January 101 4.01 Ionic and Covalent Compounds
4.01. Ionic CompoundsWhat happens when electrons interact ?
Dr. Fred Omega GarcesChemistry 111, Miramar College
January 102 4.01 Ionic and Covalent Compounds
Regions of the Periodic Table• Nonmetals, Metals, Metalloids, Noble gases
January 103 4.01 Ionic and Covalent Compounds
Charge of Elemental IonsThe common charge (oxidation state) of many representative and some transition metals elements can be determine by the periodic table.
January 104 4.01 Ionic and Covalent Compounds
Classification of matter (compounds)Matter can be classified to mixtures and pure substances. Compounds
falls under the category of pure substances
January 105 4.01 Ionic and Covalent Compounds
Compounds and electron interactionsCompounds can be broken up in a manner in which electrons from atoms interact
with each other.
If the electrons are mutually shared, these compounds are called Covalent Compounds.
If the electrons are transferred, these
compounds are called ionic compounds.
MoleculesCovalent
IonicCompounds
Polar-Covalent
PurePureSubstancesSubstances
Compounds
•Sharing electrons•non-metals
•transfer electrons•metal + nonmetal
•unequal sharing electrons•metals or non-metals
If the electrons areunequally shared, then
these are called polar covalent compounds.
January 106 4.01 Ionic and Covalent Compounds
Chemical Formulas RepresentationRepresentation of Molecules
Chemical Name - Word name for chemical substance.i.e., water, methane, salt, acid, ammonia, glucose
Chemical Formulas - General formula terminology for chemical substancei.e., NaCl, C6H12O6 , C2H5OH
Molecular Formula-Formula for molecular substance which indicates type of atom and number of atoms. i.e, H2O, CH4, NH3, C6H12O6
Structural Formula-Pictorial representation showing bonding connectivity of chemical substance;
Empirical Formula-Lowest ratio of atoms in chemical substance; i.e., C6H12O6 g CH2O
Formula Unit-Empirical formula for ionic substances;NaCl, KOH, Fe(NO3)2
January 107 4.01 Ionic and Covalent Compounds
Chemical Formulas RepresentationRepresentation of Molecules
Chemical Name - Word name for chemical substance.i.e., water, methane, salt, acid, ammonia, glucose
Chemical Formulas - General formula terminology for chemical substancei.e., NaCl, C6H12O6 , C2H5OH
Molecular Formula-Formula for molecular substance which indicates type of atom and number of atoms. i.e, H2O, CH4, NH3, C6H12O6
Structural Formula-Pictorial representation showing bonding connectivity of chemical substance;
Empirical Formula-Lowest ratio of atoms in chemical substance; i.e., C6H12O6 g CH2O
Formula Unit-Empirical formula for ionic substances;NaCl, KOH, Fe(NO3)2
January 108 4.01 Ionic and Covalent Compounds
How are compounds formed ?
Two main type of compounds
Octet Rule:Atoms will transfer or share electrons in order to have the same number of electrons as its closest noble gas.
Covalent compounds are formed by atoms sharing as many electrons needed to obey the Octet Rule
January 109 4.01 Ionic and Covalent Compounds
Behavior of atoms to form Compounds Two main type of compounds
Atoms will transfer or share electrons in order to have the same number of electrons as its closest noble gas
Sodium and chlorine cooperate symbiotically in electron transfer in order to have eight electrons in its valence shell.
F-F
9 p10 n
Na+Na
11 p12 n
11 p12 n
9 p10 n
11 p12 n
9 p10 n
NaF
Fluorine prefers to share its electrons to obtain 8 total in its valence shell
F
9 p10 n 9 p
10 n
F
9 p10 n
9 p10 n
F2
...
.
..
.. ..
January 1010 4.01 Ionic and Covalent Compounds
Forming Compounds from ElementsPrinciple of electrical neutrality allows prediction of formulas of ionic compounds.
Ionic bond forms between Na+ and Cl-due to electrostatic attraction between cation and anion.LATTICE ENERGY
Na Na+
[Ne] 3s1 [Ne]e-
Cl Cl-
[Ne] 3s23p5 [Ne]3S23p6
Na+ Cl-+ NaCl
Force of attraction between ions lead to ionic bond formation.
