Chapter 8 Summary

Section 8.1 describes what molecules and molecular compounds are. Molecules that are monatomic are consisted of only single atoms. Molecular compounds are only between non-metals. Another topic is that it tells us what a covalent bond is. It is formed by a pair of electrons by two atoms.

Section 8.2, it shows and teaches us about how covelant bonds are formed, and what type of bonds it can form. It shares that covalent bonds' electrons usually occur so that atoms attain the electron confliguration of the noble gases. An example of this would be a pair of hydrogen atoms to form a hydrogen molecule, which will attain the electron confliguration of helium, which is a noble gas and has 2 electrons. A single covelant bond joins 2 atoms which are held together by a pair of electrons. An example of how this could be written is H:H where the colon is represented by the shared electrons. Another way of writing the same formula is H-H. When there is a dash, you are writing a structural formula. It may be confusing when writing this because a similar symbol is H2. The difference is that H2 means that there are two molecules in the atom Hydrogen. H-H or H:H means that there is a covalent bond connecting two different atoms which are sharing electrons. They are drawn for molecules of compounds The opposite of this is called an unshared pair, when a pair of valece (outer) electrons that are not shared between atoms. This is also known as a lone pair or a nonbonding pair. Using dot structure can be used between 2 different atoms. Let's say we are trying to figure out dot structure for ammonia (NH3). All that would happen would have N in the middle and have the 3 H's around it. These sections have done very well explaining what it had to teach.