Question

The elements \(\mathrm{H}, \mathrm{N}, \mathrm{O}, \mathrm{P},\) and \(\mathrm{S}\) are commonly bonded to carbon in organic \(\mathrm{com}-\) pounds. Arrange these elements in order of increasing electronegativity.

Short answer

P, H, S, N, O

Step-by-step solution

Understanding Electronegativity

Electronegativity is the tendency of an atom to attract electrons in a chemical bond. The higher an atom's electronegativity, the more it attracts electrons.

Knowing Electronegativities of Elements

The known electronegativities for the given elements are approximately: \(\text{H} = 2.20\), \(\text{N} = 3.04\), \(\text{O} = 3.44\), \(\text{P} = 2.19\), and \(\text{S} = 2.58\).

Arrange Elements

Using the provided electronegativities, arrange the elements in order of increasing electronegativity: \(\text{P} (2.19) < \text{H} (2.20) < \text{S} (2.58) < \text{N} (3.04) < \text{O} (3.44)\).

Key concepts

Chemical Bonds

Chemical bonds are the connections between two or more atoms that hold these atoms together in a molecule. These bonds make it possible for complex substances to form. There are different types of chemical bonds, but the most common ones include:

• Covalent Bonds: This is where atoms share electrons. They commonly occur between two nonmetals, such as in water (H₂O).
• Ionic Bonds: These bonds form when one atom donates electrons to another atom, resulting in a bond between a metal and a nonmetal, like in table salt (NaCl).
• Metallic Bonds: Found mainly in metals, these bonds involve a sea of electrons shared among many atoms.

Electronegativity plays an important role in determining the type of bond that will form between elements. If the difference in electronegativity between two atoms is large, they may form an ionic bond. Conversely, if the difference is small, they will likely form a covalent bond. Understanding the nature of chemical bonds can help predict molecular structure and reactivity.

Periodic Table

The periodic table is a tabular arrangement of all known chemical elements, organized by their atomic number, electron configuration, and recurring chemical properties. It is a very useful tool for understanding elements' behaviors and their relationships with one another.

• Rows and Columns: Elements in the same column, known as a group, usually have similar chemical properties because they have the same number of valence electrons.
• Trends: As you move across a period (row), atomic number increases, often leading to an increase in electronegativity and a decrease in atomic size.
• Blocks: The table is divided into blocks (s, p, d, f) which indicate the subshell that is being filled with electrons.

Elements listed in the exercise, such as hydrogen ( H ), nitrogen ( N ), oxygen ( O ), phosphorus ( P ), and sulfur ( S ), are placed within specific groups in the periodic table that hint at their bonding tendencies and electronegativity values.

Element Properties

Element properties are essential characteristics that define an element's behavior in chemical reactions and bonding. Some key properties include:

• Electronegativity: A measure of an atom's ability to attract electrons. As seen in the exercise, arranged electronegativity values help determine how atoms interact in compounds.
• Atomic Radius: This is the size of an atom; generally, it decreases across a period and increases down a group in the periodic table.
• Ionization Energy: The energy required to remove an electron from an atom. Higher electronegativity often means higher ionization energy.
• Reactivity: An element's ability to undergo chemical reactions. Elements with high electronegativity, like fluorine, are generally very reactive nonmetals.

Understanding these properties assists in predicting how an element will behave in chemical contexts, aiding in everything from simple experimentations to complex computational chemistry models.