January 1011 4.01 Ionic and Covalent Compounds
NaCl - Crystalline solid in three-dimension.No such thing as a single NaCl entity. Instead a 3-D alternating lattice between Na+ and Cl - is formed.
Three-Dimensional Lattice network
Ionic compounds are all actually a lattice 3-D array arrangement.
These atoms are held together by the lattice energy (electrostatic interaction.)
The lattice energy of these ionic compound can be overcome by dissolving the solid in water.
January 1012 4.01 Ionic and Covalent Compounds
Orbital Overlap and Electron Pairing
•In the H2 molecule the two overlapping 1s orbitals are occupied by the two 1s electrons with opposite spins. (The electrons, shown as arrows, spend most of its time between the nuclei but also moves throughout the overlapping orbital region).
H2
1s 1s
H H1s 1s+
To maximize overlap in HF, half-filled 1s hydrogen orbital and Fluorine 2p orbital overlap along the long axis of the 2p orbital of fluorine. (The 2px
orbital is shown; the other two 2p orbitals of fluorine are not shown).
In F2, the half-filled 2px orbital of each fluorine faces end to end towards each other and overlap. The overlap of the orbitals creates the bond between the two fluorine atoms.
H1s
F 2p
FH 2p1s
F 2p
F 2p
FF 2p2p
January 1013 4.01 Ionic and Covalent Compounds
IA IIA IIIA IVA VA VIA VIIA VIIIAException Boron
(will not form ion)CarbonSilicon
+1 +2 +3 -3 -2 -1 0ns 1 ns 2 ns 2 np 1 ns 2 np 2 ns 2 np 3 ns 2 np 4 ns 2 np 5 ns 2 np 6
Cation Cation Cation Anion Anion Anion Neutral
Oxidation numbers (common charge)Prediction of common charge of ion.
From Periodic TableAtoms will lose or gain e- to have complete set of electrons
in its outer most orbital.
Metals will lose electrons
to form cations
Non-metals will gain
electrons to form anions
January 1014 4.01 Ionic and Covalent Compounds
Atoms Polyatomic Action /anions vs. Action /anions
H+ F- NH4+ NO3
-
Li+ Cl- Hg22+ SO4
2-
Na+ Br- PO43-
K+ I- CO32-
Mg+2 O 2 - Cr2O7 2-
Al+3 S 2 - OH-
Ion-charge atoms / group atoms
January 1015 4.01 Ionic and Covalent Compounds
Atoms Polyatomic Action /anions vs. Action /anions
H+ F- NH4+ NO3
-
Li+ Cl- Hg22+ SO4
2-
Na+ Br- PO43-
K+ I- CO32-
Mg+2 O 2 - Cr2O7 2-
Al+3 S 2 - OH-
Ion-charge atoms / group atoms
January 1016 4.01 Ionic and Covalent Compounds
Ionic Compound: KFMetals (or cation) involved
Chemical formula - Principle of electrical neutrality is applied in order to predict formulas of ionic compound.
KFF F -K +K
Example 1: Potassium and Fluorine
Potassium and fluorine combine in a 1:1 ratio because potassium (K) is positive one (+1) and fluorine (F) is negative one (-1). Only in a 1:1 combination will the charges cancel each other.
January 1017 4.01 Ionic and Covalent Compounds
Principle of Electrical NeutralityWhen elements combine to form compounds, the principle of electrical neutrality allows prediction of formulas of the ionic compound.
Basic idea:
Sum of the charges must add to zero. That is the sum of the cation charge and the sum of the anion charge
must cancel each other so that the compound form is neutral.
S cation (charges) = S anion (charges)
Mm+ + Xn- g Mn Xm
January 1018 4.01 Ionic and Covalent Compounds
Criss-Cross method
Barium and nitrogen combine in a 3 : 2 ratio because barium (B) is positive three (+2) and nitrogen (N) is negative three (-3). Only in a 3:2 combination will the charges cancel each other.
Example 1: Barium and nitrogen
Ba3N2N3-Ba2+
N N3-Ba2+Ba
1. Write the symbols for the cation and the anion.2. Use a superscript for the charge (+/-) of each ion.3. Criss-cross step:
• Criss-cross the superscript of the cation to the subscript position of the anion (disregard the positive sign).
