Its weak attractive force between two atoms so obviously its radius will be larger than the atomic radius. Its like inter atomic & intra atomic.
AsCl3 is more volatile than PCl3 because it has a lower boiling point and weaker intermolecular forces due to the larger atomic size of arsenic compared to phosphorus. The larger atomic size of arsenic results in weaker Van der Waals forces between AsCl3 molecules, making it easier for them to overcome these forces and transition into the gas phase.
Atomic radius (calculated) of astatine: 127 pmCovalent radius (2008 values) of astatine: 150 pmAtomic radius (empirical) of tellurium: 140 pmAtomic radius (calculated) of tellurium: 123 pmCovalent radius (2008 values) of tellurium: 138 pmCovalent radius (empirical) of tellurium: 135 pmvan der Waals radius of tellurium: 206 pmData from WebElements: http://www.webelements.com/tellurium/atom_sizes.html.Atomic radius of astatine: 127 pmCovalent radius of astatine: 150 pm
Bromine and iodine are denser than fluorine and chlorine due to their larger atomic sizes and greater atomic masses. The increase in size and mass of bromine and iodine atoms results in stronger van der Waals forces between the molecules, which leads to higher density.
Van der Waals forces are weak intermolecular/inter atomic forces. Differentiated from covalent bonding, interionic attraction and hydrogen bondsThey are electrostatic forces due todipole dipole interactions (actually permanent multipoles)dipole -induced dipole interactionsinstantaneous dipole interactions (London dispersion forces- these are sometimes separated from Van der Waals)Sometimes intermolecular repulsion is included and these are due to Pauli exclusion principle.
Xenon has a higher boiling point than Neon because Xenon is a heavier noble gas with larger atomic mass and a greater number of electrons, leading to stronger van der Waals forces of attraction between its atoms. These stronger intermolecular forces require more energy to overcome, resulting in a higher boiling point for Xenon.
Helium has the smallest atomic radius among all the elements on the periodic table. This is because helium has a small number of electron shells and a strong nuclear attraction, which results in a compact atomic structure.
I believe that it has something to do with the van der Waals radii of the electron,
First, the value of the atomic radius is not fixed, but depends on the definition you're using. Second, no element has an atomic radius as large as 152 nm. All atomic radii are about 1000 times smaller than that. Finally, assuming that you meant to say 152 pm, lithium has a metallic radus of 152 pm, oxygen has a van der Waals radius of 152 pm, and cobalt has a calculated atomic radius of 152 pm.
The radius of an atom is typically determined by measuring the distances between the nuclei of two bonded atoms in a molecule, often using techniques like X-ray crystallography or electron microscopy. Atomic radii can also be estimated based on the arrangement of electrons around the nucleus, which influences the effective size of the atom due to electron-electron repulsion and the distribution of electron clouds. Additionally, different types of atomic radii exist, such as covalent radius, van der Waals radius, and metallic radius, each defined by the specific interactions between atoms.
Van der Waals radius of Carbon is 170 pm (170*10-12m)
AsCl3 is more volatile than PCl3 because it has a lower boiling point and weaker intermolecular forces due to the larger atomic size of arsenic compared to phosphorus. The larger atomic size of arsenic results in weaker Van der Waals forces between AsCl3 molecules, making it easier for them to overcome these forces and transition into the gas phase.
The strongest Van Der Waals forces is the hydrogen bond. These forms a permanent dipole-dipole attraction, and there bond occur between the hydrogen and end of one molecule of fluorine, oxygen, or nitrogen.
van der waal radius is greater than co valent radius because van der waal radius is the distance between the nucleus of two atoms of different compound whereas covalent radius is distance between nucleus of atoms of same compound.
The other word for atomic radius includes the Van der Waals radius, ionic radius, and covalent radius. The atomic radius refers to half the distance between the nuclei of identical neighboring atoms in the solid form of an element.
Atomic radius (calculated) of astatine: 127 pmCovalent radius (2008 values) of astatine: 150 pmAtomic radius (empirical) of tellurium: 140 pmAtomic radius (calculated) of tellurium: 123 pmCovalent radius (2008 values) of tellurium: 138 pmCovalent radius (empirical) of tellurium: 135 pmvan der Waals radius of tellurium: 206 pmData from WebElements: http://www.webelements.com/tellurium/atom_sizes.html.Atomic radius of astatine: 127 pmCovalent radius of astatine: 150 pm
Bromine and iodine are denser than fluorine and chlorine due to their larger atomic sizes and greater atomic masses. The increase in size and mass of bromine and iodine atoms results in stronger van der Waals forces between the molecules, which leads to higher density.
this is because there are more electrons in the atom leading to greater van der waals forces, also larger atom so larger electron cloud, and again greater van der waals. so key thing is van der waals increases and this means stronger forces and greater melting point this is because there are more electrons in the atom leading to greater van der waals forces, also larger atom so larger electron cloud, and again greater van der waals. so key thing is van der waals increases and this means stronger forces and greater melting point