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This is the second of our many quizzes on Ionic bonds. Click on this to access more such competitive quizzes on Physical Chemistry.

Ionic bonds Quiz 2

chemistry

 Amay discovered that an AB-type crystal, which is the main raw material used in the industrial manufacturing of $N{{a}_{2}}C{{O}_{3}}$ and $NaHC{{O}_{3}}$, acts as a non-conducting material when solid, but its solution begins conducting electricity. Which crystalline compound is mentioned?

 The AB-type ionic crystal has the same ratio of anion and cation present in the crystal. 

 The AB-type crystal specified is NaCl, which is formed by the ionic bond formation between $N{{a}^{+}}  \text{ and } C{{l}^{-}}$ ions. NaCl is used as the major raw material for the manufacturing of $N{{a}_{2}}C{{O}_{3}}$ and  $NaHC{{O}_{3}}$ and also finds application in glass manufacturing. As it is dissolved, the lattice structure is broken, allowing free ions to enter the solution and conduct electricity.

 Raghav was surveying the solubility values of Li compounds and he proposed its lattice energy from the solubility value, which compound would have the highest lattice energy?

 $ \text{Solubility}\alpha \dfrac{\text{1}}{\text{Lattice}\,\text{energy}} $  

 The compound's solubility is inversely proportional to the compound's lattice energy. If the solubility value is low, the lattice energy is maximised, implying that the bond between the ions is stronger. Because of the small size of the cation and anion and the strength of the ionic bond formed, LiF has the least solubility, meaning that the lattice energy is maximised.

 NaF possesses the highest melting point due to:

 Check the physical property of the compound form of which NaF belongs.

 We know that the NaF is an ionic compound, which is formed by the ionic bond formation between $N{{a}^{+}}$ and ${{F}^{-}}$ ions. The higher melting point of ionic compounds is one of their most distinguishing characteristics. As a result of its high ionic character, NaF has the highest melting point. Since the cation is larger and the anion is smaller in size, a strong ionic bond is formed, requiring more energy to melt or break the lattice.

 Adit was assigned the task of measuring the lattice energy of four compounds; which compound would have the highest lattice energy?

 $ Lattice\,energy=\dfrac{k{{q}_{1}}{{q}_{2}}}{r} $

 If we know the charge of the ions and the distance between them, we can measure the lattice energy using the formulae given below. Lattice energy  = $\dfrac{k{q}_{1}{q}_{2}}{r}$ , where k is the proportionality constant, r is the distance between the charges, ${q}_{1}$ and ${{q}_{2}}$ are the charges of the ions. MgO will have the maximum lattice energy as Mg in MgO has +2 charge and O has -2 charge.

  Amala plotted a graph of the first, second, and third ionization of an element (A) against its ionization enthalpies which are $565$, $1576$, and $1670$ kJ/mol. Predict the formula of chloride of this element<img  src="https://cmds-vedantu.s3.ap-southeast-1.amazonaws.com/prod/question-sets/249f7007-de5a-4ff8-a3e0-84f7d020304e3328350099058926018.png"/>

 The charge associated with the metal atom is calculated by subtracting the value of ionisation enthalpy from the preceding value.

 We may determine the charge on a metal atom by considering the ionisation energy value. The charge associated with the metal is determined by a large difference in the value of ionisation enthalpy from the preceding value. The charge associated with the metal is +2 since the second ionisation value is much greater than the first ionisation value. Metal A has a charge of +2, while metal Cl has a charge of -1. By crisscrossing the charges we get the formulae of the compound as $AC{{l}_{2}}.$