Answer. 57.3K+ Views. Hint: The ability which allows an electron to get close to the nucleus is known as penetration. It is known as the proximity of the electron in the orbital to the nucleus. We consider it for each shell and subshell as the relative density of the electrons near the atom nucleus.

The orbital (n) and subshell (ml) define how close an electron can approach the nucleus. The ability of an electron to get close to the nucleus is penetration. This is because of shielding, or simply the electrons closest to the nucleus decrease the amount of nuclear charge affecting the outer electrons.

Shielding effect : Shielding effect can be defined as a reduction in the effective nuclear charge on the electron cloud, due to a difference in the attraction forces of the electrons on the nucleus. Penetrating effect : Penetration refers to how effectively electrons can get close to the nucleus.

“Penetrating power” is defined as the power (length) of an electron beam transmitted for a substance. In the case of a TEM, electrons that do not pass through the objective aperture are regarded to be absorbed.

Poor shielding means poor screening of nuclear charge. In other words, the nuclear charge is not effectively screened by electrons in question. The shielding effect of different orbitals is as follows:​ s orbital’s > p orbital’s> d orbital’s> f orbital’s.

The effective nuclear charge is the net positive charge experienced by valence electrons. It can be approximated by the equation: Zeff = Z – S, where Z is the atomic number and S is the number of shielding electrons.

Zeff (Mg), Zeff(Mg+), Zeff (Mg2+) = Part B lonization energy for Mg is 738 kJ mol-1, for Mg+ is 1450 kJ mol-1, and for Mg2+ is 7732 kJ mol-1.

Going across a period, Effective Nuclear Charge (Zeff) increases. Ionization energy increases across a period. Going across a period, Effective Nuclear Charge (Zeff) increases. Distance and shielding remain constant.

Effective nuclear charge is really important, because it determines the size and energy of orbitals, which determine most properties of atoms. So it’s useful to be able to predict effective nuclear charge!

Slater’s rules allow you to estimate the effective nuclear charge Zeff from the real number of protons in the nucleus and the effective shielding of electrons in each orbital “shell” (e.g., to compare the effective nuclear charge and shielding 3d and 4s in transition metals).

They all have the same number of valence electrons.

Subtract S from Z Finally subtract the value of S from Z to find the value of effective nuclear charge, Zeff. For example, Us the Lithium atom, then Z =3 (atomic number) and S = 1.7. Now put the variables in the formula to know the value of Zeff (effective nuclear charge).

The effective nuclear charge may be defined as the actual nuclear charge (Z) minus the screening effect caused by the electrons intervening between the nucleus and valence electron. Effective nuclear charge, Z* = Z – σ Where, Z= Atomic number, σ = Shielding or screening constant.

s orbital

The poor shielding effect of d orbital is due to the very worst attraction with the nucleus because of great affection of electrons in s and p orbitals and also due to the interelctronic repulsion . Due to these factors they can not shield the incoming electrons so effectively as the p and s orbitals can.

The s has the highest shielding power followed by the p orbital, d, and then f, d orbital cannot shield the nucleus effectively due to its shape, and therefore the last electrons are very easy to knock out. The elements are always in a state to attain a stable electronic configuration: d0 , d5 , d10.

Explanation: The penetration power of an electron, in a multi-electron atom, is dependent on the values of both the shell and subshell. And for different values of shell (n) and subshell (l), penetrating power of an electron follows this trend: 1s>2s>2p>3s>3p>4s>3d>4p>5s>4d>5p>6s>4f.

They are named s,p,d,f . The s, p, d, and f stand for sharp, principal, diffuse and fundamental, respectively. The letters and words refer to the visual impression left by the fine structure of the spectral lines which occurs due to the first relativistic corrections, especially the spin-orbital interaction.

These subshells are called as s, p, d, or f. The s-subshell can fit 2 electrons, p-subshell can fit a maximum of 6 electrons, d-subshell can fit a maximum of 10 electrons, and f-subshell can fit a maximum of 14 electrons. The first shell has only an s orbital, so its called as 1s.

1s 2s 2p 3s 3p represents the electron orbital energy levels.

The superscript is the number of electrons in the level. The number in front of the energy level indicates relative energy. For example, 1s is lower energy than 2s, which in turn is lower energy than 2p. The number in front of the energy level also indicates its distance from the nucleus.

Element	Atomic number	Electron configuration
silicon	14	1s22s22p63s23p2
phosphorus	15	1s22s22p63s23p3
sulfur	16	1s22s22p63s23p4
chlorine	17	1s22s22p63s23p5

Ge (Germanium) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2. As (Arsenic) 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3.

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p1. Gallium is a chemical element with symbol Ga and atomic number 31. It is in group 13 of the periodic table, and thus has similarities to the other metals of the group, aluminium, indium, and thallium.

Electron Configuration Matching Game

A	B
1s2 2s2	Be
1s2 2s2 2p3	N
1s2 2s2 2p6 3s2 3p6 4s2 3d3	V
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3	As

Electron Configurations

A	B
Phosphorous	1s2 2s2 2p6 3s2 3p3
Hydrogen	1s1
Helium	1s2
Lithium	1s2 2s1

Explanation: The element Barium has electronic configuration; 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2. It is a member of group 2 in the periodic table hence it forms a divalent ion Ba^2+.

[Ar] 4s2 3d10 4p3 is the electron configuration of a(n) atom. Which is the correct ground state electron configuration for silver? At maximum, an f-subshell can hold ____ electrons, d-shell can hold ____ and p-shell can hold ____ electrons. Which 2 elements have the same ground state electron configuration?