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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2.1 A chemical bond is a strong attractive force that holds atoms together in a molecule or crystal. 2.2.1 The molecules with only covalent bonds and that are non-polar are H_2, N_2, and CH_4. A 2.2.2 A non-polar molecule with polar bonds is CH_4. The C-H bonds are polar, but the tetrahedral geometry of the molecule results in the bond dipoles cancelling out, making the molecule non-polar overall. D 2.3.1 The shape of the molecule in substance D (CH_4) is tetrahedral. 2.3.2 The Lewis structure for the molecule in substance E (HCN) is: H-C: 2.4 Step 1: Identify the electronegativity values for Li and F. The electronegativity of Li is approximately 1.0. The electronegativity of F is approximately 4.0. Step 2: Calculate the electronegativity difference. Electronegativity difference = 4.0 - 1.0 = 3.0 Step 3: Determine the type of bond based on the difference. Since the electronegativity difference (3.0) is greater than 1.7, the bond between Li and F is predominantly ionic. 2.5 The Lewis structure for substance B (N_2) is: :N: Nitrogen gas (N_2) is unreactive at room temperature and normal pressures because it contains a very strong triple covalent bond between the two nitrogen atoms. A large amount of energy is required to break this bond, making it difficult for N_2 to react. 2.6.1 The ion formed when substance C (NH_3) reacts with the H^+ ion is the ammonium ion (NH_4^+). 2.6.2 Two requirements for the formation of dative covalent bonds are: • One atom must have a lone pair of electrons to donate. • Another atom or ion must have an empty orbital to accept the lone pair of electrons. Send me the next one 📸