Structure and Bonding
Structure and bonding
Ionic bonds are chemical bonds formed through an electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between an metal and a non-metal. The metal loses an electron or electrons form its highest energy level becoming a positively charged Ion and the non-metal gains an electron or electrons in its highest energy level, becoming a negatively charged Ion.
Covalent bonds are strong bonds between two non-metal atoms. A covalent bond forms when two non-metal atoms share a pair of electrons. The electrons involved are in the highest occupied energy levels - or outer shells - of the atoms. By sharing electrons, both atoms are able to complete their highest energy level, meaning the atom is stable.
Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between the free electrons and metal ions. Metallic bonds are strong, so metals can maintain a regular structure and usually have high melting and boiling points. Metals are good conductors of electricity and heat, because the free electrons carry a charge or heat energy through the metal. The free electrons allow metal atoms to slide over each other, so metals are malleable and ductile.
Ionic Bonding is the type of bonding which takes place between the sodium and chlorine ions. Sodium has 11 electrons and chlorine has 13. Sodium loses one of its electrons, leaving it with 10 and therefore stable. Chlorine gains an electron and so ends up with 14, meaning it is also stable as it has an even number of electron sin its higest energy level. There are many ionic bonds in an ionic compound such as sodium chloride, arranged in giant lattice structures. Ionic compounds have very strong bonds and a lot of energy is required to break them, meaning they have high melting and boiling points.
Oxidation and Reduction
Oxidation: the gain of oxygen from a
Ionic bonds are chemical bonds formed through an electrostatic attraction between two oppositely charged ions. Ionic bonds are formed between an metal and a non-metal. The metal loses an electron or electrons form its highest energy level becoming a positively charged Ion and the non-metal gains an electron or electrons in its highest energy level, becoming a negatively charged Ion.
Covalent bonds are strong bonds between two non-metal atoms. A covalent bond forms when two non-metal atoms share a pair of electrons. The electrons involved are in the highest occupied energy levels - or outer shells - of the atoms. By sharing electrons, both atoms are able to complete their highest energy level, meaning the atom is stable.
Metals form giant structures in which electrons in the outer shells of the metal atoms are free to move. The metallic bond is the force of attraction between the free electrons and metal ions. Metallic bonds are strong, so metals can maintain a regular structure and usually have high melting and boiling points. Metals are good conductors of electricity and heat, because the free electrons carry a charge or heat energy through the metal. The free electrons allow metal atoms to slide over each other, so metals are malleable and ductile.
Ionic Bonding is the type of bonding which takes place between the sodium and chlorine ions. Sodium has 11 electrons and chlorine has 13. Sodium loses one of its electrons, leaving it with 10 and therefore stable. Chlorine gains an electron and so ends up with 14, meaning it is also stable as it has an even number of electron sin its higest energy level. There are many ionic bonds in an ionic compound such as sodium chloride, arranged in giant lattice structures. Ionic compounds have very strong bonds and a lot of energy is required to break them, meaning they have high melting and boiling points.
Oxidation and Reduction
Oxidation: the gain of oxygen from a