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CHEMICAL BONDING

CHEMICAL BONDING. A force that holds two atoms together is known as a Chemical Bond . The bond occurs when two nuclei attract the same electrons. Bonding is when a chemical bond is formed. When chemical bonds are broken and new bonds formed, this is a Chemical Reaction . Valence: Outer.

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CHEMICAL BONDING

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  1. CHEMICAL BONDING • A force that holds two atoms together is known as a Chemical Bond. • The bond occurs when two nuclei attract the same electrons. • Bonding is when a chemical bond is formed. • When chemical bonds are broken and new bonds formed, this is a Chemical Reaction.

  2. Valence: Outer • The valence energy level (shell) is the highest energy level in an atom where there is at least one electron. • The electrons in the highest energy level of an atom are known as Valence Electrons. • Chemical bonding involves a transfer of valence electrons.

  3. Noble Gases These six elements form only very few bonds. What similarities do they have? Consider their valence energy levels. • Helium • Neon • Argon • Krypton • Xenon • Radon

  4. Noble Gases • He – 1s2 • Ne – 2s2 2p6 • Ar – 3s2 3p6 • Kr – 4s2 4p6 • Xe – 5s2 5p6 • Rn – 6s2 6p6 • Helium has only the 1st energy level and room for electrons. • All the others have two sublevels (s and p) in their valence energy levels. • This means that eight electrons will fill the valence energy level.

  5. Octet There is something special about having eight electrons in the valence energy level. It is called an OCTET. All of the Noble gases are chemically inactive (inert) because the valence energy level is stable.

  6. Chemical Reactions!!! All of the other elements have between one and seven valence electrons. All of the other elements will react in order to get an octet. This can occur by either by the transfer of electron or by the sharing of electrons.

  7. IONIC BONDING Ionic bonding is a transfer of electrons from one atom to another. Most elements that lose electrons are metals. Most elements that gain electrons are nonmetals.

  8. IONIC BONDING Ionic bonds are formed between a metal and a nonmetal. The metal loses electrons and becomes positive. The nonmetal gains electrons and becomes negative. The positive ion attracts the negative ion… and they BOND. An IONIC BOND!!

  9. Let’s look at a typical metal POTASSIUM K 1s22s22p63s23p64s1 Potassium’s valence shell is the fourth energy level. If potassium lost an electron, then the third energy level would be the valence or outermost level. K 1s22s22p63s23p6 Now the valence shell only has 8 electrons in it. By losing an electron, the K atom has become a positive ion, a cation. K+ 1s22s22p63s23p6

  10. Now let’s look at a typical nonmetal Chlorine Cl 1s22s22p63s23p5 Chlorines valence shell is the third. If Cl is to have a stable octet, it must gain one more electron. By gaining another electron, the Cl atom has become a negative ion, an anion. Cl- 1s22s22p63s23p6

  11. The Plot Begins To Unfold K needs to get rid of one electron: K 1s22s22p63s23p64s1 Cl needs to accept one electron: Cl 1s22s22p63s23p5 The results are a positive K ion, a CATION, and a negative Cl ion, and ANION.

  12. The potassium gives the chlorine an electron and…

  13. The cation attracts the anion and…. K+ Cl- ….an ionic bond is formed. The compound Potassium chloride. KCl

  14. In some cases more than one electron must be transferred in order to give all the atoms a complete valence energy level. For instance, when magnesium bonds to fluorine. Magnesium 1s2 2s2 2p63s2 Fluorine 1s2 2s2 2p5 Magnesium can give fluorine one electron to give it a complete octet, but then magnesium is 1s2 2s2 2p61s2 2s2 2p63s1

  15. So, Magnesium can give an electron to another fluorine. Now it has a complete octet in the second energy level. 1s2 2s2 2p6 Mg+2 + F-1 + F-1 MgF2

  16. Covalent Bonding • Bonds are formed by sharing electrons. • Electrons are held in overlapping orbitals. • Typically this occurs when a nonmetal bonds to another nonmetal.

  17. Electron Dot Structures This type of bonding can be easily demonstrated with electron dot structures.

  18. Diatomic Elements 7 elements naturally bond in pairs. These can be easily shown with electron dot structures. Hydrogen is first, it shares its one electron with another hydrogen atom to form the diatomic H2. Any hydrogen gas found in nature is H2.

  19. Column VII Notice how the elements of column VII share electrons to get an octet.

  20. Oxygen Oxygen has a double bond, the oxygen you breath is O2.

  21. Nitrogen Nitrogen in the air has a triple bond, sharing 6 electrons.

  22. DIATOMICS There are 2 ways to remember the diatomic elements: ClIF H. BrON is the name of the person who discovered the diatomics. Not really, but the letters in his name are the symbols of the diatomic elements. Cl - chlorine I - iodine F - fluorine H - hydrogen Br - bromine O - oxygen N - nitrogen

  23. 7 Diatomic Elements The other way to remember the diatomic elements is the number 7. There are 7 diatomic elements and they kind of form a 7 on the periodic table. H N O F Cl Br I

  24. Coordinate Covalent Bond Typically when two atoms share electrons, one electron comes from one atom and one electron comes from the other atom. But in a coordinate covalent bond, both electrons in the bond come from one atom.

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