Ions

1. Ions

2. Changing An Atom Changing an Atom

3. Review: Representing atoms with the Bohr model

4. Representing atoms with the Bohr Model

5. Bohr Model – Simplified but Useful Model P1 P2 P3

6. Bohr Model & the Periodic Table Making Conclusions Compare and Contrast • Why are elements placed in a group (column)? • Why are elements placed in a period (row?)

7. Representing atoms with the Bohr Model

8. Ions • How are ions made? • Ions are: • The valence electron(s): • Metals _________ valence electrons to become a (positive or negative) ion, called a ____________. • Non-metals __________ valence electrons to become a (positive or negative) ion, called an ___________. • The Octet Rules: atoms tend to lose or gain valence electrons in order to have a stable number of __________(hint: what number?)

9. Ions Calcium atom - Calcium ionIon Symbol p+ p+ nº nº e- e- Oxygen atom Oxygen ion Ion Symbol p+ p+ nº nº e- e-

10. How many valence electrons does each of the main group (Representative: Groups 1 & 2, 13-18) elements have ? What is the charge?

11. When forming a stable ion: • Calcium atom will gain/lose this # of e⁻s____ • Phosphorus atom will gain/lose this # of e⁻s____ • Lithium atom will gain/lose this # of e⁻s____ • Aluminum atom will gain/lose this # of e⁻s____ • Sulfur atom will gain/lose this # of e⁻s____ • Chlorine atom will gain/lose this # of e⁻s____ • Sodium atom will gain/lose this # of e⁻s____ • Oxygen atom will gain/lose this # of e⁻s____

12. Ions • Atoms can lose or gain electrons when bonding to make ionic compounds • We keep track of the number of electrons that can be lost or gained with ____________(also known as _____________) • Ions are ____________–when an atom has too many or too few electrons to be neutral • No change to the nucleus • Proton and neutrons ___________________________.

13. Why are ions important? The ___________________ charged particles are like a magnet. Therefore, they are strongly held together in an ______________ _____________ forming an _____ ________________.

14. Forming Ionic CompoundsCharges of the total compound =0 • Formula Name • Li ⁺¹ and F ⁻¹ = • Ca⁺² and F⁻¹= • Name: • Ca⁺² and O⁻² = • Name • Li⁺¹ and O⁻²= • Name:

15. Ions and ChargeNet electric charge Note change 8

16. Ions and Charges for Representative Elements (Oxidation number keep track of electrons)

17. Ion Making Holy Molee Song

18. Making an ion of an alkali metal, First column in the periodic chart, Leaves all the ions with a plus one charge And they’re all a whole lot smaller than they were before.

19. Second column over, Alkaline earths, Loses 2 electrons easily, So their ions all have a plus 2 charge, And they’re smaller than their neighbors to the left.

21. Next door, aluminum, the 3rd step over has 3 electrons It’d like to have removed. When they are gone, it has a +3 charge, And, by gosh!, It’s even smaller than the “lefter” two.

22. But add one electron To the halogen group, So they all have a Negative one charge. They get 8x bigger than They were before. Puffed up, very large.

24. Sulfur and oxygen need 2 electrons to give each a full and complete electron shell. Thus, minus 2 is their ionic charge. And they’re a little larger Than the “Hal-ions”.

25. Add three electrons to the nitrogen group. So that group has a triple minus charge. And the pattern we see makes it very clear. Negative ions are large!

27. Review Ions Lithium atom - Lithium ion Ion Symbol p+ p+ nº nº e- e- Fluorine atomFluorine ion p+ p+ nº nº e- e-

28. Ions and ChargeNet electric charge Note change 8

29. Ions and Charges for Representative Elements (Oxidation number keep track of electrons)