The document covers the topic of chemical bonding, detailing how atoms bond through the arrangement of electrons in energy levels and the formation of electron dot diagrams. It explains different types of bonds such as ionic, covalent, and metallic, along with how to name compounds and their characteristics. The document also emphasizes the importance of valence electrons in determining an atom's ability to bond and provides examples for practice.

1. Chemical Bonding
Chapter 1
Interactions of Matter

2. REVIEW
 Identify the 4 atoms whose models are on the
bulletin board.
 How did you identify these elements?

3. Electron Arrangements
Energy Level Maximum
Number of
Electrons
1 2
2 8
3 8 (then 10 more
later)
Remember
electrons
arrange in
energy levels
outside the
nucleus.

4. Electron Dot Diagrams
 Show ONLY outer level electrons
 Also called Lewis diagrams
1. Begin with the element’s symbol
2. Use the PT to determine the number of
outer level electrons
3. Place up to 2 dots per side for a total of up
to 8 electrons
 Put the first 2 dots together on one
side, then put single dots on the remaining
sides until you have to pair them

5. Electron Dot Diagrams
 Ex: 1 electron
X

6. Electron Dot Diagrams
 Ex: 2 electrons
X

7. Electron Dot Diagrams
 Ex: 3 electrons
X
Choose a clockwise or counterclockwise
direction and fill empty sides with an
electron before pairing any electrons.

8. Electron Dot Diagrams
 Ex: 4 electrons
X
Choose a clockwise or counterclockwise
direction and fill empty sides with an
electron before pairing any electrons.

9. Electron Dot Diagrams
 Ex: 5 electrons
X
Choose a clockwise or counterclockwise
direction and fill empty sides with an
electron before pairing any electrons.

10. Electron Dot Diagrams
 Ex: 6 electrons
X
Choose a clockwise or counterclockwise
direction and fill empty sides with an
electron before pairing any electrons.

11. Electron Dot Diagrams
 Ex: 7 electrons
X
Choose a clockwise or counterclockwise
direction and fill empty sides with an
electron before pairing any electrons.

12. Electron Dot Diagrams
 Ex: 8 electrons
X
THIS IS THE MOST ELECTRONS THAT EVER ARE
INCLUDED IN ELECTRON DOT DIAGRAMS.

13. Electron Dot Diagrams
 Time to practice what you’ve learned
 For the following elements, create electron dot diagrams
using M&M’s as electrons. Be sure to write large size
symbols on your paper.
 YUM, but no eating allowed until all your work is
checked and is correct!
aluminum potassium argon oxygen
phosphorus silicon barium iodine
BRING IN YOUR ATOMIC MODEL TOMORROW!

14. CHEMICAL BONDING
 The number of electrons in the ____________ energy
level determines whether an atom will form bonds.
 These electrons are also called ___________ electrons.
 Atoms bond to get a ________ outer level.
 For all E levels beyond the first, the outermost E level is
considered to be full if it contains ______ (#) electrons.
 The first E level is full with ____ (#) electrons.
 Why are noble gases nonreactive?

15. CHEMICAL BONDING
 Atoms bond by __________, ____________, or
___________ electrons to have a filled outermost
energy level containing 8 valence electrons.
 ___(#) types of bonds hold atoms together.
1. IONIC BOND- force of electrostatic attraction between 2
oppositely charged ______.
 Ions form when electrons are _________________.
2. COVALENT BOND- force of attraction between nuclei of atoms
and the electrons _______________ by the atoms.
 Neutral atoms held by covalent bonds are called
__________________.
3. METALLIC BOND- force of attraction between a ____________
charged metal ion and the electrons in a metal.

