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Naming Chemicals. AP Chemistry. Classes of Chemicals. Elements Ionic Compounds Covalent Compounds Organic Compounds. Gold. Elements. All elements on the periodic table All just one word: iron, sodium, neon, etc. All neutrally charged Mostly monatomic: Fe, Na, Ne - PowerPoint PPT Presentation
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Naming Chemicals
AP ChemistryAP Chemistry
Classes of Chemicals
ElementsElements Ionic CompoundsIonic Compounds Covalent CompoundsCovalent Compounds Organic CompoundsOrganic Compounds
Elements
All elements on the periodic tableAll elements on the periodic table All just one word: iron, sodium, neon, etc.All just one word: iron, sodium, neon, etc. All neutrally chargedAll neutrally charged Mostly monatomic: Fe, Na, NeMostly monatomic: Fe, Na, Ne Some Some didiatomic:atomic: H H2 2 OO2 2 NN2 2 ClCl2 2 BrBr2 2 II2 2 FF22
Some Some polypolyatomic: Satomic: S88, P, P44
Gold
Ionic Compounds
Made of one metal positive ion (cation) and Made of one metal positive ion (cation) and one non-metal negative ion (anion)one non-metal negative ion (anion)
Always two words starting with the cation Always two words starting with the cation and ending with the anionand ending with the anion
Cation is same name as elementCation is same name as element Anion always has a different suffixAnion always has a different suffix
Sodium chloride
Anion Suffixes
MonatomicMonatomic atoms end with atoms end with –ide–ide Oxygen atom = OOxygen atom = O OxOxideide ion = O ion = O-2-2
Sulfur atom = SSulfur atom = S SulfSulfideide ion = S ion = S-2-2
Chlorine atom = ClChlorine atom = Cl ChlorChlorideide ion = Cl ion = Cl-1-1
Oxy-Anions
Oxy-Oxy-anions end in anions end in –ate–ate Sulfate = SOSulfate = SO44
-2-2 Chlorate = ClOChlorate = ClO33-1-1
Chromate = CrOChromate = CrO44-2-2 Nitrate = NONitrate = NO33
-1-1
If the anion is further oxidized then add the If the anion is further oxidized then add the prefix prefix per-per-
ClOClO33-1-1 = chlorate = chlorate ClO ClO44
-1-1 = = perperchloratechlorate
Less Oxidation
If the anion is less oxidized by 1 then change If the anion is less oxidized by 1 then change the –the –ateate suffix to an – suffix to an –iteite suffix suffix
SOSO44-2-2 = sulf = sulfateate SOSO33
-2-2 = sulf = sulfiteite ClOClO33
-1-1 = chlor = chlorateate ClOClO22-1-1 = chlor = chloriteite
If the anion is less oxidized If the anion is less oxidized againagain then add then add the prefix the prefix hypo-hypo-
ClOClO-1-1 = = hypohypochlorchloriteite SOSO22-2-2 = = hypohyposulfsulfiteite
Summary
Per- -atePer- -ate -ate-ate -ite-ite Hypo- -iteHypo- -iteChlor-Chlor- ClOClO44
-1-1
PerchloratePerchlorateClOClO33
-1-1
chloratechlorateClOClO22
-1-1
chloritechloriteClOClO-1-1
hypochloritehypochlorite
Sulf-Sulf- SOSO44-2-2
sulfatesulfateSOSO33
-2-2
SulfiteSulfiteSOSO22
-2-2
HyposulfiteHyposulfite
Nitr-Nitr- NONO33-1-1
NitrateNitrateNONO22
-1-1
NitriteNitrite
Phos-Phos- POPO44-3-3
PhosphatePhosphatePOPO33
-3-3
PhosphitePhosphite
Sulfur Replacement
If one of the oxygens in an oxy-anion is If one of the oxygens in an oxy-anion is replaced with a sulfur then add the prefix replaced with a sulfur then add the prefix thio-thio-
SOSO44-2-2 = sulfate = sulfate SS22OO33
-2-2 = = thiosulfatethiosulfate
SOSO33-2-2 = sulfite = sulfite SS22OO22
-2-2 = thiosulfite = thiosulfite CNOCNO-1-1 = cyanate = cyanate CNSCNS-1-1 = thiocyanate = thiocyanate
Anion Summary
Mon-atomic anions end in –ideMon-atomic anions end in –ide Oxy-anions end in –ate or –iteOxy-anions end in –ate or –ite Add prefixes per- and hypo- when Add prefixes per- and hypo- when
necessarynecessary Add thio- prefix when a sulfur replaces and Add thio- prefix when a sulfur replaces and
oxygenoxygen
Combining Ions•Ionic compounds are always neutrally charged so the number of each ion within the compound is fixed •Sodium oxide:
Na+1 O-2 Since the compound must be neutral we need another positive charge
Na+1 Now we have two sodium atoms to balance out the oxide so the final formula is:
Na2O
Parenthesis
Use parenthesis for multiple polyatomic Use parenthesis for multiple polyatomic ionsions
Aluminum chromate
