Question

Which outer electron configurations would you expect to belong to a noble gas? To a metalloid? a. \(n s^{2}\) b. \(n s^{2} n p^{6}\) c. \(n s^{2} n p^{5}\) d. \(n s^{2} n p^{2}\)

Short answer

The outer electron configuration expected to belong to a noble gas is b. \(n s^{2} n p^{6}\). The configurations that could belong to a metalloid are a. \(n s^{2}\), c. \(n s^{2} n p^{5}\), and d. \(n s^{2} n p^{2}\) as they have partially filled p subshells.

Step-by-step solution

Identify Noble Gas Configuration

Noble gases have completely filled outer shells. This is represented by the electron configuration that includes a filled s-subshell and a filled p-subshell in the outermost energy level.

Match Electron Configuration to Noble Gas

The electron configuration that represents a noble gas is the one with filled s and p subshells in the outermost energy level. That is the electron configuration with an s-subshell holding 2 electrons and a p-subshell holding 6 electrons.

Identify Metalloid Configuration

Metalloids have properties intermediate between metals and non-metals. They tend to have partially filled p subshells in their outer energy level, which allows them to share electrons with other elements.

Match Electron Configuration to Metalloid

The electron configuration that represents a typical metalloid is the one with a partially filled p subshell. That is an electron configuration with an s-subshell holding 2 electrons and a p-subshell that is not completely filled with electrons.

Key concepts

Noble Gas Configuration

Noble gases, the elements in group 18 of the periodic table, are known for their chemical inertness. This peculiar property is due to their electron configuration, specifically the outermost shell which is fully occupied. A typical noble gas configuration involves having both the s and p orbitals in the highest energy level completely filled. In terms of notation, this is expressed as the letter 'n' representing the principal quantum number followed by the orbitals and their corresponding electrons.For instance, the notation for a noble gas would be in the form of n s² n p⁶. Here, the 's' orbital can accommodate 2 electrons and the 'p' orbital can accommodate 6, totaling 8 valence electrons. This full valence shell configuration gives noble gases their characteristic stability. The octet rule is a chemical rule of thumb that reflects this stability pattern through which atoms tend to combine in such a way that they each have eight electrons in their valence shells, resembling a noble gas. Therefore, when looking at option 'b', it clearly matches this stable electron arrangement.

Metalloid Electron Configuration

Metalloids are elements that possess a blend of both metallic and non-metallic properties, which often makes their electron configurations unique. Unlike noble gases, metalloids don't have a completely filled valence shell, but rather partially filled p orbitals in their outer energy levels. This allows them the flexibility to either lose, gain, or share electrons when they form chemical bonds, adapting their behavior depending on the situation.The sparse electron population in the p orbitals is typically represented by configurations where 'n' signifies the energy level, 's' is always filled with 2 electrons because it's the lower energy subshell, and 'p' has a few electrons but not the full 6. Therefore, configurations like n s² n p² or n s² n p⁵, where the p orbital doesn't have all of its electron positions occupied, can be seen in metalloids. These configurations correspond to options 'c' and 'd'. Their ability to share electrons is what allows metalloids to form various types of chemical bonds and makes them especially versatile in semiconductor technology where precise control over electron movement is required.

Outer Shell Electron Configuration

The outer shell electron configuration of an element is crucial as it determines the chemical properties and reactivity of the element. It includes the electrons found in the outermost shell, or energy level, of an atom. These electrons, also known as valence electrons, are the ones involved in forming chemical bonds with other atoms. For most atoms, achieving a full outer shell is synonymous with chemical stability, which is often represented by a noble gas configuration.Different elements aim to either lose, gain or share electrons to achieve a full outer shell, mimicking the electron configuration of the closest noble gas. This drive is encapsulated in the octet rule for main-group elements. A typical representation of outer shell electron configuration uses principal quantum number 'n' followed by the orbital labels and the actual count of electrons within them, like n s² or n s² n p^x, where x can be any number from 1 to 6 depending on the element. It is worth noting here that while 'a' symbolizes a noble gas precursor due to it having a full s subshell, the configurations in 'c' and 'd' are indicative of elements which would readily form bonds to complete their octet, showcasing reaction versatility.