Using the periodic table as a guide, write the condensed electron configuration and determine the number of unpaired electrons for the ground state of d. Sb

Verified step by step guidance

1. Identify the atomic number of antimony (Sb) from the periodic table, which is 51.
2. Determine the nearest noble gas preceding Sb, which is krypton (Kr) with an atomic number of 36.
3. Write the condensed electron configuration starting from Kr: \([\text{Kr}]\).
4. Continue filling the electron orbitals following the order: 5s, 4d, and 5p, until you reach the total of 51 electrons.
5. Count the number of unpaired electrons in the 5p orbital, as this will determine the number of unpaired electrons in the ground state of Sb.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is typically represented using a notation that indicates the energy levels and sublevels occupied by electrons. For example, the condensed electron configuration uses the nearest noble gas to simplify the representation, making it easier to understand the arrangement of electrons in an atom.

Periodic Table and Element Position

The periodic table organizes elements based on their atomic number and electron configurations. Each element's position indicates its electron shell and subshell filling order, which is crucial for determining its chemical properties. For antimony (Sb), located in group 15 and period 5, understanding its position helps in predicting its electron configuration and the number of unpaired electrons.

Unpaired Electrons

Unpaired electrons are those that occupy an orbital alone, without a partner of opposite spin. The presence of unpaired electrons is significant as it influences an atom's magnetic properties and reactivity. In the case of antimony, identifying the number of unpaired electrons in its ground state configuration is essential for understanding its chemical behavior and bonding characteristics.