Names of Common Polyatomic Ions Ion Name Ion Name NH 4 ammonium CO 3 2 carbonate NO 2 nitrite HCO 3 ID: 238275
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Slide1
Common Polyatomic Ions
Names of Common Polyatomic Ions
Ion Name Ion Name
NH4 + ammonium CO3 2- carbonate *NO2 - *nitrite HCO3 - bicarbonate NO3 - nitrate *IO3- *iodate *SO3 2- *sulfite *IO4- *periodate SO4 2- sulfate *ClO - *hypochlorite HSO4- hydrogen sulfate *ClO2 - *chlorite OH - hydroxide ClO3 - chlorate CN - cyanide *ClO4 - *perchlorate C2H3O2- acetate *BrO3- *bromate MnO4 - permanganate C2O42- oxalate PO4 3- phosphate Cr2O7 2- dichromate *PO3 3- *phosphite CrO4 2- chromate H2PO4 - dihydrogen phosphate O2 2- peroxide
Zumdahl, Zumdahl, DeCoste,
World of Chemistry 2002, page 100
Memorize the BOLD ions
* = you will be responsible for knowing theseSlide2
Polyatomic Ion Trends
*Charges NEVER change between different forms
“Normal”
“–ate” form
BrO3-bromateClO3-chlorate
IO
3-iodate
NO
3
-
nitrate
CO32-carbonateSO42-sulfatePO43-phosphate
BrO2-ClO2-IO2-NO2-CO22-SO32-PO33-
BrO-ClO-IO-
BrO4-ClO4-IO4-
-1 oxygen“-ite” form
-2 oxygens“hypo___ite”
+1 oxygen“Per____ate”
bromite
chlorite
iodite
nitrite
sulfite
phosphite
hypobromite
hypochlorite
hypoiodite
perbromate
perchlorate
periodate
carboniteSlide3
Atomic Theory ReviewSlide4
Electron Cloud Model
Orbital
(“electron cloud”) instead of “orbits”
Region in space where there is 90% probability of finding an electronCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Electron Probability vs. Distance
Electron Probability (%)
Distance from the Nucleus (pm)
100
150
200
250
500
01020
3040
Orbital
90% probability of
finding the electron
Orbital ShapeSlide5
Shapes of s, p, and d-Orbitals
each
holds 2
electrons (s2)each of 5 orbitals holds 2 e - = 10 total d electrons (d10)
each of 3 orbitals holds 2 e - = 6 total p electrons (p6)Slide6
s, p, and d-orbitals
s orbitals:
Each holds 2
electrons
(outer orbitals ofGroups 1 and 2)p orbitals:Each of 3 sets holds 2 electrons = 6 electrons(outer orbitals of Groups 3 to 8)d orbitals:Each of 5 sets holds 2 electrons= 10 electrons(found in elements in third periodand higher)Orbital Filling VideoSlide7
