Identify the specific element that corresponds to each of the following electron configurations and indicate the number of unpaired electrons for each: (d) 3Kr45s24d105p4.

Verified step by step guidance

1. Identify the noble gas in the electron configuration and use it as a reference point. In this case, the noble gas is Krypton (Kr).
2. Write out the electron configuration starting from the noble gas. After Kr, the configuration continues with 5s2, 4d10, 5p4.
3. Determine the element by adding the electrons in the configuration beyond Kr to the atomic number of Kr (36). The total number of electrons is 36 (Kr) + 2 (5s) + 10 (4d) + 4 (5p) = 52.
4. Locate element 52 on the periodic table to identify it as Tellurium (Te).
5. Count the number of unpaired electrons in the outermost p orbital (5p4). Since the p orbital can hold up to 6 electrons and 5p4 configuration means 4 electrons are present, there are 2 unpaired electrons in the 5p orbital.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It is represented by a series of numbers and letters that indicate the energy levels and types of orbitals occupied by electrons. Understanding electron configurations is essential for determining an element's identity and its chemical properties.

Periodic Table and Element Identification

The periodic table organizes elements based on their atomic number and electron configurations. Each element corresponds to a unique electron configuration, which helps in identifying the element. By analyzing the given electron configuration, one can determine the element's position in the periodic table and its associated properties.

Unpaired Electrons

Unpaired electrons are those that occupy an orbital alone rather than in pairs. The number of unpaired electrons in an atom is significant as it influences the atom's magnetic properties and its reactivity. Identifying unpaired electrons is crucial for understanding the element's behavior in chemical reactions and bonding.