1. Bell Ringer: 3/4/15
Classify the following elements as either a Metal, Non-Metal or Metalloid. As Na Br Ni Kr C F Fr

2. Ionic Compounds and Metallic Bonds
Chapters 6 and 7

3. Chemical Formulas Chemical Formula NaCl CO2 MgCl2 Na3P 1 Na and 1 Cl
Subscripts show numbers
No Subscript = 1 atom
NaCl
CO2
MgCl2
Na3P
1 Na and 1 Cl
1 C and 2 O
1 Mg and 2 Cl
3 Na and 1 P
end

4. Chemical Formulas # of total atoms (counting atoms): H2SO4 KNO3 Fe2O3
Hg2Cl2
end

5. Ba(OH)2 Chemical Formulas Cu (NO3)2 If you see ( )… Ba OH Cu NO3 O N H
Subscript applies to all atoms inside ( )
Ba(OH)2 Ba OH O H
Cu (NO3)2 Cu
NO3 N O
end

6. Chemical Formulas # of total atoms: Cu(NO3)2 KMnO4 Al2(SO4)3 (NH4)3PO4
end

7. Chemical Bonds Valence Electrons e- in highest energy level
Determine chemical properties
How many in: Li S Ba P F Al
end

8. Chemical Bonds Octet Rule To get 8 valence, atoms either:
Atoms want 8 val. e-
Stable Configuration
Nobel Gas: ns2 np6
Transition metals also want:
Half-Filled d-orbital: ns2 np6 nd5
Filled d-orbital: ns2 np6 nd10
To get 8 valence, atoms either:
Transfer Electrons
Share Electrons
end

9. Formation of a Chemical Bond
Force holding 2 atoms together
3 types:
Ionic (Metal and Nonmetal)
Covalent (Nonmetal and Nonmetal)
Metallic (Metal and Metal)

10. Chemical Bonding Ionic or Covalent? CaCl2 LiBr CO2 SO3 H2O BaSO4
NaF NO2
CH4 AlPO4
end

11. Chemical Bonding
Complete #1-10 on “Types of Chemical Bonds”

12. Ionic Bonds Ionic Bonds Metal and Nonmetal (or Polyatomic Ion)
ΔEN > 1.7
Electrons are TRANSFERRED
Ions (atom with a charge)
Charges = Oxidation States
Combine to make neutral compounds
Ionic Compounds = Salts
end

13. Ionic Bonds Ions Atoms with a charge
Formed by losing/gaining electrons
Positively charged = Lost e- = Cation
Negatively charged = Gain e- = Anion
end

14. Ionic Bonds The Periodic Table can predict the charges
Metals will lose electrons
Cations
Nonmetals will gain electrons
Anions
The charge is known as the Oxidation Number
Arranged by Group
Cannot predict a Transition Metal’s charge
Ions will combine so the overall charge = 0
end

15. Ionic Bonds Group: 1 2 13 14 15 16 17 18 # of 1 2 3 4 5 6 7 8 Valence:
Oxidation States follow the Valence Electrons
Group:
# of
Valence:
Oxidation
State: ±
end

16. Ionic Compounds Lattice Energy
Physical Properties of Ionic Compounds:
High M.P. & B.P.
Brittle
Conduct Electricity as liquids (molten) or when dissolved
Crystal Lattice structure
Anions and Cations alternate
Lattice Energy
Energy needed to break apart the crystal lattice
end

17. Naming Ionic Compounds
3 steps
Name the Cation
Name the Anion
Change the Ending to –ide
NaBr
Sodium
Bromine
Sodium
Bromide
end

18. Naming Ionic Compounds
Name the following:
BaS
MgF2
Ca3N2
end

19. Naming Ionic Compounds
Complete the following on “Naming Binary Compounds (Ionic)”

20. Naming Ionic Compounds
More than 2 elements = POLYATOMIC ION!!!
Get name from the REFERENCE TABLE!!!
DON’T change the ending!!!
NaNO3
Sodium
Nitrate
end

21. Naming Ionic Compounds
Name the following:
KOH
NaC2H3O2
(NH4)2O
Sr3(PO4)2
end

22. Naming Ionic Compounds
Complete 1-8, 10, 11 on “Naming of Non-Binary Compounds”

23. Writing Ionic Compounds Binary & Ternary

24. Writing Ionic Formulas
Writing formulas:
3 steps:
Write the cation, with charge
Write the anion, with charge
Cross the charges to get subscripts
Do NOT put the “+” or “-”
end

