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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Here are the explanations for the observations and the properties of the elements: 2. Explain the following observations: a) Melting point of sodium is higher than that of potassium. Sodium has a smaller atomic radius than potassium. This leads to stronger metallic bonds in sodium due to a greater electrostatic attraction between the positively charged sodium ions and the delocalized electrons. More energy is required to overcome these stronger bonds, resulting in a higher melting point for sodium. b) The melting point of sodium fluoride is higher than that of sodium iodide. Both are ionic compounds. The melting point of ionic compounds depends on the lattice energy. Fluoride ions (F-) are significantly smaller than iodide ions (I-). The smaller ionic radius of F- leads to a stronger electrostatic attraction between the Na+ and F- ions, resulting in a higher lattice energy for sodium fluoride. More energy is needed to break these stronger ionic bonds. c) Molecular substances have low melting points. Molecular substances are composed of discrete molecules held together by weak intermolecular forces (such as van der Waals forces, dipole-dipole interactions, or hydrogen bonds). Only a small amount of energy is required to overcome these weak forces to change the substance from a solid to a liquid, hence their low melting points. d) Both graphite and diamond are allotropes of carbon. Graphite conducts electricity whereas diamond does not. Explain. In diamond, each carbon atom is sp3 hybridized and covalently bonded to four other carbon atoms in a rigid tetrahedral structure. All valence electrons are involved in strong covalent bonds, leaving no free or delocalized electrons to conduct electricity. In graphite, each carbon atom is sp2 hybridized and covalently bonded to three other carbon atoms, forming hexagonal layers. The remaining valence electron on each carbon atom is delocalized across the entire layer, creating a "sea" of mobile electrons. These delocalized electrons are free to move and conduct electricity. 3. What is the physical state at room temperature of? a) Chlorine: Gas b) Bromine: Liquid c) Iodine: Solid 4. What is the colour of? a) Chlorine: Yellow-green gas Send me the next one 📸