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28 Sep 2019

Ionization energy typically increases as one moves across a row inthe periodic table.
However, the first ionization energy of sulfur (1,000 KJ/mol) issmaller than phosphorus
(1,012 KJ/mol). Why is this an exception?

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 Which of the following statements is true? a. Both ionization energy and electron affinity increase as you move across a row of the periodic table. b. Both metallic character and electron affinity increase as you move across a row of the periodic table. increases and electron affinity decreases as you move across a c. Ionization energy row of the periodic table. character increases and ionization energy decreases as you move across a d. Metallic row of the periodic table.

a. Using the element phosphorus as an example, write the equation for a process in which the energy change will correspond to the ionization energy and to the electron affinity.

b. Explain why the first ionization energy tends to increase as one proceeds from left to right across a period. Why is the first ionization energy of aluminum lower than that of magnesium, and the first ionization energy of sulfur lower than that of phosphorus?

c. Why do the successive ionization energies of an atom always increase? Note the successive ionization energies for silicon given in Table 7.5. Would you expect to see any large jumps between successive ionization energies of silicon as you removed all the electrons, one by one, beyond those shown in the table?

bronzealligator355

Using the element phosphorus as an example, write the equation for a process in which the energy change will correspond to the ionization energy and to the electron affinity.

Explain why the first ionization energy tends to increase as one proceeds from left to right across a period. Why is the first ionization energy of aluminum lower than that of magnesium and the first ionization energy of sulfur lower than that of phosphorus?

Why do the successive ionization energies of an atom always increase? Note the successive ionization energies for silicon given in Table 2-5. Would you expect to see any large jumps between successive ionization energies of silicon as you removed all the electrons, one by one, beyond those shown in the table?

amethystmuskrat759

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Ionization energy typically increases as one moves across a row inthe periodic table.
However, the first ionization energy of sulfur (1,000 KJ/mol) issmaller than phosphorus
(1,012 KJ/mol). Why is this an exception?

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Ionization energy typically increases as one moves across a row inthe periodic table.However, the first ionization energy of sulfur (1,000 KJ/mol) issmaller than phosphorus(1,012 KJ/mol). Why is this an exception?

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Related textbook solutions

Basic Chemistry

Principles of Chemistry Molecular Approach

Chemistry: Structure and Properties

Principles of Chemistry Molecular Approach

Chemistry: A Molecular Approach

Chemistry: A Molecular Approach

Principles of Chemistry: A Molecular Approach

Chemistry: The Central Science

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Ionization energy typically increases as one moves across a row inthe periodic table.
However, the first ionization energy of sulfur (1,000 KJ/mol) issmaller than phosphorus
(1,012 KJ/mol). Why is this an exception?