Chemistry ionic bonding to giant covalent structures

Ionic bonding

Ionic bonding

• Metals react with non-metals

• Metal atoms lose 1 or more electrons, giving them a + charge

• Non metal atoms gain 1 or more electrons, giving them a - charge

• They attract each other called an ionic bond and both have full outer shells

Electrolysis

• Contains two electrodes:

  • Anode: The positive electrode.

  • Cathode: The negative electrode.

• These electrodes are connected to a power source.

• The electrolyte (liquid or molten ionic compound) provides ions to carry the charge.

• Positively charged ions (cations) in the electrolyte move toward the negatively charged cathode.

• Negatively charged ions (anions) move toward the positively charged anode.

• At the cathode, reduction occurs (gain of electrons) and unless the substance is gold, silver, platinum, copper, hydrogen (H⁺) gets produced.

• At the anode, oxidation occurs (loss of electrons) and unless this substance is a halogen (group 7), oxygen gas (O₂) is produced.

Covalent bonding

Occurs between non-metal atoms where electrons are shared to achieve full outer electron shells. Each shared pair of electrons constitutes a covalent bond. Covalent compounds typically have lower melting and boiling points compared to ionic compounds. They do not conduct electricity in solid or molten state, are often insoluble in water, and can exist in any state at room temperature. For some compounds, more electrons may need to be shared. They can have up to 3 bonds per atom.

Simple molecular structures

Structures formed by covalent bonds between non-metal atoms, typically consisting of small groups of atoms (molecules) held together. These structures can exist in various states at room temperature, ie. solids, liquids, and gases. Simple molecular substances generally have low melting and boiling points due to weak intermolecular forces that require little energy to overcome.

Giant covalent structures

Large networks of atoms connected by covalent bonds in a lattice. Unlike simple molecular structures, they consist of a vast number of atoms, resulting in strong intermolecular forces that contribute to high melting and boiling points. These structures do not conduct electricity due to the lack of free-moving charged particles and are insoluble in water, although graphite and graphene are exceptions as they only use 3 electrons in bonding, leaving an electron which is free to move and carry a charge.