Unit 3 Nomenclature

1
Unit 3 Nomenclature
2
Types of Compounds

• Ionic Compounds - electrons are transferred from
  the metal to the nonmetal.
• Covalent Compound - electrons are shared between
  2 nonmetals.

3
Practice!

• Identify the following as ionic or covalent
• NaCl
• H2O
• CCl4
• LiF
• NO2
• MgO

Sodium chloride
4
Answers

• Ionic
• Covalent
• Covalent
• Ionic
• Covalent
• ionic

5
Is it possible for a compound to have both ionic
and covalent bonds?

• YES!
• Mg(NO3)2

covalent
ionic
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Anion- negative ion Cation- positive ion Octet
Rule- rule that states that atoms tend to gain,
lose, or share electrons so that each atom has
full outermost energy level which is typically 8
electrons. Polyatomic Ion- charged group of
covalently bound atoms Monatomic Ion- ion formed
from a single atom Molecule- neutral group of
atoms united by covalent bonds Alloy- homogeneous
mixture of metals Unshared Pair- pair of
electrons that is not involved in bonding but
instead is held exclusively by one atom.
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Names vs. Formulas

• Chemical Name - indicates what atoms are present
  in the compound
• Chemical Formula - short hand way of writing the
  name of the compound that indicates how many
  atoms of each element are present in the
  compound.
• MgCl2

2 Chlorine atoms
1 Magnesium atom
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Types of Ionic Compounds

• Binary Ionic Compounds
• Metal nonmetal
• Ternary Ionic Compounds
• Metal polyatomic ion
• Binary Ionic Compounds with Transition Metals
• Transition metal nonmetal
• Ternary Ionic Compounds with Transition Metals
• Transition Metal polyatomic ion
• Ternary Ionic Compounds with 2 Polyatomic Ions

9
Naming Binary Ionic Compounds

• Name the metal ion.
• Name the nonmetal ion.
• Ex NaCl
• Metal ion sodium
• Nonmetal ion chloride
• You try
• LiCl
• MgO

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Writing formulas for Binary Ionic Compounds

• Determine the oxidation number (charge) for each
  ion

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• 1 2 -3 -2 -1 0

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Determining Oxidation Numbers

• Alkali Metals (group 1) --gt 1
• Alkaline Earth Metals (group 2) --gt 2
• Transition Metals --gt can have multiple oxidation
  numbers so we cant predict
• B group - exceptions
• C group - exceptions
• N group --gt -3
• O group --gt -2
• Halogens --gt -1
• Noble Gases --gt 0

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Writing formulas for Binary Ionic Compounds

• Determine oxidation number.
• Ex magnesium chloride
• Mg --gt 2
• Cl --gt -1
• Cross over - oxidation number of metal becomes
  the subscript of the nonmetal. Oxidation number
  of the nonmetal becomes the subscript of the
  metal.

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Writing formulas for Binary Ionic Compounds

• Mg2 Cl-1
• Only the number crosses, not the or -
• Dont write a 1
• MgCl2

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Practice!

• Name the following
• CaCl2
• KF
• Li2O
• Write formulas for the following
• Magnesium bromide
• Calcium sulfide
• Potassium chloride

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Answers

• Calcium chloride
• Potassium fluoride
• Lithium oxide
• MgBr2
• CaS
• KCl

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Naming Ternary Ionic Compounds

• Name the metal
• Name the polyatomic ion
• Ex Na2SO4
• Metal --gt sodium
• Polyatomic ion --gt sulfate
• Name --gt sodium sulfate
• You try
• LiNO3
• Mg3(PO4)2

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Writing formulas for Ternary Ionic Compounds

• Determine the oxidation number of the metal.
• Write the formula for the polyatomic ion.
• Cross over.
• Ex lithium phosphite
• Li1 (PO3)-3
• Li3PO3

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Practice!

• Write the formula for the following
• Sodium nitrate
• Magnesium sulfate
• Potassium perchlorate
• Name the following
• KNO2
• CaSO4
• LiNO3

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Answers

• NaNO3
• MgSO4
• KClO4
• Potassium nitrite
• Calcium sulfate
• Lithium nitrate

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Determining Oxidation States from Compounds

• Oxidation state charge
• Compounds are neutral, so the charges have to
  equal the charges
• Ex CuS
• S (group 16) ? -2
• No subscripts, so we know the charges cancelled
  each other out
• So, Cu ? 2

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Naming Binary Ionic Compounds with Transition
Metals

• Identify the transition metal in the formula.
• Determine the oxidation number of the transition
  metal.
• Name the transition metal.
• Use a roman numeral to note the oxidation number
  of the transition metal.
• Name the nonmetal ion.

