For carbon and nitrogen, use the effective nuclear charges given in Figure 4.7 and the atomic radii given in Figure 4.6 to compare the attractive force between the nucleus in each atom and the valence electron that would be removed by the first ionization.
Interpretation: For the two given atoms the force of attraction and the first ionization energy between them should be compared.
Concept Introduction:
Coulombs law: It states that the force of attraction between two point charges is directly proportional to the product of the point charges and inversely proportional the square of the distances between the charges.
First ionization energy:
The ionization energy is the minimum energy required to remove the electron from an isolated atom which is in the gaseous state results to give gaseous ion with one positive charge.
Valence electron: The electron is considered as valence electron if it present in outermost shell of atom which gets involved in the formation of chemical bond.
Effective nuclear charge: It is the overall positive charge experienced by the outermost electrons present in the atom from the nucleus of the atom.
Screening Effect: The core electrons present near the nucleus shields the outermost electrons (valence electrons) from the charge of the nucleus.
To compare: The force of attraction and the first ionization energy for the two given atoms.
Answer to Problem 4.6WE
Answer
The force of attraction in
The force for
Explanation of Solution
Determine the force of attraction for the two given atoms.
The force of attraction for given atoms are determined by substituting the effective nuclear charge and the radii values to the given formula results to give
Analyze the obtained values for the given atoms.
Examining the obtained values shows us that attraction forces are stronger in
Stronger attraction forces in
Conclusion
The force of attraction and first ionization energy for the given atoms are compared using the coulombs law and the size.
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Chapter 4 Solutions
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