4.01. Ionic Compounds - San Diego Miramar Collegefaculty.sdmiramar.edu/.../04_BondingReactions/401/401_IonicCompo… · 8 4.01 Ionic and Covalent Compounds January 10 How are compounds

January 101 4.01 Ionic and Covalent Compounds

4.01. Ionic CompoundsWhat happens when electrons interact ?

Dr. Fred Omega GarcesChemistry 111, Miramar College


Regions of the Periodic Table• Nonmetals, Metals, Metalloids, Noble gases


Charge of Elemental IonsThe common charge (oxidation state) of many representative and some transition metals elements can be determine by the periodic table.


Classification of matter (compounds)Matter can be classified to mixtures and pure substances. Compounds

falls under the category of pure substances


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.


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


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


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


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

...

.

..

.. ..


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.


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.


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


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


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


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


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.


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


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.


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.


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


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.


4.01b. Ionic CompoundsWhat happens when electrons interact ?

Dr. Fred Omega GarcesChemistry 111, Miramar College


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.


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-


Extensive List of Polyatomic ions


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


... 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


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.


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


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+


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


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


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?


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?


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


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


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


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


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


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


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


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


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


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


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


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


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.

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4.01. Ionic Compounds - San Diego Miramar Collegefaculty.sdmiramar.edu/.../04_BondingReactions/401/401_IonicCompo… · 8 4.01 Ionic and Covalent Compounds January 10 How are compounds