This chemistry question involves key chemical concepts and calculations. The detailed solution below walks through each step, from identifying the reaction type to computing the final answer.
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Step 1: Identify elements W and Y. Element W has atomic number 11, which is Sodium (Na). Its electron configuration is 2, 8, 1. It tends to lose 1 electron to form W^+ (Na^+). Element Y has atomic number 9, which is Fluorine (F). Its electron configuration is 2, 7. It tends to gain 1 electron to form Y^- (F^-). a) Write the formula of the compound. Since W forms W^+ and Y forms Y^-, they combine in a 1:1 ratio to form a neutral compound. The formula of the compound is WY (or NaF). b) State the type of bond present in the compound formed. Element W (Sodium) is a metal, and element Y (Fluorine) is a non-metal. When a metal and a non-metal react, they form an ionic bond. The type of bond is ionic bond. c) Identify the type of structure formed. Ionic compounds form a crystal lattice structure where ions are held together by strong electrostatic forces. The type of structure is giant ionic lattice. --- 9) Determine its molecular formula. Step 1: Calculate the moles of each element in 100 g of the compound. Assume a 100 g sample: Mass of Carbon (C) = 40 g Mass of Hydrogen (H) = 6.7 g Mass of Oxygen (O) = 53.3 g Moles of C = massmolar mass = 40\, g12\, g/mol ≈ 3.33\, mol Moles of H = massmolar mass = 6.7\, g1\, g/mol = 6.7\, mol Moles of O = massmolar mass = 53.3\, g16\, g/mol ≈ 3.33\, mol Step 2: Determine the simplest mole ratio (empirical formula). Divide each mole value by the smallest number of moles (3.33 mol): For C: (3.33)/(3.33) = 1 For H: (6.7)/(3.33) ≈ 2.01 ≈ 2 For O: (3.33)/(3.33) = 1 The empirical formula is CH_2O. Step 3: Calculate the empirical formula mass. Empirical formula mass of CH_2O = (1 × 12.0) + (2 × 1.0) + (1 × 16.0) = 12.0 + 2.0 + 16.0 = 30.0. Step 4: Determine the molecular formula. The relative molecular mass is given as 180. Let n be the number of empirical formula units in the molecular formula. n = Relative molecular massEmpirical formula mass n = (180)/(30.0) = 6 Multiply the subscripts in the empirical formula by n: Molecular formula = (CH_2O)_6 = C_6H_12O_6. --- 10) Explain the difference in their melting points. Phosphorus trichloride (PCl_3) is a simple molecular substance. It consists of discrete PCl_3 molecules held together by weak intermolecular forces (van der Waals forces and dipole-dipole interactions). Only a small amount of energy is required to overcome these weak forces, leading to its low melting point of -91°C. Sodium chloride (NaCl) is an ionic compound with a giant ionic lattice structure. It consists of Na^+ and Cl^- ions held together by strong electrostatic forces of attraction throughout the lattice. A large amount of energy is required to overcome these strong forces to break down the lattice, resulting in its high melting point of 801°C. Got more? Send 'em 📸