Pre-Class Activity 12/1

Pass around the box. “Examine” what is inside without opening the box. Try to figure out what is in the box. What observations did you make to come to this conclusion?

Section 5.1 Homework Quiz Wednesday 12/3

Unanswered Questions

Rutherford’s model did not address the following questions:

1. What is the arrangement of electrons in the atom?

2. What keeps the electrons from converging on the nucleus?

3. What accounts for the differences in chemical behavior among elements?

Chemical Behavior Related to the Arrangement of Electrons

In the early 1900’s scientist observed that when they heated elements in a flame, the elements emitted colored light. Analysis of the light led scientist to determine that the arrangement of electrons in an atom is related to the elements chemical behavior.

Understanding Light – Characteristics of Waves

CA

1 sec

D

E

Using the word bank below, match the words to the lettered parts of the diagram

B = 3/s

Frequency Amplitude Peak Trough Wavelength

Waves Characteristics

Wavelength () the shortest distance between two equivalent points on a wave.

(unit of measure: meters, centimeters, or nanometers)

Frequency (v) the number of waves that pass a given point per second.

(unit of measure: Hz, waves/second, /s, s-1)

c v

Waves

c=v

Speed of Light ( c )

Relationship Between Wavelength and Frequency

c=vF

requ

enc

y

Wavelength

Problems

What is the wavelength of a wave that has a frequency of 7.8 x 1010Hz?

What is the frequency of a wave that has a wavelength of 6.5 x 10-4cm?

Pre-Class Activity 12/2

Which of the following waves has the longest wavelength? Which has the greatest frequency?

5.1 Quiz tomorrow, Atomic Emission Spectroscopy Lab on Thursday

Electromagnetic Spectrum

Electromagnetic radiation – Form of energy that exhibits wave-like behavior.

Electromagnetic spectrum – encompasses all forms of electromagnetic radiation. The only differences between each form is their characteristic wavelengths and frequencies.

White Light – a continuous spectrum of colors, each with a unique wavelength and frequency.

Particle Nature of Light

Concept developed to explain why only certain frequencies of light are given off by heated objects and why metals will eject electrons from their surface when certain frequencies of light is shine on them.

Max Planck and the Quantum

By examining the light emitted by glowing objects, Planck concluded that matter can gain and lose energy in only small specific amounts called quanta

Quantum – the minimum amount of energy that can be gained or lost by an atom.

Tem

pera

ture

Energy

Tem

pera

ture

Energy

Planck Continued

Equantum=hvE = energy

h = Planck’s constant=6.626 x 10-34J

V = frequency

Relationships between wavelength, frequency and Energy

Fre

que

ncy

Wavelength

En

erg

y

FrequencyE

ner

gy

Wavelength

Photoelectric Effect

Electrons are emitted from a metal’s surface when light of a certain minimum frequency of 1.14 x 1015 Hz shines on the surface.

(Conversion of light energy to electrical energy)

Einstein’s Contribution

Ephoton=hv

Explained that electromagnetic radiation behaves both like waves and particles.

Photon – a particle of electromagnetic radiation with no mass that carries a quantum of energy.

Bohr Model of the Atom

Lowest allowable energy level = ground state

Electrons move around the nucleus in only certain allowable circular orbit

Each orbit is associated with a certain amount of energy

The larger the orbit (farther away from the nucleus) the greater the energy

Line Spectra

Electrons as Waves (Louis de Broglie)

Each energy level represents multiples of a whole wavelength

de Broglie proposed the idea that all particles have wavelengths

mv

h

Heisenberg Uncertainty Principle

Premise: It is impossible to make any measurement on an object without disturbing the object.The position of electron can be determined by shooting photons at electrons in an atom

It is impossible to know precisely both the velocity and position of a particle at the same time

Quantum Mechanical Model

Like Bohr, electrons energies are limited to a certain value

Unlike Bohr, electrons do not travel in prescribed paths.

Electrons travel within a particular volume of space surrounding the nucleus

Organization of Electrons in an Atom

Energy Levels n=1,2,3,4,5,6,7 Energy levels increase as distance from the

nucleus increases

Sublevels (s,p,d,f) Corresponds to the shape of the atoms orbitals

Ground-State Electron Configuration

Arrangement of electron in an atom at rest The lowest energy arrangement is the

most stable

Three Rules that govern how electrons can be arranged in an atom:

Aufbau Principle (each electron occupies the lowest energy orbital available)

Pauli Exclusion Principle (A maximum of two electrons can occupy a single orbital)

Hund’s Rule (Electrons with the same spin must occupy each orbital before electrons with opposite spins can occupy each orbital)

Orbital Filling Diagram

Electron Configuration

Fluorine (atomic #9)

2 2 5

Orbital Diagram

Nobel Gas Configuration

To shorten the amount of writing required to represent the configuration of elements with large numbers of electrons, the symbol for the noble gas that directly precedes an element can represent all of the electrons up to that point.

1s2 2s2 2p6 3s2 3p6 4s2 [Ar] 4s2

Long Hand Short Hand

Exceptions to Predicted Configurations