1. What happens to electrons in a covalent bond?
Compare and contrast ionic and covalent bonds in terms of electron movement.
In an ionic bond, metals tend to become electron (donors/acceptors), and non-metals tend to become electron (donors/acceptors).
What happens to electrons in a covalent bond?

2. Covalent & Ionic Name two types of chemical bonds.
Compare and contrast ionic and covalent bonds in terms of electron movement.
Name two types of chemical bonds.
Covalent & Ionic
What happens to electrons in an ionic bond?

3. What is an ion?
An ion is a charged atom. It is formed when an atom gains or loses electrons.
What information is shown in a Lewis/Dot Diagram?

5. IONIC
BONDING

6. Ionic Compounds
When electrons are transferred from a metal to a non-metal, ionic bonds form from the attractions between oppositely charged ions.
Metal + Nonmetal
Metals tend to lose electrons to become positively charged (cations)
Nonmetals tend to gain electrons to become negatively charged (anions)

7. Example F K
Lewis Dot Structures
(show valence electrons)

8. K F

9. Ions + _ K F
Stable ionic bonds have the same number of positive and negative charges.

10. K F _ This ionic bond is the attraction between the positive K+ ion
and the negative F- ion

11. KF
Put the symbols together and you
have the chemical formula

12. Naming Ionic CompoundsKF
For the first element, use the full element name
Potassium
For the second element, change the ending to “-ide”
Fluoride
Potassium Fluoride

13. Mg2+ Oxidation Number Shows the charge of an ion
Write the oxidation numbers across the top of your periodic table
Mg2+

14. Periodic Table Ion Trend+1 +2 +3
+/-4 -3 -2 -1

15. More Practice Sodium and Chlorine Calcium and Fluorine
Magnesium and oxygen

16. BR: What is an ion?
An ion is a charged atom. It is formed when an atom gains or loses electrons.
EQ: What information is shown in a Lewis/Dot Diagram?
Lewis/Dot Diagrams are used to show the number of valence electrons for a given element.

17. BR: What is an ion?
An ion is a charged atom. It is formed when an atom gains or loses electrons.
What information is shown in a Lewis/Dot Diagram?
Lewis/Dot Diagrams are used to show the number of valence electrons for a given element.

18. What happens to electrons when an ionic bond is formed?
Valence electrons are transferred from a metal to a non-metal.
How can you check/be sure that your ionic formula is stable?
In a stable ionic compound, there are equal numbers of positive and negative charges.

19. When should you use the “-ide” ending?
Use “-ide” as the ending for a non-metal.

20. Ionic Compounds Cation (positive ion)
TRANSITION METALS
Many of these metals form more than one monoatomic ion
Give the element name
Use roman numerals to denote charge
Cr chromium
Cr2+ chromium (II)
Cr3+ chromium (III)
MAIN GROUP
Give the element name
Li lithium
Li+ lithium

21. How would you name the following?
Ag +2
Ba +2
Mg +2
Fe +3
Na+1
Zn +4
Al +3
Co +3
Silver (II)
Barium
Magnesium
Iron (III)
Sodium
Zinc (IV)
Aluminum
Cobalt (III)

23. Ionic Compounds Anions (negative ion)
Give the element name but drop the ending
Add the “-ide” ending
F fluorine
F- fluoride ion

24. How would you name the following?
P -3
Cl -1
S -2
N -3
Br -1
Oxide
Phosphide
Chloride
Sulfide
Nitride
Bromide

25. Binary Ionic Compounds
Binary compound: compounds composed of two different atoms
Write the name of the cation first
Write the name of the anion last
MgO
Magnesium Oxide

26. How would you name the following?
AgO
Ba3P2
MgCl2
FeS
Fe2S
Na3N
ZnBr4
Al 2O3
CuBr2
CuBr
Silver (II) oxide
Barium phosphide
Magnesium Chloride
Iron (II) sulfide
Iron (I) sulfide
Sodium nitride
Zinc (IV) bromide
Aluminum oxide
Copper (II) bromide
Copper (I) bromide

27. What does the roman numeral in iron (III) oxide tell you?
Roman numerals show the charge of a transition metal. Iron has a +3
What is the formula for iron (III) oxide?
Fe2O3

