Transcript Unit 07 Ionic Bonding

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
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
3
4
5
7
8
9
Lithium
Beryllium
Boron
Nitrogen
Oxygen
Fluorine
1s22s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
Valence
# Electrons
Electrons Gained
Lost
1
2
3
5
6
7
1
2
3
3
2
1
Ion Electron
Configuration
Ion
Symbol
w/ charge
1s2
1s2
1s2
1s2 2s2 2p6
1s2 2s2 2p6
1s2 2s2 2p6
Li+1
Be+2
B+3
N-3
O-2
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