1. CH H H H Chemistry All you need to know about bonding (unless you really want to know a lot) (And a lot of random science facts)

2. CH H H H Ionic Bonds Ionic Bonds are formed when one atom gives up some of its electrons to another element which needs it. An ionic bond would be formed that can hold the two atoms together as a molecule. Examples of ionic bonds include the famous NaCl, MgO and a variety of others. Na Cl

3. CH H H H Covalent Bonding There are 4 types of bonding, ionic bonding, covalent bonding, metallic bonding and dative bonding. Covalent Bonding is one of them where electrons are shared between 2 atoms. Each of the atoms would have a full shell. Examples of covalent bonds are Water (H 2 O), Methane (CH 4 ), Ethanol (C 2 H 5 OH) etc. C H H H H O HH

4. CH H H H Metallic and Dative Bonding Metallic bonding in short and simple words is a sea of electrons moving around many nuclei that are in a fixed position. Dative bonding is a covalent bond where one atom donates both the electrons. An example is the ammonium ion (NH 4+ ) or Boron Trifluoride where nitrogen and boron forms a dative bond with hydrogen and fluorine respectively N H HH H Non-Bonding or lone pair of electrons, forms a bond with any element willing to take the electrons

5. CH H H H Giant Molecular Structures Giant Molecular Structures are either Giant Ionic Structures or Giant Covalent Structures. Giant Ionic Structures tend to be able to be dissolved in water, have high boiling points and conduct electricity when molten or dissolved in water. (e.g. NaCl) Giant Covalent Structures tend to not be able to be dissolved in water, have high boiling points but do not conduct electricity. (e.g. SiO2, Diamond, Graphite) Na Cl Many NaCl molecules make a giant ionic structure

6. CH H H H Electronegativity Electronegativity is the measure of how readily an atom will grab or give up electrons. Atoms with higher electronegativity will attract electrons more easily than those that have lower electronegativities. The highest electronegativity is Fluorine with 3.98 (Source: Wikipedia). The lowest electronegativity on Wikipedia’s list is Francium with 0.7.

7. CH H H H Polar Bonds Polar Bonds are formed when atoms of different electronegativities are bonded together by a covalent bond. It creates a slightly positive charge (represented by δ+) in the atom with the lower electronegativity as well as a slightly negative charge (represented by δ-) in the atom with the higher electronegativity as the electron tends to spend more time in the element that is more electronegative. It causes special characteristics. (i.e. some molecules with polar bonds can be dissolved in water) O HH δ-δ- δ+δ+δ+δ+

8. CH H H H Non-Polar Bonds Non-Polar Bonds occurs when two atoms with the same electronegativity (usually from the same element) form a covalent bond. The electrons do not favour one atom over the other, therefore, no charge develops. Cl

9. CH H H H Hydrogen Bonds Hydrogen bonds are temporary bonds formed when hydrogen from one atom affects a highly electronegative atom (i.e. oxygen, nitrogen, fluorine etc.) in another atom (or the same atom). They are stronger than normal van der Waals interactions. They cause water’s high boiling point compared to other similar molecules. O HH O H H Temporary hydrogen bonds

10. CH H H H References http://en.wikipedia.org/wiki/Electronegativities_of_the_elements_(data_ page) http://en.wikipedia.org/wiki/Electronegativities_of_the_elements_(data_ page) http://www.webchem.net/notes/chemical_bonding/dative_bonding.htm http://en.wikipedia.org/wiki/Hydrogen_bond Stop Faking It Chapter 1 Advanced Chemistry for You by Lawrie RYAN Microsoft Office Clip Art