Question

The electronic configuration of the most electronegative element is: (a) \(\mathrm{ls}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{5}\) (b) \(\mathrm{Is}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{4}, 3 \mathrm{~s}^{1}\) (c) \(\mathrm{ls}^{2}, 2 \mathrm{~s}^{2}, 2 \mathrm{p}^{6}, 3 \mathrm{~s}^{1}, 3 \mathrm{p}^{5}\) (d) \(1 s^{2}, 2 s^{2}, 2 p^{6}, 3 s^{2}, 3 p^{5}\)

Short answer

Option (a) is the correct electronic configuration: \(1s^2, 2s^2, 2p^5\).

Step-by-step solution

Identify the Most Electronegative Element

The most electronegative element on the periodic table is fluorine. Its high electronegativity means it has a strong tendency to attract electrons.

Determine the Electronic Configuration of Fluorine

Fluorine is the ninth element of the periodic table. Its electronic configuration will be determined by filling electrons into its orbitals following the Aufbau principle.

Write the Electronic Configuration for Fluorine

Based on its atomic number (9), the electronic configuration of fluorine is: \(1s^2, 2s^2, 2p^5\). This matches the pattern of completing orbitals up to the 2p subshell.

Compare Options with Fluorine's Configuration

Examine each option: - (a) matches \(1s^2, 2s^2, 2p^5\), - (b), (c), and (d) do not match as they involve third shell orbitals or incorrect configurations.

Key concepts

Electronegativity

Electronegativity is an essential concept in chemistry. It refers to the ability of an atom to attract electrons towards itself when forming a bond with another atom. In simple terms, it's a measure of how strongly an atom can "pull" electrons. The higher the electronegativity, the more an atom tends to attract electrons. This property is crucial when predicting how atoms interact in molecules.

Electronegativity values are frequently used to determine the type of bond that will form between atoms:

• If the difference in electronegativity between two bonding atoms is significant, usually greater than 1.7, the bond is considered ionic.
• When the electronegativity difference is small, typically less than 0.4, the bond tends to be nonpolar covalent.
• If the difference is moderate, the bond is polar covalent, indicating partial charges on the atoms in the bond.

The most electronegative element is fluorine, with a value of 3.98 on the Pauling scale. This means that in a bonding situation, fluorine has an incredibly strong tendency to attract electrons from other atoms, making it an important player in many chemical reactions.

Fluorine Element

Fluorine is a fascinating element located in Group 17 of the periodic table, known as the halogens. As the ninth element, it has the atomic number 9, and its most stable isotope has a mass number of 19, yielding the symbol F. One of the key features of fluorine is its high reactivity, which is mainly due to its high electronegativity and small atomic size. Due to these attributes, it forms compounds with almost all elements.

Fluorine's electronic configuration is crucial to understanding its chemical behavior:

• The configuration is represented as: \(1s^2, 2s^2, 2p^5\). This indicates that fluorine has a partially filled 2p orbital, which plays a significant role in its high reactivity.
• With seven valence electrons, fluorine atoms need only one more electron to complete their outer shell and achieve a stable noble gas configuration, instigating their eagerness to gain electrons.

You'll find fluorine compounds in a myriad of applications, from the manufacturing of Teflon to its use in toothpaste to prevent dental cavities. The element's unique properties make it indispensable in many chemical processes and industries.

Periodic Table

The periodic table is a crucial tool in chemistry for understanding the properties and relationships of different elements. It is a systematic arrangement of elements in order of increasing atomic number. Here are some key features of the periodic table:

• Periods and Groups: The table is divided into horizontal rows called periods and vertical columns known as groups or families. Elements in the same group often exhibit similar chemical properties.
• Trends: Electronegativity, ionization energy, and atomic size are some important trends observed in the periodic table. Electronegativity tends to increase across a period from left to right and decrease down a group. This pattern helps predict the reactivity and bonding behavior of elements.
• Element Placement: Elements are placed in a way that showcases periodicity — the repeating pattern of chemical properties. This arrangement allows scientists to predict elemental behavior and discover new elements.

The periodic table isn't just a chart; it's a powerful framework through which chemists can understand and predict the behavior of chemical elements. With elements like fluorine at the pinnacle of electronegativity, the table becomes an invaluable resource for both education and research in the field of chemistry.