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Naming Chemical Compounds

Binary Ionic Compounds. Binary = 2 types of elementsIonic = made of ionsCompound = atoms bonded together. Ionic Compounds. Positive ions are attracted to Negative ionsFORMULA UNITCation always comes first, then anion. Elemental anions . When an element becomes an anion, it starts to end in i

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Naming Chemical Compounds

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    1. Naming Chemical Compounds

    2. Binary Ionic Compounds Binary = 2 types of elements Ionic = made of ions Compound = atoms bonded together

    3. Ionic Compounds Positive ions are attracted to Negative ions FORMULA UNIT Cation always comes first, then anion

    4. Elemental anions When an element becomes an anion, it starts to end in ide Fluoride Chloride Bromide Oxide Sulfide Nitride Phosphide

    5. Type I The cation has a predictable charge Alkali Metals +1 Alkaline Earth Metals +2 Group 3A +3 Silver Ag+ Zinc Zn2+

    6. Type II The cation has a variable charge All Transition metals except for Ag and Zn (for our purposes) The name will have a roman numeral to denote the CHARGE on the cation Fe2+ Fe3+ Cu+ Cu2+

    7. Naming ionic compouds (Type I and II) First name cation Just the name of element if Type I Name of element and roman numeral with charge on cation if Type II Then name anion Elemental anions end in ide When determining the formula, remember swap n drop

    8. Name the following: Na3N MgCl2 Al2O3 CuCl CuCl2 PbBr4 Sodium nitride Magnesium chloride Aluminum oxide Copper(I) chloride Copper(II) chloride Lead(IV) bromide

    9. Determine the formula of the following Aluminum chloride Magnesium Oxide Sodium nitride Calcium chloride Copper(I) sulfide Lead (II) bromide Iron(III) oxide AlCl3 MgO Na3N CaCl2 Cu2S PbBr2 Fe2O3

    10. Polyatomic Ions Many anions are not just ions of elements. Polyatomic Ions = many atomed particle with an overall charge Mostly nonmetals bonded to Oxygens

    11. Polyatomic Ion Naming Main polyatomic ion Ends in ate Example: Chlorate ClO3- One fewer oxygens Ends in -ite Example: Chlorite ClO2- Even fewer oxygens Hypo = under Example: Hypochlorite ClO- More oxygens than main ion Hyper = over, shortened to per Example: Perchlorate ClO4-

    12. Common Polyatomic Ions

    13. Common Polyatomic Ions Hydrogen can attach to the polyatomic ions as H+ This adds an H and reduces the overall charge by 1

    14. Name these compounds with PAIs AlPO4 Cu(NO3)2 Na2SO4 NaHCO3 Mg3(PO4)2 Aluminum phosphate Copper(II) nitrate Sodium sulfate Sodium bicarbonate Magnesium Phosphate

    15. Molecular Compounds Molecular compounds are not bonded by positive and negative ions They SHARE electrons Made of two non-metals Cannot predict or explain charges (no charges, because not LOSING or GAINING electrons SHARING)

    16. Naming Molecular Compounds (Type III) Because there is no way to neutralize the compounds (like for ions) we must determine how many there are another way: Use PREFIXES

    17. How to tell if its Type III Check the FIRST element is it a non-metal? If YES, its a Type III Name the first element as the element Name the second element ending in -ide

    18. Prefixes 1 2 3 4 5 6 7 8 9 10 Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

    19. Using prefixes If there is only one of the first element, you may omit the mono You may not omit any other prefixes The more electronegative element goes last (upper right hand corner) F, O, N, Cl,

    20. Name the following PCl3 CO2 NO N2O4 N2F5 OF2 Phosphorus trichloride Carbon dioxide Nitrogen monoxide Dinitrogen tetroxide Dinitrogen pentafluoride Oxygen difluoride

    21. Naming Practice! For each of the following compounds, determine whether it is type I, II, or III. FeCl3 NaCl Cu(OH)2 N2O BaSO4 PO5 (NH4)CO3 SnBr2

    22. Naming Practice! For each of the following compounds, determine the CHARGE on the cation (+1, +2, +3, or +4) FeCl3 Cu(OH)2 Cr2S3 NiS Pb(NO3)2 SnCl4

    23. Acids All acids have the H+ ion in them as the cation. All acids have acid in their name Consider Hydrochloric Acid HCl

    24. Naming Acids If the anion DOES NOT CONTAIN OXYGEN: Prefix hydro- Root name of anion element Suffix ic Examples HF H2S

    25. Naming Acids If the anion CONTAINS OXYGEN (ie: is a polyatomic ion) Root name of the PAI If anion ends in -ate, acid ends in ic If anion ends in ite, acid ends in ous

    26. Naming Acids Examples H2SO4 H2SO3 HNO3 HNO2 HC2H3O2 Phosphoric Acid Carbonic Acid Sulfuric Acid Sulfurous Acid Nitric Acid Nitrous Acid Acetic Acid H3PO4 H2CO3

    27. Organic Molecules Carbon based Naming is based on number of carbons Functional groups Sets of molecules attached to the carbons Naming is also based on what functional groups are where

    28. Alkanes The simplest organic molecules are Alkanes. Carbons are all single bonded to each other When not bonded to another carbon, bonded to a Hydrogen All alkanes end in -ane

    30. Prefixes Note that the prefixes pertain to all types of carbon based molecules with any types of functional groups or chains

    31. Alkenes and Alkynes A functional group can be a set of atoms, or the way they are bonded. Alkenes Carbons have double bonds between them Alkynes Carbons have triple bonds between them

    32. Alkenes and Alkynes To Name All alkenes end with ene. All alkynes end with yne Number the carbons in the longest chain. Carbon 1 is at the end of the chain closest to the first functional group Put the number that the bond is on, then the chain length (some name by putting the number BEFORE the functional group ending)

    33. Isomer = molecule with SAME formula but DIFFERENT structure

    34. Alcohols Have an OH group attached Name the carbon chain (prefix and bond) End in ol Indicate which carbon the OH is on 2-propanol 1-Butanol 3-Octenol

    35. What are the formulas for these alcohols?

    36. Alcohols

    37. Branched Hydrocarbons The longest continuous chain of carbon atoms gives the root name/prefix. Substituent is named by the number of carbons. Specify location of substituent by numbering carbon atoms in longest chain. Substituent often referred to as R or R (for second substituent)

    38. Substituent often referred to as R or R (for second substituent) If more than one alkyl group, use prefix di, tri, etc. to alkyl name Substituents listed in alphabetical order (disregarding prefix)

    39. Branched Hydrocarbon Substituent Alkyl groups

    40. What is the name of the compound?

    42. Halohydrocarbons Functional group is a halogen (X = F, Cl, Br, I) General Formula R X Naming Select longest chain containing halogen Number so that C with halogen gets lowest number

    43. Ethers Functional group - O General Formula R O R Naming Name the R group as an alkyl Name the R group as an alkyl End in ether

    44. Aldehydes Functional group - C H General Formula R C H Naming Name the R group Change the ending to -al

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