Textbook Question
(c) Detailed calculations indicate that the effective nuclear charge is 5.6+ for the 3s electrons and 4.9+ for the 3p electrons. Why are the values for the 3s and 3p electrons different?
10. Periodic Properties of the Elements
Periodic Trend: Effective Nuclear Charge
Multiple Choice
Which of the following periodic trends is NOT primarily explained by shielding and effective nuclear charge (ENC)?
A
Atomic radius
B
Electronegativity
C
Melting point
D
Ionization energy
Verified step by step guidance1
Understand that shielding and effective nuclear charge (ENC) primarily affect how strongly the nucleus attracts electrons in an atom, influencing properties related to electron cloud size and electron removal or attraction.
Recall that atomic radius, electronegativity, and ionization energy are all properties directly influenced by ENC and shielding because they depend on the attraction between the nucleus and electrons.
Atomic radius decreases across a period because ENC increases, pulling electrons closer; ionization energy increases because more energy is needed to remove an electron due to stronger ENC; electronegativity increases as atoms more strongly attract bonding electrons due to higher ENC.
Melting point, however, depends more on the type of bonding and intermolecular forces between atoms or molecules, such as metallic bonding, covalent networks, or van der Waals forces, rather than on ENC or shielding effects.
Therefore, melting point is the periodic trend that is NOT primarily explained by shielding and effective nuclear charge.
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