Bonding Chemistry

This is a maindmap all to do with Bonding in chemsitry C2. 

HideShow resource information
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.
    • 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
    • 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 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.

Comments

No comments have yet been made

Similar Science resources:

See all Science resources »See all Atoms resources »