(a)
Interpretation:
The
Concept introduction:
The ionization energy in periodic table
In periodic table the ionization energy is increases from left to right in a period due to increasing effective nuclear charge and it decreases from top to bottom of a group due to size of the atom is increases and the force of the attraction between centre of the nucleus and outer most electrons is decreases.
(b)
Interpretation:
The electron affinity of given hypothetical elements X and Z have to be comparatively explained.
Concept introduction:
Electron affinity is well-known as the electron gain enthalpy. Electron gain enthalpy is the amount of energy released when an isolated gaseous atom accepts an electron to form a monovalent gaseous anion.
(c)
Interpretation:
The electron affinity of given hypothetical elements X and Z have to be comparatively explained.
Concept introduction:
The ionization energy in periodic table
In periodic table the ionization energy is increases from left to right in a period due to increasing effective nuclear charge and it decreases from top to bottom of a group due to size of the atom is increases and the force of the attraction between centre of the nucleus and outer most electrons is decreases.
Electron affinity:
Electron affinity is well-known as the electron gain enthalpy. Electron gain enthalpy is the amount of energy released when an isolated gaseous atom accepts an electron to form a monovalent gaseous anion.
(d)
Interpretation:
The electron affinity of given hypothetical elements X and Z have to be comparatively explained.
Concept introduction:
The ionization energy in periodic table
In periodic table the ionization energy is increases from left to right in a period due to increasing effective nuclear charge and it decreases from top to bottom of a group due to size of the atom is increases and the force of the attraction between centre of the nucleus and outer most electrons is decreases.
Electron affinity:
Electron affinity is well-known as the electron gain enthalpy. Electron gain enthalpy is the amount of energy released when an isolated gaseous atom accepts an electron to form a monovalent gaseous anion.
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Chapter 8 Solutions
Student Solutions Manual for Ebbing/Gammon's General Chemistry, 11th
- Using your knowledge of the trends in element sizes on going across the periodic table, explain briefly why the density of the elements increases from K through V.arrow_forwardCompare the elements Na, Mg, O, and P. (a) Which has the largest atomic radius? (b) Which has the most negative electron attachment enthalpy? (c) Place the elements in order of increasing ionization energy.arrow_forwardAnswer the questions below about the elements A and B, which haw the electron configurations shown. A = [Kr]5s1 B =[Ar]3d104s24p4 (a) Is element A a metal, nonmetal, or metalloid? (b) Which element has the greater ionization energy? (c) Which element has the less negative electron attachment enthalpy? (d) Which element has the larger atomic radius? (e) What is the formula for a compound formed between A and B?arrow_forward
- Name 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_forwardDoes the information on alkali metals in Table 2-8 of the text confirm the general periodic trends in ionization energy and atomic radius? Explain.arrow_forwardAnswer the following questions about first ionization energies. (a) Generally ionization energies increase on proceeding across a period, but this is not true for magnesium (738 kJ/mol) and aluminium (578 kJ/mol). Explain this observation. (b) Explain why the ionization energy of phosphorus (1012 kJ/mol) is greater than that of sulphur (1000 kJ/mol) when the general trend in ionization energies in a period would predict the opposite.arrow_forward
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