1.3 Bonding

• Between what types of elements does ionic bonding occur?

  Between a metal and a non-metal
• In ionic bonding, what happens to electrons between atoms?

  Electrons are transferred
• What do metal and non-metal atoms achieve by transferring electrons in ionic bonding?

  Full outer shells
• What are charged particles called that are formed when electrons are transferred?

  Ions
• What force holds oppositely charged ions together in ionic bonding?

  Electrostatic forces
• What structure do oppositely charged ions form through electrostatic forces?

  Giant ionic lattice
• What ions form sodium chloride?

  Na+ and Cl- ions
• In the formation of sodium chloride, what does sodium do with an electron?

  Sodium loses an electron
• In the formation of sodium chloride, what does chlorine do with an electron?

  Chlorine gains an electron
• What is the formula for a sulfate ion?

  SO42-
• What is the formula for a hydroxide ion?

  OH-
• What is the formula for a nitrate ion?

  NO3-
• What is the formula for a carbonate ion?

  CO32-
• What is the formula for an ammonium ion?

  NH4+
• Between what types of elements do covalent bonds form?

  Two non-metals
• In covalent bonding, what happens to electrons between atoms?

  Electrons are shared
• What do non-metal atoms achieve by sharing electrons in covalent bonding?

  Full outer shell
• What can be shared to produce multiple covalent bonds?

  Multiple electron pairs
• What type of diagrams can be used to represent shared electron pairs in covalent bonding?

  Dot and cross diagrams
• How is a covalent bond shown in diagrams?

  With a straight line
• When do dative or coordinate bonds form?

  Electrons in shared pair are from single atom
• What symbol indicates a dative bond?

  An arrow
• Which molecule has a lone pair of electrons that can form a dative bond with a H+ ion?

  Ammonia (NH3)

  
• What ion is produced when ammonia forms a dative bond with a H+ ion?

  Ammonium ion (NH4+)

  
• How is a dative bond treated once it has formed?

  As a standard covalent bond
• Why is a dative bond treated as a standard covalent bond once formed?

  It reacts in exactly the same way
• What does metallic bonding consist of?

  Lattice of positive ions in delocalised electrons

  
• What is present between oppositely charged particles in metallic bonding?

  Electrostatic force of attraction
• What effect does a greater charge on the positive ion have on the attractive force in metallic bonding?

  Increases the attractive force
• How does the size of an ion affect the attraction in metallic bonding?

  Larger ions have weaker attraction
• Why do larger ions produce weaker attraction in metallic bonding?

  Due to their greater atomic radius
• Which physical properties are influenced by bonding and crystal structure?

  Boiling point, melting point, solubility, conductivity
• What are the four main types of crystal structure?

  Ionic, metallic, simple molecular, macromolecular
• Why do ionic crystal structures have high melting and boiling points?

  Strong electrostatic forces require a lot of energy
• Under what conditions can ionic substances conduct electricity?

  Molten or in solution
• Why can molten or dissolved ionic compounds conduct electricity?

  Ions are free to move and carry charge
• What happens when the layers of alternating charges in an ionic crystal are distorted?

  Like charges repel, lattice breaks

  
• Why are metallic structures good conductors of electricity?

  Delocalised electrons can move and carry charge
• Why are metals malleable?

  Layers of ions slide, delocalised electrons prevent fragmentation
• Why do metallic substances have high melting points?

  Strong electrostatic forces require a lot of energy