Search results
Results From The WOW.Com Content Network
Calcium chloride was apparently discovered in the 15th century but wasn't studied properly until the 18th century. [11] It was historically called "fixed sal ammoniac" (Latin: sal ammoniacum fixum [12]) because it was synthesized during the distillation of ammonium chloride with lime and was nonvolatile (while the former appeared to sublime); in more modern times (18th-19th cc.) it was called ...
In chemistry, a salt or ionic compound is a chemical compound consisting of an assembly of positively charged ions and negatively charged ions , [1] which results in a compound with no net electric charge (electrically neutral). The constituent ions are held together by electrostatic forces termed ionic bonds.
Sodium atoms have 11 electrons, one more than the stable configuration of the noble gas neon. As a result, sodium usually forms ionic compounds involving the Na + cation. [1] Sodium is a reactive alkali metal and is much more stable in ionic compounds. It can also form intermetallic compounds and organosodium compounds.
Thus, bonding is considered ionic where the ionic character is greater than the covalent character. The larger the difference in electronegativity between the two types of atoms involved in the bonding, the more ionic (polar) it is. Bonds with partially ionic and partially covalent character are called polar covalent bonds. For example, Na–Cl ...
This driving force is what causes sodium and chlorine to undergo a chemical reaction, wherein the "extra" electron is transferred from sodium to chlorine, forming sodium cations and chloride anions. Being oppositely charged, these cations and anions form ionic bonds and combine to form sodium chloride , NaCl, more commonly known as table salt.
Ca(ClO 3) 2 + 2 KCl → 2 KClO 3 + CaCl 2. This is the second step of the Liebig process for the manufacture of potassium chlorate. [2] Solutions of calcium chlorate react with solutions of alkali carbonates to give a precipitate of calcium carbonate and the alkali chlorate in solution: Ca(ClO 3) 2 + Na 2 CO 3 → 2 NaClO 3 + CaCO 3
If pure sodium chloride is used, a metallic sodium emulsion is formed in the molten NaCl which is impossible to separate. Therefore, one option is to have a NaCl (42%) and CaCl 2 (58%) mixture. The anode reaction is: 2Cl − → Cl 2 (g) + 2e −. The cathode reaction is: 2Na + + 2e − → 2Na (l) for an overall reaction of 2Na + + 2Cl − → ...
For example, sodium hydroxide, NaOH, is a strong base. NaOH(aq) → Na + (aq) + OH − (aq) Therefore, when a strong acid reacts with a strong base the neutralization reaction can be written as H + + OH − → H 2 O. For example, in the reaction between hydrochloric acid and sodium hydroxide the sodium and chloride ions, Na + and Cl − take ...