28. Bond With Your Classmates Part I

29. Ionic Compound Grid Determine the charge of each ion.
Make a stable ionic compounds.
Determine the number of total electrons transferred to form each compound.
Oxide
Bromide
Sulfide
nitride
Sodium
Copper II
Potassium
Iron III
Calcium
Gallium
Iron II

30. Ionic Compound Grid Oxide Bromide Sulfide nitride Iodide phosphide
Sodium
Na O
Na Br
Na S
Na N
Na I
Na P
Copper II
Cu O
Cu Br
Cu S
Cu N
Cu I
Cu P
Potassium
K O
K Br
K S
K N
K I
K P
Iron III
Fe O
Fe Br
Fe S
Fe N
Fe I
Fe P
Calcium
Ca O
Ca Br
Ca S
Ca N
Ca I
Ca P
Gallium
Ga O
Ga Br
Ga S
Ga N
Ga I
Ga P
Iron II

31. Chemistry CAT Joke

32. 1. What is the name for NaCl?
A. sodium chloride B. sodium chlorine C. sodium I chloride

33. 2. What is the correct formula for Aluminum chloride?
A. AlCl B. Al3Cl C. AlCl3

34. 3. What is the correct formula for Ba+2 and Cl-1?
A. Cl2Ba B. BaCl C. BaCl2

35. 4. What is the name for CaF?
A. calcium fluoride B. calcium fluorine C. calcium II fluoride

36. 5. What is the correct formula for a compound formed when a sodium ion combines with a fluoride ion?
A. NaF2 B. NaF C. Na2F

37. 6. What is the correct formula for Magnesium chloride?
A. MgCl B. Mg2Cl C. MgCl2

38. 7. What is the correct formula for calcium oxide ?
A. CaO2 B. CaO C. Ca2O

39. 8. What is the name for MgS?
A. magnesium II sulfide B. magnesium sulfur C. magnesium sulfide

40. 9. What is the correct formula for Ag+1 Cl -1?
A. SiCl B. AgCl C. AgCl3

41. 10. What is the formula formed by a potassium ion and a sulfur ion?
A. K2S B. KS C. KS2

42. 11. What is the compound formed from Ca +2 and I-1?
A. CaI B. I2Ca C. CaI

43. 12. What is the formula formed by Li +1 and O-2?
A. Li2O B. LiO C. LiO2

44. Mock Quiz Potassium & sulfur Name  Formula Sodium chloride
Valence Electrons Ions Formula & Name
Potassium & sulfur
Name  Formula
Sodium chloride
Aluminum sulfide
MgI2
Na2O

45. Mock Quiz Potassium & sulfur Name  Formula Sodium chloride
Valence Electrons Ions Formula & Name
Potassium & sulfur
Name  Formula
Sodium chloride
Aluminum sulfide
MgI2
Na2O

46. What does the roman numeral in iron (IV) oxide tell you?
Roman numerals show the charge of a transition metal. Iron has a +4
What is the formula for iron (IV) oxide?
FeO2

47. How do ionic compounds form?
When electrons are transferred from a metal to a non-metal, oppositely charged ions attract to form an ionic bond.

48. BONDING
PART II

49. Covalent
Compounds

50. Covalent Compounds
In covalent bonding, atoms still want to achieve stability by having a full outer energy level.
Atoms SHARE electrons rather than lose or gain
Nonmetal—Nonmetal

51. EXAMPLE:
Chlorine forms a
Covalent bond with itself
Cl2

52. How
will these
two chlorine atoms
become stable? Cl Cl

53. Cl Cl
Each chlorine atom wants to
gain one electron to achieve 8.

54. Cl Cl do to achieve an octet? What’s the solution – what can they
Neither atom will give up an electron …
What’s the solution – what can they
do to achieve an octet?

