Ch 7: Ionic BondingFormula Writing

My Name is Bond. Ionic Bond. Taken NOT shared

Review

1) Why do atoms come together? 2) What types of atoms form an ionic bond? 3) What is the relationship between ionic

bonding and electronegativity? 4) What happens to the electrons in an ionic

bond?

Review Answers

1) Atoms come together to achieve stability by filling their valence shells.

2) A metal with a nonmetal 3) Ionic bonds form between atoms with a huge

difference in electronegativity:4) One atom is so much stronger (more

electronegativity), it TAKES the electrons

2 Types of Ions

• Cation = a positively charged ion (lost e-)– Less electroneg./metal

• Anion = a negatively charged ion (gained e-) – More electroneg. /nonmetal

Monatomic Ions

• “Mono” = One • “Atomic” = Atom• Monatomic Ion: An ion in which a single atom

has a positive or negative charge

Charge and the Periodic Table

Transition Metals

• Have multiple charges• Positive charge (Cations) • Their charge is indicated by the Roman

Numeral following their name– Iron (II) = Fe+2

– Iron (III) = Fe+3

Ions and Electron Configuration

Atomic Number

Element Electron Configuration

Valence Electrons

# Electrons Ion Electron Configuration

Ion Symbol

w/ chargeGained Lost

3 Lithium 1s22s1 1 1 1s2 Li+1

4 Beryllium 1s2 2s2 2 2 1s2 Be+2

5 Boron 1s2 2s2

2p1 3 3 1s2 B+3

7 Nitrogen 1s2 2s2 2p3 5 3 1s2 2s2 2p6 N-3

8 Oxygen 1s2 2s2 2p4 6 2 1s2 2s2 2p6 O-2

9 Fluorine 1s2 2s2 2p5 7 1 1s2 2s2 2p6 F-1

Polyatomic Ions

• “Poly” = Many• “Atomic” = Atom• An ion containing more than one atom that

has collectively lost or gained electrons• Ex. NO3

-1

Ionic Compounds

• Attraction between cation and anion• The cation is always written first and gets to

keep his name• Subscripts = the number of IONS in the

formula. Use ( ) for polyatomic ions. • Overall charge of the compound is zero

Examples #1-4: Monatomic & Main Group Ionic Compounds

#1) Sodium Fluoride

#2) Magnesium Chloride

#3) Beryllium Sulfide

#4) Aluminum Oxide

Examples #5-6 Monatomic & Transition Metal Compounds

#5) Iron (II) Bromide

#6) Silver Nitride

Examples #7-9 Main Group Metals with Polyatomic Anion

#7) Lithium Nitrate

#8) Calcium Carbonate

#9) Aluminum Periodate

Examples #10-11: Transition Metal with Polyatomic Anion

#10) Copper (II) Phosphate

#11) Iron (III) Dichromate

Example #12 An Exception: A Polyatomic Cation!

#12) Ammonium Cyanide

Nomenclature

• Nomenclature = Naming

• An ionic bond has 2 ions (a cation and an anion) so its name will always have 2 parts.

Rules for Naming Ionic Compounds

• The metal cation is always written first

• The metal cation gets to keep its name – Ex. Na = Sodium – Ex. Ca = Calcium

• ONE EXCEPTION: One polyatomic cation = ammonium (NH4

+)

Rules for Naming

• Transition metals need a Roman Numeral – Ex. CuO

– Ex. Cu2O

Rules for Naming

• A Monatomic anion will keep its name but the ending is changed to “ide” – Ex. Cl-1 = Chloride– Ex. O-2 = Oxide– Ex. N-3 = Nitride

• A polyatomic anion will end in “ate,” “ite” etc. – On your Common Ion Sheet or in your memory!

Naming Binary Compounds: Main Group Cations

• Binary = Made up of 2 types of elements 1. KBr

2. SrCl2

3. Rb2O

Naming Binary Compounds: Transition Metal Cations

4. NiO

5. Ni2O3

6. SnO2

Naming: Main Group Cations + Polyatomic Anions

7. Al(NO3)3

8. MgCO3

10. NaC2H3O2

Naming: Transition Metal Cation + Polyatomic Anion

9. Cu2SO4

11. Zr3(PO4)2

Naming: An exception

12. NH4IO