3.1.3 Electrons and the Periodic Table Flashcards
What two things does a higher principal quantum number mean?
- The higher the energy level;
2. The further the shell is from the nucleus;
In what order of shells do the orbitals increase?
s < p < d < f;
Name the order that shells are filled in.
1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f
These shells are filled:
- 4s before 3d (as 4s is a lower energy level, because these quantum principal numbers ‘overlap’ at this point);
How should the filling of a shell be written?
1s^22s^2 ect
These powers only go up to 2 for the s shells, 6 for the p shells and 10 for the d shells (where each shell can hold 2 electrons and there are x number of shells - with dumbbell p orbitals, these are the x,y and z orbitals).
How can the last shell of the electron configuration of an element be worked out, and why would this need to be done? Give the example of Oxygen.
- Oxygen is the 4th element in the 2p block; so 2p^4;
- This is important because it allows us to focus on which electrons are in the outer shell - these are the ones that react, this can also be used to check the whole configuration.
Hoe can the electron configuration be shortened? Word of warning?
- It is abbreviated by basing the inner-shell configuration on the noble gas that comes before it on the periodic table:
Li: 1s^22s^1 would become [He]2s^1
Na: ….3s^1 would become [Ne]2s^1 - BE VERY CAREFUL ABOUT CHOOSING THE CORRECT NOBLE GAS, WITHT THE HIGHEST POSSIBLE NUMBER OF ELECTRONS.
What can you tell from the electron configuration of an element?
Which block it comes from on the periodic table;
What is ‘n,’ in the case of orbitals?
The principal quantum number (shell no.).
Give the electron configuration of an element with one electron.
1
Hydrogen H
1 1s1
Give the electron configuration of an element with 2 electrons.
2 Helium
He
18 1s2
Give the electron configuration of an element with 3 electrons.
3 Lithium
Li
1 [He] 2s1 s-block, Group 1 Alkali Metal,
Give the electron configuration of an element with 4 electrons.
4 Beryllium
Be 2 [He] 2s2 s-block, Group 2 Alkaline Earth Metal,
Give the electron configuration of an element with 5 electrons.
5 Borom B
13 [He] 2s2 2p1 p-block, Group 3/13
Give the electron configuration of an element with 6 electrons.
6 Carbon C
14 [He] 2s2 2p2 p-block, Gp4/14,
Give the electron configuration of an element with 7 electrons.
7 Nitrogen
N
15 [He] 2s2 2p3 p-block, Gp5/15,
Give the electron configuration of an element with 8 electrons.
8 Oxygen O
16 [He] 2s2 2p4 p-block, Gp6/16,
Give the electron configuration of an element with 9 electrons.
9 Fluorine F
17 [He] 2s2 2p5 p-block, G p7/17 Halogen,
Give the electron configuration of an element with 10 electrons.
10 Neon Ne
18 [He] 2s2 2p6 p-block, Gp 0/18 Noble Gas,
Give the electron configuration of an element with 11 electrons.
11 Sodium Na
1 [Ne] 3s1 Gp1 Alkali Metal,
Give the electron configuration of an element with 12 electrons.
12 Magnesium
Mg
2 [Ne] 3s2 s-block, Gp2 Alkaline Earth Metal,
Give the electron configuration of an element with 13 electrons.
13 Aluminium
Al
13 [Ne] 3s2 3p1 p-block, Gp3/13,
Give the electron configuration of an element with 14 electrons.
14 Silicon
Si
14 [Ne] 3s2 3p2 p-block, Gp4/14,
Give the electron configuration of an element with 15 electrons.
15 Phosphorus
P
15 [Ne] 3s2 3p3 p-block, Gp5/15,
Give the electron configuration of an element with 16 electrons.
16 Sulphur
S
16 [Ne] 3s2 3p4 p-block, Gp6/16,
Give the electron configuration of an element with 17 electrons.
17 Chlorine
Cl
17 [Ne] 3s2 3p5 p-block, Gp7/17 Halogen,
Give the electron configuration of an element with 18 electrons.
18 Argon
Ar
18 [Ne] 3s2 3p6 p-block, Gp 0/18 Noble Gas,
Give the electron configuration of an element with 19 electrons.
19 Potassium
K
1 [Ar] 4s1 s-block, Gp1 Alkali Metal,
