chapter 7 chemical formulas and bonding

LABORATORY CHEMISTRY

CHAPTER 7 1

Chapter 7Chapter 7chemical formulas and bondingchemical formulas and bonding


CHAPTER 7 2

CHAPTER 7:CHAPTER 7:CHEMICAL FORMULAS AND BONDINGCHEMICAL FORMULAS AND BONDINGIONIC BONDINGIONIC BONDING

DESCRIBE THE DISTINGUISHING DESCRIBE THE DISTINGUISHING CHARACTERISTICS OF AN IONIC BONDCHARACTERISTICS OF AN IONIC BOND

DESCRIBE SOME PROPERTIES OF IONIC DESCRIBE SOME PROPERTIES OF IONIC COMPOUNDSCOMPOUNDS

EXPLAIN THE OCTET RULEEXPLAIN THE OCTET RULE DRAW LEWIS DOT DIAGRAMS TO SHOW DRAW LEWIS DOT DIAGRAMS TO SHOW

THE VALENCE ELECTRONS OF AN ATOMTHE VALENCE ELECTRONS OF AN ATOM DISTINGUISH AMONG ANIONS, CATIONS, DISTINGUISH AMONG ANIONS, CATIONS,

AND POLYATOMIC IONSAND POLYATOMIC IONS


CHAPTER 7 3

IONIC BONDINGIONIC BONDING

IONIC BONDS AND IONIC IONIC BONDS AND IONIC COMPOUNDSCOMPOUNDS– STATIC ELECTRICAL ATTRACTION IS THE BASIS STATIC ELECTRICAL ATTRACTION IS THE BASIS

FOR IONIC BONDSFOR IONIC BONDS IN AN IONIC BOND, A POSITIVELY CHARGED ION IS IN AN IONIC BOND, A POSITIVELY CHARGED ION IS

ATTRACTED TO A NEGATIVELY CHARGED ION.ATTRACTED TO A NEGATIVELY CHARGED ION.– A COMPOUND THAT IS COMPOSED ENTIRELY OF A COMPOUND THAT IS COMPOSED ENTIRELY OF

IONS IS CALLED ANIONS IS CALLED AN IONIC COMPOUND. IONIC COMPOUND. ALL IONIC COMPOUNDS CONSIST OF POSITIVELY ALL IONIC COMPOUNDS CONSIST OF POSITIVELY

CHARGED IONS, CALLEDCHARGED IONS, CALLED CATIONSCATIONS, , AND NEGATIVELY AND NEGATIVELY CHARGED IONS, CALLEDCHARGED IONS, CALLED ANIONSANIONS..

IONIC COMPOUNDS ARE ELECTRICALLY NEUTRAL, SO IONIC COMPOUNDS ARE ELECTRICALLY NEUTRAL, SO THATTHAT THE ELECTRICAL CHARGES OF THE CATIONS AND THE ELECTRICAL CHARGES OF THE CATIONS AND THE ANIONS MUST BALANCETHE ANIONS MUST BALANCE


CHAPTER 7 4


– PROPERTIES OF IONIC COMPOUNDS:PROPERTIES OF IONIC COMPOUNDS: HIGH MELTING POINTSHIGH MELTING POINTS BRITTLEBRITTLE DISSOLVE IN WATER (SOLUBLE)DISSOLVE IN WATER (SOLUBLE)

– SEPARATED IONS MOVE ABOUT FREELY IN WATER, WHICH SEPARATED IONS MOVE ABOUT FREELY IN WATER, WHICH MAKES THEM GOOD CONDUCTORS OF ELECTRICITYMAKES THEM GOOD CONDUCTORS OF ELECTRICITY

MOLTEN IONIC COMPOUNDS ARE GOOD MOLTEN IONIC COMPOUNDS ARE GOOD CONDUCTORS OF ELECTRICITYCONDUCTORS OF ELECTRICITY

DO NOT CONDUCT ELECTRICITY IN THE SOLID DO NOT CONDUCT ELECTRICITY IN THE SOLID STATESTATE

– IONS ARE HELD IN POSITION AND CANNOT MOVE FREELYIONS ARE HELD IN POSITION AND CANNOT MOVE FREELY


CHAPTER 7 5

IONIC BONDINGIONIC BONDING THE OCTET RULETHE OCTET RULE

– ATOMS TEND TO GAIN, LOSE, OR SHARE ELECTRONS ATOMS TEND TO GAIN, LOSE, OR SHARE ELECTRONS IN ORDER TO ACQUIRE A FULL SET OF VALENCE IN ORDER TO ACQUIRE A FULL SET OF VALENCE ELECTRONS.ELECTRONS.

MOST ATOMS HAVE 8 VALENCE ELECTRONS, OR AN MOST ATOMS HAVE 8 VALENCE ELECTRONS, OR AN OCTET, IN A FULL SET.OCTET, IN A FULL SET.

– THE EXCEPTIONS INCLUDE HYDROGEN AND HELIUM, THE THE EXCEPTIONS INCLUDE HYDROGEN AND HELIUM, THE FIRST PRINCIPAL ENERGY LEVEL IS FULL WITH ONLY 2 FIRST PRINCIPAL ENERGY LEVEL IS FULL WITH ONLY 2 ELECTRONSELECTRONS


CHAPTER 7 6


Na Na+

- -

Na

[Ne] 3s1

Na+

[Ne]

A SODIUM ATOM READILY LOSES ONE OF ITS ELECTRONS


CHAPTER 7 7


Cl Cl--

-

THE CHLORINE ATOM READILY GAINS AN ELECTRON

Cl[Ne] 3s2, 3p5 Cl-

[Ne] 3s2, 3p6

-


CHAPTER 7 8


THE OCTET RULETHE OCTET RULE– ATOMS TEND TO GAIN, LOSE, OR SHARE ATOMS TEND TO GAIN, LOSE, OR SHARE

ELECTRONS IN ORDER TO ACQUIRE A ELECTRONS IN ORDER TO ACQUIRE A FULL SET OF VALENCE ELECTRONS.FULL SET OF VALENCE ELECTRONS.

MOST ATOMS HAVE 8 VALENCE MOST ATOMS HAVE 8 VALENCE ELECTRONS, OR AN OCTET, IN A FULL SET.ELECTRONS, OR AN OCTET, IN A FULL SET.

– THE EXCEPTIONS INCLUDE HYDROGEN AND THE EXCEPTIONS INCLUDE HYDROGEN AND HELIUM, THE FIRST PRINCIPAL ENERGY LEVEL IS HELIUM, THE FIRST PRINCIPAL ENERGY LEVEL IS FULL WITH ONLY 2 ELECTRONSFULL WITH ONLY 2 ELECTRONS


CHAPTER 7 9


Cl--Na+

IN BOTH CASES THE ION THAT FORMS HAS THE ELECTRON CONFIGURATION OF A NOBLEGAS

Ne Ar


CHAPTER 7 10

IONIC BONDINGIONIC BONDING LEWIS DOT DIAGRAMSLEWIS DOT DIAGRAMS

– GILBERT LEWIS (1875-1946)GILBERT LEWIS (1875-1946)– VALENCE ELECTRONS ARE REPRESENTED AS DOTS VALENCE ELECTRONS ARE REPRESENTED AS DOTS

PLACED AROUND THE ELEMENT SYMBOL (SMALL x’s PLACED AROUND THE ELEMENT SYMBOL (SMALL x’s AND o’s CAN ALSO BE USED INSTEAD OF DOTS)AND o’s CAN ALSO BE USED INSTEAD OF DOTS)

– THE DOTS ARE PLACED ALONE OR IN PAIRS AROUND THE DOTS ARE PLACED ALONE OR IN PAIRS AROUND THE ELEMENT SYMBOL.THE ELEMENT SYMBOL.

