1. Chapter : 5 Chemical Bonding
Cartoon courtesy of NearingZero.net

3. Chemical Bonds lesson 1
Forces that hold groups of atoms together and make them function as a unit.
Ionic bonds – transfer of electrons Metal + Nonmetal Ex) NaCl Li2O
Covalent bonds – sharing of electrons. 2 nonmetals Ex) H2O CO2
Metallic bonds- electrons are free to move throughout the material. Metals

4. Ionic Bonding and Compounds
Ionic Compound- is composed of positive and negative ions combined so that the positive & negative charges are equal. (Metal + nonmetal)
Where are metals located? ON THE LEFT CALLED “CATIONS
Where are nonmetals located?
RIGHT CALLED “ANIONS”

5. Writing Formulas Write the symbols of each element
Put their charge in their upper right corner
Crisscross the numbers down (Not the charges).
Example:
Write the formula for Magnesium Chloride
Mg Cl positive first “CATION”
Mg+2 Cl Write down the charges
Mg+2 Cl Crisscross numbers
MgCl2
MgCl2

6. Ide Don’t forget the Oxygen------------------oxide
Nitrogen nitride
Chlorine chloride
Fluorine Floride

7. F O N Ne Na 8e- 2e- 10p+ 11p+ 7p+ 8p+ 9p+ +1 -1 +4 IA +2 +3 -4 -3 -2+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

8. Be F +2 -1 2e- 2e- 4p+ 9p+ +1 -1 +4 IA -3 +2 +3 -4 -2 IIA VIIA VIIIA+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

9. F Be F 2e- 9p+ -1 2e- 4p+ +2 2e- 9p+ -1 +1 -1 +4 IA +2 +3 -4 -3 -2 IIA+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

10. Berylium Fluoride F Be F BeF2 -1 +2 -1 +1 -1 +4 IA +2 +3 -4 -3 -2 IIA+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

11. For ionic compounds with a metal from group 1A, 2A, & 3A place the metal first and name it first. The non-metal is put last and named last. The number of metals or non-metals is depends on how many it takes to balance the charges. Are you ready to try some? +1 -1 IA
VIIA
VIIIA +2 -3 -2
IIA
IIIA
IVA VA
VIA

12. Aluminum Chloride Cl Cl Cl Al Cl AlCl3 Al -1 -1 -1 +3 -1 +3 +1 -1 +4+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

13. Writing Formulas Practice+1 +2 -1
Write the formula for:
Aluminum Bromide
Calcium Oxide
Calcium Nitride
Sodium Chloride

14. Writing Formulas Practice+1 +2 -1
Write the formula for:
Aluminum Bromide Al Br3
Calcium Oxide
Calcium Nitride
Sodium Chloride

15. Writing Formulas Practice+1 +2 -1
Write the formula for:
Aluminum Bromide
Calcium Oxide CaO
Calcium Nitride
Sodium Chloride

16. Writing Formulas Practice+1 +2 -1
Write the formula for:
Aluminum Bromide
Calcium Oxide
Calcium Nitride Ca3 N2
Sodium Chloride

17. Writing Formulas Practice+1 +2 -1
Write the formula for:
Aluminum Bromide
Calcium Oxide
Calcium Nitride
Sodium Chloride NaCl

18. Writing Names Practice
1) MgS ___________________
2) KBr ____ _______________
3) Ba3N2 __________________
4) Al2O3 ___________________

19. Writing Names Practice
1) MgS ____Magnesium Sulfide
2) KBr ____ Potassium Bromide
3) Ba3N2 ___Barium Nitride
4) Al2O3 ____Aluminum Oxide

20. O Fe O O O Fe O Fe2O3 Fe Fe -2 -2 -2 +3 -2 +3 +3 +1 -1 +4 IA +2 +3 -4+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA

21. Lesson 2 polyatomic
The following two slides show how polyatomic ions would combine. This will help you with naming compounds that contain polyatomic ions.

