Standards: C.7.A name ionic compounds containing main group transition

metals, covalent compounds, acids, and bases, using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules

C.7.B write the chemical formulas of common polyatomic ions, ionic compounds containing main group or transition metals, covalent compounds, acids

C.7.C construct electron dot formulas to illustrate ionic and covalent bonds

C.7.D describe the nature of metallic bonding and apply the theory to explain metallic properties such as thermal and electrical

conductivity, malleability, and ductility C.7.E predict molecular structure for molecules with linear, trigonal

planar, or tetrahedral electron pair geometries using Valence ShellElectron Pair Repulsion (VSEPR) theory

Naming Chemical Compounds… slide 4Naming Acids and Bases… slide 11Writing Chemical Formulas… slide 16Chemical Bonding… slide 22Molecular Geometry, VSEPR Theory… slide 31

C.7.A name ionic compounds containing main group transition metals, covalent compounds, using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules.

Types of CompoundsThere are three main types of compounds

when working on Naming Compounds.Metal Binary Compounds (Ionic) – Contain a

metal and a non-metal. They form an ionic bond.

Non-Metal Binary Compounds (Molecular)– Contain two non-metals. They form a covalent bond.

Ternary Compounds (Polyatomic)– Contain polyatomic ions. The formula will have three or more elements in it.

Metal Binary Compounds (Ionic)Name the first element. (This will always be

the metal.)Replace the ending on the second element

with an “ide” ending. ( This element will be the non-metal)

Example:NaCl sodium and chlorine becomes

sodium chlorideMgS magnesium and sulfur becomes

magnesium sulfide

Naming Compounds with a Transition metalWhen some atoms can have more than one possible

charge, you name the charge on the atom.The following elements must have a roman numeral: Cr-Cu, Au, Hg, Sn, & PbCopper +1 and +2 Iron +2 and +3 Cu +1 is copper (I) Fe +2 is iron (II) Cu +2 is copper (II) Fe +3 is iron (III) CuCl is copper (I) chloride FeCl2 is iron (II) chloride CuCl2 is copper (II) chloride FeCl3 is iron (III) chloride

Non-Metal Binary Compounds (Molecular)Name the first elementReplace the ending on the second element with

“ide”Use Prefixes to indicate the number of atoms in

the formula.*Exception: A prefix is not required when the

first element only has 1 atom.Ex: CO2 carbon and oxygen is carbon dioxideN2O nitrogen and oxygen is dinitrogen

monoxide

Pre-fixes1 atom = mono2 atoms = di3 atoms = tri4 atoms = tetra5 atoms = penta6 atoms = hexa7 atoms = hepta8 atoms = octa9 atoms = nona10 atoms = deca

Ternary Compounds (Polyatomic)Name the first part of the compound.

Element or polyatomic ion.Name the second part of the compound.

Element or polyatomic ion.Example:MgSO4 NH4OHmagnesium sulfate ammonium

hydroxideK3PO4potassium phosphate

C.7.A name, acids using International Union of Pure and Applied Chemistry (IUPAC) nomenclature rules

Naming Acids without OxygenAcids without Oxygen are named with the

prefix “hydro” and end in “ic”Examples:HCl hydrochloric acidHF hydrofluoric acidHBr hydrobromic acid

Naming Acids with OxygenAcids with oxygen have several forms. The “ic” or regular ending for an acid comes

from the polyatomic ion with the “ate” ending. This gives the regular count for the oxygen for this type of acid.

Example:H2SO4SO4 is sulfate so this acid is called sulfuric

acid

Once you know the “ic” ending you count the number of oxygen in the other forms to find the name for the acid. (REMEMBER: The regular “ic” form comes from the polyatomic ion that ends with “ate”)

Two less oxygen hypo ________ ous acidOne less oxygen ________ ous acid Regular “ic” form ________ ic acidOne more oxygen per ________ ic acid

The other names for the acids will come from the count based from the “regular acid name”

H2SO4 -ate ending so it is sulfuric acid H2SO3 -ite ending so it is sulfurous acidH2SO2 two less oxygen will have the prefix

hypo and the –ous ending. hyposulfurous acid.

H2SO5 one more oxygen will have a prefix per and the regular -ic ending. persulfuric acid

C.7.B write the chemical formulas of common polyatomic ions, ionic compounds containing main group or transition metals, covalent compounds, acids

Writing Formulas: Ionic CompoundsWrite chemical symbol for each part of the

compound.Write the charge (oxidation #) for the element.

Do the charges add together and equal zero?

Yes, Stop this is the formula. The number of electrons given away is the same as what is being taken by the second atom.

