Hassium (Hs) Position: Group, Period, and Block

To determine the position of an element in the periodic table, specifically its group, period, and block, we need to understand its atomic number and electronic configuration. The element in question is Hassium (Hs), and its atomic number is given as 108.

Determining Electronic Configuration

The electronic configuration helps us locate the element. Hassium (Hs) has an atomic number ($Z$) of 108. We can determine its configuration by building upon the preceding noble gas, which is Radon (Rn), with an atomic number of 86.

The configuration starts as: $[Rn]$

We need to add the remaining electrons ($108 - 86 = 22$ electrons) following the order of filling orbitals for period 7 elements. The general filling order after Radon is $7s$, followed by $5f$ (Actinides), and then $6d$ (Transition Metals).

• The $7s$ orbital fills next: $7s^2$. (2 electrons added, total electrons = $86 + 2 = 88$)
• The $5f$ orbitals fill next: $5f^{14}$. (14 electrons added, total electrons = $88 + 14 = 102$)
• The $6d$ orbitals fill with the remaining electrons: $108 - 102 = 6$ electrons. So, $6d^6$. (6 electrons added, total electrons = $102 + 6 = 108$)

Therefore, the complete electronic configuration for Hassium (Hs) is: $[Rn] 5f^{14} 6d^6 7s^2$.

Identifying Period, Block, and Group

We can now use this electronic configuration to find the element's properties:

Finding the Period

The period number corresponds to the highest principal quantum number ($n$) occupied by electrons. In the configuration $[Rn] 5f^{14} 6d^6 7s^2$, the highest principal quantum number is 7 (from the $7s^2$ subshell). Thus, Hassium (Hs) is in the 7^th period.

Identifying the Block

The block is determined by the type of orbital that receives the last electron. Since the last electrons in Hs enter the $d$ subshell ($6d^6$), Hassium belongs to the d-block. Elements in the d-block are transition metals.

Calculating the Group

For d-block elements, the group number is calculated by summing the number of electrons in the outermost $s$ subshell and the penultimate ($n-1$) $d$ subshell.

Electrons in the outermost $s$ subshell ($7s$) = 2

Electrons in the penultimate $d$ subshell ($6d$) = 6

Group Number = (Electrons in $(n-1)d$ subshell) + (Electrons in $ns$ subshell)

Group Number = $6 + 2 = 8$.

Therefore, Hassium (Hs) is in the 8^th group.

Conclusion

Based on the electronic configuration and the rules for determining position in the periodic table, Hassium (Hs) with atomic number 108 is located in the:

• Group: 8^th group
• Period: 7^th period
• Block: d-block