Atomic radius increases or decreases along period?

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Raj Kumar

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The atomic radii tend to decrease across a period from left to right. The atomic radius usually increases while going down a group.
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decreases
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Online Chemistry tutor with 15 years of experience

Due to increase in nuclear charge along a period there is a decrease in atomic radius
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Decreases along a period
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Decreases from left to right
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Decreases as the force of attraction by nucleus on the valence electrons increases
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The atomic radii tend to decrease across a period from left to right. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell). However, diagonally, the number of electrons has a larger effect than the sizeable radius. For example, lithium (145 picometer)...
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The atomic radii tend to decrease across a period from left to right. The atomic radius usually increases while going down a group due to the addition of a new energy level (shell). However, diagonally, the number of electrons has a larger effect than the sizeable radius. For example, lithium (145 picometer) has a smaller atomic radius than magnesium (150 picometer). Atomic radius decreases from left to right across a period, and also increases from top to bottom down a group. read less
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B.E.Electronics engineering

Atomic radius decreases in moving from left to right along a period. This is due to an increase in nuclear charge which tends to pull the electrons closer to the nucleus and reduces the size of the atom.
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Mechanical Engineer

In a periodic table, the atomic radius tend to decrease across a period from left to right.
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B.Tech, Spoken English, EEC, MATLAB, CET Coaching Tutor with 20 years of experience

As you move across a period, atomic radius decreases, because, across a period, electrons are added to the same energy level. At the same time, protons are being added to the nucleus. The concentration of more protons in the nucleus creates a "higher effective nuclear charge." In other words, there...
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As you move across a period, atomic radius decreases, because, across a period, electrons are added to the same energy level. At the same time, protons are being added to the nucleus. The concentration of more protons in the nucleus creates a "higher effective nuclear charge." In other words, there is a stronger force of attraction pulling the electrons closer to the nucleus resulting in a smaller atomic radius. read less
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