Copyright
©
2006 Pearson Benjamin Cummings. All rights reserved.
Orbitals overlap each other as you get farther from the nucleusSlide8
f-orbitals
7 f
orbitals @ 2 e- each =
14 e-Slide9
s, p, d and f orbitals
How many g orbitals could exist?Slide10
theoretical g-orbitals
9 g orbitals @ 2 e- each = 18 e-Slide11
s
p
d
f
6
7
Periodic Patterns for Electron Config
1
s
2
s
3s4s5s6s
7s3d4d5d6d
1s2p3p
4p5p6p7p
4
f
5
f
1
2
3
4
5
6
7
1
2
(n-1)
(n-2)
n
3
5
6
7
8
4Slide12
s-block
1st Period
1s
1
# of e- in that orbital(s)
Periodic Patterns
Example - HydrogenCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chemSlide13
Shorthand Configuration
S 16e
-
Valence Electrons
(Highest energy level)Core ElectronsS 16e- [Ne] 3s2 3p41s22s2
2p6
3s2
3p4Electron Configuration ReviewLonghand ConfigurationCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
S
32.066
16Slide14
[Ar]
4s
2
3d
104p2
Periodic Patterns
Example -
Germanium
Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem
Ge
72.61
32Slide15
[ ]
neon's electron configuration
(1
s22s22p6)Shorthand Configuration[Ne] 3s1
3rd energy level (or 3
rd
period)
1 electron in the
s
orbital
orbital shape (s,p,d,f…etc.)1s22s22p6 3s1electron configurationABCD
Na =[Ne]Slide16
Shorthand Configuration Practice
[Ar] 4
s
2
Electron configurationElement symbol
[Ar] 4
s2 3d3
[Rn] 7s2 5
f
14
6
d4[He] 2s2 2p5[Kr] 5s2 4d9[Kr] 5s2 4d10 5p5[Kr] 5s2 4d10 5p6[He] 2s22p
63s23p64s23d6CaVSg
F
Ag
I
Xe
Fe
[Ar] 4
s
2
3
d
6Slide17
Periodic Patterns Review
Period # (1-7)
energy level
(subtract for d & f)Group # (1-8…excluding d block)total # of valence e-Column within Sublevel block# of e- in sublevel/orbitalCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chemSlide18
s
p
d
f
6
7
Periodic Patterns and Charge Trends
1
s
1
2
3
4
5
67
+1
+2
(n-2)
n
+3
- 3
- 2
- 1
Variable Charge
METALS
NON-METALSSlide19
Electron Configurations for Cations
Metals lose e
-
to attain a noble gas configurationMetals form positive ionsCations are “paws”itiveMetal ions will lose e- from configurationNa: 1s22s22p63s1Na+:
1s22s22p6 noble gas configurationSlide20
Formation of a Cation
11
p
+
sodium atomNa[Ne] 3s1e-loss of one valence electrone-e-e-e-e-e-e-e-
e
-e-
sodium ionNa+[Ne]
11
p
+
e-e-e-e-e-e-e-e-e-e-e-Slide21
Electron Configurations for Anions
Non-metals gain electrons to attain a noble gas configuration
They form negative ions
Take a look at the e- configurationS 1s22s22p63s23p4 (6 valence electrons) + 2e
-S2- 1s22s22p63s23p6 (noble gas configuration)Slide22
Formation of an Anion
17
p
+
chlorine atomCl[Ne]3s23p5e-e-e-e-e-e-e-e-e-e-
e
-e-
e-e-e-e-
e
-
e
-gain of one valence electronchloride ionCl –[Ne]3s23p6 or [Ar]e-17p+e-e-e-e-e-e-e-e-e-e-
e-e-e-e-e-e-e-Slide23
Stable Electron Configurations
All atoms react to achieve noble gas configuration
Noble gases have two
s and six p electronsEight valence electrons Also called the octet ruleArSlide24
Bonding Review and Writing Ionic Formulas
Table saltSlide25
Formation of Ionic Bond
sodium ion
Na
+
11p+e-e-e-e-e-e-e-e-e-e-
chloride ion
Cl -
17p+e-e-
e
-
e
-e-e-e-e-e-e-e-e-e-e-e-e-e-e-+
-Slide26
Ionic Bonding
Anions and cations are held together by opposite charges
All ionic compounds are called salts
Simplest ratio is called the formula unitThe bond is formed through the transfer of electronsElectrons are transferred to fill all available orbitals, or achieve a noble gas configurationSlide27
O
2-
K
+
K+
Mg
2+
Br
-
Br
-
K
Brpotassium atombromine atom
e
-
e-
Br
-
K
+
potassium ion
bromide ion
potassium bromide
KBr
MgBr
2
K
2
O
magnesium bromide
potassium oxideSlide28
Bonding Practice
Ca
2+
Al
3+
Na+
Pb
4+
OH
-
N
3-
Mg2+OH -
OH -
N3-
Pb
4+
N
3-
N
3-
Pb
4+
N
3-
Pb
4+
N
3-
?
