Quantum Mechanical Model of the Atom- Introduction

Quantum Mechanical Model of the Atom

Introduction

Following this presentation, you should be able to:

• Explain how electrons are organized in the atom

• Describe energy levels, sublevels, and orbitals in an atom

• Draw a representative shape of each sublevel

• Determine the maximum number of electrons in each energy level, sublevel, or orbital

Basic Atom

• Shows electrons in orbits

• Not entirely correct, but easy to understand

Principal Energy Levels

• designated as "n", so n = 1, n= 2, n=3, etc.

• Represents the average distance of an electron from the nucleus

• The lower the number, the closer to the nucleus

Multiple Choice

Which energy level has a higher energy?

• n = 2

• n = 4

• n = 1

• n = 3

These are areas where the electrons can exist

Sublevels

• Each energy level is divided into sublevels

• 3-D areas where the electron can exist in the atom

• Labeled as s, p, d, f, and other letters where an electron can jump to if enough energy is added

• n = 1: 1 sublevel, n = 2: 2 sublevels, etc

Multiple Choice

How many sublevels would the 4th energy level have?

• 1

• 2

• 3

• 4

Energy Levels and Sublevels:

• n = 1: 1 sublevel---s

• n = 2: 2 sublevels---s & p

• n = 3: 3 sublevels---s, p, & d

• n = 4: 4 sublevels: s, p, d, & f

• n = 5: 5 sublevels: s, p, d, f, & g but no electrons are in g in ground state

• the sublevels have different energies: s<p<d<f in energy

Atomic Orbitals

• Each sublevel has an orientation in space, each of these orientations are called an atomic orbital

• Each orbital can hold a maximum of 2 electrons

Open Ended

If the 3rd energy level has s, p, and d sublevels, what is the maximum number of electrons that can fit in this level?