Look at the problem from the other angle why does it take energy to break up an ionic lattice. It is because of the electrostatic attrction of the ions which has to be overcome. A measure of the is energy is the lattice enthalpy which depends on the charges, th einterionic distances and the geometry of the lattice.
Generally speaking, "bond breaking" is endothermic and "bond making" is exothermic. When an ionic bond happens, that's usually a bond between two monatomic ions, and it's being formed. Since no bond is breaking, you have an overall exothermic process.
transferring the ion from its stable ionic state to unstable state
It is exothermic because heat is released. ATP is on the products side. =] =) =I =p
Compounds are not generally considered endothermic or exothermic. These terms refer to processes. So, the process of formation, or the process of decomposition, would be an endothermic process or an exothermic process.
A compound is never exothermic. Its reaction with some other substance is endothermic or exothermic like when calcium oxide reacts with water large amount of heat is evolved.
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For an element to lose an electron, that electron must become excited to the point it can escape the attractive force. This requires a net energy input, making it endothermic.
False. Formation of a compound is usually exothermic because a Noble Gas configuration forms around each atom. Therefore energy is given off during formation, and the atoms in the compound are more stable.
At least, one anion and one cation participate in forming a crystalline ionic lattice. Every ionic compound forms a lattice, they do not form molecules.
The compound sodium bromide is formed by the formation of ionic bonds between sodium and bromide ions.
Formation of choloform is endothermic or exothermic reaction?
The lattice energy of an ionic solid is a measure of the strength of bonds in that ionic compound. It is usually defined as the enthalpy of formation of the ionic compound from gaseous ions and as such is invariably exothermic. The concept of lattice energy has initially been developed for rocksalt-structured and sphalerite-structured compounds like NaCl and ZnS, where the ions occupy high-symmetry crystal lattice sites. In case of NaCl, the lattice energy is the energy released by the reaction
This step alone cannot be used to predict solubility.
lose an electron and become a positive ion.