Ionic Bonding 2008
Upcoming SlideShare
Loading in...5
×

Like this? Share it with your network

Share
  • Full Name Full Name Comment goes here.
    Are you sure you want to
    Your message goes here
    Be the first to comment
    Be the first to like this
No Downloads

Views

Total Views
679
On Slideshare
675
From Embeds
4
Number of Embeds
2

Actions

Shares
Downloads
14
Comments
0
Likes
0

Embeds 4

http://acker.pbwiki.com 3
http://www.slideshare.net 1

Report content

Flagged as inappropriate Flag as inappropriate
Flag as inappropriate

Select your reason for flagging this presentation as inappropriate.

Cancel
    No notes for slide

Transcript

  • 1. Chemical Bonds: Ionic Bonding Parts 4.2 & 4.3
  • 2. Goal 1 Understand the basis of and describe the characteristics of ionic bonding
  • 3.
    • Why bond?
      • Full outer shell
      • Valence electrons
  • 4.
    • Full outer shell
      • H  2 e-
      • All others  8 e-
      • Happy!
  • 5.
    • Recall Ion formation
      • Gain or loss of electron
      • Gain electron = “-” charge
      • Lose electron = “+” charge
  • 6.
    • Characteristics of Ionic Bonds
      • Metal bonded with nonmetal
  • 7.
      • Forms “ionic compounds” aka “salts”
  • 8.
      • ** TRANSFER ** electrons
        • Metals Give (+ charge)
        • Non-metals Receive (- charge)
  • 9.
      • Conducts electricity only
        • In solution
        • As liquid
      • Because of electron movement
  • 10. Goal 2 Determine the chemical formula of an ionic compound by using the charge on each ion
  • 11.
    • Metals give away electrons (+ charge)
      • Recall how to determine charge…
      • Group #
      • Energy levels
      • Li  1+
      • Mg  2+
      • Ca  ___
      • K  ___
  • 12.
    • Nonmetals receive electrons ( - charge)
      • Recall how to determine charge
      • 8 electrons
      • Group #
      • Energy level
      • F  1-
      • O  2-
      • P  ___
      • Br  ___
  • 13.
    • Ionic compounds strive for combined neutral (0) charge
      • Neutral charge = 0 charge
      • Combined ions = 0 charge
      • Sum of charges must = 0
  • 14.
    • Try it…
      • Na  1+
      • Cl  1-
      • How many of each to = 0 charge?
  • 15.
      • Na 1+ and Cl 1- = 0 charge
      • (The charges should add to 0)
      • One sodium ion + One chlorine ion = 0 charge
      • Chemical formula is
      • NaCl
  • 16.
    • That was fun!
    • Let’s try it again!!
  • 17.
      • Mg  2+
      • Cl  1-
      • How many of each to = 0 charge?
  • 18.
      • Mg 2+ and Cl 1- = 1+ charge
      • (2) + (-1) = 1
      • Uh Oh!!!
      • One Magnesium ion + One chlorine ion = 1+
  • 19.
      • Mg 2+ and Cl 1- and Cl 1- = 0 charge
      • 2 + (1-) + (1-) = 0
      • For every one magnesium ion, we need two chlorine ions
      • Chemical Formula
      • MgCl 2
  • 20.
    • Your turn…
    • What is the chemical formula for an ionic compound of
    • potassium
    • and
    • sulfur ?
  • 21.
    • K 2 S
    • Were you correct?
  • 22.
    • Try some more
    • Sodium and Phosphorus
    • Lithium and Nitrogen
    • Strontium and Bromine
  • 23.
    • Ask Ms. Acker about the
    • Criss - Cross
  • 24. Goal 3 Name ionic compounds
  • 25.
    • Step one:
      • Say the metal
    • Step two:
      • Say the nonmetal with an “ ide” ending
  • 26.
    • NaCl = Sodium Chlor ide
    • KCl = Potassium Chlor ide
    • MgCl 2 = Magnesium Chlor ide
    • KF = _________________
    • Li 2 S = __________________
    • ______= Beryllium Sulf ide
    • ____ = Sodium phosph ide
  • 27. Goal 4 Use electron dot structures to show ionic compound formation
  • 28.
    • It’s all about the valence electrons
    • Metals give (away extras)
    • Nonmetals receive (to fill outer shell)
    • Ms. Acker will now show you on the board
    • Please take note