Nomenclature

Chemical Names&

Formulas

Introduction to Chemical Bonding

Two types of Bonding _____________________ - transfer of electrons

_____________________ - sharing of electrons

Bonding takes place at the __________ energy level, ____ and ____ sublevels.

If there are less than half the electrons between the s and p sublevels, the atom will _________ the electrons.

If there are half or more electrons between the s and p sublevels, the atom will __________ electrons.

Know the trends on the periodic table for how many electrons will be gained or lost.

Ionic BondingBecause there is a ____________ of

electrons, elements will lose or gain electrons.

If an element loses or gains electrons, it will then become a charged particle - _________. Positive ion - ________________ Negative ion - _______________

CationsSubstance that has ________

electrons. The charge is equal to the number of

electrons that are transferred.Ca2+ - calcium that has transferred

two electrons to another substance (anion).

Mg2+ - magnesium that has transferred two electrons to another substance (anion).

AnionSubstance that has ________ electrons.

The charge is equal to the number of

electrons that are transferred.F1- - fluorine that has accepted one

electron from another substance (cation).

O2- - oxygen that has accepted two electrons from another substance (cation).

Ionic Size

______________ is a charged particle.All atoms are _________________ – the

protons and electrons are equal to one another.

The only way an atom becomes a charged particle is if it _______________ or ________________ electrons.

Ionic Size

_______________ – positively charged ions Lost electrons – more _________________ than

______________________ ____________________ tend to lose electrons

________________ – negatively charged ions Gained electrons – more _________________

than ______________________ _______________________ tend to gain

electrons

Ionic Size - Cations

Cations are ___________ than their parent atoms.

The outermost electron is removed and repulsions are reduced.

Ionic Size - Anions

Anions are ___________ than their parent atoms.

Electrons are added and repulsions are increased.

Ions _____________ in size as you go down a column. Due to

increasing value of the energy levels.

Ionic BondingIonic bonding is the _______________ or _______________ of electrons.

Metals are _______________.Nonmetals are _____________.Hence, ionic bonding will occur between ___________ and _________________.

Oxidation NumbersPossible _______________ on an element.

Any single element, by itself, has a charge of ____________.

An element takes on a charge when put with other elements.

Basic Rules of Oxidation NumbersGroup 1 elements are always 1+.Group 2 elements are always 2+.Group 3 elements are always 3+Group 17 elements will be 1-.Group 16 elements will be 2-.Group 15 elements will be 3-.

Other Elements

Ag = 1+

Zn = 2+ Cd = 2+

Al = 3+ Ga = 3+ In = 3+

Other Elements with Multiple Charges

Cr2+ and Cr3+

Fe2+ and Fe3+

Co2+ and Co3+

Ni2+ and Ni3+

Cu+ and Cu2+

Sn2+ and Sn4+

Pb2+ and Pb4+

Writing Formulas from Ions

The total overall charge of a compound is ___________________

Use subscripts to balance the charge to zero.

Ca2+ and S2-

CaS

Na+ andCl-

NaCl

Ba2+ andN3-

Ba3N2

Writing Ions from Compounds

Go with what you know.

MgCl2

Mg2+ and Cl-

CuBr2

Cu2+ and Br-

FeCl3

Fe3+ and Cl-

Polyatomic IonsMany atomed charged particle

that acts as a single unit.Polyatomic ions have specific

names. Use the names.Common polyatomic ions include:

Nitrate ____________ Sulfate ____________ Phosphate ____________ Carbonate ____________ Hydroxide ____________ Chlorate ____________

Other Polyatomic Ions

Ammonium NH4+

Permanganate MnO4-

Bromate BrO3-

Iodate IO3-

Acetate C2H3O2-

Chromate CrO42-

Dichromate Cr2O72-

Changing the Oxygen

Per - _____ - ate _____ -

ate _____ - iteHypo - _____ - ite _____ -

ide

Move down – lose 1 oxygen each step

Move up – gain 1 oxygen each step

Ba2+ andSO42-

BaSO4

Na+ andClO3-

NaClO3

Fe2+andCO32-

FeCO3

KNO3

K+ and NO3-

CoSO4

Co2+ and SO42-

LiClO3

Li+ and ClO3-

More than one of the Polyatomic Ion Needed to

Balance the Charge

If more than one of the polyatomic ions is needed to balance the charge, you must use parentheses ( ) around the ion.

Ba(NO3)2

Ba2+ and NO3-

Mg2+ and ClO3-

Mg(ClO3)2

Fe3+and SO42-

Fe2(SO4)3

Co3+ and NO3-

Co(NO3)2

Naming Ionic Compounds

Binary Ionic Compounds - Types 1 & 2 A compound that contains a positive ion (______________) and a negative ion (_______________).

Bi- means two Positive ion is written ___________, negative ion is written ______________ in a chemical formula.

