1. Unit 4: Chemical Bonds

2. Vocabulary Electron configuration Crystal lattice Molecule
Electron dot diagram
Covalent bond
Polarity
Electron transfer
Binary compound
Valence electron
Chemical formula
Ionic bond
Extrapolate
Cation
Oxidation
Anion
Polyatomic ion
**Cannot be printed directly from Quizlet

3. Purpose: Understand the meaning of a stable electron configuration & represent atoms using electron dot diagrams.
Purpose on top of ISN 90.
Notes/Practice on ISN 91. (Lewis Structure Handout)
Homework on ISN 90:
Write your own step-by-step rules for making an e- dot diagram.
WKBK 93 Create

5. Lewis Structures (Electron Dot Diagrams)
Find your element on the periodic table.
Determine the number of valence electrons.
This is how many electrons you will draw.

6. Lewis Structures Find out which group (column) your element is in.
This will tell you the number of valence electrons your element has.
You will only draw the valence electrons.

7. Groups - Review Group 8 = 8 electrons Group 1 = 1 electron
Except for He, it has 2 electrons
Group 2 = 2 electrons
Each column is called a “group”
3, 4, 5, 6, 7
Each element in a group has the same number of electrons in their outer orbital, also known as “shells”.
The electrons in the outer shell are called “valence electrons”

8. C Lewis Structures Write the element symbol.
Carbon is in the 4th group, so it has 4 valence electrons.
Starting at the right, draw 4 electrons, or dots, counter-clockwise around the element symbol. C

9. C Lewis Structures Check your work.
Using your periodic table, check that Carbon is in the 4th group.
You should have 4 total electrons, or dots, drawn in for Carbon. C

10. C Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al C

11. H Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al H

12. P Lewis Structures On your worksheet, try these elements on your own:Ca Ar Cl Al P

13. Ca Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al Ca

14. Ar Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al Ar

15. Cl Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al Cl

16. Al Lewis Structures On your worksheet, try these elements on your own:P Ca Ar Cl Al Al

17. Notes/Practice on ISN 93. Ionic or Covalent Bond handout.
Purpose: Understand how atoms obtain a stable electron configuration by transferring or sharing electrons & differentiate molecules based on the type of bonds within.
Purpose on top of ISN 92.
Notes/Practice on ISN 93. Ionic or Covalent Bond handout.
Homework on ISN 92:
Write your own rule for determining whether an element grouping will have an ionic bond or a covalent bond.
WKBK 123 Determine

18. H2O Chemical Formula 1 oxygen atom 2 hydrogen atoms Shows:
1) elements in the compound
2) ratio of their atoms
H2O
1 oxygen atom
2 hydrogen atoms

19. Strong attractive force between atoms or ions in a molecule or compound.
Formed by:
transferring e- (losing or gaining)
sharing e-

20. Ne Octet Rule most atoms form bonds in order to have 8 valence e-
full outer energy level
like the Noble Gases! Ne
Stability is the driving force behind bond formation!

21. Transferring e-
Sharing e-

22. Comparison Chart IONIC COVALENT transferred from metal to nonmetal
shared between nonmetals
Electrons
Melting
Point
high
low
Soluble in
Water
yes
usually not
yes (solution or liquid)
Conduct Electricity no
crystal lattice of ions, crystalline solids
molecules, odorous liquids & gases
Other
Properties

23. Pop Quiz Show the Lewis structure for the following elements: Mg O ArAl
What type of bond is formed between the following compound/molecules?
NaF
SO3 KI
FeCl3
H2O

24. Purpose: Explore the transfer of electrons & characteristics of ionic bonding & ionic structure.
Purpose on top of ISN 94.
Notes/Practice on ISN 95.
Homework on ISN 94:
WKBK 98 all
Write your own rules for remembering the difference between cation and anion.

25. Attraction between 2 oppositely charged ions
Ions - charged atoms
formed by transferring e- from a metal to a nonmetal

26. Cation- positive charge because of lost electron(s)
Anion- negatively charged ion because of gained electron(s)

27. ions form a 3-D crystal lattice
NaCl

28. Purpose: Understand how electrons are shared by exploring the formation of covalent bonds & the characteristics of covalent bonds & molecules.
Covalent Bonding Activity:
Write the symbols for each element.
Use beans to create the Lewis structures for each. Each type of atom has a different color.
Rearrange the electrons (beans) to show the sharing of electrons.
Draw circles to show the sharing of electrons.
Draw the bond structure using symbols & lines. Use 1 line for each pair of electrons that is shared.
Write the chemical formula for each molecule.
Use a colored pencil to draw where the bean was when you remove it.
Purpose on top of ISN 96
Notes/Practice on ISN 97. Write Activity instructions here also.
Homework on ISN 96: Write a short (2-3 sentence) summary of what you learned from the activity.
Covalent Bonding video

29. Attraction between neutral atoms
formed by sharing e- between two nonmetals
Covalent Bonding Animation

30. covalent bonds result in discrete molecules
NH3
H2O
Cl2

31. Beans & Covalent Bonds Activity
These molecules will be done on ISN 80. Make sure you leave plenty of room between each molecule.
Hydrogen + Hydrogen
Hydrogen + Oxygen
Chlorine + Chlorine
Oxygen + Oxygen
Carbon + Oxygen
Carbon + Hydrogen

32. Purpose: Explore the nature of covalent bonds by examining the polarity & non-polarity of simple covalent compounds.
Purpose on top of ISN 98
Notes/Practice on ISN 99. Draw the pictures of the types of bonds.
Homework on ISN 98: WKBK 109 all & top of 110.

