Bonding

• What type of elements participate in ionic bonding?

  Metal and non-metal
• What happens to electrons during ionic bonding?

  Electrons are transferred from metal to non-metal
• What are charged particles created during ionic bonding called?

  ions
• What type of structure is formed by oppositely charged ions?

  A giant ionic lattice
• What ions are formed in sodium chloride?

  Na​+​ and Cl​-​ ions
• How does sodium chloride achieve full outer electron shells?

  Sodium loses an electron, chlorine gains one
• What are common compound ions?

  • Sulfate - SO​4​2-
  • Hydroxide - OH​-
  • Nitrate - NO​3​-
  • Carbonate - CO​3​2-
  • Ammonium - NH​4​+
• What type of elements form covalent bonds?

  Two non-metals
• How are electrons handled in covalent bonding?

  Electrons are shared between outer shells
• What can multiple electron pairs produce in covalent bonding?

  Multiple covalent bonds
• How can shared electron pairs be represented?

  Using dot and cross diagrams
• What is a dative bond?

  Electrons in the shared pair come from one atom
• What is an example of dative bonding?

  Ammonia forming ammonium ion
• How is a dative bond treated after formation?

  As a standard covalent bond
• What is metallic bonding characterized by?

  A lattice of positively charged ions
• What surrounds the positively charged ions in metallic bonding?

  A ‘sea’ of delocalised electrons

  
• What happens to the attractive force in metallic bonding as the charge increases?

  The attractive force becomes stronger
• How does the size of ions affect metallic bonding?

  Larger ions produce weaker attraction
• What are physical properties of substances influenced by?

  Type of bonding and crystal structure
• What are the four main types of crystal structure?

  • Ionic
  • Metallic
  • Simple molecular
  • Macromolecular
• What is a characteristic of ionic substances regarding melting and boiling points?

  They have high melting and boiling points
• Why do ionic substances conduct electricity when molten or in solution?

  Ions are free to move and carry charge
• What happens to ionic substances when layers are distorted?

  They break apart into fragments
• What is a characteristic of metallic substances regarding conductivity?

  They are good conductors
• Why are metals malleable?

  Layers of positive ions can slide over each other

  
• What is the state of most metallic substances at room temperature?

  They are nearly always solid
• What type of structure do simple molecular substances have?

  Covalently bonded molecules
• What holds simple molecular substances together?

  Weak van der Waals forces
• Why do simple molecular substances have low melting and boiling points?

  Weak forces require little energy to overcome
• What is an example of a simple molecular substance with high boiling point?

  Water due to hydrogen bonding
• What is a characteristic of macromolecular substances?

  They have a giant lattice structure
• What gives macromolecular substances a very high melting point?

  Multiple strong covalent bonds
• What makes diamond one of the hardest materials?

  Its strong covalent lattice structure
• How does graphite differ from diamond in structure?

  Graphite has flat sheets of carbon atoms
• What allows graphite to conduct electricity?

  Free electrons move between layers
• What determines the shape of a molecule?

  Number of electron pairs around central atom
• How do electron pairs affect bond angles?

  They repel each other to maximize angles
• What effect do lone pairs have on bond angles?

  They reduce bond angles by 2.5°
• How do you determine the shape of a molecule?

  1. Find the number of electron pairs.
  2. Identify bonding and lone pairs.
  3. Analyze the basic shape and repulsion effects.
• What are common molecule shapes and their bond angles?

  • Linear: 180° (2 bonding pairs)
  • V-Shaped: 104.5° (2 bonding, 2 lone pairs)
  • Trigonal Planar: 120° (3 bonding pairs)
  • Triangular Pyramid: 107° (3 bonding, 1 lone pair)
  • Tetrahedral: 109.5° (4 bonding pairs)
  • Trigonal Bipyramid: 90° and 120° (5 bonding pairs)
  • Octahedral: 90° (6 bonding pairs)