16. IONIC BONDS
 Chem 4 Kids example
METALS
•have a low/high number of valence electrons.
•metals lose/gain electrons when bonding.
•form positive/negative ions.
NONMETALS
•have a low/high number of valence electrons.
•lose/gain electrons when bonding.
•form positive/negative ions.
•ions end in –ide

17. IONIC BONDS

18. Naming IONIC compounds
Binary compounds- contain only 2 elements
 negative ion ends in -ide
 Ex: Name NaCl
 Ex: Name AlF3
 Ex: Name Li2S
 compounds are neutral so use subscripts to make (+)=(-)
 Write the chemical formula for
 Ex: strontium sulfide
 Ex: potassium oxide
 Ex: calcium chloride

19. Naming IONIC compounds
Binary compounds- containing transition elements
 Transition metals- the charge is in parenthesis
following the name of the metal except for Ag, Cd,
and Zn (see PT)
 ex: chromium (II) chloride
ex: iron (III) oxide

Ex: NiF2 vs. NiF

Ex: CrI4 vs. CrI2

20. Naming IONIC compounds
What about compounds with more than 2 elements
 Look on page 159 for polyatomic ions
 Polyatomic ions- groups of atoms that are bonded
together with a charge
 Usually end in -ate
Ex: BaSO4
Ex: potassium phosphate
Ex: iron (III) carbonate

21. IONIC BONDS- metal ion + nonmetal ion
CHARACTERISTICS OF IONIC COMPOUNDS
•Hard, brittle solids at room temp
•High melting and boiling points
•Ions are held in a crystal lattice
•Conduct electricity when dissolved in H2O

22. Quick Review
1.Barium sulfide
2.Aluminum carbonate
3.NaClO3
4.SiO2
5.Dinitrogen pentoxide

23. COVALENT BONDS
 Unlike ionic bonds with transferred electrons, covalent
bonds __________ electrons.
IONIC BOND COVALENT BOND

24. COVALENT BONDS
 Unlike ionic bonds that generally form between metals
and nonmetals, covalent bonds form between
________________.
 Classify the bonds as ionic or covalent
1. Na-Cl
2. H-O
3. C-O
4. Ca-F
5. N-N
6. Cr-S NOTE: Group 14
has a strange e-dot
diagram

25. COVALENT BONDS
 Use electron dot diagrams to model molecules
 Examples:
1. H2
2. H2O
3. NH3

26. COVALENT BONDS
 Some molecules are simple with only one element
 7 elements are not found in nature as atoms

They always are found in pairs- called diatomic
N2 O2 F2
Cl2
Br2
I2
And H2 (always the exception)

27. COVALENT BONDS
 EXAMPLES OF COVALENT COMPOUNDS
 water
 plastic
 sugar
 Gasoline oils & fats
 CHARACTERISTICS OF COVALENT COMPOUNDS
1. Do NOT conduct an electrical current
2. Low melting and boiling points
3. Lightweight molecules: generally gases and liquids at
room temp
4. Heavier molecules: generally solids at room temp

28. COVALENT COMPOUNDS
 Naming covalent compounds involves using prefixes to
indicate the number of atoms in the formula.

Website w/prefixes and rules

29. COVALENT COMPOUNDS
• When atoms share electrons, they don’t
always share them equally.
• Nonpolar covalent compounds:
share e- equally
• Will not conduct an electrical
current at all
• All diatomic molecules are
nonpolar
• Polar covalent compounds: share e-
unequally
• Can conduct an electrical current

30. COVALENT COMPOUNDS
• Polarity affects how chemicals mix.
• “Like dissolves like.”
• Nonpolar compounds mix with other
nonpolar compounds.
• Ex:
• Polar compounds mix with other polar
compounds.
• Ex:
• Nonpolar compounds will not mix with
polar compounds.
• Ex:
• How does this affect how soap is made?

31. METALLIC BONDS
 EXAMPLES CONTAINING METALLIC BONDS
 Cu, Fe
 Alloys- mixtures of metals
 EX: brass, bronze, steel
 CHARACTERISTICS OF METALS
1. Malleable & ductile
2. Good conductors
 “sea of electrons” allows metals to be shaped without
breaking
 Close metal atoms have overlapping outer E levels
 Valence electrons can move freely between positive metal
ions