(a)
Interpretation:
The elements with least first ionization energy in periodic table has to be circled.
Concept introduction:
Ionization energy:
In a gaseous state isolated neutral atom, the amount of energy required to eject an electron from outermost shell is known as ionization energy. Ionization energy increases from left to right across periods due to increase of effective nuclear charge. Ionization energy decreases down the group due to addition of electrons enters into new orbital which is far from nucleus.
(b)
Interpretation:
The elements with greatest atomic radii in periodic table has to be circled.
Concept introduction:
Atomic radii:
The distance between center of nucleus and outer most orbital in an atom is called as atomic radii. Addition of electrons leads to accumulation of electrons in new orbital which increases atomic radii. Down the group atomic radii increases.
(c)
Interpretation:
The elements with most negative value of
Concept introduction:
Electron affinity:
In a gaseous state isolated neutral atom, energy released when an electron is introduced in outermost shell is known as electron affinity. Greater the negative value of electron affinity, the atom has more tendency to accept an electron.
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General Chemistry: Atoms First
- Without looking at the figures for the periodic properties, compare the three elements B, AI and C. (a) Place the three elements in order of increasing atomic radius. (b) Rank the elements in order of increasing ionization energy. (c) Which element, B or C, is expected to have the more negative electron attachment enthalpy value?arrow_forwardIdentify the atom or ion corresponding to each of the following descriptions: (a) an atom with ground-state electron configuration [Kr]4d105s25p1 (b) an ion with charge 22 and ground-state electron configuration [Ne]3s23p6 (c) an ion with charge +4 and ground-state electron configuration [Ar]3d3arrow_forwardWhich is higher, the third ionization energy of lithium orthe energy required to eject a 1s electron from a Li atomin a PES experiment? Explain.arrow_forward
- Comparison statement about the Lithium and Helium that interactedin terms of why they require different amounts of ionization energy.arrow_forward(2) The element with an electron configuration of 1s22s22p63s2 is in group ______and period ____.arrow_forwardThe first ionization enthalpy for Li is 520 kJ mol^-1. This value corresponds to complete removal of the electron from the nucleus and is achieved when n = infinity. From this value, calculate the effective charge felt by the 2s electron of Li. Why is this less than the actual charge of +3?arrow_forward
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