(a)
Interpretation:
Which element is a metal should be determined.
Concept introduction:
Most of the elements found in the periodic table are metals. All elements in group 1 and 2 are metals except hydrogen. All elements in d block are metals. They are called
(b)
Interpretation:
Which element has the greater ionization energy should be determined.
Concept introduction:
Ionization energy is amount of energy must be absorbed by a gaseous atom in ground state to remove an electron. Further away the electron from the nucleus; it’s easy to remove the electron from the atom/ion. Hence, ionization energy will be less.
(c)
Interpretation:
Which element has the larger atomic radius should be determined.
Concept introduction:
Atomic radius is the distance between the nucleus and the valence electron shell of the atom.
(d)
Interpretation:
Which element has the greater
Concept introduction:
Electron affinity is the change in energy when an electron is added to an atom to form a negative ion.
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General Chemistry: Principles and Modern Applications (11th Edition)
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- Match each element on the right with a set of characteristics on the left. a A reactive, pale yellow gas; the atom has a large electron affinity b A soft metal that reacts with water to produce hydrogen c A metal that forms an oxide of formula R2O3 d A colorless gas; the atom has a moderately large negative electron affinity Oxygen (O2) Gallium (Ga) Barium (Ba) Fluorine (F2)arrow_forwardName the element corresponding to each characteristic below. (a) the element with the electron configuration 1s22s22p63s23p3 (b) the alkaline earth element with the smallest atomic radius (c) the element with the largest ionization energy in Croup 5A (d) the element whose 2+ ion has the configuration [Kr]4d5 (e) the element with the most negative electron attachment enthalpy in Croup 7A (f) the element whose electron configuration is [Ar]3d104s2arrow_forwardWhich main group atom would be expected to have the lowest second ionization energy?arrow_forward
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