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,
Give the electron configuration of an element with 20 electrons.
20 Calcium
Ca
2 [Ar] 4s2 s-block, Gp2 Alkaline Earth Metal,
Give the electron configuration of an element with 21 electrons.
21 Scandium
Sc
3 [Ar] 3d1 4s2 3d block, not true Transition Metal
Give the electron configuration of an element with 22 electrons.
22 Titanium
Ti
4 [Ar] 3d2 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 23 electrons.
23 Vanadium
V 5 [Ar] 3d3 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 24 electrons.
24 Chromium Cr
6 [Ar] 3d5 4s1 3d block, a true Transition Metal
Give the electron configuration of an element with 25 electrons.
25 Manganese Mn
7 [Ar] 3d5 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 26 electrons.
26 Iron
Fe
8 [Ar] 3d6 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 27 electrons.
27 Cobalt
Co 9 [Ar] 3d7 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 28 electrons.
28 Nickel
Ni 10 [Ar] 3d8 4s2 3d block, a true Transition Metal
Give the electron configuration of an element with 29 electrons.
29 Copper
Cu 11 [Ar] 3d10 4s1 3d block, a true Transition Metal
Give the electron configuration of an element with 30 electrons.
30 Zinc
Zn 12 [Ar] 3d10 4s2 3d block, not true Transition Metal
Give the electron configuration of an element with 31 electrons.
31 Gallium
Ga 13 [Ar] 3d10 4s2 4p1 p-block, Gp3/13,
Give the electron configuration of an element with 32 electrons.
32 Germanium
Ge 14 [Ar] 3d10 4s2 4p2 p-block, Gp4/14,
Give the electron configuration of an element with 33 electrons.
33 Arsenic
As 15 [Ar] 3d10 4s2 4p3 p-block, Gp5/15,
Give the electron configuration of an element with 34 electrons.
34 Selenium
Se 16 [Ar] 3d10 4s2 4p4 p-block, Gp6/16,
Give the electron configuration of an element with 35 electrons.
35 Bromine
Br 17 [Ar] 3d10 4s2 4p5 p-block, Gp7/17 Halogen,
Give the electron configuration of an element with 36 electrons.
36 Krypton Kr 18 [Ar] 3d10 4s2 4p6 p-block, Gp 0/18 Noble Gas,
What are the exceptions to the rules of filling orbitals? Name their electronic configurations.
There are two:
- Chromium: [Ar] 3d5 4s1;
- Copper: [Ar] 3d10 4s1;
Define disproponation.
A type of redox reaction in which reduction and oxidisation both occur.
Define deliquescent.
A salt which gains more water of crystallisation from the atmosphere with time.
Where would an element with the electron configuration …6p be?
- In the block (this is located in the right most block of non metal elements);
- In period 6;
Where would an element with the electron configuration …1s be?
- In the p block (this is located in the first period and in G1 - left most group);
- In period 1;
- He or H;
Where would an element with the electron configuration …2s be?
- In the s block (this is located in the first period and in G1 - the left most group);
- In period 2;
- Li;
Where would an element with the electron configuration …3s be?
- In the s block (this is located in the first period - and in G1 - the left most group);
- In period 3;
- Na;
Where would an element with the electron configuration …4s be?
- In the s block (this is located in the first period and in G1 - the left most group);
- In period 4;
- K;
Where would an element with the electron configuration …5s be?
- In the s block (this is located in the first period and in G1 - the left most group);
- In period 5;
- Rb;
Where would an element with the electron configuration …6s be?
- In the s block (this is located in the first period and in G1 - the left most group);
- In period 6;
- Cs;
Where would an element with the electron configuration …7s be?
- In the s block (this is located in the first period and in G1 - the left most group);
- In period 7;
- Fr;
Where would an element with the electron configuration …3d be?
- In the d block (this is located in the transition metals);
- In period 4;
Where would an element with the electron configuration …4d be?
- In the d block (this is located in the transition metals);
- In period 5;
Where would an element with the electron configuration …5d be?
- In the d block (this is located in the transition metals);
- In period 6;
Where would an element with the electron configuration …4f be?
- In the f block (this is located in the lanthanides);
- In the first of the two rows of the f block;
Where would an element with the electron configuration …5f be?
- In the f block (this is located in the lanthanides);
- In the second of the two rows in the f block;
Where would an element with the electron configuration …2p be?
- In the p block (this is located in the right most block of non metal elements);
- In period 2;
Where would an element with the electron configuration …3p be?
- In the p block (this is located in the right most block of non metal elements);
- In period 3;
Where would an element with the electron configuration …4p be?
- In the p block (this is located in the right most block of non metal elements);
- In period 4;
Where would an element with the electron configuration …5p be?
- In the p block (this is located in the right most block of non metal elements);
- In period 5;
Where is the s block?
- In the whole of period 1 and in G1 (the left most group of elements).
- Starting at 1s and ending at 7s;
Where is the p block?
- In the right most block of non metal elements on the periodic table.
- Starting at 2p and ending at 6p;
Where is the d block?
- In the transition metals.
- Starting at 3d and ending at 5d;
Where is the f block?
- In the lanthanides.
- Starting at 4f and ending at 5f;
