topic c2- bonding, structure- properties of matter

• ionic bonding

  
• ionic bonding

  • transferring electrons between elements, forming ions
  • when a metal and non-metal react
• ionic bonding

  • Mg loses 2 electrons
  • become Mg2+
  • loses 2 negative charges
  • Cl gains 1 electron each
  • become Cl-
  • gains 1 negative charge
• covalent bonding

  
• covalent bonding

  • sharing electrons between elements, forming covalent bonds
  • when two non-metals react
• covalent bonding

  • Nitrogen (N) has 5 electrons on its outer shell (group 5 on periodic table), needing 3 more
  • hydrogen (H) has 1 needing 1 more
  • by sharing, each atom completes their outer shell
  • covalent bonds have been formed
• metallic bonding

  
• metallic bonding

  • 'delocalised' (free ton move) electrons in the outer shell are attracted to the positive charge on a metal ion
  • those attractions hold the atom in a strong, regular structure
• substances held together by metallic bonding include

  • alloys
  • elements
• properties of ionic bonding

  • metal + non-metal
  • high melting and boiling points
  • electrical conductors when melted
  • electrons are transferred
• properties of covalent bonding

  • low melting and boiling points due to weak forces
  • don't conduct electricity
  • electrons are shared
• properties of metallic bonding

  • metal + metal
  • high melting and boiling points
  • good heat conductors
  • good electrical conductors due to delocalised electrons
• polymers- monomers

  
• polymers

  long chain of repeating units, called monomers
• states of mass- solid

  
• states of mass- liquid

  
• states of mass- gas

  
• properties of solids

  • fixed positions
  • vibrate to transfer energy
  • strong forces
• properties of liquids

  • fit base of container
  • constant movement, faster with heat
  • weaker forces
• properties of gases

  • fill container
  • random motion
  • very weak forces
• properties of ionic structures- giant ionic lattice

  • strong electrostatic forces
  • high melting and boiling points
  • electrical conductors when melted
• properties of covalent structures- simple molecular

  • low melting and boiling points due to weak forces
  • gases/ liquids at room temperature
  • don't conduct electricity
• properties of covalent structures- giant covalent structures

  • very high melting and boiling points
  • don't conduct electricity
  • main examples include diamond and graphite
• properties of metals- metals

  • mostly solid at room temperature
  • good heat conductors
  • good electrical conductors
  • malleable
  • can be bonded to make alloys, enhances properties
• polymers

  • longer chains of polymers have more bonds overall
  • so the overall melting and boiling points are often higher
  • as it requires more energy to break all of them
• solid to liquid

  • melting
• liquid to a gas

  evaporation
• gas to a liquid

  condensation
• liquid to a solid

  freezing
• solids

  • vibrate
  • no movement
  • regular lattice
  • cannot be compressed
  • fixed positions
• liquids

  • move slightly
  • can't be compressed
• gases

  • move around freely
  • high energy
  • can be compressed
• changing states of matter- examples

  • solidification/ freezing
  • condensing
  • sublimation
  • evaporation/ boiling
  • melting
• ionic bonding

  • metals always lose outer electrons
  • when they bond
  • to leave an empty outer shell
• magnesium's ion is

  Mg2+
• non-metals are involved in

  ionic bonding and covalent bonding
• ionic bonding

  • metals + non-metals
  • metals lose electrons
  • non-metals gain electrons
• covalent bonding

  • non-metals
  • share electrons
• metallic bonding is

  metal ions form a lattice surrounded by a 'sea' of delocalised electrons
• metals are good conductors of heat because

  electrons are transferred