transition and polyatomic ions 2008
DESCRIPTION
TRANSCRIPT
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