Please answer question 16 part A and C **Electrostatic Attraction and Ionic Bond Formation**The electrostatic attraction between oppositely charged ions is called an *ionic bond*. The net energy change in the formation of an ionic bond is a composite of five steps, which can involve energy absorption or release. These steps for a generic metal, M, and a diatomic halogen, X₂, include:1. **Sublimation of the metal**2. **Dissociation of the X–X bond**3. **Ionization of the metal**4. **Transfer of the electron to X**5. **Crystalline solid formation**The overall energy transfer is the sum of the energy changes for each step. The **magnitude of the potential energy** of two interacting charges, E (related to Lattice energy), reflects the strength of ionic attraction. It is calculated as:\[ E = \frac{1}{4\pi\epsilon_0} \frac{q_1 \times q_2}{d} = k \frac{q_1 \times q_2}{d} \]Where:- \( k \) is a constant \( \left(\frac{1}{4\pi\epsilon_0} = \frac{1}{1.11 \times 10^{-10} \, \text{C}^2/(\text{J} \cdot \text{m})}\right) \)- \( q_1 \) and \( q_2 \) are charges of the ions- \( d \) is the distance between ion nuclei**Part A**For the formation of CsCl from Cs(s) and Cl₂(g), the steps are:1. Cs(s) → Cs(g)2. \( \frac{1}{2} \) Cl₂(g) → Cl(g)3. Cs(g) → Cs⁺(g) + e⁻4. Cl(g) + e⁻ → Cl⁻(g)5. Cs⁺(g) + Cl⁻(g) → CsCl(s)**Activity:**Identify which steps absorb or release energy by placing the steps in the appropriate categories.**Diagram Explanation:**The interactive diagram allows users to drag steps to categorize them under "Absorbs energy" or "Releases energy." There are buttons labeled 1 to 5 representing each step. Users can click 'Reset' to start over and **Part C**Consider the lattice energy of any ionic compound. What combination of ions and charges will produce the largest (in magnitude) lattice energies?- View Available Hint(s)**Options:**- small ions and small charges- large ions and large charges- small ions and large charges- large ions and small charges

Part (A): During the change in physical state of a substance heat energy is involved in the following manner: Solid→∆ Liquid .......Heat absorbedLiquid→∆ Gas .......Heat absorbed Gas→ Liquid ........Heat releasedLiquid → Solid .......Heat releasedGiven reaction: (1) Cs (s) → Cs(g) The system is changing from solid to gas (sublimation), hence, this process absorbs energy. (2) 1/2 Cl2 (g) → Cl (g) In this reaction, the bonds of Cl2 break to form Cl. And the process of breaking of bonds absorbs energy. (3) Cs (g) → Cs+ (g) + e- In this reaction, an electron is being ejected (ionization). This process absorbs energy.(4) Cl (g) + e- → Cl- (g) In this reaction, an electron is being added (electron affinity), so, this process releases energy. (5) Cs+ (g) + Cl- (g) → CsCl (s) In this reaction, an ionic compound is formed from the constituent ions. And ionic compounds are very stable because this process releases energy.Part (C): Lattice energy is the amount of energy released when one mole of a lattice is formed from its constituent ions. More lattice energy means more stability of the lattice. Small ions and large charges will produce the largest magnitude of lattice energies. Hence, the correct answer is option (3): Small ions and large charges.