s, p, d, and f Blocks of the Periodic Table of the Elements Chemistry Tutorial

⚛ Electrons making up an atom are arranged in subshells.⁽¹⁾

⚛ There are four types of subshells.

⚛ Each of the subshells is designated by a letter, either s, p, d or f:

s subshell, p subshell, d subshell, and f subshell

⚛ By considering which type of subshell is being filled with electrons we can see a pattern in the Periodic Table of the Elements:

s subshell: Group 1 , Group 2, hydrogen and helium

d subshell: Groups 3 to 12 (transition metals)

p subshell: Groups 13 to 18

f subshell: lanthanoids and actinoids⁽²⁾

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The Periodic Table below probably looks a little bit different to the one you are used to seeing.
We have separated hydrogen (H) and helium (He) from the other main group elements.

Notice the location of the labels:

s block: first 2 columns on the left hand side of the Periodic Table

d block: 10 columns in the middle of the Periodic Table

p block: last 6 columns on the right hand side of the Periodic Table

f block: bottom 2 rows separated from the rest of the Periodic Table

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There is a distinct pattern to the location of the s, p, d and f blocks, which is directly related to the Groups of the Periodic Table:

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The labels s, p, d and f blocks of the Periodic Table refer to the subshell that is being filled with electrons.

⚛ Group 1 elements occur at the beginning of a new row (Period) of the Periodic Table.
The highest energy level (valence shell) contains only 1 electron in an s subshell.

⚛ Group 2 elements occur directly to the right of Group 1 elements.
The highest energy level (valence shell) contains 2 electrons, both electrons occupy an s subshell.
The s subshell for this energy level (shell) is now full.

⚛ The highest energy level (valence shell) of a Group 13 element already has 2 electrons in an s subshell, so the next electron occupies a p subshell to make 3 valence electrons in total (2 s electrons + 1 p electron).
As you proceed from left to right across the Period from Group 13 to Group 18 elements, electrons are being added to the p subshell.
Group 18 elements have 2 s electrons and 6 p electrons in their highest energy level (shell) which completes the s and p subshell.

⚛ Transition metals are filling their d subshell with electrons, starting with Group 3 elements which have 1 electron in a d subshell.
Group 12 elements have 10 electrons in a d subshell, which corresponds to a completed d subshell.

⚛ Lanthanoids and actinoids are filling their f subshells with electrons.

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In the section of the periodic table shown below, the letters K, L, M and N have replaced the chemical symbols of four of the elements.

Identify the element which belongs to the d block of the periodic table.

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