TRADITIONALLY, THE DOTS ARE WRITTEN ALONG THE SIDES TRADITIONALLY, THE DOTS ARE WRITTEN ALONG THE SIDES OF AN IMAGINARY BOX, AND NO MORE THAN TWO DOTS ARE OF AN IMAGINARY BOX, AND NO MORE THAN TWO DOTS ARE PLACED ON ANY SIDE OF OF THE BOXPLACED ON ANY SIDE OF OF THE BOX

– LEWIS DOT MAY ALSO BE USED TO ILLUSTRATE HOW LEWIS DOT MAY ALSO BE USED TO ILLUSTRATE HOW ELECTRONS ARE REARRANGED DURING CHEMICAL ELECTRONS ARE REARRANGED DURING CHEMICAL REACTIONSREACTIONS


CHAPTER 7 11

IONIC BONDINGIONIC BONDING ns1 an

d ns2

np1

np2

np3

np4

np5

np6


CHAPTER 7 12

LEWIS DOT DIAGRAMSLEWIS DOT DIAGRAMS

ELEMENTELECTRON

CONFIGURATIONLEWIS DOTDIAGRAM

Li [He]2s1 Li

Be [He]2s2 Be

B [He]2s2,2p1 B

C [He]2s2, 2p2 C

N [He]2s2, 2p3 N

O [He]2s2, 2p4 O


CHAPTER 7 13



CHAPTER 7 14

IONIC BONDINGIONIC BONDING TYPES OF IONSTYPES OF IONS

– MONOATOMIC IONS (“ONE-ATOM” IONS)MONOATOMIC IONS (“ONE-ATOM” IONS) FORMED FROM ONE (1) ATOMFORMED FROM ONE (1) ATOM MONOATOMIC CATIONSMONOATOMIC CATIONS

– METALS THAT HAVE ONLY ONE KIND OF CATIONMETALS THAT HAVE ONLY ONE KIND OF CATION THESE METALS HAVE ONLY ONE POSSIBLE OXIDATION NUMBER THESE METALS HAVE ONLY ONE POSSIBLE OXIDATION NUMBER

AND THEREFORE CAN ONLY BOND IN ONE WAYAND THEREFORE CAN ONLY BOND IN ONE WAY BECAUSE OF THIS THE NAMING PROCEDURE FOR COMPOUNDS BECAUSE OF THIS THE NAMING PROCEDURE FOR COMPOUNDS

WITH MONOATOMIC CATIONS IS WITH MONOATOMIC CATIONS IS “STRAIGHT FORWARD”:“STRAIGHT FORWARD”:– THE METAL NAME IS ALWAYS THE FIRST WORD IN THE THE METAL NAME IS ALWAYS THE FIRST WORD IN THE

COMPOUNDCOMPOUND– METALS THAT HAVE MORE THAN ONE KIND OF CATIONMETALS THAT HAVE MORE THAN ONE KIND OF CATION

THESE METALS HAVE MORE THAN ONE OXIDATION NUMBER THESE METALS HAVE MORE THAN ONE OXIDATION NUMBER AND THEREFORE CAN BOND IN MORE THAN ONE WAYAND THEREFORE CAN BOND IN MORE THAN ONE WAY

BECAUSE OF THIS THE NAMING PROCEDURE MUST REFLECT THE BECAUSE OF THIS THE NAMING PROCEDURE MUST REFLECT THE SPECIFIC CATION BEING USED.SPECIFIC CATION BEING USED.

– POLYATOMIC IONS (“MANY- ATOMS”)POLYATOMIC IONS (“MANY- ATOMS”) FORMED FROM MORE THAN ONE ATOMFORMED FROM MORE THAN ONE ATOM

– THESE ARE GENERALLY ANIONS !THESE ARE GENERALLY ANIONS ! ( (THE EXCEPTION IS THE EXCEPTION IS AMMONIUM NHAMMONIUM NH44 ) )


CHAPTER 7 15

LABORATORY CHEMISTRYOXIDATION REFERENCE CHART

COMMON METAL MONOATOMIC CATIONS WITH ONE PRIMARY OXIDATION NUMBER

(Name of the metal + Name of the NonMetal….”-ide”)

1+ 2+ 3+ 4+ Cs cesium Ba barium Al aluminum Ge germanium Li lithium Cd cadmium B boron Th thorium H hydrogen Ca calcium Ga gallium Zr zirconium K potassium Sr strontium Ce cerium Rb rubidium Zn zinc Au gold (also has a 1+) Na sodium Mg magnesium Ag silver


CHAPTER 7 16


– MONOATOMIC ANIONSMONOATOMIC ANIONS TO NAME THE MONOATOMIC….REPLACE TO NAME THE MONOATOMIC….REPLACE

THE SUFFIX OF THE ELEMENT NAME WITH THE SUFFIX OF THE ELEMENT NAME WITH THE SUFFIX THE SUFFIX “-IDE”“-IDE”

CHLORCHLORINE INE ATOM ATOM CHLORCHLORIDE IDE IONION

OXOXYGENYGEN ATOM ATOM OX OXIDEIDE ION ION SULFSULFURUR ATOM ATOM SULF SULFIDEIDE ION ION


CHAPTER 7 17


COMMON NONMETAL MONOATOMIC ANIONS

1- 2- 3- 4-/ 4+ F fluorine O oxygen N nitrogen* C carbon* Cl chlorine S sulfur* P phosphorus* Si silicon* Br bromine Se selenium* As arsenic* I iodine Te tellurium* At astatine H hydrogen* (hydride)

* denotes elements that have both metal and nonmetal properties


CHAPTER 7 18


1+(-ous) 2+(-1+(-ous) 2+(-ic)ic)

2+(-ous) 3+(-2+(-ous) 3+(-ic)ic)

2+(-ous) 4+(-2+(-ous) 4+(-ic)ic)

3+(-ous) 5+(-3+(-ous) 5+(-ic)ic)

Cu copper (cuprum)Cu copper (cuprum) Fe iron (ferrum)Fe iron (ferrum) Pb lead Pb lead (plumbum)(plumbum)

As* arsenic (arsenum)As* arsenic (arsenum)

Hg mercury Hg mercury (mercurum)(mercurum)

Ni nickel Ni nickel (niccolum)(niccolum)

Sn tin (stannum)Sn tin (stannum) Sb* antimony Sb* antimony antimonum)antimonum)

Co cobalt Co cobalt (cobaltum)(cobaltum)

COMMON METALS WITH TWO PRIMARY OXIDATION NUMBERSCOMMON METALS WITH TWO PRIMARY OXIDATION NUMBERS(“-ous” or “-ic” ending on the metal or Roman Numerals after the metal + nonmetal with “-ide” ending)(“-ous” or “-ic” ending on the metal or Roman Numerals after the metal + nonmetal with “-ide” ending)

Some elements commonly form more than one kind of cation.These elements include the transition metals, which do not

Follow the octet rule in forming cations.


CHAPTER 7 19


METALSMETALS NONMETALS/METALLOIDSNONMETALS/METALLOIDS

Bi bismuth 3+, 5+Bi bismuth 3+, 5+ S* sulfur S* sulfur 2-,2-, 2+, 4+, 6+ 2+, 4+, 6+

Cr chromium 2+, 3+, 6+Cr chromium 2+, 3+, 6+ N* nitrogen N* nitrogen 3-,3-, 1+, 2+, 3+, 1+, 2+, 3+, 4+, 5+4+, 5+

Mn manganese 2+, 3+, 4+, 5+, Mn manganese 2+, 3+, 4+, 5+, 6+, 7+6+, 7+

P* phosphorus P* phosphorus 3-,3-, 3+, 5+ 3+, 5+

Mo molybdenum 2+, 3+, 4+, 5+, Mo molybdenum 2+, 3+, 4+, 5+, 6+6+

C* carbon C* carbon 4-,4-, 4+ 4+

W tungsten 2+, 3+, 4+, 5+, W tungsten 2+, 3+, 4+, 5+, 6+6+

Si* silicon Si* silicon 4-,4-, 4+ 4+

Sb* antimony Sb* antimony 3-,3-, 3+, 5+ 3+, 5+

As* arsenic As* arsenic 3-,3-, 3+, 5+ 3+, 5+

Se* selenium Se* selenium 2-,2-, 4+, 6+ 4+, 6+

Te* tellurium Te* tellurium 2-,2-, 4+, 6+ 4+, 6+

COMMON ELEMENTS WITH SEVERAL OXIDATION NUMBERSCOMMON ELEMENTS WITH SEVERAL OXIDATION NUMBERS(“MONO-, DI-, TRI-, TETRA-, PENTA-, HEXA-, SEPTA-, OCTO-, NONA-, DECA-”)(“MONO-, DI-, TRI-, TETRA-, PENTA-, HEXA-, SEPTA-, OCTO-, NONA-, DECA-”)

(Prefix is used on the metal and nonmetal (to designate the subscript) or use Roman Numerals after the metal)(Prefix is used on the metal and nonmetal (to designate the subscript) or use Roman Numerals after the metal)


