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Ionic Compounds (p. 176 – 180, 203 – 211). Ionic Compounds. M ost of the rocks and minerals that make up Earth’s crust consist of positive and negative ions held together by ionic bonding. An ionic compound is composed of positive and negative ions that are

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Ionic compounds p 176 180 203 211
Ionic Compounds (p. 176 – 180, 203 – 211)


Ionic compounds
Ionic Compounds

  • Most of the rocks and minerals that make up Earth’s crust consist of positive and negative ions held together by ionic bonding.

  • An ionic compound is composed of positive and negative ions that are

    combined so that the numbers of positive and negative charges are equal.

  • Most ionic compounds exist as crystalline solids


Ionic compounds1
Ionic Compounds

  • The chemical formula of an ionic compound merely represents the simplest ratio of the compound’s combined ions that gives electrical neutrality.

  • A formula unit is the simplest

    collection of atoms from which an ionic compound’s formula can be

    established.





Dot diagrams
Dot Diagrams

  • show transfer of e-


Dot diagrams1
Dot Diagrams

show transfer of e-






Ionic Bonding

Ca+2

Ca+2

P -3

Ca+2

P -3


Ionic Bonding

Ca3P2

Calcium phosphide


Ionic nomenclature
Ionic Nomenclature

Common Ion Charges

1+

0

2+

3+

NA

3-

2-

1-

varies


Binary ionic compounds
Binary Ionic compounds

  • Made of two different elements that have formed ions

  • End in -ide


Monatomic ions p 205
Monatomic ions – p. 205

  • Ions formed from a single atom

  • Metals from positive monatomic ions

  • Nonmetals form negative monatomic ions ( nonmetal ions end in –ide, ex. Chlorine becomes the chloride ion)


Variable oxidation s
Variable oxidation #’s

  • Some elements have more than one oxidation number.

  • Groups 3 - 12, tin, lead. The stock system of nomenclature uses roman numerals to indicate the oxidation number.

  • (p.205)


Al 3+ O 2-

Al 2 O 3

(6 +) + (6-) = 0

Formula is Al2O3


Write the formulas for these
Write the formulas for these

  • Lithium sulfide

  • tin (II) oxide

  • tin (IV) oxide

  • Magnesium fluoride

  • Silver chloride

  • Iron (III) phosphide

  • Iron (III) sulfide

  • Potassium iodide


Write the formulas for these1
Write the formulas for these

  • Sodium sulfide

  • Aluminum sulfide

  • Aluminum nitride

  • Copper (II) bromide

  • Iron (II) oxide

  • Lead (II) chloride

  • Mercury (II) sulfide


Compounds with polyatomic ions
Compounds with polyatomic ions

  • Review the list on page 210

  • All are negative except the ammonium ion

  • Most are oxyanions (contain oxygen)

  • When more than one polyatomic ion is in a compound, parentheses must be placed around the polyatomic ion.


Compounds with polyatomic ions1
Compounds with polyatomic ions

  • Copper (II) sulfate

  • calcium nitrate

  • barium nitrate

  • Ammonium chloride

  • ammonium sulfide

  • Lithium nitrate

  • Sodium carbonate

  • Potassium perchlorate


Naming binary ionic compounds
Naming Binary Ionic Compounds

  • Write the name of the cation first

  • Write the root of the anion, end in -ide

  • NaCl = sodium chloride

  • MgBr2 = magnesium bromide

  • KI = potassium iodide

  • BaO = barium oxide


Naming binary ionic compounds1
Naming Binary Ionic Compounds

  • The problem comes with the variable transition metals.

  • You must determine the roman numeral.


CuO

CoCl3

Cu2S

Fe2O3

SnCl2

CrN

Sc3P2

PbO

PbO2


Ionic compounds with polyatomic ions
Ionic Compounds with polyatomic ions

the ending of the polyatomic ion doesn’t change

NaNO3

CaSO4

CuSO3

(NH4)2O

LiCN

Fe(OH)3


(NH4)2CO3

NiPO4

FeCrO4

Pb3(PO4)2

  • See Sample Problems 7-1,7-2,7-3

    (p.207,209,211)

  • h.w. p. 236 # 27, 41,Handout p.2


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