No, Cross the absolute value of the charge to the opposite element as a subscript. Multiply the new subscript by the charge and see if the new values will add together and equal zero. If yes, Stop you have the formula

potassium bromide Formula

K +1 Br -1 +1 + -1 = 0 Yes KBr

magnesium chloride Mg +2 Cl -1 +2 + -1 = +1 No Mg 1 Cl 2 Mg (1 x +2)= +2 Cl (2

x -1)= -2 Yes MgCl2

Transition ElementsSame rules as normal ionic compounds. The

charge for the transition metal will come from the name of the compound.

iron (III) chlorideFe +3 Cl -1 +3 + -1 = +2 NoFe1 Cl 3 Fe (1 x +3) +3 Cl (3 x -1) -3

Yes FeCl3

Molecular CompoundsUse the prefix to determine the subscript of

each element in the formula.NO PREFIX on the first element indicates a

subscript of 1Write the correct formula using the correct

symbol and subscript for each element.Ex: carbon dixoide CO2

Polyatomic IonsThe rules for polyatomic ions will be the

same as ionic compounds. *Polyatomic ions must be placed in parenthesis if the

subscript is larger than 1 when criss-crossing.magnesium sulfate Mg +2 SO4 -2 MgSO4iron (III) phosphateFe +3 PO4 -3 FePO4

sodium hydroxideNa +1 OH -1 NaOH

calcium hydroxideCa +2 OH -1 Ca(OH)2

aluminum phosphate

Write the symbol and charge (oxidation #) of each element. If the charges do not add up to zero, criss-cross the

oxidation #.Ex: hydrosulfuric acid

H+1 S-2 = H2S

Acids without Oxygen

Acids with OxygenWrite the symbol and the charge for the polyatomic ion

(oxyanion). If the charges do not add up to zero, criss-cross the

oxidation numbers. 1 more oxygen per ____________ic MEMORIZED(-ate) ____________ic 1 less oxygen (-ite) ____________ous 2 less oxygen hypo___________ous

H2SO3 sulfurous acid

C.7.C construct electron dot formulas to illustrate ionic and covalent bonds

There are three main types of chemical bonding. ionic, covalent, and metallic.

Ionic bonding occurs when there is a transfer of electrons.

Covalent bonding occurs when atoms share electrons.

Metallic bonding consist of the attraction of free floating valance electrons for positively charged metal ions.

Electro negativities are used to determine what type of bond is formed when atoms come together in a chemical reaction.

To find the type of bond find the difference in the electronegativities.

If the difference is greater than 1.67 an ionic bond is formed.

If the difference is less than 1.67 a covalent bond is formed.

All atoms want to obtain eight electrons in the valence energy level. To do so they will give, take, or share electrons.

Rules for Ionic BondsThe element with the fewest atoms goes in

the center.The other atoms go around the central atom.Show the transfer of the electrons with a

positive for the atom that lost the electrons and a negative for the atoms that gain the electrons.

NaCl sodium chloride sodium: (1.01) chlorine:

(2.83)

Na: 1s22s22p63s1 Cl: 1s22s22p63s23p5

Sodium transfers the 3s1 to chlorine to complete the 3p energy level.

The electronegativity difference is 1.72 An ionic bond is formed.

Rules for showing Covalent BondsThe element with the fewest atoms goes in

the center.The other elements go around the central

atom.A bonding pair can only form where there is

an unpaired electron.Shared pairs or bonding pairs are shown with

a dash. One dash equals two electrons.

AsI3 arsenic triiodidearsenic (2.20) iodine (2.21)

As: 1s22s22p63s23p64s23d104p3

I: 1s22s22p63s23p64s23d104p65s24d105p64d105p5

The electronegativity difference is .01A covalent bond is formed. The atoms share

the electrons.

C.7.E predict molecular structure for molecules with linear, trigonal planar, or tetrahedral electron pair geometries using Valence Shell Electron Pair Repulsion (VSEPR) theory

Molecular GeometryThe shape that a covalently bonded substance

will take is referred to as its Molecular Geometry.

The shape is determined by the central atom, and the number of shared and unshared electron pairs around the atom.

Electron pairs around the central atom will spread out as far as possible to minimize the repulsive forces.

This gives bond angles depending on the shape.

Total number of electron pairs.

Number of shared pairs

Number of unshared

pairs

Shape Bond Angle

2 2 0 Linear 180 0

Total number of electron pairs.

Number of shared pairs

Number of unshared pairs

Shape Bond Angle

3 3 0TrigonalPlanar 120 0

Total number of electron pairs.

Number of shared pairs

Number of unshared pairs

ShapeBond Angle

4 4 0 Tetrahedral

109.5 0

Total number of electron pairs.

Number of shared pairs

Number of unshared pairs

Shape Bond Angle

4 3 1TrigonalPyramid

al107.3 0

Total number of electron pairs.

Number of shared pairs

Number of unshared pairs

Shape Bond Angle

4 2 2 Bent 104.5 0

LinearTrigonal Planar

Tetrahedral

Trigonal Pyramidal Bent