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(a)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(b)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(c)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
(d)
Interpretation:
An element from the given pair that can give up one electron more easily is to be identified by using the trends within the periodic table.
Concept introduction:
The trends within the periodic table describe the change in the properties such as atomic size, ionization energy, metallic character etc. within a group or in a period.
The energy required for the removal of an electron of an atom from its gaseous state is known as ionization energy. Higher the ionization energy, more difficult is to remove an electron from an atom.
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Chapter 3 Solutions
Chemistry for Today: General Organic and Biochemistry
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