Nomenclature:
Naming Chemicals
PO43phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
SAVE PAPER AND INK!!! When you
print out the notes on PowerPoint,
print "Handouts" instead of
"Slides" in the print setup. Also,
turn off the backgrounds
(Design>Hide background graphics
with all slides selected)
Before&naming….&
! Some%things%you%MUST%
know%to%be%successful….%You%
really%need%to%commit%these%
things%to%memory%
1
Ions:&A&Refresher&
! Atoms%or%groups%of%atoms%with%a%charge.%
! Cations@%positive%ions%@%get%by%losing%
electron(s).%
! Anions@%negative%ions%@%get%by%gaining%
electron(s).%
! Ionic%bonding@%held%together%by%the%
opposite%charges@%electrostatic%attractions.%
! Ionic%solids%are%called%salts.%
! Salts%are%electrolytes;%they%conduct%
electricity%when%dissolved%in%water%(aq.)%
" Conductors
of heat and electricity
" Make cations (lose e to become + charged)
" Malleable (made into sheets)
" Ductile (made into wire)
-
2
"  Are
a brittle solid or a gas
"  Make anions (gain e- to become - charged)
"  Covalently bond to each
other
• Characteristics of both
metals and nonmetals
• More metallic as you go
down PT
3
Alkali Metals
Alkaline Earth Metals
4
Transition metals
Inner Transition Metals
5
Halogens
Noble Gases
6
+1
Common Ions of Elements
+3
+2
+/-
4 -3 -2 -1 0
Variable, always +
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
0
Cd+2
7
Polyatomic&Ions&
!  Groups%of%covalently%
bonded%atoms%that%
have%a%charge.%
*%NO3'((:nitrate%ion%
*%NO2'((:nitrite%ion%
!  Yes,%you%have%to%
memorize%them.%
!  Listed%in%your%
resource%handbook:%
memorize(the(
required(list!!!!(
Pa9erns&for&Polyatomic&Ions&
! @ate%ion%
!  chlorate%=%ClO3@%
! @ate%ion%plus%1%O%⇒%same%charge,%per$%prefix%
!  perchlorate%=%ClO4@%
! @ate%ion%minus%1%O%⇒%same%charge,%@ite%
suffix%
!  chlorite%=%ClO2@%
! @ate%ion%minus%2%O%⇒%same%charge,%hypo$%
prefix,%@ite%suffix%
!  hypochlorite%=%ClO@%
8
Polyatomic%Ions%
You can make additional polyatomic ions by adding a H+
to the ion!"
!  CO3 -2 is carbonate:"
–
!  HCO3 is hydrogen carbonate"
!  PO43- is phosphate:"
!  HPO4
2-
is hydrogen phosphate"
–
!  H2PO4 is dihydrogen phosphate"
2-
!  SO4 is sulfate"
–
!  HSO4 is hydrogen sulfate"
The 3 types of Chemical Bonds:
Metallic, Ionic and Covalent!
!  Electronegativity%and%Bond%Type%
!  Bond%type%can%be%determined%by%the%difference%
in%electronegativty%between%the%bonds%involved%
!  Differences%of:%
!
2%=%ionic%
≥
!  0.5@1.9%=%polar%covalent%
!
%≤%0.4%=%nonpolar%covalent%
.
!  Metals%bonded%to%other%metals%are%metallically%
bonded,%regardless%of%the%difference%in%
electronegativity%
9
Metallic bonds&
! The atoms of metals
are held together when
the atom’s valence
electrons float around
the nuclei of the
metals – the “sea of
electrons”"
! Electrostatic forces
keep everything
together"
Ionic&Bonds&
"
!  Complete transfer of 1 or more
electrons from one atom to another
(or a polyatomic ion)"
!  one loses one or more e-, the other
gains those e-s"
!  Atoms%involved%are%%
!
a%metal%%and%either%a%non@metal%or%a%
polyatomic%ion%
!  The%cation%and%anion%are%attracted%to%
%
each%other%by%electrostatic%attraction%%
10
Ionic&compounds&are&neutral&
! Ionic%compounds%are%neutral%
! That%is,%they%have%no%overall%charge%
!  This%is%because%the%number%of%electrons%that%
are%given%up%by%the%metal%is%the%same%number%
of%electrons%that%are%gained%by%the%anion%for%
the%formula.%
! Formulas%reflect%this%neutrality@%the%
charges%on%the%individual%ions%are%not%
written%in%because%they%cancel%out%overall%
for%the%compound%
COMPOUNDS
FORMED FROM
IONS&
CATION +
ANION --->
COMPOUND!