CHAPTER 7 20


– POLYATOMIC IONSPOLYATOMIC IONS IONS THAT CONSIST OF MORE THAN 1 IONS THAT CONSIST OF MORE THAN 1

ATOMATOM BONDED TOGETHER BY COVALENT BONDED TOGETHER BY COVALENT

BONDS…BUT ACT AS A UNIT.BONDS…BUT ACT AS A UNIT. POLYATOMIC IONS FORM AN IONIC BOND POLYATOMIC IONS FORM AN IONIC BOND

WITH AN ION OF THE OPPOSITE CHARGEWITH AN ION OF THE OPPOSITE CHARGE ALMOST ALL POLYATOMICS ARE ALMOST ALL POLYATOMICS ARE

NEGATIVE IONS (EXCEPT NEGATIVE IONS (EXCEPT AMMONIUMAMMONIUM [NH[NH44]]++ ) )


CHAPTER 7 21

POLYATOMIC IONS

1+ 1- 2- 3- 4- AMMONIUM NH4 carbonate

CO3 aluminate AlO3 ferrocyanide

Fe(CN)6 1- Dihydrogen

phosphate H2PO4 chromate CrO4

arsenate AsO4 pyrophosphate P4O7

acetate C2H3O2 hydrazide N2H3 dihydrogen phosphate H2PO4

arsenite AsO3

amide NH2 Hydrogen sulfide HS

Dichromate Cr2O7 borate BO3

azide N3 hydrogen sufate HSO4

hexafluorosilicate SiF6

Citrate C6H5O7

benzoate C2H5O2 hydrogen sulfite HSO3

hydrogen phosphate HPO4

ferricyanide Fe(CN)6

Bicarbonate HCO3 hydroxide OH hydrogen phosphite HPO3

Phosphate PO4

bisulfide HS Iodite IO2 manganate MnO3 phosphite PO3 bisulfate HSO4 iodate IO3 oxalate C2O4 bisulfite HSO3 triiodide I3 Metasilicate SiO4 bitartrate HC4H4O6 nitrate NO3 molybdate MoO4 bromate BrO3 nitrite NO2 selenate SeO4

perchlorate ClO4 permanganate MnO4 silicate SiO3 chlorate ClO3 monobasic phosphate

dihydrogen H2PO4 phosphate

sulfate SO4

chlorite ClO2

thiocyanate SCN sulfite SO3

hypochlorite ClO tartrate C4H4O6 cyanate OCN Tetraborate B4O7 cyanide CN thiosulfate S2O3


CHAPTER 7 22

IONIC BONDINGIONIC BONDING BINARY IONIC COMPOUNDSBINARY IONIC COMPOUNDS

– CONTAIN THE IONS OF ONLY TWO CONTAIN THE IONS OF ONLY TWO ELEMENTS.ELEMENTS.

TYPES OF CHEMICAL FORMULASTYPES OF CHEMICAL FORMULAS– GENERAL FORMULASGENERAL FORMULAS– EMPIRICAL FORMULASEMPIRICAL FORMULAS– MOLECULAR FORMULASMOLECULAR FORMULAS– STRUCTURAL FORMULASSTRUCTURAL FORMULAS

LISTED IN ORDER OF INCREASIN

G SPECIFICIT

Y


CHAPTER 7 23

FORMULASFORMULAS

GLUCOSEGLUCOSE– GENERAL FORMULAGENERAL FORMULA CCnnHH2n2nOOnn

BASIC MATHEMATICAL STRUCTUREBASIC MATHEMATICAL STRUCTURE

– EMPIRICAL FORMULAEMPIRICAL FORMULA C HC H22 O O RATIO (CARBOHYDRATE)RATIO (CARBOHYDRATE)

– MOLECULAR FORMULAMOLECULAR FORMULA CC66HH1212OO66 SIX-CARBON MONOSACCHARIDESIX-CARBON MONOSACCHARIDE

– STRUCTURAL FORMULASTRUCTURAL FORMULA -D-GLUCOSE-D-GLUCOSE

OH

O

OHOH

CH2OH

CC

OH

C

C

CH

H H

H H


CHAPTER 7 24

IONIC BONDINGIONIC BONDING What is an ionic bond?What is an ionic bond? List the properties of ionic compounds.List the properties of ionic compounds. State the octet rule. Use the octet rule State the octet rule. Use the octet rule

to describe the reaction between to describe the reaction between chlorine and sodium.chlorine and sodium.

Describe the Lewis dot diagram to show Describe the Lewis dot diagram to show valence electrons of an atom.valence electrons of an atom.

Distinguish among anions, cations, and Distinguish among anions, cations, and polyatomic ions.polyatomic ions.


CHAPTER 7 25

COVALENT BONDINGCOVALENT BONDING

A COVALENT BOND IS FORMED BY A COVALENT BOND IS FORMED BY A SHARED PAIR OF ELECTRONS A SHARED PAIR OF ELECTRONS BETWEEN TWO ATOMS.BETWEEN TWO ATOMS.– REMEMBER!!! THE OCTET RULEREMEMBER!!! THE OCTET RULE

MOLECULES AND THEIR FAMILIESMOLECULES AND THEIR FAMILIES– A GROUP OF ATOMS THAT ARE UNITED BY A GROUP OF ATOMS THAT ARE UNITED BY

COVALENT BONDS IS CALLED A MOLECULE.COVALENT BONDS IS CALLED A MOLECULE.– A SUBSTANCE THAT IS MADE OF A SUBSTANCE THAT IS MADE OF

MOLECULES IS CALLED A MOLECULAR MOLECULES IS CALLED A MOLECULAR SUBSTANCESUBSTANCE


CHAPTER 7 26

COVALENT BONDS

COVALENT BONDINGCOVALENT BONDING DESCRIBING COVALENT BONDSDESCRIBING COVALENT BONDS

– LEWIS STRUCTURE:LEWIS STRUCTURE:

H

H

H

N NH H H

UNSHARED PAIROF ELECTRONS

COVALENT BONDSOCTET RULE:OCTET RULE:

Nitrogen = 8 e-

Hydrogen = 2e-

NHNH33 COVALENT BONDS

SINGLE COVALENT

BONDS

SINGLE COVALENT

BOND


CHAPTER 7 27


MULTIPLE BONDSMULTIPLE BONDS– SINGLE COVALENT BOND (SINGLE SINGLE COVALENT BOND (SINGLE

BONDS)BONDS) IN A SINGLE BOND, 2 ATOMS SHARE EXACTLY ONE IN A SINGLE BOND, 2 ATOMS SHARE EXACTLY ONE

PAIR OF ELECTRONSPAIR OF ELECTRONS

– DOUBLE COVALENT BOND (DOUBLE DOUBLE COVALENT BOND (DOUBLE BOND)BOND)

CONSISTS OF TWO PAIRS OF SHARED ELECTRONSCONSISTS OF TWO PAIRS OF SHARED ELECTRONS

– TRIPLE COVALENT BOND (TRIPLE BOND)TRIPLE COVALENT BOND (TRIPLE BOND) CONSISTS OF THREE PAIRS OF ELECTRONSCONSISTS OF THREE PAIRS OF ELECTRONS


CHAPTER 7 28


– DOUBLE BONDSDOUBLE BONDS FORMALDEHYDE (HFORMALDEHYDE (H22CO)CO)

YOU CAN REPLACE THE PAIRED ELECTRON YOU CAN REPLACE THE PAIRED ELECTRON DOTS WITH A REPRESENTATIVE DASH ( ).DOTS WITH A REPRESENTATIVE DASH ( ).

– ( ) = single bond( ) = single bond– ( ) = double bond( ) = double bond– ( ) = triple bond( ) = triple bond

H

H

C OH

H OC

DOUBLE BOND

SINGLEBOND

H C

H

O


CHAPTER 7 29


– TRIPLE BONDSTRIPLE BONDS ETHYNE (CETHYNE (C22HH22))

H HC C H C C H

TRIPLE BOND

H C C H

TRIPLE BOND

SINGLEBOND

SINGLEBOND


CHAPTER 7 30

DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES

DRAWING LEWIS STRUCTURESDRAWING LEWIS STRUCTURES1.1. SUM THE VALENCE ELECTRONS FROM ALL ATOMSSUM THE VALENCE ELECTRONS FROM ALL ATOMS

A. Don’t worry about keeping track of which A. Don’t worry about keeping track of which electrons electrons come from which atoms. Only come from which atoms. Only the total number is the total number is important. important.

