Which of the following explains the reason why atomic radii decrease across a period?

As you move across the period, the number of protons increases, which increases the nuclear charge. The number of electrons remains the same creating a larger Coulombic attraction and decreasing the radii.

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As you move across the period, the number of protons and electrons increases. The increased Coulombic attraction decreases the overall size of the atom.

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As you move across the period, the number of protons remains constant while the number of electrons increases. The decreased Coulombic attraction decreases the overall size of the atom.

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The atomic radii do not decrease across a period. It actually increases, duh!

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Solution

The correct option is B As you move across the period, the number of protons and electrons increases. The increased Coulombic attraction decreases the overall size of the atom.
Atomic radius decreases from left to right within a period. This is caused by the increase in the number of protons and electrons across a period. One proton has a greater effect than one electron; thus, electrons are pulled towards the nucleus, resulting in a smaller radius
As you move across the period, the number of protons and electrons increases. The increased Coulombic attraction decreases the overall size of the atom.
Option B is correct

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Similar questions

Q. Assertion :Atomic size decreases across period but increases down a group of the periodic table. Reason: Moving from left to right across a period, electrons are added one at a time to the outer energy shell. Electrons within a shell cannot shield each other from the attraction to protons, while moving down a group in the periodic table, the number of electrons and filled electron shells increases.

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