Transition Metals & Polyatomic Ions

Goal 1

Name ionic compounds that contain transition metals

• Transition Metals– Total charge on compound = 0– Electron loss can vary– Roman numerals

• Indicate charge

• Step 1: Determine total charge on nonmetal

MnO O = 2-

Fe2S3 S3 = 6-

• Step 2: Determine needed charge on transition metal to create an equal opposite charge (multiply by subscript)

MnO Mn = 2+ O = 2-

Fe2S3 Fe = 3+ S3 = 6-

• Step 3: Use charge on transition metal to determine your roman numeral

MnO Mn = 2+ O = 2-

manganese(II) oxide

Fe2S3 Fe = 3+ S3 = 6-

iron(III) sulfide

• Try it backwards!

• Chemical formula from a name

Tin(II) oxide

• Step 1: Determine charge on transition metal

Tin(II) oxide

Sn = 2+

• Step 2: Determine charge on nonmetal ion

(use periodic table)

Tin(II) oxide

Sn = 2+ O = 2-

• Step 3: Determine how many of each needed to equal 0 charge (CC&R)

Tin(II) oxide

Sn = 2+ O = 2-

SnO

Try it…

Iron(III) fluoride

Were you correct?

Iron(III) fluoride

FeFl3

Try again (this time backwards)

TiN

Were you correct?

TiN

titanium(III) nitride

And again…

PbO2

Were you correct?

PbO2

lead(IV) oxide

Goal 2

Name ionic compounds using polyatomic ions

• Polyatomic ions– Covalently bonded elements with a charge– May be indicated by parentheses

(OH-)

(OH-)2

– Use the same as a single ion– Information found on back of periodic table

Hydroxide ion

• Step 1: recognize use of polyatomic ion– Name ends in “-ate” or “-ite” – Name that is not an element… cyanide– Parentheses used in chemical formula– Or… check anyways

Sodium sulfate

Na2(SO4)

• Step 2: use back of your periodic table to determine charge on the polyatomic ion

Sodium sulfate2-

• Step 3: determine how many metal ions needed to make a 0 charge (criss-cross)

Sodium1+2 sulfate2-

Na2(SO4)

Try it….

Calcium chlorate

Try it….

Calcium chlorate

Try it….

Calcium chlorate1-

Try it….

Calcium2+ chlorate1-2

Ca(ClO3)2

CC&R stays OUTSIDE of polyatomic parentheses