Which element is located in the family represented by ns²np³?
A) Ti
B) Se
C) AS
D) I
E) Sb
What do you think? And why? I will be happy to critique your thinking.
It's Nitrogen due to the s²p³ would land straight with Nitrogen's family.
To determine which element is located in the family represented by ns²np³, we need to understand the electronic configuration of the elements. In this case, the representation ns²np³ represents elements from the p-block on the periodic table.
The number 'n' represents the principal quantum number, which indicates the energy level of the electron shell. The 's' and 'p' represent the different subshells within the principal quantum level where the electrons can be found.
For ns²np³, 'ns²' states that there are two electrons in the 's' subshell. The 'np³' states that there are three electrons in the 'p' subshell.
Let's analyze each option using this information:
A) Ti: The electron configuration of Titanium is [Ar] 4s² 3d². It does not match the ns²np³ configuration.
B) Se: The electron configuration of Selenium is [Ar] 4s² 3d¹⁰ 4p⁴. While it has five electrons in the 'p' subshell, the 's' subshell has four electrons, so it doesn't match the ns²np³ configuration.
C) As: The electron configuration of Arsenic is [Ar] 4s² 3d¹⁰ 4p³. It has three electrons in the 'p' subshell, which matches the ns²np³ configuration. This appears to be the answer we are looking for.
D) I: The electron configuration of Iodine is [Kr] 5s² 4d¹⁰ 5p⁵. It has five electrons in the 'p' subshell, but the 's' subshell contains two electrons, so it doesn't match the ns²np³ configuration.
E) Sb: The electron configuration of Antimony is [Kr] 5s² 4d¹⁰ 5p³. It has three electrons in the 'p' subshell, which matches the ns²np³ configuration. However, since Arsenic also matches the configuration and appears earlier in the periodic table, it is the preferred answer.
Therefore, the element located in the family represented by ns²np³ is C) As (Arsenic).