honors chemistry september 16, 2013. preview of lesson where are electrons found around the nucleus?...
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Honors Chemistry
September 16, 2013
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Preview of Lesson• Where are electrons found around the nucleus?• 4 different shaped orbitals (x-ray diffraction and
electron microscopy)– s, p, d, f
• Higher energy levels have more shapes• Each orbital can hold 2 e-
– Locate the e- 90% of the time
• Orbital is also called Subshells
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Bohr's ModelBohr's Model
• Model ofelectronsin fixedorbits to explain quantization Figure 6.14
• Transitionsbetweenorbitsemits orabsorbslight 07m07an107m07an1
07m07an1.mov.lnk
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Observation of unique line spectra led to Quantum Theory
Nucleus
First
Second
Third
FourthE=hν
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Orbital Diagrams and Electron Configurations
• n = Principle quantum number • Describes the energy level the electron occupies (PT)
n = 1
n = 2n = 3n = 4
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Orbital Energy Levels
Ground stateGround state
Excited statesExcited states
• Shape of orbitaldesignated by theletters
s, p, d, f
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Shapes of OrbitalsShapes of Orbitals• Shape of orbital designated by the letters
s, p, d, f• Orbitals have
different shapes
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The s orbital has a spherical shape centered aroundthe origin of the three axes in space.
s Orbital shapes Orbital shape
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There are three dumbbell-shaped p orbitals in each energy level above n = 1, each assigned to its own axis (x, y and z) in space.
p orbital shapep orbital shape
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Things get a bit more complicated with the five d orbitals that are found in the d sublevels beginning with n = 3. To remember the shapes, think of “double dumbells”
…and a “dumbell with a donut”!
d orbital d orbital shapesshapes
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Shape of f orbitalsShape of f orbitals
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CombinationCombination
of electronof electron
microscopymicroscopy
and x-rayand x-ray
diffractiondiffraction
producedproduced
image ofimage of
orbitalsorbitals
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Sets of Orbitals (Subshells)Sets of Orbitals (Subshells)
• Depending on the type of orbital, we find that they occur in sets differing in their orientationsets differing in their orientation in space in space
• s - set of 1• p - set of 3• d - set of 5 • f - set of 7
• Label P.T.
Orbitals.exe.lnk
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Sizes of orbitals• Size depends on the value of n
• Orbitals with the same n are about the same size
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Check for understanding
• What is the principal quantum number for Ar?• What are the subshells?• How many sets of electrons are found in each
subshell?
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Electron Configurations of Some Atoms(Stop P1 + 5)
Electron Configurations of Some Atoms(Stop P1 + 5)
• The firstten elements
1s1
1s2
1s2 2s1
1s2 2s2
1s2 2s2 2p1
1s2 2s2 2p2
1s2 2s2 2p3
1s2 2s2 2p4
1s2 2s2 2p5
1s2 2s2 2p6
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Shorthand Notation for OrbitalsShorthand Notation for Orbitals• Combinations of first two quantum numbers;
number of orbital types equals the shell number (n).
• 1s• 2s, 2p• 3s, 3p, 3d• 4s, 4p, 4d, 4f• 5s, 5p, 5d, 5f, (5g)• 6s, 6p, 6d, 6f, (6g, 6h)
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Refer to electron configuration worksheet
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Agenda
• Brain Teaser• Grade Worksheet• Review
– Writing Electron Configuration
• Notes: Orbital Diagram• Homework
– Short Hand Electron Configuration– Orbital Diagram
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Grade Homework
• Refer to Worksheet (Arrangement of Electrons I)
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Check for understanding (P6)
• What is the principal quantum number for Ar?• What are the subshells?• How many sets of electrons are found in each
subshell?
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Aufbau Principle
• Aufbau Principle: start with the nucleus and empty orbitals, then “build” up the electron configuration using orbitals of increasing energy
Aufbau.exe
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Electron ConfigurationsElectron Configurations
• Electron Spin and Pauli Exclusion Principle:– Only two electrons can occupy a
single orbital and they must have opposite spins
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Electron Configurations
• Hund's Rule: –When filling a subshell, such as the set
of 3 p orbitals, place 1 electron in each before pairing up electrons in a single orbital
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Electron Configurations
• Arrangement of electrons in the orbitals is called the electron configuration of the atom
• The ground state configuration can be predicted, using the Aufbau Principle, the Pauli Exclusion Principle, and Hund’s Rule.
Electron configurationsElectron configurations Filling _ rules.exeFilling _ rules.exe
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How do we know what the filling order is?
• What chemistry tool might we rely on?
