Models of the Atom

Goals for this Lesson Recognize that there are 3 different models for the atom DO NOT NEED TO KNOW MANY SPECIFICS!! Decipher the 4 different atomic orbital shapes Be able to know, in general, what they look like and how many shapes there are for each orbital Recall how many electrons can fit in each atomic orbital

Rutherford’s Model of the Atom Great at showing the relationship between protons, neutrons and electrons Lacking a major detail Couldn’t show the chemical properties of elements Example Why, when heated, metals turn red, than orange, than yellow, than white Need a better model to show these properties

Neils Bohr and the Bohr Model Danish physicist Student of Rutherford What he proposed (used the Hydrogen atom for his experiment = 1 e-) Electrons exist in specific circular paths, or orbits, around the nucleus Each electron orbit has a fixed energy Energy level Electrons can jump from one energy level to the next

The Bohr Model What it did not prove What happens with an element that has more than 1 electron? Do the electrons collide, do they dance with each other? Bohr’s Model couldn’t predict this

Quantum Mechanical Model The amount of energy it takes to propel an electron from one energy level to the next Erwin Schrodinger Used math to figure out the energy levels of electrons Where electrons are at any given point in time What did Schrodinger prove? Electrons exist in clouds around the nucleus Used math to say what the probability it is to find an electron in any specific area of the cloud

Quantum Mechanical Model What does the quantum mechanical model prove? Gives you the energy levels of the electrons Tells you where each electron is for any element Located in the energy levels (the quantum levels) Explains why elements have certain chemical properties We excite electrons up and down energy levels

Goals From Now On! Decipher the 4 different atomic orbital shapes Recall how many electrons can fit in each atomic orbital

Take a Deep Breath Energy Levels Within each energy level There are 4 energy levels n = 1, 2, 3, or 4 Within each energy level We have atomic orbitals The region of space where there is a high probability you will find an electron 4 Atomic orbitals (also called sublevels) s orbital p orbital d orbital f orbital

s orbital

p orbitals

d orbitals

f orbitals

Energy Levels Energy Level 1 ( n =1) Energy Level 2 (n = 2) s orbital (1 shape) 2 possible electrons in this level Energy Level 2 (n = 2) s orbital (1 shape) and p orbitals (3 shapes) 2 possible electrons in the s orbital 6 possible electrons in the p orbital 8 total

Energy Levels Energy Level 3 ( n = 3) Energy Level 4 ( n = 4) s orbital (1 shape), p orbitals (3 shapes) and d orbitals (5 shapes) 2 electrons in the s orbital 6 electrons in the p orbital 10 electrons in the d orbital 18 total Energy Level 4 ( n = 4) s orbital (1 shape), p orbitals (3 shapes), d orbitals (5 shapes), and f orbitals (7 shapes) 14 electrons in the f orbital 32 electrons