Na+%+%Cl@%@@>%NaCl%
%
%%
A neutral compound !
requires!
equal number of + !
and - charges.!
11
Covalent&Bonds&
"
!  2, 4, or 6 valence electrons that are shared
between atoms"
!  We are going to name only simple covalent
compounds that have 2 elements involved"
Most&bonds&are&somewhere&in&between&
ionic&and&covalent&(as&you&already&know)&
!  Because%not%all%atoms%share%e@%equally%
!  The%conventions%of%naming%assume%absolute%difference%
in%bond%types%
!  Metals%bonded%to%nonmetals%or%polyatomic%ions%are%
classified%as%having%ionic%bonds*%
!  Materials%made%out%of%all%non@metals%are%classified%as%
having%covalent%bonds*%
!  *%semimetals%are%not%a%classification%in%naming;%you%need%
to%treat%the%elements%that%are%on%the%right%of%the%line%as%
non@metals,%and%those%on%the%left%as%metals.%%
!  For%more%on%this,%go%back%to%bonding%%
12
Naming&things:&
If%there%is%only%one%element%present,%name%it.%
& !  Atomic%substances%do%not%require%“special”%
naming.%
!  For%anything%with%more%than%one%element,%
remember%that%there%is%ONE%MAIN%THING%to%
look%for:%%
! Is%there%a%metal%first?%%
%
So…some&general&help&for&naming:&
& !  Look%to%see%if%there%is%a%metal%first%in%the%
formula%
!
Again,%semimetals%are%not%a%classification%in%
naming;%you%need%to%treat%the%elements%that%are%on%
the%right%of%the%line%as%non@metals,%and%those%on%the%
left%as%metals.%
!  If%there%are%only%metals,%name%both%metals%
!  (metallic%bonding;%nothing%else%need%be%done)%
!  If%ONLY%the%first%element%is%a%metal,%then%the%
compound%is%an%ionic%compound%%
!  Nonmetals%only%signify%a%covalent%compound%
!  There%is%a%flow%chart%in%your%handbook%to%help!%
%
13
Naming&ionic&compounds:&
! Remember%that%those%are%compounds%that%
have%a%metal%first%in%the%formula*,%and%then%a%
nonmetal%or%a%polyatomic%ion.%%
! We%can%handle%these%as%simple%types%
!  binary%(2%elements)%compounds%
!  Ternary(more%than%2%element)%compounds%
! Names%are%always%for%the%smallest%whole%
number%ratio%of%the%elements,%the%formula%unit%
*Two%exceptions%to%this%rule:% %%
!  Compounds%that%start%with%either%ammoniums%(NH4+)%or%hydronium%(H3O+)
%
General&informaHon&for&naming&
ionic&compounds&
! If%the%cation%is%monatomic@%Name%
the%metal%(cation).%%
! Use%Roman%Numerals%for%transition%
metals%(ONLY)%after%the%metal%%
! If%the%cation%is%polyatomic@%name%it.%
! If%the%anion%is%monatomic@%name%it%
but%change%the%ending%to%–ide.%
! %If%the%anion%is%poly%atomic@%just%name%it%
14
Example: CaCl2, or calcium chloride
"  Name
the cation first, then the anion root
with an –ide suffix
"  For
CaCl2, the monatomic cation is Ca2+ ,
calcium, and the monatomic anion is Cl ,
named chloride.
"
We use chloride because the root for
chlorine is chlor, and we use = root + -ide
for the second element in binary
compounds
"  CaCl2 = calcium chloride
PracHce&Naming&Binary&Ionic&Compounds&
!
