notes ch 5 electron configurations telling electrons where they can go!!
TRANSCRIPT
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Notes CH 5Electron Configurations
telling electrons where they can go!!
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Electrons.. Where are they?
And why do we need to know?The chemical behavior of an element is determined by the number of electrons and how they are arranged.
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Bohr’s modelHelped explain why elements give off certain colors of light (excited electrons jumping to lower energy levels)Electrons travel in specific energy “orbits” but not in between them.
1st2nd
3rdElectron can be here
But not here
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Review…Bohr’s model of the atom
Each level has a certain number of e-1st = 22nd = 83rd = 18 (or 8)4th = 32 (or 18 or 8)5th = 32 (or 18 or 8)6th = 18 (or 8)7th = 8**Note= last level cannot have more than 8 valence e-
nucleus Energy levels
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Bohr models of various atoms.
1. Draw (or write) the Bohr sequence for Calcium (20)
2. Give the # of valence electrons (last level)
3. Tell if will lose e- (like metals, have less than 4) or gain e- (like non-metals, have more than 4) or metalloids (either gain or lose)
4. Give the isotope symbol
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Bohr models of various atoms.
1. Draw (or write) the Bohr sequence for Bromine
2. Give the # of valence electrons (last level)
3. Tell if will lose e- (like metals, have less than 4) or gain e- (like non-metals, have more than 4) or metalloids (either gain or lose)
4. Give the isotope symbol
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Example
For all the element Bromine (35):1) Draw (or write) the Bohr sequence
2) Give the # of valence electrons 3) Tell if will lose e- (like metals) or gain
e- (like non-metals)
4) Give the ion symbol and charge
2 – 8 – 18 - 7
7
Will gain one electron
80 35 Br -1
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QuestionWhy do elements give off different colors of light when heated? (need to know for LAB on Friday)
Some of the electrons (ground state) gain enough energy from the heat to jump up to a higher energy level (excited state). They are unstable here so they jump back to a lower level and give off the energy gained as photons. The photon’s energy determines the frequency (and color) of light.
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Flame tests and SpectraEach element has a characteristic pattern of light that it emits.This can be used as a “fingerprint” for identification.
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Niels Bohr’s Atomic model
Yes! It’s Bohring!
http://videos.howstuffworks.com/hsw/5787-niels-bohrs-atomic-model-video.htm
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Assignment = Simple atomic models
1. a. Bohr’s modelb. isotope symbolc. charge
For these elements: S, As, Sr, Ar, Cl, Ag
2. Pg 145 # 10, 12-14 (show details for calculations)
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Modern views of the AtomElectrons can act as particles and sometimes as waves (dual nature)Electrons travel in paths that look like clouds. The size and shape of these depend on how much energy the electrons have.The 4 quantum numbers describe the location of the electrons:Principal QN (symbol “n”) refers to the number of energy levels and indicates the relative size and energies in the atomic orbitals.
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Secondary or angular QN (symbol “l” ) indicates the sublevel (s, p, d, or f)Magnetic QN (symbol “m”) indicates the orbital the electron is in (px, py or pz)
Spin QN (symbol “s” ) indicates the direction the electron is spinning (left or right)There are 7 energy levels divided into different sublevels which are divided into orbitals. An orbital is the space where two electrons travel. They have the shape of the sublevel but different orientations.Sublevels:s = 2 e- max p = 6 e- d = 10 e- f = 14 e-
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“s” =
“p” =
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Shape of d
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Shape of f
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Mind Blowing!!Just imagine an atom with for example 92 electrons like Uranium. All are whizzing around the nucleus at the speed of light in different shaped paths.
Just read
Video orbitals!http://www.youtube.com/watch?v=K-jNgq16jEY&feature=related
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Electron configuration (long form)
This gives MORE information about predicting properties. The placement of an elements electrons is written as:
1s2, 2s2, 2p6, 3s2, 3p6
These add up to total # of e-4p6
4th Energy level 6 electrons
Sublevel p
How many total electrons?
What element is it?
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There are rules!Aufbau rule: Electrons occupy the lowest energy orbitals first.Hund’s rule: States that single electrons must occupy separate orbitals before pairing up.Pauli Exclusion Principle: No two electrons in an atom have all 4 quantum numbers the same. One quantum number must be different. Aka SPIN!
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The “Arrow” DiagramElectrons arrange themselves in orbitals of increasing energy.
This is on page 160.
s = 2 p = 6 d= 10 f = 14
Examples:
N
Al
K
Br
Ag
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Take sulfur for example. It has an atomic number of 16, so it has 16 electrons. Let’s put these in order.
1s2, 2s2, 2p6, 3s2, 3p4
Valence e-? _____ on level ____How many e- lost/gained? _______Charge of ion? _______Check it! it should be in group 6 and on period 3 ……is it?
