Chemistry Chapter 5Chemistry Chapter 5Electrons in AtomsElectrons in Atoms

The 1998 Nobel Prize in Physics was awarded "for the discovery of a new form of quantum fluid with fractionally charged excitations." At the left is a computer graphic of this kind of state.

Electrons in AtomsElectrons in Atoms

•Thomson – plum pudding•Disproven

•Rutherford – •Bohr

The Puzzle of the AtomThe Puzzle of the Atom   Protons and electrons are attracted to each

other because of opposite charges

  Electrically charged particles moving in a curved path give off energy

  Despite these facts, atoms don’t collapse

So why didn’t the atom collapse??

Why doesn’t the electron lose energy as it orbits???

• Hold onto your spectral tubes!!

• The answer actually has to do with light and other electromagnetic radiation.

Wave-Particle DualityWave-Particle DualityJJ Thomson won the Nobel prize for describing the electron as a particle.

His son, George Thomson won the Nobel prize for describing the wave-like nature of the electron.

The electron

is a particle!

The electron is an energy

wave!

So there was a difference in opinion between a father and son. Has this ever happened to you?

Electrons have properties of

Waves and Particles

So father and son BOTH right!!

Confused??? You’ve Got Confused??? You’ve Got Company!Company!

“No familiar conceptions can be woven around the

electron; something unknown is doing we

don’t know what.”

Physicist Sir Arthur Eddington

The Nature of the Physical World

1934So even the smart dudes were baffled

The Wave-like ElectronThe Wave-like Electron

Louis deBroglie

The electron propagates through space as an energy

wave. To understand the atom, one must

understand the behavior of

electromagnetic waves.Ok …. so in order to argue with my dad I need to understand light?

Maybe I should learn about light

c = C = speed of light, a constant (3.00 x 108 m/s)

= frequency, in units of hertz (hz, sec-1)

= wavelength, in meters

Electromagnetic radiation Electromagnetic radiation propagates through space as a wave propagates through space as a wave moving at the speed of light.moving at the speed of light.

Types of electromagnetic radiation:Types of electromagnetic radiation:

E = h EE = Energy, in units of Joules (kg·m= Energy, in units of Joules (kg·m22/s/s22))

hh = Planck’s constant (6.626 x 10-34 J·s)= Planck’s constant (6.626 x 10-34 J·s)

= frequency, in units of hertz (hz, sec= frequency, in units of hertz (hz, sec-1-1))

The energy (The energy (E E ) of electromagnetic ) of electromagnetic radiation is directly proportional to radiation is directly proportional to the frequency (the frequency () of the radiation.) of the radiation.

Long Wavelength

= Low Frequency

= Low ENERGY

Short Wavelength

= High Frequency

= High ENERGY

Wavelength TableWavelength Table

…produces all of the colors in a continuous spectrum

Spectroscopic analysis of the visible of the visible spectrum…spectrum…

…produces a “bright line” spectrum

Spectroscopic analysis of the Spectroscopic analysis of the hydrogen spectrum…hydrogen spectrum…

This produces bands of light with definite wavelengths.

Electron Electron transitionstransitionsinvolve jumps of involve jumps of definite amounts definite amounts ofofenergy.energy.

Spectral tubes, flame tests and fireworks…all colored by electrons changing energy levels.

The Bohr Model of the AtomThe Bohr Model of the Atom

Neils Bohr

I pictured electrons orbiting the nucleus much like planets orbiting the sun.But I was wrong! They’re more like bees around a hive.

WRONG!!!

  Standing waves do not propagate through space   Standing waves are fixed at both ends  

Only certain sized orbits can contain whole numbers of half wave lengths.

The electron as a standing The electron as a standing wave:wave:

Quantum NumbersQuantum Numbers

Each electron in an atom has a unique set of 4 quantum numbers which describe it.

Principal quantum number (n) Angular momentum quantum number (l) Magnetic quantum number (m) Spin quantum number

Pauli Exclusion PrinciplePauli Exclusion Principle

No two electrons in an atom can have the same four quantum numbers.

Wolfgang Pauli

Principal Quantum NumberPrincipal Quantum NumberGenerally symbolized by n, it denotes the shell (energy level) in which the electron is located.

Number of electrons that can fit in a shell:

2n2

Angular Momentum Angular Momentum Quantum NumberQuantum Number

The angular momentum quantum number,

generally symbolized by l, denotes the orbital (subshell) in which the electron is located.

Magnetic Quantum NumberMagnetic Quantum NumberThe magnetic quantum number, generally symbolized by m, denotes the orientation of the electron’s orbital with respect to the three axes in space.

Assigning the NumbersAssigning the Numbers The three quantum numbers (n, l, and m) are integers. The principal quantum number (n) cannot be zero. n must be 1, 2, 3, etc. The angular momentum quantum number (l) can be any integer between 0 and n - 1. For n = 3, l can be either 0, 1, or 2. The magnetic quantum number (m) can be any integer between -l and +l. For l = 2, m can be either -2, -1, 0, +1, or +2.

Principle, angular momentum, and magnetic quantum Principle, angular momentum, and magnetic quantum numbers: numbers: nn, , ll, and , and mmll

Spin Quantum NumberSpin Quantum NumberSpin quantum number denotes the behavior (direction of spin) of an electron within a magnetic field.

Possibilities for electron spin:

1

2

1

2

Orbital shapes are defined as the surface that contains 90% of the total electron probability.

An orbital is a region within an atom where thereAn orbital is a region within an atom where thereis a probability of finding an electron. This is a is a probability of finding an electron. This is a probability diagram for the s orbital in the probability diagram for the s orbital in the first first energy level…energy level…

Schrodinger Wave EquationSchrodinger Wave Equation

22

2 2

8dh EV

m dx

Equation for probabilityprobability of a single electron being found along a single axis (x-axis)Erwin Schrodinger

Heisenberg Uncertainty Heisenberg Uncertainty PrinciplePrinciple

You can find out where the electron is, but not where it is going.

OR…

You can find out where the electron is going, but not where it is!

“One cannot simultaneously determine both the position and momentum of an electron.”

Werner Heisenberg

Orbitals of the same shape (s, for instance) grow larger as n increases…

Nodes are regions of low probability within an orbital.

Sizes of Sizes of ss orbitals orbitals

Orbitals in outer energy levels DO penetrate into lower energy levels.

This is a probability Distribution for a 3s orbital.

What parts of the diagram correspond to “nodes” – regions of zero probability?

Penetration #1

Which of the orbital types in the 3rd energy level Does not seem to have a “node”?

WHY NOT?

Penetration #2

The s orbital has a spherical shape centered around the origin of the three axes in space.

s orbital shape

There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.

PP orbital shape orbital shape

Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”

…and a “dumbell with a donut”!

d orbital shapes

Shape of f orbitalsShape of f orbitals

Orbital filling tableOrbital filling table

Electron configuration of the Electron configuration of the elements of the first three elements of the first three

seriesseries

Irregular confirmations of Cr and CuIrregular confirmations of Cr and Cu

Chromium steals a 4s electron to half fill its 3d sublevel

Copper steals a 4s electron to FILL its 3d sublevel

We have colors because of the movement of electron!! Ahh ChemisTRY

Chemistry ChapterChemistry Chapter 55Atomic StructureAtomic Structure

Presented by Mr. Presented by Mr. MoleMole

You will learn about You will learn about him later…him later…

Mole Day 6:02 October 23

• Poor mister mole….we never celebrate his day because it takes to long to light his 6.02 x 10 23 candles