Based on molecular structure, arrange the binary compounds in order of increasing acid strength. Explain your choice. H₂Te, HI, H₂S, NaH

Verified step by step guidance

1. Identify the type of acids involved: Binary acids are typically composed of hydrogen and one other element.
2. Consider the periodic trends: Acid strength in binary acids generally increases across a period and down a group in the periodic table.
3. Analyze the molecular structure: The strength of an acid is influenced by the bond strength between hydrogen and the other element. Weaker bonds typically result in stronger acids.
4. Apply the concept to the given compounds: Compare the bond strengths and electronegativities of the elements in H2Te, HI, H2S, and NaH.
5. Arrange the compounds: Based on the analysis, order the compounds from weakest to strongest acid.

Key Concepts

Acid Strength

Acid strength refers to the ability of a compound to donate protons (H+) in a solution. Strong acids completely dissociate in water, while weak acids only partially dissociate. The strength of binary acids, which consist of hydrogen and one other element, often increases with the size and electronegativity of the non-hydrogen element.

Binary Acids

Binary acids are compounds formed from hydrogen and one other nonmetal element. The general formula is HA, where A is a nonmetal. The strength of binary acids typically increases down a group in the periodic table due to the decreasing bond strength between hydrogen and the nonmetal, making it easier for the acid to release a proton.

Electronegativity and Bond Strength

Electronegativity is the tendency of an atom to attract electrons in a bond. In binary acids, higher electronegativity of the nonmetal can lead to stronger H-A bonds, but as you move down a group, larger atomic size results in weaker bonds. This interplay affects the acid's ability to dissociate and thus its strength, with larger, less electronegative atoms generally leading to stronger acids.