10.4 energy levels of electrons electrons move in definite energy levels; these are labeled 1 - 7...
TRANSCRIPT
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10.4 Energy Levels of Electrons
• Electrons move in definite energy levels; these are labeled 1 - 7
• Each level has sublevel(s) which are probability shapes that show where the electrons may be at any one time. Also known as orbitals.
• S orbital can hold up to 2 electrons (0, 1, 2)• p orbital can hold up to 6 electrons (0-6)• d orbital can hold up to 10 electrons (0-10)• f orbital can hold up to 14 electrons (0-14) • Aufbau chart shows how electrons fill into the
main energy levels and the sublevels or orbitals
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Energy Levels and Sublevels
• 1s• 2s 2p• 3s 3p 3d• 4s 4p 4d 4f• 5s 5p 5d 5f• 6s 6p 6d 6f• 7s 7p 7d 7f
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Aufbau Diagram or Chart
• 1s START HERE and follow• 2s 2p the arrows!• 3s 3p 3d• 4s 4p 4d 4f• 5s 5p 5d 5f• 6s 6p 6d 6f• 7s 7p 7d 7f
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Electron Configuration
• 4 Be
• 1s2 2s2
• 15 P
• 1s22s22p63s23p3
• 25 Mn
• 1s22s22p63s23p64s23d5
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Pauli Exclusion Principle
• Pauli exclusion principle states that no more than 2 electrons can be in the same suborbital. Even so, this would cause them to have precisely the same quantum address. So Pauli decided there has to be a way to tell one electron from another. In other words, they must differ by at least one quantum number!
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Pauli Exclusion Principle
• So they invented spin (+1/2 or -1/2) called spin up and spin down. Has nothing to do with the direction of the electron--we don’ t know how they move just where they may be at with 90% chance of finding it inside the energy level and orbital designated.
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Hund’s Rule
•Hund’s rule states that electrons fill unpaired until there is no more room then they will pair (applies to p, d and f orbitals)
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Orbital Diagrams
S orbitals get one box
P orbitals get 3 boxes (2 e- per box)
D orbitals get 5 boxes and f gets 7
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Orbital Diagrams (cont.)
• Insert electrons (using arrows into each box according to Hund’s and Pauli)
2 p3
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Answer
• 2p3 (arrows can all point up or down)
• Now try 4f10
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Answer to 4f10
• Arrows may point up or down if they are in boxes individually; however, if there are 2 electrons in a box, one must point up and one down.
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Electrons and the Periodic Table Revisited
History of the TablePeriodic Law
Important People
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Mendeleev
• Mendeleev was a Russian chemist who arranged the known elements in vertical columns in order of increasing mass and noticed a pattern in physical and chemical properties
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Mosley
• Mosley was a British physicist who determined the atomic number (number of protons) of the atoms of elements and then arranged the elements according to their atomic number.
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Periods and Groups
• Periods of the periodic table are the rows across
• Groups or Families are columns on the periodic table.
• Currently we have 18 groups. We will use the 1-18 designations not the A/B or Roman Numerals
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Areas of the Periodic Table
•Representative elements or Main Group are those that are in Groups 1, 2, 13, 14, 15, 16, 17, 18
•Transition elements are Groups 3 - 12 , also called the Heavy Metals
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Inner Transition
• Rare Earth elements that are located in the bottom two rows (away from the rest of the table) of the periodic table
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Periodic Table GROUP NUMBERS
Heavy Metals or Transition elements
Main group
Main Group or Representative elements
Inner Transition Elements
1
2
3
4
5
6
7
Period Numbers
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Groups with names
• Group 1 = Alkali Metals• Group 2 = Alkaline Earth Metals• Group 18 = Inert or Noble Gases• Group 17 = Halogens
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Periodic Table and Electron Configuration
• The light metals compose the s block.
• The transition elements are the d block.
• The nonmetals are p block. • The inner transition (rare earth)
metals are the f block.
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Periodic Table
1
2
3
4
5
6
74f
5f
4
5
6
7
3
4
5
6
s block
d block
p block
f block
Noble (inert) gases
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Complete the electron configurations for the Noble Gases (Hint: Group 18)
• He • 1s2
• Ne • 1s22s22p6
• Ar = • 1s22s22p63s23p6
• Kr = • 1s22s22p63s23p64s23d104
p6
• Xe = 1s22s22p63s23p64s23d104p6
5s24d105p6
• Rn = 1s22s22p63s23p64s23d104p6
5s24d105p66s24f145d106p6 Except He, do you see a trend in all of the noble gas configurations?
• What do they all end in?
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Shorthand Notation
• We use the noble gases in shorthand notation
• Find the closest noble gas that has an atomic number LESS than that of the element
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Example • Ex. K • What is K’s atomic number? • 19• Closest noble gas?• Ar• What is Ar’s atomic number?• 18 = 1s22s22p63s23p6
• = [Ar] 4s1 = Means the first 18 electrons are arranged like argon and the last electron is called the VALENCE ELECTRON (outermost shell)
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Example for you to try
•You try Ba•Ba = [Xe] 6s2
•Try Pb•Pb = [Xe] 6s24f145d106p2