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Chapter 1: Problem 3

Problem \(1.3\) Judging from their relative positions in the Periodic Table, which element in each set is the more electronegative? (a) Lithium or potassium (b) Nitrogen or phosphorus (c) Carbon or silicon

Short Answer

Expert verified
Answer: The more electronegative elements in each pair are lithium (Li), nitrogen (N), and carbon (C).

Step by step solution

01

Determining electronegativity of lithium and potassium

We first need to locate lithium (Li) and potassium (K) in the Periodic Table. Li is in Group 1 and Period 2, while K is in Group 1 and Period 4. As we move down a group, electronegativity decreases, so the more electronegative element is lithium (Li).
02

Determining electronegativity of nitrogen and phosphorus

We now locate nitrogen (N) and phosphorus (P) in the Periodic Table. N is found in Group 15 and Period 2, while P is in Group 15 and Period 3. Electronegativity decreases down a group, so nitrogen (N), being in a higher period, is more electronegative than phosphorus (P).
03

Determining electronegativity of carbon and silicon

Finally, we locate carbon (C) and silicon (Si) in the Periodic Table. Carbon (C) is in Group 14 and Period 2, while silicon (Si) is in Group 14 and Period 3. Since electronegativity decreases down a group, carbon (C), being higher up in the Periodic Table, is more electronegative than silicon (Si).

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Most popular questions from this chapter

Predict all bond angles for these molecules. (a) \(\mathrm{CH}_{3} \mathrm{OH}\) (b) \(\mathrm{PF}_{3}\) (c) \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

Write and compare the ground-state electron configurations for each pair of elements. (a) Carbon and silicon (b) Oxygen and sulfur (c) Nitrogen and phosphorus

Draw structural formulas for (a) The eight alcohols with the molecular formula \(\mathrm{C}_{5} \mathrm{H}_{12} \mathrm{O}\). (b) The eight aldehydes with the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}\). (c) The six ketones with the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}\). (d) The eight carboxylic acids with the molecular formula \(\mathrm{C}_{6} \mathrm{H}_{12} \mathrm{O}_{2}\). (e) The nine carboxylic esters with the molecular formula \(\mathrm{C}_{5} \mathrm{H}_{10} \mathrm{O}_{2}\). \(\mathbf{1 . 4 8}\) Identify the functional groups in each compound.

Draw structural formulas for the three secondary amines with the molecular formula \(\mathrm{C}_{4} \mathrm{H}_{11} \mathrm{~N}\).

(a) Draw a Lewis structure for the ozone molecule, \(\mathrm{O}_{3}\). (The order of atom attachment is \(\mathrm{O}-\mathrm{O}-\mathrm{O}\), and they do not form a ring.) Chemists use ozone to cleave carboncarbon double bonds (Section 6.5C). (b) Draw four contributing resonance structures; include formal charges. (c) How does the resonance model account for the fact that the length of each \(\mathrm{O}-\mathrm{O}\) bond in ozone \((128 \mathrm{pm})\) is shorter than the \(\mathrm{O}-\mathrm{O}\) single bond in hydrogen peroxide (HOOH, \(147 \mathrm{pm}\) ) but longer than the \(\mathrm{O}-\mathrm{O}\) double bond in the oxygen molecule \((123 \mathrm{pm})\) ?
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