Ionic Compounds and Acid Nomenclature. The force that holds two elements together. - Bonds form to seek the lowest energy state and to meet the maximum.

Ionic Compounds and Acid Nomenclature

The force that holds two elements together.

- Bonds form to seek the lowest energy state and to meet the maximum number of valence electrons.

Chemical Bonds

Lewis Dot Compounds

Ionic Compounds

Ions= atoms or groups of atoms that have a positive or negative charge.

The difference in charge holds the two atoms together

Negative= gaining an electron (-)Positive= losing or donating an electron (+)

1. Have high melting and boiling points2. Forms Solids

3. Made from a metal and non-metal.

Ionic Compounds

If an atom is normally neutral (same # of Protons and Electrons)

AndIt donates one electron away it is no longer neutral but

positive.

So the Sodium becomes Positive known as a CationChlorine becomes Negative known as a Anion

Cation wrote as Na⁺Anion wrote as Cl¯

Cation=Metals and PositiveAnions=Non-Metals and Negative

MONOATOMIC IONS- ONLY HAVE ONE ATOM AND HAVE A SPECIFIC (+) OR (-) CHARGE.

OXIDATION NUMBER OR IONIC CHARGE- CHARGE OF A MONOATOMIC ION AND IS EQUAL TO THE NUMBER OF ELECTRONS TRANSFERRED FROM OR TO AN ATOM.

Ions

Oxidation NumbersOxidation numbers are

written as superscripts to indicate charge but are not

included in the formula.Ex: Li1+ or O2-

NAMING MONOATOMIC IONS

CationsName the element and add the word Ion.

Example: Na⁺= Sodium Ion

AnionsDrop the ending off the element name and adding

“ide”Example: O²¯= Oxide

Naming Transition Metal IonsTransition Metals have more than one Ionic

charge.Example: Iron can form two Cations

Fe²⁺ or Fe³⁺

Fe²⁺= Iron (II) ionFe³⁺= Iron (III) ion

Practice

Lithium=Fluorine=Oxygen=Carbon=Barium=Cesium=Au2+=

Gold (III) Ion =

Binary Ionic Compounds

Binary Ionic Compound- made of two ions/elements;

Naming Binary Ionic CompoundsThe cation keeps the normal name from

periodic table and the Anion receives an –ide ending.

Example:NaCl= Sodium ChlorideKI= Potassium Iodide

Writing a formula for Ionic Compounds

Binary Ionic Compounds = cation + anion1. Determine the oxidation number of

each cation and anion.2. The net charge of the compound must

equal “0”Example: Sodium Chloride

Na⁺ and Cl¯+1 and -1 =0

Formula = NaCl

Naming Simple Binary Ionic Compounds

Example 2Calcium Chloride

Ca²⁺ and Cl¯

2+ and -1 = +1Add one more Cl to = 0

Formula= CaCl₂

Naming Simple Binary Ionic Compounds

Practice!!!Potassium Iodide=

Calcium Phosphide=Magnesium Chloride=Magnesium Oxide=

Li₂O=KBr=

Metals Always Placed Before Non-Metals!!!!!!

Polyatomic Ions

Polyatomic Ions-Tightly bound group of atoms that behave as a unit and carry a charge.

Ex. SO₃²¯, ClO₂⁺

Names for Polyatomic Ions

Most of the names end with –ite or –ate but not all.

The –ite ending indicates one less oxygen than the

-ate ending.

But –ite and –ate does not determine the actual number of oxygen atoms.

Cations and Polyatomic Ions

When adding Cations (metals) to polyatomic ions add the basic element

name to the Polyatomic Ion.Example: CaSO₄ = Calcium Sulfate

Writing FormulasThe charge for the whole compound must equal “0”.

Example: Magnesium Chlorate

Writing Formulas with Cations and Polyatomic Ions

The charge for the whole compound must equal “0”.Example: Magnesium Chlorate

Magnesium= +2 and Chlorate = -1We must have 2 chlorate for the

compound to equal Zero.Formula= Mg(ClO₃)₂

When adding an extra Polyatomic Ion Use Parenthesis and add desired amount behind.

Ionic Compounds with Transition Metals

Naming1. Recognize the metal is a transition metal.

FeCl₂Fe = Iron a transition metal unknown charge

2. Use the Non-metal to determine the charge of the transition metal.

Chlorine charge = -1 x 2 = -23. The charge of the whole compound must equal zero.

Iron must have a +2 Charge

Name of FeCl₂ = Iron (II) Chloride

Naming AcidRules

Anion Ends In –ideHydro- stem-ic Acid

Example with Chlorine = Hydrochloric AcidAnion Ends In –ite

Stem of Anion –ous AcidExample with Sulfite= Sulfurous Acid

Anion Ends In –ateStem of Anion-ic Acid

Example with Nitrate= Nitric Acid

Acids

Acids- compounds that produce hydrogen ions when dissolved in water

Acids to KnowHydrochloric Acid=HCl

Sulfuric Acid= H₂SO₄Nitric Acid= HNO₃

Acetic Acid= HC₂H₃O₂Phosphoric Acid= H₃PO₄

Carbonic Acid= H₂CO₃

END OF Unit 4!!!

Naming Covalent/Molecular Compounds

Covalent Compounds are made of two non-metals.

Pre-fixes are used to indicate the number of atoms in each compound.

Naming Covalent/Molecular Compounds

Rules1. The first element name is given followed by

the second with an “ide” ending.2. The first element gets a prefix if more than

one.3. The second element always gets a prefix.

ExamplesNO=Nitrogen MonoxideN₂O= Dinitrogen MonoxideN₂O₄=Dinitrogen TetraOxide

Naming Covalent/Molecular Compounds

FormulaCopper(II) Sulfate = CuS

Roman Numeral = Charge of your MetalUse the Roman Numeral to figure out the

charge on your non-metal.

Copper (II) equals + 2 Charge

The total charge on the whole compound must still equal 0.

Molecular Compounds

Molecular Compounds or when two atoms of different elements create bonds.

Examples: CO₂, H₂O, PCL₃

Characteristics:1. Low melting points and Low boiling points

2. Form liquids or gases.3. Made from two or more non-metals

MOLECULE-MADE UP OF TWO OR MORE ATOMS OF THE

SAME ELEMENT.EXAMPLES: 0₂ (OXYGEN YOU BREATHE)

O₃ (OZONE)Molecules and Bonds

Ionic Bonds Vs. Covalent Bonds

Ionic Bonds Covalent Bonds

Bonded together by the attraction of opposite charges

(+ and -)

Bonded together by the sharing of electrons

Electrons are donated/transferred and taken giving one atom a (+) charge and the other a (-) charge.

Electrons are shared between both atoms charges remain the same.

Polar Molecule Non-Polar Molecule

Made of a metal and non-metal Made up of two non-metals

Weaker Bonds Stronger Bonds