(Examples:(
(
NaCl((
((
ZnI2 ((
((
Al2O3
(
((
15
Learning&Check&&
(Complete(the(names(of(the(following(binary(
compounds:(
(Na3N
(
((
(KBr
(
((
(Al2O3
(
((
(MgS
(
((
%
If&the&Metal&is&a&TransiHon&Metal…&
Transition(metals(are(Type(II(Cations,(and(are(
elements(that(can(have(more(than(one(possible(
charge.((They(MUST(have(a(Roman(Numeral(to(
indicate(the(charge(on(the(individual(ion.(
(1+(or(2+((((((((((((((2+(or(3+(
((
(
Cu+,(Cu2+ ((((((((((((Fe2+,(Fe3+(
copper(I)(ion((((((((iron(II)(ion((
(copper((II)(ion((((iron(III)(ion (
(((
(%
%
16
Type&II&CaHons&
(These(elements(REQUIRE(Roman(Numerals(
(
because(they(can(have(more(than(one(possible(
charge:(
(anything(except(Group(1A,(2A,(Ag,(Zn,(Cd,(and(Al(
(
((You(should(already(know(the(charges(on(these!)(
(
Or(another(way(to(say(it(is:(Transition(metals(and(the(metals(in(groups(4A(and(
(
(5A((except(Ag,(Zn,(Cd,(and(Al)(require(a(Roman(Numeral.(
(
(FeCl3
((Fe3+)(
(iron((III)(chloride
((
(CuCl
((
(copper((I)(chloride(
4+
(
(SnF4((((((((((
((Sn )
(tin((IV)(fluoride(
2+
(PbCl2((((((((
((Pb )
(lead((II)(chloride(
3+
((((Fe2S3
((((((((( ((Fe )(
(iron((III)(sulfide(
((Cu+()(
You(will(appreciate(this(more(when(we(go(from(names(to(formulas!(
Type&II&CaHons&
Some%Type%II%cations%have%a%name%using%the%
“old”%system%as%well%as%the%“new%system”.%%%
%
The%old%system,%still%widely%used,%adds%to%the%
root%or%stem%of%the%Latin%name%of%the%metal%
the%suffixes%–ous%and%–ic.%%These%represent%
the%lower%and%higher%charges%respectively.%%
17
Examples&of&Older&Names&of&CaHons&formed&from&
TransiHon&Metals&
(you&do&not&have&to&memorize&these)&
Learning&Check&&
(Complete(the(names(of(the(following(binary(
compounds(with(variable(metal(ions:(
(FeBr2
(
((
(CuCl
(
((
(SnBr4
(
((
(((Fe2O3
(
((
(Hg2S
(
((
(
%
18
WriHng&Formulas&for&Ionic&Compounds&from&
Names&
Formulas(of(ionic(compounds(are(determined(
(
( from(the(charges(on(the(ions
(
(((((((((((((
Na( (+((((F(((("→
((((((((((((((((((((((((
(
((Na+(((((+(((((F'((("→(((NaF(
(((((((((((((((((((((((((
Sodium(atom(+((fluoride(ion(((((((((sodium(fluoride(
(((Charge(balance:(((((((((((1+((((((+((((((1'(((((((((((((=((0(
(
Remember(that(all(ionic(compounds(have(no(net(charge,(
and(that(the(charges(are(not(written(in!(Ever.(Nope.(
%
Neutral,&you&say?&
! Formulas%are%written%to%make%the%
compound%have%a%neutral%charge%overall.%%%
! You%do%NOT%write%the%charges%in%the%
formula%because%they%MUST%cross%out%to%
accurately%represent%the%compound.%%
! Ex:%NaF2%is%INCORRECT%for%sodium%chloride%
because%Na%has%an%oxidation%state%of%+1,%and%
F%of%@1.%%There%is%a%one%to%one%ratio%of%Na+%to%
F@%to%make%a%neutral%ionic%compound.%
19
WriHng&the&formula…&
(Write(the(formula(for(the(barium(chloride,(the(
compound(that(will(form(between(Ba2+(and(Cl'.(
(Solution:((
1.(Write(the(cation,(and(then(the(anion(
2.(Balance(charge(with((the(number(of(+(and(–(ions((
( Ba++
ClThink:
(((((( ((((((((((((
Cl
Why is Cl- written twice?
