Q3 : Week 2 – 2/6 – 2/10

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TODAY’s NOTES:

Electrons are arranged from lowest energy to higher energy = Aufbau Principle

 So they fill from lower n to higher n  and from lower energy orbitals (l) to higher energy orbitals. Electrons fill sublevels in order ( s,p,d,f).

 

Electron are arranged in        n = principle energy levels

                                                    l  = sublevels

                                                 m_s =  individual orbitals (actual 3 -d shape where pairs of electrons can exist)

 

Every Electron has a unique set of 4 quantum numbers (including spin m_s) = Pauli Exclusion Principle

These quantum numbers describe how the electrons are arranged in the atom based on energy.

 

                                      The basic organization is principle energy level (n = 1, 2, 3, etc.) – “shell”

 

                                                                                     sublevel  (s,  p,  d,  f, ) – type of orbital and all of its orientations

                                                                                                   l = 0,  1,   2,  3

 

                                                                                      orbital (individual orbital of a single orientation of a sublevel)

                                                                                                        m_l = -l , 0, +l

 

This arrangement uses notation that describes the organization of the electrons in principle energy levels and sublevels. The exponent is the number of electrons in the TOTAL sublevel that includes all the orbitals of different orientation of the same sublevel.

 

s = 1 orbital   (l = 0, m_l = 0)

p = 2 orbitals (l = 1, m_l = -1,  0, +1)

d = 5 orbitals (l = 2, m_l = -2, -1, 0, +1, +2)

f  = 7 orbitals (l  = 3, m_l = -3, -2, -1, 0, +1, +2, +3)

g =  ?

 

Electron configuration of Al:           Nucleus:  1s²2s²2p⁶3s²3p¹

 

Orbital notation for Al:

Each box represents a single orbital.

 

Which electrons are the most stable? Unstable?

 

*Connections – Our quantum numbers refer to specific energy levels allowable by each quantized element.  The arrangement of electrons in quantized energy orbitals that were solutions to the Erwin Schrodinger equation (quantum numbers) are actually hidden in the periodic table that was already arranged according these energy levels (unbeknownst to Mendeleev and Moseley!!) The periodic table that we use is a condensed version that does not insert the  f block ( l = 3) because it would not fit on most pages!!!!

 

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2/6 – Monday’s Homework: – 

_______________________________________________________________________                                  Jump to: Tuesday Homework / top

2/7 – Tuesday – A Day – 2/3a Lab, 4   

TODAY’s NOTES:

Electrons are arranged from lowest energy to higher energy = Aufbau Principle

 So they fill from lower n to higher n  and from lower energy orbitals (l) to higher energy orbitals. Electrons fill sublevels in order ( s,p,d,f).

 

Electron are arranged in        n = principle energy levels

                                                    l  = sublevels

                                                 m_s =  individual orbitals (actual 3 -d shape where pairs of electrons can exist)

 

Every Electron has a unique set of 4 quantum numbers (including spin m_s) = Pauli Exclusion Principle

These quantum numbers describe how the electrons are arranged in the atom based on energy.

 

                                      The basic organization is principle energy level (n = 1, 2, 3, etc.) – “shell”

 

                                                                                     sublevel  (s,  p,  d,  f, ) – type of orbital and all of its orientations

                                                                                                   l = 0,  1,   2,  3

 

                                                                                      orbital (individual orbital of a single orientation of a sublevel)

                                                                                                        m_l = -l , 0, +l

 

This arrangement uses notation that describes the organization of the electrons in principle energy levels and sublevels. The exponent is the number of electrons in the TOTAL sublevel that includes all the orbitals of different orientation of the same sublevel.

 

s = 1 orbital   (l = 0, m_l = 0)

p = 2 orbitals (l = 1, m_l = -1,  0, +1)

d = 5 orbitals (l = 2, m_l = -2, -1, 0, +1, +2)

f  = 7 orbitals (l  = 3, m_l = -3, -2, -1, 0, +1, +2, +3)

g =  ?

 

Electron configuration of Nitrogen:           Nucleus:  1s²2s²2p³

 

Orbital notation for N:

Each box represents a single orbital.

 

The orbital diagram of Nitrogen above reveals a new situation where electrons will occupy empty orbitals OF THE SAME SUBLEVEL before they pair up in a single orbital.

This did not occur in the s sublevel because there is only 1 orbital in the s sublevel.