Pb
4+
N
3-
Pb
3
N
4
lead (IV) nitride
or
plumbic nitride
NaOH
Mg(OH)
2
AlN
CaBr
2
Ca(OH)
2
CaOSlide29
Fe
2+
Ca
2+
Ca
2+
Ca
2+
PO
4
3-
PO43-
PO43-NH4+
NH4+
NH4+
O
2-
Al
3+
Al
3+
O
2-
O
2-
O
2-
Ca
3
(PO
4
)
2
(NH
4
)
3
PO
4
FeO
Al
2
O
3Slide30
Subscripts, Superscripts and Coefficients
Mg
3
(PO4 )2coefficientsubscripts
superscripts
MAGNESIUM
PHOSPHATE
P
O
4
3- Mg2+5Slide31
Writing Formulas of Ionic Compounds
chemical formula
:
has neutral charge; shows types of atoms and how many of eachTo write an ionic compound’s formula, we need: 1. the two types of ions 2. the charge on each ion
Na+ and F– Ba2+ and O2– Na+ and O2– Ba2+ and F– NaFBaONa2OBaF2Slide32
ide
Calcium hydrox
ide
Ca
2+OH-
CaOH
2
Ca(OH)
2
Ca - O
H
HHO - Ca - OH vs.
The Importance of ParenthesesThe formulas imply two totally different compounds!Slide33
(NH
4
)
3NFe2(Cr2O7)3
Sn(SO4)2NH4ClO3Mg(NO2)2BaSO4Writing Formulas w/Polyatomic IonsParentheses are required only when you need more than one “bunch” of a particular polyatomic ionBa2+ and SO42– Mg2+ and NO2– NH
4+ and ClO3
–
Sn4+ and SO42– Fe3+ and Cr2O
7
2–
NH4+ and N3– Slide34
Element Latin root
-ic -ous
gold, Au
aur- Au3+ Au1+lead, Pb plumb- Pb4+ Pb2+tin, Sn stann- Sn4+ Sn2+copper, Cu cupr- Cu2+ Cu1+iron, Fe ferr- Fe3+ Fe2+Traditional (OLD) System of Nomenclature …used historically (and still some today) to name compounds w/multiple-charge cationsTo use: 1. Use Latin root of cation. 2. Use -ic ending for higher charge “ -ous “ “ lower “
3. Then say name of anion, as usual.
;
(“icky” food is good for you!)
;
(“delici
ous”
food is not good for you!)Slide35
Cu
2
S
AuNFeF2plumbic phosphide
plumbous phosphidestannic chlorideFe2+ Write formulas:Write names:cuprous sulfideauric nitrideferrous fluoridePb3P43 Pb? 4 P3–Cu
1+
Pb3P2
3 Pb? 2 P3–Au3+
SnCl
4
Sn
? 4 Cl1–S2– N3– F1– Slide36
Nomenclature -
Humor
“Ferrous Wheel”
Fe = iron (Latin = ferrum)
Fe2+ = lower oxidation state = ferrousFe3+ = higher oxidation state = ferricBaNa2
“
BaNaNa”
Fe
2+
Fe
2+
Fe2+Fe2+Fe2+Fe2+
Fe2+Fe2+What weapon can you make
from the elements nickel, potassium and iron?A KNiFeSlide37
Teacher: What is the formula for water?
Student: H, I, J, K, L, M, N, O
Teacher: That’s not what I taught you.
Student: But you said the formula for water was…H to O.
Website: Dihydrogen monoxide Information Campaign
mis
mis
“Little Johnny took a drink,
Now he shall drink no more.
