Physical Science Chapter 4.3 Modern Atomic Theory
Energy levels
1st energy level= 2 electrons (max) 2nd energy level=8 electrons(max) 3rd energy level=8 electrons (max)
Erwin Schrodinger(1926$
Agreed with Niels Bohr that electrons occupied different energy levels He did not believe that electrons moved in perfect circular orbits Electron cloud model
Exited state
Any unstable electron configuration in which electrons jump to higher eneryblevels( usually as a result of heating)
Electron cloud
Electrons are free to move within less restricted orbital "regions"
The colors of the different flames produce because
Electrons heat up, enter an excited state and jump to higher levels
valence electrons
Electrons on the outermost energy level of an atom
Electrons cannot go in between
Energy levels
Niels Bohr (1913) •Believed that electrons moved around the nucleus in fixed orbits at constant speed. •The arrangement of electrons orbits was different for each element. •Under certain conditions electrons could jump from one energy level to another.
He called the orbits energy levels
Electrons orbitals furthest from the nucleus have the
Highest energy
valence electrons are the furthest from the nucleus and have the
Highest energy of all the electrons in an atom
valence electrons play a key role in chemical reactions and are responsible for
How elements combine to form compounds
Electrons orbitals closest to the nucleus have the
Lowest energy
An example of Bohr's model is
Most like a family : a mother, father and their child
ground state
The most stable electron configuration in which all the electrons are i the lowest possible Energy level
Each flame will produce a different color light because
each has a different electron configuration