Chemical Nomenclature

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Chemical Nomenclature
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Learning Targets

• Write name write symbol of selected elements
• Write name write formula of a variety of
  compounds.

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Naming Inquiry

• Formula Name
• NaCl Sodium Chloride
• KI Potassium Iodide
• MgCl2 Magnesium Chloride
• What is a binary compound?

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Naming Inquiry

• Formula Name
• NaCl Sodium Chloride
• KI Potassium Iodide
• MgCl2 Magnesium Chloride
• What does the chemical formula of each indicate?

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Naming Inquiry

• Formula Name
• NaCl Sodium Chloride
• KI Potassium Iodide
• MgCl2 Magnesium chloride
• Why are there two chlorines for one magnesium?

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Naming Inquiry

• Formula Name
• NaCl Sodium Chloride
• KI Potassium Iodide
• MgCl2 Magnesium Chloride
• What are some naming rules that can be
  discovered from these examples?

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• Elements (periodic table)
• Symbols come from the first letter, or first two
  letters of the elements name.
• First letter is always UPPERCASE, second letter
  always lower case.
• Co, cobalt vs. CO, carbon monoxide
• No, nobelium vs. NO, nitrogen oxide
• Some use latin name for symbol, ex. Gold (latin
  name aurum or Au)

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NOTES

• Formula Represents composition of a compound
• Tells proportions of elements in a compound
  relative to each other.
• Subscripts are used to indicate number of atoms
  of each element in a compound. (ALWAYS Whole
  numbers!!)
• The subscript follows the atom or atoms it refers
  to. If subscript follows ( ) then everything
  inside the ( ) is multiplied by the subscript.

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• Examples
• CO2
• One atom of C, 2 atoms of O
• H2O
• 2 atoms of H, one atom of O
• Fe3(PO4)2
• 3 atoms of Fe, 2 atoms of P 8atoms of O

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Formulas, continued

• All atoms have oxidation numbers (valence
  charge). This is the combining power of the
  atom.
• ex Everything in Group 1 has a 1 charge.
  Group 17 has -1 charge
• Na 1 Cl -1 combined 0
• You want your valences to always 0

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Examples continued

• What happens when it doesnt 0?
• Mg2 Cl-1 0
• You add another Cl-1
• 
  -2
• so it now looks like this
• MgCl2
• Now the combined power is 0

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You Try

• Ca2 N-3
• K P-3
• Al3 O-2

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• Polyatomic ions or radicals are groups of atoms
  that behave as if they are single atoms. They
  also have oxidation numbers. Examples SO4-2
  (sulfate ion), NO3-1 (nitrate ion)

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• We will use the concept of valence to write
  formulas
• Valence is either or -
• In ALL compounds, the sum of the valences adds up
  to zero.
• Metals are always
• Non-metals can be or -
• Most radicals are -, only common radical is
  NH41 (ammonium)

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• Application
• Example 1 Lithium Chloride Li 1 and Cl 1-, so
  the formula must be LiCl.
• Example 2 Calcium Oxide Ca 2 and O 2-, so the
  formula must be CaO
• Example 3 What about Lithium Oxide?
• Answer you need two lithium atoms for every one
  oxygen to balanceLi2O

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• Atoms that have a constant valence
• (1) first column and Ag,
• (2) 2nd column plus Zn and Cd
• (3) Al. (See columns already marked on your
  periodic table.)
• (H can be -1 in some special cases)

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• Naming Binary Salts Writing their Formulas
• Metal plus a non-metal (two elements).
• Named by adding the name of the first element
  (metal) to the second element (non-metal) whose
  name is modified to end in ide.
• Examples
• oxygen becomes oxide
• chlorine becomes chloride
• sulfur becomes sulfide
• etc

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Now The Rules

• Rule 1 ends in ide Binary salt
• NaCl
• Sodium chloride
• Al2O3
• Aluminum oxide
• KI
• Potassium iodide
• Rule 2 valences must 0

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• Most metals have a variable valence and this must
  be indicated in the name of the compound.
• The Stock System The valence () of the metal
  is given as a Roman numeral.
• How does the Stock System Work?

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How does the Stock System Work?

• For metals in Groups 3-16
• Iron (II) chloride
• The (II) tells me the valence of Fe.
• I know that each Cl has a -1 charge. I have 2
  Cls for a total charge of -2, so the Fe has to
  be 2 to make the valences add up to zero
• FeCl3 what is the oxidation of Fe?
• Iron (III) chloride, Fe3

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You Try -

• Write the name or the formula using the Stock
  System
• CuCl
• Copper (I) chloride
• CrO3
• Chromium (VI) oxide
• Tin (IV) oxide
• SnO2if you have subscripts that can be reduced
  DO IT!!
• Nickel (II) oxide
• NiO

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• Salts with Radicals
• (polyatomic ions)
• Four ways to identify salts
• Metal non-metal (binary)
• Metal Radical
• Radical Non-metal
• Radical Radical