3.(Write(the(number(of(ions(needed(as((
((((((((subscripts: (%
BaCl2
So&what&if&the&oxidaHon&numbers&
aren’t&even?&
!  If%the%oxidation%numbers%or%charges%do%not%
balance,%you%can%write%the%number%of%ions%of%each%
until%you%get%the%same%number%of%each%charge%in%
total.%
Is#there#an#easier#way?#
%
!  Yes.%%The%“Criss%Cross”%method.%You%take%the%
charge%number%from%the%cation,%and%you%make%
it%the%number%of%anions%(subscript)and%take%
the%charge%on%the%anion,%and%you%make%that%
many%cations%(subscript).%%%
20
CrissTCrossing&in&acHon:&
Example:%Lead%(II)%nitrate%
%
Pb2+%%N3@
%
%
Pb2+%%N3@%%%
%*the%charges%do%not%balance%
%
%
%%
%Pb3N2%%%%%%%%%%%%
%
!  The%2%and%the%3%are%brought%down%to%the%
opposite%element,%so%that%there%are%now%3%Pb2+%
ions%and%2%N3@%ions%
!  This%means%there%were%6e@%transferred%from%the%
lead%atoms%to%the%nitrogen%atoms;%the%compound%
is%neutral%
Learning&Check&&
(Write(the(correct(formula(for(the(
compounds(containing(the(following(
ions:(
(1.( (Na+(and((S2'(
((( (a)((NaS ((((b)(Na2S (
(c)(NaS2(
(2.((Al3+(and(Cl'(
((( (a)((AlCl3 ((((b)((AlCl( (
(c)(Al3Cl(
(3.((Mg2+(and(N3'(
((( (a)((MgN ((((b)(Mg2N3
(c)(Mg3N2(
(
21
Ternary&Ionic&Compounds:&
! Contain(at(least(3(elements(
! There(MUST(be(at(least(one(polyatomic(ion(
( ((it(helps(to(circle(the(ions)(
Examples:(
(NaNO3 (
(Sodium(nitrate(
(K2SO4 (
(Al(HCO3)3
(
(
(
(Potassium(sulfate(
(Aluminum(bicarbonate(
((Aluminum(hydrogen(carbonate)(
((
(
(
Examples: NaNO3, and Co(NO3)2
"  Name
the cation first, then polyatomic ion
"  For
NaNO3, the monatomic cation is Na+ ,
sodium, and the polyatomic anion is NO3 ,
named nitrate.
•  NaNO3 is sodium nitrate
"
For Co(NO3)2, the monatomic cation is Co
cobalt (II) and the polyatomic anion is
NO3 , named nitrate.
+2,
•  Co(NO3)2 is cobalt (II) nitrate
22
Learning&Check&&
Match(each(set(with(the(correct(name:(
1.%%%%% %Na2CO3
(
(a)(((magnesium(sulfite((
(
(MgSO3
(
(b)(((magnesium(sulfate(
(
(MgSO4
(
(c)(((sodium(carbonate( ((
(
2(.
(Ca(HCO3)2 (
(a)(calcium(carbonate(
(((((( (CaCO3
(
(b)((calcium(phosphate(
(((((( (Ca3(PO4)2( (c)((calcium(bicarbonate(
WriHng&Formulas&for&Ternary&Ionic&Compounds&
!  Write%the%cation%first,%then%the%anion.%%%
!  Overall%charge%must%equal%zero.%
!  If%charges%cancel,%just%write%symbols.%
!  If%not,%use%subscripts%to%balance%charges.%
!  Use%parentheses(to(show(more(than(one(of(a(
particular(polyatomic(ion.%
!  Use%Roman(numerals%indicate%the%ion’s%charge%when%
needed%(transition%metals)%
!  Remember%that%the%final%formula%should%not%have%
charges%written%in.%
23
WriHng&Formulas,&cont’d&
Example:%
Cr2+%%PO43@
%*
the%charges%do%not%balance%
%
Cr2+%%PO43@%%% %Cr3(PO4)2%
%
The(polyatomic(ions(is(in(
parentheses(whenever(a(subscript(
is(added.(
This(is(so(that(we(know(to(count(a(
number(of(those(groups!(
Learning&Check&&
1.((aluminum(nitrate((
( (((a)((AlNO3((((((((((b)(Al(NO)3((((c)((Al(NO3)3(
2.((copper(II)(nitrate(
((((a)(CuNO3
(b)(Cu(NO3)2
(c)((Cu2(NO3)
((
3.((Iron((III)(hydroxide(
((((a)((FeOH
(b)((Fe3OH (
4.((Tin(IV)(hydroxide(
((((a)((Sn(OH)4(((b)((Sn(OH)2(((((
(c)((Fe(OH)3(
(c)((Sn4(OH)(
(
%
24
Ternary&Ionic&Nomenclature:&
You(Criss'cross(these,(too.((