For what he thought was H
2
O,Was H2SO4.”Under aged Pb walks into a bar and the bartender turns to the goldBouncer and says, “Au, get the lead out!”"H-O-H"?! WHAT'STHAT SPELL?!WATER?Slide38
Four Types of Naming
Fixed Charge Ionic Compounds
Variable Charge Ionic Compounds
Acidic CompoundsCovalent Molecules
Contain a metal with a fixed charge and a non-metal (ionic) Contain H+ with various anions (ionic when aqueous) Contain 2 or more nonmetals onlyContain a metal with a variable charge and a non-metal (ionic)Slide39
Li
3
H
1He2
C6N7O8F9Ne10Na11B5Be4H1Al13Si14
P15
S16
Cl17Ar18K19
Ca
20
Sc
21Ti22V23Cr24Mn25Fe26Co27Ni28Cu29Zn30Ga31Ge32As33Se34Br35
Kr36Rb37Sr38Y 39Zr40Nb41Mo42Tc43Ru44
Rh45Pd46Ag47Cd
48In49Sn50Sb51
Te52
I53
Xe54
Cs55
Ba56
Hf
72
Ta73
W
74Re
75
Os76
Ir77
Pt78
Au79
Hg
80
Tl81
Pb
82
Bi83
Po
84
At85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
*
W
Fixed charge cations
Variable charge cations
Elemental anions
1+
2+
3+
1-
2-
3-Slide40
Fixed Charge Exceptions
Start with Al
Go backwards down the stairs
Decrease the charge after each stairAl13Zn30
Ag473+2++
3+Slide41
Fixed Charge Compound Nomenclature
Metals (fixed charge) + NonmetalsSlide42
Fixed Charge Compounds
Compounds that contain a metal with a fixed charge
(group 1, 2, and 3, with Zn
2+
, Ag+, etc.), and a non-metalTo name these compounds, use the name of metal and thename of the non-metal with the ending replaced by the suffix –ideExamples:NaCl (Na+ Cl-)
CaS (Ca
2+ S2-)
AlI3 (Al3+ 3I-)
sodium chlor
ide
calcium sulf
idealuminum iodideSlide43
Cations and Anions
Common Simple Cations and Anions
Cation Name Anion Name*
H
+ hydrogen H - hydride Li+ lithium F - fluoride Na+ sodium Cl - chloride K+ potassium Br - bromide Cs+ cesium I - iodide Be2+ beryllium O 2- oxide Mg2+ magnesium S 2- sulfide Al3+ aluminum N 3- nitride Ag+ silver P 3- phosphide Zn2+ zinc *The root is given in color Zumdahl, Zumdahl, DeCoste, World of Chemistry
2002, page 86
EXCEPTIONSSlide44
“Perhaps one of you gentlemen would mind telling me just
what is outside the window that you find so attractive..?”
Image courtesy NearingZero.net Slide45
Fixed Charge Naming Practice
Formula Name
BaO ____________________
________________ sodium bromide
MgI2 ____________________ KCl ____________________________________ strontium fluoride________________ cesium fluoridebarium oxideNaBr
magnesium iod
ide
potassium chlor
ide
SrF
2
CsFSlide46
(NH
4
)
3NNa2Cr2O7
Al2(SO4)3NH4ClO3Mg(NO2)2BaSO4Fixed Charge Nomenclature w/Polyatomic IonsSimply insert the name of the polyatomic ion into the final nameBa2+ and SO42– Mg2+ and NO2–
NH
4+
and ClO3– Al3+ and SO42–
Na
+
and Cr2O72– NH4+ and N3– barium sulfatemagnesium nitriteammonium chloratealumnium sulfate
sodium dichromateammonium nitrideSlide47
Polyatomic Ions Quiz
phosphate
sulfate
dichromate
permanganateacetatePO43- ……………SO42- ……………Cr2O72- …………..MnO4- …………..CH3COO- …….Slide48
Variable Charge Compound Nomenclature
Metals (variable charge) + NonmetalsSlide49
Roman Numeral Review
Greek
Number
Roman Numeral
1I2II3III4
IV
5
V6
VI
7
VII
8VIII9IX10XNumberRoman Numeral
1I5V10X
50L100
CSlide50
Li
3
H
1He2
C6N7O8F9Ne10Na11B5Be4H1Al13Si14
P
15S
16Cl17Ar18K
19
Ca
20
Sc21Ti22V23Cr24Mn25Fe26Co27Ni28Cu29Zn30Ga31Ge32As33Se34Br
