1. Chemical
Bonding 1

2. 2
GOALS
1. Compare & contrast ionic and covalent bonds in terms of electron position.
2. Predict formulas for stable binary ionic compounds based on balance of charges.
3. Use IUPAC nomenclature for transition between chemical names and chemical formulas of
- binary ionic compounds
- binary covalent compounds
4. Apply the Law of Conservation of Matter by balancing the following types of
chemical equations:
• Synthesis
• Decomposition
• Single Replacement
• Double Replacement 34 16

3. Why do Atoms Form Compounds?3
Why do Atoms Form Compounds?
Stability.
What makes an atom stable?
Full outer energy level.
Eight.
Chart page 576.

4. Ionic Covalent A Chemical Bond holds atoms together in a compound.4
A Chemical Bond holds atoms together in a compound.
Two basic types:
Ionic
Covalent

5. Ionic Bonding Transfer of electrons from one atom to another atom.5
Ionic Bonding
Transfer of electrons from one atom to another atom.
Occurs between metals and nonmetals.
Remember: Atoms need a full outer energy level to be stable.
EIGHT!

6. Occurs between metals and nonmetals.6
Occurs between metals and nonmetals.
Metals are electron donors.
Non-metals are electron accepters.
Called compounds.

7. 7

8. 8
OPPOSITES ATTRACT!

9. 9
Ionic Bonding
CLIP

10. Covalent Bonding Occurs between nonmetals and nonmetals.10
Covalent Bonding
Occurs between nonmetals and nonmetals.
The sharing of electrons between atoms.
Called Molecules.

11. 11

12. 12
Hydrogen and Fluorine
Hydrogen and Chlorine

13. 13
Single, Double, Triple

14. 14
Clip

15. When one atom has a greater positive charge15
Unequal Sharing δ+ δ_
Polar
When one atom has a greater positive charge

16. NaPO4 CO2 HCl H2O NaF NaCl KCl MgCl2 CaCO3 NO2 N2 H2SO4 Cl2 NaF 16
clip

17. Writing
Chemical
Formulas
Goals revisited

18. 17 The chemical formula for water is H2O. Carbon Dioxide is CO2.
Writing chemical formulas is a shorthand way of indicating what a substance is made of. 
These formulas also let you know how many atoms of each type are found in a molecule. 
The chemical formula for water is H2O. 
Carbon Dioxide is CO2. 
Why does oxygen combine in different ratios, in different compounds? 
The chemical formula for table salt is NaCl. Calcium Chloride is CaCl2.
Why does chlorine combine in different ratios, in different compounds? 

19. The simplest compounds are ones with only two elements18
The simplest compounds are ones with only two elements
These are called binary
KI, CO, H2O, NaCl

20. Oxidation numbers +1
Tell you how many electrons an atom must gain, lose or share to become stable. -2 +2 +3 -3 -1 19

21. All compounds are neutral That means the overall charge is ZERO!20
Oxidation numbers
We can predict the ratio of atoms in ionic compounds based on their oxidation numbers +1 -1
1 valence electron K Cl
7 valence electron
All compounds are neutral
Tells you how many electrons an atom must gain, lose or share to become stable.
KCl
That means the overall charge is ZERO!

22. To make it ZERO, you need 1 Ca & 2 Br.+1 -1 +2 -1 Na Br Ca Br
To make it ZERO, you need 1 Ca & 2 Br.
NaBr
CaBr2
Subscripts show the number of atoms of that kind in the compound 21

23. Some elements have more than one oxidation number (Chart p588)+3 -2 +2 -2 Fe O Fe O
Fe2O3
FeO
We call these elements- Multivalent Elements 22

24. Now You Try writing Binary Ionic formulas
K + Br
Mg + Cl
Ca + I
K + O
K + I
Sr + Br
Na + O
Ga + Br
Fe+2 + O
Fe+3 + O
Cu+2 + F
Cr+3 + O
Mg + O
Al + P

25. Groups of Covalently Bonded atoms that stay together.24
Polyatomic Ions
Cations:
ammonium, NH4+
Anions:
nitrate, NO3-
sulfate, SO42-
hydroxide, OH-
phosphate, PO43-
carbonate, CO32-
chlorate, ClO3-
permanganate, MnO4-
chromate, CrO42-
Groups of Covalently Bonded atoms that stay together.

26. Try these……. Na + SO4 K + PO4 Mg + PO4 NH4 + NO3 Ca + CO3 H + SO425
Try these…….
Na + SO4
Mg + PO4
Ca + CO3
Na + OH
Mg + OH
NH4 + OH
K + PO4
NH4 + NO3
H + SO4
Ca + SO4
K + NO3
Na + PO4

27. Naming
Chemical
Formulas

28. Naming Binary Compounds and Molecules26
Steps:
If it is Binary-
Decide if it is an ionic or covalent bond.
Metal- nonmetal…..
Ionic
Nonmetal- nonmetal….
Covalent
Example:
NaCl

29. If ionic ……. Examples: NaCl K2O AlCl3 BaF2 KI Li2O
Check to see if any elements are multivalent.
If all single valent, write the name of the positive ion first.
Write the root of the negative ion and add –ide.

