Why does the ionization energy of group 16 elements decrease?
Why does the ionization energy of group 16 elements decrease?
Therefore, more amount of energy is required to remove an electron compared to that of the partially filled orbitals (ns2 np4) of group 16 elements of the corresponding period. Hence, elements of group 16 have lower ionization enthalpy values compared to those of group 15 elements.
Which has the highest ionization energy in group 16?
oxygen
Hence, oxygen has maximum ionisation enthalpy in 16th group.
Which has higher ionization energy group 15 or 16?
Group 16 elements have a lower value of first ionization enthalpy as compared to group 15 elements.
Which has more electron gain enthalpy in group 16?
UPLOAD PHOTO AND GET THE ANSWER NOW! Solution : (i) Electron gain enthalpy : Group-16 elements have high electron gain enthalpy. Oxygen has less negative electron gain enthalpy because of the compact nature (Small size) of oxygen atom.
Why does ionization energy increase down the group?
Ionization energy depends mainly on the strength of the attraction between the negative electron and the positive nucleus. When we move down a group in the periodic table, more energy levels are added, and so valence electrons would become further and further away from the positive nucleus.
Why does ionization energy increase across a period and decrease down a group?
On the periodic table, first ionization energy generally decreases as you move down a group. This is because the outermost electron is, on average, farther from the nucleus, meaning it is held less tightly and requires less energy to remove.
Which group has the highest ionization energy?
the noble gases
The elements that belong to the noble gases or inert gases or (Group VIII-A) have the highest ionisation energy.
Why is the first ionization energy of group 16 lower than Group 15?
Group 16 elements have a lower value of first ionization enthalpy as compared to group 15 elements. As group 15 elements have half filled p-orbital due to which group 15 have got extra stability.
Why is ionization enthalpy of Group 15 is more than group 16?
Answer: Since group 15 has symmetrical distribution of electrons due to half filled p orbitals therefore the atom of group 15 becomes more stable compared to group 16 elements. Thus , first ionisation enthalpy of group 15 will be higher than group 16 elements.
What is the order of electron affinity in group 16?
Therefore, combining the effect of size and electron gain enthalpy the electron affinity of Sulphur is a bit higher than selenium and that of oxygen is least in the group. Hence, The correct order of electron affinity is $ O < Se < S $ .
Why does electron gain enthalpy decreases down the group?
This is because, as we go down the group both the atomic size and nuclear charge increases, but the effect of atomic size is more prominent than that of nuclear charge. Hence, the force of attraction between the nucleus and the added electron decreases and thus enthalpy becomes less negative.
