Chapter 4: Problem 22

How do the electron configurations of the transition metals differ from those of the metals in Groups 1 and 2\(?\)

Short Answer

Expert verified

The transition metals, unlike metals in Groups 1 and 2, have their outermost electrons in a 'd' orbital. Additionally, the 'd' orbital in transition metals can be filled before fully filling the 's' orbital of the next energy level. Group 1 and 2 metals, on the other hand, simply add an electron to the 's' orbital of each successive energy level.

Step by step solution

Define Electron Configuration

Electron configuration is the distribution of electrons of an atom or molecule in atomic or molecular orbitals. For atoms, it is denoted by numbers, which are the atomic number, and letters, which represent the type of orbital (s, p, d, f), followed by the number of electrons in the orbital.

Understand Group 1 and 2 Metals Configurations

Group 1 and 2 metals, also known as S-block elements, have their outermost electrons in an 's' orbital. Group 1 elements have one electron in their outer energy level, while Group 2 elements have two. For example, the electron configuration of the Group 1 element Lithium (Li) can be written as 1s2 2s1, and for the Group 2 element Beryllium (Be) it is 1s2 2s2.

Understand Transition Metals Configurations

Transition metals are the d-block elements in the periodic table. Unlike group 1 and 2 metals, transition metals have their outermost electrons in a 'd' orbital. The unique feature of transition metals' electron configuration is that the 'd' orbital can be filled before fully filling the 's' orbital of the next energy level. For example, the electron configuration of the transition metal Iron (Fe) can be written as 1s2 2s2 2p6 3s2 3p6 4s2 3d6, showing that the 4s orbital is filled before the 3d orbital.

Compare between Transition Metals and Group 1 & 2 Metals Configurations

The main difference in the electron configurations of transition metals and metals in Groups 1 and 2 is in the filling of the outermost orbitals. In Group 1 and 2 metals, the outermost electrons are in the s orbital, whereas in transition metals, the outermost electrons are generally in the d orbital. Furthermore, the filling order of orbitals in transition metals is not always as per the energy levels. This is not the case for group 1 and 2 metals.

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How do the electron configurations of the transition metals differ from those of the metals in Groups 1 and 2\(?\)

Short Answer

Step by step solution

Define Electron Configuration

Understand Group 1 and 2 Metals Configurations

Understand Transition Metals Configurations

Compare between Transition Metals and Group 1 & 2 Metals Configurations

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