What is the relationship between the atomic numbers and ionic radii of the elements in the group 7a
1 answer:
Answer:
The ionic radii increase as the atomic numbers increase.
Explanation:
As we go down a Group, we are adding one more electron shell to the ion.
Each successive shell is bigger than the one before it, so the ionic radius should increase with increasing atomic number.
Here is a table of the ionic radii of the X⁻ ions.
<u>Element </u> <u> Z </u> <u> </u><u>r/pm </u>
F 9 133
Cl 17 181
Br 35 196
I 53 220
At 85 227
However, the relation between r and Z is not linear (see graph).
All we can say is the ionic radius increases as the atomic number increases.
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Answer:
See explanation below
Explanation:
You forgot to put the picture to do so. In this case, I manage to find one, and I hope is the one you are looking for. If not, then post it again and I'll gladly help you out again.
According to the picture with the answer, we have a cyclohexane with 4 methyl groups there. Two of them are facing towards the molecule with a darker bond. This means that the alkyl bromide, should have a bromine in one of the bonds, and in order to produce an E2 reaction, this bromine should be facing in the opposite direction of the methyl groups which are facing towards. This is because an E2 reaction occurs with the less steric hindrance in the molecule. If the bromine is in the same direction as the methyl group, it will cause a lot more of work to do a reaction, and therefore, an E2 reaction. I will promote instead a E1 or a sustitution product.
Therefore the alkyl bromide should be like the one in the picture 2.
Answer : The Lewis-dot structure for the following molecules are shown below.
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'.
Now we have to determine the Lewis-dot structure for the following molecules.
(a) The given molecule is,
As we know that iodine and chlorine have '7' valence electrons.
Therefore, the total number of valence electrons in = 7 + 7 = 14
According to Lewis-dot structure, there are 2 number of bonding electrons and 12 number of non-bonding electrons.
(b) The given molecule is,
As we know that phosphorous has '5' valence electrons and hydrogen has '1' valence electrons.
Therefore, the total number of valence electrons in = 5 + 3(1) = 8
According to Lewis-dot structure, there are 6 number of bonding electrons and 2 number of non-bonding electrons.
(c) The given molecule is,
As we know that phosphorous has '5' valence electrons.
Therefore, the total number of valence electrons in = 4(5) = 20
According to Lewis-dot structure, there are 6 number of bonding electrons and 14 number of non-bonding electrons.
(d) The given molecule is,
As we know that sulfur has '6' valence electrons and hydrogen has '1' valence electrons.
Therefore, the total number of valence electrons in = 6 + 2(1) = 8
According to Lewis-dot structure, there are 4 number of bonding electrons and 4 number of non-bonding electrons.
(e) The given molecule is,
As we know that nitrogen has '5' valence electrons and hydrogen has '1' valence electrons.
Therefore, the total number of valence electrons in = 2(5) + 4(1) = 14
According to Lewis-dot structure, there are 10 number of bonding electrons and 4 number of non-bonding electrons.
(f) The given molecule is,
As we know that chlorine has '7' valence electrons, oxygen has '6' valence electrons and hydrogen has '1' valence electrons.
Therefore, the total number of valence electrons in = 1 + 7 + 3(6) = 26
According to Lewis-dot structure, there are 12 number of bonding electrons and 14 number of non-bonding electrons.
(g) The given molecule is,
As we know that bromine has '7' valence electrons, oxygen has '6' valence electrons and carbon has '4' valence electrons.
Therefore, the total number of valence electrons in = 4 + 6 + 2(7) = 24
According to Lewis-dot structure, there are 8 number of bonding electrons and 16 number of non-bonding electrons.
