Chemistry-Bonding

• Metallic bonding occurs between metal atoms, where delocalized electrons move freely throughout the lattice structure.
• Covalent bonds are formed when two atoms share pairs of electrons.
• Ionic bonding is the transfer of electrons from one atom to another.
• Ionic bonding involves the transfer of one or more electrons from one atom to another, resulting in positively charged cations (metal) and negatively charged anions (non-metal).
• Covalent bonds form when two non-metals share pairs of valence electrons.
• Ionic compounds have high melting points due to strong electrostatic forces holding the positive and negative ions together.
• covalent bonds have low boiling and melting point due to the weak bonds between the molecules
• metallic compounds are malleable, ductile and have high melting and boiling points.
• Metallic bonding occurs when metal atoms lose their outermost electron(s), forming a sea of delocalised electrons that hold the positive ions together by electrostatic attraction.
• In ionic solids, there are no free electrons available for conduction, so they do not conduct electricity.
• Ionic compounds are hard and brittle and have high melting points due to the strong electrostatic forces of attraction between the positive and negative ions
• metallic compounds are malleable because they are made of layers so the can slide over each other.
• metallic compounds are ductile because they are made up of layers which allows them to be stretched into wires without breaking.
• the melting and boiling points of metals are very high as it takes a lot of energy to break the strong metallic bonds.
• Covalent bonding involves sharing pairs of electrons between non-metal atoms.