1. Bonding

2. 1. What two types of bonds form and how do they form?

3. Chemical Bonds This is the force of attraction between two elements.
Bonds involve valence electrons.
Valence electrons: Electrons in the outermost energy level of an atom.
Atoms react (form bonds) to have a stable octet (noble gas structure).

8. Covalent Bonds
A covalent bond is formed when valence electrons are shared by both atoms.

9. Covalent Bonds
Covalent bonds are between nonmetals and nonmetals.

10. Covalent Bonds
A pair of shared electrons forms a single bond.

11. Covalent Bonds
Both atoms become stable (octet) due to the covalent bonding.

12. Ionic Bonds:
Ionic Bonds are formed by the attraction of equal and opposite charges.

13. Electrons are transferred in an ionic bond.
Ionic Bonds
Electrons are transferred in an ionic bond.

14. Ionic Bonds

15. Ionic Bonds – Electrostatic Attraction

16. Ions
Atoms that have a positive or negative charge.

17. Metals – Cations (+)
Nonmetals – Anions (-)
Metalloids
Periodic Table

19. Ionic Bonds occur between:
A metal (cation) and a nonmetal (anion)
A metal (cation) and a negative polyatomic ion
A positive polyatomic ion and a nonmetal (anion)
A positive polyatomic ion and a negative polyatomic ion

20. Cations – Positive Ions
Cations are ions formed by metals that are positively charged due to the loss of an electron.

21. Cations – Positive Ions
Cations have low ionization energy.
They lose electrons easily to become positive.

22. Anions – Negative Ions
Anions are nonmetals that are negatively charged due to the gain of an electron.

23. Anions – Negative Ions Non-metals have high electronegativity.
They gain electrons to become negative and form anions.

24. POLYATOMIC IONS
Polyatomic ions are mostly made of two (or more) non-metals.
They stay together – Treat as one ion.
Ions with -1 charge
perbromate BrO4-1
bromate BrO3-1
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
acetate C2H3O2-1
Permanganate MnO4-1
bicarbonate HCO3-1
Ions with a -2 Charge
carbonate CO3-2
sulfate SO4-2
sulfite SO3-2
chromate CrO4-2
dichromate Cr2O7-2
oxalate C2O4-2
Ions with a -3 Charge
phosphate PO4-3
phosphite PO3-3
arsenate AsO4-3
Ions with +1 charge
ammonium ion NH4+1

25. Oxidation Number Group Oxidation Number 1A 1+ 2A 2+ 3A 3+ 4A 4+/4- 5A3- 6A 2- 7A 1-
The charge on an ion.
positive (cation) negative (anion)
Predicted by the group/family (column).

26. Ionic Bonds The bone represents an electron.
The dog that takes the bone is negative.
The dog that loses the bone is positive.

27. Ionic Bonds - Review
Electrons are transferred from a metal to a nonmetal.
Metals give up electrons to form cations; Non-metals take electrons to form anions
The attractive forces bring the cation and anion together.
Both achieve an octet of electrons.

28. Ionic Bonds Quiz 1) In an ionic bond, electrons are _____.
2) The type of electrons involved are ___ or outer
shell electrons.
3) Metals ___ electrons, nonmetals ___ electrons in
order to get a ___ gas configuration (stable octet).
4) Cations have a __ charge and are formed by __.
5) Anions have a __ charge and are formed by __.
6) ____ charges hold the compound together.

29. 2. How are ionic compounds formed?

31. Ionic Bonds Essential Question #2: See Essential Question #1

32. 3. How are ionic compounds named?

33. Naming Binary Ionic Compounds
The cation (+ ion) is written first, followed by the anion (- ion).
Atoms combine so that they are neutral.
Name 1st element as is (cation).
Name 2nd element (anion) using the “ide” ending.
What is the name of AlBr3?
Aluminum bromide

34. Practice Naming Ionic Compounds
1) NaCl
Sodium chloride
2) MgF2
Magnesium fluoride
3) Al2O3
Aluminum oxide
4) CaS
Calcium sulfide
5) GaP
Gallium phosphide
6) K2O
Potassium oxide

35. NAMING TERNARY Ionic COMPOUNDS (POLYATOMIC IONS)
1) Name cation (+) ion.
2) Name the polyatomic ion as a group (ate, ite)
Ex. CaSO4
cation=calcium
anion=sulfate
Name: Calcium Sulfate

36. Practice: Name the Compound
1) NaClO3
sodium chlorate
2) AlPO4
aluminum phosphate
3) (NH4)2S
ammonium sulfide
5) CaCl2 calcium chloride

37. Writing Formulas for Ionic Compounds
The oxidation numbers have to add up to zero.
Determine oxidation numbers of the ions.
Cations – Look at Periodic Table.
Anions – Look at the Periodic Table or Polyatomic Ion chart.
Balance the charges by adding subscripts.
Put polyatomic ions in parenthesis if there is more than one.

