Uploaded on

 

More in: Technology
  • 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
587
On Slideshare
0
From Embeds
0
Number of Embeds
0

Actions

Shares
Downloads
16
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. Atomic Structure
  • 2. The atom
    • Def: the smallest particle of an element that retains its identity in a chemical reaction.
    • Atoms are tiny!
      • If you lined up 100,000,000 copper atoms side by side, they would produce a line only 1 cm long.
  • 3. Initial Thoughts
    • Democritus – atoms are indivisible and indestructible
    • Dalton modified this theory through research. He determined that:
      • 1.elements are composed of tiny indivisible particles called atoms
      • 2.atoms of the same element are identical
      • 3.atoms can combine to form compounds
      • 4.chemical reactions occur when atoms are separated from their compounds
    • Thompson was the first to discover that atoms contain subatomic particles
  • 4. Subatomic Particles Particle Location Charge Mass Proton (p + ) 1.67 x 10 -28 g Neutron (n o ) 1.67 x 10 -28 g Electron (e - ) negligible
  • 5. Using the Periodic Table
    • How do I determine the number of protons?
    • How do I determine the number of electrons?
    • How do I determine the mass number?
    • How do I determine the number of neutrons?
    • Practice on your own
  • 6. Isotopes
    • Isotopes of an element have the same number of protons but different number of neutrons
    • Ex: Lithium -7 and Lithium-6
    • Draw Bohr models of Carbon-12 and Carbon-13
    • Why does mass number (protons + neutrons) differ from atomic mass (the number you find on the periodic table)?
      • (pg 114)
  • 7. Electrons
    • According to the discovery Bohr made, electrons are found in orbitals (or energy levels) surrounding the nucleus
    • 1 st energy level – can hold 2 electrons
    • 2 nd energy level– can hold 8 electrons
    • 3 rd energy level – can hold 18 electrons
  • 8. Valence Electrons
    • The number of valence electrons can be determined by looking at the Roman Numeral at the top of each group (or family) or the periodic table.
    • The number of valence electrons can give us hints about the reactivity of that element
      • Metals lose valence electrons to form cations
      • Non-metals gain valence electrons to form anions
      • Pg 162
  • 9. Rutherford’s Gold Foil Experiment
    • Proposed that:
      • the atom is mostly empty space
      • the nucleus is concentrated in the center of the atom
      • Think of a dime in the middle of football field
      • Demo 1
  • 10. In-class assessment
    • You have the next 2o-25 minutes to complete an open notebook quiz.
  • 11. HW
    • Section 4.1 review worksheet – due Thursday
    • Section 4.2 review worksheet – due Friday