GPS

SC1. Students will analyze the nature of matter and its classifications.

c. Predict formulas for stable ionic compounds (binary and tertiary) based on balance of charges.

d. Use IUPAC nomenclature for both chemical names and formulas of:

• Ionic compounds• Covalent compounds• Acidic compounds

Vocabulary

• Ion Oxidation number

• Cation Ionic compound

• Anion Covalent molecule

• Polyatomic ions Transition metals

• Binary compounds

• Monatomic ions

Binary Ionic Compounds

YES NO

Is compound binary?

YES NO

Is the 1st elementa METAL ? 2nd

element a nonmetal.

YES NO

Is it a group Arepresentative

METAL ? (gp. 1 or 2)

•Name both ions:•Name the cations 1st, •Anion 2nd

Change the ending of the anion to ~ide

EX: NaCl =

Sodium ChlorideRETURN TO BEGINNING

Examples

1. CaCl2

2. BaS

3. AlCl3

4. KI

5. MgO

YES NO

Is it a group Btransition

METAL ? (gp. 3-12) or heavy metal (Pb, Sn, etc.)

ROMAN NUMERALS???

•Transition metals can exist in more than one oxidation state (have more than 1 charge)

To determine the charge on the ion in question:1. Determine the charge of the ANION (look on periodic table)2. Look at the number of anions present (written down below)3. Determine the TOTAL negative charge4. Look at the number of cations present5. Divide TOTAL negative charge by number of cations present6. This is the Roman numeral you place in ( ) after the cation name

Show me an example

BACK TO NAME

To determine the charge on the ion in question:1. Determine the charge of the ANION (look on periodic table)2. Look at the number of anions present (written down below)3. Determine the TOTAL negative charge4. Look at the number of cations present5. Divide TOTAL negative charge by number of cations present6. This is the Roman numeral you place in ( ) after the cation name

Fe2O3

1. Oxygen’s charge is –2 2. There are 3 anions present 3. Total –charge is -64. There are 2 cations present5. 6/2= 3 6. Therefore each Fe caion must have a +3 charge

Iron (III)BACK TO NAME

•Name both ions•Use proper roman numeral in ( )with the cation•Change the ending of the anion to ~ide

EX: FeCl2 =

Iron (II) ChlorideRETURN TO BEGINNING

How do I figure out the

roman numeral?

Example

• 1) CuS

• 2) PbBr4

• 3) Pb3N2

• 4) Fe2O3

• 5) FeI2

• 6) Sn3P4

YES NO

Is it a Polyatomic Ion?

•Name cation •If anion is: •single element change the ending of the anion to ~ide•also polyatomic write name of anion

EX: NH4Cl = Ammonium ChlorideEX: NH4NO3=Ammonium Nitrate

RETURN TO BEGINNING

•Name the cation•Name the anion

*will end with ~ate or ~ite* (hydroxide is exception)

EX: LiCO3 = Lithium Carbonate

RETURN TO BEGINNING

Practice

1. NH4Cl _____________________________

2. Ni2CO3 ____________________________

3. Cr(OH)3 ___________________________

4. CoSO4 ___________________________

5. NH4 NO3 __________________________

6. (NH4)2 CO3 ________________________

7. Au2 SO4 _________________________

Naming Ionic Compounds

• Common Anions:– Oxygen= oxide– Sulfur= sulfide– Phosphorus= phosphide– Nitrogen= nitride

Writing Ionic Compounds/ formulas

• To write formula: • Always write metal 1st; nonmetal 2nd • Write symbols w/charges• Drop charges• Cross superscripts to other

subscripts to write completed formula.

• Aluminum sulfide

• magnesium sulfide

• sodium sulfide

– Al3+ + S

– Mg2+ + S

– Na+ + S2

Al2S3

MgS

Na2S

C. Ionic Nomenclature

Ionic Cpmds w/ Polyatomic ions (PA)

• PA ions: ions made up of more than one atom. The charge assigned to a PA ion represents the charge on the entire group. Ex.) NH4

+1 = +1 charge on the entire ammonium ion

• To determine the name of cmpds w/ PA ions, follow the same rule as naming monatomic ionic compounds.

