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Unit 3 Electron configurations. Part B Bohr’s Model of Hydrogen. Discharging Tubes. What have we learned so far?. The Flame Test. The light coming out of the excited atomic entities is very specific to particular element! Results are quite reproducible.

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Unit 3 electron configurations

Unit 3 Electron configurations

Part B

Bohr’s Model of Hydrogen


What have we learned so far

Discharging Tubes

What have we learned so far?

The Flame Test

The light coming out of the excited atomic entities is very specific to particular element!

Results are quite reproducible.


Unit 3 electron configurations

Electromagnetic radiations (lights) coming out or being absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).

No nuclear changes have ever been observed indicate that the energy changes have to come from electrons surrounding the nucleus.


Unit 3 electron configurations

How Come? absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).

Classic Model:

Electron anywhere it ‘wants’ to be

Problems with classic model:

E moving through electric field will emit light & from the classic model, emitted light should have differing wavelengths


Unit 3 electron configurations

Niels Bohr absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).(1885 – 1962)

Increasing energy with

greater distance from nucleus


Bohr s model of hydrogen atom

} absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).

Bohr’s Model of Hydrogen Atom

Fifth-excited

  • Further away from the nucleus means more energy.

  • There is no “in between” energy

  • Energy Levels

Fourth

Third

Increasing energy

Second

First-ground

Nucleus


Bohr s model of hydrogen atom1
Bohr’s Model of Hydrogen Atom absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).

quantum– quantity of energy gained or lost by an atom when electrons are excited

photon– a quantum of light

ground state – lowest energy level of an atom

excited state – a heightened state of energy in an atom

Electrons of hydrogen circle the nucleus in orbits

1. orbits have a fixed amount of energy in the ground state.

2. orbits are a fixed distance from the nucleus.

3.orbits furthest from the nucleus have the greatest energy.


Bohr s model of hydrogen atom2
Bohr’s Model of Hydrogen Atom absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).


Bohr s model of hydrogen atom3
Bohr’s Model of Hydrogen Atom absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).


Bohr s model of hydrogen atom4
Bohr’s Model of Hydrogen Atom absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).


Unit 3 electron configurations

Bohr’s Model of Hydrogen absorbed by atoms indicate that there are very specific energy changes within the atomic entities (atoms and ions).Atom

Orbits

Transitions of e between those orbits involve change in energy

Change in energy (E(n2 –n1) has to be accounted for

By photons

Successful in accounting for most of the H-1 emission/absorption spectral lines

BUT only works for H-1