35Kr36Rb37Sr38Y 39Zr40Nb41Mo42Tc43Ru
44Rh45Pd46Ag47
Cd48In49Sn50Sb51
Te52
I53
Xe54
Cs
55Ba
56
Hf
72Ta
73
W74
Re75
Os76
Ir77
Pt
78Au
79
Hg80
Tl
81
Pb82
Bi
83
Po84
At
85
Rn
86
Fr
87
Ra
88
Rf
104
Db
105
Sg
106
Bh
107
Hs
108
Mt
109
Mg
12
Ce
58
Pr
59
Nd
60
Pm
61
Sm
62
Eu
63
Gd
64
Tb
65
Dy
66
Ho
67
Er
68
Tm
69
Yb
70
Lu
71
Th
90
Pa
91
U
92
Np
93
Pu
94
Am
95
Cm
96
Bk
97
Cf
98
Es
99
Fm
100
Md
101
No
102
Lr
103
La
57
Ac
89
1
2
3
4
5
6
7
*
W
Single charge cations
Variable charge cations
Elemental anions
1+
2+
3+
1-
2-
3-Slide51
Stock System
of nomenclature
Variable Charge Ionic Compounds
To name, given the formula:
1. Figure out charge on cation2. Write name of cation3. Write Roman numerals in ( ) to show cation’s chargeCompounds that contain a metal with variable charge (Pb, Sn, and the transition metals—not including Ag or Zn), and a non-metalSlide52
Variable charge Naming Practice
4. Write name of anion:
FeO Fe
? O2– Fe2
O3 2 Fe? 3 O2– CuBr Cu? Br – CuBr2 Cu? 2 Br – iron(II) oxideiron(III) oxidecopper(I) bromidecopper(II) bromideSlide53
Variable Charge Cations
Common Type II Cations
Ion Stock System Traditional System
Fe 3+ iron (III) ferric Fe 2+ iron (II) ferrous Cu 2+ copper (II) cupric Cu 1+ copper (I) cuprous Co 3+ cobalt (III) cobaltic Co 2+ cobalt (II) cobaltous Sn 4+ tin (IV) stannic Sn 2+ tin (II) stannous Pb 4+ lead (IV) plumbic Pb 2+ lead (II) plumbous Hg 2+ mercury (II) mercuric Hg2 2+ mercury (I) mercurous *Mercury (I) ions are always bonded together in pairs to form Hg2 2+ Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90Slide54
To find the formula, given the name:
2. Balance charges to write formula
cobalt (III) chloride Co
3+
Cl– tin (IV) oxide Sn4+ O2– tin (II) oxide Sn2+ O2– 1. Write symbols for the two types of ionsVariable Charge Ionic CompoundsSnOSnO2CoCl3Slide55
Naming Variable Charge Ionic Compounds
Formula Name
Hg
2
O ____________________ HgO ____________________________________ copper (II) fluoride________________ copper (I) sulfide Cr2O3 ____________________________________ lead (IV) oxidemercury (I) oxidePbO2
mercury (II) oxide
CuF2
Cu2S
chromium (III) ox
ideSlide56
Ionic Compounds with Polyatomic Ions
________________ iron (II) phosphate
________________ ammonium carbonate
________________ aluminum sulfate
V2SO3 ____________________ AgCN ____________________ Ba(ClO3)2 ____________________________________ copper (II) hydroxideFe3(PO4) 2(NH4)2CO3Al2(SO4)3vanadium (I) sulfitesilver cyanidebarium chlorate
Cu(OH)
2Slide57
Acidic Compounds
Oxysalts + H
2
O
OxyacidsSlide58
Acidic Compounds
(Nonmetals Dissolved in Water)
The prefix
hydro
- is used to represent hydrogen, followed by the root name of the nonmetal with its ending replaced by the suffix –ic acid.Examples: *HCl(aq) HBr(aq) *The name of this gas would be hydrogen monochloride if it was NOT dissolved in water.Acids(aq) without oxygenHydrochloric acid
Hydro
bromic acid
(aq) = aqueous or dissolved in waterSlide59
Acidic Compounds
Nonmetals Dissolved in Water
Start with the name of the polyatomic ion (with oxygen), and change the ending based on the following rule:
If the ion ends in “ate,” change the suffix to –ic acid. If the ion ends in “ite,” change the suffix to –ous acid.
