Download - Chapter 7 chemical formulas and bonding
LABORATORY CHEMISTRY
CHAPTER 7 1
Chapter 7Chapter 7chemical formulas and bondingchemical formulas and bonding
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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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
LABORATORY CHEMISTRY
CHAPTER 7 4
IONIC BONDINGIONIC BONDING
– 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
LABORATORY CHEMISTRY
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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
LABORATORY CHEMISTRY
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IONIC BONDINGIONIC BONDING
Na Na+
- -
Na
[Ne] 3s1
Na+
[Ne]
A SODIUM ATOM READILY LOSES ONE OF ITS ELECTRONS
LABORATORY CHEMISTRY
CHAPTER 7 7
IONIC BONDINGIONIC BONDING
Cl Cl--
-
THE CHLORINE ATOM READILY GAINS AN ELECTRON
Cl[Ne] 3s2, 3p5 Cl-
[Ne] 3s2, 3p6
-
LABORATORY CHEMISTRY
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IONIC BONDINGIONIC BONDING
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
LABORATORY CHEMISTRY
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IONIC BONDINGIONIC BONDING
Cl--Na+
IN BOTH CASES THE ION THAT FORMS HAS THE ELECTRON CONFIGURATION OF A NOBLEGAS
Ne Ar
LABORATORY CHEMISTRY
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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
LABORATORY CHEMISTRY
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IONIC BONDINGIONIC BONDING ns1 an
d ns2
np1
np2
np3
np4
np5
np6
LABORATORY CHEMISTRY
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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
LABORATORY CHEMISTRY
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IONIC BONDINGIONIC BONDING
LABORATORY CHEMISTRY
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 ) )
LABORATORY CHEMISTRY
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
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IONIC BONDINGIONIC BONDING
– 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
LABORATORY CHEMISTRY
CHAPTER 7 17
LABORATORY CHEMISTRYOXIDATION REFERENCE CHART
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
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LABORATORY CHEMISTRYOXIDATION REFERENCE CHART
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.
LABORATORY CHEMISTRY
CHAPTER 7 19
LABORATORY CHEMISTRYOXIDATION REFERENCE CHART
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)
LABORATORY CHEMISTRY
CHAPTER 7 20
IONIC BONDINGIONIC BONDING
– 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]]++ ) )
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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.
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
CHAPTER 7 27
COVALENT BONDINGCOVALENT BONDING
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
LABORATORY CHEMISTRY
CHAPTER 7 28
COVALENT BONDINGCOVALENT BONDING
– 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
LABORATORY CHEMISTRY
CHAPTER 7 29
COVALENT BONDINGCOVALENT BONDING
– TRIPLE BONDSTRIPLE BONDS ETHYNE (CETHYNE (C22HH22))
H HC C H C C H
TRIPLE BOND
H C C H
TRIPLE BOND
SINGLEBOND
SINGLEBOND
LABORATORY CHEMISTRY
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..
LABORATORY CHEMISTRY
CHAPTER 7 31
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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.
LABORATORY CHEMISTRY
CHAPTER 7 32
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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
LABORATORY CHEMISTRY
CHAPTER 7 33
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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
LABORATORY CHEMISTRY
CHAPTER 7 34
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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!
LABORATORY CHEMISTRY
CHAPTER 7 35
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
P Cl
Cl
Cl
FOURTH, PLACE THE REMAINING TWO
ELECTRONS ON THE CENTRAL ATOM,
COMPLETING THE OCTETAROUND THAT ATOM
AS WELL.
LABORATORY CHEMISTRY
CHAPTER 7 36
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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
LABORATORY CHEMISTRY
CHAPTER 7 37
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
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
LABORATORY CHEMISTRY
CHAPTER 7 38
DRAWING LEWIS DRAWING LEWIS STRUCTURESSTRUCTURES
DRAW THE LEWIS STRUCTURE DRAW THE LEWIS STRUCTURE FOR THE FOLLOWING FOR THE FOLLOWING COMPOUNDSCOMPOUNDS– CHCH44
– HCNHCN
– SOSO442-2-
– CFCF22ClCl22
LABORATORY CHEMISTRY
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:
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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.
