Chapter 7-9 selected

1. Chemical Bonding
Honor Chemistry

2. Overview of Types of Bonds
• Metal and Nonmetals = ionic bond= transfer of electrons
• Nonmetal and Nonmetal= covalent bond=sharing electrons
• Metal and Metal = metallic bond

3. ION BONDS LEQ’S & OBJECTIVES:
• What is an ionic bond and
how does it form?
• What are the properties of
ionic compounds?
• How are ionic formula units
written?
• How are ionic compounds
named?
• Use know and use the
identified vocabulary.
• Determine the number of
valance electron for an element
in the representative families
and the transition metal
identified.
• Apply the octet rule to an
element.
• Explain how ions form.
• Write the chemical formula
• Name binary compounds.
• Describe the properties of an
ionic compound.

4. Ionic Bonds
http://www.pbslearningmedia.org/asset/lsps07_int_ionicbonding/
Ionic bonds are formed from the electrostatic force between ________
with opposite _______________ that makes them “stick” together.
The ions are formed when one or more ______________ from one atom
are ___________ to another. The atom that loses an electron is a
____________ and has a ________________ charge. The atom that gains
an electron is a _______________ and has a ______________ charge.

5. How do you know what ions are
formed?
• Metals form _____________; Nonmetals
form_____________.
• The octet rule states: (p188)
_________________________________________
_________________________________________
______________
• Look at the diagrams of electron configuration change in
sodium (p 189) and oxygen (p192).
• For each representative group find the charge of the ion produced

6. Charges
• You must MEMORIZE the charges of the representative groups.
 Group 1 = +1
 Group 2 = +2
 Group 13 = +3
 Group 15 = -3
 Group 16 = -2
 Group 17 = -1

7. Polyvalant Metals
Most Transition Metals can have more than one
charge, polyvalent.
A few have only one cation, so MEMORIZE:
Zn +2
Ag +1
Cd +2
Otherwise you will be told the charge in the
name!

8. Why are they called formula units?
The ions are attracted to each other by
the electrostatic charges and form 3-D
shape called a ________________
The simplest ratio that ions combine in
is _____________________.
Give two examples:

9. Writing Formula Units
• Compounds have NO charge, so
Total Positive Charge = Total Negative Charge
Example: K+1 and S-2
Ca+2 and Cl-1
Cr+3 and Br-1
Fe+2 and O-2
Fe+3 and O-2

10. Names of Ions
(We will only learn the modern Stock names)
 For metals in the group 1, 2 and the metals that only
have one cation, just say the name.
 Al +3 = aluminum cation
 For metals with more than one cation, the name is
followed by a Roman number giving the charge.
 Fe+2 = Iron (II)= “iron two cation”
 For nonmetals keep the stem of the element name and
add –ide.
 Cl-1 = chloride anion
 To Name a Compound: name the cation and the anion.
 CuCl2 = Copper(II) Chloride
*Notice: the 2 in the name is NOT the number of ions
in the compound!

11. Naming
K2S
CaCl2
CrBr3
FeO
Fe2O3

12. Practice Writing and Naming
Ba+2 and O-2
K+1 and S-2
Ca+2 and Cl-1
Fe+3 and Br-1
Cr+3 and O-2

13. And in Reverse
• Iron(II) Bromide
• Silver Chloride
• Potassium Oxide
• Copper (II) Telleride

15. Polyatomic Ion
• A covalently bonded group of atoms that
has a charge and behaves as a unit.
• List on the back cover.
• Writing the formula unit is the same
process, but use ( ) around the group if you
have more than one.

16. Master List
• You have a list of ions that you will be able to use
on practice and tests but it is helpful to recognize
a few things:
 Most polyatomic ions are anions; ammonium is the
exception.
 Most do end in –ate or ite; the exception are
cyanide, peroxide, and hydroxide.
 A family has the same charge; oxides of sulfur are -
2, oxides of nitrogen are -1.

17. Practice
• Ag NO3
• Ca CO3
• Ca (PO4)

18. Examples
• Potassium chlorate
• Iron(II) nitrate
• Zinc phosphate
• Barium hydoxide

19. Properties of Ionic Compounds
•Crystalline Solids at Room
Temperature
•High Melting Point
•Conductors if molten or in solution

20. Crystalline Structure

21. High Melting Point

22. Conducts Electricity when molten or
in solution.

24. Covalent Tutorial
• http://www.pbslearningmedia.org/resource/lsps07.sci.phys.matter.cov
alentbond/covalent-bonding/

25. What are covalent bonds
• A covalent bond is formed by _________
pairs of _____________. It is the stable
balance force of __________ between the
nucleus and the electrons and the force of
repulsion between the two _________.
• The __________ occurs at the point where
the potential energy is the lowest.

26. What are single, double and triple
bonds?
• A single bond results from _____________ 1
pair (2 electrons).
• A double bond results from sharing
_____________ pairs (4 electrons).
• A triple bond results from sharing 3 pair (
______ electrons).

27. What are the characteristics of
covalent compounds?
• Gases, liquids or solids made of
molecules.
•Low melting and boiling points
• Poor conductors in all phases

28. Naming
• The first element is given using its name
• The second element is name likes its anion
(with –ide)
• Prefixes are added to tell the number of
atoms present for each.
• Mono- is not used to name the first
element.

29. The prefixes (memorize)
• Mono- 1
• Di- 2
• Tri- 3
• Tetra- 4
• Penta- 5
• Hexa- 6
• Hepta- 7
• Octa- 8
• Nona- 9
• Deca- 10

30. Examples
• dinitrogen difluoride:
• carbon tetrachloride
• CO2
• CO

31. DoNow
• What naming system do you think will give
you the most problems? Why?

32. Polar Bonds and Molecules
• Nonpolar share the electrons equally
• Polar bond is a covalent bond where
the electrons are shared unequally
resulting in regions of charge.
• The difference in electronegativity
determines the bond type.

33. How do you know?

34. Naming Acids
• If hydrogen is with a strong nonmental : hydro______ic acid
• ex HCl: hydrochloric acid
• If hydrogen with polyatomic ending in -ate: _____ic acid
• Ex H2SO4 Sufuric acid
• If hydrogen with polyatomic ending in -ite: _____ous acid
• Ex H2SO3 Sufurous acid

35. Written Practice
• Beyond here are DoNows or TOD to prepare for open ended
questions

36. A certain compound consists of
potassium, nitrogen, and oxygen.
Hypothesize a possible formula and
name for this compound. Explain your
reasoning.

37. Describe the bonding in potassium
hydroxide.
Use 5: covalent, ionic, atom, cation, anion,
polyatomic ion, formula unit, charge.

38. Draw and describe a water molecule.
(use 4)
Use 4: polar, covalent, electron pairs, atom,
molecule, positive, pole, negative,
electronegativity, ς