• Criss-cross the superscript of the anion to the subscript position of the cation (disregard the negative sign).
4. Remove the superscript from both cation and anion.5. If possible, divide the subscripts by their greatest common factor to
reduce to simplest whole ratio.
January 1019 4.01 Ionic and Covalent Compounds
Ionic Compound: Al2S3
Aluminum and sulfur combine in a 2 : 3 ratio because aluminum (Al) is positive three (+3) and sulfur (S) is negative two (-2). Only in a 2:3 combination will the charges cancel each other.
Example 2: Aluminum and Sulfur
Al2S
3S-2Al +3
S S-2
Al +3Al
Writing the formula for an ionic compound involves writing the cation and anion ration so that there is a net zero
charge or the compound is electrical neutrality. That is sum of the charges of all ions in the compound equals zero.
January 1020 4.01 Ionic and Covalent Compounds
Predicting Formulas of Ionic Compounds
Cation + AnionElectrostatic attraction g electrically neutralityRepresent ionic compound by empirical formula
Na + I2 -in waterg Na+ + 2 I-
Na+ + Na+ + I- + I- g NaI + NaI
G-IA G-VIIA -in waterg NaI Sodium Iodide
Similarly,
Na + O2 g 4 Na+ + 2O-2 g Na2O Sodium oxideCo + SO42- g 2 Co+3 + 3 SO42- g Co2 (SO4)3 Cobalt(III) sulfate
Side notes: Diatomic molecules: H2, N2, O2, F2, Cl2, Br2, I2
January 1021 4.01 Ionic and Covalent Compounds
Chemical Formula SummaryCompounds can be formed by elements combining and
i) electron transfer occurs, here ionic compounds forms.ii) electrons are shared between elements
if there is mutually sharing, covalent compounds forms if there is unequal sharing, polar covalent compounds forms
Compounds are always electrically neutralFor ionic compounds,
“Principle of Electrical Neutrality” is obeyed.For covalent compounds,
There is no charge with the elements in the compoundelectrons are shared. Electrical Neutrality does not apply.
Ionic substances will dissociate in water into their ionsCovalent compounds stays intact in water as their molecules.
January 1022 4.01 Ionic and Covalent Compounds
4.01b. Ionic CompoundsWhat happens when electrons interact ?
Dr. Fred Omega GarcesChemistry 111, Miramar College
January 1023 4.01 Ionic and Covalent Compounds
Charge of Elemental Ions; Revisited
The common charge (oxidation state) of many representative and some transition metals elements can be determine by the periodic table.
January 1024 4.01 Ionic and Covalent Compounds
Most common polyatomic ionsExample of polyatomic ions
Previously we discussed how ions
are formed from elements. Ions can
also be formed from group of atoms
that are covalently held together.
These group of atoms which are
charged are called polyatomic ions.
Top thirteen of this ions are
summarized here.
CationsAmmonium NH4
+
Polyatomic anions12. Chromate CrO4
2-
11. Permanganate MnO4-
10. Perchlorate ClO4-
9. Dichromate Cr2O72-
8. Acetate CH3CO2-
7. Carbonate CO32-
6. Phosphate PO43-
5. Sulfate SO42-
4. Nitrate NO3-
3. Cyanide CN-
2. Peroxide O22-
1. Hydroxide OH-
January 1025 4.01 Ionic and Covalent Compounds
Extensive List of Polyatomic ions
January 1026 4.01 Ionic and Covalent Compounds
Common polyatomic ionsCations : ammonium NH4
+ & Hg22+
Anions (charge)-
-1: hydroxide, OH-; cyanide, CN- ; nitrate, NO3-
-2: carbonate, CO32-, chromate CrO4
2-, Dichromate Cr2O72-, sulfate SO4
2-
-3 : phosphate, PO43-
Polyatomic oxy-ions: Chlorate, bromate, iodinate, sulfate, nitrate, phosphate, chromateSome form four anions
chlorate: perchlorate g chlorate g chlorite g hypochlorite
Some form only two oxy anions
sulfate: sulfate ® sulfite
Some form only on oxy anion
carbonate: carbonate
January 1027 4.01 Ionic and Covalent Compounds
... helpful hints about anions-ide -ate -ite
elemental ions oxy ions oxy ionsX-m XOn
-m XOn-1-m
P-3 phosphide PO4-3 phosphate PO3
-3 phosphite
As-3 arsenide AsO4-3 arsenate AsO3
-3 arsenite
S-2 sulfide SO4-2 sulfate SO3
-2 sulfite
Se-2 selenide SeO4-2 selenate SeO3
-2 selenite
N-3 nitride NO3- nitrate NO2
- nitrite
Cl- chloride ClO3- chlorate ClO2
- chlorite
Br- bromide BrO3- bromate BrO2
- bromite
I- iodide IO3- iodate IO2
- iodite
January 1028 4.01 Ionic and Covalent Compounds
Chemical Nomenclature:Ways Compounds Ionic and Covalent Forms
Ionic Compounds: Type I & IIBinary Form - Composed from two different elements bonding.
