Element Information:

Name: Barium, Alkaline-Earth
Address: 62 Alaina Avenue
Birthday: June 20, 1744
Gender: Metal
Family Name: Alkaline-Earth
Other Family Members: Beryllium, Magnesium, Calcium, Suonium, Radium
Family Characterists: Shiny, silver, silver white color, highly reactice, metals, all found in Earth's crust.
General Inforamtion: 56 protons, 81 neutrons, 56 electrons, 2 valence electrons

Lewis Structure picture.


Covalent Bonding
The whole reason elements bond is because they want a full outer shell of valance electrons! Atoms want to have a full outer shell. When the outer shell is full, it is said to be stable. If the outer shell is not full, the atom will try to bond with another atom. In Covalent bonding the elements share the valence electrons rather then taking them! You can have polar and non-polar covalent bonds. Polar bonds mean that different atoms are bonding. Non-polar means that the same atoms are bonding like in my examples below! Only two non-metals can form covalent bonds.
I cannot form a covalent bond because I am a metal and only non-metals can form covalent bonds!

Covalent bonds are formed when:

  • Atoms share one or more pairs of electrons.
  • They are only formed between non-metal atoms.
  • The electrons are not sent from one atom to another. I
  • Instead, they are shared by both atoms
I cannot form a Covalent Bond because I am a metal! Only non-metals can use covalent bonding.

Here are rules/steps for making Covalent Bonds:

  1. Write the symbols.
2. Fill in the valance electrons.

3. Find holes where valance electrons are needed.
4. Draw arrows from the electrons to the holes.
5. Rewrite the bond with another atom with a bar symbolizing that those elements are sharing valance electrons.

Ionic Bonding -
An ion is an electrially charged atom. They are usually poitive or negative. Positivly charged ions are called anions. Negativly charged ions are called cations! In order to have a charge, an element will want to have a full outer shell. To do this elements will either give away or gain electrons. Usually elements with 1-3 elements wil give away their electrons making them positively charged! And elements with 5-7 electrons will gain electrons manking them negativly charged! And elelments with 4 electrons are the oddballs and they can give or take depending on stuff that we haven't learned yet! This bond can only be formed between non-metals and metals.

How an ion is formed:

How Ionic bond is formed:
An ionic bond is formed by one element giving away an eletron and another element gaining that electron making both of these elements happy becuase they both have a full outer shell!I can form an ionic bond because i am not an oddball, i have two electrons so i give away electrons making myself positive!

Example of Ionic Bonding:

this bond will turn out to be H+Cl-

I can bond with Florine, Bromine and Chlorine with Ionic bonding.
A group bond I can form is with Myself, Hydrogen and Chlorine!

Metallic Bonding- A metallic bond is a bond formed by the attraction between positively charged metal ions and the electrons around them.
Electrons move freely between metal ions.
Friends, Please Join Me!
I can form Ionic and Metallic bonds.
Metallic bonds I can form with are all metals!
Ionic bonds I can form bonds with are:

  • Hydrogen (group bonds only)
  • Flourine
  • Clorine
  • Bromine
  • Iodine

I Want to Join
On another element's page (created by another student), click edit the page and type in this section only. Add a blank line under this area and explain in a sentence or two who you are (element and class period - hydrogen3), what type of bond you would form with the element on this page, and why you would form a bond with this element. After you have typed your sentence, highlight your element name (hydrogen3) and click the "Insert Link" button from the editing toolbar (Globe with a chain at the bottom). Make sure that the link text and the page name are your element name and period number. Do not change them or put a space in between them. Click "OK" and now "Save" the page. Click on your element name to link back to your element's page. If your page does not appear, ask for assistance and go back and redo the link on this section.