Objective: To interpret (correctly write) formulas and names for compounds – using IUPAC convention

Warm-up: review names & formulasReview: Binary Ionic CompoundsMore Complex Ionic Compounds

With Polyatomic IonsWith Transition Metals

Covalent Compounds

Agenda: 3/17 – 3rd block

Homework: Re-write in paragraph form – notes pages 1 and 3. Add additional information learned in practice.

Formula Type of Bond and Compound

Name

MgCl₂

SO₂

PCl₃

AlBr₃

K₃N

BrO₃

H₂O

Warm-up: Review names & formulas

Inorganic Compound

s

Ionic

M & NM

With Roman

numeral

3 or more

elements

Covalent

(molecules)

NM & NM

Diatomic Molecules

Acids

Language of chemistry: Standardize system to represent compounds

Ionic CompoundsMetals lose valence electrons

Non-metals gain 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

Ionic Bonding: Transfer of valence electrons

Cl Ca Cl

= Ca Cl

Electron Dot Diagram (Lewis)

Some Ionic Compounds are more complex

Include polyatomic ions

Ionic compounds: Found in minerals and rocks

Barite = BaSO₄Used to make paper & glassSource of barium used For x-rays of the digestivesystem

Ionic compounds: Found in minerals and rocks

Gypsum = CaSO₄· 2H₂O

Used for plaster for walls, ceilings, sculptures

Ionic compounds: Found in minerals and rocks

Calcite = CaCO₃Used in paint,Antacids, calciumSupplement for food

Ionic compound with polyatomic ions

Sodium acetateIn Heat packs

Calcium sulfate in casts

Barium sulfate to absorb x-rays

Acetate uses

Sodium hydrogen carbonate(old name: sodium bicarbonate)

Medical: used in emergency situations to correct pH of blood

Baking soda: to make cakes rise

Bleach

Dentistry: Clean and disinfectRoot canals

Rocket fuels:Source of oxygen

POLYATOMIC IONS

Ions with -1 chargeperbromate 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 chargeammonium ion

NH4+1

Examine the names & formulas: What is the pattern? Do they end in “–ide?”

Compounds vs. Polyatomic Ions

Polyatomic ions that you must know: NAME FORMULA CHARGE

Nitrate

Acetate

Carbonate

Sulfate

Phosphate

Hydroxide

Ammonium

Sodium + nitrate Calcium + nitrate

Formula

Name:

Using polyatomic ions:

Cl¹⁻ CO₃²⁻

OH SO₄²⁻

PO₄³⁻

NO₃¹⁻

Na¹⁺

NH₄¹⁺

Zn²⁺

Co³⁺

Writing Formulas (criss –cross method)

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=

Ionic Compounds with Transition Metals

Examples Iron II oxideIron III oxide

Write the formulas for:Copper I oxideCobalt III chlorideNickel II sulfide

Transition metals

Sulfide Sulfate Oxide Carbonate

Mercury II

Iron III

Iron II

Formula Writing Practice

Many transition and post transition metals have multiple oxidation numbers (charges)

Ni: oxidation numbers of _____ & _____ Fe: Find other examples:

Write formulas Write names

Practice: Writing Binary Formulas

Inorganic Compounds

Ionic

M & NM

With Roman

numeral

3 or more

elements

Covalent (molecules

)

NM & NM

Diatomic Molecule

sAcids

Language of chemistry: Standardize system to represent compounds

Covalent CompoundsMolecules

Names & Formulas for Inorganic Covalent Compounds

Compounds

-Stable

-Most atoms are bonded in compounds

-Separated with chemical reactions

-Usually need high heat or electricity

Earth’s atmosphere

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 firstOn the Periodic Table – across /down

Prefix Numbermono- 1

di- 2tri- 3

tetra- 4penta- 5hexa- 6hepta- 7octa- 8nona- 9deca- 10

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

Write the formula

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:

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

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 =

Inorganic covalent compounds

7 Diatomic Molecules

Heck No Halogens

Named with the element name

Common Names for 3 MoleculesMolecular name and formula: common

name Dihydrogen monoxide = Carbon tetrahydride = Nitrogen trihydride =

Methane: CH₄

Ammonia: NH₃

Water: H₂0

 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

Common elements found in the Earth's rocks.

Group Typical Minerals  Chemistry Compound Name

SulfidesCinnabar HgS

Galena PbSPyrite FeS2

HalidesFluorite CaF2

Halite NaCl

OxidesCorundum Al2O3

Cuprite Cu2OHematite Fe2O3

Carbonates(Nitrates and Borates)

Calcite CaCO3

Dolomite CaMg(CO3)2

Malachite Cu2(CO3)(OH)2

SulfatesAnhydrite CaSO4

Gypsum CaSO4 -2(H2O)

Phosphates Apatite Ca5(F,Cl,OH)(PO4 )

Silicates Quartz SiO₂ (metalloid & oxygen)

Important Minerals found in Rocks