Examining the crystal structure of CsCl (Caesium Chloride), the Cs+ions form the 8 corners of a cube and the Cl−ion is a the center of the cube. From first-principles calculation, it was determined that the lattice constant of CsCl is 4.209 ̊A. (a) Calculate in detail the electrostatic force exerted by all the Cs+ atoms to the Cl−atom; (b) Assuming that 1 Cs+atom is missing in crystal structure (crystal is said to have a defect), calculate in detail what will be the net electrostatic force on the Cl−ion due to the remaining Cs+ions.

At standard temperature and pressure, the molar volumesof Cl2 and NH3 gases are 22.06 and 22.40 L, respectively.(a) Given the different molecular weights, dipole moments,and molecular shapes, why are their molar volumes nearlythe same? (b) On cooling to 160 K, both substances formcrystalline solids. Do you expect the molar volumes todecrease or increase on cooling the gases to 160 K? (c) Thedensities of crystalline Cl2 and NH3 at 160 K are 2.02 and0.84 /cm3, respectively. Calculate their molar volumes.(d) Are the molar volumes in the solid state as similar asthey are in the gaseous state? Explain. (e) Would you expectthe molar volumes in the liquid state to be closer to thosein the solid or gaseous state?

Aluminum metal is produced by heating aluminumoxide, Al2O3(s), and other substances to almost1000 °C until the mixture melts. Molten aluminumoxide is an excellent conductor. An electric currentpassed through liquid aluminum oxide can providethe electrons needed to convert the aluminumions to neutral metal atoms. Explain the followingproperties of aluminum oxide in terms of ionicbonding: K/U(a) its high electrical conductivity when molten(b) its high melting point

Analyze the properties and applications of nanoparticles in modern chemistry. Discuss how size-dependent properties of nanoparticles differ from bulk materials and their potential uses in various fields.