For each element, indicate the number of valence electrons, core electrons, and unpaired electrons in the ground state: (a) sodium (b) sulfur.

Verified step by step guidance

1. Identify the atomic number of sodium, which is 11, indicating it has 11 electrons.
2. Write the electron configuration for sodium: \(1s^2 2s^2 2p^6 3s^1\).
3. Determine the number of valence electrons: Valence electrons are those in the outermost shell, so sodium has 1 valence electron in the 3s orbital.
4. Calculate the number of core electrons: Core electrons are those not in the outermost shell, so sodium has 10 core electrons (\(1s^2 2s^2 2p^6\)).
5. Identify the number of unpaired electrons: In the ground state, sodium has 1 unpaired electron in the 3s orbital.

Key Concepts

Valence Electrons

Valence electrons are the outermost electrons of an atom and are crucial for determining how an element will react chemically. For sodium (Na), which has an atomic number of 11, there is one valence electron in its outermost shell (3s1). This single valence electron plays a significant role in sodium's reactivity, particularly in forming ionic bonds.

Core Electrons

Core electrons are the electrons that are not involved in chemical bonding and are located in the inner shells of an atom. In sodium, there are 10 core electrons, which are found in the first two energy levels (1s2 and 2s2 2p6). These electrons shield the valence electron from the full effect of the nucleus's positive charge, influencing the atom's overall stability.

Unpaired Electrons

Unpaired electrons are those that occupy an orbital alone rather than in pairs, and they are significant in determining the magnetic properties and reactivity of an atom. In the case of sodium, there is one unpaired electron in the 3s orbital. This unpaired electron is responsible for sodium's tendency to lose an electron and form a positive ion (Na+), which is a key aspect of its chemical behavior.