Question

To which element does each of the following electron configurations correspond? \(\begin{array}{ll}{\text { a. } 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2}} & {\text { c. } 1 s^{2} 2 s^{2} 2 p^{6}} \\ {\text { b. } 1 s^{2} 2 s^{2}} & {\text { d. } 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{6}}\end{array}\)

Short answer

The elements corresponding to the given electron configurations are: a. Silicon (Si) - \(1s^2 2s^2 2p^6 3s^2 3p^2\) b. Beryllium (Be) - \(1s^2 2s^2\) c. Neon (Ne) - \(1s^2 2s^2 2p^6\) d. Argon (Ar) - \(1s^2 2s^2 2p^6 3s^2 3p^6\)

Step-by-step solution

Adding up the electrons in the configuration

Calculate the total number of electrons for each configuration, as this will help in determining the corresponding element. a. \(1s^2 2s^2 2p^6 3s^2 3p^2\) Total electrons: 2 + 2 + 6 + 2 + 2 = 14 b. \(1s^2 2s^2\) Total electrons: 2 + 2 = 4 c. \(1s^2 2s^2 2p^6\) Total electrons: 2 + 2 + 6 = 10 d. \(1s^2 2s^2 2p^6 3s^2 3p^6\) Total electrons: 2 + 2 + 6 + 2 + 6 = 18

Match the electron configurations with the elements

Now that we know the total number of electrons, we can use the periodic table to find the corresponding element with the same atomic number as the total electrons. a. 14 electrons The element with an atomic number of 14 is silicon (Si). b. 4 electrons The element with an atomic number of 4 is beryllium (Be). c. 10 electrons The element with an atomic number of 10 is neon (Ne). d. 18 electrons The element with an atomic number of 18 is argon (Ar).

Summarize the results

Based on the electron configurations given, we can conclude the following elements: a. Silicon (Si) - \(1s^2 2s^2 2p^6 3s^2 3p^2\) b. Beryllium (Be) - \(1s^2 2s^2\) c. Neon (Ne) - \(1s^2 2s^2 2p^6\) d. Argon (Ar) - \(1s^2 2s^2 2p^6 3s^2 3p^6\)

Key concepts

Periodic Table

The periodic table is a tabular arrangement of chemical elements, organized on the basis of their atomic numbers, electron configurations, and recurring chemical properties. Elements are presented in order of increasing atomic number, which is the number of protons in an atom's nucleus. The structure of the periodic table highlights periodic trends, such as elements with similar behavior in the same column.

For example, the noble gases, which are very non-reactive, reside in the far right column. Understanding the layout of the periodic table is crucial to learning about elements' properties and their relations. The periodic table provides a useful framework for analyzing chemical behavior and is widely used in chemistry, physics, and other sciences.

When it comes to electron configurations, the periodic table can be used like a map to determine the energy levels and orbitals that are filled with electrons for a given element. The periodic table is divided into blocks corresponding to the characteristic subshell (such as s, p, d, f) being filled with electrons. This makes it easier to see at a glance how electrons are organized in an atom.

Atomic Number

The atomic number of an element is a fundamental attribute defined as the number of protons found in the nucleus of an atom. It is denoted by the symbol Z and effectively determines the identity of an element. The atomic number is also equal to the number of electrons in a neutral atom, which is why it plays a key role in determining the electron configuration of an element.

For instance, hydrogen, the simplest element, has an atomic number of 1, meaning it has one proton and one electron. The atomic number increases by one in each subsequent element, defining the sequence of elements in the periodic table. During the analysis of electron configurations, knowing an element's atomic number allows us to understand the sequential filling of electron orbitals, and how this relates to the element's position on the periodic table.

Chemical Elements

Chemical elements are the simplest forms of matter that cannot be broken down into simpler substances by ordinary chemical means. Each chemical element is characterized by the number of protons it contains, known as its atomic number, and it has unique properties and a specific electron configuration. Elements can vary greatly in their physical and chemical properties, and these differences are reflected in their place on the periodic table.

The electron configuration of a chemical element details how electrons are distributed in atomic orbitals and energy levels. For example, helium's electron configuration is simply written as \(1s^2\), indicating that its two electrons fill the first energy level's s orbital. As elements become more complex, understanding their electron configurations requires knowledge of the rules governing the order in which atomic orbitals are filled, known as the Aufbau principle, as well as Hund's rule and the Pauli exclusion principle. These concepts are essential for students learning about chemical elements and their behaviors.