1. Chemical Bonding: PART 1 - IONIC
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2. Chemical
Bond 8
Chemical bonding is 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 Imagine 2 children playing together and sharing their toys
A force that keeps the children together is their mutual attraction to the toys they share.
In a similar fashion, two atoms can be held together by their mutual attraction for electrons they share
A chlorine atom for example has a strong attraction for one additional electron to fill its outermost shell

15. Group 2 Imagine 2 children playing together and sharing their toys
A force that keeps the children together is their mutual attraction to the toys they share.
In a similar fashion, two atoms can be held together by their mutual attraction for electrons they share
A chlorine atom for example has a strong attraction for one additional electron to fill its outermost shell

16. Group 13 Imagine 2 children playing together and sharing their toys
A force that keeps the children together is their mutual attraction to the toys they share.
In a similar fashion, two atoms can be held together by their mutual attraction for electrons they share
A chlorine atom for example has a strong attraction for one additional electron to fill its outermost shell

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. NaCl Na + Cl Na+ + Cl- 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. K+ F _ 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
Point out metals on periodic table Mg

29. Electron Dot Diagram for Positive Ions (EDD for + Ions)
Metals have few valence electrons
Electrons are given away Mg
Point out metals on periodic table

30. Electron Dot Diagram for Positive Ions (EDD for + Ions)
Metals have few valence electrons
Electrons are given away
Positive Ions are formed
Point out metals on periodic table
Mg2+

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

32. Electron Dot Diagram for Negative Ions (EDD for - Ions)
Non-Metals have more valence electrons
Point out metals on periodic table 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
Point out metals on periodic table 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
Point out metals on periodic table
Negative Ions are formed
P -3

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

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

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

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

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

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

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

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

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

51. Electrons FARTHEST from Nucleus Electrons CLOSEST to Nucleus
Electron Energy
Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus

52. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus

53. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS

54. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE

55. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons

56. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons
EASIER

57. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons
EASIER
HARDER

58. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons
EASIER
HARDER
Amount of electron energy available for bonding

59. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons
EASIER
HARDER
Amount of electron energy available for bonding

60. Electron Energy Electrons FARTHEST from Nucleus
Electrons CLOSEST to Nucleus
Pull on electrons by positive nucleus
LESS
MORE
Ability to remove electrons
EASIER
HARDER
Amount of electron energy available for bonding

61. BONDING REACTIVITY METALS NONMETALS
More reactive with MORE energy levels because WEAKER force pulling electrons into the nucleus
More reactive the LOWER the element is in the group
Group 1 MORE reactive than Group 2 because it is easier to remove 1 electron than 2
More reactive with FEWER energy levels because STRONGER force pulling electrons into the nucleus
More reactive the HIGHER the element is in the group
Group 17 MORE reactive than Group 16 because it is easier to gain 1 electron than 2

62. Electron Energy

64. Quote of the Day: “Equipped with his five senses, man explores the universe around him and calls the adventure Science.”  ~Edwin Powell Hubble, The Nature of Science, 1954

65. And Remember:

66. Name (first AND last) Date Period
Head Your Papers!
Name (first AND last) Date Period