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A carbonate is a salt of carbonic acid, (H 2 CO 3), [2] characterized by the presence of the carbonate ion, a polyatomic ion with the formula CO 2− 3.The word "carbonate" may also refer to a carbonate ester, an organic compound containing the carbonate group O=C(−O−) 2.
The bicarbonate ion carries a negative one formal charge and is an amphiprotic species which has both acidic and basic properties. It is both the conjugate base of carbonic acid H 2 CO 3; and the conjugate acid of CO 2− 3, the carbonate ion, as shown by these equilibrium reactions: CO 2− 3 + 2 H 2 O ⇌ HCO − 3 + H 2 O + OH − ⇌ H 2 CO ...
Each blue halo represents one half of a negative charge. In chemistry, an oxocarbon anion is a negative ion consisting solely of carbon and oxygen atoms, and therefore having the general formula C x O n− y for some integers x, y, and n. The most common oxocarbon anions are carbonate, CO 2− 3, and oxalate, C 2 O 2− 4. There are however a ...
To a single metal ion, carbonate is observed to bind in both unidentate (κ 1-) and bidentate (κ 2-) fashions. [5] In the covalent bond classification method, κ 1-carbonate is anX ligand and κ 2-carbonate is an X 2 ligand. With two metals, the number of bonding modes increases because carbonate often serves as a bridging ligand.
A simple example of a polyatomic ion is the hydroxide ion, which consists of one oxygen atom and one hydrogen atom, jointly carrying a net charge of −1; its chemical formula is O H −. In contrast, an ammonium ion consists of one nitrogen atom and four hydrogen atoms, with a charge of +1; its chemical formula is N H + 4.
Neodymium(III) carbonate is an inorganic compound, a salt, where neodymium is in the +3 oxidation state and the carbonate ion has charge -2. [1] It has a chemical formula of Nd 2 (CO 3) 3. The anhydrous form is purple-red, [2] while the octahydrate is a pink solid. [3] Both of these salts are insoluble in water. [4]
It is manufactured by treating an aqueous solution of potassium carbonate or potassium hydroxide with carbon dioxide: [1] K 2 CO 3 + CO 2 + H 2 O → 2 KHCO 3. Decomposition of the bicarbonate occurs between 100 and 120 °C (212 and 248 °F): 2 KHCO 3 → K 2 CO 3 + CO 2 + H 2 O. This reaction is employed to prepare high purity potassium carbonate.
For cations that take on multiple charges, the charge is written using Roman numerals in parentheses immediately following the element name. For example, Cu(NO 3) 2 is copper(II) nitrate, because the charge of two nitrate ions (NO − 3) is 2 × −1 = −2, and since the net charge of the ionic compound must be zero, the Cu ion has a 2+ charge ...