Chapter 5 Notes Waves.notebook - Honors...
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Chapter 5 Notes Waves.notebook 1 October 23, 2015 Blank Calendar Sunday Monday Tuesday Wednesday Thursday Friday Saturday 13 14 20 17 16 15 21 22 28 27 24 23 31 30 29 demo day elements test vocab quiz PSAT make notecards 7th Waves waves ws
Transcript of Chapter 5 Notes Waves.notebook - Honors...
Chapter 5 Notes Waves.notebook
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October 23, 2015
Blank
CalendarSunday Monday Tuesday Wednesday Thursday Friday Saturday
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demo dayelements test
vocabquizPSAT
make notecards 7th
Waves
waves ws
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The Nature of Matter:By the early 20th century it was understood by most scientists that energy and matter were separate.
Atoms were matter and light was energy...
Light behaved as a wave...
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What did scientists know about the atom by the early 20th century?
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What are Waves?
Parts of waves:
Types of Waves:
What do you think of?
What are wave made out of?
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Trough
Crest
Amplitude
Wavelength
Parts of Waves:
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Trough
Crest
Amplitude
Wavelength
Wavelength (λ): Is the shortest distance between equivalent points on a continuous wave (crest to crest or trough to trough) commonly measured in meters, centimeters or nanometers
Crest: Top of the waveTrough: Bottom of the wave
Amplitude: Is the wave's height from the origin to a crest, or from the origin to a trough. (wavelength and frequency do not affect amplitude)
Frequency (υ): Is the number of waves that pass a given point per second. Hertz (Hz) is the SI unit for frequency
Parts of Waves:
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Electromagnetic radiation:Light is defined as electromagnetic radiation, a form of energy that exhibits wavelike behavior as it travels through space
Radio waves
microwaves
infrared waves
visible light
ultraviolet waves
xrays
gamma rays
Examples:
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Electromagnetic Spectrum:A spectrum that includes all forms of electromagnetic radiation, with the only difference in the types of radiation being their frequencies and wavelengths
ROYGBIV
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Wave Mathematical RelationshipsC = λ * υ
λ Wavelengthυ frequency
C Speed of lightSpeed of light is 3.00 x 108 m/sThis speed is constant for all electromagnetic waves inside a vacuum (space)
Practice: What is the frequency of an Xray with a wavelength of 1.15 x 1010 m?
Note: As frequency increases, wavelength decreases (inverse relationship)
Note: As frequency increases, energy of the wave increases
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HOmewOrk!Wavelength
Practice: What is the frequency of an Xray with a wavelength of 1.15 x 1010 m?
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Light as a wave failed to explain:
Why heated objects emit only certain frequencies of light
Why do some metals emit electrons when light at a given temperature shines on them (photoelectric effect)?
These colors correspond to different wavelength and frequencies
black body phenomena
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Photoelectric EffectSome metals will eject electrons form their surface with light of a certain frequency (or higher) hits their surface
Light was affecting matter...How?
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Max Planck (1900)A German physicist was searching for an explanation of these phenomena.He found that matter could either gain or lose energy but only in small specific amounts called he called quanta
Quantum is the minimum amount of energy that can be gained or lost by an atom
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Energy of a Quantum
E = h * υ
Planck came up with a relationship between the energy of a quantum and the frequency of a wave
E Energy of a quantumh Planck's Constant h = 6.626 x 1034 J*sυ frequency of the wave
This showed scientists that these quanta (packets of energy) were whole number multiples of hυ
hυ 2hυ 3hυ 4hυ 5hυ 8hυ7hυ6hυ
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Stair step analogy
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Albert Einstein (1905)Duality of lightlight can be both a wave and a particle
It is a beam of bundles of energy called photons
Photonsa massless particle that carries a quantum of energy. This energy depends on the frequency of the photonsEPhoton = hυEphoton = Energy of the photonh = Plank's Constantυ= frequency
The blue color in some fireworks occurs when copper chloride is heated to approximately 1500K and emits blue light with a frequency 6.67 x 1014 Hz. How much energy does one photon of this light carry?
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The blue color in some fireworks occurs when copper chloride is heated to approximately 1500K and emits blue light of wavelength 4.50x102 nm. how much energy does one photon of this light carry?
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Warmup: What two phenomena were not explainable by Rutherford's atomic model and scientist's understanding of matter and energy at the turn of the 20th century?
