Why the radii decreases as you go across a period but increases as you go down a group?

On the periodic table, atomic radius generally decreases as you move from left to right across a period (due to increasing nuclear charge) and increases as you move down a group (due to the increasing number of electron shells).

How does atomic radii decrease from left to right?

The atomic radius of atoms generally decreases from left to right across a period. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. These electrons are gradually pulled closer to the nucleus because of its increased positive charge.

Why are the radii changing as you move across the table from left to right within one row?

The size of an element’s ionic radius follows a predictable trend on the periodic table. As you move down a column or group, the ionic radius increases. This is because each row adds a new electron shell. Ionic radius decreases moving from left to right across a row or period.

Why does the atomic radius decrease as the atomic number increases?

As the atomic number increases along each row of the periodic table, the additional electrons go into the same outermost shell, causing the atomic radius to decrease due to the increasing nuclear charge.

Why atomic radii increase down the group?

In general, atomic radius decreases across a period and increases down a group. Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius.

How do atomic radii vary in a period and in a group explain?

In general, the atomic radius decreases as we move from left to right in a period with an increase in the nuclear charge of the element. The atomic radius increases when we go down a group because of the addition of an extra shell.

How does atomic radii increase on the periodic table?

An atom gets larger as the number of electronic shells increase; therefore the radius of atoms increases as you go down a certain group in the periodic table of elements. In general, the size of an atom will decrease as you move from left to the right of a certain period.

How do atomic radii change with the increase in atomic number in any period explain it with diagram?

Periodic Trends of Atomic Radius

1. An atom gets larger as the number of electronic shells increase; therefore the radius of atoms increases as you go down a certain group in the periodic table of elements.
2. In general, the size of an atom will decrease as you move from left to the right of a certain period.

How do atomic radii vary in a group and period?

Summary. Atomic radius is determined as the distance between the nuclei of two identical atoms bonded together. The atomic radius of atoms generally decreases from left to right across a period. The atomic radius of atoms generally increases from top to bottom within a group.

Why does atomic radii increase down a group?

Down a group, the number of energy levels (n) increases, so there is a greater distance between the nucleus and the outermost orbital. This results in a larger atomic radius. Ionic radius is the distance from the nucleus to the outer edge of the electron cloud of an ion.

Why does atomic radius decrease across a period and increase down?

Likewise, why does atomic radius decrease across a period and increase down a group? Atomic radius decreases across a period because valence electrons are being added to the same energy level at the same time the nucleus is increasing in protons.

How does the number of protons affect the radius of an atom?

On coming down the group, Number of protons increases → nuclear charge increases → atomic size decreases. Number of shells increases → atomic radius increases. The shielding effect increases (since now electrons from previous shells also contribute to the shielding effect) → atomic radius increases.

Why do the atomic radii increase down a vertical row?

Going down a vertical row the atomic radii increase simply because additional electron shells get filled. These shells are more distant from the nucleus than elements in the previous vertical position of a group of similar elements, hence the increased radii.

Why does effective nuclear charge increase down a group?

The effective nuclear charge, Zeff, increases down a group which draws electrons closer towards the nucleus, decreasing atomic radius. In respect to this, why does atomic radius increase in a group? This is caused by the increase in the number of protons and electrons across a period.