– cation= name of cation or polyatomic cation– anion= name of polyatomic anion ( do not change ending)– balance the charges of the cation and anion– Ex.) sodium & nitrate = Na+1 + NO3

-1 → NaNO3

• If there is >1 polyatomic ions in the compound, place a parenthesis around the entire ion and write the subscript outside the parenthesis.

• Ex.) Magnesium & nitrate= Mg+2 + NO3-1 → Mg(NO3)2

• Ex.) Aluminum & carbonate= Al+3 + CO3-2 → Al2(CO3)3

Ionic Cpmds w/ Polyatomic ionsName Formula

Ammonium Oxide

Sodium phosphate

Sodium nitrate

Magnesium sulfate

NH4OH

Ca(OH)2

KNO3

Li2CO3

Ionic Cpmds w/ Transition Metals

• Oxidation number: represents the charge on a monatomic ion, i.e. ionic charge.

• Some transition metals can form >1 oxidation state, so the charge of the different ion must be indicated.

• Ex) Iron has two charges: Fe 2+, Fe 3+

• Following the same rules for naming & writing formulas.• Except: Transition metal ionic compounds: use roman

numeral in parenthesis after metal name to indicate oxidation # of transition metal.

• Ex) Pb+2 + Cl-1 → PbCl2 = Lead (II) chloride • Ex) Cu2+ + Cl → CuCl2 = Copper (II) chloride

Common ions of Transition Metals & other Metals

Group Ions

4 Ti 2+ , Ti 3+

5 V 2+ , V 3+

6 Cr 2+ , Cr 3+

7 Mn 2+ , Mn 3+ , Tc 2+

8 Fe 2+ , Fe 3+

9 Co 2+ , Co 3+

10 Ni 2+, Pd 2+, Pt 2+, Pt 4+

11 Cu1+, Cu 2+, Ag1+, Au1+, Au3+

12 Zn 2+, Cd2+, Hg22+, Hg2+

13 Ga2+, Ga3+, In1+, In2+, In3+,

Tl 1+, Tl 3+

14 Sn 2+, Sn 4+, Pb 2+, Pb 4+

Ionic Cpmds w/ Transition MetalsName Formula

Copper (II) Oxide

Iron (II) Sulfide

Cobalt (III) Chloride

Titanium (II) nitride

TiO

FeCl3

Cu2O

CuO

Binary Molecular Molecules

YES NO

Is compound binary?

YES NO

Is the 1st elementa METAL ? 2nd

element a nonmetal.

YES NO

Is the 1st & 2nd element a nonmetal.

• Then you have a binary molecular compound with 2 nonmetals.

• They share valence electrons instead of exchanging them to form ions…..

• Not cations or anions formed.

Molecular Compounds

• Binary Molecular Cmpd: AKA – Covalent molecules

• A binary compound is a cmpd formed by the combination of 2 elements btwn 2 nonmetals that share valence electrons.

Names for molecular binary compounds consist of two words.

• The 1st word is a prefix + a complete element’s name. (No prefix is used if there’s only 1 atom of the 1st element).

– Ex. CO2 ------------1st name= Carbon

• The 2nd word is a prefix plus the root of the element’s name plus the ending -ide.

• [PREFIX + ROOT NAME OF ELEMENT + -IDE]

– Ex. CO2 ------------2nd name= dioxide

– CO2 =Carbon dioxide

*Prefix: tells how many atoms of each element are present in the compound.

• Common Greek prefixes used in chemical

names

Prefix #

mono 1

Di (or –bi) 2

tri 3

tetra 4

penta 5

hexa 6

hept 7

octa 8

nona 9

deca 10

Practice

• CO

• P2O5

• N2O4

• SF4

Writing formulas for covalent compounds:

• Write the symbols for each element

• If the atom has a prefix, then write the number representing the prefix as a subscript after the element’s symbol.