What did Planck discover?
How did Einstein explain Planck's discovery?
RED RIBBON WEEK!RED RIBBON WEEK!
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Atomic Emission Spectra: the set of frequencies of the electromagnetic waves emitted by atoms of the element
These are used to identify elements and elements within compounds
Scientists did not have a scientific reason to explain this...
Each element has a very specific range of colors that are emitted
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Niels Bohr (1913)Studied the hydrogen atom and, based off of Planck's and Einstein's concepts of quantized energy, determined that the atom only had certain allowable energy states
• Lowest possible energy state is called Ground State
• When the atom absorbs energy, it is said to be in an Excited State
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Bohr's Model of the AtomBohr suggested that the electrons around the hydrogen atom could only be allowed in certain circular orbits around the nucleus
• The smaller the electron's orbit, the lower the atom's energy state or energy level
• The larger the electron's orbit, the higher the atom's energy level
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Bohrs Atomic orbit
Quantum number
Orbit Radius (nm)
Corresponding atomic energy level
Relative Energy
First n = 1 0.0529 1 E1
Second n = 2 0.212 2 E2 = 4E1
Third n = 3 0.476 3 E3 = 9E1
Fourth n = 4 0.846 4 E4 = 16E1
Fifth n = 5 1.32 5 E5 = 25E1
Sixth n = 6 1.90 6 E6 = 36E1
Seventh n = 7 2.59 7 E7 = 49E1
Quantum Number: The number Bohr gave to each orbit around the atom
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Energy StateGround State for Hydrogen is when hydrogen's single electron is in the first energy level or the first quantum level
• The hydrogen atom does not give off energy in the ground state
Once energy is added the single electron moves up to a higher energy orbit (such as n = 2) making the atom in an excited state
• The electron will fall back into its original quantum level (ground state) and release the energy as a photon
Since these quanta are set, only set energies can be absorbed and emitted by the atom, therefore only specific frequencies are emitted by the atom
What did this explain?
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Atomic Emission SpectraElectrons around an atom's nucleus will absorb energy in quanta, the electrons will then jump up and fall back down to what is called ground state and release that same amount of energy.
This energy has a specific frequency which can be seen as colors; meaning the frequency of the photons release is within the visible light of the electromagnetic spectrum
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Therefore the wavelength of light emitted by excited electrons could be used to determine the energy absorbed by the electron.
E= hυ C = λ * υWhat is the energy absorbed by the electron on the diagram?
λ = 3.45 x 109 meters
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Louis de Broglie (1924)If light can have both wave and particlelike characteristics, then matter (electrons) can behave as bothPredicted that all moving particles have wavelike characteristics (including cars or baseballs)
λ = h/mυλ = Wavelengthh = Planck's constant
m = massυ = frequency
Why can we not see the wavelength of a moving baseball? (Do the math)
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Werner Heisenberg (19011976)• Stated that it is impossible to take any measurement of an object without disturbing the object
Heisenberg uncertainty principle: states that it is fundamentally impossible to know precisely both the velocity and position of an electron at the same time
• Meaning Bohr's defined orbits were not accurate
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Erwin Schrodinger (1926)Austrian Physicist
Quantum Mechanical model of the atom: the atomic model in which electrons are treated as waves
• This allowed for scientists to determine particular volumes of space around the nucleus in which the probability of finding an electron is very high
Atomic Orbital: the probable location of an electron within an atom; it is 3D in shape
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Atomic OrbitalsPrincipal quantum number (n)number of the atomic orbitals. (also called Principal energy level)
• As n increases, the orbitals become larger and have more energy
These levels contain what are called energy sublevels• The first energy level contains 1 sublevel; the second energy level contains 2 sublevels,the third energy level contains 3 sublevels, etc.
There are a total of 4 sublevels labeled s, p, d and f
• These sublevels are then broken down further into orbitals
• A single orbital can only hold 2 electrons total
• Meaning if there are 3 orbitals there can be a total of 6 electrons in that sublevel
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SSublevelThe ssublevel has a spherical shape
The ssublevel only has one orbital and therefore ssublevel can only hold two electrons
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PSublevelThe psublevel is a dumbbell shape
The psublevel contains 3 orbitals and therefore contains 6 electrons total
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Electron ConfigurationChap. 5.3
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ReviewEnergy levels can be found by looking at what on the periodic table?
