chapter 5 electrons in atoms chemistry section 5.1 light and quantized energy at this point in...

Chapter 5

Electrons in AtomsChemistry

Section 5.1 Light and Quantized Energy

• At this point in history, we are in the early 1900’s. Electrons were the 1st subatomic particle to be discovered.

• Chemists have a Rutherford Model of the atom. There is a small, dense, positively charged center of the atom called a nucleus. Electrons move around outside the nucleus.

The Atom and Unanswered Questions

• In Rutherford's model, the atom’s mass is concentrated in the nucleus and electrons move around it.

• The model doesn’t explain how the electrons were arranged around the nucleus.

• The model doesn’t explain why negatively charged electrons aren’t pulled into the positively charged nucleus.

• In the early 1900s, scientists observed certain elements emitted visible light when heated in a flame.

• Analysis of the emitted light revealed that an element’s chemical behavior is related to the arrangement of the electrons in its atoms.

The Wave Nature of Light

• Visible light is a type of electromagnetic radiation, a form of energy that exhibits wave-like behavior as it travels through space.

• All waves can be described by several characteristics.

• The wavelength (λ) is the shortest distance between equivalent points on a wave.

• The frequency (ν) is the number of waves that pass a given point per second.

• The amplitude is the wave’s height from the origin to a crest.

What relationship do you see between λ, v, and c?

• The speed of light (3.00 108 m/s) is the product of it’s wavelength and frequency.

c = λν

What relationship do you see between λ and ν?

• Sunlight, or visible light, contains a continuous range of wavelengths and frequencies.

• A prism separates sunlight into a continuous spectrum of colors – pg. 138.

• The separation of white light by a prism• The electromagnetic spectrum includes all

forms of electromagnetic radiation – pg. 139.

The Electromagnetic Spectrum

Visible Light …

Note the trends: Blue light has shorter λ, higher v, andmore energy. Red light has longer λ, lower v, and lessenergy.

Brain Pop - The EM Spectrum

• The wave model of light cannot explain all of light’s characteristics.

• An example is the photoelectric effect , when electrons are emitted from a metal’s surface when light of a certain frequency shines on it (how solar calculators work).

• Photoelectric Effect Simulation

• Albert Einstein proposed in 1905 that light has a dual nature.

• Einstein suggested a beam of light has wavelike and particlelike properties.

• A photon is a particle of electromagnetic radiation with no mass that carries a quantum of energy.

Ephoton = h

Ephoton represents energy, h is Planck's constant (6.626 x 10-34 J-s), & represents frequency.

Atomic Emission Spectra • Light in a neon sign is produced when

electricity is passed through a tube filled with neon gas and excites the neon atoms.

• The excited atoms emit light to release energy.

Emission Spectrum for Hydrogen

• The atomic emission spectrum of an element is the set of frequencies of the electromagnetic waves emitted by the atoms of the element.

• Each element’s atomic emission spectrum is unique – they have their own fingerprints!

Absorption and Emission Spectra's

Section 5.2 Quantum Theory and the Atom

Bohr's Model of the Atom…• Bohr suggested that an

electron moves around the nucleus only in certain allowed circular orbits - Planetary Atomic Model.

• The lowest allowable energy state of an atom is called its ground state.

• When an atom gains energy, it is in an excited state.

Planetary Atomic Model

Bohr Model

• Bohr assigned a quantum number for each principal energy level.

• The highest quantum number can be found by the period the element is in on the Periodic Table.

• He tried to predict the spectral lines for elements following Hydrogen, but was not successful.

• The behavior of electrons is still not fully understood, but it is known they do not move around the nucleus in circular orbits.

Big Discoveries…• Louis de Broglie

hypothesized that particles, including electrons, could also have wavelike behaviors.

• Werner Heisenberg showed it is impossible to take any measurement of an object without disturbing it.

• The Heisenberg uncertainty principle states that it is fundamentally impossible to know precisely both the velocity and position of a particle at the same time.

• The only quantity that can be known is the probability for an electron to occupy a certain region around the nucleus.

Our Current Atomic Theory…

• Erwin Schrödinger treated electrons as waves in a model called the quantum mechanical model of the atom. Most people call this the Electron Cloud Model.

• This model applied to all elements!!!

• The Electron Cloud is a 3-D arrangement of electrons around the nucleus.

• Within the cloud, electrons are arranged by energy level, sublevel, and orbital shape.

• When combined, a spherical shape is the result.

• There is an attraction between the positively charged nucleus and the negatively charged electrons in the electron cloud.

Orbital Shapes…

Section 5.3 Electron Configuration

Valence Electrons• Valence electrons are defined as electrons

in the atom’s outermost orbitals—those associated with the atom’s highest principal energy level.

• An element’s valence electrons determine the chemical properties of the element.

• The number of valence electrons can be found using its group number on the periodic table.

• Electron-dot structure consists of the element’s symbol representing the nucleus and inner electrons, surrounded by dots representing the element’s valence electrons.