Group 17 elements form a) -1 b) +1 C) +17 d)-17
The statement provided doesn't correlate with the characteristics of Group 17 elements, which are commonly known as halogens.
Group 17 elements have a valence electron configuration of ns²np⁵, meaning they have 7 valence electrons. Due to the electronegativity and electron affinity of these elements, they tend to gain one electron to achieve a stable, noble gas configuration, resulting in a -1 charge.
Therefore, the correct statement is:
a) -1
Group 17 elements, also known as the halogens, are found in Group 17 of the periodic table. They include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
These elements are highly reactive and tend to gain one electron to achieve a stable electron configuration. This results in a charge of -1 for their ions. So, the answer is:
a) -1
Group 17 elements in the periodic table are known as the halogens. They include fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At).
Now, to determine the oxidation states of these elements, we need to consider their position in the periodic table and the number of valence electrons they have.
The halogens are located in Group 17, also known as Group VIIA or Group 7. Elements in this group have 7 valence electrons.
To determine the oxidation states of these elements, we need to consider the rule that elements tend to gain or lose electrons to achieve a stable electron configuration, often referred to as the octet rule.
Based on this rule, halogens tend to gain one electron to achieve a full outer shell, which results in an oxidation state of -1. This is because by gaining one electron, they achieve a stable electron configuration similar to the noble gas located to their immediate right on the periodic table.
Therefore, the answer to your question is:
a) -1
So, the correct option is a) -1 for the oxidation state of the Group 17 elements.