1. Ionization

3. Atoms Vs. Ions
Atoms are neutral, they have the same amount of protons (+) and electrons (-)
# of electrons in the outer orbit of an atom determines how it will react
Ions are NOT neutral - they give or steal electrons
An ion is an electrically charged atom or group of atoms.
Ionization results in metals and non-metals forming Compounds.

4. Atoms Becoming Ions
Octet Rule: atoms always want to have a complete/full outer orbital of valence electrons - so they become ions!
Atoms want to
gain or lose elections to become more stable and less reactive
end up with a completely filled energy levels of electrons.

5. When Ionization occurs:
An anion is a negatively charged ion
formed when electrons are gained, giving more electrons in the remaining structure than protons
most anions form when non-metal atoms gain electrons.
non-metals are missing electrons so they accept electrons to become a negative ion
A cation is a positively charged ion
formed when electrons are lost, leaving more protons in the remaining structure than electrons
metals have extra electrons so they donate electrons they become a positive ion

6. The noble gases all have their outer level FULL!!
holds 2 electrons
holds 8 electrons
holds 8 electrons
The noble gases all have their outer level FULL!! *

7. Let’s take a look at chlorine
Since chlorine has 7 electrons in its’ outer shell, it can do one of two things: it can give up 7 electrons OR pick up 1 electron. Since it is much easier to gain 1 than lose 7, it grabs an electron from wherever it can. *

8. General Rule: All metals tend to lose electrons to become more stable.
All non-metals tend to gain electrons to become more stable.
Elements become more stable when they have the same number of electrons in their outer energy level as the nearest noble gas does.

9. Lithium has 3 electrons has 1 extra electron in the outer orbital
will give away 1 e
as an ion

10. Magnesium has 12 electrons has 2 extra electron in the outer orbital
will give away 2 e
as an ion

11. Sulfur has 16 electrons is missing 2 electrons in the outer orbital
will steal 2 e
as an ion

12. Flourine has 9 electrons is missing 1 electron in the outer orbital
will steal 1 e
as an ion

13. Argon
has 18 electrons
all orbitals are complete so Argon does not react
Argon does not make an ion Ar

14. Electrons in Last Orbital
Ions
Column
Electrons in Last Orbital
Gain/Loose Electrons
Ion Charge
Example
I-A 1
Lose 1 +1
K +
II-A 2
Lose 2 +2
Ca 2+
III-A 3
Lose 3 +3
Al 3+
IV-A 4
Gain/Lose 4
-/+4 C
V-A 5
Gain 3 -3
P 3-
VI-A 6
Gain 2 -2
S 2-
VII-A 7
Gain 1 -1
Br -
VIII-A 8
Balanced Ne

16. What is an isotope?
12 = Mass number
Isotopes are elements with the same number of protons but different number of neutrons.
Carbon-12
Carbon-14
Carbon-16
14 = Mass number
16 = Mass number
For Carbon – 14:
14 = # of protons + # of neutrons =
For Carbon – 12:
12 = MASS NUMBER (# of p+ + # of no)
12 = # of protons + # of neutrons =
For Carbon – 16:
16 = # of protons + # of neutrons =

17. Naming: name - mass number Example: carbon-12
Element symbol
Naming: name - mass number
Example: carbon-12

18. Practice: Do the Isotopes and Ions worksheet

19. Extra Stuff

20. Ionization
When an atom gains or loses one or more of their outermost electrons and results in the formation of an ion.
Give away extra electrons
metals have extra electrons so they donate electrons they become a positive ion
Steal electrons
non-metals are missing electrons so they accept electrons to become a negative ion

21. Octet Rule
Chemist Gilbert Lewis summarized the behaviour of the elements on the periodic table, saying they react to have 8 electrons in their outer (or valence) energy level. This is called the octet rule.
Every element wants to be just like a noble gas with a full outer energy levels of valence electrons. *