Organic Chemistry: A Guided Inquiry
2nd Edition
ISBN: 9780618974122
Author: Andrei Straumanis
Publisher: Cengage Learning
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Textbook Question
Chapter 2, Problem 6E
For each element, predict (and draw a Lewis structure of) the most commonly occurring ion (some of these have a charge greater than
a. sulfur c. magnesium
b. iodine d. oxygen
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6. Write the singly bonded Lewis dot structure for BF3. Which of the following statements
best describes this structure?
A. It obeys the octet rule on all atoms.
B. It has less than an octet on at least one atom.
C. It has a lone pair of electrons on the boron atom.
D. It has less than an octet of electrons on all atoms.
A. State the Octet Rule.B. Write the Lewis symbol of neon. Is the neon atom stable? Does neon exist as atoms in nature? If not, how does neon exist in nature.C. Write the Lewis symbol of nitrogen. Is the nitrogen atom stable? Does nitrogen exist as atoms in nature? If not, how does nitrogen exist in nature.
Lewis structure for each of the following atoms.a. Rb (Z = 37) d. Ba (Z = 56)b. Cl (Z = 17) e. P (Z = 15)c. Kr (Z =36) f. At (Z = 85)
Chapter 2 Solutions
Organic Chemistry: A Guided Inquiry
Ch. 2 - Prob. 1CTQCh. 2 - The valence shell of an atom in a legitimate Lewis...Ch. 2 - Prob. 3CTQCh. 2 - Prob. 4CTQCh. 2 - Prob. 5CTQCh. 2 - It is impossible to draw a legitimate Lewis...Ch. 2 - Describe how to calculate the total number of...Ch. 2 - Prob. 8CTQCh. 2 - Prob. 9CTQCh. 2 - Prob. 10CTQ
Ch. 2 - Prob. 11CTQCh. 2 - Prob. 12CTQCh. 2 - A complete Lewis structure must show all nonzero...Ch. 2 - Prob. 14CTQCh. 2 - Prob. 15CTQCh. 2 - Prob. 16CTQCh. 2 - Prob. 17CTQCh. 2 - Prob. 18CTQCh. 2 - Complete the rest of the table for N, O or X by...Ch. 2 - Prob. 20CTQCh. 2 - Prob. 21CTQCh. 2 - Make a checklist that can be used to determine if...Ch. 2 - Prob. 2ECh. 2 - Prob. 3ECh. 2 - Draw the Lewis structure of a neutral molecule...Ch. 2 - Prob. 5ECh. 2 - For each element, predict (and draw a Lewis...Ch. 2 - Predict which of the following species is least...Ch. 2 - The molecules BH3 and SF6 and the ion SO42 exist...Ch. 2 - These are NOTlegitimate Lewisstructures (and...Ch. 2 - Fill in missing formal charges where needed (all...Ch. 2 - Below each structure in the previous question is a...Ch. 2 - Prob. 12ECh. 2 - Carbon monoxide (CO) is an example of an overall...Ch. 2 - Explain why this Lewis structure for CO is not as...Ch. 2 - Prob. 15ECh. 2 - Prob. 16ECh. 2 - Prob. 17ECh. 2 - Prob. 18ECh. 2 - Prob. 19E
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- Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?arrow_forwardWhat is meant by a chemical bond? Why do atoms form bonds with each other? Why do some elements exist as molecules in nature instead of as free atoms?arrow_forwardFor three simple molecules of your own choice, apply the rules for writing Lewis structures. Write your discussion as if you are explaining the method to someone who is not familiar with Lewis structures.arrow_forward
- c) Explain which would have the lowest second ionization energy. Explain which species in each of the following pairs would have the greater electronegativity. a. lithium or nitrogen b. sulfur or selenium Consider the following table of ionization energies in kJ/mole. Element 1st 2nd 3rd 4th 5th 6th Na 496 4562 6912 9544 13353 16610 738 1451 7733 Mg Al 10540 13630 17995 18378 578 1817 2745 11577 14831 Si 786 1577 3232 4356 16091 19785 P 1012 1903 2912 4957 6274 21269 a. Explain why the first ionization energy generally increases as one goes down the group of elements listed above. b. Explain why for a particular element , the second ionization energy is greater than the first jonization energy, the third is greater than the second etc. c. Explain why Mg has a higher first ionization energy than does Na, but a lower second ionization energy than does Na. d. Explain why for aluminum there is a large increase in ionization from 3rd to 4tharrow_forwardWhy does the octet rule not apply to transition metals? a. the octet rule does apply to transition metals as they are all classified as metals b. transition metals do not form cations or anions c. most transition elements form ions with more than one positive charge d. transition elements cannot be assigned with charges to form ions What do you call the process of positive and negative ions of an ionic compound separating from each other when solubilized in water? a. dissociation b. solubilization c. differentiation d. precipitation Which of the following statements is considered true? a. The size of an atom is determined by the size of the outermost occupied orbital b. Higher ionization energy means that the electron is more difficult to remove c. both are correct d. both are incorrectarrow_forwardDraw Lewis structures for each atom, assigning the correct number of valence electrons and the correct charges. a. Na + Cl NaClb. Zn + O ZnOc. Mg + 2I IMgIarrow_forward
- 1. Draw Lewis Structures (including resonance structures if applicable) for the following molecules/ions: A. NO3– B. NO2– C. NO2+ D. O3 2. Which of the following items in Number 1 are isoelectronic?arrow_forwardWhich is the correct number of electrons in the Lewis structure for NH3 A. zero B.one C.four D.eightarrow_forwardchalcogen 10. It is a measure of how equally the electrons in a bond are distributed between the two atoms involved in a covalent bond. A polarity B. octet rule C. ionization energy D. electron affinityarrow_forward
- Write Lewis structures that obey the octet rule for each of the following. a. HCN b. PH3 c. CHCl3 d. NH4+ e. H2CO f. SeF2 g. CO2 h. O2 i. HBr Except for HCN and H2CO, the first atom listed is the central atom. For HCN and H2CO , carbon is the central atom.arrow_forwardIn drawing Lewis structures what does octet rule mean? O a. atoms lose electrons until they have only 8 electrons left O b. atoms are stable if they have 8 p electrons OC. Atoms are the most stable if they have 8 valence electronsarrow_forward2. Avogadro does not "waste" his time drawing a Lewis structure before determining the shape of PF3. He thinks that the shape of PF3 must be trigonal planar because there are three fluorine atoms bonded to the central phosphorus atom. a. Draw the Lewis structure for PF3. b. Was Avogadro's answer for the shape of a PF3 molecule correct? Explain c. Why is it important to draw the Lewis structure for a molecule before identifying the shape of the molecule?arrow_forward
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