22. Polyatomic Ions Lesson 2
Many atoms with a charge.
Example (SO4)-2
Covalent Bonds (sharing of electrons)
Back of periodic table

24. O Zn N NO3 NO3 Zn NO3 Zn(NO3)2 Zn -1 -1 -1 +2 +2 +1 -1 +4 IA +2 +3 -4+4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
Zinc = +2
IIIA
IVA VA
VIA

25. Now called Iron(III) sulfateFe
SO4 -2
SO4 -2 Fe +3
SO4 -2 Fe +3 -2
SO4
Fe2(SO4)3 Fe +3 +1 -1 +4 IA
VIIA
VIIIA +2 +3 -4 -3 -2
IIA
IIIA
IVA VA
VIA
Now called Iron(III) sulfate
Iron=+3

26. Polyatomic Ion Formulas
Concept:
Polyatomic ions are groups of atoms that behave as one unit.
Fact 4:
Some ions have more that one atom but their overall charge can be determined.
Examples: (SO4) = S +6 and O -8 = -2
(NO3)= N +5 and O -6 = -1
(NH4) = N -3 and H +4 = +1

27. Polyatomic Ion Formulas
Fact 5: These group ions, polyatomic ions, are treated like single ions in formulas, but must have parentheses when more than one is used in a formula.
Examples: Ca2+(NO3) 1- === Ca(NO3) 2
Ga3+ (SO4) 2- === Ga 2 (SO4) 3
(NH4) 1+O ==== (NH4) 2 O

28. Polyatomic Ion Formulas
Fact 6:
The polyatomic ions are named based on the atoms that they contain. Those with oxygen and another nonmetal are often name "____ate" with the root of the other nonmetal in the blank.
Examples: (NO3)1- is nitrate
(SO4)2- is sulfate
(ClO3) 1- is chlorate

29. Polyatomic Ion Formulas
Fact 7:
Those polyatomic ions with one oxygen less than the "ate" ions are named "----ite" ions.
Examples: (NO2) is nitrite
(SO3)2- is sulfite
(ClO2)1- is chlorite

30. Polyatomic Ion Formulas
Fact 9:
These ion groups are named hydrogen ____
or bi ______.
Examples: H(CO3)1- is called hydrogen carbonate or bicarbonate
H(SO4) 1- is called hydrogen sulfate or bisulfate

31. Examples - Formulas to Names
1. Write the names of the ions
2. Determine the charge of the positive ion
I’m a polyatomic ion
Ba(ClO4)2
barium
perchlorate
If the positive ion has a fixed charge, you are finished.
Final Name

32. Practice Problems
By now you should have an idea of what is expected when naming covalent binary compounds using prefixes.
In order to master this naming system you need to practice until you feel proficient in naming compounds using prefixes.

33. Practice Problem #1 No, you do not use prefixes
Al(NO3)3
Choose the correct name for the compound
1. Aluminium
No, you do not use prefixes
2. nitrate
No, you have the wrong oxidation number
3. Aluminum nitrite
No, you need to review polyatomic ions
4. Aluminum nitrate
Very good, click arrow to continue
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Polyatomic Ions

34. Practice Problem #2 No, you need to review prefixes
sodium chlorite
Choose the correct formula for the compound
1. NaCl
No, you need to review prefixes
2. NaClO
No, you need to review prefixes
3. NaClO2
Very good, click arrow to continue
4. Na(ClO)2
No, you have several errors
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Prefixes

35. Practice Problem #3 No, you need to review prefixes
sodium carbonate
Choose the correct formula for the compound
1. NaCO2
No, you need to review prefixes
2. Na2CO3
Very good, click arrow to continue
3. NaClO2
No, you need to review prefixes
4. Na(CO)3
No, you have several errors
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Prefixes

36. Practice Problem #4 No, you do not use prefixes
Al2(SO4)3
Choose the correct name for the compound
1. Aluminium
No, you do not use prefixes
2. nitrate
No, you have the wrong oxidation number
3. Aluminum nitrite
No, you need to review polyatomic ions
4. Aluminum sulfate
Very good, click arrow to continue
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Polyatomic Ions