Retain any prefixes such as “per” or “hypo” in front of the acid name. NEVER use “hydro”! Examples: HClO3(aq) HBrO(aq) Acids(aq) WITH oxygen (oxyacids)Chloric acidHypobromous acid
ClO3- = chlor
ate
BrO- = hypobromiteSlide60
An
acid
with aname ending in
An ion with aname ending in-ic-ous
-ate-iteHill, Petrucci, General Chemistry An Integrated Approach 1999, page 60Oxyacid Naming RulesSlide61
Common Oxyacid Names
The following table lists the most common families of oxy acids.
one more
oxygen atom
most“common”one lessoxygen
two fewer
oxygens
HClO
4
per
chlor
ic acidHClO3chloric acidHClO2chlorous acidHClOhypochlorous acidH2SO4sulfuric acidH2SO3sulfurous acidH3PO4phosphoric acidH3PO3phosphorous acidH3PO2hypophosphorous acidHNO3nitric acidHNO2nitrous acidSlide62
Acid Nomenclature Practice
Formula Name
HCl ____________________
HClO ____________________
________________ sulfuric acid________________ hydrofluoric acid H3N ____________________________________ periodic acidhydrochloric acidHIO4hypochlorous acid
H
2SO4
HFhydronitric acidSlide63
Covalent Compounds
Nonmetal + NonmetalSlide64
Writing Formulas of Covalent Compounds
Covalent Compounds
contain two or more non-metals
(NO METALS!) Key: FORGET CHARGES
To Name, given the formula: 1. Use Greek prefixes to indicate how many atoms of each element, but don’t use “mono” on first element (least electronegative, excluding H) 2. Add the suffix –ide to the second element (most electronegative) 1 mono 6 hexa 2 di 7 hepta 3 tri 8 octa 4 tetra 9 nona 5 penta 10 decaPrefixes to memorize!Slide65
Covalent Nomenclature Practice
EXAMPLES:
carbon dioxide
CO
dinitrogen trioxide SF6 carbon tetrachloride NI3 CO2carbon monoxideN2O3sulfur hexafluorideCCl4
nitrogen triiodideSlide66
More Practice with covalent compounds…
________________ diarsenic trisulfide
________________ sulfur dioxide
P
2O5 ____________________________________ nitrogen trihydride N2O5 ____________________ H2O ____________________As2S3SO2diphosphorus pentoxideNH3dinitrogen pentoxidedihydrogen monoxideSlide67
Naming Simple Chemical Compounds
Ionic (metal and nonmetal)
Covalent (2 nonmetals)
Metal
Formsonly onepositive ionFormsmore thanone positiveionNonmetalUse the name of elementUse elementname followedby a Romannumeral toshow the chargeFirstnonmetalSecondnonmetalBeforeelement name use a prefixto matchsubscriptUse a prefixbeforeelement name and end with ideSingleNegative IonPolyatomic IonUse the nameof the
element, butend with ide
Use thename ofpolyatomicion (ate
orIte)Slide68
fluoride
sulfide
sulfide bromide diphosphide iodide tetrachloride oxide phosphideiridium (III) calcium titanium (IV) hydrochloric acid barium trinitrogen hydrofluoric acidzinc nitrogen gold (III) sodium IrCaTiHBa
