Electron Configuration Flashcards
What are main energy levels/ shells split into?
- Sub-shells (orbitals.)
What are the 4 types of orbitals?
- s,p,d,f.
How many sub-orbitals does an s orbital contain?
- One sub- orbital.
MAXIMUM NUMBER OF ELECTRONS IN SUB SHELL = 2
How many electrons does 1 sub- orbital hold?
- 2 electrons.
How many sub -orbitals does a p orbital cotain?
- Three sub- orbitals
MAXIMUM NUMBER OF ELECTRONS IN SUB-SHELL = 6
How many sub- orbitals does a d orbital contain?
- Five sub- orbitals
MAXIMUM NUMBER OF ELECTRONS IN SUB-SHELL = 10
What sub-shell does the first energy level have?
- An s sub-shell.(orbital)
What sub-shells does the second energy level have?
- An s sub-shell. (orbital)
- A p sub shell. (orbital)
What sub-shells does the third energy level have?
- An s sub-shell (orbital)
- A p sub-shell (orbital)
- A d sub-shell (orbital.)
What sub-shells does the fourth energy level have?
- An s sub shell (orbital)
- A p sub shell (orbital)
- A d sub shell (orbital)
- (A f sub-shell.)
What order are the sub-shells filled with electrons in?
(Draw out diagram/ do cross down technique.)
1s, 2s, 2p,3s,3p,4s,3d,4p,5s, 4d, 5p, 6s
Finish sentence
Groups 1 and 2 are ….. ……. elements.
s block
FIllin gaps
Groups 3 to 12 are ….. ……. elements.
d block
Fill the gaps
Groups 3 to 0 are ….. ….. elements
p block.
Explain what each aspect of this configuration: (1s¹) means
- 1 = first MAIN ENERGY LEVEL.
- s: type of orbital.
- 1 = number of electrons in the orbital.
What is an orbital?
- Orbital: a region of space where there is a high probability of finding an electron.
What equation will allow you to calculate the total number of electrons found in n main energy level?
2n²
What shape does the s sub-shell have?
- A spherical shape.
What is the shape of the p orbital?
- Each sub-orbital in p orbital in shape of dumbell.
- All together = shape of flower
Refer to Gautum notes if needed.
Give two reasons why the 1s orbital is the most stable.
- Closest orbital to nucleus.
- Posesses least amount of energy.
Finish the sentence
As the energy of the orbitals increase, the stability of the orbitals …….
- Decreases.
How many sub-orbitals is f orbital made up of?
- 7 sub -orbitals
MAXIMUM OF 14 ELECTRONS OVERALL
What are the two elements that are the exceptions to filling orbitals in order and then moving onto the next (ie. they have a half-filled orbital?)
- Chromium
- Copper.
What would you EXPECT the electron configuration of chromium to be?
What actually is the configuration?
- EXPECT: 1s²2s²2p⁶3s²3p⁶4s²3d⁴
- ACTUAL:
- 1s²2s²2p⁶3s²3p⁶4s¹3d⁵
(Only PARTIALLY FILLED s orbital.)
What would you expect the electron configuration of copper to be? What actually is the configuration?
EXPECT:
- 1s²2s²2p⁶3s²3p⁶4s²3d⁹
ACTUAL:
- 1s²2s²2p⁶3s²3p⁶3d¹⁰4s¹
Why is the s orbital only partially filled in chromium and copper (ie. only one electron filled in s orbital and the electrons start filling in d orbital straight awa?)
- The arrangements are of lower energy so are more stable.
What property do electrons have (beginning with s?)
- Spin.
What is the spin of two electrons in the same orbital like?
- ## They have opposite spins.
What are electrons represented by in the spin diagrams? What does the direction of the arrows show?
- Electrons are represented by arrows.
- Direction of the arrows show the different directions of spin.
When doing box diagrams (ie. bus seating) how are the electrons filled in the sub-orbitals?
- You fill each sub-orbital individually before you start to pair the electrons up.
- Ie. if you had a p orbital –> 3 sub-orbitals and there were 3 electrons, the 3 electrons would go in the 3 separate sub orbitals (no two electrons would be paired together.)
Why do electrons fill individually in sub-orbitals before being paired up?
- Because if two electrons are in the same sub-orbital they will repel each other even more (requires even more energy to put the electrons in the same sub-orbital.)
What does the opposite direction of spin of electrons in each sub-orbital reduce?
- The opposite direction of each of electrons in each sub-orbital reduces the mutal repulsion between the paired electrons.
What is the short-hand way of writing the electron configuration of Titanium (22 electrons?) How do you do the short-hand electron configuration?
- (Ar) 4s²3d²
- Locate noble gas above the element.
- Go horizontally across until you reach your element (as you enter s block fill the s orbital and move onto the d block - fill the d orbital until you reach titanium: in this example.)
Short-hand configuration of chromium.
(Ar) 4s¹ 3d⁵
Where are electrons removed from when we ionise transition metals?
- Electrons are lost from the 4s orbital FIRST and then from the 3d, 3p, 3s etc (going down.)
What is the short- hand electronic structure of Chromium? What does spin diagram look like?
(Ar)4s¹3d⁵
All filled up to 3p. 4s only partially filled, one extra in 3d.
the s orbital is partially-filled even in the short-hand configuration
KLP
Short-hand notation of V³⁺
(Ar) 3d²
NORMAL SHORT- HAND STRUCTURE? - (Ar)4s² 3d³.
- Take away 3 electrons - take two from 4s FIRST and then from the 3d!!
KLP
If you want to write the electron configuration of a transition ion, what should you do?
3 STEPS!!
1.) Write electron configuration of the atom.
2.) Then, take out electrons from the 4s first AND then the 3d.
3. ) There, you will have the full electron configuration of the ion.
In general, how do we fill electrons in spin diagrams? Why do we do this?
- Put each electron in separate sub-orbital before starting to pair them up.
- This requires less energy to do than if you started pairing electrons up to start off with (repulison force.)
Past Paper Q
Which block contains the element Samarium (Sm?)
- f block
What are: 2p, 2s, 3s, 4s…. etc. known as?
- Sub-orbitals.
