Name an element in the fourth period (row) of the periodic table with the following: a. two 3d electrons

Verified step by step guidance

1. Step 1: Understand that the fourth period of the periodic table includes the elements from potassium (K) to krypton (Kr).
2. Step 2: Recall that the 3d subshell starts filling up after the 4s subshell is filled. This happens from the fourth period onwards.
3. Step 3: Identify that the 3d subshell starts filling from the element scandium (Sc). Scandium is the first element in the fourth period to have electrons in the 3d subshell.
4. Step 4: Count the number of elements from scandium to find the element with two 3d electrons. The element immediately after scandium will have two 3d electrons.
5. Step 5: The element with two 3d electrons in the fourth period is titanium (Ti).

Key Concepts

Periodic Table Structure

The periodic table is organized into rows (periods) and columns (groups) based on atomic number and electron configuration. Elements in the same period have the same number of electron shells, while groups share similar chemical properties. The fourth period includes elements with atomic numbers 19 to 36, where the filling of the 3d subshell begins.

Electron Configuration

Electron configuration describes the distribution of electrons in an atom's orbitals. For transition metals, the 3d subshell is filled after the 4s subshell. An element with two 3d electrons will have an electron configuration that reflects this, typically seen in transition metals located in the fourth period, such as titanium (Ti) or chromium (Cr).

Transition Metals

Transition metals are elements found in groups 3 to 12 of the periodic table, characterized by their ability to form variable oxidation states and colored compounds. They typically have partially filled d orbitals, which contribute to their unique properties. In the fourth period, the transition metals include scandium (Sc) through zinc (Zn), with specific configurations that can include two 3d electrons.