Mercury I ions

Mercury(I) ions can be produced in solution by dissolving excess mercury in dilute nitric acid ... [Pg.437]

Examples P2O5, diphosphorus pentaoxide or phosphorus)V) oxide Hgj, mercury(I) ion or dimercury(2-l-) ion K2[Fe(CN)g], potassium hexacyanoferrate(II) or potassium hexacyanofer-rate(4—) PbJPb 04, dilead(II) lead(IV) oxide or trilead tetraoxide. [Pg.216]

Compact, ready-prepared calomel electrodes are available commercially and find wide application especially in conjunction with pH meters and ion-selective meters. A typical electrode is shown in Fig. 15.1(h). With time, the porous contact disc at the base of the electrode may become clogged, thus giving rise to a very high resistance. In some forms of the electrode the sintered disc may be removed and a new porous plate inserted, and in some modern electrodes an ion exchange membrane is incorporated in the lower part of the electrode which prevents any migration of mercury(I) ions to the sintered disc and thus... [Pg.552]

Self-Test I.2B The mercury(I) ion, Hg22+, consists of two Hg+ ions joined together. Write the net ionic equation for the reaction in which colorless aqueous solutions of mercury(I) nitrate, Hg2(N03)2, and potassium phosphate, K3P04, react to give a white precipitate of mercurv(I) phosphate. [Pg.93]

Explain why the formula for mercury(I) ion is Hg22 + rather than Hg+. [Pg.108]

Write the net ionic equation and the half-reactions for the disproportionation of mercury(I) ions in aqueous solution to give liquid mercury and aqueous mercury(II) ions. Assume that mercury(I)... [Pg.468]

In their 1966 treatise, Phillips and Williams33 pointed out that the mercury(I) ion, Hg2+ (9), can be regarded formally as a very stable complex of the type HguL where L is Hg° they also speculated about the possible existence of Hgf+ (10), which by the same formalism is a complex of the type LHgnL. The position of equilibrium (2) (n = 1) in water does favour (9) very strongly a recent value of log Kx is 8.28 at 25 °C, I = 0.1 M NaC104,34 in between log K values reported35 for the... [Pg.3]

The mercury(I) ion is Hg22+, with two Hg+ ions bonded together. [Pg.115]

The appearance of a yellow precipitate, lead chromate (PbCr04), indicates the presence of lead ions. To separate silver ions and mercury I ions, ammonium hydroxide (NH4OH), which converts to NH3, is added to the precipitates ... [Pg.334]

Rosdahl J, Persson I et al (2004) On the solvation of the mercury(I) ion. A structural, vibration spectroscopic and quantum chemical study. Inorg Chem A 357 2624... [Pg.278]

Hot, concentrated sulphuric acid dissolves mercury as well. The product is mercury(I) ion if mercury is in excess... [Pg.200]

Reactions of mercury(I) ions A solution of mercury(I) nitrate (0 05m) can be used for the study of these reactions. [Pg.200]

Tin(II) chloride reduces mercury(I) ions to mercury metal, which appears in the form of a greyish-black precipitate ... [Pg.203]

What happens if solid silver bromide is placed in water The solubility table states that bromide compounds are soluble with the exception of silver, lead (II), and mercury (I) ions. Therefore, the silver bromide would be insoluble and remain a solid. [Pg.50]

In Chapter 6, we learned how to name cations. In the Stock system, the charges on monatomic ions were used to distinguish between different ions of the same element. For example, Cu and Cu are named copper ion and copper(ll) ion, respectively. The Roman numeral actually represents the oxidation number, not the charge on the ion. Of course, for monatomic ions, the charge is equal to the oxidation number, and thus we used the charge to determine which Roman numeral to use. By using oxidation numbers, however, we can extend our compound-naming ability to include compounds other than those of monatomic ions. For example, Hg2 is called the mercury(I) ion because the oxidation number of each mercury atom is +1. [Pg.449]

In Chap. 6 we placed Roman numerals at the ends of names of metals to distinguish the charges on monatomic cations. It is really the oxidation number that is in parentheses. This nomenclature system is called the Stock system. For monatomic ions, the oxidation number is equal to the charge. For other cations, again the oxidation number is used in the name. For example, Hg2 + is named mercury(I) ion. Its charge is 24- the oxidation number of each atom is 4-1. Oxidation numbers are also used for other cations, such as dioxovanadium(V) ion, V02". The prefix 0x0- stands for oxygen. Oxidation numbers can be used with nonmetal-nonmetal compounds, as in sulfur(VI) oxide for SO3, but the older system using prefixes (Table 6-2) is still used more often. [Pg.205]

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