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Chemical Nomenclature
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Ionic Bonds vs Covalent Bonds
Metal + Non-Metal Metal (CATION) always first followed by Non-metal (ANION) Electrons are Transferred Covalent Bonds (Sometimes called Molecular) Non-metal + Non-metal Electrons are Shared We will talk more about how these bonds form, their properties, etc next semester
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Two Types of Compounds Ionic Molecular Smallest piece Formula Unit
Molecule Types of elements Metal and Nonmetal Nonmetals Solid, liquid or gas State solid Melting Point High >300ºC Low <300ºC
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Ionic Compounds with Transition Metals
IONIC NOMENCLATURE Ionic Nomenclature Binary Compounds Ternary Compounds Ionic Compounds with Transition Metals
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Binary Ionic Compounds
Binary = 2 elements total in the cmpd Naming Binary Compounds Take the cation (metal) and name it just like the element on the periodic table Take the anion (non-metal) and change the ending of the element to –ide Ex: Al2O3 = Aluminum Oxide
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Most commonly missed –ide changes
Oxygen = Oxide Sulfur = Sulfide Hydrogen = Hydride Phosphorus = Phosphide Nitrogen = Nitride Silicon = Silicide Selenium = Selenide Carbon = Carbide
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Practice These: NaCl Mg3N2 K2S LiH SrBr2 AlP
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Writing Formulas for Binary Ionic Compounds
Step 1 Write elements with their charges (M first, then NM) Step 2 Cross charges and make subscripts from them (remove + or - ) Write elements together as compound Step 3 If necessary, simplify subscripts to lowest terms Al+3 O2- Al2O3 Step 3 not necessary
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When Step 3 is needed Step 1 Step 2 Step 3 Al+3 N3- Al3O3 AlO
Write elements with their charges (M first, then NM) Step 2 Cross charges and make subscripts from them (remove + or - ) Write elements together as compound Step 3 If necessary, simplify subscripts to lowest terms Al+3 N3- Al3O3 AlO (3 & 3 both divisible by 3 to give 1)
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When Step 3 is needed Step 1 Step 2 Step 3 Mn+4 O2- Mn2O4 MnO2
Write elements with their charges (M first, then NM) Step 2 Cross charges and make subscripts from them (remove + or - ) Write elements together as compound Step 3 If necessary, simplify subscripts to lowest terms Mn+4 O2- Mn2O4 MnO2 (2 & 4 both divisible by 4 to give 1 & 2)
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Ternary Ionic Compounds
Ternary = 3 or more elements in compound Naming Ternary Ionic Compounds Name like Binary (element name + --ide)EXCEPT when POLYATOMIC IONS are used as metals or non-metals You will need to memorize the most common polyatomic Ions
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Polyatomic Ions to Memorize (Name, Formula & Charge)
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Practice (it may help to put parentheses around polyatomic when you ID them)
NH4Cl Mg(OH)2 NaNO3 AlPO4 K2SO4 H2O2
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Formulas for Ternary Compounds (involve polyatomic ions)
Still… cation FIRST, anion SECOND Na+ OH- Criss-cross the superscript charge to get the subscripts. Na1 OH1 Reduce the subscript to the least whole number ratio if needed. NaOH
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Ternary Compounds (Cont.)
If polyatomic ion has a subscript in the formula greater than 1, you must put parentheses around the polyatomic ion and place the subscript outside the parenthesis. Al(OH)3
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Practice Example: Barium nitrate
1. Write the symbols/formulas for the cation and anion, including CHARGES! 2. Cross Charges. 3. Simplify subscripts. Use parentheses if you need more than one of a polyatomic ion.
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Practice Example: Ammonium sulfate
1. Write the formulas for the cation and anion, including CHARGES! 2. Cross Charges. 3. Simpifly subscripts. Use parentheses if you need more than one of a polyatomic ion.
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Try these on your own… Magnesium carbonate Strontium hydroxide
Aluminum phosphate
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Ionic Compounds with Transition Metals
Remember Transition Metals are called transition because they can have varying oxidation states!!!
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Metals that form more than One Cation
The name of metals with two or more positive ions (cations) use a Roman numeral to identify ionic charge. Lead Pb lead(II) Pb lead(IV) Copyright © by Pearson Education, Inc. Publishing as Benjamin Cummings
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Naming Ionic Compounds with Transition Metals
Step 1: The easiest way to do this is to uncross the subscripts back to charges. ALWAYS MOVE THE ANION’S CHARGE BACK FIRST! CHECK & MAKE SURE THE ANION CHARGE IS WHAT IT SHOULD BE! Ex. Fe3N2 uncrossed: Fe2+ N3- What we expect on N Ex. MnO2 uncrossed: Mn+2 O-1 NOT WHAT WE EXPECT ON O! WE KNOW O should be a -2 which meant the subscripts simplified. So…. REAL ANSWER: MnO2 uncrossed: Mn+4 O2-
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Naming Ionic Compounds with Transition Metals
Step 2-4 Once you know the charges, now name the transition metal with Roman Numerals: I II III IV V VI Ex: Fe+3 O2- Iron (III) Oxide Ex: Mn+4 O2- Manganese (IV) Oxide
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Writing Formulas for Ionic Compounds with Transition Metals
Just like Binary & Ternary Rules Now the metal charge is given to you, you don’t need to remember it or look it up! Don’t forget ONLY transition metals use roman numerals Don’t forget about your polyatomics
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Practice!!! Mn2O7 NbCl5 TiP Pd(SO4)2 PtF2 Os2O3 Ir(NO3)4 Co(ClO)2
Fe2S3 AuI3 Manganese (VII) Oxide Niobium (V) Chloride Titanium (III) Phosphide Palladium (IV) Sulfate Platinum (II) Fluoride Osmium (III) Oxide Iridium (IV) Nitrate Cobalt (II) Hypochloride Iron (III) Sulfide Gold (III) Iodide
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Sometimes…. You will see Transition metals named by their classical/traditional names. I want you to be aware of the following, but you won’t be tested over them in this class
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Traditional (Classical)
Systematic (STOCK) Name Traditional (Classical) Fe3+ Iron (III) Ferric Fe2+ Iron (II) Ferrous Cu2+ Copper (II) Cupric Cu1+ Copper (I) Cuprous Sn4+ Tin (IV) Stannic Sn2+ Tin (II) Stannous Pb4+ Lead (IV) Plumbic Pb2+ Lead (II) Plumbous
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Traditional System Name the metal first; use Latin names of metals.
