What do you understand by the following terms
a. Ionisation enthalpy.
b. Lattice enthalpy.
c. Bond enthalpy
d. Bond angle
e. electron gain enthalpy
f. electronegativity
Answers
Explanation:
a. Ionisation enthalpy: Ionization energy or Ionization enthalpy of elements is defined as
the amount of energy required by an isolated gaseous atom to lose an electron in its ground state.
b. Lattice enthalpy: Lattice enthalpy is a measure of the strength of the forces between the ions in an ionic solid. The greater the lattice enthalpy, the stronger the forces. Those forces are only completely broken when the ions are present as gaseous ions, scattered so far apart that there is a negligible attraction between them.
c.Bond angle: Bond angle can be defined as the angle formed between two covalent bonds that originate from the same atom
d.bond enthalpy: Bond energy is a measure of the strength of a chemical bond. It can be defined as the energy required to break all covalent bonds of a specific type in one mole of a chemical compound
e .electron gain enthalpy: Electron gain enthalpy is defined as the amount of energy released when an electron is added to an isolated gaseous atom. During the addition of an electron, energy can either be released or absorbed.
f.electronnegetivity:Electronegativity is a measure of the tendency of an atom to attract a bonding pair of electrons. The Pauling scale is the most commonly used. Fluorine (the most electronegative element) is assigned a value of 4.0, and values range down to cesium and francium which are the least electronegative at 0.7.