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 formed during ionic bonding called?

  ions
• How do oppositely charged ions interact in ionic bonding?

  They attract through electrostatic forces
• What ions are formed from sodium and chlorine in sodium chloride?

  Na​+​ and Cl​-​ ions
• What is the purpose of transferring electrons in ionic bonding?

  To achieve full outer shells
• 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 involved in covalent bonding?

  Electrons are shared between two 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?

  When both electrons in a shared pair come from one atom
• How is a dative bond indicated?

  With an arrow from the lone electron pair

  
• What happens to a dative bond after it forms?

  It is treated 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 does the strength of metallic bonding depend on?

  The charge on the positive ion
• How does the size of an ion affect metallic bonding strength?

  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?

  Because ions are free to move
• What happens to ionic substances when layers are distorted?

  They break apart into fragments
• What is a property 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 only liquid metal at room temperature?

  Mercury
• What type of structure do simple molecular substances have?

  Covalently bonded molecules held by weak forces
• What type of forces hold 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 unique about water's boiling point compared to other simple molecular substances?

  It has an unusually high boiling point
• Why are simple molecular substances poor conductors?

  They contain no charged particles
• What characterizes macromolecular structures?

  Covalently bonded into a giant lattice
• 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 moving between layers
• What determines the shape of a molecule?

  Number of electron pairs around the 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 to determine the shape of a molecule?

  1. Find the number of electron pairs.
  2. Determine bonding and lone pairs.
  3. Analyze basic shape and repulsion effects.