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NOMENCLATURE

• NAMES AND FORMULAS OF CHEMICAL COMPOUNDS

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TYPES OF COMPOUNDS

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RECOGNIZING BONDS

• COVALENT BONDS BETWEEN TWO NONMETALS

• IONIC BONDS BETWEEN ONE METAL AND ONE NONMETAL

• REMINDER THAT METALS ARE LEFT OF STAIRSTEPS AND NONMETALS ARE RIGHT

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RECOGNIZING BOND EXAMPLES

• WHAT KIND OF BOND IS BETWEEN:– K AND Cl– S AND P– Ba AND O– Pb AND N

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BONDS AND COMPOUND TYPES

• COMPOUNDS FORMED FROM– IONICALLY BONDED ELEMENTS ARE

CALLED IONIC COMPOUNDS– COVALENTLY BONDED ELEMENTS ARE

CALLED MOLECULAR COMPOUNDS

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NAMES OF BINARY MOLECULAR COMPOUNDS

• PREFIXES INDICATE THE NUMBER OF ATOMS IN A COMPOUND

• DON’T USE PREFIX FOR FIRST ELEMENT IF THERE IS ONE ATOM

• SECOND ELEMENT ENDS IN “IDE”

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PREFIXES FOR MOLECULAR COMPOUNDS

• MONO

• DI

• TRI

• TETRA

• PENTA

• HEXA

• HEPTA

• OCTA

• NONA

• DECA

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EXAMPLE MOLECULAR NAMES

• CO2

• CARBON DIOXIDE• CO• CARBON MONOXIDE• N2O5

• DINITROGEN PENTOXIDE• As3N6

• TRIARSENIC HEXANITRIDE

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2ND ELEMENT SPELLING

NITRIDE OXIDE FLUORIDE

PHOSPHIDE SULFIDE CHLORIDE

ARSENIDE SELENIDE BROMIDE

TELLURIDE IODIDE

ASTATIDE

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MOLECULAR COMPOUND FORMULAS

• CHANGE PREFIX TO SUBSCRIPT

• DON’T WRITE A “1” SUBSCRIPT

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EXAMPLE MOLCULAR FORMULAS

• ARSENIC TRIFLUORIDE

• AsF3

• CARBON TETRAFLUORIDE

• CF4

• DIPHOSPHORUS HEXABROMIDE

• P2Br6

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MOLECULES

• ATOMS OF TWO (OR MORE) DIFFERENT ELEMENTS COVALENTLY BONDED

• SIMPLEST UNIT OF COVALENTLY BONDED ATOMS

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MOLECULE EXAMPLES

• ARE THE FOLLOWING MOLECULES?– BaS

– N2O

– Br2

– S8

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IONS

• CATION - ATOM THAT HAS LOST 1 OR MORE ELECTRONS IS IS POSITIVE

• ANION - ATOM THAT HAS GAINED 1 OR MORE ELECTRONS AND IS NEGATIVE

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VALENCE NUMBER

• CHARGE ON AN ION AFTER IT HAS GAINED OR LOST ELECTRONS

• ALSO CALLED OXIDATION STATE

• SHOWN ON PERIODIC TABLE

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VALENCE NUMBERS

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MULTI-VALENCE METALS

• METALS IN SUNKEN SECTION OF PERIODIC TABLE CAN HAVE MORE THAN ONE CHARGE OR VALENCE NUMBER

• MUST LOOK THEM UP ON PT

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FORMULA UNIT

• SIMPLEST UNIT OF IONICALLY BONDED ATOMS

• LOWEST POSSIBLE SUBSCRIPTS MUST BE USED FOR IONIC COMPOUNDS TO HAVE CORRECT FORMULA UNIT

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IONIC COMPOUNDS

• FORMED FROM A CATION AND AN ANION

• TOTAL POSITIVE CHARGE = TOTAL NEGATIVE CHARGE

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FORMULAS OF BINARY IONIC COMPOUNDS

• CATIONS ARE ALWAYS WRITTEN 1ST

• Na+1 Cl-1

• Na1Cl1• DON’T WRITE 1’S

• NaCl

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CRISSCROSS RULE

• CROSS VALENCE NUMBERS (IGNORE SIGNS)

• REDUCE TO LOWEST VALUES

• INSURES FORMULA UNITS ARE NEUTRAL (CHARGES CANCEL)

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EXAMPLES OF BINARY IONIC COMPOUNDS

• Mg Cl

• MgCl2• Ca O

• Ca2O2

• WHICH REDUCES TO CaO• Sn+4 S

• SnS2

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NAMES OF BINARY IONIC COMPOUNDS

• WRITE NAME OF CATION• FOLLOW WITH NAME OF THE ANION

BUT CHANGE ENDING TO “IDE”• NUMBER OF ATOMS DOES NOT

AFFECT NAME OF AN IONIC COMPOUND!