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Naming Binary Ionic Compounds with Transition
Metals

• Ex FeCl2
• What is the transition metal? Fe
• What is the ox. Number of the t.metal? 2
• What is the nonmetal ion? Cl
• Name
• Iron (II) chloride
• You try
• CuCl
• Cr2O3

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Writing formulas for Binary Ionic Compounds with
Transition Metals

• The roman numeral in the compound name gives the
  oxidation number of the metal ion.
• Determine the metal ion.
• Determine the nonmetal ion.
• Cross over.
• Ex Iron (III) fluoride
• Metal --gt Fe
• Metal ox. Number --gt 3
• Nonmetal --gt F-1
• Formula --gt FeF3

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Practice!

• Name the following
• CrCl3
• CuF2
• CuF
• Write the formula for the following
• Iron (II) sulfide
• Iron (III) sulfide
• Copper (II) oxide

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Answers

• Chromium (III) chloride
• Copper (II) fluoride
• Copper (I) fluoride
• FeS
• Fe2S3
• CuO

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Naming Ternary Ionic Compounds with Transition
Metals

• Determine oxidation number of transition metal.
• Determine name of polyatomic ion.
• Name transition metal ion.
• Roman Numeral indicates the charge on the
  transition metal
• Name the polyatomic ion.
• Ex Cu(NO3)2 is named Copper (II) nitrate

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Writing formulas for Ternary Ionic Compounds with
Transition Metals

• Determine oxidation number of transition metal.
• Write formula for polyatomic ion.
• Cross over.
• Ex chromium (II) phosphate
• Cr2 (PO4)-3
• Cr3(PO4)2

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Practice!

• Name the following
• CuSO4
• FePO4
• Cr(NO3)3
• Write the formula for the following
• Iron (II) nitrate
• Copper (I) nitrate
• Copper (II) perchlorate

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Answers

• Copper (II) sulfate
• Iron (III) phosphate
• Chromium (III) nitrate
• Fe(NO3)2
• CuNO3
• Cu(ClO4)2

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Another way

• Memorize the Latin names for the transition metal
  ions.
• Ex Fe3 Ferric
• Ex Fe2 Ferrous
• Ex FeCl3 is named 2 ways
• Iron (III) chloride
• Ferric chloride

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Ternary Ionic Compounds with 2 Polyatomic Ions

• The polyatomic cation has to be NH41!
• Name ammonium.
• Name polyatomic anion.

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Naming Acids

• Acids always have hydrogen at the front of the
  formula
• Ex HCl, HBr, HClO4, H2SO4
• To Name Binary Acids (H element)
• Hydro _____ ic Acid
• To Name Ternary Acids (H polyatomic ion)
• Name the polyatomic ion
• If the polyatomic ion ends in -ate, the acid will
  end in -ic acid
• If the polyatomic ion ends in -ite, the acid will
  end in -ous acid
• If the polyatomic ion ends in -ide, the acid will
  be named hydro _____ ic acid

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Examples

• HCl - hydrochloric acid
• HBr - hydrobromic acid
• HF - hydrofluoric acid
• HNO3 - nitric acid (nitrate --gt nitric)
• HNO2 - nitrous acid (nitrite --gtnitrous)
• HCN hydrocyanic
• acid

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Writing Formulas for Acids

• Hydrogen always has 1 ox. Number
• Cross over charge of polyatomic ion.
• Ex H1 (SO4)-2
• H2SO4

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Naming Bases

• Bases always have hydroxide (OH-1) as the anion
• KOH - potassium hydroxide
• Ca(OH)2 - calcium hydroxide
• Fe(OH)2 - iron (II) hydroxide

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Writing formulas for Bases

• Determine the oxidation number for the cation.
• Cross over the oxidation number of the cation to
  the hydroxide.
• Mg2 (OH)-1
• Mg(OH)2

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Types of Covalent Compounds

• Polar covalent - electrons are shared unequally
  (one element has a stronger pull on the electrons
  than the other)
• Nonpolar covalent - electrons are shared equally
• Both are named the same way!

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Naming Covalent Compounds

• Count the number of atoms present of each
  nonmetal.
• Assign a greek prefix for that number of atoms.

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Greek 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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Naming Covalent Compounds

• Ex N2O5
• Name --gt Dinitrogen Pentaoxide
• Note When the first atom only has one atom
  present, you do not use the mono prefix.
• Ex CO2
• Name --gt Carbon Dioxide (not monocarbon dioxide)

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Writing formulas for Covalent Compounds

• The greek prefix indicates how many atoms of each
  element are present.
• Ex sulfur hexafluoride
• SF6

43
Practice!

• Name the following
• CO
• SF4
• NO2
• Write the formulas for the following
• Sulfur trioxide
• Nitrogen trifluoride
• Carbon tetrachloride

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Answers

• Carbon monoxide
• Sulfur tetrafluoride
• Nitrogen dioxide
• SO3
• NF3
• CCl4

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Naming Hydrates

• Hydrate - a molecule (covalently bonded atoms)
  that is surrounded by water molecules
• CuSO4 . 5H2O
• Name Copper (II) sulfate pentahydrate