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QUANTIZATION OF THE ATOM
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DATE TITLE PAGE #
TABLE OF CONTENTS
X Chemical/Physical IP 28
X Chemical/Physical 29
X Atoms & Elements 30
X Book Learning (Theory) 31 – 32
X History of the Atomic Theory notes 33
X History IP 34
X Structure of the Atom notes 35
X Structure of the Atom IP#1 & 2 36
X Bohrs Model 37
X Bohr IP#1 38
X Bohr IP#2 (PT) 39
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THE CURRENT ATOM
Electrons “-”
Protons “+”
Neutrons “0”
+
+
+
0
0
0
0
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BOHR’S MODEL
• Bohr studied the light produced
when atoms were excited by
heat or electricity.
• Rutherford's model
couldn't explain why
unique colors were
obtained by atoms of
different elements.
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BOHR’S MODEL
• Electrons orbit the nucleus like planets orbit the sun.
• Bohr proposed that electrons are in orbits & when excited jump to a higher orbit. When they fall back to the original they give off light.
Lower energy level
Higher energy
level
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BOHR’S MODEL
• Each electron shell (ring) can hold a
certain number of electrons
• Electron shells are filled from the
inside out
+ Noble Gases have full outer electron
shells and are STABLE, NON-
REACTIVE
Argon (Ar)
“Noble Gas”
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BOHR’S MODEL• The electrons in the
outermost ring (valence
shell) are called valence
electrons
+ The number of electron
shells is the same as the
period number
+ The number of valence
electrons is the same as
the group number
Valence
e-
Valence
shell
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USE THE PERIODIC TABLE TO CREATE YOUR BOHR MODEL!
• Protons, neutrons, electrons
• Rings (energy shells)
• How you should “fill up” each ring
• Valence electrons
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CFU #1: CARBON
• Total electrons
• How many on ring 1?
• How many on ring 2 (valence)?
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CFU #1: NEON• Total electrons
• How many on ring 1?
• How many on ring 2 (valence)?
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Non- METALS
METALS
1 2 GROUPS “valence electrons” 3 4 5 6 7 8
1. Sulfur (S)2. Fluorine (F)
3. Aluminum (Al)
HOW MANY VALENCE ELECTRONS?
CFU #3
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Non- METALS
METALS
1. Sulfur (S)2. Fluorine (F)
3. Aluminum (Al)
1
2
3
4
5
SHELLS
HOW MANY SHELLS (RINGS)?
KEY
CFU #2
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CFU!
Non- METALS
METALS
1 2 GROUPS “valence electrons” 3 4 5 6 7 8
1
2
3
4
5
SHELLS
CFU!
Which element has 18 valence electrons, 4 shells?CFU!
Which element has 2 valence electrons, 5 shells?CFU! e
Which element has 5 valence electrons, 3 shells?
BONUS
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DRAWING BOHR MODELS
1. Draw the nucleus.
2. Write the number of neutrons and the number of protons in the nucleus.
3. Draw the first energy level.
4. Draw the electrons in the energy levels according to the rules below. Make sure you draw the electrons in pairs.
5. Keep track of how many electrons are put in each level and the number of electrons left to use.
You must fill one level before going
on to draw the next level!
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GUIDED PRACTICE
• Protons: _____ Neutrons: _____Electrons: ______
• How many energy shells will this have? ____
• How many valence (outer) electrons does this element
have? ____
• Bohr Model:
11
Na
Sodium
22.990
11 12 113
1
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GUIDED PRACTICE
• Protons: _____ Neutrons: _____Electrons: ______
• How many energy shells will this have? ____
• How many valence (outer) electrons does this element
have? ____
• Bohr Model:
15
PPhosphorous
30.974
15 16 153
5
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GUIDED PRACTICE
• Protons: _____ Neutrons: _____Electrons: ______
• How many energy shells will this have? ____
• How many valence (outer) electrons does this element
have? ____
• Bohr Model:
6
C
Carbon
12.011
6 6 62
4
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WE DO – BOHR MODEL RACES
• You will see a symbol displayed.
• Create an accurate Bohr Model using what you
know about atoms and energy level rules.
• Check answers when time is up.
Any beads found on the floor will
result in class materials deductions
KEY
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helium
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lithium
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beryllium
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boron
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carbon
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nitrogen
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oxygen
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fluorine
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neonFull valence shell = non-reactive
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ABSORPTION AND EMISSIONHOW IS LIGHT ABSORBED AND
EMITTED BY ATOMS IN INTERSTELLAR GASES OR STARS?
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THE ELECTROMAGNETIC SPECTRUM
low frequency
low energy
High frequency
High energy
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MODELS OF LIGHT
LIGHT IS A WAVE LIGHT IS A PARTICLE
So which one is
right?