2.2. WRITE THE SYMBOLS FOR THE ATOMS TO SHOW WRITE THE SYMBOLS FOR THE ATOMS TO SHOW WHICH ATOMS ARE ATTACHED TO WHICH, AND WHICH ATOMS ARE ATTACHED TO WHICH, AND CONNECT THEM WITH A SINGLE BOND ( ).CONNECT THEM WITH A SINGLE BOND ( ).

A. Atoms are often written in the order in which A. Atoms are often written in the order in which they are they are connected in the molecule or ion, as in connected in the molecule or ion, as in HCN. When the HCN. When the central atom has a group of central atom has a group of other atoms bonded to it, other atoms bonded to it, we usually write the we usually write the

central atom first, as in COcentral atom first, as in CO332-2- and and SF SF44..


CHAPTER 7 31


3. COMPLETE THE OCTETS OF THE ATOMS 3. COMPLETE THE OCTETS OF THE ATOMS BONDED TO THE CENTRAL ATOM.BONDED TO THE CENTRAL ATOM.

A. Remember, however, that hydrogen can A. Remember, however, that hydrogen can only have only only have only two electrons. two electrons.

4. PLACE ANY LEFTOVER ELECTRONS ON THE 4. PLACE ANY LEFTOVER ELECTRONS ON THE CENTRAL ATOM, EVEN IF DOING SO RESULTS IN CENTRAL ATOM, EVEN IF DOING SO RESULTS IN MORE THAN AN OCTET.MORE THAN AN OCTET.

5. IF THERE ARE NOT ENOUGH ELECTRONS TO 5. IF THERE ARE NOT ENOUGH ELECTRONS TO GIVE THE CENTRAL ATOM AN OCTET, TRY GIVE THE CENTRAL ATOM AN OCTET, TRY MULTIPLE BONDS.MULTIPLE BONDS. A. Use one or more of the unshared pairs of A. Use one or more of the unshared pairs of electrons on electrons on the atoms bonded to the central the atoms bonded to the central atom to form atom to form double or triple bonds. double or triple bonds.


CHAPTER 7 32


DRAWING THE LEWIS STRUCTURE FOR PHOSPHORUS TRICHLORIDE PCl3

FIRST, SUMTHE VALENCE

ELECTRONS

P3, 4+, 5+ [Ne] 3s2, 3p3

= 5

Cl1- [Ne] 3s2, 3p5

= 7 x(3)

26


CHAPTER 7 33


P Cl

Cl

Cl SECOND, ARRANGE THE

ATOMS TO SHOWWHICH ATOM IS

CONNECTED WHICH,AND DRAW A SINGLE

BOND BETWEENTHEM.

THERE ARE VARIOUS WAYS THE ATOM MIGHT BE ARRANGED. IN BINARY COMPOUNDS, THE FIRST ELEMENT LISTED IS GENERALLY SURROUNDED BY THE REMAINING ATOMS


CHAPTER 7 34


P Cl

Cl

Cl

THIRD, COMPLETE THE OCTETS ON THE ATOMS

BONDED TO THE CENTRALATOM. THIS ACCOUNTS

FOR 24 ELECTRONS

REMEMBER THATTHE BONDED

ELECTRONS (DASH)ACCOUNT FOR TWO

ELECTRONS!


CHAPTER 7 35


P Cl

Cl

Cl

FOURTH, PLACE THE REMAINING TWO

ELECTRONS ON THE CENTRAL ATOM,

COMPLETING THE OCTETAROUND THAT ATOM

AS WELL.


CHAPTER 7 36


C OO

CO2

==

412

16THAT’S 20

ELECTRONS !!

XX XXXX

XX

WAIT…I’LL FIX IT !!!

NOW YOU HAVE 16

ELECTRONS AND I STILL

FOLLOW THE OCTET RULE !!

CARBON HAS 8

CARBON HAS 8

OXYGEN HAS 8

THAT’S SWEET DUDE !!

COCO22


CHAPTER 7 37


DRAWING LEWIS STRUCTURES FOR OXYIONS (POLYATOMICS) BrO3

1-

Br OO

O

1-

NOTE: THE TOTAL NUMBER OF VALENCE ELECTRONS (Br=7)+ (O3=18)=25. TO SATISFY THE OCTET RULE THERE ARE 26 ELECTRONS (ONE MORE THAN REQUIRED). THE COUMPOUND IS PLACED IN BRACKETS AND THE EXTRA NEGATIVE CHARGE(S) IS/ ARE RECORDED AS A SUPERSCRIPT OUTSIDE THE BRACKETS.

BrO3

==

71825


CHAPTER 7 38


DRAW THE LEWIS STRUCTURE DRAW THE LEWIS STRUCTURE FOR THE FOLLOWING FOR THE FOLLOWING COMPOUNDSCOMPOUNDS– CHCH44

– HCNHCN

– SOSO442-2-

– CFCF22ClCl22


CHAPTER 7 39

RESONANCE STRUCTURESRESONANCE STRUCTURES

WE SOMETIMES ENCOUNTER WE SOMETIMES ENCOUNTER SUBSTANCES IN WHICH THE SUBSTANCES IN WHICH THE KNOWN ARRANGEMENT OF KNOWN ARRANGEMENT OF ATOMS IS NOT ADEQUATELY ATOMS IS NOT ADEQUATELY DESCRIBED BY A SINGLE LEWIS DESCRIBED BY A SINGLE LEWIS STRUCTURE.STRUCTURE.– CONSIDER OZONE (OCONSIDER OZONE (O33), WHICH MUST ), WHICH MUST

HAVE ONE DOUBLE BOND TO ATTAIN HAVE ONE DOUBLE BOND TO ATTAIN AN OCTET OF ELECTRONS AROUND AN OCTET OF ELECTRONS AROUND EACH ATOM:EACH ATOM:


CHAPTER 7 40

RESONANCE STRUCTURESRESONANCE STRUCTURES

OO O

OO O

OO O

THE TWO ALTERNATIVE STRUCTURES FOR OZONE ARE EQUIVALENT EXCEPT FOR THE PLACEMENT OF THE ELECTRONS. THE REAL MOLECULE IS DESCRIBED BY AN AVERAGE (BLEND) OF THE STRUCTURES. THE MOLECULE DOES NOT OSCILLATE RAPIDLY BETWEEN THE FORMS (THERE IS ONLY ONE FORM OF THE MOLECULE).

INDICATES RESONANCE FORMS


CHAPTER 7 41

EXCEPTIONS TO THE OCTET EXCEPTIONS TO THE OCTET RULERULE

ATOMS WITH LESS THAN AN OCTETATOMS WITH LESS THAN AN OCTET– MANY COMPOUNDS OF MANY COMPOUNDS OF BORONBORON DO NOT DO NOT

FOLLOW THE OCTET RULE FOLLOW THE OCTET RULE (BF(BF33))

– WE COULD COMPLETE THE OCTET BY WE COULD COMPLETE THE OCTET BY FORMING A DOUBLE BOND CREATING FORMING A DOUBLE BOND CREATING POSSIBLE RESONANCE STRUCTURES.POSSIBLE RESONANCE STRUCTURES.

– THESE STRUCTURES FORCE FLUORINE TO THESE STRUCTURES FORCE FLUORINE TO SHARE ADDITIONAL ELCTRONS WITH THE SHARE ADDITIONAL ELCTRONS WITH THE BORON ATOM…HOWEVER….THIS IS BORON ATOM…HOWEVER….THIS IS INCONSTENT WITH THE HIGH INCONSTENT WITH THE HIGH ELECTRONEGATIVITY OF FLUORINE.ELECTRONEGATIVITY OF FLUORINE.


CHAPTER 7 42


ATOMS WITH MORE THAN AN ATOMS WITH MORE THAN AN OCTETOCTET– SOME ATOMS FOUND BEYOND THE 2SOME ATOMS FOUND BEYOND THE 2NDND

PERIOD OF THE PERIODIC TABLE (MOST PERIOD OF THE PERIODIC TABLE (MOST NOTABLY SULFUR AND PHOSPHORUS) NOTABLY SULFUR AND PHOSPHORUS) SOMETIMES FORM BONDS THAT GIVE THEM SOMETIMES FORM BONDS THAT GIVE THEM MORE THAN AN OCTET OF ELECTRONS.MORE THAN AN OCTET OF ELECTRONS.