LABORATORY CHEMISTRY
CHAPTER 7 42
EXCEPTIONS TO THE OCTET EXCEPTIONS TO THE OCTET RULERULE
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-
LABORATORY CHEMISTRY
CHAPTER 7 43
EXCEPTIONS TO THE OCTET EXCEPTIONS TO THE OCTET RULERULE
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
LABORATORY CHEMISTRY
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..
LABORATORY CHEMISTRY
CHAPTER 7 45
BOND POLARITY AND BOND POLARITY AND ELECTRONEGATIVITYELECTRONEGATIVITY
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)
LABORATORY CHEMISTRY
CHAPTER 7 46
BOND POLARITY AND BOND POLARITY AND ELECTRONEGATIVITYELECTRONEGATIVITY
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
LABORATORY CHEMISTRY
CHAPTER 7 47
BOND POLARITY ANDBOND POLARITY AND
ELECTRONEGATIVITYELECTRONEGATIVITY
COMPOUNDCOMPOUND
ELECTRONEGATIVITYELECTRONEGATIVITY
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
LABORATORY CHEMISTRY
CHAPTER 7 48
BOND POLARITY ANDBOND POLARITY AND
ELECTRONEGATIVITYELECTRONEGATIVITY
– 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
LABORATORY CHEMISTRY
CHAPTER 7 49
BOND POLARITY ANDBOND POLARITY AND
ELECTRONEGATIVITYELECTRONEGATIVITY
– 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+ -
LABORATORY CHEMISTRY
CHAPTER 7 50
BOND POLARITY ANDBOND POLARITY AND
ELECTRONEGATIVITYELECTRONEGATIVITY
– 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
LABORATORY CHEMISTRY
CHAPTER 7 51
BOND POLARITY ANDBOND POLARITY AND
ELECTRONEGATIVITYELECTRONEGATIVITY
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)?
LABORATORY CHEMISTRY
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!!
!!!!
LABORATORY CHEMISTRY
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
(1) Check the oxidation number
of the nonmetal
LABORATORY CHEMISTRY
CHAPTER 7 54
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER
Na
1Cl
1-
Oxidation Number (Valence)
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
LABORATORY CHEMISTRY
CHAPTER 7 55
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER
METALS WITH ONE OXIDATION NUMBERMETALS WITH ONE OXIDATION NUMBER
Na1+
Cl1- = 0
1 11 1
1+ 1- = 0
X X
NaNaClCl
LABORATORY CHEMISTRY
CHAPTER 7 56
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER
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
LABORATORY CHEMISTRY
CHAPTER 7 57
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER
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
LABORATORY CHEMISTRY
CHAPTER 7 58
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH ONE PRIMARY MONOATOMIC METALS WITH ONE PRIMARY OXIDATION NUMBEROXIDATION NUMBER
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
LABORATORY CHEMISTRY
CHAPTER 7 59
(3) If the metal is monoatomic….
NAME THE METAL
Ca NO3
calcium
(1) Check the oxidation number
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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.
LABORATORY CHEMISTRY
CHAPTER 7 62
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
METALS WITH TWO OXIDATION NUMBERSMETALS WITH TWO OXIDATION NUMBERS
Fe2
Cl
1-
Oxidation Number (Valence)
Oxidation Number (Valence)
Metal: Written first !
NonMetal: Written Second
NAME THE METAL ION NAME THE NONMETAL ION
IRON CHLORIDEIDE
2
Subscript: to balance the charges
LABORATORY CHEMISTRY
CHAPTER 7 63
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
But iron has two possible oxidation numbershow can we explainwhich one to use in the compound?
Fe2+/3+
LABORATORY CHEMISTRY
CHAPTER 7 64
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 65
NAME THE NONMETALUSE THE ROOT
+“IDE”
(BINARY COMPOUND)
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 66
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
* ( ) may or may not be used
LABORATORY CHEMISTRY
CHAPTER 7 67
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 68
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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+
LABORATORY CHEMISTRY
CHAPTER 7 69
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 70
NAMING BINARY COMPOUNDSNAMING BINARY COMPOUNDS MONOATOMIC METALS WITH TWO PRIMARY MONOATOMIC METALS WITH TWO PRIMARY OXIDATION NUMBERSOXIDATION NUMBERS
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
* ( ) may or may not be used
LABORATORY CHEMISTRY
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.
