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(c) Orbit and Orbital

( d) Ionization Energy​

Answer 1

Answer:

In physics and chemistry, ionization energy (American English spelling) or ionisation energy (British English spelling), is the minimum amount of energy required to remove the most loosely bound electron of an isolated neutral gaseous atom or molecule.[1] It is quantitatively expressed as

X(g) + energy ⟶ X+(g) + e−

where X is any atom or molecule, X+ is the ion with one electron removed, and e− is the removed electron.[2] This is generally an endothermic process. As a rule, the closer the outermost electrons to the nucleus of the atom, the higher the atom's ionization energy.

The sciences of physics and chemistry use different units for ionization energy. In physics, the unit is the amount of energy required to remove a single electron from a single atom or molecule, expressed as electronvolts. In chemistry, the unit is the amount of energy required for all of the atoms in a mole of substance to lose one electron each: molar ionization energy or approximately enthalpy, expressed as kilojoules per mole (kJ/mol) or kilocalories per mole (kcal/mol).[3]

Comparison of ionization energies of atoms in the periodic table reveals two periodic trends:

ionization energy generally increases from left to right within a given period (that is, row).

ionization energy generally decreases from top to bottom in a given group (that is, column).

An orbit is the fixed path along which electrons revolve around the nucleus of the atom.

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Differences between Orbit and Orbitals

Orbit Orbitals

An orbit is the simple planar representation of an electron. An orbital refers to the dimensional motion of an electron around the nucleus in a three-dimensional motion.

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