Atomic Relationships Read each section and carefully write your responses to the directions on this worksheet. Key Vocab Stability Valence Electrons Electron Shells Noble Gasses Octet Rule Part 1: Read the following overview and answer the questions below. Overview Atoms are constantly searching for ​
stability ​
or a way to fill their shells. The only ​
stable ​
elements on the periodic table are in Group 8 and are called the​
​
Noble Gasses.​
These elements are stable because they have full Valence Electron Shells. ​
Valence electron shells w
​ill fill with 8 electrons, unless, like Helium (He) the atom only has one shell, then its Valence shell will fill with 2 electrons. To become ​
stable,​
all elements that aren’t the noble gasses will have to form a relationship with other atoms that help make their total valence shell complete. An example of one of these relationships we are familiar with is the bond between Hydrogen and Oxygen that forms H​
0. Oxygen has 6 Valence electrons which we know because it is in 2​
group 6 of the periodic table. To have a full shell Oxygen only needs two more electrons. Hydrogen has 1 valence electron, which we know because it is in the first group of the periodic table. If Oxygen bonds with two Hydrogen (6+1+1) together they have 8 electrons. If we were to use the Lewis Dot structure to show this relationship it would look something like this: As you can see, the electrons are rearranged and drawn in a way so that the electrons fit together like puzzle pieces. Oxygen now looks like it has 8 Valence electrons and each Hydrogen atom has 2 electrons, completing its only valence shell. Many different combinations can be made between atoms in order to reach a full valence shell with 8 electrons. This tendency for main group elements (those in Groups 1 to 8 and not including transition metals) is called the ​
Octet rule​
. Reading Questions 1) What group is called the Noble Gasses and how are they different from other atoms? 2) How many electrons fill a Valence Shell? What two elements are the exception and fill with 2 electrons? 3) What is the Octet rule? Write a definition or explanation in your own words Part 2: Atomic Relationships ­ Read the directions below to complete the learning activity Atoms’ interactions with each other can be varied based on the number of Valence electrons they have. To better understand these interactions it helps to think of atoms and the bonds they form as relationships. Like people, the relationships between atoms are varied. Some Atoms don’t form bonds with others, they are content to be on their own, while other atoms rapidly form bonds and need other atoms to be stable. Furthermore some Atoms can form multiple relationships with many different types of atoms while other atoms are limited on the relationships they can form with atoms due to their valence electrons. Like people, atoms are diverse and varied in how they interact with each other. The following activity will allow you to practice drawing models of atoms and molecules as well as allow you to make creative comparisons in order to better understand bonding. Step 1)​
​
Draw​
the Lewis Dot Structures of the Atoms Step 2) ​
Identify​
what Atoms could form bonds with each other and write them in the relationship box Step 3) ​
Draw ​
the ​
relationship​
(or bond) that these atoms have using the Lewis Dot Structure. Step 4)​
Create a ​
creative description​
that describes the bonding relationship of the atoms. Example Step 2) Atoms in Relationship Step 3) Relationship Bond Step 4) Description of the Bond Sodium (Na) and Chlorine (Cl) have an interesting relationship. Though we see them often at dinner (salt), you can see that Chlorine is not good at sharing electrons and tends to keep them all to itself. There must be something we don’t know about Sodium that keeps them together. Step 1) Draw the Lewis Dot Structure for the following Atoms ( you can add more) Ca Cl F O Mg H He Ne Steps 2 ­ 4) Identify atoms, draw possible bonds and describe the relationship Atoms in Relationship Relationship Bond Description of the Bond