Naming Inorganic Compounds

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UNIT IV

• Naming Inorganic Compounds
• Lesson 1

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INORGANIC NOMENCLATURE

• Nomenclature refers to naming
• Inorganic Non Carbon compounds Elements.
• Organic chemistry study of carbon compounds.
• The periodic table organizes the elements by
  vertical columns (___________) and horizontal
  rows (______________).
• The elements are arranged depending on the
  chemical and physical properties of elements in
  repeated patterns and increasing atomic masses.

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IV.1 THE CHEMICAL ELEMENTS

• Element symbol The first letter is always in
  upper case and the second letter (if present) is
  always lower case.
• Ex Sodium (Na), Nitrogen (N)
• 3 Major classifications pg. 67

Non-Metals Metals Metalloids or Semi Metals
Grey shaded area White boxes Clustered elements around the staircase between metals and non-metals.
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Periodic table

• http//www.colgurchemistry.com/2008PeriodicTable.p
  df

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IV.2 NAMING INORGANIC COMPOUNDS

• METALS
• Found on left side in periodic table
• Form _________ ions
• Cation an ion with a positive charge
• NON-METALS
• Found on right side in periodic table
• form __________ ions
• (H is generally an exception)
• Anion an ion with a negative charge

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Naming inorganic compounds

• Some other definitions
• Monoatomic
• Diatomic
• Triatomic
• Polyatomic

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• NAMING MONATOMIC METAL IONS
• Simply use the name of the metal and add the word
  ion
• Element Name Ion Name
• Sodium Metal(Na)
• Aluminum (Al)
• Write the names of the following ions
• a) Cu
• b) Cr3
• c) Ag

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NAMING MONATOMIC METAL IONS

• If a metal has more than one possible charge, the
  charge has to be indicated by a Roman numeral, in
  parenthesis, immediately following the name.
• Ex Fe3
• Fe2
• Roman numerals are
• I 1 V 5
  IX 9
• II 2 VI 6 X
  10
• III 3 VII 7
• IV 4 VIII 8

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NAMING MONATOMIC METAL IONS

• Write the formula of the following ions to show
  their charges
• Uranium (VI) ion __________
• Iron (II) ion __________
• Nickel (II) ion __________

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• NAMING MONATOMIC NON-METAL IONS
• Take off the original ending and add an ide
  ending.
• Element Name Ion Name
• Florine (F) ?
•   Sulphur (S) ?
• Write the names of the following ions
• a) Br- __________________________
• b) Cl- __________________________
• c) I- __________________________
• d) O-2 __________________________
• e) N-3 __________________________

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• Naming Polyatomic Ions
• Rules for naming are more complicated (we wont
  learn them). But we will need to KNOW some common
  polyatomic ions (names, formula, charge).
• Know table on page 69.

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• How to write the formula and how to write the
  name of
• Ionic Compounds

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How to write the formula of ionic compounds

• An ionic compound
• A compound made up of ions ( usually a metal
  non-metal )
• The ions have charges but the compound is a
  neutral molecule.
• remember in ionic compounds , one ion loses and
  one ion gains electrons).
• The chemical name of an ionic compound always
  gives the positive ion (cation) first and the
  negative ion (anion) second.
• Ex Sodium Chloride

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Writing formula of Ionic compounds
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3 simple rules
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More examples

• Potassium oxide
• Iron (II) sulphate
• Tin (IV) oxide
• Calcium phosphide
• We do not change the endings of polyatomic ions
  because they already have special endings that
  end in ate or ite

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• How to Write the Name of an IONIC COMPOUND
• Check your periodic table to see if the
  positive ion has more than one ion charge.

