The computed sizes qualitatively correlate with the absolute size dependent properties like ionization potentials and electronegativity of elements. The d-block and f-block contractions are distinct in the calculated sizes. The set of theoretical radii are found to reproduce the periodic law and the Lother Meyer’s atomic volume curve and reproduce the expected vertical and horizontal trend of variation in atomic size in the periodic table. It does not store any personal data.A set of theoretical atomic radii corresponding to the principal maximum in the radial distribution function, 4πr 2R 2 for the outermost orbital has been calculated for the ground state of 103 elements of the periodic table using Slater orbitals. The cookie is set by the GDPR Cookie Consent plugin and is used to store whether or not user has consented to the use of cookies. The cookie is used to store the user consent for the cookies in the category 'Performance'. This cookie is set by GDPR Cookie Consent plugin. The cookie is used to store the user consent for the cookies in the category 'Other. The cookies is used to store the user consent for the cookies in the category 'Necessary'. The cookie is set by GDPR cookie consent to record the user consent for the cookies in the category 'Functional'. The cookie is used to store the user consent for the cookies in the category 'Analytics'. These cookies ensure basic functionalities and security features of the website, anonymously. Necessary cookies are absolutely essential for the website to function properly. Since the force of attraction between nuclei and electrons increases, the size of the atoms decreases. These electrons are gradually pulled closer to the nucleus because of its increased positive charge. Within a period, protons are added to the nucleus as electrons are being added to the same principal energy level. Why does atomic size decrease across a period? Which statement best describes the trend in atomic radii observed in the periodic table? The atomic radii increase, moving across a period to the left and down in a group. Which of the following best explains the trend in atomic radii down a group? The atomic radius increases when we go down a group because of the addition of extra shell. In general, the atomic radius decreases as we move from left to right in a period with an increase in nuclear charge of the element. How does atomic radius vary down the group? This is because atomic number increases down a group, and thus there is an increased distance between the valence electrons and nucleus, or a greater atomic radius. Why does the atomic radius increase as you go from top to bottom of a chemical family?įrom top to bottom down a group, electronegativity decreases.

One proton has a greater effect than one electron thus, electrons are pulled towards the nucleus, resulting in a smaller radius.

This is caused by the increase in the number of protons and electrons across a period. Why does the atomic radius increase as you go from top to bottom? Radii generally decrease along each period (row) of the table from left to right and increase down each group (column). The atomic radius of a chemical element is a measure of the size of its atoms. How does atomic radius vary across a period and a column? Across a period, effective nuclear charge increases as electron shielding remains constant. In general, atomic radius decreases across a period and increases down a group. What is the trend of atomic radius across period and group?Ītomic radius is the distance from the atom’s nucleus to the outer edge of the electron cloud.

7 Why does atomic size decrease across a period?.6 How does atomic radius vary down the group?.5 Why does the atomic radius increase as you go from top to bottom of a chemical family?.4 What is the trend in atomic size across a period *?.3 What trend in atomic radius occurs down a group?.2 How does atomic radius vary across a period and a column?.1 What is the trend of atomic radius across period and group?.

Atomic radius across a period