Memorization Assignment

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Lecture 6

• Section 2.8

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Memorization Assignment

• Greek prefixes for
• 1, 2, 3, 4, 5, 6, 7, 8, 9, 10
• Do not use italics when writing these prefixes.
• Formulas of
• Water, ammonia, hydrogen peroxide
• http//www.dhmo.org

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Discussion Questions

• What is a binary compound?
• What is the difference between Type I and Type II
  cations?
• How is the charge of a Type II cation indicated
  in the name of an ionic compound?
• How are the numbers of atoms in a molecule of a
  binary covalent compound indicated?

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Binary Ionic Compounds with Type I Cations

• Type I cations have only one charge
• Table 2.3
• Remove H
• Add Zn2 and Cd2
• You will memorize these charges for lectures 7,
  8, and 9
• Correlate the charges with periodic table position

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Examples

• Names from formulas
• NaCl
• MgBr2
• AlI3
• Ca3P2
• Formulas from names
• Cesium sulfide
• Aluminum oxide
• Potassium fluoride
• Zinc hydride

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Binary Ionic Compounds with Type II Cations

• Type II cations have more than one possible
  charge
• Table 2.4
• Remove Ag, Zn2, and Cd2
• These are just examples
• You dont need to memorize them
• Just learn how the system works
• We will not use the old system (ferrous, ferric
  cuprous, cupric plumbous, plumbic etc.)

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Examples

• Names from formulas
• CuO
• Cu2O
• Cr2S3
• UO3
• Formulas from names
• Tin(IV) bromide
• Manganese(III) oxide
• Iron(II) nitride
• Gold(I) fluoride

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Ionic Compounds with Polyatomic Ions

• Names from formulas
• (NH4)3PO4
• Al(OH)3
• Use parentheses only when you have more than one
  of a polyatomic ion
• CuSO4, not Cu(SO4)
• Formulas from names
• Mercury(I) nitrate
• Sodium peroxide
• Aluminum bicarbonate
• Iron(III) dichromate

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Binary Molecular Compounds (Type III)

• Nonmetal bonded to nonmetal
• Covalent bonds
• Ionic charges do not apply
• But compounds still end in -ide
• Greek prefixes used to specify how many atoms of
  each element are present
• Mono- not used with first element (and often
  omitted on second element except for
  clarification)

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Examples

• Names from formulas
• SO3
• Dont confuse with SO32-
• Which is present in CaSO3?
• P4O10
• Formulas from names
• Dinitrogen monoxide
• Iodine heptafluoride

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Acids

• ACIDS ARE MOLECULAR COMPOUNDS!
• They form ions in aqueous solution by reacting
  with water
• HCl H2O ? H3O Cl- chlorIDE
• HNO2 H2O ? H3O NO2- nitrITE
• HNO3 H2O ? H3O NO3- nitrATE
• The acid that makes chlorIDE is HYDROchlorIC acid
• The acid that makes nitrITE is nitrOUS acid
• The acid that makes nitrATE is nitrIC acid

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Examples

• Names from formulas
• HF(aq), HCl(aq), HBr(aq), HI(aq)
• HNO2, HClO2(aq)
• HNO3, H2CO3, HClO3
• Formulas from names
• Hydrocyanic acid
• Hypochlorous acid
• Perchloric acid, acetic acid, oxalic acid

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SulfUR and PhosphORus

• SulfURic acid, not sulfic acid
• Same with sulfURous acid, hydrosulfURic acid
• PhosphORic acid, not phosphic acid

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Figure 2.25

• Change caption to read
• An acid is best named as if it consisted of one
  or more H ions attached to an anion.
• But always remember that it does NOT consist of
  any such thing. An acid is a MOLECULAR compound
  that forms ions by reaction with water.