N3H
ZnNAuNa
F3
S
S2Cl(aq) Br2 P2F(aq) I2Cl4 2O3 3PIonic/variableIonic/fixedIonic/variableAcidIonic/fixedCovalentAcidIonic/fixedCovalentIonic/variableIonic/fixedOverall Nomenclature PracticeSlide69
dichromate
hydroxide
acid acetate acid sulfate cyanidenitrite chlorate phosphate acidiridium (III) calcium nitric platinum (II) bromous strontium potassium zinc manganese (IV) gold (III) sulfurous (Cr2O7)3
(OH)2
NO3 (aq)
(CH3COO)2BrO2(aq) SO4CN (NO2)2 (ClO
3
)
4
PO4 SO3 (aq) Ir2CaHPtHSrKZnMnAuH2Ionic/variableIonic/fixedAcidIonic/variableAcidIonic/fixedIonic/fixedIonic/fixedIonic/variableIonic/variableAcidIonic Nomenclature PracticeSlide70
Covalent
Ionic (M + NM)
Ionic (M + NM)
Two or more NM’s
Variable charge cation
Fixed charge cation
Roman
numeral
Polyatomic ions OK
Roman numeral
for
name onlyPolyatomic ions
Greek prefixesChargeCriss-CrossRule
RomannumeralOK
Where would you file these?
VCrO
4
BaO
CBr
4
Nb(ClO
4
)
5
SCl
2
Rb
2
SO
4
dinitrogen pentoxide
platinum (IV) iodate
ammonium chlorate
potassium iodide
nitrogen trichloride
manganese (V) sulfide
vanadium (II) chromate
VCrO
4
N
2
O
5
dinitrogen pentoxide
barium oxide
BaO
Pt(IO
3
)
4
platinum (IV) iodate
carbon tetrabromide
CBr
4
NH
4
ClO
3
ammonium chlorate
niobium (V) perchlorate
Nb(ClO
4
)
5
KI
potassium iodide
sulfur dichloride
SCl
2
NCl
3
nitrogen trichloride
rubidium sulfate
Rb
2
SO
4
Mn
2
S
5
manganese (V) sulfideSlide71
Suffixes have meaning
“-
ide
” binary compound sodium chloride (NaCl)“-ite” or “-ate” polyatomic compound sulfite (SO32-) sulfate (SO42-) “-ate
” means one more oxygen than “-ite”“-ol” alcohol methyl alcohol (methanol)“-ose” sugar sucrose“-ase” enzyme sucraseSlide72
Extra Slides
H
H
O
S
O
O
OSlide73
Compounds Containing Polyatomic Ions
Insert name of ion where it should go in the compound’s name.
Write formulas:
iron (III) nitrateammonium phosphide ammonium chloritezinc phosphate lead (II) permanganateFe(NO3)3(NH4)3PNH4ClO2Zn3(PO4)2
Pb(MnO4
)2
Fe3+NO31–NH4
1+
P
3–
NH41+ClO21–Zn2+PO43–Pb2+MnO41–33322Slide74
Write names:
(NH
4
)2S2O3
AgBrO3 (NH4)3N U(CrO4)3 Cr2(SO3)3Writing Formulas of Ionic Compoundsammonium thiosulfatesilver bromateammonium nitrideuranium (VI) chromate
chromium (III) sulfite
CrO4
2–SO32–3
3
2
Cr
U??6+3+Slide75
Element Latin root
-ic -ous
gold, Au
aur- Au3+ Au1+lead, Pb plumb- Pb4+ Pb2+tin, Sn stann- Sn4+ Sn2+copper, Cu cupr- Cu2+ Cu1+iron, Fe ferr- Fe3+ Fe2+Traditional (OLD) System of Nomenclature …used historically (and still some today) to name
compounds w/multiple-charge cations
To use: 1. Use Latin root of cation.