Polyatomic Form - Compounds with some part of substituents clustered together covalently with some charge.
Covalent Compounds: Type IIICombination of nonmetal atoms sharing electrons.
January 1029 4.01 Ionic and Covalent Compounds
Type I, II and IIIIonic : Type I & II
Type I : Metal - nonmetalmetal has a definite oxidation state.Ca g Ca+2, K g K+, Al g Al+3, Zn g Zn+2
Type II : Metal(Ox#) - nonmetalmetal has a variable oxidation state.Cu g Cu+2 or Cu+ , Cr g Cr+2 or Cr+4
Molecular: Type IIIType III : (prefix1)nonMetal1 - (prefix2)nonMetal2
Elements have no chargecovalent type of compounds
January 1030 4.01 Ionic and Covalent Compounds
Determining Type (I, II, III) of Compound
Show me the metal !!Type I or Type II
Is the metalGroup I, II or Al,Zn, Cd, Ag, and
Type III
Type I
Yes
YesN o N ometal-nonmetal
metal(Ox.#)-nonmetal
Type II
(Prefix)nonmetal1 (Prefix)nonmetal2
NH4+
January 1031 4.01 Ionic and Covalent Compounds
Type I, II and IIIType Anion elemental Anion polyatomic
I (Metal – nonMetal)
Cation; Rep MetalCation - Anion
Cation - Anion(ide)
Al2O3; Aluminum oxideAg2S; Silver sulfide
Cation - Anion
Cd(NO3)2: cadmium nitrate(NH4)2SO4: ammonium sulfate
II (Metal - nonMetal)
(Transition) metalCation (O St #) - Anion
Cation ; 3rd row and lower
Old method (Fe+3 vs Fe+2)higher ox.st. -iclower ox. st. -ous
Cation (oxidation st.) Anion(ide)
FeCl3; Iron(III) chloridePbS2; Lead(IV) sulfide
Cation(ic) - Anion(ide)FeBr3 ; Ferrric bromide
Iron(III) bromideCation(ous) – Anion(ide)Fe3N2 ; Ferrrous nitride
Iron(II) nitride
Cation (oxidation st.) Anion
Sn(C2H3O2)2; Tin(II) acetateAu3PO3; Gold(I) phosphite
Cation(ic) – Polyatomic anionFe(NO3)3 ; Ferrtic nitrate
Iron(III) nitrateCation(ous) – Polyatomic anionFe(NO2)2 ; Ferrrous nitrite
Iron(II) nitrite
IIIMolecular compounds -
Compounds contains nonmetal
(Prefix) nonmetal1 -(Prefix ) nonmetal2
(Prefix) nonmetal 1 - (Prefix) nonmetal 2 (ide)• Prefixes are indication of the number of atoms:
mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-• order of naming nonmetal 1 & nonmetal (ide)2
nonmetal 1 is to the left and bottom of nonmetal 2based on it is named first in the nomenclature scheme.