55. Cl Cl

56. Cl Cl
Octet: contains
8 electrons

57. Cl Cl octet circle the electrons for each atom that completes
their octets

58. Cl Cl The octet is achieved by each atom sharing the
electron pair in the middle
circle the electrons for
each atom that completes
their octets

59. Cl Cl This is the bonding pair circle the electrons for
each atom that completes
their octets

60. Cl Cl It is a single bonding pair circle the electrons for
each atom that completes
their octets

61. Single bonds are abbreviatedCl Cl
Single bonds are abbreviated
with a dash
circle the electrons for
each atom that completes
their octets

62. Chlorine is a single bond written as Cl2
circle the electrons for
each atom that completes
their octets

63. O
How will these two oxygen atoms bond?

64. O Oxygen atoms are highly electronegative.
So both atoms want to gain two electrons.

65. Both electron pairs are shared.

66. O O
6 valence electrons
plus 2 shared electrons
= full octet

67. O O
6 valence electrons
plus 2 shared electrons
= full octet

68. O O
two bonding pairs,
making a DOUBLE BOND

69. O O =
For convenience, the double bond
can be shown as two dashes.

70. Oxygen is a double bond written as=
Oxygen is a double bond written as O2

71. Naming Covalent Compounds (for compounds made with more than one element)
Use “–ide” on the end of the second element
Use numerical prefixes on both element names to show how many there are of each

72. Number of Atoms
Prefix 1
mono- 2
di- 3
tri- 4
tetra- 5
penta- 6
hexa- 7
hepta- 8
octa- 9
nona- 10
deca-

73. Examples of compounds of N and O:
NO nitrogen oxide
NO2 nitrogen dioxide
N2O dinitrogen oxide
N2O4 dinitrogen tetroxide
N2O5 dinitrogen pentoxide
In most cases, “mono” is understood

74. Select the correct name for each compound.
A. SiCl4 1) silicon chloride
2) tetrasilicon chloride
3) silicon tetrachloride
B. P2O5 1) phosphorus oxide
2) phosphorus pentoxide
3) diphosphorus pentoxide
C. Cl2O7 1) dichlorine heptoxide
2) dichlorine oxide
3) chlorine heptoxide

75. Name these compounds CO2 N2O3 BF3 SiO2 SiI4 As2O5 Carbon dioxide
Dinitrogen trioxide
Boron trifluoride
Silicon dioxide
Silicon tetriodide
Diarsenic pentoxide

76. Write the Formulas phosphorus pentachloride dinitrogen trioxide
sulfur hexafluoride
PCl5
N2O3
SF6

77. QUIZ TIME Only use numeric prefixes for covalent compounds.
When is it appropriate to use numeric prefixes in a compound name?
Only use numeric prefixes for covalent compounds.
Nonmetal + Nonmetal

78. What does the numerical prefix in a covalent compound tell you?
The numerical prefix determines the number of each nonmetal present in the covalent compound.
Carbon and Oxygen combine in many different ways to make covalent compounds. How are the formulas of the following different?
carbon monoxide
carbon dioxide
dicarbon trioxide CO
CO2
C2O3

79. Review: Valence Electrons Transferred
Aluminum and Chlorine
Dot diagrams
Charges

80. Review: Name to Formula
Potassium oxide
Lead I sulfide
Boron phosphide

81. Review: Formula to Name
BeS
Fe2O3
CaF2

82. Review: Valence Electrons Transferred
Sulfur and Chlorine
Sulfur and Oxygen
Dot diagrams
Dash structure

83. Review: Name to Formula
Iodine pentafluoride
Dinitrogen tetroxide
Phosphorous triiodide

84. Review: Formula to Name
CCl4
Si2Br6 CO

85. Timed Challenge Naming Binary Compounds (Ionic) One – Ten 6 minutes
Eleven – Twenty 4 1/2 minutes
Naming Binary Compounds (Covalent)
One – Seven 4 minutes
Eight – Fifteen 3 minutes

86. Timed Challenge Naming Binary Compounds (Ionic) One – Ten 6 minutes
Eleven – Twenty 4 1/2 minutes
Naming Binary Compounds (Covalent)
One – Seven 4 minutes
Eight – Fifteen 3 minutes

87. Number of Atoms
Prefix 1
mono- 2
di- 3
tri- 4
tetra- 5
penta- 6
hexa- 7
hepta- 8
octa- 9
nona- 10
deca-