Question

Across a period, how does the electronegativity of a nonmetal affect the acidity of its binary hydride?

Short answer

As nonmetal electronegativity increases across a period, the acidity of its binary hydride increases.

Step-by-step solution

Understand electronegativity

Electronegativity is a measure of an atom's ability to attract and hold electrons. It increases across a period from left to right on the periodic table.

Identify nonmetals in the period

Nonmetals are located on the right side of the periodic table. Identify which nonmetals are present in the period in question.

Assess nonmetal's electronegativity

Determine the electronegativity values of the nonmetals in the period. Use periodic trends to note that these values increase as you move from left to right.

Understand acidity of binary hydrides

A binary hydride consists of hydrogen and one other element. The acidity of these hydrides depends on the strength of the bond between hydrogen and the other element, as well as the resulting negative ion's stability.

Relate electronegativity to acidity

Higher electronegativity in nonmetals means they more strongly attract electrons, making it easier for the binary hydride to release a proton (H+). Thus, the acidity increases as the electronegativity of the nonmetal increases.

Conclude the relationship

Summarize that as the electronegativity of a nonmetal increases across a period, the acidity of its binary hydride also increases.

Key concepts

Electronegativity

Electronegativity is a vital concept in chemistry. It measures an atom's ability to attract and hold electrons.
This property varies across the periodic table.
As we move from left to right across a period, electronegativity increases.
For example, fluorine has a higher electronegativity than carbon.
Understanding this trend helps in predicting how atoms will interact in different chemical reactions.

Periodic Trends

In the periodic table, certain properties of elements follow predictable patterns.
This predictable variation is known as periodic trends.
One key trend is the increase in electronegativity from left to right across a period.
Other trends include atomic size, ionization energy, and electron affinity.
Recognizing these trends makes it easier to predict the behavior of substances in chemical reactions and bonding.

Binary Hydrides

Binary hydrides are compounds consisting of hydrogen and one other element.
Examples include HF (hydrogen fluoride) and NH₃ (ammonia).
The properties of binary hydrides depend on the elements involved and their positions in the periodic table.
Acidity in binary hydrides is influenced by the strength of the bond between hydrogen and the other element.
Understanding the nature of these compounds is crucial for grasping many chemical reactions and processes.

Nonmetals

Nonmetals are located on the right side of the periodic table.
They tend to have higher electronegativity values compared to metals.
Common nonmetals include oxygen, nitrogen, and sulfur.
These elements play key roles in forming covalent bonds due to their ability to attract electrons strongly.
Knowing about nonmetals and their properties helps in predicting the types of compounds they will form.

Acidity

Acidity refers to the ability of a compound to donate a proton (H+).
In the context of binary hydrides, acidity increases with the nonmetal's electronegativity.
For example, HF is more acidic than CH₄ because fluorine is more electronegative than carbon.
Understanding acidity is crucial for predicting how substances will behave in different chemical environments, especially in reactions involving proton transfer.

Chemical Bonding

Chemical bonding describes how atoms combine to form molecules.
Bonds can be ionic, covalent, or metallic, depending on the elements involved.
Electronegativity plays a significant role in the type of bond formed.
Covalent bonds form when elements share electrons, typically seen in nonmetals.
In contrast, ionic bonds involve the transfer of electrons, often between metals and nonmetals.
Understanding chemical bonding is foundational for understanding all chemical reactions and compound formations.