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Ch.6 - Ionic Compounds: Periodic Trends and Bonding Theory
All textbooksMcMurry 8th EditionCh.6 - Ionic Compounds: Periodic Trends and Bonding TheoryProblem 95
Chapter 6, Problem 95

How does electron shielding in multielectron atoms give rise to energy differences among 3s, 3p, and 3d orbitals?

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1. Electron shielding, also known as electron screening, is the phenomenon where the inner electrons of an atom shield the outer electrons from the full positive charge of the nucleus. This reduces the effective nuclear charge experienced by the outer electrons.
2. In a multi-electron atom, the 3s, 3p, and 3d orbitals are in the same energy level (n=3), but they have different shapes and spatial orientations. The 3s orbital is spherical and closest to the nucleus, the 3p orbital is dumbbell-shaped and further away, and the 3d orbital is even further away with a more complex shape.
3. Because of their different spatial orientations, the 3s, 3p, and 3d orbitals experience different amounts of electron shielding. The 3s electrons are more shielded from the nucleus by the inner electrons, while the 3p and 3d electrons are less shielded and therefore experience a higher effective nuclear charge.
4. The difference in effective nuclear charge results in different energy levels for the 3s, 3p, and 3d orbitals. The higher the effective nuclear charge, the lower the energy level. Therefore, the 3s orbital has a lower energy level than the 3p orbital, which in turn has a lower energy level than the 3d orbital.
5. This is why in multi-electron atoms, the 3s, 3p, and 3d orbitals do not have the same energy level as they would in a hydrogen-like atom, and why the energy differences among these orbitals give rise to the complex electron configurations and chemical behavior observed in these atoms.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Electron Shielding

Electron shielding occurs when inner-shell electrons repel outer-shell electrons, reducing the effective nuclear charge felt by the outer electrons. This phenomenon affects the energy levels of orbitals, as electrons in the same shell experience different levels of attraction to the nucleus based on their proximity to inner electrons.
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Orbital Energy Levels

In multielectron atoms, the energy levels of orbitals (such as 3s, 3p, and 3d) are influenced by both the principal quantum number and the angular momentum quantum number. The 3s orbital is lower in energy than the 3p, which in turn is lower than the 3d, due to differences in penetration and shielding effects, leading to distinct energy separations among these orbitals.
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Penetration Effect

The penetration effect refers to how effectively an electron in a given orbital can get close to the nucleus, thereby experiencing a stronger attraction. s orbitals have the highest penetration, followed by p and then d orbitals. This difference in penetration contributes to the varying energy levels of the 3s, 3p, and 3d orbitals, as electrons in s orbitals are less shielded and thus lower in energy.
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Related Practice
Textbook Question

Element X reacts with element Y to give a product containing X3+ ions and Y2-ions. (d) In what groups of the periodic table are elements X and Y likely to be found?

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Textbook Question
Cesium has the smallest ionization energy of all elements (376 kJ/mol), and chlorine has the most negative electron affinity 1-349 kJ/mol2. Will a cesium atom transfer an electron to a chlorine atom to form isolated Cs+1g2 and Cl-1g2 ions? Explain.
Textbook Question
Order the electrons in the following orbitals according to their shielding ability: 4s, 4d, 4f.
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Textbook Question
Many early chemists noted a diagonal relationship among ele-ments in the periodic table, whereby a given element is some-times more similar to the element below and to the right than it is to the element directly below. Lithium is more similar to magnesium than to sodium, for example, and boron is more similar to silicon than to aluminum. Use your knowledge about the periodic trends of such properties as atomic radii and Zeff to explain the existence of diagonal relationships.
Textbook Question
Heating elemental cesium and platinum together for two days at 973 K gives a dark red ionic compound that is 57.67% Cs and 42.33% Pt. (c) What are the charge and electron configuration of the platinum ion?