Si - C - As - P - N - H - Se - S - I - Br - Cl - O - F• S & 3 O forms SO3 ; Sulfur trioxide• 2 P & 5 O forms P2O5 ; Diphosphorus pentoxide
January 1032 4.01 Ionic and Covalent Compounds
Type I, II and IIIType Anion elemental Anion polyatomic
I (Metal – nonMetal)
Cation; Rep MetalCation - Anion
Cation - Anion(ide)
Al2O3; Aluminum oxideAg2S; Silver sulfide
Cation - Anion
Cd(NO3)2: cadmium nitrate(NH4)2SO4: ammonium sulfate
II (Metal - nonMetal)
(Transition) metalCation (O St #) - Anion
Cation ; 3rd row and lower
Old method (Fe+3 vs Fe+2)higher ox.st. -iclower ox. st. -ous
Cation (oxidation st.) Anion(ide)
FeCl3; Iron(III) chloridePbS2; Lead(IV) sulfide
Cation(ic) - Anion(ide)FeBr3 ; Ferrric bromide
Iron(III) bromideCation(ous) – Anion(ide)Fe3N2 ; Ferrrous nitride
Iron(II) nitride
Cation (oxidation st.) Anion
Sn(C2H3O2)2; Tin(II) acetateAu3PO3; Gold(I) phosphite
Cation(ic) – Polyatomic anionFe(NO3)3 ; Ferrtic nitrate
Iron(III) nitrateCation(ous) – Polyatomic anionFe(NO2)2 ; Ferrrous nitrite
Iron(II) nitrite
IIIMolecular compounds -
Compounds contains nonmetal
(Prefix) nonmetal1 -(Prefix ) nonmetal2
(Prefix) nonmetal 1 - (Prefix) nonmetal 2 (ide)• Prefixes are indication of the number of atoms:
mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-• order of naming nonmetal 1 & nonmetal (ide)2
nonmetal 1 is to the left and bottom of nonmetal 2based on it is named first in the nomenclature scheme.
Si - C - As - P - N - H - Se - S - I - Br - Cl - O - F• S & 3 O forms SO3 ; Sulfur trioxide• 2 P & 5 O forms P2O5 ; Diphosphorus pentoxide
January 1033 4.01 Ionic and Covalent Compounds
Distinguishing between elemental & polyatomic ions
A aluminum sulfateB Palladium (II) chromateC tungsten(IV) hypochloriteD ammonium bisulfateE Tetraphosphorus octaoxideF cobalt(III) phosphideG calcium phosphateH cesium acetateI xenon dioxideJ silver permanganateK platinum (IV) periodateL magnesium phosphiteM chlorine monobromideN Mercury(I) tellurideO Cadmium biphosphate
1 1 Mg(ClO3)2 214 CuBr2
A2 HClO 115 KMnO4
33 N2O4 116 Na2O2
1 4 NH4NO2 317 XeF4
1 5 Na3As 218 HgCO3
A6 HI A19 H2SO4
1 7 NaHCO3 1 20 NH4ClO4
1 8 Zn(C2H3O2)2 1 21 Li2Se
29 V3N 1 22 CdCO3
210 PbTe2 3 23 H2O2
1 11 NaHSO3 1 24 (NH4)2S
A12 HC2H3O2 1 24 FrF
313 SO3 226 NiO2
Identify: - Type-I
- Type-II
- Type-III -
- Acids
Which
Type-I
and
Type-II
contains
polyatomic
ions?
January 1034 4.01 Ionic and Covalent Compounds
Distinguishing between elemental & polyatomic ions
1 Mg(ClO3)2 2 CuBr2
A HClO 1 KMnO4
3 N2O4 1 Na2O2
1 NH4NO2 3 XeF4
1 Na3As 2 HgCO3
A HI A H2SO4
1 NaHCO3 1 NH4ClO4
1 Zn(C2H3O2)2 1 Li2Se
2 V3N 1 CdCO3
2 PbTe2 3 H2O2
1 NaHSO3 1 (NH4)2S
A HC2H3O2 1 FrF
3 SO3 2 NiO2
1 aluminum sulfate2 palladium (II) chromate2 tungsten(IV) hypochlorite1 ammonium bisulfate3 tetraphosphorus octaoxide2 cobalt(III) phosphide1 calcium phosphate1 cesium acetate3 xenon dioxide1 silver permanganate2 platinum (IV) periodate2 manganese(IV) phosphite3 chlorine monobromide2 mercury(I) telluride1 cadmium biphosphate
13 Type I, 5 type II, 4 type III 4 Acids = 26 6 Type I, 5 type II, 4 type III
Identify: 1- Type-I
2- Type-II
3- Type-III -
A- Acids
Which
Type-I
and
Type-II
contains
polyatomic
ions?