– THE ADDITIONAL ELECTRONS FILL THE 3d THE ADDITIONAL ELECTRONS FILL THE 3d ORBITALS OF THESE ATOMSORBITALS OF THESE ATOMS

– SFSF4 4 , AsF, AsF661-1-, PCl, PCl55, AND ICl, AND ICl44

1-1-


CHAPTER 7 43


MOLECULES WITH AN ODD NUMBER MOLECULES WITH AN ODD NUMBER OF ELECTRONSOF ELECTRONS– IN THE VAST MAJORITY OF MOLECULES IN THE VAST MAJORITY OF MOLECULES

THE NUMBER OF ELECTRONS IS EVEN, THE NUMBER OF ELECTRONS IS EVEN, AND COMPLETE PAIRING OF ELECTRON AND COMPLETE PAIRING OF ELECTRON SPINS OCCURS.SPINS OCCURS.

– A MOLECULE WITH AN ODD NUMBER OF A MOLECULE WITH AN ODD NUMBER OF ELECTRONS CANNOT FOLLOW THE ELECTRONS CANNOT FOLLOW THE OCTET RULE.OCTET RULE.

– ClOClO2, 2, , NO, NO , , AND NOAND NO22


CHAPTER 7 44

BOND POLARITY AND BOND POLARITY AND ELECTRONEGATIVITYELECTRONEGATIVITY

THE CONCEPT OF THE CONCEPT OF BOND POLARITYBOND POLARITY IS USEFUL IS USEFUL IN DESCRIBING THE SHARING OF ELECTRONS IN DESCRIBING THE SHARING OF ELECTRONS BETWEEN ATOMSBETWEEN ATOMS

A A NONPOLAR BONDNONPOLAR BOND IS ONE IN WHICH THE IS ONE IN WHICH THE ELECTRONS ARE SHARED EQUALLY BETWEEN TWO ELECTRONS ARE SHARED EQUALLY BETWEEN TWO ATOMS.ATOMS.

A A POLAR COVALENT BONDPOLAR COVALENT BOND, ONE OF THE , ONE OF THE ATOMS EXERTS A GREATER ATTRACTION FOR THE ATOMS EXERTS A GREATER ATTRACTION FOR THE ELECTRONS THAN THE OTHER.ELECTRONS THAN THE OTHER.

IF THE DIFFERENCE IN RELATIVE ABILITY TO IF THE DIFFERENCE IN RELATIVE ABILITY TO ATTRACT ELECTRONS IS LARGE ENOUGH, AN ATTRACT ELECTRONS IS LARGE ENOUGH, AN IONIC BONDIONIC BOND IS FORMED IS FORMED..


CHAPTER 7 45


ELECTRONEGATIVITY:ELECTRONEGATIVITY:– THE ABILITY OF AN ATOM, THE ABILITY OF AN ATOM, IN A IN A

MOLECULEMOLECULE, TO ATTRACT ELECTRONS TO , TO ATTRACT ELECTRONS TO ITSELF.ITSELF.

THE GREATER THE ELCETRONEGATIVITY, THE THE GREATER THE ELCETRONEGATIVITY, THE GREATER ITS ABILITY TO ATTRACT ELECTRONSGREATER ITS ABILITY TO ATTRACT ELECTRONS

– RELATED TO ITS IONIZATION ENERGY AND RELATED TO ITS IONIZATION ENERGY AND ELECTRON AFFINITYELECTRON AFFINITY

– FLUORINE HAS THE HIGHEST FLUORINE HAS THE HIGHEST ELECTRONEGATIVITY (4.0)ELECTRONEGATIVITY (4.0)

– CESIUM HAS THE LOWEST ELECTRONEGATIVITY CESIUM HAS THE LOWEST ELECTRONEGATIVITY (0.7)(0.7)


CHAPTER 7 46


0.0 0.5 1.0 1.5 2.0 2.5 3.0 3.5 4.0

< 0.4NONPOLAR

> 2.0IONIC

< 0.4NONPOLAR COVALENT

GREY AREA BETWEEN 1.67

AND 2.0

BETWEEN 0.5 AND 1.9

POLAR COVALENT


CHAPTER 7 47

BOND POLARITY ANDBOND POLARITY AND

ELECTRONEGATIVITYELECTRONEGATIVITY

COMPOUNDCOMPOUND


DIFFERENCEDIFFERENCE

TYPE OF BONDTYPE OF BOND

4.0 - 4.0 = 04.0 - 4.0 = 0 4.0 - 2.1 = 1.94.0 - 2.1 = 1.9 4.0 - 1.0 = 3.04.0 - 1.0 = 3.0

NONPOLAR NONPOLAR COVALENTCOVALENT

POLAR POLAR COVALENTCOVALENT

IONICIONIC

FF22 HFHF LiFLiF


CHAPTER 7 48



– IN FIN F22 THE ELECTRONS ARE THE ELECTRONS ARE SHARED EQUALLY BETWEEN THE SHARED EQUALLY BETWEEN THE FLUORINE ATOMS, AND THE FLUORINE ATOMS, AND THE BOND IS NONPOLAR.BOND IS NONPOLAR.

F F


CHAPTER 7 49



– IN HF, THE FLUORINE ATOM HAS IN HF, THE FLUORINE ATOM HAS A GREATER ELECTRONEGATIVITY A GREATER ELECTRONEGATIVITY THAN THE HYDROGEN ATOM.THAN THE HYDROGEN ATOM. THE SHARING OF ELECTRONS IS UNEQUAL THE SHARING OF ELECTRONS IS UNEQUAL

(THE BOND IS POLAR)(THE BOND IS POLAR) THIS IS REPRESENTED IN TWO WAYSTHIS IS REPRESENTED IN TWO WAYS

H F H F+ -


CHAPTER 7 50



– THE THE ++ AND AND -- ARE MEANT TO ARE MEANT TO REPRESENT PARTIAL POSITIVE AND REPRESENT PARTIAL POSITIVE AND NEGATIVE CHARGES RESPECTIVELY.NEGATIVE CHARGES RESPECTIVELY.

– THE ARROW REPRESENTS THE PULL OF THE ARROW REPRESENTS THE PULL OF ELECTRON DENSITY OFF THE ELECTRON DENSITY OFF THE HYDROGEN BY THE FLUORINE, LEAVING HYDROGEN BY THE FLUORINE, LEAVING THE HYDROGEN WITH A PARTIAL THE HYDROGEN WITH A PARTIAL POSITIVE CHARGEPOSITIVE CHARGE

THE HEAD OF THE ARROW POINTS IN THETHE HEAD OF THE ARROW POINTS IN THE

DIRECTION IN WHICH THE ELECTRONS ARE DIRECTION IN WHICH THE ELECTRONS ARE ATTRACTEDATTRACTED


CHAPTER 7 51



REMEMBER……THE GREATER THE REMEMBER……THE GREATER THE DIFFERENCE IN ELECTRONEGATIVITY THE DIFFERENCE IN ELECTRONEGATIVITY THE MORE POLAR THE BOND !MORE POLAR THE BOND !

Describe a covalent bond.Describe a covalent bond. What is a molecule? What does a What is a molecule? What does a

molecule’s structural formula indicate?molecule’s structural formula indicate? How does a polar covalent bond differ from How does a polar covalent bond differ from

a nonpolar covalent bond?a nonpolar covalent bond? Which type of bond is found in molecular Which type of bond is found in molecular

oxygen (Ooxygen (O22) ? In carbon monoxide (CO)?) ? In carbon monoxide (CO)?


CHAPTER 7 52

NAMING CHEMICAL NAMING CHEMICAL COMPOUNDSCOMPOUNDS

Chemists name a compound Chemists name a compound according to the atoms and bonds according to the atoms and bonds that compose it.that compose it.

NOW !! NOW !! LET’S LET’S

GET TO GET TO WORK!!WORK!!

!!!!


CHAPTER 7 53

NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER

K S

potassium

sulfide

(1) Check the oxidation number

of the metal

2-

2

0(3) If the metal is

monoatomic….NAME THE METAL

(4) To name the nonmetal drop the

suffix and add “-ide”

1+ 0

(2) Make them add-up to zero “0”

by adding the proper subscript(s)

to the metal or nonmetal


of the nonmetal


CHAPTER 7 54


Na

1Cl

1-

Oxidation Number (Valence)


Metal: Written first !