(
Sodium(Sulfate(
(
(
(
Iron((III)(hydroxide(
(
(
(
(
Ammonium(carbonate(
Write&the&Formula:&
Copper%(II)%chlorate%%%%
Calcium%nitride
%
Aluminum%carbonate
Potassium%bromide %
Barium%fluoride
%
Cesium%hydroxide %
%
%
%
%%
%
%%
%%
%%
%%
%%
25
General&naming&rules&for&
covalent&(molecular)&compounds&
! Names%are%two%words,%with%prefixes.%
!  Prefixes%tell%you%how%many.%
! Use%the%first%element’s%whole%name%with%
the%appropriate%prefix%
!  *********except%mono.%
!  NEVER%use%mono%for%the%first%element%
! For%the%second%element,%use%the%root%of%
the%name%and%the%@ide%ending%with%
appropriate%prefix%for%that%many.%
%
NEVER%
You%
criss@cross%charges%
with%covalent%
compounds.%
never&
Since%you%are%sharing%electrons,%rather%than%giving%
them%away/%picking%them%up,%the%charges%are%
not%relevant.%
%
26
Covalent&Naming&Prefixes:&
PREFIX%
%mono@%
%di@%
%tri@%
%tetra@%
%penta@%
%hexa@%
%hepta@%
%octa@%
%nona@%
%deca@%
NUMBER%
1%
2%
3%
4%
5%
6%
7%
8%
9%
10%
Example: CO2 is carbon dioxide
"  Name
the first element, using a prefix if
there is more than one atom of the element
present
"  Name
the second element, using the
appropriate prefix in all cases
"
CO2 is carbon dioxide because there is one
carbon (no prefix when there is only one
atom of the element,) and two oxygens (diprefix)
27
Learning&Check&&
1.(
(P2O5 (
(a)((phosphorus(oxide(
(
(
(
(b)((phosphorus(pentoxide(
(
(
(
(c)((diphosphorus(pentoxide(
(
2.(Cl2O7
(a)((dichlorine((heptoxide(
(
(
(
(b)((dichlorine(oxide(
(
(
(
(c)((chlorine(heptoxide((
(
(
((
3.((((( (Cl2 (
(a)((chlorine
((
(
(
(
(b)((dichlorine ((
(
(
(
(c)((dichloride(
Learning&Check&&
(Give(the(names(of(following(covalent(
compounds:(
(
(CO((( (
((
(
(CO2 (
((
(
(PCl3 ((
(
(CCl4 (
((
(
(N2O (
((
28
Covalent&Naming&Examples&
"  CCl4
"  N2O5
"  SF6
More&Covalent&Examples&
"  arsenic trichloride
"  dinitrogen pentoxide
"  tetraphosphorus decoxide
29
Hydrates:#Ionic#Compounds7Water#
! Some%salts%trap%water%crystals%when%they%
form%crystals.%%%
!  Ex:%CuSO4tH2O%
! These%are%hydrates.%
! Both%the%name%and%the%formula%needs%to%
indicate%how%many%water%molecules%are%
trapped.%
! In%the%name%we%add%the%word%hydrate%with%
a%prefix%that%tells%us%how%many%water%
molecules.%%
! CuSO4tH2O%is%copper%(II)%sulfate%pentahydrate%
Hydrates#
! In%the%formula%you%put%a%dot%and%then%write%
the%number%of%molecules.%
%
! Calcium%chloride%dihydrate%=%CaCl2•2Η2Ο&
&
! Chromium%(III)%nitrate%hexahydrate%=%
Cr(NO3)3•%6H2O%%
30
Acid&Nomenclature&
!  Acids(
!  Compounds(that(form(H+(in(water.(
!  Formulas(usually(begin(with(‘H’.(
!  In(order(to(be(an(acid(instead(of(a(gaseous(covalent(
compound,(it(must(be(aqueous(
!
Meaning(dissolved(in(water;(symbolized(by((aq)(
!  Ternary(acids(are(ALL(aqueous(
!  Two(types:%%%
!  Non@oxyacids%
!  Oxyacids(
Naming&acids:&NonTOxy&acids&
If%the%acid%doesn’t%have%oxygen%
! add%the%prefix%“hydro@”%
! change%the%suffix%“–ide”**to%“@ic*acid”*
HCl %
H2 S %
HCN %
%Hydrochloric%acid%
%Hydrosulfic%acid%
%Hydrocyanic%acid%
31
Naming&acids:&Oxy&Acids&
If%the%formula%has%oxygen%in%it%
!  write%the%name%of%the%anion,%but%change:%%
“.ate”*to*“.ic*acid”*
!  “.ite”*to%“.ous*acid”*
!
