Module Figures: Periodic Table III • Visionlearning

Periodic Table III

Figure 2: Kekule’s proposal for the structure of benzene (1872).

Table 1: Table shows the electron capacity of the three electron shells nearest the nucleus.
Electron shell	Electron capacity
1^st electron shell	2
2^nd electron shell	8
3^rd electron shell	18

Figure 3: This Bohr model of a chlorine atom shows the electrons distributed in the first 3 electron shells. The letters s and p represent subshells, which we will discuss later in the module.

Figure 4: This Bohr model shows the electrons distributed in a carbon atom’s electron shells.

Presence of subshells and maximum electron capacity for electron shells
Electron shell	Presence of an s-subshell?	Presence of a p-subshell?	Presence of a d-subshell?	Maximum electron capacity for shell
1^st electron shell	Yes (up to 2 electrons)	No (0 electrons)	No (0 electrons)	2 electrons total (2+0)
2^nd electron shell	Yes (up to 2 electrons)	Yes (up to 6 electrons)	No (0 electrons)	8 electrons total (2+6)
3^rd electron shell	Yes (up to 2 electrons)	Yes (up to 6 electrons)	Yes (up to 10 electrons)	18 electrons total (2+6+10)

Table 3: s-type, p-type, and d-type subshells and their different electron capacities
Subshell types	# of electron orbitals	Maximum electron capacity
s-type	1	2
p-type	3	6
d-type	5	10

Figure 6: The figure identifies the symbolism in the electron configuration notation.

Figure 7: The image depicts a Bohr model of a hydrogen atom, also called a “planetary model”.

Figure 8: The image depicts a Bohr model of a helium atom.

Figure 9: The image depicts a Bohr model of a lithium atom.

Figure 10: The arrow indicates increasing energy levels of the subshells, whichindicates the order in which these subshells will fill with electrons.
Increasing energy level

1s	2s	2p	3s	3p

Figure 12: The image depicts a Bohr model for a sodium atom.