The electron configuration of the outermost electrons of the halogen group is:
a)ns2np7
b)ns1
c)ns2np5
d)ns2np6(n-1)d7
e)ns2np6
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To determine the electron configuration of the outermost electrons of the halogen group, we need to refer to the periodic table and locate the halogen elements which include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
The electron configuration is a representation of the way electrons are distributed within an atom's energy levels or electron shells. Each energy level is labeled as n, with n = 1, 2, 3, and so on. The letters s, p, d, f represent sublevels within each energy level.
Looking at the periodic table, the halogens are located in the 2nd-to-last column (Group 17 or Group VIIA) of the periodic table.
The general electron configuration pattern for the outermost electrons in the halogen group is ns2np5.
This means that the outermost energy level (n) is 2, and there are 2 electrons in the s sublevel (s2) and 5 electrons in the p sublevel (np5).
Therefore, the correct answer is c) ns2np5.
The correct answer is c) ns2np5.
The halogen group consists of the elements fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). These elements are located in Group 17 of the periodic table.
To determine the electron configuration of the outermost electrons of the halogen group, we need to look at the elements in the group. The general electron configuration for these elements is ns2np5, where n represents the energy level of the outermost electron.
For example, the electron configuration of chlorine (Cl) would be 1s2 2s2 2p6 3s2 3p5. Here, the outermost electrons are in the 3p sublevel, indicated by the np5 configuration.
Therefore, the correct electron configuration for the outermost electrons of the halogen group is ns2np5.