37. Practice Problem #5 Very good, click arrow to continue
calcium phosphate
Choose the correct formula for the compound
1. Ca3(PO4)2
Very good, click arrow to continue
2. Ca3(PO3)2
No, you need to review prefixes
3. Ca(PO4)
No,NO,NO,NO
4. Na(PO)2
No, you have several errors
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Prefixes

38. Practice Problem #6 No, you need to review polyatomic ions
Mg(MnO4)2
Choose the correct name for the compound
1. Magnesium
No, you need to review polyatomic ions
2. Manganese oxide
No, you have the name
3. Magnesium Manganese
No, you need to review polyatomic ions
4. Magnesium permanganate
Very good, click arrow to continue
5. none of the above
No, there is a correct answer
next problem
Periodic Chart
Polyatomic Ions

39. Practice Problem #7 No, you need to review polyatomic
zinc chromate
Choose the correct formula for the compound
1. ZnCl
No, you need to review polyatomic
2. ZNCl2
No, you have several errors
3. ZnCr2O7
No, you need to review polyatomic
4. ZnCr2O
No, you need to review polyatomic
Very good, click arrow to continue
5. none of the above
Periodic Chart
Prefixes

40. POLYATOMIC IONS return Ions with -1 charge perbromate BrO4-1
bromite BrO2-1
hypobromite BrO-1
perchlorate ClO4-1
chlorate ClO3-1
chlorite ClO2-1
hypochlorite ClO-1
periodate IO4-1
iodate IO3-1
iodite IO2-1
hypoiodite IO-1
nitrate NO3-1
nitrite NO2-1
hydroxide OH-1
cyanide CN-1
thiocyanate SCN-1
acetate C2H3O2-1
Permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
phthalate C8H4O4-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
peroxide O2-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1
return

41. Lattice Energy- is the energy released when 1 mole of an ionic crystalline compound is formed from gaseous ions.
Ionic Compounds have high melting points & boiling points, are hard and brittle, have crystalline structure.

42. Transition Metals +1 +2 -1
Trannsition Metals

43. Lesson Three--Transition Metal Compounds
Concept:
Transition metals have electrons in d orbitals and can donate different numbers of electrons, thus giving them several different positive charges.
Fact 10:
These can be determined from the Roman numeral which is written next to the metal's name.
Example: Cu1+is Copper I
Pb2+is Lead II
Fe3+is Iron III
Sn4+s Tin IV

45. Transition Metal Compounds
Fact 11:
These transition metals are used in formulas just like other metals, once the charge is determined from the Roman numeral in the name.
Example:
Cu1+ Cl copper (I)
Pb2+O Lead ( II )
Fe3+Br Iron ( III )
Sn4+O Tin ( IV )

46. Transition Metal Compounds
Fact 11:
Roman numeral in the name.
Remember to criss cross
Example:
Cu1+ Cl copper (I) choride
Pb2+O Lead (II) Oxide
Fe3+Br Iron (III) Bromide
Sn4+O Tin (IV) oxide is actually SnO2

47. Transition Metal Compounds
Fact 12:
A few transition metal ions only have one charge and never change so they can be written without a Roman numeral in their formula name.
Example: Ag Zn2+ Cd2+

48. FeCl3 (Fe3+) iron (III) chloride
Names of Variable Ions
Use a roman number after the name of a metal that forms two or more ions
Transition metals and
the metals in groups 4A and 5A
FeCl3 (Fe3+) iron (III) chloride
CuCl (Cu+ ) copper (I) chloride
SnF (Sn4+) tin (IV) fluoride
PbCl (Pb2+) lead (II) chloride
Fe2S3 (Fe3+) iron (III) sulfide

49. Learning Check
Complete the names of the following binary compounds with variable metal ions:
FeBr2 iron (_____) bromide
Cu2O copper (_____) oxide
SnCl4 ___(_____ ) ______________
Fe2O3 ________________________
CuS __________________

