1. Bonding in chemicals
VELS 6

2. Transition from metal to non-metals 
Earth Metals
Transition from metal to non-metals 
Alkali
Group I
Alkaline
Group II
Halogen Gases
Group VII
Noble Gases
Group VIII 1
H 1+ 2 He 3
Li 1+
2,1 4
Be 2+
2,2 5
B 2+
2,3 6
C 4+
2,4 7
N 3-
2,5 8
O 2-
2,6 9
F 1-
2,7 10 Ne
2,8 11
Na 1+
2,8,1 12
Mg 2+
2,8,2 13
Al 2+
2,8,3 14
Si 4+
2,8,4 15
P 3-
2,8,5 16
S 2-
2,8,6 17
Cl 1-
2,8,7 18 Ar
2,8,8 19
K 1+
2,8,8,1 20
Ca 2+
2,8,8,2

3. Valence Electrons
The Outer Electron shell is the most important shell discussed in chemistry
It is called the Valence Electron Shell
The Electrons that occupied that shell are called Valence Electrons
They are at the highest
Energy state

4. The Most Important Thing
The number of valence electrons determines how an atom bonds with other atoms. Valence electrons cause chemical bonding to occur.
# of valence electrons
So why do elements in the same group have similar chemical properties?

5. Elements and Compounds
Elements are all the different materials in the periodic table they are one type of substance.
If you can find it in the periodic table it is an element!
Compounds are made up of more than one type of element.
To make a compound, elements are chemically bonded together.

6. Element Vs Compounds
Aluminium
Water
Boron
Carbon Dioxide
Helium

7. BONDING OPTIONS By transferring electrons (producing ions)
(metals-nonmetals)
By sharing electrons
(nonmetal- nonmetal)

8. Valence Electrons Electrons in the -outermost energy level or
-outermost electron shell or
-outermost orbital
(involved in chemical reactions)
Input Time

9. IONIC BOND Bond formed between two ions by the transfer of electrons

10. Ionic Bonds: One Big Greedy Thief Dog!

11. Transition from metal to non-metals 
Very Reactive Metals
Earth Metals
Transition from metal to non-metals 
Alkali
Group I
Alkaline
Group II
Halogen Gases
Group VII
Noble Gases
Group VIII 1
H 1+ 2 He 3
Li 1+
2,1 4
Be 2+
2,2 5
B 2+
2,3 6
C 4+
2,4 7
N 3-
2,5 8
O 2-
2,6 9
F 1-
2,7 10 Ne
2,8 11
Na 1+
2,8,1 12
Mg 2+
2,8,2 13
Al 2+
2,8,3 14
Si 4+
2,8,4 15
P 3-
2,8,5 16
S 2-
2,8,6 17
Cl 1-
2,8,7 18 Ar
2,8,8 19
K 1+
2,8,8,1 20
Ca 2+
2,8,8,2

12. Forming Ionic Bonds Potassium (K) and Fluorine (F)
Magnesium (Mg) and Chlorine (Cl)
Sodium (Na) and Oxygen (O)
Calcium (Ca) and Sulfur (S)
Do you see something in common with these combinations?
Hydrogen (H) and Chlorine (Cl)
Hydrogen a metal or non-metal?
Non-metal at normal temperature and pressure... But becomes theoretically a metal at very high pressures!
REMEMBER “non-metals and metals form ionic bonds”
Also Hydrogen is special as it can form ionic bonds with non- metals and metals as well even though it is a non-metal normally!

13. Exceptions to the Octet Rule
Hydrogen (H) only has one electron on the outer shell, thus requires another one to form bonds so that it has 2 valence electrons.

14. Input Time
IONIC BOND
Substance formed when electrons are transferred between 2 or more substances making ions. Happens between Metals and Non-metals The ions have an electrostatic attraction with each other to form an Ionic Bond.

15. Octet Rule Atoms want 8 (or 0) valence electrons
Wants to be a noble gas!! As in…wants to have a complete valence shell

17. Lets try to draw some covalent bonds!
Potassium (K) and Chloride (Cl)
Valency of K and Cl?
Octet Rule Applied!
Don’t Forget to write the formula too!!

