1. Bonding & the Periodic Table

2. Valence Electrons and Bonding
- Atoms, Bonding, and the Periodic Table
Valence Electrons and Bonding
The number of valence electrons in an atom of an element determines many properties of that element, including the ways in which the atom can bond with other atoms & it determines the way it reacts

3. Fundamental Rule All atoms want to look like the noble gasses
So they either want to get rid of all of their valence electrons, or accept more electrons.

4. Electron Configuration
Group I
Electron Configuration
Group VIII
Group II
Period 1
Group III
Group IV
Group V
Group VI
Group VII 1 2 H He 3 4 5 6 7 8 9 10
Period 2 LI Be B C N O F Ne 11 12 13 14 15 16 17 18
Period 3
Alkaline (1)
(Very Reactive)
Noble Gasses (8)
(Not Reactive)
Alkali Earth (2)
(Reactive)
Boron Family (3) Na
Carbon Family (4) Mg
Nitrogen Family (5) Al
Oxygen Family (6)
(Reactive) Si
Halogens (7)
(Very Reactive) P S Cl Ar
Notice the valence electrons. Each one wants outer shell filled. Group 1 wants to get rid of their electrons – Group 7 wants to keep it. Group 8 keeps all and never shares.
© Beadle, 2009

5. Electron Configuration
Group I
Electron Configuration
Group VIII
Group II
Period 1
Group III
Group IV
Group V
Group VI
Group VII 1 2 H He 3 4 5 6 7 8 9 10
Period 2 LI Be B C N O F Ne 11 12 13 14 15 16 17 18
Period 3
Alkaline (1)
(Very Reactive)
Noble Gasses (8)
(Not Reactive)
Alkali Earth (2)
(Reactive)
Boron Family (3) Na
Carbon Family (4) Mg
Nitrogen Family (5) Al
Oxygen Family (6)
(Reactive) Si
Halogens (7)
(Very Reactive) P S Cl Ar
Point out the valence electrons. Each one wants outer shell filled. This is what causes a reaction. Also note the empty spaces – how every atom wants 8 (filled)
© Beadle, 2009

6. - - - - - - - - - - - - - - - - - - - Metals v. Non Metals 17p+ 11p+
Becomes Positive (+)
Becomes Negative (-) - - - -
11p+ - - - - -
17p+ - - - - - - - - - -
Sodium Na (11): Metal
Gets rid of Electrons
Chlorine (17): Non Metal
Accepts Electrons
11 P & 10 E- = +1
17 P & 18 E- = -1
© Beadle, 2009

7. Metals+ Get Rid of Electrons
Non-Metals-
Accept Electrons
– Gain or Accept e-
Metalloids
Metals+
Get Rid of Electrons

8. Chemical Bonds Cause Chemical Reactions
Ionic
Metal + Non-Metal
Co-valent
Non-Metal + Non-Metal
Metallic
Metal + Metal

9. - Ionic Bonds
Ions and Ionic Bonds
When an atom loses an electron, it loses a negative charge and become a positive ion. When an atom gains an electron, it gains a negative charge and becomes a negative ion.

10. - - - Ionic Bonding M+NM 17p+ 11p+ Becomes Positive (+)
Becomes Negative (-) -
17p+ - -
11p+
Sodium Na (11): Metal
Gets rid of Electrons
Chlorine (17): Non Metal
Accepts Electrons
11p e- = +1
17p e- = -1
© Beadle, 2009

11. - - - - - - - - - - - - - - - - - - - Ionic Bonding M+NM 17p+ 11p+
Becomes Positive (+)
Becomes Negative (-) - -
(-) - - -
11p+
(+) - - - -
17p+ - - - - - - - - - -
Sodium Na (11): Metal
Gets rid of Electrons
Chlorine (17): Non Metal
Accepts Electrons
11p e- = +1
17p e- = -1
© Beadle, 2009

12. Example: Salt Crystal

13. Properties of Ionic Compounds
- Ionic Bonds
Properties of Ionic Compounds
In general, ionic compounds are
hard,
brittle crystals,
high melting points,
conduct electricity
when dissolved/melted

14. Covalent Bonding NM + NM- - - - - -
8p+
8p+ - - - - - -
Oxygen (8)
Oxygen (8) O2
© Beadle, 2009

15. Covalent Bond Examples
Ethyl Alcohol
Methane
Sugar

16. Properties of Covalent Bonds
Covalently Bonded Molecules:
Usually liquid/gas at room temp.
Sometimes you may find it in crystal form
Have low melting/boiling points
Have low viscosity
Have low density
Do not conduct electricity when dissolved.

17. - - Metallic Bonding M + M 11p+ 11p+ (-) (-) (+) (+)
- Bonding in Metals
Metallic Bonding M + M
A metal crystal consists of positively charged metal ions embedded in a “sea” of valence electrons.
(-)
(-) - -
(+)
(+)
11p+
11p+
© Beadle, 2009

18. Properties of Metals
The “sea of electrons” model of solid metals explains their ability to conduct heat and electricity…

19. Properties of Metals
The “sea of electrons” model of solid metals explains their ease with which they can be made to change shape…

20. Properties of Metals
Luster
Gold in an astronaut’s face shield reflects sunlight, protecting the wearer’s eyes.
The “sea of electrons” model of solid metals explains their luster.

21. Chemical Reactions
Chemical Reactions happen because of bonding.

22. Chemical Change (Reaction)
Chemical reactions occur when old bonds break and new bonds form.

23. Chemical Change (Reaction)
Chemical reactions involve two main kinds of changes that you can observe –
formation of new substances and
changes in energy.