10.4 Energy Levels of Electrons
description
Transcript of 10.4 Energy Levels of Electrons
![Page 1: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/1.jpg)
10.4 Energy Levels of Electrons
Electrons move in definite energy levels; these are labeled 1 - 7
![Page 2: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/2.jpg)
Sublevels in each of the 7 main energy levels
• Each level has sublevel(s) which are probability shapes that show where the electrons may be at any one time. Also known as orbitals.
![Page 3: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/3.jpg)
S orbital can hold up to 2 electrons
![Page 4: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/4.jpg)
P orbital can hold up to 6 electrons
![Page 5: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/5.jpg)
D orbital can hold up to 10 electrons
![Page 6: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/6.jpg)
F orbital can hold up to 14 electrons
![Page 7: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/7.jpg)
How do they fill?
• Aufbau chart shows how electrons fill into the main energy levels and the sublevels or orbitals
![Page 8: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/8.jpg)
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
![Page 9: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/9.jpg)
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
![Page 10: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/10.jpg)
Electron Configuration
• 4 Be
• 1s2 2s2
• 15 P
• 1s22s22p63s23p3
• 25 Mn
• 1s22s22p63s23p64s23d5
![Page 11: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/11.jpg)
Now begin working HW
Handout #1
![Page 12: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/12.jpg)
Q. O. D.—Show how you solved it! _______1. The element with atomic number 53 containsa) 53 neutrons b) 53 protons C) 26 neutrons & 27 protons d) 26 protons & 27
neutrons
108
_______2. The number of neutrons in an atom of 47 Ag isa) 47 b) 108 c) 155 d) 61
27
_______3. The number of electrons in an ion of 13 Al3+ isa) 13 b) 10 c) 27 d) 14
_______4. What is the relative atomic mass of boron if two stable isotopes of boron have the following mass and abundance:
10.0129 amu (19.91%) & 11.0129 (80.09%)a) 10.81 amu b) 10.21 amu c) 10.62 amu d) 10.51
amu
![Page 13: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/13.jpg)
Hund’s Rule
•Hund’s rule states that electrons will fill a subshell unpaired until it cannot occupy a subshell unpaired and has to pair. (Applies only to p, d, and f)
![Page 14: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/14.jpg)
Pauli Exclusion Principle
• According to the Pauli Exclusion Principle, states that when two electrons must occupy the same subshell they will have OPPOSITE spin. One will be symbolized by an UP arrow and the other by a DOWN arrow. Such as this example.
![Page 15: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/15.jpg)
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.
![Page 16: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/16.jpg)
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
![Page 17: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/17.jpg)
Orbital Diagrams (cont.)
• Insert electrons (using arrows into each box according to Hund’s and Pauli)
2 p3
![Page 18: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/18.jpg)
Answer
• 2p3 (arrows can all point up or down)
• Now try 4f10
![Page 19: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/19.jpg)
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.
![Page 20: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/20.jpg)
Now begin working on the lab activity
Electron Configurations
![Page 21: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/21.jpg)
#5.
![Page 22: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/22.jpg)
#9.
![Page 23: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/23.jpg)
Electrons and the Periodic Table
History of the TablePeriodic Law
Important People
![Page 24: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/24.jpg)
1. 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
![Page 25: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/25.jpg)
2. 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.
![Page 26: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/26.jpg)
3. Arrangement of Periodic Table
• The current periodic table is arranged in order of increasing atomic number.
![Page 27: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/27.jpg)
11. Periodic Law
• According to Mendeleev, “"The properties of the elements are a periodic function of their atomic masses"
• According to Mosley, the periodic table was arranged according to atomic number and patterns repeat periodically
![Page 28: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/28.jpg)
4. Periods
• Periods of the periodic table are the horizontal rows across
![Page 29: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/29.jpg)
5. Groups
• Groups or Families are vertical columns on the periodic table.
• Currently we have 18 groups. We will use the 1-18 designations.
![Page 30: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/30.jpg)
6. Make it into a true statement
• Elements of the same group are very similar.
![Page 31: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/31.jpg)
7. Change to a True Statement
• The characteristic properties of the elements in a period change from group to group.
![Page 32: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/32.jpg)
![Page 33: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/33.jpg)
Property SummaryMetal Metalloid Nonmetal
Physical State
Boiling & Melting Point
Conductivity
Malleability
Ductile
![Page 34: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/34.jpg)
Property SummaryMetal Metalloid Nonmetal
Physical State Mostly Solids (Hg exception)
Solids Solids, liquids (Br), and gases
Boiling & Melting Point
High Intermediate Low
Conductivity Good Semi-conductors
Poor
Malleability Good Intermediate Poor
Ductile Good Intermediate Poor
![Page 35: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/35.jpg)
![Page 36: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/36.jpg)
Transition Elements
•Groups 3 - 12 are also called the Heavy Metals
![Page 37: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/37.jpg)
Inner Transition
• Rare Earth elements that are located in the bottom two rows (away from the rest of the table) of the periodic table
![Page 38: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/38.jpg)
Groups with names
• Group 1 = Alkali Metals• Group 2 = Alkaline Earth Metals• Group 18 = Inert or Noble Gases• Group 17 = Halogens
![Page 39: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/39.jpg)
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.
![Page 40: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/40.jpg)
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
![Page 41: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/41.jpg)
Shorthand Electron Configuration
Using Noble Gases to shorten the electron configuration
![Page 42: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/42.jpg)
Complete the electron configurations for the Noble Gases (Hint: Group 18)
• He • 1s2
• Ne • 1s22s22p6
• Ar = • 1s22s22p63s23p6
• Kr = • 1s22s22p63s23p64s23d104
p6
• Xe = 1s22s22p63s23p64s23d104p65s24d105p6
• Rn = 1s22s22p63s23p64s23d104p65s24d105p66s24f145d106p6 Except He, do you see a trend in all of the noble gas configurations?
• What do they all end in?
![Page 43: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/43.jpg)
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
![Page 44: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/44.jpg)
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)
![Page 45: 10.4 Energy Levels of Electrons](https://reader036.fdocuments.net/reader036/viewer/2022081506/56815086550346895dbe82de/html5/thumbnails/45.jpg)
Example for you to try
•You try Ba•Ba = [Xe] 6s2
•Try Pb•Pb = [Xe] 6s24f145d106p2