section 5.1 models of the atom - the culp catalystmodels of the atom . essential questions: 1. what...
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Chapter 5
Section 5.1
Models of the Atom
Essential Questions:
1. What is the Bohr model of the atom?
2. How are electrons distributed in the atom?
The Bohr Model
• Neils Bohr
-electrons found only in specific circular path
–orbits around the nucleus.
• Each electron orbit has fixed energy
–called energy level
Hydrogen
Elements are the new building blocks
Hydrogen
Oxygen-8
Carbon-6
Energy Levels
• Fixed energy levels of electrons are similar to rungs of a ladder.
• The lowest possible energy level is called its ground state.
• Just like a person an electron can climb from one rung (energy level) to another.
• Electrons can NOT be found in between rungs (energy levels).
• To move from one level to another an electrons must gain or lose energy.
Quantum
• Amount of energy required to move an electron from one energy level to another.
• The amount of energy an electron gains or loses in an atom is not always the same.
• Less energy is required to move between higher energy levels because they are closer together.
Quantum Mechanical Model
• No exact electron path
• Determines energies of an electrons
•
• Electron location is based on how likely it can be found at a particular location.
Atomic Orbitals
• Region of space in which there is a high probability of finding an electron
• Energy levels are labeled by numbers, n= 1, 2, 3, 4, 5, 6 or 7
• Each energy level has orbitals
• Orbitals are labeled by letters and different letters have different shapes
• (S, P, D, F)
Summary of Principal Energy Levels, Sublevels, and Orbitals
Principal energy level Number of
sublevels
Type of sublevel
n = 1 1 1 s (1 orbital)
n = 2 2 2 s (1 orbital), 2p (3 orbtials)
n = 3 3 3s (1 orbital), 3p (3 orbtials), 3d
(5 orbitals)
n = 4 4 4s (1 orbital), 4p (3 orbtials), 4d
(5 orbitals), 4f (7 orbitals)
Maximum number of electrons
n = 1 : 2 electrons
n = 2 : 8 electrons
n = 3 : 18 electrons
n = 4 : 32 electrons
Chapter 5.2 Electron Arrangement in atoms
Electron Configuration
• Arrangement of electrons in orbitals around the nucleus of an atom
• 3 rules
–Aufbau principle
–Pauli exclusion principle
–Hund’s rule
Aufbau Principle
• Electrons enter the lowest energy level first.
Pauli Exclusion Principle
• An orbital can hold at most 2 electrons, if 2 electrons are present they must have opposite spins
• An up or down arrow indicates the electron’s spin ↑ or ↓,
• An orbital with paired electrons is written as
↑↓
Hund’s Rule • One electron goes into each orbital of one type
until they all have 1 e-, then the e- can start to double up.
Orbital filling
Electron
Element 1s 2s 2px 2py 2pz 3s Configuration
H □ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
Orbital filling
Electron
Element 1s 2s 2px 2py 2pz 3s Configuration
H □ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
□ □ □ □ □ □
Electron Configuration
Exceptional Electron Configuration
• There are always exceptions to the rules
• Cr : 1s2 2s2 2p6 3s2 3p6 3d5 4s1
• Cu :1s2 2s2 2p6 3s2 3p6 3d10 4s1
• Exceptions due to subtle electron interactions in orbitals with similar energies
Chapter 5.3 Physics & the Quantum Mechanical Model
Light • The study of light led to the quantum mechanical model
• Newton: light consists of particles
• Huygens: light travels in waves
C = λ ν
Wavelength
Speed of light = 3.00 x 108 m/s
frequency
***Wavelength and frequency of light are
inversely proportional
Electromagnetic Spectrum
What color in the visible spectrum has the longest wavelength?
Red
Which color
in the visible
spectrum
has the
highest
energy?
Violet
Calculations Calculate the wavelength of the yellow light emitted
by a sodium lamp if the frequency of the radiation is 5.10 x 1014 Hz (5.10 x 1014 /s) and the speed of light is 3.00 x 108 m/s.
c = λ v 3.00 x 108 m/s = λ • 5.10 x 1014 /s
λ = 3.00 x 108 m/s
5.10 x 1014 /S
λ = 5.88 x 10-7 m
Atomic Spectra
• Electrons climb the energy ladder when they absorb energy. To fall back down the ladder, they give off light energy.
• Each discrete line in an emission spectrum correspond to 1 exact frequency of light emitted by the atom.
Atomic emission spectrum =
fingerprint
An explanation of atomic spectra
The light emitted by an
electron moving from a
higher to a lower energy
level has a frequency
directly proportional to
the energy change of the
electron.
n = 1
n =2
h •ν
h •ν
E = h ν
Energy
Planck’s constant
frequency
Quantum Mechanics
The motions of subatomic particles and atoms as waves
Photoelectric effect:
• Einstein used Newton idea’s said light could be described as quanta of energy that behave as particles
• Light quanta = photons