LABORATORY CHEMISTRY
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?
LABORATORY CHEMISTRY
CHAPTER 7 73
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
NAMING COMPOUNDS WITH MULTIPLE OXIDATION NUMBERS
Mn
2+3+4+5+6+7+
O2-First, check out the non-metal…and get
its oxidation number.
LABORATORY CHEMISTRY
CHAPTER 7 74
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
NAMING COMPOUNDS WITH MULTIPLE OXIDATION NUMBERS
Mn
2+3+4+5+6+7+
O2-Next, check the given
formula and make sure the oxidation numbers
add up to zero.
LABORATORY CHEMISTRY
CHAPTER 7 75
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
NAMING COMPOUNDS WITH MULTIPLE OXIDATION NUMBERS
Mn
2+3+4+5+6+7+
O2-
Mn O
Mn2 O3
Mn O2
Mn2 O5
Mn O3
Mn2 O7Look at the possibilities
LABORATORY CHEMISTRY
CHAPTER 7 76
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
Mn O
Mn2 O3
Mn O2
NAMING COMPOUNDS WITH MULTIPLE OXIDATION NUMBERS
manganese
manganese
manganese
You must tellthe reader whichmanganese you
used!!
THERE ARETWO WAYS
TO DO THIS !!
LABORATORY CHEMISTRY
CHAPTER 7 77
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
Mn O
Mn2 O3
Mn O2
manganese
manganese
manganese
FIRST !!!!
mon
di
di
oxide
oxide
oxide
USE PREFIXES
tri
LABORATORY CHEMISTRY
CHAPTER 7 78
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
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 !
LABORATORY CHEMISTRY
CHAPTER 7 79
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
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
* ( ) may or may not be used
LABORATORY CHEMISTRY
CHAPTER 7 80
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION ELEMENTS WITH MULTIPLE OXIDATION NUMBERSNUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 81
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION ELEMENTS WITH MULTIPLE OXIDATION NUMBERSNUMBERS
Mn O
Mn2 O3
Mn O2
manganese
manganese
manganese
SECOND !
(II)
III
IV
oxide
oxide
oxide
USE ROMAN
NUMERALS
LABORATORY CHEMISTRY
CHAPTER 7 82
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
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
LABORATORY CHEMISTRY
CHAPTER 7 83
NAMING COMPOUNDSNAMING COMPOUNDSELEMENTS WITH MULTIPLE OXIDATION NUMBERSELEMENTS WITH MULTIPLE OXIDATION NUMBERS
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
* ( ) may or may not be used
LABORATORY CHEMISTRY
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+)
LABORATORY CHEMISTRY
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 = =
LABORATORY CHEMISTRY
CHAPTER 7 86
NAMING ACIDSNAMING ACIDS
HCl (aq)
H 2 S (aq)HF (aq)
HBr (aq)
HI (aq)
hydrochloric acid
hydrosulfuric acid
hydrofluoric acid
hydrobromic acid
hydroiodic acid
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
CHAPTER 7 88
NAMING ACIDSNAMING ACIDS
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
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
LABORATORY CHEMISTRY
CHAPTER 7 94
CRITICAL THINKING AND CRITICAL THINKING AND PROBLEM SOLVINGPROBLEM SOLVING
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
LABORATORY CHEMISTRY
CHAPTER 7 95
CRITICAL THINKING AND CRITICAL THINKING AND PROBLEM SOLVINGPROBLEM SOLVING
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
______________________________________
LABORATORY CHEMISTRY
CHAPTER 7 96
CRITICAL THINKING AND CRITICAL THINKING AND PROBLEM SOLVINGPROBLEM SOLVING
DRAW THE DRAW THE EQUIVALENT EQUIVALENT RESONANCE RESONANCE STRUCTURES STRUCTURES FOR THE FOR THE FOLLOWING FOLLOWING MOLECULESMOLECULES
SOSO33
NONO331-1-
ClOClO33
SCNSCN1-1-