Metallic Bonding

Metallic bonding→occurs between only metals, occurs between atoms from the same element or between atoms from different elements. Metal+metal

Metallic bonding involves→The atoms losing their valence electrons and becoming metal cations

The valence electrons become→Delocalised and freely move around the 3D lattice of metal cations.

Properties of metals

• Lustle(shininess)

• Conductivity (heat and electricity)

• Malleability ( can be hammered/bent)

• Ductile (can be drawn into wire)

• High Density (usually)

Ionic compounds

Ionic compounds→(ionic salts) are compounds consisting a positive and negative ion bonded by a strong electrostatic force. Eg. sodium chloride & ammonium sulphate

High melting temperature→Ionic compounds have very high melting points because of the 3D giant ionic lattice structure. Strong electrostatic forces between oppositely charged ions in the 3D lattice

Hardness→Ionic compounds are hard because the ions are held tightly in a rigid, fixed structure, making it difficult to compress.

Brittleness→Ionic compounds are brittle because of their 3D giant ionic structure. When force is applied, like charged ions may shift & repel each other, causing the structure to shatter

Electrical conductivity as a solid→Ionic compounds do not conduct electricity as solids because the ions are fixed in place & cannot move freely.

Electrical conductivity as a solution or liquid→Ionic compounds do conduct electricity when dissolved in water or melted, because the ions are free to move and carry electric current.

Ions

An atom will lose or gain electrons to→obtain a full valence shell, as this lowers its energy level.

Ionic bonding→non metal+metal. form when one or more electrons are transferred from one atom to another.

An ionic bond is an electrostatic attraction between→

Cations→Atoms that loose electrons become positively charged, Pawsitive, paw

Anion→Atoms that gain electrons that become negatively charged, Onion, sad

Metal atoms will→lose electrons

Non metal atoms will→gain electrons

No protons lost, gained→atomic number remains unchanged

Electrons that are lost by one atom→are gained by another, therefore isolated atoms cannot form ions

The name ending of the non metal element→changes to ide when it forms anion.

A transition metal→forming multiple ions can bond with multiple of the same anion.

Name indication cation range

• in Roman numerals in brackets.

• Copper(I) chloride CuCl

• Copper(II) chloride CuCl₂

• Copper (III) chloride CuCl

A polyatomic ion→Also known as molecular ion, is a charged chemical species (ion) composed of 2 or more atoms bonded together

Names & symbols of polyatomic ions→listed in Valence challenge

To have -ide ending→anions change their atoms name

Molecule anions→(with lost of oxygen) have an -ate ending. (Nitrate)

In Anion Cation table→Anion side, x-axis, Cation down- y-axis. Cat so long. Cation comes first. Cats better than onions.

Covalent bonding

Covalent bonding→a shared pair of electrons between atoms of non-metals, non metal+non metal

What forms molecules→Atoms of different elements that share a covalent bond

Atoms of the same element that share covalent bond are called→diatomic molecules

Covalently bonded molecules can be presented as→Valnece structural diagram, Lewis structural, electron dot diagram

The giant covalent bonding is very strong→causes substances to have high mb and bp

Bonded pair→shared pair of electrons that causes them to stay together

Lone pair→pair of electron that’s not involved in bonding