Bonding and Structure Flashcards
What is ionic bonding?
Non-metal + metal
metals lose electrons (positive charge)
non-metals gain electrons (negative charge)
Electrostatic force of attraction between oppositely charged ions
Formulas of silver, zinc, lead, iron ii, iron iii and copper ions
Silver Ag+ Zinc Zn+2 Lead Pb+2 IronII Fe+2 IronIII Fe+3 Copper Cu+2
Work out formula of ionic compound
Write down ionic symbols with charges
Check if charges equal zero
If not add extra ions to balance
Write the formula
Formulas of hydroxide, carbonate, nitrate, sulphate and ammonium ions
Hydroxide OH- Carbonate CO3 2- Nitrate NO3 - Sulfate SO4 2- Ammonium NH4 +
What is covalent bonding?
2 non-metal atoms (can be diatomic elements as well as compounds)
Atoms share electrons
The electrostatic force of attractions between the two nuclei and the shared pair of electrons
How are ionic compounds arranged?
In a giant ionic lattice
Properties of ionic compounds:
Usually solid
High melting and boiling points due to strong electrostatic forces of attraction which require lots of energy to overcome
ONLY conduct electricity as liquids (molten or in solution)
How are covalent compounds arranged?
In a simple molecular substance or giant covalent substance
Properties of simple molecular substances:
Usually gases or liquids
Low melting/boiling points due to weak intermolecular forces
Do not conduct electricity (molecule is not charged)
Properties of giant covalent substances (lattice):
Usually solids
High melting/boiling points due to strong covalent bonds
eg diamond, graphite (all allotropes of carbon)
Properties of diamond:
Very hard and strong
High melting point (due to strong covalent bonds)
Does not conduct electricity
Each carbon atom bonded to 4 others
Properties of graphite:
Soft, slippery surface (due to weak bonds between layers)
High melting and boiling point
Conducts electricity (due to delocalised electron)
Each carbon atom bonded to 3 others
Properties of buckminsterfullerene:
Hexagonal rings of 60 carbon atoms shaped like a football
Soft as the molecules are only held together by intermolecular forces
What is metallic bonding?
2 metal atoms
Metal atoms lose their outer shell electrons and become positively charged ions
Electrostatic force of attraction between positively charged ions and negatively charged delocalised electrons
Properties of metals:
Hard solids
High melting point
Conduct electricity and heat
Malleable (can be banged into shape) and ductile (can be drawn into wires)