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Practice
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p3
Write the electron configuration (long form) for:Arsenic ____ electrons
And for arsenic’s ion? (As3-)
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Practice
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6 , 5s2 , 4d9
Write the electron configuration (long form) for:Silver ____ electrons
And for silver ion? Hint: it loses one e-)
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HWpg. 160 #21 & 22 and WS
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BellringerTurn in HW pg 160 (21, 22)A) Write the long-form electron configuration for V (23)
B) tell how many valence e- it hasC) give the ionic charge
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d3 ; 2; 2+
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Bellringer 21. Which QN symbol means “main
energy level”?2. Which 4 symbols means “sublevel”?3. Write the long configuration for Se
(34)
4. How many valence electrons are there?
5. What will the charge of the ion be?
n
62-
s, p, d, f
1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p4
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Electron configuration Shorthand version (Noble
gas version)Ex Silver = [1s2, 2s2, 2p6, 3s2, 3p6, 4s2, 3d10, 4p6 ], 5s2 , 4d9
Take the previous Noble Gas and substitute[Kr], 5s2 , 4d9
Or do directly from PT……
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Copy or memorize… or Google
“f” before “d” d (n-1) and f (n-2)
→ ← 7p →
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More….
1. Oxygen
2. And O2- ??
3. Arsenic
4. Aluminum
5. And Al3+ ??
6. Europium
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More Practice
Fe 3+
F1-
Na1+
N 3-
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Rules? …..What rules?1. Electrons can behave as a particle but
also have wavelike behavior (dual-nature by DeBroglie)
2. Electrons will be in the lowest available energy position first. (Aufbau rule)
3. Electrons will be in separate orbitals (same energy) before pairing up. (Hund’s rule)
4. Electrons will orient themselves to have opposite spins if in same orbital. (Pauli rule)
What??? Let’s try applying this…..
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Orbital diagramsWe use boxes to indicate the orbitals
And arrows to indicate each electron
1s 2s 2p 3s
4d
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Practice
Let’s do oxygen (8e-)
So…it has 2 unpaired electrons to use for bonding with other elements.And now aluminum (13 e-)
1s 2s 2p 3s 3p
2s 2p 3s 3p1s
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More
Let’s do Neon (10 e-)
And now chlorine (18 e-)
1s 2s 2p 3s 3p
2s 2p 3s 3p1s
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AndVanadium
Selenium
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Bellringer
1. Turn in Homework
2. What is the long form electron configuration for sulfur? See
pg 160
3. How many valence electrons does it have and on what level?
4. How many e- does it need to have a complete valence level?
5. What is the short form and orbital diagram for Te (52)?
6. What is wrong with this? [Ar] 4s2, 3d6 , 4p3
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Practicea) Bohr modelb) long formc) Short formd) Orbital diagrame) Valence e-
Pd Ge Pb
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Homeworka) Bohr modelb) long formc) Short formd) Orbital diagrame) Valence e-
At (85) K(19) Se (34) P(15)
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Videohttp://www.youtube.com/watch?v=xH1k1dtgiVY
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Electron Dot DiagramsOnly show valence electronsExamples:
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Assignment
Pg 167 (Glencoe)# 81, 85, 86, 87, 90
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To turn in!Write the: a) short electron configuration.b) # of valence e c) # e- lost/gainedd) charge of ion
1. iodine 5. helium2. hafnium 6. boron3. francium 7. yttrium4. xenon 8. tin
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Exit slip
For the element Phosphorous (P) and Bromine (Br)
Write the: a) short electron configuration.b) # of valence e c) # e- lost/gainedd) charge of ione) orbital diagram
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Bellringer1. What is the long form electronWhich
symbol means “main energy level”?2. Which symbol means “sublevel”?3. Which symbol means “number of
electrons”?4. How many valence electrons are
there?5. What will the charge of the ion be?
[Ar] 4s2, 3d10 , 4p3
3 or 4
52, 3 or 10
3-
s, p or d
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Bellringer
1. What symbol is used in orbital diagrams to show one electron?
2. What rule says that electrons will occupy the lowest energy orbitals first?
3. Who first stated that electrons can behave both as a particle and as a wave?
4. What do we call the distance on a wave for a complete cycle?
5. What do we call the height (energy) of a wave?
An arrow
Aufbau
DeBroglie
Wavelength
Amplitude
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To turn in!Write the: a) Bohr sequence (ex 2-8-3)b) long electron configuration.c) # of valence e d) # e- lost/gained, charge of ion
1. Palladium 5. Argon2. Indium 6. Molybdenum3. Gadolinium 7. Polonium4. Dysprosium 8. Radium
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EMR (electromagnetic radiation)
All wavelengths = from gamma rays (very short=high energy) to radio and TV (long=low energy).All types of EMR travel at the speed of lightAre emitted when excited electrons jump to lower energy levels.A “piece” or quantum of EMR is called a photon.
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Review EMR waves
or crests
A Solving problems Show all your work, write the equation and be sure to indicate your units c= v and E photon = h v
speed of light is c=3.00 x 108 m/s Planck’s constant is h = 6.626 x 10-34J s
1) What is the wavelength of electromagnetic radiation with a frequency of 8.77 x 1014 Hz?
2) What is the frequency of light that has a wavelength of 400. nm?
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MoreCalculate the frequency for yellow light See handout
600 nm = 600 x -9 m
Calculate the frequency for a bar-code laser.
660 nm = 660 x 10 -9 m
Calculate the energy for an X-ray photon (3.88 x 10 17 Hz)
5.00 x 10 14 1/s
4.55 x 10 14 1/s
2.57 x 10 -16 J