Practice

• Example:• Diphosphorous Trisulfide • write symbol: P S

• Write the subscript that represents the prefix: P2S3

• - Nitrogen Trichloride • write symbol: N Cl

• Write the subscript that represents the prefix: NCl3

Write the chemical formulas for the following compounds

• Dinitrogen Hexafluoride

• Carbon Dioxide

• Silicon Tetrafluoride

• Carbon Tetrabromide

Extra Information

Electron Configuration in Ionic Bonding

• Valence electrons are usually the only ones involved in bonding– Shown as electron dot structures (Lewis dot

structures)

• The number of valence electrons is related to the group number

• Formula Unit- lowest whole number ratio of ions in ionic compound; ionically bonded

• Ionic compound- compounds made of cations & anions; formed from xfer or exchange of v.e.o Usually a metal (cation) & nonmetal (anion)o Smallest unit= formula unito Solid at room temp.– High MP

• Ion-charged atom that has lost or gained valence electrons.

• Cation- group of atoms that lose e- to become + charged

• Anion- group of atoms that gain e- to become – charged

Ionic Binary Compounds • Monatomic ions- ions made of 1 atom• Group 1 lose 1 e- 1+

• Group 2 lose 2e- 2+

• Group 3 lose 3 e- 3+

• Group 14- bonds covalently (no ionic bond)• Group 15 gain 3 e- 3-

• Group 16 gain 2 e- 2-

• Group 17 gain 1 e- 1-

• Group 18 Noble gases- inert

Common Ion Charges/ Oxidation1+

2+ 3+ NA 3- 2- 1-

0

C. Ionic Nomenclature

Electron Configuration in Ionic Bonding

• Electron Configurations for Cations– The octet rule applies to most atoms in compounds– An atom’s loss of valence electrons produces a

cation (positively charged ion)• The most common cations are produced by the loss of

valence electrons from metal atoms

• Most metals atoms have one to three valence electrons, which are easily removed

Electron Configuration in Ionic Bonding

• Electron Configurations for Anions– The gain of negatively charged electrons by a

neutral atom produces anions– Ions that are produced when atoms of chlorine,

or other halogens, gain electrons are called halides

• All halides have a 1- charge

– For atoms from the oxygen group to gain a noble gas configuration, they must gain 2 valence electrons, resulting in a 2- ion

Ionic Bonds

• Formation of ionic compounds– Anions and cations have opposite charges, thus

they attract one another• The forces of attraction that bind these ions are called

ionic bonds• Compounds that consist of electrically neutral groups

of ions are called ionic compounds• The total positive charges must be balanced by the

total negative charges• Ex: Na+ and Cl- form NaCl• Ionic bonds can be explained with electron config.

Ionic Bonds

• Properties of ionic compounds– At room temperature, most are crystalline

solids• The component ions are arranged in repeating 3-

dimensional patterns called unit cells

• In this arrangement, each ion is attracted strongly to each of its neighbors and repulsions are minimized

• The large attractive forces result in a very stable structure

Electron Configuration in Ionic Bonding

• Transition metals have varying numbers of valence electrons– Fe can lose two or three electrons, resulting in a 2+ or 3+

charge– Some ions formed by transition metals do not attain a noble

gas configuration, so are exceptions to the octet rule• Ag would have to lose 11e-, or gain 5e- to have a noble gas

configuration• Instead, atoms with more than 3 valence electrons tend to end up

with 18 e- in their outer energy level– Called a pseudo noble gas configuration– Having 18 valence e- is relatively favorable in compounds– Transition elements to the far right tend to do this– Cu, Au, Cd, and Hg have pseudo noble gas configurations

Bonding in Metals

• Metallic bonds and metallic properties– Metals are made up of closely packed ions,

surrounded by mobile valence electrons • These valence electrons can move freely from one

part of the metal to another

• Metallic bonds consist of the attraction of the freely-floating valence electrons to the positively charged metal ions

– Explains many of the properties of metals

Bonding in Metals

• Properties of metals– Good conductors of electricity because electrons

can flow freely in them– Ductile and malleable because of the mobility of

the valence electrons

• Crystalline structure of metals– Metals that contain just one type of atom are

among the simplest of all crystalline solids• Metal atoms are arranged in very compact and orderly

patterns

Bonding in Metals• Alloys

– Most metals you encounter are alloys– Alloys are mixtures composed of two or more

elements, at least one of which is a metal• Prepared by melting the ingredients, then allowing them

to cool• There are many different kinds of alloys

– Ex: Brass is an alloy of copper and zinc

• Alloys are important because their properties are often superior to those of the individual elements

– Today, the most important alloys are steels

• Two types of alloys are substitutional alloys and interstitial alloys (depends on formation)