Search results
Results from the WOW.Com Content Network
The primary decay mode of isotopes lighter than 35 Cl is electron capture to isotopes of sulfur; that of isotopes heavier than 37 Cl is beta decay to isotopes of argon; and 36 Cl may decay by either mode to stable 36 S or 36 Ar. [42] 36 Cl occurs in trace quantities in nature as a cosmogenic nuclide in a ratio of about (7–10) × 10 −13 to 1 ...
Substance Formula 0 °C 10 °C 20 °C 30 °C 40 °C 50 °C 60 °C 70 °C 80 °C 90 °C 100 °C Barium acetate: Ba(C 2 H 3 O 2) 2: 58.8: 62: 72: 75: 78.5: 77: 75
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.
Chlorine can be further oxidized to other oxides and oxyanions including hypochlorite (ClO −, the active ingredient in chlorine bleach), chlorine dioxide (ClO 2), chlorate (ClO − 3), and perchlorate (ClO − 4). In terms of its acid–base properties, chloride is a weak base as indicated by the negative value of the pK a of hydrochloric
Iron(III) chloride forms a 1:2 adduct with Lewis bases such as triphenylphosphine oxide; e.g., FeCl 3 (OP(C 6 H 5) 3) 2. The related 1:2 complex FeCl 3 (OEt 2) 2, where Et = C 2 H 5), has been crystallized from ether solution. [14] Iron(III) chloride also reacts with tetraethylammonium chloride to give the yellow salt of the tetrachloroferrate ...
Chloramine – NH 2 Cl; Chloric acid – HClO 3; Chlorine azide – ClN 3; Chlorine dioxide – ClO 2; Chlorine dioxide – ClO 2; Chlorine monofluoride – ClF; Chlorine monoxide – ClO; Chlorine pentafluoride – ClF 5; Chlorine perchlorate – Cl 2 O 4; Chlorine tetroxide – O 3 ClOOClO 3; Chlorine trifluoride – ClF 3; Chlorine ...
However, iron tends to form highly insoluble iron(III) oxides/hydroxides in aerobic environment, especially in calcareous soils. Bacteria and grasses can thrive in such environments by secreting compounds called siderophores that form soluble complexes with iron(III), that can be reabsorbed into the cell.
Carbonic acid is an illustrative example of the Lewis acidity of an acidic oxide. CO 2 + 2OH − ⇌ HCO 3 − + OH − ⇌ CO 3 2− + H 2 O. This property is a key reason for keeping alkali chemicals well sealed from the atmosphere, as long-term exposure to carbon dioxide in the air can degrade the material.