1. Bohr Models…
Niels Bohr explained the structure of the atom in his “Bohr models”. His model of the atom resembles a solar system. He came up with this model in Here is a typical Bohr model, what can you figure out from it

2. Bohr models show the nucleus in the center with the # of Protons (p) and Neutrons (n) in it
Around the nucleus, it shows
the electrons in orbits or shells
Each orbit/shell can only hold a
certain # of electrons and then
it is full.

3. How many e- can each orbit hold?
1st orbit can hold 2 e-
2nd orbit can hold 8 e-
3rd orbit can hold 8 e-
4th orbit can hold 18 e-
You don’t need to know any higher orbits – we won’t be covering higher elements.
You can depict any element in a Bohr model!

4. Some Bohr models…
Beryllium
4 p+ 5n 4e-
Oxygen
8p+ 8n 8e-
Aluminum

5. So how do we draw a Bohr model of… say…Sodium?
Start with a nucleus, and put in how many protons and neutrons are in sodium (look at your periodic table)
Next place some orbits around it
P: 11
N:12
P: 11
N:12

6. Next figure out how many e- are in sodium (look at your periodic table). Place them in dots in the orbits
Remember!!
2 max in 1st orbit
8 max in 2nd orbit
8 max in 3rd orbit 18 max in 4th orbit
Sodium has 11 electrons !!
they are the same as the protons
P: 11
N:12

7. The outermost electrons – the ones in the last shell/orbit are called valence electrons
Valence e- are important because when atoms react, it is the valence e- that do all the moving !!
P: 11
N:12
* Think valence penguins

8. How many Valence e- in these Bohr models??
2 ve-
6 ve-
3 ve-

9. What about Bohr models of Molecules?
Eg. What is this compound?
1p+ 0n
8 p+
8 n
1p+ 0n

10. Can you answer these questions…
Can you draw the Bohr model of H2?
Why would 2 Hydrogens be happy to bond together?
1p+ 0n
1p+ 0n

11. Valence e- what do we know…
Which group on the periodic table, do you notice, always has all it’s valence electron shell full?
 The Noble Gases. This is very significant… Why??
Because every element wants to have a full outer shell of valence e- – because then it is completely stable and never has to react. Every element wants to be a noble gas

12. End Bohr Notes Enter Ionic and Covalent bonds

13. Lewis Dot Diagrams…
Bohr had one way of depicting the atom and it’s sub atomic particles (p+, n, and e-). But another man, Gilbert Lewis used a different model, and he only showed the valence e- in it. His model is called the Lewis dot diagram He put dots around the symbols so that we can see the valence electrons for the elements (we can easily see which e- are going to react)

14. Lewis dot structure

15. The red dots show you the valence electrons in each element’s atoms

16. Lewis Dot Structures

17. 8 is the # we want – it’s stable – like a noble gas
Lewis Dot Structures
Lewis dot structures are really simple – they are just the valence e- represented as dots around an element. 2 electrons can be shown as 2 dots or by 1 line. 2 electrons together is called a lone pair. Pd
The # of valence e- is … 8
8 is the # we want – it’s stable – like a noble gas

18. How to draw …

19. Try some now…
Remember, up to 4 e-, you put separately on each side of the symbol, once you get to 5, you have to start pairing up.
1) Magnesium 2) Nitrogen
3) Flourine 4) Argon
Bonding pair N Mg F Ar

20. So what happens when atoms meet?
When 2 atoms move close together, their valence electrons interact, and they form a chemical bond between them if they are a good pair (more stable together than apart)
Having a full valence shell is what each element wants! So it will bind with other elements that make that happen!

21. Lewis Diagrams of ions
Lewis diagrams make drawing ions, and ionic bonds much less work than Bohr diagrams.
For positive ions, one electron dot is removed from the valence shell for each positive charge of the ion.
For negative ions, one electron dot is added to each valence shell for each negative charge of the ion.
Square brackets are placed around each ion to indicate transfer of electrons – 2+ –
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• • Be Cl Cl Be Cl Cl Be Cl
Each beryllium has two electrons to transfer away, and each chlorine wants one more electron
Since Be2+ wants to donate 2 electrons and each Cl– wants to accept only one, two Cl– ions are necessary
Beryllium chloride
See page 179
(c) McGraw Hill Ryerson 200

22. Lewis Diagrams of covalent bonds
Lewis diagrams of covalent bonds are also very easy.
Like Bohr diagrams, valence electrons are drawn to show sharing of electrons.
All atoms wish to have a full valence shell
The shared pairs of electrons are usually drawn as a straight line
See page 179
(c) McGraw Hill Ryerson 2007

23. Lewis Diagrams of diatomic molecules
Diatomic molecules, like O2, are also easy to draw in Lewis form
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• • O O O O O O
Several non-metals join to form diatomic molecules
Valence electrons are shared, here in two pairs!
This is drawn as a double bond
See page 180
Take the Section 4.1 Quiz
(c) McGraw Hill Ryerson 2007