30 Questions
Which electron configuration is described in the text?
1s^2 2s^2 2p^4
Why is removing an electron from a cation more difficult than from a neutral atom?
Due to the stronger electrostatic attraction to the cation.
What happens to successive ionization energies for one element?
They increase.
Why is the rapid increase in ionization energy observed after the third ionization for Sc and Ga?
Due to the removal of core electrons.
In general, what happens to ionization energies as you move across a period from left to right?
They increase.
Why is removing an electron from a cation with a higher positive charge more difficult?
Due to an increase in electrostatic attraction.
What factor makes removing an electron from Tl easier compared to Al?
Distance from the nucleus
Why does IE3(Al) require more energy than IE1(Al)?
Al2+ exerts a stronger pull on electrons compared to Al.
Which element has the highest value for IE1?
O
What type of ions exert a stronger pull on electrons compared to neutral atoms?
Cations
Which element has the highest value for IE2?
Pb
Which element would have the highest value for IE1?
Br
What factor contributes to the difficulty in removing an electron from a cation compared to a neutral atom?
Greater electrostatic attraction to the cation
Why is removing an electron from Al easier than from Tl?
Tl's electron is in a higher n orbital
What is the trend observed in ionization energies as you move from Al to Tl?
Increasing due to stronger pull on electrons
What makes removing an electron from Al(Al2+) require more energy than from Al?
Cation Al2+ exerts a stronger pull on electrons
Compared to Ba, which element is expected to have the lowest value for IE1?
O
What contributes to the large increase in ionization energies after the third ionization for Sc and Ga?
Removal of core electrons
What makes removing an electron from a cation with a higher positive charge more difficult?
Greater electrostatic attraction
Which element has the lowest value for IE3?
Pb
Which element has the lowest value for IE1: O, Po, Pb, or Ba?
Ba
Which process requires more energy: IE1 for Al or IE3 for Al?
IE3 for Al
Explain why IE1(Tl) < IE1(Al).
Removing the 6p1 electron from Tl is easier than removing the 3p1 electron from Al due to the higher n orbital being farther from the nucleus.
Predict the order of increasing energy for the following processes: IE1 for Ca, IE1 for Sc, IE2 for Ge, IE3 for As.
IE1 for Sc < IE1 for Ca < IE3 for As < IE2 for Ge
Which ionization energy process involves removing a core electron?
IE2 for Na
Why is removing an electron from a cation with a higher positive charge more difficult?
The stronger positive charge of the cation exerts a greater pull on the electron, making it harder to remove.
Compare the ionization energies for K and Ca.
IE1 for K < IE1 for Ca
Explain why IE1(Al) < IE3(Al).
The cation Al^2+ exerts a stronger pull on the electron during the third ionization, requiring more energy.
Which element exhibits a rapid increase in ionization energy after the third ionization?
Sc and Ga
Explain why IE3(Al) requires more energy than IE1(Al).
The cation Al^2+ exerts a stronger pull on the electron during the third ionization compared to the neutral Al atom.
Learn about the impact of removing electrons from the outer valence shell, resulting in a greater effective nuclear charge and the core electrons being drawn closer to the nucleus. Explore the relative sizes of Al and S atoms and how different elements compare in terms of atomic structure.
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