Names and Formulas Ionic Compounds Binary Main Group M & NM Using Polyatomic ions

Names and FormulasIonic Compounds

◦Binary Main Group M & NM ◦Using Polyatomic ions◦Transition metals with variable

charges Covalent Compounds

◦Names & Formulas

NC Essential Standards1.2: Understand the bonding that occurs in

simple compounds in terms of bond type, strength and properties.◦ 1.2.1: compare the relative strength of ionic, covalent,

and metallic bonds◦ 1.2.2: Infer the type of bond and its chemical formula

formed between atoms◦ 1.2.3: Compare inter- and intra- particle forces.◦ 1.2.4: Interpret the name and formula of compounds

using the IUPAC convention◦ 1.2.5: Compare the properties of ionic, covalent,

metallic, and network compounds.

Inorganic Compounds

Ionic

M & NM

With Roman numera

l

3 or more

elements

Covalent (molecules

)

NM & NM

Diatomic Molecule

sAcids

Language of chemistry: Standardize system to represent compounds

Inorganic Compounds

Ionic

Binary - representative metals

Formulas

Names

Transition & post

transition metals

Formulas

Names

Polyatomic ions

Formulas

Names

Covalent (molecul

es)

Binary

Formulas

Names

Diatomic molecules

Formulas

Names

Acids

Formulas

Names

Binary Ionic Compound with Representative Metals Example: Chlorine and

magnesiumRules for formula

◦Metal (cation)1st NM (anion) 2nd

◦Change number of each until charges = 0

◦Subscripts tell the number of atoms/moles

Rules for names:◦Metal 1st – metal’s element name◦NM 2nd – change ending to “-ide”◦No prefixes

Ionic compounds with polyatomic ions

Rules for formulas◦Cation 1st Anion 2nd

◦Use parentheses around the polyatomic ion◦Change number of each ion until charges =

0 ◦Check polyatomic ion: name, formula &

chargeRules for Names

◦Cation 1st Anion 2nd ◦Be careful about the ending (“-ate”, etc.) ◦No prefixes

Sodium + nitrate Ammonium + nitrideFormula

Name:

Using polyatomic ions:

Common Polyatomic IonsNAME FORMULA CHARGE

Nitrate

Acetate

NO₃⁻¹

C₂H₃O₂⁻¹

-1

-1Carbonate

Sulfate

CO₃⁻²

SO₄⁻²

-2

-2

Phosphate PO₄⁻³ -3Hydroxide OH ⁻¹ -1

Ammonium NH⁺¹ +1

Nick the Camel ate a clam for supper in Phoenix

http://www.youtube.com/watch?v=TZgv21FmEzk&list=PLs9HjZz1--dAB_gUIJJOhAu1Rrvaa56J6

Memorizing polyatomic ions

Criss – Cross methodUse the charges (oxidation numbers) to

help determine the number of atoms (moles)

Al⁺³(CO₃⁻²)Check if it the smallest (simplest) ratio

Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻

PO₄³⁻

NO₃¹⁻

Na⁺¹

NH₄⁺¹

K⁺¹

Ca⁺²

Mg⁺²

Writing Formulas (criss –cross method)selected examples from worksheet

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 chlorideTin IV sulfideNote: Check for the smallest (simplest) ratio

Transition metals

Cl¹⁻ CO₃²⁻ OH¹⁻ SO₄²⁻

PO₄³⁻

NO₃¹⁻

Zn⁺²Fe⁺³Co⁺³Fe⁺²

Writing Formulas (criss –cross method)selected examples from worksheet

Sulfide Sulfate Oxide CarbonateMercury II

Iron III

Iron II

Formula Writing Practice – selected examples

Inorganic Compounds

Ionic

M & NM

With Roman numera

l

3 or more

elements

Covalent (molecules

)

NM & NM

Diatomic Molecule

sAcids

Language of chemistry: Standardize system to represent compounds

Inorganic Compounds

Ionic

Binary - representative metals

Formulas

Names

Transition & post

transition metals

Formulas

Names

Polyatomic ions

Formulas

Names

Covalent (molecul

es)

Binary

Formulas

Names

Diatomic molecules

Formulas

Names

Acids

Formulas

Names

Inorganic Covalent Compounds Names & Formulas

Binary

Diatomic

Acids

Note: Organic compounds different naming system

Inorganic Compoun

ds

Ionic

Binary Main

metalsTransition

metalsPolyatomi

c ions

Covalent (molecule

s)

Binary Diatomic Acids

Inorganic covalent compounds

Earth’s atmosphere

Names of Binary MoleculesFirst-element name2nd – 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 + HalogenHydro + Halogen (ic) + AcidHBrHydrobromic acid

Oxyacids: common acidsContains oxygen (in a polyatomic

ion)◦Note the endings of the anion & the acid name

H + nitrate = Nitric AcidH + sulfate = H + phosphate = H + acetate =

7 Diatomic Molecules Heck No Halogens

Named with the element name

Common Names for 3 MoleculesMolecular name and formula: common

nameDihydrogen monoxide =Carbon tetrahydride =Nitrogen trihydride =

Methane: CH₄

Ammonia: NH₃

Water: H₂0