38. Writing Formulas for Ionic Compounds
Write the formula for calcium chloride.
Calcium is Ca2+
Chloride is Cl1-
Ca2+ Cl1- would have a 1+ charge.
Need another Cl1-
Ca2+ Cl21-

39. Crisscross
Switch the numerical value of the charges
Ba2+
N3- 2 3
Ba3 N2
Reduce ratio if possible

40. Crisscross

41. Practice Writing Ionic Formulas
Aluminum Bromide
cation anion
Al Br-
AlBr3
Sodium Oxide
Na O2-
Na2O

42. Stock System Nomenclature
Some metals can form more than 1 charge.
Determine the (+) charge to make the compound neutral.
Use Roman Numeral (in parentheses) to show the (+) charge.
Ex. CuCl = Copper ( ) chloride
Cl = -1 so Cu must be +1 to be neutral. (I)
Name = copper (I) chloride

43. Stock System Nomenclature
SnO
Tin ( ) oxide
Since oxide = 2- then Sn must be 2+ = 0
Tin (II) oxide
FeCl3
Iron ( ) chloride
Since chloride = 1- x 3 = Fe = +3 = 0
Iron (III) chloride

44. Stock System Formulas 1) copper (I) sulfide Cu+ S2- Cu2S
2) copper (II) sulfide
Cu S2-
CuS
3) iron (III) oxide Fe3+ O2-
Fe2O3

45. Name the Compounds * Use Stock System*
1) * CuCl
Cl = -1 Cu = Copper (I) chloride
2) * CuCl
Cl = -1 x 2 = Copper (II) chloride
3) * PbS Lead (II) sulfide
S = -2 Pb = +2
4) * PbS Lead (IV) sulfide
S = -2 x 2 = -4 Pb=+4
5) * FeBr3
Br = -1 x 3 = -3 Fe= Iron (III) bromide
6) AgI
Ag has only 1 ion, Silver iodide

46. Choose covalent (2 nonmetals) or ionic (metal+nonmetal or polyatomic)
Choose covalent (2 nonmetals) or ionic (metal+nonmetal or polyatomic). Determine Names.
KCl NO
NaNO3
NH4Cl
SO3
CBr4

47. Mixed Review Name the following compounds: 1. CaO 2. SnCl4
a) calcium oxide b) calcium(I) oxide c) calcium (II) oxide
2. SnCl4
a) tin tetrachloride b) tin(II) chloride
c) tin(IV) chloride
3. N2O3
a) nitrogen oxide b) dinitrogen trioxide
c) nitrogen trioxide

48. Mixed Review Dinitrogen monoxide Potassium sulfide Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron (III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride

49. 4. What is unique about ionic compounds that have Hydrogen as a cation?

50. Acids

51. Acids
Ionic compounds that have Hydrogen (H+) acting as a cation are called acids.
Formulas usually begin with ‘H’.
HCl
HNO3
H2SO4
HClO3
H3BO3
*CH3COOH

52. 5. How are acids named?

53. Acid Nomenclature Flowchart

54. How to Name Binary Acids:
hydro_________ic acid.
Example: HCl
- Hydrochloric Acid
Example: HF
- Hydrofluoric Acid

55. How to Name Tertiary Acids:
Tertiary acids ending in –ate: ___________ ic acid
Tertiary acids ending in –ite: ___________ous acid
An easy way to remember which goes with which…
“In the cafeteria, you ATE something ICky”

56. How to Name Tertiary Acids: Examples
H2SO4
sulfuric acid
HNO2
nitrous acid

57. 6. How are covalent compounds formed?

58. Covalent Bonds Essential Question #6: See Essential Question #1

59. 7. What are the two types of covalent compounds that can be formed based on the way electrons are shared?

60. 2 Types of Covalent bonds
1. Polar Covalent: Electrons are shared unequally Nonpolar Covalent Electrons are shared equally.

61. Polar Covalent Molecules
Unevenly matched but willing to share
Stronger dog gets a larger portion of the bone
Element that’s more electronegative pulls the pair of electrons towards it.

62. Polar Covalent Molecules
Due to the uneven sharing of electrons, there is a more positive end and more negative end to the molecule.
This causes polar covalent molecules to interact with other polar covalent molecules and ionic compounds.

63. Polar Covalent Molecules
Electronegativity is the reason for the unequal sharing of electrons. Some atoms have a stronger attraction for electrons.

64. Nonpolar Covalent Molecules
Dogs of equal strength
Both dogs have equal attraction for the bone

65. Nonpolar Covalent Molecules
There are no partial charges.
Nonpolar Covalent Molecules only dissolve in other nonpolar covalent molecules.

67. 8. How are covalent compounds named?