In binary compounds the nonmetal takes the suffix –ide. (Like before) The ion with the lower charge takes the suffix –ous The ion with the higher charge takes the suffix –ic.
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Naming Covalent Compounds
Covalent Nomenclature Diatomic Molecules Binary Molecules Remember, covalent bonds form between a non-metal and a non-metal and the electrons are shared!
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Br2I2N2Cl2H2O2F2 Diatomic Molecules
When some elements are by themselves, with no other element, they pair up with other elements that are like them. They are called diatomic molecules! We name them just by the element name on the periodic table Br2I2N2Cl2H2O2F2
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Practice Br2 H2 Oxygen Chlorine Bromine Hydrogen O2 Cl2
If these 7 elements are paired with other elements, they will NOT be named like this! They will be named like we talk about later!
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Binary Covalent Compounds
Covalent Compounds use Prefixes to name compounds ALWAYS use prefixes except: Only use mono on the second element If you have a diatomic molecule 1st: (prefixelementname) 2nd:(prefixelementendinide) PREFIXES 1-mono 2-di 3-tri 4-tetra 5-penta 6-hexa 7-hepta 8-octa 9-nona 10-deca
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Examples P2O5 diphosphorous pentoxide OF2 oxygen difluoride PBr3 phosphorous tribromide
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Practice! CO2 CO P2O5 N2O SiO2 CBr4 SO2 PBr5 ICl3 NI3 N2O3 B2H6 NBr3
SCl6 P4O10 S7O2 Carbon dioxide Carbon monoxide Diphosphorous pentaoxide Dinitrogen monoxide Silicon dioxide Carbon tetrabromide Sulfur dioxide Phosphorous pentabromide Iodine trichloride Nitrogen triiodide Dinitrogen trioxide Diboron hexahydride Nitrogen tribromide Sulfur hexachloride Tetraphosphorous decaoxide Heptasulfur dioxide
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To Get Covalent Formulas, just go backwards….
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In reverse to get Formulas!
1. Silicon tetrafluoride 2. Dinitrogen trisulfide 3. Sulfur trioxide 4. Dinitrogen tetroxide 5. Nitrogen monoxide 6. Nitrogen dioxide 7. Tetraphosphorous octaoxide 8. Tetraphosphorous nonasulfide 9. Diarsenic pentoxide 10. Phosphorous trichloride 11. Carbon tetrachloride 12. Dihydrogen monoxide 13. Selenium hexafluoride 14. Iodine heptafluoride 15. Tetraarsenic decoxide 16. Carbon disulfide 17. Oxygen difluoride SiF4 N2S3 SO3 N2O4 NO NO2 P4O8 P4S9 As2O5 PCl3 CCl4 H2O SeFl6 IF7 As4O10 CS2 OF2
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Naming Acids Acid formulas usually begin with H
We name them according to how the ANION name ends! Common Acids we use: HCl: Hydrochloric Acid HNO3: Nitric Acid H2SO4: Sulfuric Acid
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HCl: Hydrochloric Acid
Anion Ending Acid Name Example Binary Acids (no oxygen in formula) -ide Hydro-(stem) –ic Acid HCl: Hydrochloric Acid (from chloride) Ternary Acids (oxygen in the formula) -ate (stem)-ic acid HNO3: Nitric Acid (from nitrate) -ite (stem)-ous Acid H2SO3 Sulfurous Acid (from sulfite) (per)-ic per-stem-ic Acid HClO4 Perchloric Acid Hypo-ite per-stem-ous Acid HClO Hypochlorous Acid
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Acid Nomenclature Flowchart
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Acid Nomenclature HBr (aq) H2CO3 H2SO3 hydrobromic acid
No oxygen, -ide hydrobromic acid Has oxygen, -ate carbonic acid Has oxygen, -ite sulfurous acid
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Acid Nomenclature hydrofluoric acid sulfuric acid nitrous acid H+ F-
2 elements H+ F- HF (aq) 3 elements, -ic H+ SO42- H2SO4 3 elements, -ous H+ NO2- HNO2
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Name ‘Em! HI (aq) HCl H2SO3 HNO3 HIO4
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Write the Formula! Hydrobromic acid Nitrous acid Carbonic acid
Phosphoric acid Hydrotelluric acid
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Hydrates Some compounds contain H2O in their structure.
These compounds are called hydrates. This is different from (aq) because the H2O is part of the molecule (not just surrounding it). The H2O can usually be removed if heated. A dot separates water: e.g. CuSO4•5H2O is copper(II) sulfate pentahydrate. Name the ionic part (the salt) just the way you would as before; a greek prefix indicates the # of H2O groups.
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Hydrates (examples) Na2SO4•10H2O sodium sulfate decahydrate NiSO4•6H2O
sodium carbonate monohydrate barium chloride dihydrate sodium sulfate decahydrate nickel(II) sulfate hexahydrate Na2CO3•H2O BaCl2•2H2O
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Nomenclature Summary Flowchart
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