Do Now: Complete Calculating Average Atomic Mass Worksheet

YWBAT Describe what Bohr proposed in his model of the atom. Describe what the quantum mechanical model determines about the electrons in an atom. Explain how sublevels of principal energy levels differ

Revising the Atomic Model Rutherford’s atomic model could not explain the chemical properties of elements. For example, why does iron first glow dull red, then yellow, then white when heated to higher and higher temperatures?

The Bohr Model Niels Bohr (1913) Incorporated discoveries about how the energy of atoms changes when the atom absorbs or emits light. Stated that the electrons orbit the nucleus like planets orbit the Sun.

The Bohr Model Each possible electron orbit has a fixed energy known as an Energy Level Quantum of Energy Amount of energy required to move an electron from one energy level to another

The Bohr Model Bohr’s model can be compared to rungs of a ladder. Electrons cannot exist between energy levels The energy levels in atoms are unequally spaced (higher energy levels are closer together)

The Bohr Model When an electron occupies the lowest possible energy level it is said to be in its ground state. An electron can absorb energy (become excited) from an external source: – Sun – Fire (heat) – Electricity

The Bohr Model When electrons absorb energy, they can jump to higher energy levels. This is called the excited state. When the electron returns to the ground state, it releases energy in the form of light. Emission Line Spectra

The Bohr Model Scientists began wondering why the electron had to be in a specific orbit. This led to the Heisenberg Uncertainty Principle which states: At a given instant in time, it is impossible to determine both the position and the velocity of an electron

Quantum Mechanical Model Erwin Schrodinger developed and solved a mathematical equation describing the behavior of the electron in a hydrogen atom. The modern description of electrons, the quantum mechanical model, came from the solutions to the Schrodinger equation.

Quantum Mechanical Model The probability of finding an electron is represented as a fuzzy cloudlike region. The cloud is more dense where the probability of finding the electron is high. Atomic Orbital – region of space where there is a high probability of finding an electron

Quantum Numbers Used to specify properties of atomic orbitals and electrons in orbitals: 1.Principle quantum number (n) 2.Angular momentum number (l) 3.Magnetic quantum number (m l ) 4.Spin quantum number (ms)

Principle Quantum Numbers (n) Indicates the main energy level (shell) occupied by the electron Assigned values n=1,2,3,4,5,6,… Energy level corresponds to the period (row) of the periodic table – 1 st energy level = first period (n=1) – 2 nd energy level = second period (n=2)

Angular Quantum Numbers (l) Indicates the shape of the orbital L = s,p,d,f Often called the sublevel

Sublevel The number of sublevels within a principal energy level is always equal to the principal quantum number # sublevels = principal quantum number For example, n=1 has 1 sublevel (s) n=2 has 2 sublevels (s & p)

Sublevel There can be several orbital configurations within a sublevel (i.e., s,p,d,f). S - sublevel contains 1 orbital P - sublevel contains 3 orbitals D - sublevel contains 5 orbitals F - sublevel contains 7 orbitals

Sublevel Parts of the periodic table corresponds to each orbital shape (angular momentum number) Groups 1 & 2 – s block Groups – p block Groups 3-12 – d block Bottom two rows – f block

Spin Quantum Number (m s ) Indicates the spin of the electron Clockwise & Counter-clockwise A vertical arrow indicates an electron and its direction of spin. In any orbital, the spin of the 2 electrons must be opposite.

Principal Energy Levels # of orbitals in an energy level is equal to n 2 Max of 2 electrons can occupy a single orbital. The maximum number of electrons that can occupy an energy level is 2n 2

Quantum Numbers The building = atom Apartment Floors = Energy Levels (shells) Specific Apartments = Orbitals (subshells) Residents = Electrons