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The Gmelin rare earths handbook lists 1522 °C and 1550 °C as two melting points given in the literature, the most recent reference [Handbook on the chemistry and physics of rare earths, vol.12 (1989)] is given with 1529 °C.
This is an accepted version of this page This is the latest accepted revision, reviewed on 10 February 2025. This article is about the chemical element. For other uses, see Iodine (disambiguation). Chemical element with atomic number 53 (I) Iodine, 53 I Iodine Pronunciation / ˈ aɪ ə d aɪ n, - d ɪ n, - d iː n / (EYE -ə-dyne, -din, -deen) Appearance lustrous metallic gray solid ...
Ionic iodides MI n tend to have the lowest melting and boiling points among the halides MX n of the same element, because the electrostatic forces of attraction between the cations and anions are weakest for the large iodide anion. In contrast, covalent iodides tend to instead have the highest melting and boiling points among the halides of the ...
Sodium carbonate serves as a flux for silica (SiO 2, melting point 1,713 °C), lowering the melting point of the mixture to something achievable without special materials. This "soda glass" is mildly water-soluble, so some calcium carbonate is added to the melt mixture to make the glass insoluble.
Sodium iodide (chemical formula NaI) is an ionic compound formed from the chemical reaction of sodium metal and iodine. Under standard conditions, it is a white, water-soluble solid comprising a 1:1 mix of sodium cations (Na +) and iodide anions (I −) in a crystal lattice. It is used mainly as a nutritional supplement and in organic chemistry.
The following chart shows the solubility of various ionic compounds in water at 1 atm pressure and room temperature (approx. 25 °C, 298.15 K). "Soluble" means the ionic compound doesn't precipitate, while "slightly soluble" and "insoluble" mean that a solid will precipitate; "slightly soluble" compounds like calcium sulfate may require heat to precipitate.
It can be prepared by reacting a sodium-containing base such as sodium hydroxide with iodic acid, for example: HIO 3 + NaOH → NaIO 3 + H 2 O. It can also be prepared by adding iodine to a hot, concentrated solution of sodium hydroxide or sodium carbonate: 3 I 2 + 6 NaOH → NaIO 3 + 5 NaI + 3 H 2 O
Copper(I) iodide reacts with mercury vapors to form brown copper(I) tetraiodomercurate(II): . 4 CuI + Hg → (Cu +) 2 [HgI 4] 2− + 2 Cu. This reaction can be used for the detection of mercury since the white CuI to brown Cu 2 [HgI 4] color change is dramatic.