(b) Hafnium, Hf, is also found in group 4. Write the electron configuration for Hf.

Verified step by step guidance

1. Identify the atomic number of Hafnium (Hf) from the periodic table, which is 72. This number tells you the number of protons and, in a neutral atom, the number of electrons.
2. Start by filling the electron shells in order of increasing energy level. Begin with the 1s orbital, then 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, and finally 6p orbitals, following the order dictated by the Aufbau principle.
3. Remember to follow the Pauli Exclusion Principle, which states that each orbital can hold a maximum of two electrons with opposite spins.
4. Apply Hund's Rule when filling orbitals of the same energy, which states that electrons will fill an empty orbital before they pair up in an already occupied one.
5. Write the electron configuration by listing the filled orbitals in order of increasing energy, and indicate the number of electrons in each orbital. For Hafnium, the electron configuration will end with the 6s orbital being filled followed by electrons beginning to fill the 4f and 5d orbitals.

Key Concepts

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. It follows the Aufbau principle, which states that electrons fill orbitals starting from the lowest energy level to the highest. The configuration is typically written using the notation of subshells (s, p, d, f) and their respective electron counts, providing insight into the atom's chemical properties and reactivity.

Periodic Table Groups

The periodic table is organized into groups (columns) and periods (rows). Elements in the same group share similar chemical properties due to having the same number of valence electrons. Group 4 elements, like hafnium, typically exhibit similar bonding characteristics and oxidation states, which are important for predicting their behavior in chemical reactions.

Transition Metals

Hafnium is classified as a transition metal, which are elements found in groups 3 to 12 of the periodic table. Transition metals are characterized by their ability to form variable oxidation states and complex ions, as well as their use in catalysis and materials science. Understanding their electron configurations is crucial for predicting their chemical behavior and interactions.