Chapter 6: Chemical Names and Formulas Section 1: Introduction to Chemical Bonding

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Chapter 6 Chemical Names and Formulas Section 1
Introduction to Chemical Bonding

• Molecules the smallest, neutral unit of a
  substance that still has the properties of the
  substance more than one of the same atom
• e.g. oxygen (O2) and ozone (O3)
• Br2I2N2Cl2H2O2F2 diatomic molecules as they are
  found in nature

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• Compounds more than one atom of different atoms
  that are NOT ionic i.e. both atoms are nonmetals
• Carbon dioxide (CO2 )
• Water (H2O)
• Compounds
• low melting and boiling points
• Usually are gases or liquids at room temperature

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• Naming compounds use the appropriate prefixes
• CO2 Carbon dioxide (dont use mono- for first
  listed element)
• CO Carbon monoxide
• N2O Dinitrogen monoxide (first element has more
  than one, therefore use a prefix
• Prefixes are on page 159

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• Ionic compounds
• Combination of a metal and a non-metal or a
  cation and an anion
• Results in a electrically neutral compound
• The charges cancel each other out
• NaCl Na 1 and Cl -1
• MgF2 Mg 2 and F -1
• Name according to worksheet Common ions and
  their Charges

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Section 6.2

• Molecular and ionic compound formulas always tell
  you what elements and how many elements are
  present in their lowest whole number ratios
• Na2O
• H2O

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Chapter 6 Section 3

• Ionic Charges

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Monatomic Ions

• Ions consisting of only one atom
• Table 6.2 (p143)

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Transition Metals

• Most can have multiple charges
• Exceptions Silver (Ag), Zinc (Zn2) and
  Cadmium (Cd2)
• Roman Numeral is used to show the charge on the
  cation
• Example Copper (I) Cu1

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Table 6.3 Page 144
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Polyatomic Ions

• Tightly bound groups of atoms that behave as a
  unit and carry a charge.
• Change the prefix and suffix to show a change in
  the number of oxygen present.
• Exceptions Cyanide, Hydroxide and ammonium
• Practice with the common ion sheet