons in its outer shell. It gains (...) electrons to form (...) ions (depending on electrons gained to get a stable electronic structure)

FAQ
Explain how a metal and a non-metal form compounds in terms of electron transfer and electrostatic force.

(metal) has (...) electrons in the outer shell, and (non-metal) has (...) electrons in the outer shell. (...) numbers of electrons are transferred from (metal) to (non-metal) to form (metal ions and non-metal ions). (compound) is formed by strong electrostatic attraction between (metal ions) and (non-metal ions).