C.3 Structure and Bonding

• covalent • ionic • metallic

Covalent • Non metal • non metal Ionic • Metal • Non metal Metalic • Metal • Metal

• The metal transfers electron(s) • positive ion formed • To the non metal • negative ion formed

• How many electrons it needs to gain (x) for a full outer shell • x- • How many electrons it needs to loose (x) for a full outer shell • x+

• ionic compound structure • held together by strong electrostatic forces of attraction • between oppositely charged ions • high melting and boiling points due to large amount of energy needed to brake bonds • when in solution or molten they conduct electricity • ions are free to move and carry a charge

2D • clear arrangment of ions in one layer • but not how the next one is arranged Ball and stick (3D) • arrangment of ions in a large section • but forces actually act in all direction • no free space between ions

• Swap the charges of the atoms • Bring them down

• atoms share pairs of electrons • bonds are strong

• small molecules • large molecules such as polymers • giant covalent such as diamond

• giant structure of atoms • electrons in outer shell of metals atoms are decolised • free to move through the structure • metal become positive ions • sharing delocalised = strong metalic bonds

• solid (s) • liquid (l) • gas (g) • aqueuous (aq) • dissolved in water

• The energy needed to brake forces • therefore the strength of the force

• model includes no forces • particles are all spheres which are solid

• high melting and boiling point • electrostatic forces of attraction require lost of energy to break • conduct when molten or dissolved • ions are free to move and carry a charge

• have low melting + boiling points • weak intermolecular forces which require little energy to break • often liquid or gas • do not conduct • no charged particles

• The larger the molecule the stronger the intermolecular forces are • Therefore higher m.b.p

• very large molecules • atoms in polymers are linked to eachother atoms by strong covalent bonds • intermolecular forces between polymers are relatively strong so are solid at room temp

• very high melting points • strong covalent bonds which require very large amount of energy to overcome

• diamond • graphite • silicon dioxide

• giant structure of atoms with strong metallic bonds • high melting point

• in pure metals atoms are arranged in layers • which allows them to bend and be shaped easily • in alloys the layers are distorted = stronger

• mixture of two or more elemnts • one must be a metal

• Metals are good conductors of electricity • The delocalised elecrons carry electrical charge • THROUGH • the metal

• Metal are conductors of thermal energy • energy is transferred by delocalised electrons