binary acid

(noun)

molecular compounds in which hydrogen is combined with a second nonmetallic element

Related Terms

Examples of binary acid in the following topics:

  • Binary Acids

    • Binary acids are certain molecular compounds in which hydrogen is bonded with a nonmetal.
    • Binary acids are certain molecular compounds in which hydrogen is combined with a second nonmetallic element; these acids include HF, HCl, HBr, and HI.
    • The names of binary acids begin with "hydro-" followed by the name of the other element, modified to end with "-ic."
    • Binary acids are one of two classes of acids, the second being oxoacids (or oxyacids), which consist of hydrogen, oxygen, and a third element, which is often a non-metal.
    • It is a member of the binary acids.

  • Naming Acids and Bases

    • Simple acids, known as binary acids, have only one anion and one hydrogen.
    • So, HNO3 will be nitric acid.
    • Therefore, HClO4 is called perchloric acid.
    • For example, chlorous acid is HClO2.
    • For example, instead of bromic acid, HBrO3, we have hypobromous acid, HBrO.

  • Oxoacids

    • Halogen oxoacids include hypochlorous acid (HOCl); chlorous acid(HOClO); chloric acid(HOClO2); oerchloric acid(HOClO3); oerbromic acid (HOBrO3)
    • All oxoacids have the acidic hydrogen bound to an oxygen atom, so bond strength (length) is not a factor, similar to binary nonmetal acids; instead, the main determining factor for an oxacid's relative strength has to do with the central atom's electronegativity (X), as well as the number of O atoms around that central atom.
    • Consider the simple oxyacids HOI (hypoiodous acid), HOBr (hypobromous acid), and HOCl (hypochlorous acid).
    • Carboxylic acids are the most common type of organic acid.
    • Mellitic acid is an example of a hexacarboxylic acid.

  • Binary Hydrides

    • Hydrides can be used as strong bases in organic syntheses, and their reaction with weak Bronsted acids releases dihydrogen (H2).
    • Most ionic hydrides exist as "binary" materials that involve only two elements, one of which is hydrogen.
    • In these substances, the hydride bond, formally, is a covalent bond much like the bond that is made by a proton in a weak acid.
    • Such bulk transition metals form interstitial binary hydrides when exposed to hydrogen.
    • This is a space-filling model of a crystal of lithium hydride, LiH, a binary halide.

  • Halogen Compounds

    • The halogens all form binary compounds with hydrogen, and these compounds are known as the hydrogen halides: hydrogen fluoride (HF), hydrogen chloride (HCl), hydrogen bromide (HBr), hydrogen iodide (HI), and hydrogen astatide (HAt).
    • All of these except HF are strong chemical acids when dissolved in water.
    • The names of these acids are as follows:
    • All of these acids are dangerous and must be handled with great care.
    • They are also used by the body to produce stomach acid.

  • The Halogens (Group 17)

    • The halogens all form binary compounds with hydrogen, known as the hydrogen halides: hydrogen fluoride (HF), hydrogen chloride (HCl), hydrogen bromide (HBr), hydrogen iodide (HI), and hydrogen astatide (HAt).
    • However, hydrofluoric acid is quite destructive to animal tissue.
    • The names of these acids are as follows: hydrofluoric acid, hydrochloric acid, hydrobromic acid, and hydroiodic acid.
    • Some of these acids are also widely used in industry.
    • Dissolved chlorine reacts to form hydrochloric acid (HCl) and hypochlorous acid (HClO), a solution that can be used as a disinfectant or bleach:

  • Chromium

    • Chromium(III) hydroxide (Cr(OH)3) is amphoteric, dissolving in acidic solutions to form [Cr(H2O)6]3+ and in basic solutions to form [Cr(OH)6]3−.
    • The change in equilibrium is visible by a change from yellow (chromate) to orange (dichromate), such as when an acid is added to a neutral solution of potassium chromate.
    • The only binary compound is the volatile chromium(V) fluoride (CrF5).

  • Copper

    • The simplest compounds of copper are binary compounds, i.e. those containing only two elements.
    • Oxygen-containing ammonia solutions yield water-soluble complexes with copper, as do oxygen and hydrochloric acid, which form copper chlorides, and acidified hydrogen peroxide, which form copper(II) salts.
    • The simplest compounds of copper are binary compounds (i.e., those containing only two elements).
    • Amino acids form very stable chelate complexes with copper(II).

  • Polyprotic Acid Titrations

    • Polyprotic acids, also known as polybasic acids, are able to donate more than one proton per acid molecule.
    • Common examples of monoprotic acids in mineral acids include hydrochloric acid (HCl) and nitric acid (HNO3).
    • On the other hand, for organic acids the term mainly indicates the presence of one carboxylic acid group, and sometimes these acids are known as monocarboxylic acid.
    • Polyprotic acid are able to donate more than one proton per acid molecule, in contrast to monoprotic acids that only donate one proton per molecule.
    • An example of a triprotic acid is orthophosphoric acid (H3PO4), usually just called phosphoric acid.

  • Diprotic and Polyprotic Acids

    • Diprotic and polyprotic acids contain multiple acidic protons that dissociate in distinct, sequential steps.
    • As their name suggests, polyprotic acids contain more than one acidic proton.
    • Two common examples are carbonic acid (H2CO3, which has two acidic protons and is therefore a diprotic acid) and phosphoric acid (H3PO4, which has three acidic protons and is therefore a triprotic acid).
    • With any polyprotic acid, the first amd most strongly acidic proton dissociates completely before the second-most acidic proton even begins to dissociate.
    • Identify the key features that distinguish polyprotic acids from monoprotic acids.