Structure and Bonding
Elements are held together in different ways and the properties of chemical compounds are determined by the bonding between atoms and the attractive intermolecular forces between molecules.
- Created by: Tae.
- Created on: 29-11-17 17:28
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- Structure and Bonding
- Ionic Bonding
- Ionic bonding occurs when a metal and a non-metal react together.
- The metal atom loses electrons to form a positively charged ion.
- The non-metal gains those electrons to form a negatively charged ion.
- The metal atom loses electrons to form a positively charged ion.
- Oppositely charged ions are strongly attracted to each other by electrostatic forces.
- This attraction is called an ionic bond.
- For example: sodium + chlorine = sodium chloride
- magnesium + oxygen = magnesium oxide
- calcium + chlorine = calcium chloride
- magnesium + oxygen = magnesium oxide
- Ionic bonding occurs when a metal and a non-metal react together.
- Covalent Bonding
- Non-metals bond by sharing pairs of electrons.
- The group of atoms bonded this way is called a molecule.
- The atoms only share electrons in their outer shells.
- This gives them the electronic structure of a noble gas: very stable.
- Covalent compounds usually have simple molecular structures.
- They are usually gases or liquids with low melting and boiling points.
- They don't conduct electricity because there are no free electrons.
- They are usually gases or liquids with low melting and boiling points.
- Non-metals bond by sharing pairs of electrons.
- Metallic Bonding
- The particles in a metal are held together by electrons.
- Metallic bonds are strong and a lot of energy is needed to break them.
- This is why metals have very high melting and boiling points.
- This is also means they are usually solid at room temperature.
- This is why metals have very high melting and boiling points.
- The electrons in the outer shell of metal atoms are delocalised.
- They are free to carry electrical current and thermal energy through the whole structure.
- This means they are good conductors of electricity and heat.
- They are free to carry electrical current and thermal energy through the whole structure.
- Metallic bonds are strong and a lot of energy is needed to break them.
- The particles in a metal are held together by electrons.
- Giant Covalent Structures
- All the atoms are bonded to each other by strong covalent bonds.
- Lots of energy is needed to break the covalent bonds.
- This means they have very strong melting and boiling points.
- They don't contain charged particles.
- This means they usually don't conduct electricity.
- Graphite conducts because each carbon atom has a delocalised electron.
- This means they usually don't conduct electricity.
- Lots of energy is needed to break the covalent bonds.
- All the atoms are bonded to each other by strong covalent bonds.
- Ionic Bonding
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