Question

Arrange the following elements in order of increasing electronegativity: (a) \(\mathrm{N}\) (b) Ge (c) \(\mathrm{O}\) (d) \(\mathrm{P}\)

Short answer

Ge < P < N < O

Step-by-step solution

Identify Electronegativity Table or Trend

Electronegativity is a measure of an atom's ability to attract and hold onto electrons. Generally, electronegativity increases across a period (left to right) and decreases down a group (top to bottom) in the periodic table. Locate N, Ge, O, and P in the periodic table to assess their relative positions.

Locate Elements on the Periodic Table

Find nitrogen (N), germanium (Ge), oxygen (O), and phosphorus (P) on the periodic table. Nitrogen and oxygen are located in period 2 (right of the table), while germanium is in period 4 and phosphorus is in period 3 (left and below nitrogen and oxygen).

Determine Relative Electronegativity

From the periodic table and known trends: oxygen (O) has the highest electronegativity, then comes nitrogen (N), and farther left and down the table are phosphorus (P) and germanium (Ge), with germanium typically having the lowest electronegativity of these four.

Arrange in Order of Increasing Electronegativity

Based on the trend and specific positions of elements: Gemanium (Ge) < Phosphorus (P) < Nitrogen (N) < Oxygen (O). Thus, Germanium will be least electronegative and Oxygen will be most electronegative.

Key concepts

Periodic Table

The Periodic Table is like a map that organizes all known chemical elements based on their atomic number, electron configurations, and recurring chemical properties. It's a powerful tool in chemistry and helps us understand patterns in element behavior. Elements are listed in rows called periods and columns known as groups.

• Periods: These are horizontal rows. Moving from left to right in a period, elements become less metallic and more non-metallic.
• Groups: These are vertical columns. Elements in the same group often display similar chemical and physical properties because they have the same number of electrons in their outer shell.

The periodic table is indispensable when studying chemical properties like electronegativity because it visually illustrates trends that are essential for predicting how elements react with each other.

Chemical Elements

Chemical elements are the simplest substances that can't be broken down into simpler substances by chemical means. Each element is defined by the number of protons in its atomic nucleus, known as the atomic number.

When identifying elements on the periodic table, each element has a unique symbol, often derived from its English or Latin name. For instance:

• Nitrogen (N): A key component of the earth's atmosphere, and an essential part of amino acids and nucleic acids.
• Oxygen (O): Vital for respiration in most living organisms and also forms oxides with nearly all elements.
• Phosphorus (P): Important for biological molecules like DNA and ATP, and used in the manufacture of safety matches, fertilizers, and other products.
• Germanium (Ge): A metalloid used in semiconductors and infrared optics.

Each element's position on the periodic table can give us clues about its chemical behavior and potential interactions with other elements.

Electronegativity Trends

Electronegativity is a concept that describes an atom's tendency to attract and hold electrons when it forms a chemical bond. Understanding electronegativity is crucial for predicting the kind of bond elements will form: ionic, covalent, or polar covalent.

Several trends are observed with electronegativity in the periodic table:

• Across a Period: Electronegativity tends to increase as you move from left to right across a period. This happens because atoms have more protons, increasing their positive charge and pulling electrons more effectively.
• Down a Group: Moving down a group, electronegativity generally decreases. This is because the increased number of electron shells puts the outermost electrons further from the nucleus, weakening the pull.

For the elements in the original exercise, this means that Germanium (Ge) will have the lowest electronegativity, followed by Phosphorus (P), then Nitrogen (N), with Oxygen (O) having the highest electronegativity of the four. These trends are key to understanding why these elements attract electrons differently during chemical reactions.