Use the periodic table to determine each quantity. a. the number of 3s electrons in Mg b. the number of 3d electrons in Cr c. the number of 4d electrons in Y d. the number of 6p electrons in Pb

검증된 단계별 안내

Identify the atomic number of each element from the periodic table: Magnesium (Mg), Chromium (Cr), Yttrium (Y), and Lead (Pb).

Write the electron configuration for each element based on their atomic numbers. Use the Aufbau principle, Hund's rule, and the Pauli exclusion principle to fill the orbitals.

For Magnesium (Mg), focus on the 3s orbital and count the number of electrons in this orbital.

For Chromium (Cr), look at the 3d orbital and count the number of electrons present in this orbital.

For Yttrium (Y) and Lead (Pb), repeat the process by focusing on the 4d orbital for Yttrium and the 6p orbital for Lead, respectively, and count the electrons in each specified orbital.

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주요 개념

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Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. Understanding electron configuration is essential for determining the number of electrons in specific subshells, such as 3s, 3d, 4d, and 6p, as asked in the question.

Periodic Table Structure

The periodic table organizes elements based on their atomic number and electron configurations. Elements are arranged in rows (periods) and columns (groups) that reflect similar chemical properties. By knowing an element's position in the periodic table, one can infer its electron configuration and the number of electrons in specific subshells, which is crucial for answering the question.

Subshells and Orbitals

Subshells are divisions of electron shells that contain orbitals, where electrons are likely to be found. Each subshell (s, p, d, f) can hold a specific number of electrons: s holds 2, p holds 6, d holds 10, and f holds 14. Identifying the number of electrons in subshells like 3s, 3d, 4d, and 6p requires understanding these capacities and the electron configurations of the respective elements.