1. Agenda: 3/17 – 3rd block
Homework: Re-write in paragraph form – notes pages 1 and 3. Add additional information learned in practice.
Objective: To interpret (correctly write) formulas and names for compounds – using IUPAC convention Warm-up: review names & formulas Review: Binary Ionic Compounds More Complex Ionic Compounds With Polyatomic Ions With Transition Metals Covalent Compounds

2. Warm-up: Review names & formulas
Type of Bond and Compound
Name
MgCl₂
SO₂
PCl₃
AlBr₃
K₃N
BrO₃
H₂O

3. Language of chemistry: Standardize system to represent compounds
Inorganic Compounds
Ionic
M & NM
With Roman numeral
3 or more elements
Covalent (molecules)
NM & NM
Diatomic Molecules
Acids

4. Metals lose valence electrons Non-metals gain valence electrons
Ionic Compounds
Metals lose valence electrons
Non-metals gain valence electrons

5. Ionic Bonding: Transfer of valence electrons
Ionic bonding occurs when a metal loses 1 or more electrons to a non-metal in an effort to attain a stable octet of valence electrons.
Use Electron Dot Diagrams (Lewis diagrams) to show the ionic bonds for one formula unit.
Na Cl = Na⁺¹Cl⁻¹

6. Electron Dot Diagram (Lewis)
Cl Ca Cl
= Ca Cl

7. Some Ionic Compounds are more complex
Include polyatomic ions

8. Ionic compounds: Found in minerals and rocks
Barite = BaSO₄
Used to make paper & glass
Source of barium used
For x-rays of the digestive
system

9. Ionic compounds: Found in minerals and rocks
Gypsum = CaSO₄· 2H₂O
Used for plaster for
walls, ceilings, sculptures

10. Ionic compounds: Found in minerals and rocks
Calcite = CaCO₃
Used in paint,
Antacids, calcium
Supplement for food

11. Ionic compound with polyatomic ions
Calcium sulfate in casts
Barium sulfate to absorb x-rays
Acetate uses
Sodium acetate
In Heat packs

13. Sodium hydrogen carbonate
(old name: sodium bicarbonate)
Medical: used in emergency situations to correct pH of blood
Baking soda: to make cakes rise

14. Bleach
Dentistry:
Clean and disinfect
Root canals
Rocket fuels:
Source of oxygen

15. POLYATOMIC IONS Examine the names & formulas:
What is the pattern? Do they end in “–ide?”
Ions with -1 charge
perbromate BrO4-1
bromate BrO3-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
thiocyanate SCN-1
acetate C2H3O2-1
Permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
phthalate C8H4O4-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
peroxide O2-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1

16. Compounds vs. Polyatomic Ions

17. Polyatomic ions that you must know:
NAME
FORMULA
CHARGE
Nitrate
Acetate
Carbonate
Sulfate
Phosphate
Hydroxide
Ammonium

18. Using polyatomic ions:
Sodium + nitrate Calcium + nitrate
Formula
Name:

19. Writing Formulas (criss –cross method)
Cl¹⁻
CO₃²⁻ OH
SO₄²⁻
PO₄³⁻
NO₃¹⁻
Na¹⁺
NH₄¹⁺
Zn²⁺
Co³⁺

20. Ionic Compounds with Transition Metals
The transition metals are elements in Groups _____ to _______.
+ post transition metals: under the staircase.
Transition metals can have more than one charge.
Use Roman numerals after the name.
Roman numbers:
I = II = III = IV = V=

22. Transition metals Examples Iron II oxide Iron III oxide
Write the formulas for:
Copper I oxide
Cobalt III chloride
Nickel II sulfide

23. Formula Writing Practice
Sulfide
Sulfate
Oxide
Carbonate
Mercury II
Iron III
Iron II

24. Practice: Writing Binary Formulas
Many transition and post transition metals have multiple oxidation numbers (charges)
Ni: oxidation numbers of _____ & _____
Fe:
Find other examples:
Write formulas
Write names

25. Language of chemistry: Standardize system to represent compounds
Inorganic Compounds
Ionic
M & NM
With Roman numeral
3 or more elements
Covalent (molecules)
NM & NM
Diatomic Molecules
Acids

26. Molecules Names & Formulas for Inorganic Covalent Compounds

27. Usually need high heat or electricity
Compounds
Stable
Most atoms are bonded in compounds
Separated with chemical reactions
Usually need high heat or electricity

28. Earth’s atmosphere

30. Names of Binary Molecules
First-element name
2nd – end in “ide”
Use prefixes
-Always with 2nd
element
-With 1st element
except mono-
Element with lowest EN goes first
On the Periodic Table – across /down
Prefix
Number
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10

31. Practice: Complete the table in your notes. Write the names
Write the formula

32. Acids
Acids are molecules that are in aqueous solution (_________ in __________) and produce hydrogen ions (H¹⁺)
Typically start with H
Almost act as an ionic compound
Electronegativity Difference:

33. Acids: H + Halogen
Hydro + Halogen (ic) + Acid
HBr
Hydrobromic acid

34. Oxyacids: common acids
Contains oxygen (in a polyatomic ion)
Note the endings of the anion & the acid name
H + nitrate = Nitric Acid
H + sulfate =
H + phosphate =
H + acetate =

35. Inorganic covalent compounds

36. 7 Diatomic Molecules
Heck No Halogens
Named with the element name

37. Common Names for 3 Molecules
Molecular name and formula: common name
Dihydrogen monoxide =
Carbon tetrahydride =
Nitrogen trihydride =

38. Methane: CH₄

39. Ammonia: NH₃

40. Water: H₂0

41. Percent Weight in Earth's Crust
Common elements found in the Earth's rocks.
 Element
 Chemical Symbol
 Percent Weight in Earth's Crust
 Oxygen  O
 46.60
 Silicon
 Si
 27.72
 Aluminum
 Al
 8.13
 Iron
 Fe
 5.00
 Calcium
 Ca
 3.63
 Sodium
 Na
 2.83
 Potassium  K
 2.59
 Magnesium
 Mg
 2.09

42. SiO₂ (metalloid & oxygen)
Important Minerals found in Rocks
Group
Typical Minerals 
Chemistry
Compound Name
Sulfides
Cinnabar
HgS
Galena
PbS
Pyrite
FeS2
Halides
Fluorite
CaF2
Halite
NaCl
Oxides
Corundum
Al2O3
Cuprite
Cu2O
Hematite
Fe2O3
Carbonates (Nitrates and Borates)
Calcite
CaCO3
Dolomite
CaMg(CO3)2
Malachite
Cu2(CO3)(OH)2
Sulfates
Anhydrite
CaSO4
Gypsum
CaSO4 -2(H2O)
Phosphates 
Apatite
Ca5(F,Cl,OH)(PO4 )
Silicates
Quartz
SiO₂ (metalloid & oxygen)