33. Nonpolar Covalent Bond
e- are shared equally
usually identical atoms

34. + - Polar Covalent Bond
e- are shared unequally between 2 different atoms
results in partial opposite charges + -

35. Nonpolar
Polar
Ionic
View Bonding Animations.

36. Purpose: Name simple binary covalent compounds by looking at the chemical formula. Purpose: Name binary covalent compounds & write their formula using prefixes.
Purpose on top of ISN 100.
Notes/Practice on ISN 101.
Homework on ISN 100: WKBK p. 112 all & p. 113 Write

37. Naming Binary Compounds
Yes
Metal Present? No
Yes
Type III
Use Greek
Prefixes
Does the metal form
more than one cation? No
Yes
Type II
Determine the charge
of the cation; use a Roman
numeral after the cation
name.
Type I
Use the element
name for the cation.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98

38. A. Molecular Names Write the names of both elements.
Change the final ending to -ide.
Add prefixes to indicate subscripts.
Only use mono- prefix with oxide.

39. Prefixes – Binary Molecular Compounds
Greek Prefixes for Two Nonmetals
Number Indicated Prefixes
1 mono-
2 di-
3 tri-
4 tetra-
5 penta-
6 hexa-
7 hepta-
8 octa-
9 nona-
10 deca-

40. A. Molecular Names CCl4 N2O carbon tetrachloride SF6
dinitrogen monoxide
sulfur hexafluoride

41. B. Molecular Formulas Write the more metallic element first.
Add subscripts according to prefixes.

42. B. Molecular Formulas phosphorus trichloride dinitrogen pentoxide PCl3
dihydrogen monoxide
PCl3
N2O5
H2O

43. Binary Molecular Compounds
N2O dinitrogen monoxide
N2O dinitrogen trioxide
N2O dinitrogen pentoxide
ICl iodine monochloride
ICl iodine trichloride
SO sulfur dioxide
SO sulfur trioxide
Technical Note: Iodine trichloride is actually a dimer with the formula I2Cl6

44. B. Molecular Formulas The Seven Diatomic Elements
Br2 I2 N2 Cl2 H2 O2 F2

45. Binary Compounds Containing Two Nonmetals (Type III Compounds)
As2S3
________________ diarsenic trisulfide
________________ sulfur dioxide
P2O5 ____________________
________________ carbon dioxide
N2O5 ____________________
H2O ____________________
SO2
diphosphorus pentoxide
CO2
dinitrogen pentoxide
dihydrogen monoxide

46. Purpose: Name simple binary ionic compounds by looking at the chemical formula. Purpose: Extrapolate the chemical formula of binary ionic compounds from the names by using the oxidation states of the ions.
Purpose on top of ISN 102.
Notes/Practice on ISN 103.
Homework on ISN 102:
Worksheet

47. Naming Binary Compounds
Yes
Metal Present? No
Yes
Type III
Use Greek
Prefixes
Does the metal form
more than one cation? No
Yes
Type II
Determine the charge
of the cation; use a Roman
numeral after the cation
name.
Type I
Use the element
name for the cation.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98

48. A. Oxidation Number The charge on an ion.
Indicates the # of e- gained/lost to become stable. 1+ 2+ 3+ 4+ 3- 2- 1-

49. B. Ionic Names
Write the names of both elements, cation first.
Change the anion’s ending to -ide.

50. B. Ionic Names NaBr CaO sodium bromide BaCl2 Calcium oxide
barium chloride

51. C. Ionic Formulas Write each ion. Put the cation first.
Overall charge must equal zero.
If charges cancel, just write the symbols.
If not, crisscross the charges to find subscripts.

52. C. Ionic Formulas potassium chloride magnesium nitride K+ Cl-  KCl
copper(II) chloride
K+ Cl-  KCl
Mg2+ N-3  Mg3N2
Cu2+ Cl-  CuCl2

53. C. Ionic Formulas calcium oxide aluminum chloride Ca2+ O2-  CaO
iron(III) oxide
Ca2+ O2-  CaO
Al3+ Cl-1  AlCl3
Fe3+ O2-  Fe2O3

54. Purpose: Name the compound & write the formula for ionic compounds containing polyatomic ions.
Purpose on top of ISN 104.
Notes/Practice on ISN 105. Attach list of common polyatomic ions & WKST 57 Chart on this page also.
Homework on ISN 104:
WKST 58
WKBK all

55. Ionic Names
Write the names of both elements, cation first.
Change the anion’s ending to -ide.
Write the names of polyatomic ions.
For ions with variable oxidation #’s, write the ox. # in parentheses using Roman numerals. Overall charge = 0.

56. Ionic Names NaBr Na2CO3 sodium bromide FeCl3 sodium carbonate
iron(III) chloride

57. Ionic Formulas Write each ion. Put the cation first.
Overall charge must equal zero.
If charges cancel, just write the symbols.
If not, crisscross the charges to find subscripts.
Use parentheses when more than one polyatomic ion is needed.
Roman numerals indicate the oxidation #.

58. Ionic Formulas potassium chloride magnesium nitrate K+ Cl-  KCl
copper(II) chloride
K+ Cl-  KCl
Mg2+ NO3-  Mg(NO3)2
Cu2+ Cl-  CuCl2

59. Ionic Formulas calcium oxide aluminum chlorate Ca2+ O2-  CaO
iron(III) oxide
Ca2+ O2-  CaO
Al3+ ClO3-  Al(ClO3)3
Fe3+ O2-  Fe2O3