• NO PREFIXES!• SAME SPELLING AS MOLECULAR

COMPOUNDS

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EXAMPLES OF NAMES

• NaCl

• SODIUM CHLORIDE

• MgCl2• MAGNESIUM CHLORIDE

• CaO

• CALCIUM OXIDE

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NAMES OF IONIC CMPDS WITH MULTI-VALENCE

CATIONS• VALENCE NUMBER OF CATION

BECOMES ROMAN NUMERAL WRITTEN IN PARENTHESES AFTER CATION NAME

• CALLED THE STOCK SYSTEM

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NAMES W/ MULTI-VALENCE II

• REVERSE THE CRISS CROSS TO FIGURE OUT THE CATION VALENCE

• USE ANION TO DETERMINE IF REDUCING OCCURRED, IF SO UNREDUCE

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EXAMPLES OF STOCK SYSTEM NAMES

• Fe2O3

• IRON (III) OXIDE

• SnS

• TIN (IV) SULFIDE

• MnP2

• MANGANESE (VI) PHOSPHIDE

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POLYATOMIC IONS

• 2 OR MORE ATOMS COVALENTLY BONDED THAT ACT LIKE A SINGLE ION

• FORM IONIC BONDS

• USUALLY ANIONS

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EXAMPLE POLYATOMIC IONS

• NO3-1 IS NITRATE

• SO4-2 IS SULFATE

• CO3-2 IS CARBONATE

• PO4-3 IS PHOSPHATE

• SEE HANDOUT CHART FOR OTHERS

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FORMULAS FOR TERNARY IONIC

COMPOUNDS• USE PARENTHESES AROUND

POLYATOMIC ION• USE CRISS-CROSS RULE• REDUCE OUTSIDE

PARENTHESES – NOT INSIDE• REMOVE PARENTHESES ONLY

IF SUBSCRIPT OUTSIDE IS 1

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FORMULA EXAMPLES

• Na (NO3)• Na1(NO3)1 WHICH REDUCES TO

NaNO3

• Ca (IO3)• Ca(IO3)2

• Al (SO4)• Al2(SO4)3

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NAMES OF MOST TERNARY IONIC

COMPOUNDS• WRITE NAME OF CATION• FOLLOW WITH NAME OF ANION

(NO CHANGES TO POLYATOMIC NAME)

• NUMBER OF EACH DOES NOT AFFECT THE NAME

• NO PREFIXES!

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EXAMPLE OF NAMES

• NaNO3

• SODIUM NITRATE

• Na2SO4

• SODIUM SULFATE

• Ca(IO3)2

• CALCIUM IODATE

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NAMES OF IONIC CMPDS W/ AMMONIUM CATION

• WRITE AMMONIUM

• FOLLOW WITH ANION

• IF ANION IS AN ELEMENT, CHANGE ENDING TO “IDE”

• IF ANION IS POLYATOMIC, MAKE NO CHANGES

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AMMONIUM EXAMPLES

• NH4OH

• AMMONIUM HYDROXIDE

• (NH4)2CrO4

• AMMONIUM CHROMATE

• (NH4)3N

• AMMONIUM NITRIDE

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MORE POLYATOMIC NAMING EXAMPLES

• Cu(HCO3)2

• COPPER (II) BICARBONATE

• FeSO3

• IRON (II) SULFITE

• CrC2O4

• CHROMIUM (II) OXALATE

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AQUEOUS SOLUTIONS

• SOLUTION IN WHICH WATER IS THE SOLVENT IS CALLED AQUEOUS

• A SUBSCRIPT OF (aq) INDICATES AN AQUEOUS SOLUTION

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DISSOCIATION

• THE SEPARATION OF AN IONIC COMPOUND INTO IONS BY WATER (AS IT DISSOLVES)

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IONIC ACIDS

• CONTAIN HYDROGEN AS A CATION

• RELEASE HYDROGEN IONS AS THEY DISSOCIATE

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BINARY IONIC ACIDS

• NAMES BEGIN WITH HYDRO- AND END WITH –IC

• FORMULAS: CRISSCROSS VALENCE NUMBERS SUBSCRIPTS AND ADD (aq) AFTER ANION SUBSCRIPT

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EXAMPLE BINARY ACID NAMES

• HCl(aq)

• HYDROCHLORIC ACID

• HF(aq)

• HYDROFLUORIC ACID

• HI(aq)

• HYDROIODIC ACID

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EXAMPLE BINARY ACID FORMULAS

• HYDROSULFURIC ACID

• H2S(aq)

• HYDROBROMIC ACID

• HBr(aq)

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TERNARY IONIC ACID NAMES

• CONTAIN HYDROGEN AND A POLYATOMIC ANION

• NAMES DO NOT BEGIN WITH HYDRO-

• NAMES END IN –IC IF ANION ENDS IN –ATE OR –IDE

• NAMES END IN –OUS IF ANION ENDS IN –ITE

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EXAMPLE TERNARY ACID NAMES

• HNO3(aq)

• NITRIC ACID

• H2SO4(aq)

• SULFURIC ACID

• HNO2(aq)

• NITROUS ACID

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TERNARY ACID FORMULAS

• HYDROGEN MUST BE THE CATION

• DETERMINE ANION FROM ACID NAME

• FOLLOW RULES FOR IONIC COMPOUNDS WITH POLYATOMIC IONS

• ADD (aq) AFTER ANION SUBSCRIPT

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EXAMPLE TERNARY ACID FORMULAS

• CHROMIC ACID

• H2CrO4(aq)

• SULFUROUS ACID

• H2SO3(aq)

• PHOSPHORIC ACID

• H3PO4(aq)