January 1035 4.01 Ionic and Covalent Compounds
Example: Type-IGiven the Chem Formula provide the name
Name Type I: Binary Metal - nonmetal(ide)
SrSe Strontium selenide
Mg3N2 Magnesium nitrideLi2O Lithium oxide
Chem Formula Type I: Polyatomic Metal - polyatomic
SrSO4 Strontium sulfateMg3(PO4 )2 Magnesium phosphateLiClO4 Lithium perchlorate
January 1036 4.01 Ionic and Covalent Compounds
Example: Type-IGiven the Chem Formula provide the name
Name Type I: Binary Metal - nonmetal(ide)
SrSe Strontium selenide
Mg3N2 Magnesium nitrideLi2O Lithium oxide
Chem Formula Type I: Polyatomic Metal - polyatomic
SrSO4 Strontium sulfateMg3(PO4 )2 Magnesium phosphateLiClO4 Lithium perchlorate
January 1037 4.01 Ionic and Covalent Compounds
Example: Type-I
Given the name provide the chemical formula
Name Type I: Binary Metal - nonmetal(ide)potassium sulfide
Elemental symbol K & SCharge of ions K (+1) S(-2)Criss-Cross K(2) S(1) g K2S
Chem Formula Type I: Polyatomic Metal - polyatomicCadmium bisulfite
Elemental symbol Cd & HSO3Charge of ions Cd (+2) HSO3(-1)Criss-Cross Cd(1) HSO3(2) g Cd(HSO3)2
January 1038 4.01 Ionic and Covalent Compounds
Example: Type-IGiven the name provide the chemical formula
Name Type I: Binary Metal - nonmetal(ide)potassium sulfide
Elemental symbol K & SCharge of ions K (+1) S(-2)Criss-Cross K(2) S(1) g K2S
Chem Formula Type I: Polyatomic Metal - polyatomicCadmium bisulfite
Elemental symbol Cd & HSO3Charge of ions Cd (+2) HSO3(-1)Criss-Cross Cd(1) HSO3(2) g Cd(HSO3)2
January 1039 4.01 Ionic and Covalent Compounds
Example: Type-IIGiven the Chem Formula provide the name
Name Type II: Binary Metal(Ox.#) - nonmetal(ide)Mn3N2 Elemental symbol Mn (3) & N (2)
Reverse Criss-Cross Mn (2) & N (3)Ox. State of metal Ox St = 2; Mn(II) Name of Chemical Manganese(II) nitride
Chem Formula Type II: Polyatomic Metal(Ox#) - polyatomicMn(NO2)2 Elemental symbol Mn (1) & NO2 (2)
Reverse Criss-Cross Mn (2) & NO2 (1)Ox. State of metal Ox St= 2; Mn(II) Name of Chemical Manganese(II) nitrite
January 1040 4.01 Ionic and Covalent Compounds
Example: Type-IIGiven the Chem Formula provide the name
Name Type II: Binary Metal(Ox.#) - nonmetal(ide)Mn3N2 Elemental symbol Mn (3) & N (2)
Reverse Criss-Cross Mn (2) & N (3)Ox. State of metal Ox St = 2; Mn(II) Name of Chemical Manganese(II) nitride
Chem Formula Type II: Polyatomic Metal(Ox#) - polyatomic
Mn(NO2)2 Elemental symbol Mn (1) & NO2 (2)
Reverse Criss-Cross Mn (2) & NO2 (1)
Ox. State of metal Ox St= 2; Mn(II) Name of Chemical Manganese(II) nitrite
January 1041 4.01 Ionic and Covalent Compounds
Example: Type-IIGiven the name provide the chemical formula
Name Type II: Binary Metal - nonmetal(ide)
Iron(II) sulfide Elemental symbol Fe & S
Charge of ions Fe(+2) S(-2)
Criss-Cross Fe(2) S(2) g Fe2S2
Reduce ratio FeS
Name Type II: Polyatomic Metal - polyatomic
Tin(IV) sulfite Elemental symbol Sn & SO3
Charge of ions Sn(+4) SO3(-2)
Criss-Cross Sn(2) SO3(4) g Sn2(SO3)4
Reduce ratio Sn(SO3)2
January 1042 4.01 Ionic and Covalent Compounds
Example: Type-IIGiven the name provide the chemical formula
Name Type II: Binary Metal - nonmetal(ide)
Iron(II) sulfide Elemental symbol Fe & S
Charge of ions Fe(+2) S(-2)
Criss-Cross Fe(2) S(2) g Fe2S2
Reduce ratio FeS
