HYDROGEN MOLECULES

A hydrogen atom only has one electron, so it only has one s sub shell, that is 1s orbital.
Hydrogen atom is not stable. It can stable if it has 2 electrons (duplet rule). That is why, hydrogen gas consist of 2 atoms per molecule (diatomic molecule). When two hydrogen atoms are closely, the electrons are attracted by each hydrogen's protons, and share one of another to form an electron pair. As a result, there is a non polar covalent bond of hydrogen molecule, H2. The non polar bond is occurred, because these two hydrogen atoms have the same ability of attraction.

WATER COVALENT BONDING TASK

This is another example of polar covalent bond. Write an explanation text about 150 words, around 3 - 4 paragraphs.

You have to choose the best sentences which have a full meaning and short. Don't make it to long, because you will loose the relationship between concepts.

The paragraphs move from general to the specific concepts, from concreate to abstract theories.
Please try, you have to develop your writing step by step gradually, OK? So do it.

POLAR COVALENT BONDING TASK

Students, develop your thinking to the next bonding, that is polar covalent, as seen in the picture.
Before explaining this bond, firstly distinguish between polar and non polar covalent bonds. It is about polarity of bonding. The bond of H2 and Cl2 are different with the bond of HCl. The first are molecules of elements, on the other hand, the last is a molecular compound.
In writing the paragraphs, mention about electronegativity, the position of bonding electron pair (BP) between H - Cl, and the effect of this BP.

OXYGEN MOLECULES TASK

The next concept is the bond of oxygen molecules. Paragraphs that you have to write consist of Lewis structure, octet rule, non polar covalent bond, and double bond.
Firstly concern with oxygen molecules, then draw a conclusion.
After that, move on another example of non polar bond, such as nitrogen. Be careful, remember that valence electron of nitrogen atom is different with oxygen atom, so the type of non polar bond is also different.
Draw a diagram of nitrogen, similar to the diagram of oxygen in the picture.

NON POLAR COVALENT BONDING TASK

After you learn quite a lot about an ionic bond, now think another bond, that is a covalent bond.
Look at the picture, the simplest example is a hydrogen molecule. Compare this bond with ionic bond, such as in table salt, NaCl.
Is there any electron transfer in the bond between hydrogen atoms? Are you sure there is no electron transfer at all? What is the reason? Hydrogen is a non metal, so the bond is really different with NaCl, because sodium is a metal. Its OK, good point.
As before, your task is, make paragraphs which consist of clear explanation about the bond oh H2 molecules. Don't forget to mention Lewis structure, duplet rule, single covalent bond, and non polar covalent bond, including the reason of each clarification. Then apply this concept to another similar molecule, such as chlorine molecules.

COVALENT BONDING PROBLEMS

A hydrogen atom and a chlorine atom do not exist in the nature. They exist as hydrogen molecules, H2 and chlorine molecules, Cl2 because they are more stable as molecules rather than as atoms. Think about these and explain the reason.

When hydrogen gas and chlorine gas react one of another, as a result, hydrogen chloride, HCl is formed. Now what do you think about this process? Is it because the elements of H2 and Cl2 are less stable than HCl? If your answer is yes, so give me the reason. Remember, do not only say yes, OK? Always give the reason by using a strong argumentation. Write a paragraph to make a good explanation.

Don't forget to explain about duplet and octet systems; discuss the tendency of atoms in order to achieve their stability as same as the noble gas that the position is closely to these atoms, in the periodic table. Compare the Lewis structure of H2, Cl2, and HCl. Classify the type of covalent bonding, which is(are) a non polar covalent bond and which is (are) a polar one.

After you conclude the above concept, develop your knowledge by thinking about polar molecules and non polar molecules, the different polarity of molecules.