NonMetal: Written Second

NAME THE METAL ION NAME THE NONMETAL ION

SODIUM CHLORIDEIDE

METALS WITH ONE OXIDATION NUMBERMETALS WITH ONE OXIDATION NUMBER

OXIDATION NUMBERS

MUSTADD-UP TO ZERO

OXIDATION NUMBERS

MUSTADD-UP TO ZERO

OXIDATION NUMBERS

MUSTADD-UP TO ZERO

OXIDATION NUMBERS

MUSTADD-UP TO ZERO

OXIDATION NUMBERS

MUSTADD-UP TO ZERO


CHAPTER 7 55


METALS WITH ONE OXIDATION NUMBERMETALS WITH ONE OXIDATION NUMBER

Na1+

Cl1- = 0

1 11 1

1+ 1- = 0

X X

NaNaClCl


CHAPTER 7 56


c

c

Mg2+

Cl1- 0

1 2

2+ 2- = 0

To make theOxidation valuesadd-up to “0”

we must find the lowest common

multiple

The Oxidation Numbers DO NOT add up to

“0”

Then we find themultiplier that when

multiplied by the oxidation number will sum to the common

multiple

x x

Mg Cl2


CHAPTER 7 57


c

c

Zn2+

F1- 0

1 2

2+ 2- = 0

To make theOxidation valuesadd-up to “0”

we must find the lowest common

multiple

The Oxidation Numbers DO NOT add up to

“0”

Then we find themultiplier that when

multiplied by the oxidation number will sum to the common

multiple

x x

Zn F2


CHAPTER 7 58


Ca2+ + Cl1- CaCl2 calcium chloride

Mg2++ P3- Mg3P2magnesium phosphide

Ba2+ + O2- BaO barium oxide

Na1+ + F1- NaF sodium fluoride

Al3+ + S2- Al2 S3aluminum sulfide

Li1+ + O2- Li2 O lithium oxide

K1+ + N3- K3 N potassium nitride

H1+ + Cl3- HCl hydrogen chloride

Th4++ Br1- ThBr4thorium bromide


CHAPTER 7 59

(3) If the metal is monoatomic….

NAME THE METAL

Ca NO3

calcium


of the metal1- = 0

(1) Check the oxidation number of the polyatomic

(2) Make them add-up to zero “0”

by adding the proper subscript(s)

to the metal or nonmetal

(4) Name the POLYATOMIC (USE

THE REFERENCE TABLE)

2+

2

* CHECK THE FORMULA…ARE THERE > 2 ELEMENTS ?

IF SO…BRACKET THE POLYATOMIC!!!

nitrate

NAMING COMPOUNDS WITH NAMING COMPOUNDS WITH POLYATOMICSPOLYATOMICS


CHAPTER 7 60

NAMING COMPOUNDS WITH NAMING COMPOUNDS WITH POLYATOMICSPOLYATOMICS

Ca2+ + NO3

1-Mg2+ + PO4

3-Ba2+ + CO3

2-Na1+ + OH1-

Al3+ + SiO3

2-Li1+ + SO3

2-

Th4+ + IO31-

H1+ + ClO3

1-

K1+ + C6H5O7

3-

Ca(NO3)2

Mg3 ( PO4 )2

Ba (CO3) *

Na (OH) *Al2 (SiO3)3

Li2 (SO3) *

K3 (C6H5O7) *

H(ClO3) *

Th (IO3)4

calcium nitrate

magnesium phosphate

sodium hydroxide

barium carbonate

lithium sulfite

aluminum silicate

hydrogen chlorate

potassium citrate

thorium iodate

* ( ) may or may not be used


CHAPTER 7 61

NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS

THERE ARE TWO (2) WAYS TO NAME THERE ARE TWO (2) WAYS TO NAME COMPOUNDS WITH METALS THAT HAVE COMPOUNDS WITH METALS THAT HAVE TWO PRIMARY OXIDATION NUMBERS.TWO PRIMARY OXIDATION NUMBERS.

FIRST METHODFIRST METHOD– 1. DETERMINE THE OXIDATION NUMBER OF THE 1. DETERMINE THE OXIDATION NUMBER OF THE

NONMETAL (THIS WILL DRIVE THE SELECTION OF NONMETAL (THIS WILL DRIVE THE SELECTION OF THE PROPER OXIDATION NUMBER OF THE METAL). THE PROPER OXIDATION NUMBER OF THE METAL).

– 2. NAME THE METAL USING THE LATIN NAME ROOT 2. NAME THE METAL USING THE LATIN NAME ROOT – 3. ADD THE PROPER SUFFIX TO THE METAL TO INDICATE 3. ADD THE PROPER SUFFIX TO THE METAL TO INDICATE

THE OXIDATION NUMBER OF THE METAL THAT WILL THE OXIDATION NUMBER OF THE METAL THAT WILL MATCH THE NONMETAL OXIDATION NUMBER SO THAT THE MATCH THE NONMETAL OXIDATION NUMBER SO THAT THE SUM OF THE OXIDATION NUMBERS WILL ADD-UP TO ZERO. SUM OF THE OXIDATION NUMBERS WILL ADD-UP TO ZERO.


CHAPTER 7 62


METALS WITH TWO OXIDATION NUMBERSMETALS WITH TWO OXIDATION NUMBERS

Fe2

Cl

1-



Metal: Written first !

NonMetal: Written Second

NAME THE METAL ION NAME THE NONMETAL ION

IRON CHLORIDEIDE

2

Subscript: to balance the charges


CHAPTER 7 63


But iron has two possible oxidation numbershow can we explainwhich one to use in the compound?

Fe2+/3+


CHAPTER 7 64


ferric = 3+

COMMON METALS WITH TWO PRIMARY OXIDATION NUMBERS(“-ous” or “-ic” ending on the metal or roman numerals after the metal + nonmetal with “-ide” ending)

1+(-ous) 2+(-ic) 2+(-ous) 3+(-ic) 2+(-ous) 4+(-ic) 3+(-ous) 5+(-ic)

Cu copper (cuprum) Fe iron (ferrum) Pb lead (plumbum) As arsenic (arsenum)Hg mercury(mercurum) Ni nickel (niccolum) Sn tin (stannum) Sb antimony (antimonum)

Co cobalt (cobaltum)

We can use the Latin Root with

the correct suffix for the metal

ferrous = 2+

ferrum


CHAPTER 7 65

NAME THE NONMETALUSE THE ROOT

+“IDE”

(BINARY COMPOUND)


Fe O3

3+ 2-

DETERMINE THE OXIDATION NUMBER OF THE NONMETAL

CHOOSE THE CORRECTOXIDATION NUMBER

OF THE METAL

= 0

OXIDATION NUMBERSMUST ADD TO ZERO

NAME THE METALUSE THE LATIN ROOT

+ PROPER SUFFIX

FERRFERR OXOXIC IDE

2


CHAPTER 7 66


Fe2+ + Cl1-Fe3+ + PO4

3-Hg1+ + CO3

2-Hg2+ + OH1-Cu1+ + O2-

Cu2+ + S2-

Co3+ + IO31-

Sn2+ + F1-

Sn4+ + NO3

1-

FeCl2Fe ( PO4 ) *Hg2 (CO3) *

Hg(OH)2

Cu2OCuS

Sn (NO3)4

SnF2

Co (IO3)3

ferrous chloride

ferric phosphate

mercuric hydroxide

mercurous carbonate

cupric sulfide

cuprous oxide

stannous fluoride

stannic nitrate

cobaltic iodate



CHAPTER 7 67


SECOND METHODSECOND METHOD– 1. DETERMINE THE OXIDATION NUMBER OF THE 1. DETERMINE THE OXIDATION NUMBER OF THE

NONMETAL (THIS WILL DRIVE THE SELECTION OF NONMETAL (THIS WILL DRIVE THE SELECTION OF THE PROPER OXIDATION NUMBER OF THE METAL.THE PROPER OXIDATION NUMBER OF THE METAL.

