In the Lewis structure for ICl2–, how many lone pairs of electrons are around the central iodine atom.
1 answer:
Answer : The number of lone pairs of electrons around the central iodine atom are, 6 electrons
Explanation :
Lewis-dot structure : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.
In the Lewis-dot structure the valance electrons are shown by 'dot'.
The representation of valence electrons of an atom by dots around the symbol of an element is said to be the Lewis-dot symbol.
In the representation of Lewis-symbol, one electron dot must put on each side of the element symbol then paired the electrons.
The given molecule is,
As we know that iodine ans chlorine has '7' valence electrons.
Therefore, the total number of valence electrons in = 7 + 2(7) + 1 = 22
According to Lewis-dot structure, there are 4 number of bonding electrons and 18 number of non-bonding electrons.
Hence, the number of lone pairs of electrons around the central iodine atom are, 6 electrons
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Answer:
b) +2 and +3.
Explanation:
Hello,
In this case, given the molecular formulas:
And:
We can relate the subscripts with the oxidation states by knowing that they are crossed when the compound is formed, for that reason, we notice that oxygen oxidation state should be -2 for both cases and the oxidation state of X in the first formula must be +2 since both X and O has one as their subscript as they were simplified:
Moreover, for the second case the oxidation state of X should be +3 in order to obtain 3 as the subscript of oxygen:
Thus, answer is b)+2 and +3
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