Name Type II: Polyatomic Metal - polyatomic
Tin(IV) sulfite Elemental symbol Sn & SO3
Charge of ions Sn(+4) SO3(-2)
Criss-Cross Sn(2) SO3(4) g Sn2(SO3)4
Reduce ratio Sn(SO3)2
January 1043 4.01 Ionic and Covalent Compounds
Example: Type-IIIGiven the Chem Formula determine the name
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)N2O2 Elemental symbol N (2) & O (2)
Prefix dinitrogen & dioxideName of Chemical dinitrogen dioxide
XeF2 Elemental symbol Xe (1) & F(2)Prefix monoxenon & difluorideName of Chemical xenon difluoride
P4Se10 Elemental symbol P (4) & Se(10)Prefix tetraphosphorus & decaselenideName of Chemical tetraphosphorus decaselenide
January 1044 4.01 Ionic and Covalent Compounds
Example: Type-IIIGiven the Chem Formula determine the name
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)N2O2 Elemental symbol N (2) & O (2)
Prefix dinitrogen & dioxideName of Chemical dinitrogen dioxide
XeF2 Elemental symbol Xe (1) & F(2)Prefix monoxenon & difluorideName of Chemical xenon difluoride
P4Se10 Elemental symbol P (4) & Se(10)Prefix tetraphosphorus & decaselenideName of Chemical tetraphosphorus decaselenide
January 1045 4.01 Ionic and Covalent Compounds
Example: Type-IIIGiven the name determine the chemical formula
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)
Diboron trisulfide Elemental symbol B & S
Prefix for atoms B(2) & S(3)
Chemical formula B2S3
Silicon tricarbide Elemental symbol Si & C
Prefix for atoms Si(1) & C(3)
Chemical formula SiC3
Iodine monochloride Elemental symbol I & Cl
Prefix for atoms I(1) & Cl(1)
Chemical formula ICl
January 1046 4.01 Ionic and Covalent Compounds
Example: Type-IIIGiven the name determine the chemical formula
Name Type III: (prefix1)nonMetal1 - (prefix2)nonMetal2(ide)
Diboron trisulfide Elemental symbol B & S
Prefix for atoms B(2) & S(3)
Chemical formula B2S3
Silicon tricarbide Elemental symbol Si & C
Prefix for atoms Si(1) & C(3)
Chemical formula SiC3
Iodine monochloride Elemental symbol I & Cl
Prefix for atoms I(1) & Cl(1)
Chemical formula ICl
January 1047 4.01 Ionic and Covalent Compounds
SummaryAn ionic compound is named with cation first and anion last. For metals that can form more than one ion, the charge is shown with a Roman numerical. For example, copper forms the mono-cation Cu+ and the di-cation, Cu2+, these are distinguished from each other in their chemical name as copper(I) and copper (II). Oxyanions (or anions with two kinds of element one of which is oxygen) have suffixes, and some have prefixes attached to their element root name to indicate the number of oxygen atoms. For example the oxy anion containing sulfur & oxygen may form the following anions, hyposulfite SO2
2-, sulfite SO32-, sulfate SO4
2-, and persulfate SO5
2- . Binary covalent compounds nomenclature consist of writing the most electropositive elements first proceeded by a prefix which indicates the number of atoms , I.e., di-2, tri-3, tetra-4 and so on. The second more electronegative element is written next which also is proceeded by the prefix which indicates the number of atoms. For the second element, a “mono” prefix must always be written if there is only one atom in the chemical formula. i.e., carbon monoxide for CO.
Top Related