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3. Which of the following statements about atomic properties is TRUE? (a) The magnitude of the electron affinity of fluorine is greater than that of carbon. (b) The atomic radius of boron is greater than that of beryllium. (c) The radius of Sit is greater than that of aluminum. (d) The ionic radius of Cr is larger than that of t. (e) Energy is always released when an atom in the gas phase loses an electron.

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Related questions

QUESTION 8

Choose the atom or ion using a periodic table.

Reference: Ref 2-6


Larger first ionization energy, Be or B

1 points

QUESTION 9

Which of the following statements is true?

A.

The ionization energy of S2Ҁ“ is greater than that of ClҀ“.
B.

The atomic radius of Li is larger than that of Cs.
C.

The ionic radius of Fe+ is larger than that of Fe3+.
D.

All are false.
E.

The first ionization potential of H is greater than that of He.

Hydrogen is an unusual element because it behaves in some ways like the alkali metal elements and in other ways like nonmetals. Its properties can be explained in part by its electron configuration and by the values for its ionization energy and electron affinity. (a) Explain why the electron affinity of hydrogen is much closer to the values for the alkali elements than for the halogens. (b) Is the following statement true? β€œHydrogen has the smallest bonding atomic radius of any element that forms chemical compounds.” If not, correct it. If it is, explain in terms of electron configurations. (c) Explain why the ionization energy of hydrogen is closer to the values for the halogens than for the alkali metals. (d) The hydride ion is H–. Write out the process corresponding to the first ionization energy of the hydride ion. (e) How does the process in part (d) compare to the process for the electron affinity of a neutral hydrogen atom?

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