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How to Write the Name of an IONIC COMPOUND

• A) If the first ion has only one possible ion
  charge
• write the names of the ions(not elements) one
  after the other
• omit the word ion
• ZnCl2
• Ag2SO4
• Silver sulphate

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• B) If the first ion has more than one possible
  charge
• De-swap and de-drop the subscripts (to find out
  the real charge)
• check the charge on negative ion (if it is not as
  what it should be, you probably need to double or
  triple it)
• write the charge of the positive ion with roman
  numerals
• Write the charge of the negative ion with ide

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Try these on your own

• FeS
• Fe2(HPO4)3

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• Note you must memorize the common name
  of 2 compounds
• H2O water
• NH3 ammonia
• be careful of Ammonium NH41

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Naming Hydrates

• Hydrates are ionic compounds that include water
  molecules in their crystal structures.
• Naming hydrates is pretty straightforward and
  relies on using prefixes to tell how many water
  molecules are attached.
• The of water molecules is shown after a
  centered dot
• Example of a hydrate CuSO45H2O
• see table on page 72 for prefixes

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Naming Hydrates

• see table of page 72 for prefixes
• CuSO4.5H2O
• copper (II) sulphate pentahydrate
• Ca(NO3)24H2O

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Practice Time!

• Self-test on page66 ?All of it
• Ex1 on page 68
• Ex4 on page 71
• Ex 5 on page 72
• Page 73 Ex6 a, c, d, f, g, I
• Page 73 Ex7 a, b, c, d, e, f

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UNIT IV LESSON 2

• How to write the formula and how to write the
  name of
• Covalent Compounds

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• Naming COVALENT COMPOUNDS Using the Prefix-Naming
  System
• Remember covalent compounds SHARE their electrons
  ( usually two non-metals together).
• Binary Compound a compound made of two different
  types of atoms (usually two non-metals)
• SO2, Na2S, NaCl
• Tertiary Compound a compound made of three
  different types of atoms.
• H2SO4 KOH KMnO4

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Naming COVALENT COMPOUNDS Using the Prefix-Naming
System

• We use the prefix-naming system
• 1- Each compound name is made of words, each with
  a suitable prefix
• see p. 73

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Naming COVALENT COMPOUNDS Using the Prefix-Naming
System

• Prefix-system naming continued
• First word is the name of element(not ion) with a
  prefix to indicate the of atoms
• Second word is the name of the element with an
  ide ending and a prefix to indicate the of
  atoms
• P2S3 diphosphorus trisulphide
• Exception if there is only ONE atom of the first
  element, dont use the prefix mono.
• Ex CO2

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Try on your own

• Examples
• P2S3
• CO
• BrCl3
• S2Cl2

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prefix naming system

• Basically used when you have two different
  Non-Metals.
• Non-metals are usually found on the right side of
  the periodic table.
• Remember the prefixes.

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Writing formulas for covalent compounds

• Steps
• Write down the symbol for each element
• Use the prefix to determine the number of atoms
  of each element.
• Example dinitrogen tetroxide carbon
  dioxide
• Do NOT reduce !

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• Some Common Acids
• A compound is called an acid when the chemical
  formula starts with H
• ex HCl, H2SO4
• see common acids on p. 74
  KNOW THESE

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Summary

• Naming
• First identify if it is ionic or covalent
• Ionic compounds
• Metal and non-metal
• Positive ion first then negative ion
• Use roman numerals to indicate the ions with more
  than one possible charge
• For the negative ions(non-metals) change the
  ending to ide.
• Covalent compounds
• Non-metal and non-metal
• For both, we use the prefix-naming system (mono,
  di, tri, tetra, etc)
• First one, you just write the elements original
  name with prefix
• You change the second elements name to ide
  with prefix.

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Summary

• Writing Formulas
• First identify if it is ionic or covalent
• Ionic compounds
• Write formula for positive ion first then
  negative ion
• Swap and drop charges as subscripts
• Reduce if you need to.
• Covalent compounds
• Write down the symbol for each element
• Use the prefix to determine the number of atoms
  of each element.
• Do NOT reduce !

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Practice time!

• Page 74 Ex8 and Ex9.
• Page 75 writing the names question
• ( only odd numbers )
• 15 ? 89 ( only odds)
• Page 76 writing the formulas question
• ( only even numbers)
• 90 ? 162 (only evens)

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