18. Lets try to draw some ionic bonds!
Magnesium (Mg) and Chlorine (Cl)
Valency of Mg and Cl?
Octet Rule Applied!
Don’t Forget to write the formula too!!
Input Time

19. COVALENT BOND Bond formed by the sharing of electrons between (non metal - nonmetal)

20. Two fluoride atoms share one electron each to forms a covalent bond.
Covalent bonds also follow the Octet Rule (8 valence electrons each)
(except for very special cases like hydrogen 2 valence electrons)
Molecules are neutral groups of atoms held together by covalent bonds!

21. THIS IS A WATER MOLECULE!!!!!
Covalent Bonds: Hydrogen Shares electron with oxygen and vice versa!
What are these two elements?
Are they metal or non-metals?
What type of bond would they form? Remember Hydrogen is special
When bonding don’t worry about the inner electrons!!!
New count the valence electrons! Make sure there is 8 or two for hydrogen
Uh-oh not enough!!!
Find another atom to complete the share!

23. Sharing one pair creates Single Bonds
Sharing four electrons creates Double Bonds
Sharing one pair and a second separate pair
Sharing four separate pairs
Input Time

24. Summary of The Octet Rule
Input Time
REMEMBER!
All elements want to be like noble gases
Thus they want full electron shells.
Full electron shell are 8 valence electrons.
The Octet Rule
Atoms form chemical bonds so that they have an octet of valence electrons. Either by
Gaining, losing valence electrons or
Sharing valence electrons.
In other words: When atoms bond together, they each want a set of 8 valence electrons. (except for hydrogen who wants two)

25. DRAWING MOLECULAR STRUCTURES
Electron Dot Diagram
Lewis Dot Diagram
Structural Formula

26. Electron Dot Diagrams
Electron dot notation is a way of showing how many valence electrons an element has. H He Li Be B C N O F Ne

27. Lewis and Structural Lewis structures
Input Time
Lewis structures
Lone pairs are unshared electrons, which are not involved in chemical bonding. (Dotted Pairs)
Shared electrons are involved in chemical bonding. (Line)
Structural formulas
do not show dots for lone pairs of electrons. F F F F

28. How to Draw the Bonds F F F F
Step 1: Figure out how many more valence electrons each atom needs to make an octet (F needs 1). F F
Step 2: Make sure all elements in the molecule can have an octet. F
Step 3: Draw the Lewis structure. F
Step 4: Write the structural formula.

29. Hydrogen Fluoride (HF) Hydrogen Gas (H)2
Make sure all atoms have octets
(H only wants 2 valence electrons). H F H H F H
Lewis Structure H F H
Structural Formula

30. Methane (CH4) H H C H C H C H H

31. Nitrogen Trifluoride (NF3) Draw the Lewis Diagram and Structural Formula
Input Time

32. Nitrogen Trifluoride (NF3) Draw the Lewis Diagram and Structural Formula

33. Will these molecules form???
Input Time N H C F

34. mono- (use only for oxygen)
Input Time
Naming Compounds
Number of atoms
Prefix 1
mono- (use only for oxygen) 2
di- 3
tri- 4
tetra- 5
penta- 6
hexa- 7
hepta- 8
octa-
Examples
P2O5 - this is named diphosphorus pentoxide, because there are two phosphorus atoms and five oxygen atoms.   CO - this is carbon monoxide (you need the "mono-" because there's only one oxygen atom). CF4 - this is carbon tetrafluoride, because there's one carbon atom and four fluorine atoms.

35. WHICH IS BOND STRONGER?
Ionic bonds are a bit stronger than Covalent bonds but both are strong bonds

36. Strength of ionic compounds
Input Time
In an ionic compound the ionic bonds are spread evenly through the whole substance as a network so they are generally very strong with high melting points.
They tend to made solids compounds

37. Strength of covalent molecules
In a covalent molecule each molecule has strong covalent bonds inside it.
It has weaker attractions between the molecule.
Often simple molecular chemicals are gases and liquids.
Though the intermolecular bonds are weak the molecular bonds are strong
Input Time

38. Quiz
1. Draw the electron dot notation for Calcium (atomic number = 20).
Draw the Lewis structure for a molecule with 1 hydrogen atom and 1 chlorine atom, HCl (atomic numbers = 1, 17).
Book Exercises - Section 2.2 over to you questions, All of it!!!

39. Review and learn Table 1.3 page 9 of textbook

41. Naming Non-Metal Ions
Bromine
Chlorine
Iodide
Oxygen
Sulfide
Nitrate

42. Writing Formulas
Na20

43. Compound Ions
PO3
NO3
OH-