Types of Compounds

Metal Binary Compounds – Metal and Non-Metal, forms an Ionic Bond.

Non-Metal Binary Compounds – two Non-Metals, forms a Covalent Bond.

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

Metal Binary Compounds

Name the first element- a metal.Replace the ending on second element (non-

metal) with an “-ide” ending.

Examples:

NaCl Sodium + Chlorine = Sodium Chloride

MgS Magnesium + Sulfur = Magnesium Sulfide

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

charge, you name the charge on the atom.Copper is +1 or +2 Iron is +2 or +3 Cu +1 is Copper I Fe +2 is Iron II Cu +2 is Copper II Fe +3 is Iron III

CuCl = Copper (I) Chloride FeCl2 = Iron (II) ChlorideCuCl2 = Copper (II) Chloride FeCl3 = Iron (III) Chloride

Non-Metal Binary Compounds

Name the first elementReplace the ending on the second element with “-ide”Use prefixes for the number of atoms in the formula.

CO2 is Carbon + Oxygen = Monocarbon DioxideN2O is Nitrogen + Oxygen = Dinitrogen MonoxideH2O is Hydrogen + Oxygen = Dihydrogen Monoxide

Prefixes1 atom = Mono- 6 atoms = Hex-2 atoms = Di- 7 atoms = Hept-3 atoms = Tri- 8 atoms = Oct-4 atoms = Tetra- 9 atoms = Non-5 atoms = Pent- 10 atoms = Deca-

Ternary CompoundsCompounds with Polyatomic IonsName the first part of the compound- an

element or polyatomic ion.Name the second part of the compound- an

element or polyatomic ion. Examples:

MgSO4 NH4OH Magnesium Sulfate Ammonium Hydroxide

K3PO4

Potassium Phosphate

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 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 KBrMagnesium Chloride Mg +2 Cl -1

(+2) + (-1) = +1 No Mg 1 Cl 2

1 (+2) + 2 (-1) = 0 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

1 (+3) + 3 (-1) = 0 Yes FeCl3

Polyatomic IonsThe rules for polyatomic ions will be the same as

ionic compounds. Place the polyatomic ion in parenthesis.

Keep the parenthesis at the end of the process if you have a number greater than one outside of the parenthesis. If you did not cross a number or if you only crossed a one do not keep the parenthesis.

Magnesium Sulfate Mg +2 (SO4) -2 Yes MgSO4Iron III PhosphateFe +3 (PO4) -3 Yes FePO4

Sodium HydroxideNa +1 (OH) -1 Yes NaOH

Do not keep the parenthesis because there is no number crossed.

Calcium HydroxideCa +2 (OH) -1 Ca 1 (OH)2

1 (+2) + 2 (-1) = 0 Yes Ca(OH)2

Keep the parenthesis because there is a number greater than one

outside the parenthesis

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.

Electronegativities 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 electro negativities.

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.

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 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.

AsI3 Arsenic TriiodideArsenic (2.20) Iodine (2.21)

As: 1s22s22p63s23p64s23d104p3

I: 1s22s22p63s23p64s23d104p65s24d105p5

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

the electrons.

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.

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.

Linear moleculeTotal number of electron pairs.

Number of shared pairs

Number of unshared

pairs

Shape Bond Angle

2 2 0 Linear 180 0

Trigonal planar moleculeTotal number of electron pairs.

Number of shared pairs

Number of unshared pairs

Shape Bond Angle

3 3 0TrigonalPlanar 120 0

Tetrahedral moleculeTotal number of electron pairs.

Number of shared pairs

Number of unshared pairs

ShapeBond Angle

4 4 0 Tetrahedral

109.5 0

Trigonal PyramidalTotal number of electron pairs.

Number of shared pairs

Number of unshared pairs

Shape Bond Angle

4 3 1TrigonalPyramid

al107.3 0

Bent moleculeTotal 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

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 is Hydrochloric AcidHF is Hydrofluoric AcidHBr is Hydrobromic Acid

Naming Acids with OxygenSome acids with oxygen have several forms

and use suffixes with “-ic” and “-ous” endings. 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, count the number of oxygens 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 a prefix

and “-ous”ending. Hyposulfurous Acid.H2SO5 one more oxygen will have a prefix

“Per” and the regular “-ic” ending. Persulfuric Acid