Problem 11 - Chemistry The Central Science In Si Units

Question

Consider the element silicon, Si. (a) Write its electron configuration. (b) How many valence electrons does a silicon atom have? (c) Which subshells hold the valence electrons?

Step-by-Step Solution

Answer

(a) \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^2\); (b) 4 valence electrons; (c) 3s and 3p subshells.

Step 1: Understanding Silicon's Atomic Number

Silicon is the 14th element on the periodic table, which means its atomic number is 14. This indicates that a neutral silicon atom has 14 electrons. These electrons must be distributed in various energy levels and subshells according to the rules of electron configuration.

Step 2: Writing the Full Electron Configuration

We fill the electrons in the order of increasing energy levels:1. The first two electrons go into the 1s orbital: \(1s^2\).2. The next two electrons fill the 2s orbital: \(2s^2\).3. The next six electrons fill the 2p orbital: \(2p^6\).4. The next two electrons fill the 3s orbital: \(3s^2\).5. The remaining two electrons fill the 3p orbital: \(3p^2\).The full electron configuration for silicon is \(1s^2 \, 2s^2 \, 2p^6 \, 3s^2 \, 3p^2\).

Step 3: Determining the Number of Valence Electrons

The valence electrons are the electrons in the outermost energy level of an atom. For silicon, we look at the electrons in the third energy level (n=3), which are in the 3s and 3p subshells. The configuration shows \(3s^2\) and \(3p^2\), making a total of 4 valence electrons.

Step 4: Identifying Subshells Holding Valence Electrons

The valence electrons of silicon are located in the \(3s\) and \(3p\) subshells. These are the subshells on the outermost level, where the 4 valence electrons reside.

Key Concepts

Valence Electrons

Valence electrons are the electrons found in the outermost shell or energy level of an atom. They play a crucial role in chemical bonding and reactions. These electrons are the ones that an atom uses to interact with other atoms. For example, they can be involved in forming covalent bonds by sharing electrons, or ionic bonds by transferring electrons to or from another atom. To determine the number of valence electrons for an element like silicon, it is important to look at its electron configuration, particularly focusing on the electrons in the highest energy level. In the case of silicon, whose electron configuration ends in the third energy level, or "shell," we see that it has 4 valence electrons. These electrons are those found in the 3s and 3p subshells of silicon.

Energy Levels

Energy levels, or shells, are the layers surrounding the nucleus of an atom where electrons are likely to be found. Each energy level can be thought of as a step further away from the nucleus, with electrons in higher energy levels having more energy than those closer to the nucleus. The energy levels are often labeled by the principal quantum number n, where n=1 is the closest shell to the nucleus. Electrons fill these levels according to the pattern laid out by order of increasing energy, commonly following the diagonal rule to understand which subshells to fill first. For silicon, which has 14 electrons, the filling order is as follows: 1s, 2s, 2p, 3s, and then 3p. The "3" in 3s and 3p refers to the third energy level, the outermost part where the valence electrons reside.

Subshells

Subshells are subdivisions of energy levels and represent the different regions where electrons may be found around the nucleus. Each subshell can hold a specific number of electrons and is designated by a letter: s, p, d, and f. - **s Subshell:** Can hold a maximum of 2 electrons. - **p Subshell:** Can hold a maximum of 6 electrons. - **d Subshell:** Can hold a maximum of 10 electrons. - **f Subshell:** Can hold a maximum of 14 electrons. When we look at silicon, its valence electrons are found in the 3s and 3p subshells. The electron configuration shows 2 electrons in the 3s subshell and 2 electrons in the 3p subshell. This system of subshells helps us visualize not only where electrons go but how they're shared or transferred during chemical interactions.