Electron Arrangement What do we know?

Electron Arrangement What do we know? e- are in the e- cloud

Electron Arrangement What do we know? e- are in the e- cloud e- are responsible for the volume of the atom

Bohr Model

e- move certain distances from the nucleus

Bohr Model e- move certain distances from the nucleus – close to nucleus have less E – E increases as e- move away from nucleus

e- move with certain speeds due to E

– give off E only when they move to a lower E level

e- move with certain speeds due to E – give off E only when they move to a lower E level outer most e- are called valence e- and have the most E

e- move with certain speeds due to E – give off E only when they move to a lower E level outer most e- are called valence e- and have the most E – valence e- determine behavior of atoms and are involved in bonding

Energy state of an e- is described by a set of 4 numbers called quantum numbers

Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of:

Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus

Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital

Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital 3.position of orbital in 3 axis of space

Energy state of an e- is described by a set of 4 numbers called quantum numbers QN - describe the most probable location of e- in terms of: 1.distance from the nucleus 2.shape of the orbital 3.position of orbital in 3 axis of space 4.direction of spin of e-

I. Principal Quantum Number

distance indicates the most probable distance of an e- from the nucleus

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e-

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K 2L 3M 4N 5O 6P 7Q

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L 3M 4N 5O 6P 7Q

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M 4N 5O 6P 7Q

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N 5O 6P 7Q

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N32 5O 6P 7Q

I. Principal Quantum Number indicates the most probable distance of an e- from the nucleus Energy LevelShellTotal # of e- 1K2 2L8 3M18 4N32 5O 6P… 7Q…

I. Principal Quantum Number can be determined from the period/series number on the periodic table

II. Orbital Quantum Number

indicates shape of the orbital cloud

II. Orbital Quantum Number indicates shape of the orbital cloud 4 orbital shapes, represented by letters

II. Orbital Quantum Number s lowest E p d f

II. Orbital Quantum Number s lowest E p d f highest E

II. Orbital Quantum Number max # e- s 2 p 6 d10 f 14

II. Orbital Quantum Number # of orbital shapes is = to the principal QN

Principal QN # orbital shapes types of orbitals

Principal QN # orbital shapes types of orbitals

Principal QN # orbital shapes types of orbitals 11 s 2 3 4

Principal QN # orbital shapes types of orbitals 11 s

Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 44

Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 s, p, d 44

Principal QN # orbital shapes types of orbitals 11 s 22 s, p 33 s, p, d 44 s, p, d, f

III. Magnetic Quantum Number

describes the orbital positions with respect to the 3 axis of space

III. Magnetic Quantum Number

describes the orbital positions with respect to the 3 axis of space each position, regardless of type can only hold a maximum of 2 e- describes the orbital positions with respect to the 3 axis of space each position, regardless of type can only hold a maximum of 2 e-

s orbital/sublevel

1 orbital position for “s”

s orbital/sublevel 1 orbital position for “s” spherical shape

s orbital/sublevel 1 orbital position for “s” spherical shape lowest possible energy sub-level

s orbital/sublevel 1 orbital position for “s” spherical shape lowest possible energy sub-level all energy levels have an s orbital 1s, 2s, 3s, 4s…

p orbital/sublevel

second energy sublevel… more E

p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level

p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level 6 total e- possible in “p” sub-group

p orbital/sublevel second energy sublevel… more E 3 possible “p” orbitals per E Level 6 total e- possible in “p” sub-group 2p, 3p, 4p, 5p…

d orbital/sublevel

5 possible “d” orbitals per E Level

d orbital/sublevel 5 possible “d” orbitals per E Level 10 total e- possible in “d” sub-group

d orbital/sublevel 5 possible “d” orbitals per E Level 10 total e- possible in “d” sub-group 3d, 4d, 5d…

f orbital/ sublevel

7 possible “f” orbitals per E Level

f orbital/sublevel 7 possible “f” orbitals per E Level 14 total e- possible in “f” sub-group

f orbital/sublevel 7 possible “f” orbitals per E Level 14 total e- possible in “f” sub-group 4f, 5f

Quantum number summary OrbitalsPositionselectrons

Magnetic Quantum Number Summary

ADD ADD these to your e- in Atoms Questions 13) What is the Octet rule? 14) Describe what happens to e- when atoms absorb energy? 15) How does quantum mechanics differ from classical mechanics?

Orbital Filling Chart

Order for filling orbitals 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d... Aufbau Principle – e- occupy orbitals of lowest E 1 st * 4s is lower E than 3d

Orbital filling chart

1s 2s2p 3s3p3d 4s4p4d4f 5s5p5d5f 6s6p6d6f …

Order for filling orbitals 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d...

e- configuration

Quantum Number Rewind

Orbital Filling Chart

e- configuration

Write the e- configuration for the following: 1.beryllium 2.carbon 3.sodium 4.magnesium 5.aluminum 6.potassium **EC: bromine

Quantum Numbers

Principle

[E level] (n)

Principle [E level] (n) Orbital

Principle [E level] (n) Orbital [shape] (l)

Principle [E level] (n) Orbital [shape] (l) Magnetic

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] (m)

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 )

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 )

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 )

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 2 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s p 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 3 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 p 36e- 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 4 p 36e- 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s p 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s p d 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p d 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p 36e- d 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- p 36e- d 510e- 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 9 p 36e- d 510e- 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s p d

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s p d f

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p d f

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d f

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d 510e- f

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- p 36e- d 510e- f 714e-

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e- 16 p 36e- d 510e- f 714e-

Principle [E level] (n) Orbital [shape] (l) Magnetic [positions per orbital] Number of e- per orbital Number of orbitals per sublevel (n 2 ) Maximum number of electrons (2n 2 ) 1 s 12e-12 2 s 1 48 p 36e- 3 s 12e- 918 p 36e- d 510e- 4 s 12e p 36e- d 510e- f 714e-

Write the e- configuration for the following: 1.beryllium 2.carbon 3.sodium 4.magnesium 5.aluminum 6.potassium **EC: bromine

e- configuration 1.Oxygen 2.fluorine 3.Silicon 4.Copper 5.Arsenic EC: krypton

IV. Spin Quantum Number

indicates the spin of e- (clockwise & counterclockwise)

IV. Spin Quantum Number indicates the spin of e- (clockwise & counterclockwise) Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin

Hund’s Rule – an e- can not enter a half filled orbital if an empty orbital of the same E is available

place 1 e- into each p, d or f orbital before pairing them Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin

Orbital Notation uses all 4 QN to represent e- arrangement

Orbital Notation Practice 1.Fluorine 2.Magnesium 3.Phosphorus 4.Argon 5.Manganese 6.Arsenic **EC: mercury

Write e- configuration and orbital diagrams for the following 1)Boron 2)Sulfur 3)Chlorine 4)Potassium 5)Cobalt 6)Copper 7)Iodine 8)barium

Pauli Exclusion Principle – no more than 2 e- per orbital, which must be of opposite spin -The 2 Electrons spin in different directions. -Notated as… ___ 1s Principle Energy Level and Orbital or “sub-level” [The 1 st 2 Quantum Numbers] Arrows = electrons