Atoms and electrons

Page 1

Niels Bohr changed Rutherford´s model to incorporate newer discoveries about how the energy of an atom changes when the atom absorbs or emits the light.

-Orbits (energy levels in atoms)

-Quantum (amount of energy)

Bohr proposed that an electron is found only in specific circular paths around the nucleus.

The fix energies an electron can have are called quantums.

Page 2

A quantum of energy is the amount f energy requires to move an electron to one energy level to another.

The energy levels in atoms are unequally spaced.

The higher energy levels are closer together

The Bohr model explains how the energy levels of electrons in an atom change when the atom emits light.

Page 3

Erwin Shrodinger used new theoritical calculations and experimental results to devise and solve mathematical equations describing the behavior of the electron in hydrogen atom.

The quantum mechanical model came from the mathematical solutions to the Shrodinger equation.

The quantum mechanical model doesn´t specify the exact path of the electron around the nucleus.

<in the quantum mechanical modelthe probability of finding the electron interprets as a fuzzy cloud.

Page 4

The energy levels are labeled by (n)

Different atomic orbitals are denoted by letters.

2n times square tells you how many electrons in each energy level 2(3)uared = 2(9)= 18 electrons in the third level.

The principal quantum number n, always equals the number of sublevels within that principal energy level.

Page 5

1 s orbitals, 3 p orbitals and 5 d orbitals.