1. E.L. To revise ionic bonding and learn about covalent bonding
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2. The name’s BOND … … ionic Bond! 14/05/2018
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3. To understand how bonds are formed between metals and non-metals
Whats your target grade?
Success criteria:
Learning objective:
To understand how bonds are formed between metals and non-metals
Describe how ionic compounds are formed from metals and non-metals
Explain and work out the charge on an ion
Predict the formula of an ionic compound C
Good B
Great
Even
better
if… A
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4. video clip
CONNECT
Watch the clip of sodium reacting with chlorine. What is the product?

5. What happens when they react?
SODIUM + CHLORINE  SODIUM CHLORIDE
Sodium
Chlorine

6. Atoms can be joined together in 3 possible ways:
Bonding
Ionic
Covalent
Metallic
Metal
Non
metal
The bond is the chemical ‘glue’ that holds the atoms together
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7. Fluorine Oxygen Beryllium Sodium Chlorine Magnesium Metal Non-Metal
Lithium
Have students hold green, pink and blue cards in their hands. They hold the appropriate one up when the word comes up onto the screen. Just click once on this slide, then the rest is timed.
Quick Quiz
What do you already know???

8. why do atoms bond? Atoms bond to get full ‘outer’ shells of electrons
(usually 8)
…. because that makes them happy!!!

9. Here comes my friend, Sophie SodiumCl
Hi. My name’s Colin Chlorine. I’m in Group 7, so I have 7 electrons in my outer shell
Here comes my friend, Sophie Sodium Na
Hey Colin. I’m in Group 1 so I have one electron in my outer shell. This electron is far away from the nucleus so I’m quite happy to get rid of it. Do you want it?
Okay + - Na Cl
Now we’ve both got full outer shells and we’ve both gained a charge. We’ve formed an IONIC bond.

10. how do atoms form ions? +
Sodium Na Na -
Chlorine Cl Cl

11. WHAT IS AN IONIC BOND? metal Non-metal
The force of attraction between the positively charged ion and negatively charged ion.
One element is a metal, the other is a non-metal.
metal
Non-metal

12. DRAWING IONS
Apply what you have just learnt about sodium chloride to another ionic compound, Magnesium Oxide
Magnesium has 2 electrons in its outer shell
Group 2 elements lose 2 electrons (Magnesium)
Oxygen has 6 electrons in its outer shell
Group 6 elements gain 2 electrons (Oxygen)
EXTENSION TASK: If you finish, try to draw another ionic compound, Sodium Oxide (It’s a bit tricky!)

13. Mg Mg O O how do atoms form ions? 2- 2+ Oxygen Magnesium
VERY COMMON EXAM QUESTION!
how do atoms form ions? 2+
Magnesium Mg Mg
Oxygen O O 2-

14. how do atoms form ions?
MORE TRICKY! + Na Na O O 2-

15. How do these drawings help us write a formula?
Each Ionic compound is made from a metal and a non-metal.
The number of each atom depends on the ratio of each atom needed in the bonding diagram.
Sodium Na
Chlorine Cl
NaCl
Magnesium Mg
MgCl2
chloride Cl
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16. Ionic bonds form between non-metals and m………………..
Atoms can obtain completely full outer electron shells by l…………………. or g………………….…. electrons when they react with other atoms. When this happens, atoms form i………..……..
An ionic bond is formed by the force of a………………….…
between a c……………………………... and an a…………………
Ionic bonds form between non-metals and m………………..
Millions of c…….... and a…….…. join together by ionic bonding to form a 3D l…………… structure.
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17. 1. Fill in the cards with the dot cross diagrams to show the electron shell populations and write the electronic configurations in the boxes (as shown in the examples above)
2. Cut out the cards.
3. What ionic compounds can you make using the cards (there are five possibilities)
If you finish early ask for an additional pair of card sheets where you can choose your own ions to create. This will increase your newly acquired skill even further.