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dsublevelThe dsublevel has two shapes; one that looks like two dumbbells put together and the other is like a single dumbbell
The dsublevel contains 5 orbitals and therefore can hold up to 10 electrons
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fsublevelThe fsublevel has a very complex shape
The fsublevel contains 7 orbitals and therefore contains 14 electrons
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Basic goal: Break the energy levels down into sublevels and orbitals!
Energy levels
Sublevels
Orbitals
(s, p, d, and f)
Only 2 electrons
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Periodic breakdown of levels and sublevels
Notice that the energy level 1 contains only 1 sublevel (s), energy level 2 contains 2 sublevels (s and p), energy level 3 contains 3 sublevels (s, p, and d), and energy level 4 contains 4 sublevels (s, p, d, and f)
• Which is the order of the orbitals: s, p, d, and f
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Electron ConfigurationThis is the arrangement of electrons in an atom
ReviewHow many electrons can the ssublevel hold?How many electrons can the psublevel hold?How many electrons can the dsublevel hold?How many electrons can the fsublevel hold?
Where can each of the sublevels be found on the periodic table?
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Rules for Electron Configuration/orbital diagramsThere are three rules that must be followed while writing electron configurations
Rule 1: Aufbau Principle
Rule 2: Pauli Exclusion Principle
Rule 3: Hund's rule
• Each electron occupies the lowest energy orbital available
• A maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins
• Single electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital
"fill up left to right"
"ups with downs, no ups w| ups or downs with downs"
"ups before downs"
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1s 2s 2p 3s 3p 4s 3d
1s 2s 2p 3s 3p 4s 3d
1s 2s 2p 3s 3p 4s 3d
A.
B.
C.
1s 2s 2p 3s 3p 4s 3d
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Rule 1: Aufbau Principle• Each electron occupies the lowest energy orbital available
This means that you must first be able to determine the order of energy levels, sublevels and the orbitals within those sublevels
Energy levels move in the order of periods down the periodic table• Order: 1, 2, 3, 4, 5, 6 and 7
Sublevels are in the order of s, p, d, and f and how they appear on the periodic table
2p1s2s 2p3s 3p
4s 4p3d
4d5s 5p
6s 6p5d7s 6d
4f5f
7p
• Notice that the dlevel and flevel are "behind" the s and plevel
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Rule 2: Pauli Exclusion Principle • A maximum of two electrons can occupy a single orbital, but only if the electrons have opposite spins
Remember that the sublevels contain orbitals. Ssublevel contains 1 orbital, psublevel contains 3 orbitals, dsublevel contains 5 orbitals, and fsublevel contains 7 orbitals
• ssublevel can only hold 2 electrons• psublevel can only hold 6 electrons• dsublevel can only hold 10 electrons• fsublevel can only hold 14 electrons
This means that an energy level that contains ALL sublevels can only contain 32 electrons all together
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Sp
d
f
12
1 2 3 4 5 6 7 8 9 10
51 2 3 46
1 2 3 4 5 6 7 8 9 10 11 1412 13
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Lets say we want to write the electron config for Nitrogen
Sp
d
f
12
1 2 3 4 5 6 7 8 9 10
51 2 3 46
1 2 3 4 5 6 7 8 9 10 11 1412 13
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Practice:Write the electron diagram for the following elements:
Calcium
Phosphorus
Oxygen
Argon
Cobalt
Silver
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Rule 3: Hund's rule• Single electrons with the same spin must occupy each equal energy orbital before additional electrons with opposite spins can occupy the same orbital
Lets look at our electrons configuration for Nitrogen
1s22s22p3
1s 2s 2p
This is called an orbital diagram
/ Pauli Exclusion principle
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Practice:Write the orbital diagram for the following elements:
Manganese
Potassium
Gallium
Neon
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Noble gas notation:Where are the noble gasses on the periodic table?
Noble gas notation makes writing electron configs and orbital diagrams easier (and shorter)
• Let say we wanted to write out the electron configuration for Bromine
• Now instead of write ALL of that, determine the noble gas that comes BEFORE Bromine and write everything in the configuration that comes AFTER that point
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Practice:Write the Nobel gas notation for the following elements:
Sodium
Sulfur
Arsenic
Iron
Silicon
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1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p6 4s2 3d1
1s2 2s2 2p6 3s2
1s2 2s2 2p1
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1
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