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Electron Configurations and the Periodic Table
Electron Configurations and the Periodic Table
• Valence electron configurations repeat down a group
aufbau.exe.lnk
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Ground state electron configurations
• Example: Li– atomic number = 3– nucleus has 3 protons– neutral atom has 3 electrons
• 2 electrons in 1s orbital, 1 electron in 2s orbital
1s
2s
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Different ways to show electron configuration
Read this “one s two”not “one s squared”
1s
2s
1s 2s
Li 1s2 2s1
Energy level diagram Box notation
Spectroscopic notation
Write the superscript 1.Don’t leave it blank
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Practice
• Review (on separate sheet of paper)– Electron Configuration– Orbital Diagram
• Electron configuration worksheet
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Using the Periodic Table
The last subshell in the electron configuration is one of these(row #) s (row # – 1) d(row #) p (row # – 2) f
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The f-block is inserted into to the d-block
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Electron configuration of O• Atomic number of O = 8 so neutral atom has 8 e–
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Electron configuration of Co• Atomic number of Co = 27 so neutral atom has 27 e–
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Simplifying electron configurations• Build on the atom’s noble gas core
• He 1s2
O 1s22s22p4
O [He]2s22p4
• Ar 1s22s22p63s23p6
Co 1s22s22p63s23p64s23d7
Co [Ar]4s23d7
1s 2s 2p
3s 3p
4s 3d
1s 2s 2p
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Noble Gases
• Far right of the periodic table• These elements are extremely unreactive or
inert• They rarely form compounds with other
elements
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Noble Gas electron configurations
• What is the electron configurations for Neon
• Abbreviated way to write configurations– Start with full outer shell then add on
• Br• Ba
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Noble Gases
• Neon- emits brilliant light when stimulated by electricity – neon signs- 4th most abundant element in the universe.
• Helium- light non reactive gas- used balloons- inexpensive, plentiful and harmless
• Radon- radioactive gas- can cause cancer- colorless, odorless emitted from for certain rocks underground
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• Properties of atoms correlate with the number and energy of electrons
• Electron configurations are used to summarize the distribution of electrons among the various orbitals
Why are we doing all of this?Why are we doing all of this?
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PracticePractice
3-3 PracticeWrite the complete electron
configurations and noble gas shorthand #1-4
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Practice
1. Refer to a periodic table and write the electron configurations of these atoms.
2. Write the configurations using shorthand notation.
• Zn
• I
• Cs
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The f-block is inserted into to the d-block
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Find the electron configuration of Au
• Locate Au on the periodic table
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Find the electron configuration of Au
• Au [Xe]• The noble gas core is Xe
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Find the electron configuration of Au
• Au [Xe]6s2
• The noble gas core is Xe• From Xe, go 2 spaces across the s-block in the 6th row 6s2
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Find the electron configuration of Au
• Au [Xe]6s24f14
• The noble gas core is Xe• From Xe, go 2 spaces across the s-block in the 6th row 6s2
• Then detour to go 14 spaces across the f-block 4f14
– note: for the f-block, n = row – 2 = 6 – 2 = 4
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Find the electron configuration of Au
• Au [Xe]6s24f145d9
• The noble gas core is Xe• From Xe, go 2 spaces across the s-block in the 6th row 6s2
• Then detour to go 14 spaces across the f-block 4f14
– note: for the f-block, n = row – 2 = 6 – 2 = 4• Finally go 9 spaces into the d-block on the 6th row 5d9
– note: for the d-block, n = row – 1 = 6 – 1 = 5
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Electron configuration of ions
• What is an ion?• How many electrons does Cl1- have?
– What is the electron configuration for the chloride ion?
• How many electrons does Ca2+ have?– What is the electron configuration for the calcium
ion?
• What do you notice?
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Practice
• Draw the orbital diagram for sulfur.– What ion does sulfur want to form and why?
• Draw the orbital diagram for Potassium.– What ion does sulfur want to form and why?
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What does this mean
• Properties of atoms correlate with the number and energy of electrons
• Atoms like to have full outer shells.
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Why is this important
Valence electrons• Electrons in the outermost energy level
– Where all the action occurs
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Practice
• Whiteboard - Atomic Structure (continued)
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Team• Write the electron configuration for silver.• Write the noble gas configuration for silver.• What element has the following electron configuration?
1s22s22p6 3s23p64s23d4
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Today we use aspects of line spectrum to identify elements,
compounds and mixtures?
• UV-Vis Spectrometer– Distances and types of stars– Blood test- carbon monoxide poisoning– Mobile weapons detectors– Chlorophyll
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How we determine these energy levels?