2. The story of bonding is really the story of atoms and their eternal search for happiness
Lithium
Fluorine

3. = chemically unstable
= higher energy state
3 p+
9 p+
Lithium
Fluorine

4. Bonding Basics (review)
Valence electrons – Outermost s and p orbital electrons
(the electrons that interact, for the most part, with other atoms)
3 p+
9 p+
Lithium
Fluorine
1s2 2s1
1s2 2s2 2p5
1 valence electron
7 valence electrons

5. Bonding Basics (review)
Valence electrons – Outermost s and p orbital electrons
(the electrons that interact, for the most part, with other atoms)
3 p+
9 p+
Lithium
Fluorine
1s2 2s1
1s2 2s2 2p5
Valence electrons are those found in the outermost s and p orbitals of an atom
1 valence electron
7 valence electrons

6. Practice: Write the e- configurations for the following elements and identify which are the valence e-’s.
Sodium
Chlorine
Strontium
Selenium

7. Li Bonding Basics (review) Lithium 1s2 2s1
Valence electrons - Outermost s and p orbital electrons
(the electrons that interact, for the most part, with other atoms)
Electron Dot Diagrams
A way of representing an atom – shows only the valence e-
3 p+ Li
Lithium
1s2 2s1

8. F Li Bonding Basics (review) Fluorine 1s2 2s2 2p5
Valence electrons - Outermost s and p orbital electrons
(the electrons that interact, for the most part, with other atoms)
Electron Dot Diagrams
A way of representing an atom – shows only the valence e-
9 p+ F Li
Fluorine
1s2 2s2 2p5

9. Practice: Write the e- dot diagrams for the following elements.
Sodium and potassium
Calcium and strontium
Boron and aluminum
Silicon and germanium
Phosphorus and arsenic
Oxygen and sulfur
Bromine and Iodine
Neon and Krypton

10. Bonding Basics (review)
Valence electrons - Outermost s and p orbital electrons
(the electrons that interact, for the most part, with other atoms)
Electron Dot Diagrams
A way of representing an atom – shows only the valence e-
Octet Rule
Most atoms bond in order to have a noble gas configuration AKA full s and p orbitals AKA 8 electrons in their outermost shell

11. Bonding Basics (review)
Li now has an e- configuration of 1s2, which is that of He!
Lithium
3 p+
1s2 2s1
(a noble gas)
Octet Rule
Most atoms bond in order to have a noble gas configuration AKA full s and p orbitals AKA 8 electrons in their outermost shell

12. Bonding Basics (review)
9 p+
F now has an e- configuration of 1s22s22p6, which is that of Ne!
Fluorine
1s2 2s2 2p5
(a noble gas)
Octet Rule
Most atoms bond in order to have a noble gas configuration AKA full s and p orbitals AKA 8 electrons in their outermost shell

13. Practice: Use electron configurations to determine how the following atoms might lose or gain electrons in order to satisfy the octet rule. Identify the noble gas that each attains the e- configuration of.
Calcium, Lithium, Chlorine and Aluminum

14. Bonding Basics (review)
Valence electrons - Outermost s and p orbital electrons
A full shell of paired electrons (like the noble gases) is the low energy state that all atoms are trying to attain.
(the electrons that interact, for the most part, with other atoms)
Electron Dot Diagrams
A way of representing an atom – shows only the valence e-
Octet Rule
Most atoms bond in order to have a noble gas configuration AKA full s and p orbitals AKA 8 electrons in their outermost shell

15. Bonding Basics (review)
Wrap-up:
Is a sulfur atom chemically stable? Verify your answer with an electron configuration AND an electron dot diagram.
Propose a way that sulfur could satisfy the octet rule. What element is it imitating in this process?
Does satisfying the “octet rule” always mean 8 valence electrons? Which atom(s) satisfy the octet rule without having 8 valence electrons?
Why are the noble gases the only elements that exist in nature as lone elements (not bonded to other atoms)?