Shielding Constant in Atomic Structure

Play an AI-generated podcast conversation about this lesson

What is the effect of electrons close to the atom (n-2 or lower) on shielding?

They have a complex interaction with the electron of interest

They completely negate the shielding (correct)

They have no effect on the shielding constant

They increase the shielding constant

What is the Slater Rule used for in calculating the shielding constant?

To calculate the shielding constant for a specific electron (correct)

To calculate the effective nuclear charge of an atom

To determine the electron configuration of an atom

To determine the type of electron in an atom

What is the significance of the electron configuration of an atom in shielding calculations?

It is used to determine the shielding constant for a specific electron

It is used to identify the electron of interest in shielding calculations (correct)

It is used to determine the type of electron of interest

It is used to calculate the effective nuclear charge of an atom

What is the effect of the 2s and 2p electrons on the shielding constant of a 2p electron in a nitrogen atom?

They increase the shielding constant by 0.35 'charges' Signup and view all the answers

Why are the electrons to the right of the 3d electrons in the electron configuration of a bromine atom ignored in shielding calculations?

They are not relevant to the shielding constant of the 3d electron Signup and view all the answers

What is the formula for calculating the effective nuclear charge (Zeff) of an atom?

Zeff = Z - S Signup and view all the answers

What is the purpose of calculating the shielding constant (S) in atomic physics?

To understand the behavior of electrons in an atom Signup and view all the answers

What is the significance of the shielding constant (S) in the calculation of the effective nuclear charge (Zeff) of an atom?

It is subtracted from the total nuclear charge to get the effective nuclear charge Signup and view all the answers

What is the primary reason for the increase in radius of an atom when it gains an electron to become an anion?

The force of attraction on the electrons decreases Signup and view all the answers

According to Linus Pauling's method, what is the significance of Δ Bond Energies being zero?

The atoms X and Y have similar electronegativities Signup and view all the answers

What is the relationship between the charge on the ion and its radius?

As the charge on the ion becomes more positive, the radius decreases Signup and view all the answers

What is the primary factor that determines the number of electrons that can be misplaced or gained to form ions?

The number of protons in the nucleus Signup and view all the answers

What is the trend observed in the size of an atom or ion as the atomic number increases in a given period of the Periodic Table?

The size of the atom or ion increases Signup and view all the answers

What is the result of a polar molecule forming when the electronegativities of X and Y are not similar?

One atom becomes moderately negative Signup and view all the answers

What is the significance of the equations (1) and (4) in the text?

They are used to evaluate the values of r(C+) and r(A-) Signup and view all the answers

What is the primary purpose of Linus Pauling's method of explaining electronegativity?

To compare the affinities of two atoms with respect to each other Signup and view all the answers

What is the term used to describe atoms and ions with the same electron configuration?

Isoelectronic Signup and view all the answers

Which of the following isoelectronic series has the electron configuration [Ne]3s23p6?

P3–, S2–, Cl–, Ar, K+, Ca2+, and Sc3+ Signup and view all the answers

What determines the size of isoelectronic atoms and ions?

The number of protons Signup and view all the answers

What is the main difference between the Mulliken scale and the Pauling scale of electronegativity?

One is based on bond dissociation energies and the other is based on atomic properties Signup and view all the answers

Why does the atomic size of Ge decrease compared to Si?

Due to the poor screening effect of 3d electrons Signup and view all the answers

What is the term used to describe the energy required to remove the most loosely bound electron from a gaseous atom in its ground state?

Ionization energy Signup and view all the answers

What is the significance of the Mulliken definition of electronegativity?

It is more intuitive than the Pauling definition Signup and view all the answers

Why is it easier to remove the most loosely bound electron from larger atoms?

Because the electron is farther from the nucleus Signup and view all the answers

What is the basis of the Allred-Rochow Electronegativity?

Electrostatic force exerted by the effective nuclear charge on the valence electrons Signup and view all the answers

What is the process of removing electrons from atoms or ions?

Endothermic Signup and view all the answers

What is the purpose of Slater's rules?

To determine the effective nuclear charge for the Allred-Rochow Electronegativity Signup and view all the answers

Why do ionization energy values (IE) always have a positive sign?

Because energy is always required Signup and view all the answers

Why is the Mulliken electronegativity considered a better indicator of an atom's ability to draw electrons toward itself in bonding?

Because it is more intuitive than the Pauling definition Signup and view all the answers

What can be said about the correlation between the Mulliken and Pauling electronegativities?

There is a good correlation between the two Signup and view all the answers

What is a limitation of the Allred-Rochow Electronegativity?

It is based on partly empirical rules Signup and view all the answers

What is the main purpose of discussing the different electronegativity scales?

To understand the relationship between electronegativity and the tendency of atoms to form positive or negative ions Signup and view all the answers

How does effective nuclear charge, $Z_{ ext{eff}}$, change as one moves from left to right across a period?

It increases. Signup and view all the answers

What major factor explains why atoms with more electrons can have smaller atomic radii?

Higher effective nuclear charge pulls electrons closer. Signup and view all the answers

Which electrons are most effective at shielding outer electrons from the nucleus?

Core electrons Signup and view all the answers

Why do outermost electrons have higher energies and are easier to remove?

They are farthest from the nucleus and are shielded more. Signup and view all the answers

What happens to the atomic radius as one moves down a group in the periodic table?