2. Use -ic ending for higher charge “ -ous “ “ lower “ 3. Then say name of anion, as usual.
;
(“icky” food is good for you!)
;
(“delicious” food is not good for you!)Slide76
Cu
2
S
AuNFeF2
plumbic phosphideplumbous phosphidestannic chlorideFe2+ Write formulas:Write names:cuprous sulfideauric nitrideferrous fluoridePb3P4
3 Pb
? 4 P3–
Cu1+Pb3P2
3 Pb
?
2 P
3–Au3+SnCl4Sn? 4 Cl1–S2– N3– F1– Slide77
Polyatomic Ion:
a group of atoms that stay together and have a single, overall charge
.
BrO41-
Perbromate ionBrO31-Bromate ionBrO21-Bromite ion
BrO
1-Hypo
bromite ionCO
4
2-
CO
32-Carbonate ionCO22-CO2-ClO41-ClO31-Chlorate ion
ClO21-ClO1-IO41-IO31-
Iodate ionIO2
1-IO1-
NO4
1-
NO
31-
Nitrate
ion
NO
2
1-
NO
1-
PO
5
3-
PO
4
3-
Phosph
ate
ion
PO
3
3-
PO
2
3-
SO
5
2-
SO
4
2-
Sulf
ate
ion
SO
3
2-
SO
2
2-
1 more oxygen
“normal”
1 less oxygen
2 less oxygenSlide78
Two nonmetals
Multiple-charge cation
Everything else
Roman
numeral
Polyatomic ions OK
Roman numeral
for
name
only
Polyatomic ions
Greek prefixesChargeCriss-CrossRule
RomannumeralOKWhere would you file this?
VCrO4
BaO
CBr4
Nb(ClO
4
)5
SCl
2
Rb
2
SO
4
dinitrogen pentoxide
platinum (IV) iodate
ammonium chlorate
potassium iodide
nitrogen trichloride
manganese (V) sulfide
vanadium (II) chromate
VCrO
4
N
2
O
5
dinitrogen pentoxide
barium oxide
BaO
Pt(IO
3
)
4
platinum (IV) iodate
carbon tetrabromide
CBr
4
NH
4
ClO
3
ammonium chlorate
niobium (V) perchlorate
Nb(ClO
4
)
5
KI
potassium iodide
sulfur dichloride
SCl
2
NCl
3
nitrogen trichloride
rubidium sulfate
Rb
2
SO
4
Mn
2
S
5
manganese (V) sulfideSlide79
Two nonmetals
Multiple-charge cation
Everything else
Roman
numeral
Polyatomic ions
Roman numeral
for
name
only
Polyatomic ions
Greek prefixesChargeCriss-CrossRule
RomannumeralOKWhere would you file this?
VCrO4
dinitrogen pentoxide
BaO
platinum (IV) iodate
CBr
4
ammonium chlorate
Nb(ClO
4
)
5
potassium iodide
SCl
2
nitrogen trichloride
Rb
2
SO
4
manganese (V) sulfideSlide80
Write the
total number of atoms
that make up each compound.
Write the compound formed by the following ions:
1) Al3+ S2- 2) Mg2+ PO43- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide 7) N2O5
8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH3C6H2(NO2)3 10) phosphoric acid H3PO4
Extra credit: What is the formula for
plumbic iodide?
(Hint: lead is Pb2+ or Pb4+)Slide81
Write the
total number of atoms
that make up each compound.
Write the compound formed by the following ions:
1) Al3+ S2- 2) Mg2+ PO43- When a formula is given…write the proper name. When a name is given…write the proper formula. 3) BaO 4) lithium bromide
5) Ni2S3
6) triphosphorus heptoxide 7) N2O5
8) molybdenum (VI) nitride 9) trinitrotoluene (TNT)… CH3C6H2(NO2)3 10) phosphoric acid H3PO4
Extra credit: What is the formula for
plumbic iodide?
(Hint: lead is Pb2+ or Pb4+)POP QUIZ