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Define Atomic Radius: Trends Among Groups And Periods Of The Periodic Table

Referencing Styles : APA | Pages : 1

Define atomic radius

The distance between the centrum of the specific nucleus and the outer shell, which contains electrons of the nucleus is atomic radius. It is the distance between the centrum of the nucleus and the point up. The electron cloud’s density is high in the point up of the nucleus. There are three types of atomic radius are as follows:

  • Van der Waals
  • Radius
  • Covalent Radius
  • Metallic Radius

Van der Waals Radius: The radius of Van der Waals is equivalent to half distance within the two non-bonded identical atoms when the forces of electrostatic are balance between them. It is the closest distance within the two atoms. These atoms are not bonded in same molecule. For reporting about this value, the unit is used is Picometers (pm). The Van der Waals radius magnitude depends on the atoms packing when the element of the nucleus is in solid state.

Covalent Radius: The half distance of the internuclear of covalent radius is within two single bonded homo atoms. The size that measure the size of an atom that is denoted as r (cov), which creates part of a covalent bond. Covalent radius is measured either in angstroms or in Picometers. The covalent radius is equivalent to covalent bond length within two atoms, r (A) + r(B) = R(AB).

Metallic Radius: A crystal or a lattice of metal contains of metal ions or positive kernels, which are arranged in a specific pattern in mobile valance electrons. Every kernel is attracted by some mobile electrons simultaneously and every mobile electron is attracted by some ion metals. It is defined as half distance within the nucleus of two atoms. Metallic radius minimizes the period due to maximize the nuclear charge. It maximizes down the group due to minimizing the quantum number.

The trends among groups and periods of the periodic table

Periodic trends among the groups and the periods are earmarked pattern, which are present in the periodic table to elaborate the various aspects of a specific element. It includes electronic properties and its size. The prime periodic trends are electron affinity, electronegativity, atomic radius, ionization energy, metallic character and melting point. Periodic trends of groups and periods arise from the periodic table arrangements. It provides individual tools to predict the properties of the element quickly. These trends are existing as the same atomic structure is familiar with the period of the element between the groups.

Electronegativity can be defined as chemical property by describing an ability of atom to attract the electrons. Electronegativity is qualitative agent. There is not any standard method to calculate the electronegativity. The energy of ionizing energy is needed to remove the electron in the gaseous phase from the neutral atom. Electron affinity is quantitative measure of the changing energy. In a neutral gas atom, an electron is added. To break the bond the melting point is needed with its energy and it changes the substance from solid phase to liquid phase. The periodic trends in periodic table allow assuming the specific pattern in electron configuration.

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