– 2. NAME THE METAL (USE THE ENGLISH NAME)2. NAME THE METAL (USE THE ENGLISH NAME)– 3. IN PARENTHESIS BEHIND THE METAL USE ROMAN 3. IN PARENTHESIS BEHIND THE METAL USE ROMAN

NUMERALS TO INDICATE THE PROPER OXIDATION NUMERALS TO INDICATE THE PROPER OXIDATION NUMBER NUMBER

(II)(II)– 4. NAME THE NONMETAL APPROPRIATELY

I ADD THE DOTS TO REDUCE ERRORS


CHAPTER 7 68


Iron (III) = 3+

COMMON METALS WITH TWO PRIMARY OXIDATION NUMBERS(“-ous” or “-ic” ending on the metal or roman numerals after the metal + nonmetal with “-ide” ending)

1+(-ous) 2+(-ic) 2+(-ous) 3+(-ic) 2+(-ous) 4+(-ic) 3+(-ous) 5+(-ic)

Cu copper (cuprum) Fe iron (ferrum) Pb lead (plumbum) As arsenic (arsenum)Hg mercury(mercurum) Ni nickel (niccolum) Sn tin (stannum) Sb antimony (antimonum)

Co cobalt (cobaltum)

We can use the Roman Numeral with

the correct suffix for the metal

Iron (II) = 2+


CHAPTER 7 69


NAME THE NONMETALUSE THE ROOT

+“IDE”

(BINARY COMPOUND)

Fe O3

3+ 2-

DETERMINE THE OXIDATION NUMBER OF THE NONMETAL

CHOOSE THE CORRECTOXIDATION NUMBER

OF THE METAL

=0

OXIDATION NUMBERSMUST ADD TO ZERO

NAME THE METAL+

ROMAN NUMERALS IN PARENTHESIS

IRONIRON OXOX(III) IDE

2


CHAPTER 7 70


Fe2+ + ClFe3+ + PO4Hg1+ + CO3

Hg2+ + OHCu1+ + O

Cu2+ + S

Co3+ + IO3

Sn2+ + F

Sn4+ + NO3

FeCl2Fe ( PO4 )*

Hg2 (CO3) *

Hg(OH)2

Cu2OCuS

Sn (NO3)4

SnF2

Co (IO3)3

iron (II) chloride

iron (III) phosphate

mercury (II) hydroxide

mercury (I) carbonate

copper (II) sulfide

copper (I) oxide

tin (II) fluoride

tin (IV) nitrate

cobalt (III) iodate



CHAPTER 7 71

NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION ELEMENTS WITH MULTIPLE OXIDATION NUMBERSNUMBERS

THERE ARE TWO (2) WAYS TO NAME THERE ARE TWO (2) WAYS TO NAME COMPOUNDS WITH METALS THAT HAVE COMPOUNDS WITH METALS THAT HAVE MULTIPLE OXIDATION NUMBERS.MULTIPLE OXIDATION NUMBERS.

FIRST METHODFIRST METHOD1. NAME THE METAL + NAME THE NONMETAL WITH THE

APPROPRIATE PREFIX ADDED TO THE NONMETAL INDICATING THE NUMBER OF NONMETAL UNITS USED (TAKEN FROM THE SUBSCRIPT OF THE NONMETAL).

2. THERE ARE TIMES, HOWEVER, THAT CONFUSION MAY ARISE USING THIS SYSTEM RELATED TO THE FACT THAT THERE MAY BE MORE THAN ONE POSSIBLE COMPOUND FORMULA FROM A SINGLE NAME. THIS DEFEATS THE PURPOSE OF COMPOUND NAMING. IN THESE CASES IT MAY BE REQUIRED TO ADD THE PREFIX TO BOTH THE METAL AND THE NONMETAL TO MAKE THE NAMING UNIQUE.


CHAPTER 7 72

NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS

NAMING COMPOUNDS WITH MULTIPLE OXIDATION NUMBERS

Mn

2+3+4+5+6+7+

How do I Handle this

one?


CHAPTER 7 73



Mn

2+3+4+5+6+7+

O2-First, check out the non-metal…and get

its oxidation number.


CHAPTER 7 74



Mn

2+3+4+5+6+7+

O2-Next, check the given

formula and make sure the oxidation numbers

add up to zero.


CHAPTER 7 75



Mn

2+3+4+5+6+7+

O2-

Mn O

Mn2 O3

Mn O2

Mn2 O5

Mn O3

Mn2 O7Look at the possibilities


CHAPTER 7 76


Mn O

Mn2 O3

Mn O2


manganese

manganese

manganese

You must tellthe reader whichmanganese you

used!!

THERE ARETWO WAYS

TO DO THIS !!


CHAPTER 7 77


Mn O

Mn2 O3

Mn O2

manganese

manganese

manganese

FIRST !!!!

mon

di

di

oxide

oxide

oxide

USE PREFIXES

tri


CHAPTER 7 78


MnMn2+2+

MnMn 3+ 3+

MnMn4+4+

MnMn5+5+

MnMn6+6+

MnMn7+7+

OO2-2-

OO2-2-

OO2-2-

OO2-2-

OO2-2-

OO2-2-

MnOMnO manganese monoxide

MnMn22OO33

MnOMnO22

MnMn22OO55

MnOMnO33

MnMn22OO77

dimanganese trioxide*

manganese dioxide

dimanganese pentaoxidemanganese trioxide*

dimanganese septaoxide

* note the need for the prefix on the metal !


CHAPTER 7 79


Bi3+ + Cl1-Cr3+ + PO4

3-Mn4+ + CO32-

Cr6+ + F1-

C4+ + O2-

P3+ + S2-

S6+ + IO31-

N2+ + F1-

Si4+ + NO3

1-

BiCl3Cr( PO4 ) *

Mn (CO3)2

Cr F6

CO2

P2S3

Si (NO3)4

NF2

S (IO3)6

bismuth trichloridechromium monophosphate

chromium hexafluoride

manganese dicarbonate

diphosphorus trisulfide

carbon dioxide

nitrogen difluoride

silicon tetranitrate

sulfur hexaiodate



CHAPTER 7 80


SECOND METHODSECOND METHOD 1. DETERMINE THE OXIDATION NUMBER OF THE 1. DETERMINE THE OXIDATION NUMBER OF THE

NONMETAL (THIS WILL DRIVE THE SELECTION NONMETAL (THIS WILL DRIVE THE SELECTION OF THE PROPER OXIDATION NUMBER OF THE OF THE PROPER OXIDATION NUMBER OF THE

METAL).METAL).

2. NAME THE METAL2. NAME THE METAL

3. IN PARENTHESIS BEHIND THE METAL USE ROMAN 3. IN PARENTHESIS BEHIND THE METAL USE ROMAN NUMERALS TO INDICATE THE PROPER NUMERALS TO INDICATE THE PROPER

OXIDATION OXIDATION NUMBER NUMBER

(II)(II)– 4. NAME THE NONMETAL

I ADD THE DOTS TO REDUCE ERRORS


CHAPTER 7 81


Mn O

Mn2 O3

Mn O2

manganese

manganese

manganese

SECOND !

(II)

III

IV

oxide

oxide

oxide

USE ROMAN

NUMERALS


CHAPTER 7 82


MnMn2+2+

MnMn 3+ 3+

MnMn4+4+

MnMn5+5+

MnMn6+6+

MnMn7+7+

OO2-2-

OO2-2-

OO2-2-

OO2-2-

OO2-2-

OO2-2-

MnOMnO manganese (II) oxide

MnMn22OO33

MnOMnO22

MnMn22OO55

MnOMnO33

MnMn22OO77

manganese (III) oxide

manganese (IV) oxide

manganese (V) oxide

manganese (VI) oxide

manganese (VII) oxide


CHAPTER 7 83


Bi3+ + ClCr3+ + PO4

Mn4+ + CO3Cr6+ + FC4+ + O

P3+ + S

S6+ + IO3

N2+ + F

Si4+ + NO3

BiCl3Cr( PO4 )

Mn (CO3)2 *Cr F6

CO2

P2S3

Si (NO3)4

NF2

S (IO3)6

bismuth (III) chloride

chromium (III) phosphate

chromium (VI) fluoride

manganese (IV) carbonate

phosphorus (III) sulfide

carbon (IV) oxide

nitrogen (II) fluoride

silicon (IV) nitrate

sulfur (VI) iodate



CHAPTER 7 84

NAMING ACIDSNAMING ACIDS

H+H+

H+H+

H+H+

H+H+

H+H+

Cl-Cl- Cl-Cl-Cl-Cl-

Cl-Cl-

Cl-Cl-

HYDROGEN IONS

H+

CHLORINEIONS

Cl-

HCl

HYDROGEN CHLORIDE

HYDROGEN IONS (cations)

H+

CHLORIDEIONS (anions)

Cl-

HCl (g) + HOH (l) H+ + Cl- + HOH [ HCl (aq) ]

(aq) = aqueous

An acid is a molecular substance that

dissolves in water to produce hydrogen

ions (H+)


CHAPTER 7 85

NAMING ACIDSNAMING ACIDS BINARY ACIDSBINARY ACIDS

– ALL BINARY ACIDS HAVE ONLY TWO ELEMENTS ALL BINARY ACIDS HAVE ONLY TWO ELEMENTS IN THE FORMULAIN THE FORMULA..