18. Ionic bonding conclusion
Ionic bonding involves electrons being transferred (“given up” or “stolen away”)
This type of “tug of war” between a METAL and NONMETAL is called an IONIC BOND, which results in a SALT being formed

19. The unspoken hero: “Covalent Bond”
Covalent Bonding
The unspoken hero: “Covalent Bond” 
Covalent Bonding section edited from the powerpoint by Mr. Samaniego: Lawndale High School, Somewhere

20. Molecular Compounds
Now you will learn about another type of bond in which electrons are shared
Covalent Bonds are atoms held together by SHARING electrons between NONMETALS

21. Salt versus Molecules
A metal cation and nonmetal anion are joined together by an ionic bond called SALT
A group of atoms joined together by a covalent bond is called a MOLECULE
A Compound is a group of two or more elements bonded together (Ionic or Covalent).

22. Monatomic vs. Diatomic Molecules
Most molecules can be monatomic or diatomic
Diatomic Molecule is a molecule consisting of two atoms
There are 7 diatomic molecules (SUPER 7) – N2, O2, F2, Cl2, Br2, I2, H2
You can also remember them as: H2O2F2Br2I2N2Cl2

23. Properties of Molecular Compounds
Liquids or gases at room temperature
Lower Melting Points than Ionic Compounds (which means that they are weaker than ionic)

24. Molecular Formulas
The Molecular Formula is the formula of a molecular compound
It shows how many atoms of each element a molecule contains
Example
H2O contains 3 atoms (2 atoms of H, 1 atom of O)
C2H6 contains 8 atoms (2 atoms of C, 6 atoms of H)

25. Practice
How many atoms total and of each do the following molecular compounds contain? H2 CO
CO2
NH3
C2H6O

26. Practice: True or False
All molecular compounds are composed of atoms of two or more elements.
All compounds are molecules.
Molecular compounds are composed of two or more nonmetals.
Atoms in molecular compounds exchange electrons.
Molecular compounds have higher melting and boiling points than ionic compounds.
TRUE
FALSE
TRUE
FALSE
FALSE

28. Ionic versus Covalent (copy into your books)
Bonded Name
Salt
Molecule
Bonding Type
Transfer e-
Share e-
Types of Elements
Metal & Nonmetal
Nonmetals
Physical State
Solid
Solid, Liquid, or Gas
Melting Point
High (above 300ºC)
Low (below 300 ºC)
Solubility
Dissolves in Water
Varies
Conductivity
Good
Poor

29. Covalent Bonding
Remember that ionic compounds transfer electrons in order to attain a noble gas electron configuration
Covalent compounds form by sharing electrons to attain a noble gas electron configuration
Regardless of the type of bond, the Octet Rule still must be obeyed (8 valence electrons)

30. Single Covalent Bond
A Single Covalent Bond consists of two atoms held together by sharing 1 pair of electrons (2 e-)

31. Electron Dot Structure

32. Shared versus Unshared Electrons
A Shared Pair is a pair of valence electrons that is shared between atoms
An Unshared Pair is a pair of valence electrons that is not shared between atoms

33. Practice Lewis Dot Structures
Chemical Formula
# of Valence Electrons
Single Line Bond Structure
# of Remaining Electrons
Lewis Dot Structure
Octet Check All Atoms=8
Hydrogen=2 F2
H2O
NH3
CH4

34. Double Covalent Bonds
Sometimes atoms attain noble gas configuration by sharing 2 or 3 pairs of electrons
A Double Covalent Bond is a bond that involves 2 shared pairs of electrons (4 e-)

35. Triple Covalent Bond
A Triple Covalent Bond is a bond that involves 3 shared pairs of electrons (6 e-)

36. Covalent Bonds

37. Practice Lewis Dot Structure
Chemical Formula
# of Valence Electrons
Single Line Bond Structure
# of Remaining Electrons
Lewis Dot Structure
Octet Check All Atoms=8
Hydrogen=2 O2
CO2 N2
HCN