Chemistry Portfolio; 10th Grade

CHEMISTRY PORTFOLIO







By; Nick Bolyard






Period 5












The octet rule is a simple rule that states that atoms can or tend to combine so that they have eight valence electrons in their outermost shell. The maximum number of electrons allowed is eight in the outermost shell
Now that you know what the octet rule is, you may find yourself asking, “What is a valence electron?” A valence electron is an electron, or up to eight (stated in Octet rule), that is in the outermost electron shell.
Now, there are also many differences between ions. There are anions and cations. The cations (notice the T), are positive ions. The anions (notice the first N), are negative ions. Below, there are two pictures. One picture represents a cation, and the other pictorially explains an anion.


CATION ANION
Na +1 S -2

The “pluses” and the “minuses” represent the number of valence electrons that it would take to fill the octet rule. The positive, plus one, means that the atom has to actually lose one electron due to the fact that electrons are negatively charged, and the same goes for the negative, or minus two for anions.








NOBLE GASES; GROUP 18

•
Helium; __ He
1s

For this element, it does not gain OR lose any electrons because it is already a noble gas.




••
NEON; __ __ __ __ __ ••Ne ••
1s 2s 2p 2p 2p ••

This element is another noble gas, which means that the outermost electron shell is full.







Argon; __ __ __ __ __ __ __ __ __
1s 2s 2p 2p 2p 3s 3p 3p 3p
••
•• Ar ••
••
This is another noble gas, which does not lose or gain ANY valence electrons.











HALOGENS; GROUP 17


FLOURINE; __ __ __ __ __
1s 2s 2p 2p 2p
••
••F••
•

The black arrow in the 3p column represents the arrow that is needed to fill the octet rule. This means that this specific element is a -1.





CHLORINE; __ __ __ __ __ __ __ __ __
•• 1s 2s 2p 2p 2p 3s 3p 3p 3p
••Cl••
•

Similar to Fluorine, Chlorine must gain one electron to fill the octet rule. This element, being similar to Fluorine, is -1 as well.


















NON-METALS; GROUP 16

OXYGEN; __ __ __ __ __
1s 2s 2p 2p 2p
••
••O•
•

This element must gain two electrons to fulfill the octet rule, so the ionic charge for Oxygen is -2.








SULFUR; __ __ __ __ __ __ __ __ __
1s 2s 2p 2p 2p 3s 3p 3p 3p

••
••S•
•
This element has to gain 2 electrons to fulfill the octet rule, so the element is also a -2.


















NON-METALS; GROUP 15

NITROGEN; __ __ __ __ __
1s 2s 2p 2p 2p
••
•N•
•
For the elements in group 15, they must all gain three electrons, so their charge is -3.

NON-METALS; GROUP 14

CARBON; __ __ __ __ __
1s 2s 2p 2p 2p
•
•C•
•

This element, along with the other non-metals in group 14, is very unique. These elements are neutral elements, that don’t know what to do with themselves. We are unsure on whether or not they will lose or gain any electrons at all, so they are neutral.






















ALKALINE EARTH METALS; GROUP 2

BERYLLIUM; __ __
1s 2s
•
Be
•
Beryllium is a +2 because it loses two electrons.


MAGNESIUM; __ __ __ __ __ __
1s 2s 2p 2p 2p 3s
•
Mg
•
Magnesium is a lot like the other Alkaline Earth Metals, which means that it is +2 as well.



CALCIUM; __ __ __ __ __ __ __ __ __ __
1s 2s 2p 2p 2p 3s 3p 3p 3p 4s

•
Ca
•
Calcium, which is very similar to Magnesium and Beryllium, is also +2.















ALKALINE METALS; GROUP 1
“When the Saints came marching in”
HYDROGEN; _
1s
•
H

LITHIUM; __ __
1s 2s
•
Li

SODIUM; __ __ __ __ __ __
1s 2s 2p 2p 2p 3s
•
Na

POTASSIUM; __ __ __ __ __ __ __ __ __ __
1s 2s 2p 2p 2p 3s 3p 3p 3p 4s


The Alkaline Metals are a very unique group. This group is willing to give up their only valence electron.