Nomenclature

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Nomenclature

• CH. 3

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The Types of Compounds

• Ionic
• salts, acids and bases (Electrolytes)
• Minerals
• Covalent
• inorganic from non living systems
• organic/biological- hydrocarbons, from living
  systems
• polymers - large hydrocarbons
• Metallic compound
• Pure elements, alloys and amalgams
• biometallic - proteins or large compounds with
  metal centers

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COVALENT Compounds

• Covalent compounds usually form when two non
  metal atoms which both have a desire to gain
  electrons create a bond by sharing the electrons
  between them.
• Neither atoms has full possession of the
  electron therefore neither atom is charged.
• Most organic compounds or hydrocarbons would fit
  into this category.
• With over 10 million compounds, organics comprise
  90 of all the known matter.

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IONIC Compounds

• Ionic Compounds involve the transfer of electrons
  from one atom making a cation to another atom
  making an anion.
• The bond forms when the cation with a positive
  charge is attracted to the anion with a negative
  charge.
• This electrostatic attraction is the ionic bond
  and usually occurs between a metal and a non
  metal atom.

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Balancing Charge

• Na O-2
• Nax O-2y x(1) y(-2) 0
• find the smallest common factor
• Na2O
• Ca2 N-3 x(2) y(-3) 0
• Ca3N2

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Fixed Charge Metals

• 1A always carries a 1 charge.
• Electron configuration - ns1
• 2A always carries a 2 charge
• Electron configuration - ns2
• 3A metals and 3B always carries 3
• electron configuration - ns2np1 or ns2nd1

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Naming inorganic compounds

• When an element forms only one compound with a
  given anion.
• name the cation
• name the anion using the ending (-ide)

NaCl sodium chloride MgBr2 magnesium
bromide Al2O3 aluminum oxide K3N potassium
nitride
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Naming ionic compounds

• Many metals form more than one compound with some
  anions.
• For these, roman numerals are used in the name
  to indicate the charge on the metal.
• Cu1 O2- Cu2O
• copper(I) oxide copper(I)
  oxide
• Cu2 O2-
  CuO
• copper(II) oxide copper(II)
  oxide

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Metals with multiple charges

• Transition metals.
• Here it is easier to list the ones that to only
  have a single common oxidation state.
• All Group 3B - 3
• Ni, Zn, Cd - 2
• Ag - 1
• Lanthanides and actinides - 3

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Summary

• Simple rules that will keep you out of trouble
  most of the time.
• Groups IA, 2A, 3A (except Tl) only have a single
  oxidation state that is the same as the group
  number - dont use numbers.
• Most other metals and semimetals have multiple
  oxidation states - use numbers.
• If you are sure that a transition group element
  only has a single state, dont use a number.

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Polyatomic Ions need to know

• Nitrate NO31-
• Carbonate CO3-2
• Sulfate SO4-2
• Phosphate PO4-3
• Chlorate ClO31-

• Hydroxide OH-
• Cyanide CN-
• Acetate C2H3O21-
• Ammonium NH4

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Polyatomic ions

• When a compound contains a polyatomic ion, you
  simply use the given name.
• NH4Cl ammonium chloride
• NaOH sodium hydroxide
• KMnO4 potassium permanganate
• (NH4)2SO4 ammonium sulfate

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Acids and Bases

• Acid
• HCl HNO3 H2SO4 H3PO4
• Base
• NaOH KOH Ba(OH)2 Al(OH)3
• The bases listed are metal hydroxides and
  therefore are named as an ionic compound

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Acids

• Binary acids
• the anion is a single element ending in -IDE
• the acid is named hydro - root - ic acid
• HCl - Hydrogen Chloride or
• hydro- chlor - ic acid

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Ternary Acids

• Anion ends in -IDE
• hydro - root - ic acid
• HCN, hydrogen cyanide is hydro cyan ic acid
• anion ends in -ATE
• root - ic acid
• HNO3, hydrogen nitrate is nitr ic acid
• anion ends in -ITE
• root -ous acid
• H3PO3, hydrogen phosphite is phosphorous acid

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Naming Covalent Molecules

• A simple set of rules can be used.
• name elements in the order they appear in the
  formula.
• use prefixes to indicate how many atoms there are
  of each type.
• mono 1 tetra 4 hepta 7
• di 2 penta 5 octa 8
• tri 3 hexa 6 deca 10
• use the ending (-ide) for the second element
  listed in the formula.

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Naming covalent compounds
N2O5 CO2 CO SiO2 ICl3 P2O5 CCl4
dinitrogen pentoxide carbon dioxide carbon
monoxide silicon dioxide iodine
trichloride diphophorous pentoxide carbon
tetrachloride

• The rule may be modified to improve how a name
  sounds.
• Example - use monoxide not monooxide.

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Naming Organic Compounds

• Contain Carbon and hydrogen atoms
• Use prefix to count number of carbons present in
  the compound
• functional groups

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Nomenclature overview

• Now that a large number of nomenclature rules
  have been introduced, we need to review them.
• Simple binary ionic compounds
• Ionic compounds of metals with multiple charges
• Compounds containing polyatomic ions
• Simple molecular compounds
• Its useful to be able to identify which system
  to use by looking at the chemical.

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A bit more on nomenclature

• When the first element is a metal then usually
• If only one other element is present and
• the second element is a non-metal -
• name the metal first - as element.
• Name non-metal second with -ide ending
• If more than one other element is present -
• name the metal first - as element.
• The rest is most likely a polyatomic ion
• so use the name from the table in book.

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A bit more on nomenclature
No
Is a metal present as the first element?
Use prefixes (mono, di, tri ...)
Yes
Can the metal have more than one oxidation state?
No
Roman numerals are not needed.
Yes
Use Roman numerals to indicate oxidation state
of metal
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Naming Activities

• Naming Flowchart