Name an element in the fourth period (row) of the periodic table with the following: d. full s and p sublevels

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Identify the fourth period (row) of the periodic table, which includes elements with atomic numbers 19 to 36.

Understand that a full s sublevel means the s orbital in that period is completely filled with 2 electrons.

Recognize that a full p sublevel means the p orbitals in that period are completely filled with 6 electrons.

Combine the full s and p sublevels to determine that the element must have a total of 8 electrons in its outermost shell (2 in s and 6 in p).

Locate the element in the fourth period that has a completely filled s and p sublevel, which corresponds to the noble gas at the end of the 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. Each period corresponds to the filling of electron shells, with the fourth period containing elements that have electrons filling the 4s and 3d subshells. Understanding this structure is essential for identifying elements based on their electron configurations.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For elements in the fourth period, the full s and p sublevels indicate that the 4s and 4p orbitals are completely filled. This concept is crucial for determining the chemical properties and reactivity of elements, as it influences how they bond with other atoms.

Sublevel Filling Order

The order in which atomic orbitals are filled with electrons follows the Aufbau principle, which states that electrons occupy the lowest energy orbitals first. In the fourth period, after filling the 4s sublevel, electrons begin to fill the 3d sublevel. Recognizing this filling order helps in identifying elements with specific electron configurations, such as those with full s and p sublevels.