– THEY ARE USUALLY IN AQUEOUS SOLUTIONSTHEY ARE USUALLY IN AQUEOUS SOLUTIONS THE FIRST (METAL) THE FIRST (METAL) MUST BE A HYDROGEN ATOM.MUST BE A HYDROGEN ATOM. THE NONMETAL MUST BE A SINGLE ELEMENT.THE NONMETAL MUST BE A SINGLE ELEMENT.

– THE NAME OF THE ACID IS DETERMINED BY THE THE NAME OF THE ACID IS DETERMINED BY THE NONMETAL USING THE FOLLOWING FORMAT:NONMETAL USING THE FOLLOWING FORMAT:

HYDRO- (NONMETAL ROOT)

-IC

HYDRO-chlor

-IC Hydrochloric acidHCl HCl = =


CHAPTER 7 86


HCl (aq)

H 2 S (aq)HF (aq)

HBr (aq)

HI (aq)

hydrochloric acid

hydrosulfuric acid

hydrofluoric acid

hydrobromic acid

hydroiodic acid


CHAPTER 7 87

NAMING ACIDSNAMING ACIDS TERNARY ACIDSTERNARY ACIDS

– ALL TERNARY ACIDS HAVE MORE THAN TWO ALL TERNARY ACIDS HAVE MORE THAN TWO ELEMENTS IN THE FORMULAELEMENTS IN THE FORMULA

THEY ARE USUALLY IN AQUEOUS SOLUTIONSTHEY ARE USUALLY IN AQUEOUS SOLUTIONS MANY OF THEM ARE OXY-ACIDS (WHICH MEANS THAT MANY OF THEM ARE OXY-ACIDS (WHICH MEANS THAT

THEY HAVE A POLYATOMIC NONMETAL THAT CONTAINS THEY HAVE A POLYATOMIC NONMETAL THAT CONTAINS AN OXYGEN)AN OXYGEN)

– THE NAME OF THE ACID IS DETERMINED BY THE THE NAME OF THE ACID IS DETERMINED BY THE POLYATOMIC NAME USING THE FOLLOWING FORMATPOLYATOMIC NAME USING THE FOLLOWING FORMAT

(POLYATOMIC ROOT) +

POLYATOMIC SUFFIX = -ATE

THE ACID SUFFIX = -IC

POLYATOMIC SUFFIX = -ITE

THE ACID SUFFIX = -OUS


CHAPTER 7 88


HNO3

H2SO3

H3PO4

HC2H3O2

HClO4

HClO

HNO2

H2SO4

hydrogen nitratehydrogen nitritehydrogen sulfatehydrogen sulfite

hydrogen phosphatehydrogen acetatehydrogen perchloratehydrogen hypochlorite

nitric acid

sulfurous acidphosphoric acidacetic acid

perchloric acidhypochlorous acid

nitrous acidsulfuric acid


CHAPTER 7 89

NAMING HYDRATESNAMING HYDRATES

HYDRATES:HYDRATES:– HYDATES ARE CHEMICAL COMPOUNDS HYDATES ARE CHEMICAL COMPOUNDS

COMBINED WITH WATER IN A DEFINITE COMBINED WITH WATER IN A DEFINITE RATIO. RATIO.

CaCl2 • 2HOH

(1) NAME THE COMPOUND

(2) INDICATE THE COEFFICIENT FOR WATER (USE THE GREEK PREFIX)

(3) ADD THE TERM “HYDRATE” AT THE END

calcium chloride

dihydrate


CHAPTER 7 90

NAMING HYDRATESNAMING HYDRATES

CuSO4 · 5HOH

CoCl2 · 2HOH

BaCl2 · 2HOH

Ca(NO3)2 · 3HOH

Na2CO3 · 7HOH

Mg3(PO4)2 · 4HOH

copper (II) sulfate pentahydratecobaltous chloride dihydrate

barium chloride dihydrate

calcium nitrate trihydrate

sodium carbonate septahydratemagnesium phosphate tetrahydrate


CHAPTER 7 91

NAMING COMPOUNDS:NAMING COMPOUNDS:THE LAST WORDTHE LAST WORD

PREFIXES AND SUFFIXES ARE USED IN THE PREFIXES AND SUFFIXES ARE USED IN THE NAMES OF THESE IONS TO INDICATE THE NAMES OF THESE IONS TO INDICATE THE OXYGEN CONTENT OF THE POLYATOMIC ION IN OXYGEN CONTENT OF THE POLYATOMIC ION IN RELATION TO OTHER IONS IN A SERIES OF RELATION TO OTHER IONS IN A SERIES OF SIMILAR IONS.SIMILAR IONS.

PREFIPREFIXX

SUFFISUFFIXX

INCREASING INCREASING OXYGEN OXYGEN CONTENTCONTENT

PER-

HYPO-

-ATE-ATE

-ITE

-ITE

EXAMPLEXAMPLEEClO4

-

ClO3-

ClO2-

ClO -

perchloratechlorate

chlorite

hypochlorite


CHAPTER 7 92

NAMING COMPOUNDS:NAMING COMPOUNDS:THE LAST WORDTHE LAST WORD

HBrO3 (aq)

NaBrONH4IOKMnO4

AlClO

H3C6H5O7 (aq)BaClO4

Ca(NO4)2

H2SO2 (aq)

bromic acid

ammonium hypoioditepotassium permanganate

aluminum hypochlorite

hyposulfurous acidcalcium pernitratebarium perchloratecitric acid

sodium hypobromite


CHAPTER 7 93

CRITICAL THINKING AND CRITICAL THINKING AND PROBLEM SOLVINGPROBLEM SOLVING

DETERMINE DETERMINE FORMULAS FOR FORMULAS FOR THE FOLLOWING THE FOLLOWING COMPOUNDSCOMPOUNDS– silver nitratesilver nitrate– magnesium hydroxidemagnesium hydroxide– carbon tetrachloridecarbon tetrachloride– sulfuric acidsulfuric acid– lead(II) acetatelead(II) acetate– iron(III) nitrateiron(III) nitrate

DRAW LEWIS DOT DRAW LEWIS DOT DIAGRAMS FOR DIAGRAMS FOR THE FOLLOWING THE FOLLOWING ELEMENTSELEMENTS– carboncarbon– hydrogenhydrogen– potassiumpotassium– sulfursulfur– magnesiummagnesium– iodineiodine


CHAPTER 7 94


DRAW LEWIS DRAW LEWIS STRUCTURES FOR STRUCTURES FOR EACH OF THE EACH OF THE FOLLOWING FOLLOWING COMPOUNDS. COMPOUNDS. IDENTIFY EACH IDENTIFY EACH BOND AS POLAR BOND AS POLAR OR NONPOLAR.OR NONPOLAR.

HH22OO

COCO22

ClCl22

HCNHCN

NClNCl33

NN22


CHAPTER 7 95


DETERMINE THE DETERMINE THE NAME OF EACH NAME OF EACH OF THE OF THE FOLLOWING FOLLOWING COMPOUNDSCOMPOUNDS

SbSb22SS33 ______________ ______________

FeS ________________FeS ________________

NaNa22O ______________O ______________

HH22COCO33 ______________ ______________

SiOSiO22 8 H 8 H22OO

______________________________________ CaSOCaSO44 2 HOH 2 HOH

______________________________________


CHAPTER 7 96


DRAW THE DRAW THE EQUIVALENT EQUIVALENT RESONANCE RESONANCE STRUCTURES STRUCTURES FOR THE FOR THE FOLLOWING FOLLOWING MOLECULESMOLECULES

SOSO33

NONO331-1-

ClOClO33

SCNSCN1-1-

chapter 7 chemical formulas and bonding

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set of valence electrons