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Transcript of Agenda Midterm – October 26 th / 27th Chapter 5 Quiz – October 21 Formal Lab – October 21 st...
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Agenda
Midterm – October 26th / 27thChapter 5 Quiz – October 21
Formal Lab – October 21st
Homework (wb 5) – October 24/25th
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Light• Electromagnetic radiation– Form of energy that exhibits wavelike behavior
Terms to know– Wavelength• Measured from crest to crest (measured in meters, m)
– Amplitude• A waves height
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– Frequency• Number of waves that pass a given point
Low frequency
High frequency
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The speed of Light
C is a given = 3.00 x 108 m/sλ = wavelength (meters, m)ν = frequency (Herts, Hz = waves per second)
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Answer the following questions pg 121• What is the frequency of a green light, which has a
wavelength of 4.90 x 10 -7m?• An X ray has a wavelength of 1.15 x 10 -10m?• What is the speed of an electromagnetic wave that
has a frequency of 7.8 x 10 -6 Hz• A popular radio station broadcast with a frequency
of 94.7 MHz What is the wavelength of the broadcast? (1MHz = 10 6 Hz)
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Particle nature of Light• Quantum = minimum amount of energy that can
be gained or lost by an atom• The energy of a quantum is related to the
frequency of the emitted radiation
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Planck’s Constant
• Equantum = hν– H = 6.626 x 10 -34 J(s)– ν = frequency measure per second
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Answer the following Question pg 124• What is the energy of each of the following types
of radiation?– A 6.32 x 1020 s-1
– b. 9.50 x 1013 Hz– c. 1.05 x 10 16 s-1
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• Answer the questions on page 147 #s 65-76
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N - 1
N - 5N - 4
N - 2 N - 3
N - 5
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Bohr Model of the Atom• A single electron moves around the nucleus in
only certain allowed circular orbits.• Each orbit has an energy level– Larger the orbit…larger the energy level
• “n” = the quantum number– This the orbit and the corresponding energy level.
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Bohr’s Model of the atom
The larger the orbital, the further the e- are from the nucleus
+
n = 1
n = 2
n = 3n = 4
Quantum # (n)- Indicated energy level or orbital
The probability of finding e- in certain regions of an atom is described by an orbital
Orbitals have characteristic shapes, size and energies, but do NOT tell how e- move
Neils Bohr
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Energy LevelsN-1• S orbital only…2 electronsN-2• S orbital…P orbital…6 electronsN-3• S & P orbitalN-4• S…3d orbital (10 electrons)…P N-5• S…4d orbital (10 electrons)…P N-6• S…5d orbital (10 electrons)…4f orbital (14 electrons)…P N-7• S…6d orbital (10 electrons)…5f orbital (14 electrons)…P
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Quantum model
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• Each Orbital has energy levels
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Ground State Electron Configurations
• Aufbau principle…each electron occupies the lowest energy orbital available.
• Pauli exclusion principle– 2 electrons occupy a single orbital– Each electron has an opposite spin
• 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 orbitals. Pg 136
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Aufbau Principle
• Each electron occupies the lowest energy orbital available
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Pauli’s Exclusion Principle
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Pauli’s Exclusion Principle
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Hund’s Rule
• Single electrons with the same spin must occupy each equal-energy orbital before additional electrons with opposite spins can occupy same orbitals
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Hund’s Rule
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The Orbitals
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Orbital diagrams
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Noble Gas Notation
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Electron Spin- e- spin either clockwise or counterclockwise which creates a magnetic field
Pauli Exclusion Principle –
- an orbital with 2e- of opposite spin are said to have a pair of e-
Sublevels # Orbitals Max # of e- s 1 2 p 3 6 d 5 10 f 7 14
Figure 4-24
each orbital in an atom can hold up to 2e- that must have opposite spin ( and )
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Electron ConfigurationsDefinition
Distribution of e- among orbitals; describes where e- are and what energy they have
Aufbau Principle –
Hund Rule –
_____ _____ _____ _____ _____ 1s 2s 2px 2py 2pz 1s2 2s2 2p6
e- are added one at a time to the lowest energy level available
e- occupy equal energy orbitals so the maximum number of unpaired e- result
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• 1s2 2s2 2p6
•
• Orbital Last level of energy
• Number of electrons in a particular orbital
Level of energy
This particular atoms has2 levels of energy 10 electron total 2 + 2 +68 electrons in the last level of energy 2 +6
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How To Do Energy Diagrams
Step 1
Step 2
Step 3
Step 4
Determine atomic number
Determine number of e-- if neutral: # e- = atomic #- if ion: # e- = atomic # - charge
Fill in atomic orbital energy diagram using following principles- Pauli: 2e- max per orbital with opposite spin- Aufbau: 1e- at a time filling lowest energy levels first- Hund: max # of unpaired e-
Determine number of paired and unpaired e-
Step 5 Write e- configuration
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Example Determine the e- configuration of Ne by using an atomic orbital energy diagram
3s _____2p _____ _____ _____
2s _____1s _____
Atomic # = 10# e- = 10 – 0 = 10
Paired = 5Unpaired = 0
e- config: 1s22s22p6
Example Determine the e- configuration of S by using an atomic orbital energy diagram
4s _____3p _____ _____ _____
3s _____2p _____ _____ _____
2s _____1s _____
Atomic # = 16# e- = 16 – 0 = 16
Paired = 7Unpaired = 2
e- config: 1s22s22p63s23p4
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Example Determine the e- configuration of Fe+ by using an atomic orbital energy diagram
3d _____ _____ _____ _____ _____4s _____
3p _____ _____ _____ 3s _____
2p _____ _____ _____2s _____1s _____
Atomic # = 26# e- = 26 – 1 = 25
Paired = 10 Unpaired = 5
e- config: 1s22s22p63s23p64s23d5
Example Determine the e- configuration of F- by using an atomic orbital energy diagram
3s _____2p _____ _____ _____
2s _____1s _____
Atomic # = 9# e- = 9 – -1 = 10
Paired = 5 Unpaired = 0
e- config: 1s22s22p6
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36Start with 1s and read up the arrow
Order of Energy Levels from Lowest (1s) to Highest
Group 1 – Alkali Metals
Group 2 – Alkaline Earth Metals
Group 1- 10 – Transition Metals
Group 5 – Nitrogen Group
Group 8 – Nobel Gas
Group 3 – Boron GroupGroup 4 – Carbon Group
Group 6 – Oxygen GroupGroup 7 – Halogens
Period 4f– LanthanidesPeriod 5f– Actinides
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Valence Electrons
• Only certain electrons can determine the chemical properties of an element– Valence Electrons
• Valence electrons are defined as electron’s in the atom’s outermost orbital…or highest energy level
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Valence Electrons
• Steps to create Lewis Structures for single elements– Find the number of electrons in the last S and P
orbitals…or look on the chart to find the number of valence electrons on the periodic table
– Arrange electrons around Element symbol evenly– Ex: Chlorine• 7 Valence Electrons
Cl
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Valence Electrons
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Valence Electrons• Electrons in the atom’s most outer orbitals– The electrons in the last S and P orbitals
Boron – 1s2 2s2 2p1
Iodine– 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p5
Electron Dot…
• H C O He
• Li P F Ar