Question

Indicate the number of unpaired electrons for the following: [noble gas]ns2(n-1)d10np1?

Answer 1

The given electron configuration has one unpaired electron, which is found in the np1 orbital following Hund's rule.

Step-by-step explanation:

The question asks to indicate the number of unpaired electrons in a general electron configuration represented by [noble gas]ns2(n-1)d10np1. First, we should explain the meaning of the electron configuration provided. Electrons fill orbitals in a way that minimizes the energy of the atom. For example, in a noble gas configuration, all electron orbitals are filled, so there are no unpaired electrons. When we move beyond a noble gas, additional electrons are added to the available subshells (s, p, d, f).

In this configuration, the ns2 suggests that the s orbital in the valence shell (denoted by n) is fully occupied with two electrons. The (n-1)d10 indicates that the d subshell in the previous energy level is completely filled with ten electrons. Lastly, np1 tells us that there is one electron in the p subshell of the valence shell. According to Hund's rule, which states that electrons will fill an empty orbital before they pair up, this single electron in the np1 orbital will be unpaired.

Therefore, the number of unpaired electrons in the given electron configuration is one, represented by the single electron in the np1 orbital.

Answer 2

The number of unpaired electrons for the given electron configuration [noble gas]ns²(n-1)d¹⁰np¹ is 1.

Step-by-step explanation:

The electron configuration provided, [noble gas]ns²(n-1)d¹⁰np¹, represents an atom in a specific energy level arrangement. Let's break down the configuration:

1. noble gas: This part represents the electron configuration of a noble gas that precedes the given element. Noble gases have completely filled electron shells, so this part is essentially a placeholder for a fully filled electron configuration.

2. ns²: This signifies that there are two electrons in the s subshell.

3. (n-1)d¹⁰:This indicates that the (n-1)d subshell is completely filled with ten electrons.

4. np¹: Finally, this part represents one electron in the np subshell.

To find the number of unpaired electrons, we look at the last part, which is np¹. In this case, there is only one electron in the np subshell, and since the np subshell has a single orbital, this electron is unpaired.

The presence of unpaired electrons is crucial in understanding the chemical reactivity of an element, as unpaired electrons are more available for forming chemical bonds.

In summary, the electron configuration [noble gas]ns²(n-1)d¹⁰np¹ has one unpaired electron, making it particularly reactive in certain chemical reactions.