Chapter 11 Modern Atomic Theory

Jelani Onigbinde

Electron Behavior

  • Arrangement of electrons on their behavior
  • Need to look at energy and light to understand electron behavior
  • Light can act as a with a frequency and a wave length
Arrangement- the action, process, or result of arranging.

Behavior-the way on which one acts or conducts oneself

Energy- strength and vitality for sub stained

Light- the natural agent that stimulates sight and makes things visible

Wave- move one's hand to and fro in getting or as an sign

Frequency- the rate at which something occurs or is repeated over a particular period of time or in a given sample

Wave-length- the distance between successive crest of a wave, esp points. Physical or mental activity.

Copper= blue/green color in flame

Energy change (high to low) corresponds to a produces colors in the visible region of the electromagnetic spectrum

Unique pattern for every element


Quanzed-energy levels only have certain values and we see their different color patterns


Atoms organized like ladders

Rungs= placement of electrons

Niels Bohr


Bohr created a model of the atom that accounted for this energy

Orbitals- electrons exist in their own orbits


Electron Configurations


S=sphere

Maximum of 2 electrons per s orbital

p=dumbbell shape-only 3 per level beginning at level 2

Maximum of 6 electrons in the p orbitals

Maximum of 10 electrons for the d orbitals

Maximum of 14 electrons for the f orbitals

Arrow/Orbital/Spin Configuration

  • May have un-shared pairs of electrons
Valence Electrons

last s and p

Periodic Trends

  • Malleable change shape without breaking
  • Ducle- can be draw into a wire
  • Conduct heat
  • Conduct Electricity
  • Found on the Le of the staircase
Periodic Trends

Found on right of staircase

  • Silicon, germanium, arsenic, anmony, tellurium, polonium, and astane.

Ionization Energy= energy required to remove an electron


Electronegativity- the ability to gain or lose an electron when bonding.