They are both right...and they are both wrong.
That’s called W A V E - P A R T I C L E duality
•In some experiments, the wave model works
best.
•In other experiments, the particle model
works best.
•Thus, we use both.
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LIGHT IS A WAVESynonyms for “light”
• Electromagnetic wave
• Electromagnetic radiation
• Radiation
Visible light is light that oureyes are sensitive to;however, that is not theonly type of electromagneticradiation
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WAVELENGTH VS. FREQUENCY
Wavelength ()the distance between successive crests of a wave, especially points in a sound wave or electromagnetic wave.
Frequency (f)the rate at which a vibration
occurs that constitutes a
wave, either in a material (as
in sound waves), or in an
electromagnetic field (as in
radio waves and light),
usually measured per second.
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CALCULATIONS BETWEEN WAVELENGTH, FREQUENCY AND
ENERGY Wavelength (): the distance between
successive crests of a wave, especially
points in a sound wave or
electromagnetic wave.
Speed of Light (c): the distance light
can travel in a unit of time through a
given substance.
In a vacuum, v = c = 3.00 x 108 m/s.
Frequency (f): the rate at which a
vibration occurs that constitutes a
wave, either in a material (as in
sound waves), or in an
electromagnetic field (as in radio
waves and light), usually measured
per second.
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Check for Understanding
Find Frequency (v) using the equation A gamma ray has a wavelength of 0.039 nm. What is the frequency of the wave?
Find Wavelength () using the equation What is the wavelength of an X ray that has a frequency of 7.8 X 1017 Hz?
∁= 𝜆 ∗ 𝑣
Speed of light = 3.00 x 108 m/s
𝑐
𝜆
𝑐
𝑣
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LIGHT COMES IN MANY WAVELENGTHS
• White light is a combination of all colors in the color spectrum.
• When white light passes through a glass prism (or a diffraction grating), it separates
into colors.
• These colors have different wavelengths.
• This group of wavelengths is the visible part of the electromagnetic spectrum.
• When you “see” the entire spectrum with no thin dark bands, it is a continuous
spectrum.
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ELECTROMAGNETIC SPECTRUM
Add colors to this portion:
NOTE:
• Energy
• Frequency
• wavelength
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CHECK FOR UNDERSTANDING
1. What is the wavelength range for the visible light spectrum?
2. Which color of light has a longer wavelength purple or red?
3. Suppose that a certain medical treatment requires exposing certain tissues to high frequency radiation. Would that radiation likely be gamma rays or radio waves?
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LIGHT AS A PARTICLE(SMALL REGION OF SPACE)
• A photon is a “particle” or
“packet” of energy according to
Max Planck called a QUANTUM
• A quantum of energy is the
minimum amount of energy that
can be lost or gained by an atom.
• High frequency photons have high
energy
• Low frequency photons have low
energy
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BOHR MODEL
• The Bohr model is a planetary model, where the electron orbits the nucleus like a planet orbits the Sun.
• An electron is only allowed in DISCRETE orbits (n=1, n=2, n=3, etc.)
• The higher the orbit, the higher the energy of the electron.
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ABSORPTION, EMISSION, AND ENERGY
• When an atom absorbs a photon, it gains
energy.
• When an atom loses energy, it emits a photon.
• An atom can only absorb or emit photons of
“specific” energy.
• Those “right energies” correspond to the
DIFFERENCES in energy between the allowed
energy levels.
Absorption
photon
Emission
photon
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HYDROGEN ENERGY SPECTRUM
-13.6 eV
-3.40 eV
-1.51 eV
-0.850 eV
-0.544 eVn=5
n=4
n=3
n=2
n=1
Energy Level Energy
• Only certain energies are allowed
• The change in the energy between two levels
corresponds to a certain color photon absorbed or
emitted by the atom.
• The lowest energy level is the ground state.
• Higher energy levels are called excited states.
ground
excited
Lower energy level
“ground state”
Higher energy
level
“excited state”
!
CFU
1. If an atom is in the ground state (n=1)
and is excited to n=3, what energy
photon was absorbed?
2. If a hydrogen atom is in the state n=4,
to what level must it “fall” in order to
emit a blue photon?
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ABSORPTION SPECTRUM
• If light of a continuous spectrum is incident on a gas of hydrogen atoms, then electrons will absorb some of the light.
• As a result, bands of the spectrum are missing; these are called absorption lines.
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EMISSION SPECTRUM
• If excited hydrogen atoms fall to lower energy states, photons will be emitted.
• The emitted photons will be detected as light of certain bands of frequencies (i.e. colors).
• The collection of bands (or lines) forms an emission spectrum.