Question

Give the electron configurations for the following atoms. Use the noble gas notation.

Short answer

\(Electron\ configurations\ for\ the\ given\ atoms:\) 1. Atom: Chlorine (Cl) Atomic number: 17 Noble gas: Argon (Ar) Electron configuration: \([Ar] 3s^2 3p^5\) 2. Atom: Calcium (Ca) Atomic number: 20 Noble gas: Argon (Ar) Electron configuration: \([Ar] 4s^2\) 3. Atom: Bromine (Br) Atomic number: 35 Noble gas: Krypton (Kr) Electron configuration: \([Kr] 4s^2 3d^{10} 4p^5\) Please note that specific atoms must be provided for more accurate answers.

Step-by-step solution

Identify the atom and its atomic number

Determine which atom is given, and find its atomic number (the number of protons and electrons in a neutral atom). For this exercise, we need the specific atoms for which electron configurations are required to proceed.

Identify the noble gas with the least number of electrons close to the given atom

Consult a periodic table and identify the noble gas with the atomic number closest to, but less than, the atomic number of the given atom. Noble gases are elements in group 18 of the periodic table: Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn).

Write the noble gas notation

Write the noble gas in square brackets, followed by the remaining electron configuration up to the given atom's number. Example: If the given atom is Chlorine (Cl), with an atomic number of 17: Step 1: Cl - atomic number: 17 Step 2: The closest noble gas with a lower atomic number is Argon (Ar) with an atomic number of 18. Step 3: Write the electron configuration for Cl using the noble gas notation: \([Ar] 3s^2 3p^5\). Please provide the atoms for which electron configurations are required to complete the solution.

Key concepts

Noble Gas Notation

Understanding electron configurations of atoms is crucial in the study of chemistry, and the noble gas notation is a simplified way to express these configurations. The noble gas notation aims to streamline the process of writing out an atom’s electron configuration by using a preceding noble gas as a reference point.

The noble gases—Helium (He), Neon (Ne), Argon (Ar), Krypton (Kr), Xenon (Xe), and Radon (Rn)—all have their outermost energy levels fully filled with electrons. This trait makes them particularly stable and unreactive. Since noble gases are the endpoints of electron configurations, they serve as the starting point for configurations of subsequent elements.

To write the noble gas notation:

• Identify the closest noble gas with a lower atomic number than the element of interest.
• Place the noble gas symbol in square brackets to represent its complete electron configuration.
• Continue writing out the remaining electron configuration for the element in question, following the periodic table sequence.

This shorthand method significantly reduces the complexity of electron configurations, especially for elements with a large number of electrons.

Periodic Table

The periodic table is an organized chart of all known elements, arranged by increasing atomic number. The atomic number reflects the number of protons in the nucleus of an atom and, by default, the number of electrons in a neutral atom.

The table is structured into rows called periods and columns known as groups or families, which contain elements with similar properties. The position of an element in the table provides valuable information about its chemical behavior, and it is integral to determining electron configurations.

Groups and Periods

Groups are the vertical columns and are often marked from 1 to 18. Elements in the same group have the same number of valence electrons, contributing to their similar chemical characteristics. Periods are the horizontal rows, with elements arranged from metals on the left to nonmetals on the right, becoming progressively non-metallic and ionizing more easily.

Understanding the Block Layout

The table is also divided into blocks: s, p, d, and f blocks, based on the subshell that is being filled with electrons in that section of elements. These blocks help in correlating the electron configuration with the position of an element on the periodic table.

Atomic Number

The atomic number of an element is one of the most fundamental aspects of its atomic structure. It is denoted by the letter 'Z' and refers to the number of protons found in the nucleus of an atom. Since atoms are electrically neutral, the atomic number also determines the number of electrons in a non-ionized atom.

The atomic number is unique to each element and dictates its position on the periodic table. It also underpins the entire concept of electron configurations, as it directly corresponds to the number of electrons an atom must fill into its orbitals.

When writing electron configurations, especially in noble gas notation, the atomic number reveals where to start the configuration. For example, if an element has an atomic number of 17, like chlorine, you start its electron configuration after the noble gas with an atomic number of 18 (Argon), as it is the closest noble gas with fewer electrons.

Significance in Chemical Behavior

The atomic number is not only a unique identifier for an element but also indicates its chemical properties. As elements with sequential atomic numbers generally add one electron and proton at a time, their chemical properties change progressively along the periodic table.