Electronegativity, Bond Type and Drawing Lewis Structures

1,299 views
723 views

Published on

Great graphics depicting how electronegativity affects bond type and Lewis structure of compounds, including a table comparing/contrasting ionic, covalent and metallic bonds with a guided notes, blank chart for students.

Published in: Education
0 Comments
0 Likes
Statistics
Notes
  • Be the first to comment

  • Be the first to like this

No Downloads
Views
Total views
1,299
On SlideShare
0
From Embeds
0
Number of Embeds
1
Actions
Shares
0
Downloads
7
Comments
0
Likes
0
Embeds 0
No embeds

No notes for slide

Electronegativity, Bond Type and Drawing Lewis Structures

  1. 1. Difference in Electronegativity Affects the Bond Type Electronegativity differences between bonding elements is used to predict the bond type. H2 – Electronegativity difference = 2.20 – 2.20 = 0 so a Covalent bond is formed. HF – Electronegativity difference = 4.00 – 0.96 = 3.04 so an Ionic bond is formed ELECTRONEGATIVITY DIFFERENCE Ionic Bonds • Held together by electrical attraction •Strong; hard to break Covalent Bonds • Held together by shared electrons • Not as strong
  2. 2. 4 Step Process: Drawing Lewis Dot Structures Key consideration – The octet rule Step 1: Arrange atoms • Central atom lower electronegativity Step 2: Add up the valence electrons of all atoms Step 3: Draw single bonds • Subtract 2 electrons for each single bond from total counted in Step 2 Step 4: Deal out remaining electrons • Satisfy octet rule (except for Hydrogen)
  3. 3. Comparing and Contrasting Ionic and Covalent Bonds Ionic Bond Electrons Bond Electronegativity Differences State Melting Pt. Conductivity Water Solubility Covalent Bond

×