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• Salts with Radicals (polyatomic ions)
• Rule 3
• B. Naming Salts (other than binary)
• Name of metal name of radical
• Name of radical name of non-metal (still ends
  in ide) or radical

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• Salts with Radicals (polyatomic ions)
• The common-form of the radical MUST BE
  MEMORIZED
• common form ate ending
• a. Make Flash-Cards!!!!!
• 2. Other endings are based on ate ending

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You Try Write formula or name

• Calcium phosphate
• Ca2 PO4-3
• Potassium acetate
• K1 C2H3O2-1
• NaOH
• Al2(CO3)3

Ca3(PO4)2
KC2H3O2
Sodium hydroxide
Aluminum carbonate
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• Salts with Radicals (polyatomic ions)
• 3. More Rules
• Rule 4 if there is one less oxygen, then name
  ends in ite
• Rule 5 If there are 2 less oxygens the name
  starts with hypo ends in ite
• Rule 6 I more oxygen then common form starts
  with per and ends in ate

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• 4. Examples NaNO3, NaNO2, NaNO, and NaNO4
• Naming compounds w/Radicals
• One more Oxygen
• Common Form
• One less Oxygen
• 2 less Oxygen

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• 4. Examples NaNO3, NaNO2, NaNO, and NaNO4
• Naming compounds w/Radicals
• One more Oxygen NaNO4 Sodium pernitrate
• Common Form NaNO3 Sodium nitrate
• One less Oxygen NaNO2 Sodium nitrite
• 2 less Oxygen NaNO Sodium hyponitrite
• So what is the difference? http//www.edinformati
  cs.com/interactive_molecules/nitrite_and_nitrate_m
  olecules.htm

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You Try

• Na2SO5
• Sodium persulfate
• Ca3(PO2)2
• Calcium hypophosphite
• Magnesium hypofluorite
• Mg(FO)2
• Iron (II) nitrite
• Fe(NO2)2

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• V. Naming Acids (YepMore Rules!! ?)
• 1. Binary Acids all have H as first element and
  are aqueous ? dissolved in water.
• 2. Can be named as common salts if not dissolved
  in water.
• hydrogen non-metal.
• Rule 7 - Named by
• a. Change hydrogen ? hydro
• b. Change non-metal -ide ? -ic.
• c. Followed by the word acid.
• d. Example HCl (aq) is Hydrochloric acid

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You Try

• What would these be?
• HF (aq)
• Hydrofluoric Acid
• HBr (aq)
• Hydrobromic Acid
• (Most are from Group 17)
• H2S (aq)
• hydrosulfuric acid

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• 3. Ternary Acids hydrogen radical.
• Rule 8 Named for the radical. ate ending
  changes to ic is followed by acid
• Ex HNO3 (aq) Nitric Acid
• Rule 9 ite ending (Rule 4) changes to ous
• Ex HNO2(aq)
• Common form NO3-1 nitrate
• one less O, nitrous acid
• Also uses hypo ous per ic

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You Try Ternary Acids
Name Formula
of Oxygens
HClO4 (aq) HClO3 (aq)
HClO2 (aq) HClO (aq)
1
Perchloric acid
Common form
Chloric acid
-1
Chlorous acid
-2
Hypochlorous acid
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REVIEWso far

• Binary Salts
• Ternary Salts
• Ternary Salts
• Different of O
• Binary Acids
• Ternary Acids
• Ternary Acids
• Different of O

How do you recognizewhat are the clues?
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VI. Molecular Compounds

• Greek System of naming
• Only used for 2 non-metals
• Ends in ide
• Number of each kind of atom is indicated by a
  Greek numerical prefix (list on next slide)

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• Greek prefixes used for molecular compounds.
• Mono 1 Hexa 6
• Di 2 Hepta 7
• Tri 3 Octa 8
• Tetra 4 Nona 9
• Penta5 Deca 10

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Examples

• CO2
• Carbon dioxide
• You Try P2O5, N2O4, PCl3, Chlorine heptoxide
• Diphosphorous pentoxide
• Dinitrogen tetroxide
• Phosphorous trichloride
• ClO7

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• Can you fill in the blanks?
• Formula Name
• CO2 Carbon Dioxide
• N2O5 ______________
• N2O4 _______________
• _____ Phosphorous
  Trichloride
• P4O10 _______________

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• A few more rules for naming binary compounds of
  non-metals

• Rule 10 The prefix mono- is usually omitted
  except where it is used for emphasis, as in
  carbon monoxide.
• Rule 11 Common usage omits the double vowel
  as in the example above carbon monoxide is not
  carbon mono-oxide.
• FYI Some names for compounds dont fit the
  rules (ex H2O water NH3 ammonia)

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Naming Test

• 3rd Period Test 10/20
• 6th Period Test 10/21
• Assignments due on Test day
• Worksheets 1 9
• Graphs for Elements Naming