Which situation will violate the octet rule?
a. 3 bonds to boron
b. 3 bonds to and a lone pair on oxygen
c. 5 bonds to carbon
d. 3 bonds to carbon
3 bonds to boron
why please and thank you
Actually, I don't like the answers BECAUSE c and d make no sense what-so-ever. What does carbon have to do with the question? As far as that goes, what does oxygen and answer b have to do with the question?
Look up the Lewis structure of BF3 on the internet. B has 3 electrons and it pair with 3 F atoms to make 3 covalent bonds to form BF3. You see there is no lone pair on B so there are only 6 electrons, not eight, around B. So it violates the octet rule.
.B.
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The octet rule states that in a stable molecule, atoms tend to gain, lose, or share electrons in order to achieve a full outer shell of eight electrons.
Let's analyze each of the given situations to determine which one violates the octet rule:
a. 3 bonds to boron: Boron has 3 valence electrons. If it were to form three bonds, it would only have 6 electrons in its outer shell, falling short of the octet. This situation violates the octet rule because it lacks a full outer shell of 8 electrons.
b. 3 bonds to and a lone pair on oxygen: Oxygen has 6 valence electrons. If it forms three bonds and has a lone pair, it would have a total of 8 electrons in its outer shell, satisfying the octet rule. This situation does not violate the octet rule.
c. 5 bonds to carbon: Carbon has 4 valence electrons. If it forms five bonds, it would have a total of 10 electrons in its outer shell, exceeding the octet. This situation violates the octet rule because it exceeds the limit of 8 electrons in the outer shell.
d. 3 bonds to carbon: Carbon has 4 valence electrons. Forming three bonds allows it to have a total of 6 electrons in its outer shell, falling short of the octet. This situation does not violate the octet rule.
Based on the analysis, the situation that violates the octet rule is option c. 5 bonds to carbon.