Which of the following contains an atom that does not obey the octet rule? BrF3 SiO2 NaCl BrF

Chemistry

2 answers:

mario62 [17]3 years ago

6 0

Answer:

BrF₃

Explanation:

Octet rule -

Octet rules determines the stability of an atom , depending on the number and arrangement of atoms .

The atoms with eight electrons are considered to be following the octet rule , are are stable .

The atoms with atoms less than or more than 8 are considered to be unstable and violating the octet rule .

from the given options in the question , BrF₃ violates the octet rule , as it has only 6 electrons .

mrs_skeptik [129]3 years ago

5 0

The octet rule signifies towards the capability of the atoms to prefer to exhibit eight electrons in the valence shell. In case, when the atoms possess lesser than eight electrons, they seem to react and produce more stable components. While discussing octet rule, one does not consider d or f electrons.

According to the octet rule, the atoms of the prime-group elements seem to bind in such a manner that each atom exhibit eight electrons in its valence shell, providing it the similar electronic configuration as a noble gas.

In the given question, in BrF3, fluorine follows octet rule, while bromine does not follow the octet rule.

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Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C is red. In the reactions in

igor_vitrenko [27]

Explanation:

Oxidizing agents are defined as the agents which oxidize other substance and itself gets reduced. These agents undergoes reduction reactions.

Reducing agents are defined as the agents which reduces the other substance and itself gets oxidized. These agents undergoes reduction reactions.

When oxidizing agent-A get reduced it changes green to colorless.

$A+e^-\rightarrow A^-$

When oxidizing agent-B get reduced it changes yellow to colorless.

$B+e^-\rightarrow B^-$

When oxidizing agent-C get reduced it changes red to colorless.

$C+e^-\rightarrow C^-$

1) When we added solution C that oxidizing agent-C in solution containing $B^-$ ions changes from red to yellow:

$C+B^-\rightarrow C^-+B(yellow)$

So, in this C is oxidizing $B^-$ ion into B which yellow in color.

C is reduced and $B^-$ ions is oxidized.

Here, $B^-$ are oxidized by C which means that C a better oxidizing agent than B.

2) When a solution of C is mixed with one containing A- ions, the color remains red.

$C+A^-\rightarrow$ no reaction

As we had observed that no color change was seen on adding substance C to the solution with $A^-$ ions which indicates that C was unable to oxidize $A^-$ ions. Hence, not a better oxidizing agent than A