chapter 5 notes atomic theory look at the photographs on the next pages and tell me how they are all...
TRANSCRIPT
Chapter 5 Notes
Atomic Theory
Look at the photographs on the next pages and tell me how they
are all similar?
• They all are practical applications of Atomic Emission by Excited Electrons!• It’s this principle that helped
Bohr formulate his model of the atom.
Atomic Emission: How It Works
1. Normally, electrons are in the lowest energy levels (closest to the nucleus) called the ground state,
2. Electrons can absorb energy. The energy can be heat energy (a fire), or chemical energy (battery), or electrical energy (an outlet).
3. When an electron absorbs energy, it "jumps" to a higher energy level, and spins in the higher energy level called the excited state.
4. When the electron ‘falls’ back to the lower energy level, it emits (gives off) energy of specific wavelengths (lines) of LIGHT!
5. When the light is looked at through a prism or diffraction grating, bands of colored light can be seen called Bright-Line Spectra or simply Line Spectra.
6. Each element’s spectra is unique and can be used to identify it just like your fingerprints identify you!
Ground vs Excited State Notes
Ground State = electron in lowest energy state
Excited State = electron in higher energy state
Ground State Excited State
Ground State Excited State
Line Spectra – Unique bands of color emitted when excited electrons return to the ground state.
Electron GAINS energy & jumps to a higher energy level
Electron EMITS light energy & falls to a lower energy level
Backgound Only(Don’t copy to notes)
• Hot objects give off light. • When the light from a light bulb passes through
a prism, a RAINBOW or CONTINUOUS SPECTRUM forms.
• Remember ROY G. BIV?Red, Orange, Yellow, Green, Blue, Indigo, Violet
•
When the light from an element gas tube passes through a prism, only some colors are seen – called a BRIGHT-LINE SPECTRUM.
Gas Tube Power Supply Hydrogen gas gives off pink light
Hydrogen’s Bright Line Spectrum as viewed through a prism
Often Shown This Way
This site shows the Line Spectra of Various Elementshttp://jersey.uoregon.edu/elements/Elements.html
Repeat
White light forms a Continuous Spectrum (Rainbow).
Each element has unique spectra that can be used to identify it – Bright-Line Spectra or Line Spectra or Emission Lines.
Electron Configuration & Bohr ModelsHow to tell if its for the Ground or Excited state?
For Ground State1) Periodic Table is for ground state.2) The maximum # of electrons that can fill each
successive shell is 2, 8, 18, 32 (2n2).3) Fill one shell before filling the next.4) Some exceptions: So count up electrons to
figure out the atomic number and see if its on the PT. If NOT on PT, it’s excited state.
Practice: Excited or Ground
1) 2 – 3
2) 2 – 8 – 6 – 1
3) 2 – 8 – 8 – 2
4) 2 – 8 – 14 – 2
5) 2 – 8 – 2 – 1
Bohr Model for Boron
Ground State 10.81 +3 Excited State
5 B
5 p+6 no
5 p+6 no
2- 3
Electron Configuration 2-3 Electron Configuration 2 - 2 -1
Do you know:
• Difference between excited and ground state?• How atoms become excited?• How atoms return to ground state?• Why spectra lines are important?• Ground or excited state? 2 – 5 – 1 Why?