Question

When writing a complete electron configuration, you write the filled sublevels in order first, and then if there is a partially filled sublevel, you write it last in the sequence. You can identify the last sublevel containing electrons by finding the element in the periodic table, and determining which block and sublevel the element corresponds to.

Identify the last occupied sublevel, which can be completely or partially filled, for each of the following elements.

Answer 1

The last occupied sublevel in electron configuration can be determined by looking at the block and sublevel that the element corresponds to in the periodic table.

Step-by-step explanation:

The electron configuration of an element is determined by the filling order of subshells in the periodic table. To identify the last occupied sublevel for each element, we look at the block and sublevel that the element corresponds to. The last occupied sublevel is the one that is either completely filled or partially filled. For example, the last occupied sublevel for oxygen (O) is the 2p sublevel, while the last occupied sublevel for potassium (K) is the 4s sublevel.

The last occupied sublevel in an electron configuration can be identified by using the periodic table, which is organized based on energy levels and subshells as per the Aufbau principle. It is significant in understanding an element's reactivity and bonding characteristics.

Understanding Last Occupied Sublevels in Electron Configurations

When identifying the last occupied sublevel in an electron configuration, which may be completely or partially filled, one can use the periodic table's arrangement based on the Aufbau principle. The Aufbau principle guides us to fill electrons into subshells beginning with the lowest energy levels first and moving to higher levels as needed. Determining the last occupied sublevel helps to understand the chemical reactivity and properties of an element.

For instance, hydrogen has its last electron in the 1s subshell (1s¹), and helium's last subshell is similarly the 1s, but it is completely filled (1s²). In general, you can determine the last sublevel by locating the element on the periodic table and noting the block in which it falls, such as s-block, p-block, d-block, or f-block. Anomalies like chromium (Cr) and copper (Cu) have adjustments in their configurations due to the stability conferred by half-filled or completely filled subshells.

The periodic table is designed to reflect this systematic filling of subshells, so that the position of an element within the table reveals its valence electrons and thus its reactivity. Elements in a group share the same number of valence electrons due to their similar outer electron configurations, which are critical to chemical bonding and reactions.