Al+3 CrO4-2
Al2(CrO4)3
Be careful of Hydroxides!Calcium hydroxide
Ca+2 OH-1
Ca(OH)2CaOH2
Transition Metals
Transition Metals
Transition Metals often have more than one Transition Metals often have more than one chargecharge
Examples: FeExamples: Fe+2+2 and Fe and Fe+3+3
This makes a difference in formulae:This makes a difference in formulae: Iron chloride could be:Iron chloride could be: FeClFeCl22 or FeCl or FeCl33
So what do we do? Since FeClSince FeCl22 and FeCl and FeCl33 are obviously not the same are obviously not the same
compound, they can’t both have the same name.compound, they can’t both have the same name. We differentiate them by using a Roman Numeral We differentiate them by using a Roman Numeral
to indicate the charge on the transition metalto indicate the charge on the transition metal FeFe+2+2 and Cl and Cl-1-1 FeCl FeCl22 = iron (II) chloride = iron (II) chloride FeFe+3+3 and Cl and Cl-1-1 FeCl FeCl33 = iron (III) chloride = iron (III) chloride Be sure to note that the roman numeral indicates Be sure to note that the roman numeral indicates
chargecharge and not and not numbernumber..
Quick practice Sodium bromideSodium bromide NaBrNaBr
• Calcium oxide • CaO• Aluminum nitrate • Al(NO3)3
• Ammonium phosphate • (NH4)3PO4
• Barium hydroxide • Ba(OH)2
• Copper (I) sulfide • Cu2S• Copper (II) sulfate • CuSO4
• Iron (III) dichromate • Fe2(Cr2O7)3
More practice Potassium hypochloritePotassium hypochlorite KClOKClO
• Sodium sulfite • Na2SO3
• Aluminum bromate • Al(BrO3)3
• Ammonium phosphite • (NH4)3PO3
• Magnesium nitrite • Mg(NO2)2
• Iron (III) perchlorate • Fe(ClO4)3
• Strontium cyanate • Sr(CNO)2
• Copper (I) thiosulfate • Cu2S2O3
Covalent Compounds
Comprised of two or more non-metals Comprised of two or more non-metals covalently bondedcovalently bonded
Start with less electronegative and end with Start with less electronegative and end with more electronegativemore electronegative
Name as normal except that all compounds Name as normal except that all compounds change the second element to an –change the second element to an –ideide endingending
Covalent Examples
CO = carbon oxCO = carbon oxideide CSCS22 = carbon sulf = carbon sulfideide NFNF33 = nitrogen fluor = nitrogen fluorideide
Notice in each example the more Notice in each example the more electronegative atom is second and ends in electronegative atom is second and ends in -ide-ide
Problem
Covalent compounds can combine in Covalent compounds can combine in multiple proportions- that is there can be multiple proportions- that is there can be more than one ratio of atoms in a compoundmore than one ratio of atoms in a compound
COCO vs. vs. COCO22
They can’t both be carbon oxideThey can’t both be carbon oxide NONO22 vs.vs. NN22OO44
They can’t both be nitrogen oxideThey can’t both be nitrogen oxide
Solution?
Use prefixes to indicate the number of Use prefixes to indicate the number of covalently bonded atoms present in the covalently bonded atoms present in the moleculemolecule
COCO vs.vs. COCO22
Carbon Carbon monmonoxideoxide Carbon Carbon didioxideoxide
Prefixes 11 22 33 44 55 66 77 88 99 1010
Mono-Mono- Di-Di- Tri-Tri- Tetra-Tetra-
Hexa-Hexa- Penta-Penta-
Hepta-Hepta- Octa-Octa- Nona-Nona- Deca-Deca-
Overall Covalent Rules Comprised of two or more non-metals covalently Comprised of two or more non-metals covalently
bondedbonded Start with less electronegative and end with more Start with less electronegative and end with more
electronegativeelectronegative Name as normal except that all compounds change Name as normal except that all compounds change
the second element to an –the second element to an –ideide ending ending Add a prefix to indicate number of atoms in the Add a prefix to indicate number of atoms in the
compoundcompound The second atom ALWAYS gets a prefixThe second atom ALWAYS gets a prefix The first atom can ignore MONO-The first atom can ignore MONO-
Practice COCO Carbon monoxideCarbon monoxide NN22OO55
Dinitrogen pentoxideDinitrogen pentoxide PClPCl55
Phosphorus pentachloridePhosphorus pentachloride
SOSO33 Sulfur trioxideSulfur trioxide
NN22OO Dinitrogen monoxideDinitrogen monoxide
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