30. If ionic ……. FeO Fe2O3 CuO Cu2O PbCl4 PbI2 30 Examples:
Check to see if any elements are multivalent.
If multivalent ions, determine the oxidation number of the element.
Use Roman numerals in parentheses after the name of the element.
Write the root of the negative ion and add –ide.

31. 31
If Covalent...
Use Greek prefix to indicate how many atoms of each element are in the molecule
Add -ide to the more electronegative element
Greek Prefixes
1- mono-
2- di-
3- tri-
4- tetra-
5- penta-
6- hexa-
7- hepta-
8- octa-
Example: NO
Nitrogen Monoxide
PCl3
Phosphorous trichloride

32. If it contains a polyatomic ion...32
If it contains a polyatomic ion...
Write the name of the positive ion.
Write the name of the polyatomic ion.
Examples:
NaCO3
KNO3
NaC2H3O2
Example:
KOH
Potassium Hydroxide
CaCO3
Calcium Carbonate

33. Name the following: CaSO4 KBr NH4OH HCl CaCO3 MgO Cu(ClO3) 2 CaCl33
Name the following:
CaSO4
NH4OH
CaCO3
Cu(ClO3) 2
Cr2O 3
SrI 2
CCl4
KBr
HCl
MgO
CaCl
H2O
NO2
CuSO4

34. 34
Writing & Balancing
Chemical Equations
Goals revisited

35. 35
Chemical Reactions
A chemical reaction is a change in which one or more substances are converted into new substances.
Rearrangement of bonds in compounds and molecules.
Chemical Equations make it possible to see clearly what is happen during a chemical reaction

36. Chemical equations are a shorthand way to show chemical reactions.36
Chemical equations are a shorthand way to show chemical reactions.
Reactants
Products
H2 + O2
H2O

37. The mass of the products always equals the mass of the reactants37
Conservation of Mass
The mass of the products always equals the mass of the reactants

38. 2 Hydrogen atoms & one Oxygen atom38
H2 + O2
H2O
Does this meet the Conservation of Mass Law?
2 Hydrogen atoms
2 Oxygen atoms
2 Hydrogen atoms & one Oxygen atom
Must Balance the Equation to show Conservation of Mass.

39. 39
Can add coefficients to Balance equations. 2
H2 + O2 2
H2O 4 2 2 2 4 2 1
Balanced!!
Steps:
1. Count Atoms on both sides
2. If not Balanced, add coefficients to balance.
3. Recount atoms after adding each coefficient.
4. Keep adding coefficients until balanced.

40. 40
Types of
Chemical
Reactions

41. Single Replacement (Single Displacement) 41
Synthesis
Decomposition
Single Replacement (Single Displacement)
Double Replacement (Double Displacement)

42. Synthesis
“to make”
A + B AB
Cu + O CuO
2H2 + O H2O

43. Decomposition
“to breakdown”
AB A + B
2H2O H O2
NaOH Na + OH

44. When one element replaces another element in a compound
Single Replacement
When one element replaces another element in a compound
A + BC AC + B
Cu+AgNO3 Cu(NO3)2+ 2Ag
The more reactive metal will always replace the less reactive metal. (p749)

45. Single Replacement
Clip

46. Double Replacement AB + CD AD + CB Ba(NO3)2+K2SO4 BaSO4 2KNO3 Clip
Positive Ion of One compound replaces the positive ion of another compound and a Precipitate is formed.
AB + CD AD + CB
Ba(NO3)2+K2SO BaSO4 2KNO3
Clip

47. Clip

48. Chemical Reactions
and
Energy

49. Chemical Reactions and Energy51
Chemical Reactions and Energy
All chemical reactions release or absorb energy.
Heat, light, sound
Chemical reactions are the making and breaking or bonds.

50. 1. Exergonic
Chemical reactions that releases energy are called exergonic.
Glow sticks
If heat is released, it is called exothermic.

51. 2. Endergonic
Chemical reactions that require energy are called endergonic.
Ex: Cold Packs
If heat is absorbed, it is called endothermic

52. Catalysts and Inhibitors
Some reactions proceed slowly.
They can be sped up by a catalysts.
Catalysts are not used up in the reaction.
EX: enzymes (biological catalysts)
Some reactions proceed too fast.
They can be slowed down by inhibitors.
EX: Preservatives in food

53. GOALS Revisited…..
1. Compare & contrast ionic and covalent bonds in terms of electron position.
2. Predict formulas for stable binary ionic compounds based on balance of charges.
3. Use IUPAC nomenclature for transition between chemical names and chemical formulas of
• binary ionic compounds
• binary covalent compounds
4. Apply the Law of Conservation of Matter by balancing the following types of
chemical equations:
• Synthesis
• Decomposition
• Single Replacement
• Double Replacement