 

IF l = 0 (s sublevel) → ml = 0 (only 1 solution thus only 1 orbital for the s sublevlel)  thus a second electron had no other choice but to pair up in an s orbital due to the Aufbau Principle. That is this second electron was more stable (lower in energy ) in a paired s orbital than a p orbital of higher energy.

 

 If the electron in an sublevel with multiple degenerate orbitals (different orientations in space) will occupy an empty orbital before pairing up = Hund’s Rule.

 

*Connections – Our quantum numbers refer to specific energy levels allowable by each quantized element.  The arrangement of electrons in quantized energy orbitals that were solutions to the Erwin Schrodinger equation (quantum numbers) are actually hidden in the periodic table that was already arranged according these energy levels (unbeknownst to Mendeleev and Moseley!!) The periodic table that we use is a condensed version that does not insert the  f block ( l = 3) because it would not fit on most pages!!!!

 

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2/7 – Tuesday’s Homework: – 

1.  Please complete Atomic Structure 4b -Electron configuration.pdf worksheet and review the key if you have not done already.    

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2/8 – Wednesday – B Day – 2, 3b/4 Lab

TODAY’s NOTES:

Important Vocabulary that you will need in this unit:

 

Z  = #of protons    synonyms:    Z = nuclear charge and   Z = Atomic Number (Thanks Moseley!)

 

Z_eff = effective nuclear charge – (the nuclear charge that the electron feels as a result of electron – electron interactions ( screening or electron – electron repulsions).

 

n = principle energy level, the larger the n the larger the number of core electrons 

                                                      and larger the orbitals. n defines the proximity of electrons to the  

                                                      nucleus.  The farther that an electron is from the nucleus the lower the  

                                                      coulombic  attractions that the electron feels and thus is less stable           

                                                      than electrons closer to the nucleus.

 

Armed with Z, Z_{eff, and n you can explain almost everything in periodicity and electron}  

                                                                                                                                           _{configurations.}

 

_{****Since we are continuously evaluating the energy levels of electrons that are bound in an atom or ion in this unit, Ionization energy values are very helpful in determining stability of an electron.}  

 

_{Ionization Energy = the energy needed to remove an electron (Einstein’s Binding Energy).}

                                             _{Electrons with higher IE are more stable (takes more energy to remove!)}

                                             _{Electrons with lower IE are less stable (takes less energy to remove!)} 

 

Example for Na (sodium):                  IE₁          +            Na     —->      Na⁺        +         e- 

                                                      _{first Ionization Energy}

 

_{Ionization Energy is often described as the First Ionization Energy (1st IE) or the Second Ionization Energy (2nd IE) and so on…} 

 

_{– The Second Ionization Energy is the Energy needed to remove a second electron (after a single electron was removed)}

     

                                                                   IE₂          +           Na⁺     —->      Na⁺²        +         e-

                                                              _{Second Ionization Energy}

So the 2nd IE is the energy needed to remove the second electron.  Would it require the same amount as the 1st IE?  No it would require much more because Na⁺ the second electron would be removed from a filled principle energy level!! These are core electrons that are more stable. Do not lose site that IE is a measure of electron stability.

 

Stable Electrons =          High coulombic attraction to nucleus =         lower energy orbitals =      High IE

   Lower energy                               Lower n, Higher Z_{eff                               closer to the nucleus}

 

Successive IE values have verified the existence of Valence electrons!!! Look at the diagram below.

Notice when a successive IE “JUMPS THROUGH THE ROOF”.   

                    

                              Na (atom) :   1s²2s²2p⁶3s¹                                             Na⁺¹ (atom):  1s²2s²2p⁶

 

           Removing valence electron (less stable)                    Removing a core electron (more stable)

                          3s electron has higher n                                             2p electron has lower n            

                         3s electron has lower Zeff                                    2p electron has higher Zeff

                                   Z = 11                                                                                       Z = 11

                           

                            IE₁  =   500 kJ/mol          —— 9 x increase——->              IE₂ = 4560 kJ/mole

                           removing valence e^–     “jumps through the roof”           removing core e^–

 

                                                               Thus Na has 1 valence electron                               

 

 

– Wrote the electron configuration of Uranium and Ag / Ag⁺ /Shorthand/ and U⁺⁶

 

                                                                  “ALL of  This is about Energy “

 

ALL of this is about Energy Lecture!

                                                                                                                              

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2/8 – Wednesday Homework: –

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2/9 – Thursday – A Day – 2/3a Lab, 4 

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2/9 – Thursday Homework: –

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2/10 – Friday – B Day – 2, 3b/4 Lab

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2/10 – Friday Homework: –

1. Complete th