50. Solution
Complete the names of the following binary compounds with variable metal ions:
FeBr2 iron ( II ) bromide
Cu2O copper ( I ) oxide
SnCl4 tin (IV) chloride
Fe2O3 iron (III) oxide
CuS copper (II) sulfide

51. Solution
Complete the names of the following binary compounds with variable metal ions:
FeBr2 iron ( II ) bromide
Cu2O copper ( I ) oxide
SnCl4 tin (IV) chloride
Fe2O3 iron (III) oxide
CuS copper (II) sulfide

52. Learning Check 3) cobalt trioxide Name the following compounds: A. CaO
1) calcium oxide
2) calcium(I) oxide
3) calcium (II) oxide
B. SnCl4
1) tin tetrachloride 2) tin(II) chloride
3) tin(IV) chloride
C. Co2O3
1) cobalt oxide ) cobalt (III) oxide
3) cobalt trioxide

53. Solution Name the following compounds: A. CaO 1) calcium oxide
B SnCl4 3) tin(IV) chloride
C. Co2O3 2) cobalt (III) oxide

54. Lesson Four--Using Formulas in Problem Solving
Concept: Correctly written chemical formulas hold a large amount of information for the prepared student to find.
Fact 13:
The subscripts tell us the number of atoms of each kind that is present in the compound.
Example: NaCl has one atom of sodium and one atom of chlorine.
H2SO4 has two atoms of hydrogen, one atom of sulfur and four atoms of oxygen

55. Using Formulas in Problem Solving
Fact 14:
The sum of the atomic masses times the number of atoms of each kind of element is equal to the mass of one mole of the substance.
Examples: Na = 23g/mol and Cl = 35.5g/mol so NaCl has a molar mass of 58.5g/mol
Nitric acid is HNO3so its molar mass is
H = 1 x 1 = 1
N = 14 x 1 = 14
O = 16 x 3 = 48
Total = 63g/mol

56. Metallic Bonding
Metals- conduct heat, have low ionization energy & electronegativity, give up e-
Metallic Bond- is a chemical bond resulting from the attraction between positive ions and surrounding mobile e-.
Malleability and ductility

57. Molecular Geometry
VSEPR Theory- “Valence- shell, electron-pair repulsion”
states that repulsion between the sets of valence-level electrons surrounding an atom cause these sets to be oriented as far apart as possible.

58. Determining VSEPR H-O-H E2 B B A Determine the VSEPR for H2O
Draw the Lewis Dot
Draw the Structural Formula
Label the central atom as A
Label any atoms attached to the center atom as B
Label any paired electrons on the central atom that are not used in the bond as E
H-O-H E2 B B A
VSEPR AB2E2
Shape Bent (look on chart)

59. VSEPR Chart VSEPR SHAPE AB or AB2 Linear AB2E Bent AB3 Trigonal-Planar
Tetrahedral
AB3E
Trigonal-Pyramidal
AB2E2
AB5
Trigonal-Bipyramidal
AB6
Octahedral

60. Hybridization-The Blending of Orbitals.
Dipole- is created by equal but opposite charges that are separated by a short distance.
Dipole-Dipole Attractions-Attraction between oppositely charged regions of neighboring molecules.
Hydrogen Bonding- Bonding between hydrogen and more electronegative neighboring atoms such as oxygen and nitrogen. Hydrogen bonding in Kevlar, a strong polymer used in bullet-proof vests.
London Dispersion Forces- The temporary separations of charge that lead to the London force attractions are what attract one nonpolar molecule to its neighbors. London forces increase with the size of the molecules.

61. “Electronegativity chart”. Table. Aug. 9, 2006. http://www
“Lewis Structures”. Drawings. Aug. 9,
“Oscar”. Photo. Aug. 9,
“Water Structural Formula”. Drawing. Aug. 10,
“Periodic Table of Elements”. Chart. Aug. 9,
“Information”. Aug 11,
Holt, Rinehart and Winston. Modern Chemistry. Harcourt Brace & Company