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Metallic bonding consists of a giant lattice of positive metal ions. These ions are surrounded by a sea of delocalised electrons that are free to move. The strong electrostatic attraction between these positive ions and the delocalised electrons holds the structure together. Covalent bonds involve sharing electron pairs, while ionic bonds involve the transfer of electrons between atoms. A mixture contains different substances that are not chemically bonded.

Metals are good conductors of electricity because the delocalised electrons are free to move through the giant metallic lattice when a voltage is applied. In contrast, simple molecular compounds like water or methane have no free electrons or ions to carry a charge, making them poor conductors. Ionic compounds only conduct when molten or aqueous because the ions are then free to move, but not in the solid state. Graphite is a non-metal that conducts, but most non-metals do not.

Metallic lattices are malleable and ductile. This is because the layers of positive ions can slide over each other when a force is applied. The sea of delocalised electrons moves with the ions, so the metallic bond is not broken. In giant covalent structures like diamond, the bonds are rigid and break if the atoms move, making them brittle. Compounds and mixtures have different physical properties based on their specific compositions.

A sodium atom has a proton number of 11. It has 11 electrons. The electronic configuration is 2,8,1. It has three occupied electron shells, so it is in Period 3. It has one electron in its outer shell, so it is in Group I.

Isotopes are atoms of the same element. They have the same number of protons but different numbers of neutrons. Isotopes of the same element have the same chemical properties. This is because they have the same number of electrons and the same electronic configuration.

Ionic bonds form when a metal atom gives electrons to a non-metal atom. This creates positive ions and negative ions. An ionic bond is a strong attraction between these oppositely charged ions. These compounds have high melting points because the attractions in the giant lattice are very strong and need a lot of energy to break.

Metallic bonding consists of a giant lattice of positive metal ions. These ions are surrounded by a sea of delocalised electrons that are free to move. The strong electrostatic attraction between these positive ions and the delocalised electrons holds the structure together. Covalent bonds involve sharing electron pairs, while ionic bonds involve the transfer of electrons between atoms. A mixture contains different substances that are not chemically bonded.

Metals are good conductors of electricity because the delocalised electrons are free to move through the giant metallic lattice when a voltage is applied. In contrast, simple molecular compounds like water or methane have no free electrons or ions to carry a charge, making them poor conductors. Ionic compounds only conduct when molten or aqueous because the ions are then free to move, but not in the solid state. Graphite is a non-metal that conducts, but most non-metals do not.

Metallic lattices are malleable and ductile. This is because the layers of positive ions can slide over each other when a force is applied. The sea of delocalised electrons moves with the ions, so the metallic bond is not broken. In giant covalent structures like diamond, the bonds are rigid and break if the atoms move, making them brittle. Compounds and mixtures have different physical properties based on their specific compositions.

Metallic bonding involves an attraction between positive metal ions and a sea of delocalised electrons. These electrons can move through the lattice, which allows the metal to conduct electricity.

Malleability is the property that allows a metal to be hammered into sheets without breaking. This happens because the layers of metal ions can slide over each other while the delocalised electrons maintain the bond.

An element is a pure substance. It contains only one kind of atom. Gold and oxygen are examples of elements.

A mixture contains different substances. These substances are not joined together. You can separate a mixture easily by physical ways.

A sodium atom has a proton number of 11. It has 11 electrons. The electronic configuration is 2,8,1. It has three occupied electron shells, so it is in Period 3. It has one electron in its outer shell, so it is in Group I.

Isotopes are atoms of the same element. They have the same number of protons but different numbers of neutrons. Isotopes of the same element have the same chemical properties. This is because they have the same number of electrons and the same electronic configuration.

Ionic bonds form when a metal atom gives electrons to a non-metal atom. This creates positive ions and negative ions. An ionic bond is a strong attraction between these oppositely charged ions. These compounds have high melting points because the attractions in the giant lattice are very strong and need a lot of energy to break.