Quantum Mechanics and Configuration

Slides:



Advertisements
Similar presentations
The Bohr Model 2: Quantum Mechanics.
Advertisements

Lecture 2210/26/05. Moving between energy levels.
Wave-Particle Duality 2: The Quantum Mechanical Model
Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave.
Chapter 5 Section 5.3 & 5.4 The Quantum Model. Problems with the Bohr Model 1. Worked well for predicting hydrogen spectrum, but not for elements with.
The Quantum Model of the Atom. Proposed that the photoelectric effect could be explained by the concept of quanta, or packets of energy that only occur.
The Bohr model for the electrons
Quantum Atom. Louis deBroglie Suggested if energy has particle nature then particles should have a wave nature Particle wavelength given by λ = h/ mv.
Class Opener: Tues., Oct. 14th **on back of new notes**
Bohr Model Since the energy states are quantized, the light emitted from excited atoms must be quantized and appear as line spectra. After lots of math,
Electrons in Atoms Chapter 5. Duality of Light Einstein proved that matter and energy are related E = mc 2 Einstein proved that matter and energy are.
Quantum Theory the modern atomic model. Bohr Model of the Atom a quantum model proposed by Niels Bohr in 1913 It helped to explain why the atomic emission.
Quantum Atom. Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement.
Arrangement of Electrons in Atoms
The Quantum Model of the Atom Section 4.2. Bohr’s Problems Why did hydrogen’s electron exist around the nucleus only in certain allowed orbits? Why couldn’t.
Section 3.2 – page 174. De Broglie  Proposed the dual nature of light; it could act as a particle or a wave. 
Electronic Structure of Atoms 6.4 The Wave Behavior of Matter 6.5 Quantum Mechanics and Atomic Orbitals 6.6 Representation of Orbitals.
Quantum Theory and the Atom. Learning Objective Describe the relationship between electron levels, sublevels and atomic orbitals.
Electrons in Atoms Chapter Wave Nature of Light  Electromagnetic Radiation is a form of energy that exhibits wavelike behavior as it travels through.
Chem - mystery What has more energy, a heat lamp or a tanning lamp?
EMR exhibits particle (photon) and wave (ν, λ, Amp) properties and all energy is transferred in quantum. Elements have unique emission spectra because.
Quantum Atom. Problem Bohr model of the atom only successfully predicted the behavior of hydrogen Good start, but needed refinement.
Bulls-eye Activity. Did the pennies consistently drop in the same ring? Can we use our empirical evidence to predict exactly where a penny would land?
Quantum Mechanical Model of Atom. Name This Element.
Recap – Last Lecture Bohr model of the atom: electrons occupy orbits of certain energies. Evidence of this from atomic spectra in which wavelength of light.
Light Light is a kind of electromagnetic radiation, which is a from of energy that exhibits wavelike behavior as it travels through space. Other forms.
The Quantum Mechanical Model of the Atom
Postulates of Bohr model
Quantum Model of the Atom
Chapter 4: Arrangement of Electrons in Atoms
Chapter 5 section 1 models of the atom.
Structure & Properties of Matter
The Bohr Model, Wave Model, and Quantum Model
Atomic Models Scientist studying the atom quickly determined that protons and neutrons are found in the nucleus of an atom. The location and arrangement.
The Quantum Model Section 4.2.
Postulates of Bohr model
Quantum Mechanical Model of the Atom
the quantum model of the atom
4.7 – NOTES Intro to Electron Configurations
The Electronic Structure of Atoms
Models of the Atom Foothill Chemistry.
Section 3: The Quantum Mechanical Model of the Atom
Quantum Model of the Atom
III. Quantum Model of the Atom (p )
The Quantum Mechanical Model
The Quantum Model of the Atom.
Quantum Theory Light Theory Part 4.
Models of the atom & quantum theory
Chemistry – Mrs. Cameron
4.8 – NOTES Intro to Electron Configurations
Quantum Numbers Mr. Tsigaridis.
Chemistry 1 Chapter 5 Notes Part II Quantum Theory of the atom
Electrons in Atoms Chapter 5.
The Quantum Model of the Atom
Electron Orbitals Heisenberg 1. The ____________ ______________ principle states that it is impossible to determine simultaneously both the position and.
Chapter 4 Electrons as Waves
BELLWORK 10/26/17 What is a photon? Is light a particle or a wave?
The Quantum Model of the Atom
Orbitals, Spins, and More
Quantum Mechanical Model of the Atom
Electromagnetic Spectrum Atomic Emission Spectrum.
Section 5.2 Quantum Theory and the Atom
Electron Configuration
QUANTUM MECHANICS VIEW OF THE ATOM.
III. Quantum Model of the Atom (p )
Section 2: Quantum Theory and the Atom
2.4- Quantum Mechanical Model
Unit 4: Electrons in the Atom
Quantum Theory Electrons!.
The Bohr Model, Wave Model, and Quantum Model
Presentation transcript:

Quantum Mechanics and Configuration The Bohr Model 2: Quantum Mechanics and Configuration

C12-2-06 ELECTRON CONFIGURATION OUTCOME QUESTION(S): C12-2-06 ELECTRON CONFIGURATION Relate the electron configuration of an element to its valence electron(s) and its position on the Periodic Table. Include: quantum energy level, shapes, and orbitals. Write the electron configuration for a variety of atoms and ions using the 3 configuration laws. Include: shorthand notation and valence configuration Vocabulary & Concepts  Principal quantum number (n)

de Broglie (1924) – developed an equation that predicts wave qualities for all matter. If waves of light could contain photon-particles, could matter have wave properties? Suggests orbits are fixed because electrons (as a wave) could only move as strict standing wavelength

The famous “double-slit” experiment proved the “wave-particle duality” of matter (click the TV link below)

Think - trying to catch a frog in the dark with a flashlight… Problems: World is 3-dimensional Bohr’s math failed to explain all spectra Matter also has wave properties Heisenberg (1925) - it is impossible to know precisely the velocity and position of a particle at the same time – Heisenberg Uncertainty Principle Think - trying to catch a frog in the dark with a flashlight…

Schrödinger (1926) – developed a wave equation that describes the energies and behaviour of subatomic particles. Determines the probability of finding an electron in a 3-D volume of space around the nucleus. At this point, scientists couldn’t really figure matter out experimentally, so they turned to math and computers…

Each energy level's boundary is the area of electron location 90% of the time

principle quantum number (n) Bohr’s orbits are now called: principle quantum number (n) The (n) number indirectly describes the size and energy requirements of an orbit (electrons have more energy further out)

distance from the nucleus 2. Angular momentum (l) shape of orbital The probable location of every electron is now described by a set of 4 quantum numbers: This is a lot of detail – focus on the words not the letters (distance, shape, orientation, spin) QUANTUM NUMBERS Principal (n) distance from the nucleus 2. Angular momentum (l) shape of orbital 3. Magnetic (m) orientation in 3D space 4. Spin momentum (s) spin of the election

Principal (n) - distance Number of shapes (l) in each level equals the principal quantum number (n) for that level NUCLEUS n = 1 s n = 2 s p n = 3 s p d Like a stadium, the further from the stage (nucleus) the more “sections” of seating for people (electrons)

S – sphere P – dumbbell D – clover F - ?? 2. Angular momentum (l) - shape Higher quantum numbers (n) contain many sections of probable electron location – shapes (l) There are four shapes appearing in this order: S – sphere P – dumbbell D – clover F - ?? These shapes represent probable locations for finding electrons around the nucleus

3. Magnetic (m) – orientation Shapes (l) can be made of multiple orbitals (m) that occupy the axes of 3D space (x, y, z) “s” shape (sphere) – 1 orbital orientations “p” shape (dumbbell) – 3 orbital orientations “d” shape (clover) – 5 orbital orientations “f” shape (indeterminate) – 7 orbital orientations Think about how many ways each shape can be represented in space – the next picture will help…

“s” shape – 1 orbital orientations (just one – in the middle of x, y and z axis) “p” shape – 3 orbital orientations (along the x, the y or the z axis) “d” shape – 5 orbital orientations (along x and y, xz, yz…) “f” shape – 7 orbital orientations (along the …I don’t know what that is)

Notice the distance, shape, orientation OLD way NEW way Notice the distance, shape, orientation

4. Spin momentum (s) – spin Each orbital holds two spinning electrons (s) Level Shapes orbitals e- capacity 1 s 1 = 1 2 s,p 1+3 = 4 8 3 s,p,d 1+3+5 = 9 18 4 s,p,d,f 1+3+5+7 = 16 32 n n types n2 2n2

1s2 2s2 2p6 3s2 3p6 3d10 n = 3 n = 2 n = 1 2e- 8e- 18e- 2e- 8e- 8e- OLD way NEW way

C12-2-06 ELECTRON CONFIGURATION CAN YOU / HAVE YOU? C12-2-06 ELECTRON CONFIGURATION Relate the electron configuration of an element to its valence electron(s) and its position on the Periodic Table. Include: quantum energy level, shapes, and orbitals. Write the electron configuration for a variety of atoms and ions using the 3 configuration laws. Include: shorthand notation and valence configuration Vocabulary & Concepts  Principal quantum number (n)