Name an element in the third period (row) of the periodic table with the following: d. two 3s electrons and no 3p electrons

검증된 단계별 안내

Identify the electron configuration pattern for elements in the periodic table.

Recognize that the third period corresponds to the principal quantum number n=3.

Understand that the 3s subshell can hold a maximum of 2 electrons, and the 3p subshell can hold a maximum of 6 electrons.

Determine which element in the third period has a full 3s subshell (2 electrons) and an empty 3p subshell (0 electrons).

Conclude that the element with this electron configuration is the first element in the third period.

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주요 개념

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Periodic Table Structure

The periodic table is organized into rows (periods) and columns (groups) based on atomic number and electron configuration. Elements in the same period have the same number of electron shells. The third period includes elements with three electron shells, where the outermost electrons fill the 3s and 3p subshells.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For elements in the third period, the 3s subshell can hold a maximum of two electrons, while the 3p subshell can hold up to six. The question specifies an element with two electrons in the 3s subshell and none in the 3p subshell, indicating a specific electron arrangement.

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining chemical properties and reactivity. In the context of the third period, an element with two 3s electrons and no 3p electrons would have its valence electrons fully occupying the 3s subshell, making it a Group 2 element, specifically magnesium (Mg).