68. Naming Covalent Compounds
Number of atoms
(subscript)
Prefix 1
mono- 2
di- 3
tri- 4
tetra- 5
penta- 6
hexa- 7
hepta- 8
octa- 9
nona- 10
deca-

69. Covalent Bond Naming Rules
Use Prefixes to indicate the number of atoms of each element (Look at the subscripts).
Add the suffix “–ide” to the ending of the name of the last element.
Remember that “mono” is not used for the first element, only subsequent elements.

70. Binary Covalent Compound Naming Practice
= carbon dioxide CO
= carbon monoxide
SO2
SO3
P2O5 NO
BH3

71. Covalent Compounds with “Common Names”
Chemical Name
H2O
Water
NH3
Ammonia
N2H4
Hydrazine
N2O
Nitrous Acid (Laughing Gas)

72. 9. What are organic compounds and how are they named?

74. Organic Compounds
These are carbon-containing compounds made of hydrocarbons and their derivitives.
Organic compounds are covalently bonded.
They are often produced by living things.
Carbon is able to bond and form many different compounds.

75. Hydrocarbons These are the simplest organic compounds.
They contain only Hydrogen and Carbon.

76. Methane is the simplest alkane.
Alkanes
Organic Compounds with only single bonds.
“Saturated”
Methane is the simplest alkane.

77. ALKANE SERIES # of Carbons Prefix 1 Meth 2 Eth 3 Prop 4 But 5 Pent 6
Hex 7
Hept 8
Oct 9
Non 10
Dec
“Me Eat Peanut Butter!

78. QUIZ 1) Most carbon containing compounds are ____.
2) Hydrocarbons contain the elements __ & __.
3) Hydrocarbons containing all single bonds belong to the ___series and are _____.
4) The prefixes for hydrocarbons are:
1= 2= 3= 4= 5= 6= 7= 8= 9= 10=

79. Alkanes The formula for Alkanes is CnH2n+2 . n= # carbons
Example: How many H’s does Hexane have?
C6H2(6)+2
C6H14

80. Alkanes
Example: How many H’s does Pentane have?
C5H2(5)+2
C5H12

81. Alkanes
Name this Alkane.
Ethane

82. Types of Alkane Chains Branched Chains Straight Chains Iso-Butane
These are “Isomers.” They have the same formula, but a different structure.
C4H10

84. Alkyl Groups
These are the branches of the chain.
“yl” endings

85. Alkyl Groups What are the isomers of pentane? Pentane
2-methylbutane (Name the group from the shortest end.)
2,2-dimethylpropane

86. Naming Alkanes (IUPAC Rules)
Count # Carbons in longest continuous chain (parent chain).
Number Carbons in parent chain (choose a side so that substituent groups have the smallest sum). Name each alkyl group (“yl” ending). Place this name before name of parent chain.
If same alkyl group occurs more than once as a branch, use prefix (di-, tri-, tetra, etc.) before the name to indicate the number of groups.
If different alkyl groups occur, name in alphabetical order.
Write entire name using hyphens (to separate numbers from words) and commas (to separate numbers).

87. Name the Isomers of Hexane.

88. Name these Isomers:

89. Cyclic Alkanes (Cycloalkanes)
These are alkanes that have a ring structure.
Count the number of carbons in the ring.
Add “cyclo” as a prefix.
Cyclohexane

92. Alkane Quiz Alkanes can be in straight chains or ____.
To show a branch, use the “___” ending.
Hydrocarbons that have the same formula but different structure are called ___.
___ alkanes have a ring structure. They are named using the prefix “_____”.

94. Properties of Alkanes Alkanes are nonpolar covalent molecules
This means there is less attraction between molecules.
Therefore, alkanes are immiscible (insoluble) in water. (Water is polar).

95. Properties of Alkanes Alkanes have low boiling points (b.p.)
Boiling Point increases as carbon number increases.

96. Properties of Alkanes
Due to nonpolar bonds and strong bonds between Carbon and Hydrogen, Alkanes have low reactivity.
Alkanes burn. CH O2  CO2 + 2 H2O
Notice that combustion & respiration have similar products.

97. Properties of Alkanes Quiz
Alkanes are immiscible in water because they are ___.
They have ___ boiling points because they have __ intermolecular forces.
Boiling point __ as carbon number increases.
Alkanes show ___ reactivity because of strong H-C bonds.
Alkanes undergo ___ reactions (burning).
When alkanes burn, they react with __ in the air to form ____ and water.
Combustion has the same products as ____.

98. 2,2-dimethylpropane

99. 3,3-dimethylhexane

100. 3-ethyl-4,5-dipropyloctane

101. Alkene and Alkyne
Alkanes are organic compounds that only contain single bonds.
Alkenes are organic compounds that have double bonds.
Alkynes are organic compounds that have triple bonds.

102. Bonding
The End