!  Watch%out%for%sulfuric%and%sulfurous!%
H2CrO4 %%
HMnO4%%
HNO2%%
Chromic%acid%
Manganic%acid%
Nitrous%acid%
Acid&Nomenclature&Flowchart&
ACIDS
start with 'H'
2 elements
3 elements
hydro- prefix
-ic ending
no hydro- prefix
-ate ending
becomes
-ic ending
-ite ending
becomes
-ous ending
32
Anion
Ending
Binary #
Ternary
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”
Acid&Nomenclature&
"  HBr (aq)
"  H2CO3 (aq)
"  H2SO3 (aq)
33
Acid
Name
HNO3
HNO2
H2SO4
H2SO3
H3PO4
HC2H3O2
Name&‘Em!&
! HI%(aq)%
! HCl%(aq)%
! H2SO3%(aq)%
! HNO3%(aq)%
! HIO4%(aq)%
34
Formulas&for&acids&
! Backwards%from%names.%
! If%it%has%hydro@%in%the%name%it%has%no%
oxygen%
! Anion%ends%in%“.ide”*
! No%hydro,%anion%ends%in%“.ate*or*–ite”*
! Write%anion%and%add%enough%H’s%to%
balance%the%charges.%
Acid&Nomenclature&
"  hydrofluoric acid
"  sulfuric acid
"  nitrous acid
35
Formulas&for&acids&
hydrofluoric%acid%
dichromic%acid%
carbonic%acid%
hydrophosphoric%acid%
hypofluorous%acid%
perchloric%acid%
phosphorous%acid%%
Write&the&Formula!&
!  Hydrobromic%acid%
!  Nitrous%acid%
!  Carbonic%acid%
!  Phosphoric%acid%
!  Hydrotelluric%acid%
36
Common&Names&
!  A(lot(of(chemicals(have(common(
names(as(well(as(the(proper(
IUPAC(name.(
!  Chemicals(that(should(always(be(
named(by(common(name(and(
never(named(by(the(IUPAC(
method(are:(
!  H2O
(water,(not(dihydrogen(
monoxide(
!  NH3(((ammonia,(not(nitrogen(
trihydride(
Mixed&PracHce&
1.
2.
3.
4.
5.
6.
7.
8.
9.
Dinitrogen%monoxide%
Potassium%sulfide%
Copper%(II)%nitrate%
Dichlorine%heptoxide%
Chromium%(III)%
sulfate%
Iron%(III)%sulfite%
Calcium%oxide%
Barium%carbonate%
Iodine%monochloride%
37
!  Match(each(set(with(the(correct(name:(
Na2CO3
MgSO3
MgSO4
(
Ca(HCO3)2
CaCO3
Ca3(PO4)2(
(
(
(
(a)(sodium(carbonate(
(b)(magnesium(sulfite(
(c)(magnesium(sulfate( ((
(
(
(
(a)(calcium(bicarbonate(
(b)((calcium(carbonate(
(c)((calcium(phosphate(
Mixed&PracHce!&
Name%the%following:%
1.  Na2O%% %
%
2.  CaCO3 %%
3.  PbS2
%
%%
4.  Sn3N2% %
%%
5.  Cu3PO4%
6.  HgF2 %
%%
%%
38
Mixed&Review&&
Name(the(following(compounds:(
1.(( (CaO(
(
(
2.((
(
(
(
3.((
(
%
(a)((calcium(oxide (
(c)((calcium((II)(oxide
(b)(calcium(I)(oxide(
(d)(calcium(monoxide(
(SnCl4(
((
((
(a)((tin(tetrachloride (b)(tin(II)(chloride(((
(c)((tin(IV)(chloride ((
(N2O3(
(a)((nitrogen(oxide(((
%c)((nitrogen(trioxide
(b)(dinitrogen(trioxide(
(
%
Mixed&PracHce&
1.  BaI2%
2.  P4S3%
3.  Ca(OH)2%
4.  FeCO3%
5.  Na2Cr2O7%
6.  I2O5%
7.  Cu(ClO4)2%
8.  CS2%
9.  B2Cl4%
39
DONE!&
Now&it&is&Hme&to&study!&
Rainbow&Matrix&Game&
!  Link(on(Chemistry(Geek.com(on(Chemistry(
I(page(
!  http://chemistrygeek.com/rainbow(
(
Use([(](to(represent(subscripts(since(you(can’t(
enter(subscripts(into(the(computer(
So(H2O(would(be(H[2]O(
And(Al2(SO4)3(would(be(Al[2](SO[4])[3](
(
Additional(Polyatomic(Ions((you(do(not(have(
to(memorize(these,(but(they(are(in(the(
game!)(
Borate(=(BO3('3((;((Silicate(=(SiO4('4((;(
Manganate(=(MnO4('2((permanganate(is('1)(
40