Type 1 - Binary Ionic Compound

The cation of a Type 1 has only ________ possible charge.

Name the first element (cation) as is.

Name the second element (anion) as is with an ending of “-ide”.

Example: CaCl2

Calcium chloride

More Examples:

NaBr - ________________MgO - ________________KBr - ________________BaS - ________________

Type 2 - Binary Ionic CompoundsThe cation has multiple charges -

copper can have a charge of 1+ or 2+.

Determine which charge is being used. Use the anion as the guide.

Name the element as is.Use a Roman numeral to indicate

the charge being used.

Name the anion as is, using an ending of “-ide” as with Type 1 compounds.

Example: CuCl2

Copper (II) chloride

MnO2 - Manganese (IV) oxide

NiO - Nickel (II) oxide

Naming Type 1 & 2 with Polyatomic Ions

Form compounds called ______________ compounds - compound that contains atoms of three different elements.

______________________ - many atomed charged particle acting as a single unit. poly - many atomic - atom ion - charged particle

Type 1 & 2 Compounds with Polyatomic Ions

Name the cation using the rules for Type 1 or Type 2 compounds.

Name the polyatomic ion as is - use the name on the chart.

Examples: NaNO3 - ______________ BaSO4 - ______________

Name these:LiOH - ________________Mg(NO3)2 - ________________

CrCl3 - ________________

Al2O3 - ________________

CoBr2 - ________________

Fe2O3 - ________________

Covalent BondingCovalent bonding involves the

________________ of electrons between substances.

________________ - smallest neutral unit of a substance that still has the properties of the substance.

________________ - shows the kinds of numbers of atoms present in a molecule of a compound.

Occurs between ________________ and ________________.

Because these are molecules and are covalently bonded, ions are ________________ - there is no transferring of electrons to form ions.

Prefixes are used in naming nonmetal-nonmetal compounds.

Prefixesmono - 1di- - 2tri- - 3tetra- - 4penta- - 5hexa- - 6hepta- - 7octa- - 8nona- - 9deca- - 10

Prefixes:Only used for nonmetal-nonmetal compounds.

Mono- is never used on the first element.

Second element always has a prefix.

Naming Molecular CompoundsName the first element as is. If

there is more than one of the first element, you must use a prefix.

Name the second element with a prefix to indicate how many atoms there are and add the ending “-ide”.

Example: CO2 - carbon dioxide

Name these:N2O- ____________________

PCl3- ____________________

SF6 - ____________________

P4O6 - ____________________

SO2 - ____________________

NO3 - ____________________

SO4 - ____________________

Naming AcidsWhen dissolved in water, certain

molecules produce ____________________ - H+.

These substances are called ____________________.

An acid can be viewed as a molecule with one or more H+ ions attached to an anion.

The rules for naming acids depend on whether the anion contains ____________________.

Naming AcidsIdentify the compound as being

an acid - the first element is hydrogen (two exceptions are H2O and H2O2)

Find the anion on the chart.Name the anion.Following across to the name of

the acid.Name the acid.

Naming Acids

If you move up the chart, you ____________________ oxygen.

If you move down the chart, you ____________________ an oxygen.

Start with what you know - usually the -ate group.

Examples:HCl

The chloride ion (anion) is a single element and ends in “-ide”.

It is at the bottom of the chart.

Move across and the name of this acid is hydrochloric acid.

H3PO4

The anion is phosphate. Move across to the acids and the name of this acid is phosphoric acid.

H2SO4

The anion is sulfate. Move across to the acids and the name of this acid is sulfuric acid.

HClO2

Identified as an acid. The anion is ClO2

1-, which is one less oxygen than chlorate, ClO3

1-. Lose an oxygen, move down the chart.

Move down the chart and the name of the anion is chlorite.

Move across to the acid and the name of this acid is chlorous acid.

Name these:HNO3 - ________________

H2CO3 - ________________

H2SO3 - ________________

HNO2 - ________________

HC2H3O2- ________________

HClO4 - ________________

Name these Compounds

LiOH ___________________CuBr2 ___________________

H2S ___________________

Na2SO3 ___________________KI ___________________CCl4 ___________________

Na2SO4

Cu(ClO4)2

N2O5

MgI2

Sr(NO2)2

HgCl2

CaCO3

PbC2O4

Cr2(Cr2O7)3

Iron (III) chromate

Potassium hydroxide

Triphosphorus hexaoxide

Potassium thiocyanate

Silver nitrate

Aluminum sulfite

Carbon disulfide

Ammonium sulfate

Nickel (II) chromate

Xenon tetraoxide

Phosphorus trihydride

Potassium carbonate

Disulfur dichloride

Lithium oxide

Cobalt (III) hydroxide

Sodium hydroxide

Dinitrogen monoxide

Ammonium nitrate