Ch 7: Ionic Bonding Formula 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 Atoms come together to achieve stability by filling their valence shells. A metal with a nonmetal Ionic bonds form between atoms with a huge difference in electronegativity: 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/ charge Gained Lost 3 Lithium 1s22s1 1 1s2 Li+1 4 Beryllium 1s2 2s2 2 Be+2 5 Boron 1s2 2s2 2p1 B+3 7 Nitrogen 1s2 2s2 2p3 1s2 2s2 2p6 N-3 8 Oxygen 1s2 2s2 2p4 6 O-2 9 Fluorine 1s2 2s2 2p5 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

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 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