Bonding Chemistry
This is a maindmap all to do with Bonding in chemsitry C2.
- Created by: jatyization
- Created on: 28-03-13 16:39
View mindmap
- Bonding C2
- Ionic Bonding
- Ionic bonding is when a non-metal element reacts with a metal element to give one or more electrons . This happened to make them have a full outer shell of electrons (8).
- The Metal Atoms loose electrons and become positive ions.
- The Non-metal atoms gain electrons and become negative ions
- For example: A sodium atom loses an electron to form a sodium ion with a 1+ charge. A chlorine atom then gains the electron to form a chlorine ion with a 1- charge
- The opposite charged ions are electrostacitcaly attracted
- Ionic bonds have high melting and boiling points
- Ionic compounds can conduct electricity ONLY if the ions are free to carry the electric current.
- E.g: Solid sodium chloride does not conduct electricity as the ions cannot move, but dissolved in water or molten, it can conduct electricity.
- Ionic bonding is when a non-metal element reacts with a metal element to give one or more electrons . This happened to make them have a full outer shell of electrons (8).
- Covalent Bonding
- Covalent bonding is when two elements share electrons in order to have a full outer shell
- Covalent Bonds share electrons to achieve noble gas electronic structures which are stable
- outer electron shells overlap
- An oxygen atom shares two electrons with another oxygen atom to make a DOUBLE BOND; two shared electrons
- the nuclei of both atoms involved in a covalent bond are positively charged and the electrons involved are attracted to the nuclei, and so remain a fixed distance apart from each nucleus. this distance is called the bond length.
- Covalent bonds have low boiling and melting points because they have weak attractions between the molecules these are called intermolecular forces
- Covalent bonds are strong but they only exist between the atoms in the molecule
- cannot dissolve in water
- Cannot conduct electricity because there are no particles free to move
- Covalent bonding is when two elements share electrons in order to have a full outer shell
- Metallic Bonding involves charged metal nuclei and a sea of delocalised electrons
- They are malleable as they can slide over each other
- Ionic Bonding
- Ionic Bonding
- Ionic bonding is when a non-metal element reacts with a metal element to give one or more electrons . This happened to make them have a full outer shell of electrons (8).
- The Metal Atoms loose electrons and become positive ions.
- The Non-metal atoms gain electrons and become negative ions
- For example: A sodium atom loses an electron to form a sodium ion with a 1+ charge. A chlorine atom then gains the electron to form a chlorine ion with a 1- charge
- The opposite charged ions are electrostacitcaly attracted
- Ionic bonds have high melting and boiling points
- Ionic compounds can conduct electricity ONLY if the ions are free to carry the electric current.
- E.g: Solid sodium chloride does not conduct electricity as the ions cannot move, but dissolved in water or molten, it can conduct electricity.
- Ionic bonding is when a non-metal element reacts with a metal element to give one or more electrons . This happened to make them have a full outer shell of electrons (8).
Comments
Report