Chapter 4 Nomenclature

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Chapter 4Nomenclature

• BEWARE!!!
• There is a lot memorization involved
• with this chapter.

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• In the old days compounds had common names like
  water, milk of magnesia, gypsum, quicklime, etc.
• Today we know of over 4 million compounds.
  Commonnames wont work
• Therefore we have a system!
• First we will learn aboutbinary compounds,
  compounds made of two elements
• There are two classes
• 1) metal/nonmetal
• 2) nonmetal/nonmetal

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4.1 Naming Compounds that Contain a metal and a
Nonmetal

• Metals tend to lose electrons e-,
• Nonmetals gain electrons e-
• Metals like to be positive
• Nonmetals like to be negative -
• These get together to form binary ionic compounds

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• When writing the
• formula the cation is
• first, anion second
• When naming justsay their names
• Some cations haveonly one chargeever (called
  Type I ion)
• Some have more thanone (Type II ion)
• There are also Type I compounds and Type II
  compounds

KNOW YOUR IONS!!!
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Type I Binary ionic compounds

• Reviewing the rules

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Type II binary ionic compounds

• Some cations can form more than one charge!!!
• (Type II ion!)
• Lets look at an example.
• iron can form 2 and 3 ions
• so what is the iron in iron chloride? Fe2 or
  Fe3?
• must be a way to distinguish the two!
• use Roman numerals

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• So what is the nameof FeCl2?
• Chloride always hasa 1- charge, and thereare
  two, so
• The positive guy musthave a total2 charge,
  and
• There is only one cation so it get the whole 2
  charge all to itself, so
• It must be iron(II), so
• It is iron(II) chloride
• Know Table 4.2 (the systematic is emphasized in
  this class!!)

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examples

• CuCl
• copper(I) chloride
• HgO
• mercury(II) oxide
• Fe2O3
• iron(III) oxide
• Mn2O4
• manganese(IV) oxide
• PbCl4
• lead(IV) chloride

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• summary of Type I and Type II

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summaryexamples

• CoBr2
• cobalt(II) bromide
• CaCl2
• calcium chloride
• Al2O3
• aluminum oxide
• CrCl3
• chromium(III) chloride

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4.2 Naming Binary Compounds that Contain only
Nonmetals (Type III)

• Type III contain only NM!
• think prefixes!
• (note water and ammonia are Type III but always
  keep their common names)

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examples

• BF3
• boron trifluoride
• NO
• nitrogen monoxide
• N2O5
• dinitrogen pentoxide
• PCl5
• phosphorus pentachloride
• SF6
• sulfur hexafluoride
• SO2
• sulfur dioxide

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4.3 naming binary compoundsa review
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4.4 Naming Compounds that contain Polyatomic Ions

• There is another(!) type of compound, one that
  involves
• Polyatomic ions. Ions with more than one type of
  atom in it
• gotta know Table 4.4

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• Notice many have O in them
• Called oxyanions
• Most common is called root-ate (e.g. sulfate)
• One less O than most common?
• root-ite (nitrite)
• One less than that?
• hypo-root-ite (hypochlorite)
• One more than most common?
• per-root-ate (perchlorate)
• Must be able to recognize Polyatomic ions!!!

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examples

• Na2SO4
• sodium sulfate
• Fe(NO3)3
• parentheses here mean there are 3 of whats
  inside.NO33 is nonsense!
• iron(III) nitrate
• Mn(OH)2
• manganese(II) hydroxide

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summary examples

• Na2CO3
• sodium carbonate
• FeBr3
• iron(III) bromide
• PCl3
• phosphorus trichloride
• CsClO4
• cesium perchlorate
• CuSO4
• copper(II) sulfate

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4.5 Naming Acids

• Some things when dissolved in water can lose an
  H right off them
• called acids
• taste sour
• know these!
• have their ownname system

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4.6 Writing Formulas from Names

• so far weve done formulas to names
• now we do reverse! yippee!
• you HAVE TO KNOW all the names I warned you
  about!!!

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examples

• potassium hydroxide
• KOH
• sodium carbonate
• Na2CO3
• nitric acid
• HNO3
• calcium chloride
• CaCl2
• dinitrogen pentoxide
• N2O5
• ammonium perchlorate
• NH4ClO4

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if this helps, use it. if it doesnt, dont!