4-1 Ions & Ionic Bonding

  • 791 views
Uploaded on

 

  • 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
791
On Slideshare
0
From Embeds
0
Number of Embeds
0

Actions

Shares
Downloads
14
Comments
0
Likes
0

Embeds 0

No embeds

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. Warm-Up
    • Which metals are the most reactive?
      • Alkali metals
    • Which non metals are the most reactive?
      • Halogens
    • Why don’t metals in group 1A have identical properties?
      • Elements in group 1A don’t have identical properties because their valence electrons are in different energy levels.
  • 2. 4-1 Ions & Ionic Bonding
    • Recognize stable electron configurations.
    • Predict an element’s chemical properties using number of valence electrons and electron dot diagrams.
  • 3. Stable Electron Configuration
    • The highest occupied energy level of an atom is filled with electrons.
    • Nobel gases have 8 valance electrons (He-2).
    • The highest energy level is completely full.
    • Noble gases are colorless, odorless, and un-reactive .
      • Very few compounds form with Nobel gases.
  • 4.  
  • 5. Electron-Dot Diagram
    • A model of the atom to represent the valence or outer shell electrons.
    • The number of dots = number of valence electrons.
    • The symbol in the center represents the nucleus and all other electrons.
    • Electron dot diagram helps to determine stability.
  • 6.  
  • 7. Formation of Ions
    • Atoms that lose or gain electrons are called ions .
    • Ions are charged atoms.
    • Ions have unequal numbers of protons and electrons.
    • Charge can be positive or negative.
    • Ions are formed because atoms want to have a stable electron configuration.
  • 8. Types of Ions
    • Positive ions
      • Lose electrons or lose negative charge.
      • Subtracting negatives = positives.
      • Atoms that have lost electrons are called cations (“cat-ions”)
      • Metals
    • Negative Ions
      • Gain electrons or gain negative charge.
      • Atoms that have gained electrons are called anion (“ant-ion”).
      • Nonmetals
  • 9. Na + Al 3+ K + Mg 2+ Ca 2+
  • 10. N 3- F - P 3- O 2- S 2- Cl -
  • 11. Ionic Bonds
    • Chemical bonds is a force that holds atoms together as a unit.
      • Ionic bonds are the cations being attracted to the anions
      • Particles with opposite charges are attracted.
    • Ionic bonds are formed when atoms transfer electrons from one atom to another.
  • 12.  
  • 13.  
  • 14. Ionic Compounds
    • Compounds are substances that contain more that one atom in chemical ratios.
    • The ratio is known as the chemical formula.
    • Ions don’t bond in random ways.
    • Ion will bond with the number of atoms to give a full shell of electrons.
    • Ions also bond to balance charges.
  • 15. Summary
    • What happens to atoms when they form ionic bonds?
      • One atom in the compound had to loose an electron and one atom in the compound had to gain an electron.
    • What type of elements form ionic bonds?
      • Metal and nonmetal