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