25. Writing Ionic Formulas
Write the formulas for the following:
Beryllium Phosphide
Calcium Fluoride
Strontium Sulfide
end

26. Writing Ionic Compounds

27. Writing Ionic Formulas
Polyatomic Ions ARE A GROUP
Write ( ), then cross charges
Write the formula for the following:
Calcium Phosphate
Barium Nitrate
Sodium Chromate
Ammonium Acetate
end

28. Writing Ionic Formulas
Homework:
p.207 #2 a-f
p.211 #2 b-d, & f
p. 235 #7

29. Bell Ringer Name the following compounds: BaCl2 K2CrO4 Na2CO3
Pb(NO3) 2
Identify the cations and anions:

30. Transition Metals 2 valence electrons But Many Oxidation States
Names show the charge
Exceptions:
Silver: Ag+
Zinc: Zn2+
Lead (Pb) and Tin (Sn) can either be 2+ or 4+
end

31. Transition Metals The metal's charge is the Roman Numeral
Vanadium (III) Sulfide
V S2-
V2S3
Metal's Charge
end

32. Transition Metals Write formulas for the following:
Osmium (V) Fluoride
Silver Nitride
Technetium (VII) Phosphate
end

33. Transition Metals
Complete “Writing Binary Formulas Worksheet”

34. Transition Metals Names MUST have a Roman Numeral!
To get charge, uncross subscripts!
Fe2O3
Fe O2-
iron (III) oxide
end

35. Transition Metals
Name the following:
HgF2
Hf2S5 YP
end

36. Naming Ionic Compounds
Complete the following on “Naming Binary Compounds (Ionic)”
3 12
4 13
5 16
6 19
7 20

37. HW
Silver oxide Copper (I) bromide Copper (II) bromide Iron (II) oxide Iron (III) oxide
Chromium (II) chloride Chromium (III) chloride Mercury (I) Iodide Manganese (II) oxide Manganese (III) oxide

38. DRY LAB -IONIC BONDING

39. Bell Ringer: Chemical Bonding Review:
1. What are the three types of Chemical Bonds?
2. What is the Octet Rule?
3. What kind of ion has a positive charge?
4. During Ionic Bonding, what type of atom loses their electrons, and which type of atom gains electrons?
5. What is an atom's oxidation state?
6. Why does a transition metal have a roman numeral in its chemical name?
Get your Worksheet out from Friday (Acids on Back)

40. Mixed Ionic Review With Transition Metals

42. Acids Acids Hydrochloric Acid HCl Nitric Acid HNO3 Sulfuric Acid H2SO4
Start with hydrogen (H)
Ionize when mixed with water
Produce H+ and anions
Common acids:
Hydrochloric Acid HCl
Nitric Acid HNO3
Sulfuric Acid H2SO4
Acetic Acid HC2H3O2 or CH3COOH
end

43. NAMING ACIDS Binary Acids Hydrogen + 1 element
Name as: hydro- ___ -ic acid HF
H3P
H2S
H2O
end

45. NAMING ACIDS Oxyacids ___ -ate  ___ -ic acid ___ -ite  ___ -ous acid
Hydrogen + Polyatomic Ion
Follow polyatomic names
___ -ate  ___ -ic acid
___ -ite  ___ -ous acid
end

47. NAMING ACIDS
H3PO4
HClO2
HNO2
HClO3
end

48. Formulas of Acids *Honors*
Cross charges like Ionic Formulas
Hydrogen = H+
Watch out for elements/polyatomic ions
Write formulas for:
Hydrosulfic acid
Hydrochloric acid
Nitric acid
Carbonous acid
end

49. NAMING ACIDS
Complete #1-20 on “Naming Acids”

50. Metallic Bonds Metallic Bond Metal and Metals
Valence e- shared between ALL atoms
Metal Cation + a “sea of electrons”
end

51. Metallic Bonds More Shared Electrons = Stronger Bond
Properties of Metals:
High M.P. & B.P.
Conductive
Malleable/Ductile
end

52. Homework
Complete Back Side of Worksheet on Acids