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

18. 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

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

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

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

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

23. 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

24. 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).

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

26. 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.

27. 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.

28. 2. How are ionic compounds formed?

30. 3. How are ionic compounds named?

31. 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

32. 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

33. 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

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

35. 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.

36. 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-

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

38. Crisscross

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

40. 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

41. 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

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

43. 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

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

45. Acids

46. 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

47. 5. How are acids named?

48. Acid Nomenclature Flowchart

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

50. 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”

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

52. 6. How are covalent compounds formed?

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

54. 2 Types of Covalent bonds
1. Polar Covalent: Electrons are shared unequally Nonpolar Covalent Electrons are shared equally.

55. 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.

56. 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.

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

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

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

61. 8. How are covalent compounds named?

62. 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-

63. 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.

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

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

66. 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

67. 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

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

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

70. Bonding
The End