Chemical Bonding: PART 1 - IONIC

1. Chemical Bonding: PART 1 - IONIC You know you LOVE notes because they help you learn! 

2. Chemical Bond 8 Chemical bondingis the way atoms are attracted to each other to form compounds. Chemical bonding determines nearly all of the chemical properties we see in life. And as we know, the number “8” is very important to chemical bonding!

3. Bonding Basics • All atoms want to have a FULL outer energy level – just like the Noble Gases – because this means stability! • Atoms want 8 valence electrons (except H & He who want 2 because 2 electrons mean FULL)

4. Compound • a pure substance formed by two or more elements • Examples: • FeO2 – Rust • HCl – An acid found in your stomach • CH4 – A gas produced in your body (methane) • CO2 – Soda pop bubbles (carbon dioxide)

5. Compound • a pure substance formed by two or more elements • Examples: • NH3 – You’ll know this when you smell it (ammonia) • C12H22O11 – It will make your life sweeter (table sugar) • NaHCO3 – Something you’ll need to make good cakes and cookies (baking soda) • C8H10N4O2 – This will give you some pep! (caffeine)

6. Compound • a pure substance formed by two or more elements • Examples: • CO – A dangerous gas (carbon monoxide) • H2SO4 – Acid found in car batteries • CaCO3 – Used to write on a blackboard (calcium carbonate) • H2O2 – Used to disinfect wounds (hydrogen peroxide)

7. Valence Electrons • How many valence electrons? • What group number? • What family?

8. Valence Electrons • How many valence electrons? • What group number? • What family?

9. Valence Electrons • How many valence electrons? • What group number? • What family?

10. All in the Family… • Group 1: Alkali Metals • Group 2: Alkaline Earth Metals • Groups 3-12: Transition Metals • Group 13: Boron Group • Group 14: Carbon Group • Group 15: Nitrogen Group • Group 16: Oxygen Group • Group 17: Halogens • Group 18: Noble Gases

11. Electron Dot Diagrams… H Mg B C N O Cl Ne

12. Ionic Bonding • In an Ionic Bond, electrons are lost or gained in order to reach a FULL outer energy level which results in the formation of Ions

13. Positive Ions • METAL elements LOSE electrons to form positive ions: cations • It is easier to lose 1-2 electrons than gain 6-7 • Groups 1,2,13

14. Group 1

15. Group 2

16. Group 13

17. Negative Ions • NON-METAL elements GAIN electrons to become negative ions: anions • It is easier to gain 1-2 electrons than lose 6-7 • Groups 15,16,17

18. How to Ionic Bond… • Metal + Non-metal (Metal always listed first) • Opposite charges must balance • + and -charges hold ions together Na + Cl Na+ + Cl- NaCl

19. Opposites Attract!

20. Becoming Potassium Fluoride: K F

21. Becoming Potassium Fluoride: K F

22. Becoming Potassium Fluoride: K F

23. Becoming Potassium Fluoride: K F

24. Becoming Potassium Fluoride: • The ionic bond is the attraction between the ________ ion (K+) and the ________ ion (F-) K+ F_ POSITIVE NEGATIVE

25. Positive Ions

26. NEXT SLIDE ADVANCED STUDENTS ONLY

27. Electromagnetic Attraction • The + and – ions have an electromagnetic attraction (similar to static electricity).

28. Electron Dot Diagram for Positive Ions (EDD for + Ions) • Metals have few valence electrons Mg

29. Electron Dot Diagram for Positive Ions (EDD for + Ions) • Metals have few valence electrons • Electrons are given away Mg

30. Electron Dot Diagram for Positive Ions (EDD for + Ions) • Metals have few valence electrons • Electrons are given away • Positive Ions are formed Mg2+

31. Examples of Positive Ions : Li Li+ Group 1 Mg Al Mg+2 Group 2 Al+3 Group 13

32. Electron Dot Diagram for Negative Ions (EDD for - Ions) • Non-Metals have more valence electrons P

33. Electron Dot Diagram for Negative Ions (EDD for - Ions) • Non-Metals have more valence electrons • Electrons are gained to fill outer energy shell P P

34. Electron Dot Diagram for Negative Ions (EDD for - Ions) • Non-Metals have more valence electrons • Electrons are gained to fill outer energy shell P -3 • Negative Ions are formed

35. Examples of Negative Ions : N I N-3 Group 15 S S-2 Group 16 I- Group 17

36. What about group 18? They rarely bond because they are already happy and stable with 8 valence electrons! 

37. Putting Ions Together 1 to 1 ratios: Groups 1 & 17 (Alkali Metals & Halogens) NaCl Na+ + Cl-

38. Putting Ions Together 2.Groups 2 & 16 (Alkaline-Earth Metals & Oxygen Family) CaO Ca+2 + O-2

40. Putting Ions Together 2 to 1 ratios: Groups 1 & 16 (Alkali Metals & Oxygen Family) Na2O Groups 2 & 17 (Alkaline-Earth Metals & Halogens) Na+ + O-2 Ca+2 + Cl- CaCl2

42. Putting Ions Together LiBr Li+ + Br- Lithium + Bromine Lithium Bromide KCl K+ + Cl- Potassium + Chlorine Potassium Chloride Mg+2 + F- MgF2 Magnesium + Fluorine Magnesium Fluoride Al+3 + I- AlI3 Aluminum + IodineAluminum Iodide

43. Putting Ions Together NaCl Na+ + Cl- Sodium + Chlorine Sodium Chloride CaO Ca+2 + O-2 Calcium + Oxygen Calcium Oxide Ca+2 + Cl- CaCl2 Calcium + Chlorine Calcium Chloride Na+ + O-2 Na2O Sodium + Oxygen Sodium Oxide

44. Sodium + Fluorine Tin Fluoride Putting Ions Together Na+2 + F- SnF2

46. FINAL SLIDES ADVANCED STUDENTS ONLY

47. Electron Energy • The energy level relates to the amount of energy electrons have within the atom.

48. What are the characteristics of electrons closer to the nucleus?? Farther away?? How does that affect bonding??

50. Electron Energy