Concept explainers
(a)
Interpretation:
The number and arrangement of electron pairs around the indicated atom in the given molecule are to be stated.
Concept Introduction:
The representation an element along with its valence electrons is referred to as Lewis symbol or Electron Dot Symbol. The Lewis structure exhibits the connection between atoms. Each dot around an atom represents electrons.
The geometry of molecule is determined by electron pair present around the central atom.
The formula to calculate the number of electron pairs in compound is,
Generally, the shape of the molecule will be linear if electron pairs are two and the shape of the molecule will be trigonal planar if electron pairs are
(b)
Interpretation:
The number and arrangement of electron pairs around the indicated atom in the given molecule are to be stated.
Concept Introduction:
The representation an element along with its valence electrons is referred to as Lewis symbol or Electron Dot Symbol. The Lewis structure exhibits the connection between atoms. Each dot around an atom represents electrons.
The geometry of molecule is determined by electron pair present around the central atom.
The formula to calculate the number of electron pairs in compound is,
Generally, the shape of the molecule will be linear if electron pairs are two and the shape of the molecule will be trigonal planar if electron pairs are
(c)
Interpretation:
The number and arrangement of electron pairs around the indicated atom in the given molecule are to be stated.
Concept Introduction:
The representation an element along with its valence electrons is referred to as Lewis symbol or Electron Dot Symbol. The Lewis structure exhibits the connection between atoms. Each dot around an atom represents electrons.
The geometry of molecule is determined by electron pair present around the central atom.
The formula to calculate the number of electron pairs in compound is,
Generally, the shape of the molecule will be linear if electron pairs are two and the shape of the molecule will be trigonal planar if electron pairs are
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Chapter 12 Solutions
Introductory Chemistry: A Foundation
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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_forwardBond Enthalpy When atoms of the hypothetical element X are placed together, they rapidly undergo reaction to form the X2 molecule: X(g)+X(g)X2(g) a Would you predict that this reaction is exothermic or endothermic? Explain. b Is the bond enthalpy of X2 a positive or a negative quantity? Why? c Suppose H for the reaction is 500 kJ/mol. Estimate the bond enthalpy of the X2 molecule. d Another hypothetical molecular compound, Y2(g), has a bond enthalpy of 750 kJ/mol, and the molecular compound XY(g) has a bond enthalpy of 1500 kJ/mol. Using bond enthalpy information, calculate H for the following reaction. X2(g)+Y2(g)2XY(g) e Given the following information, as well as the information previously presented, predict whether or not the hypothetical ionic compound AX is likely to form. In this compound, A forms the A+ cation, and X forms the X anion. Be sure to justify your answer. Reaction: A(g)+12X2(g)AX(s)The first ionization energy of A(g) is 400 kJ/mol. The electron affinity of X(g) is 525 kJ/mol. The lattice energy of AX(s) is 100 kJ/mol. f If you predicted that no ionic compound would form from the reaction in Part e, what minimum amount of AX(s) lattice energy might lead to compound formation?arrow_forwardIn Section 12.10 of your text, the term “effective pairs" is used. What does this mean?arrow_forward
- Draw the Lewis structure for a molecule of each of thesecompounds and ions.a. H 2 S c. S O 2b. B F 4 — d. SeC l 2arrow_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_forwardName the highlighted chemical group in each molecule. Lewis structure name of highlighted group н н Н — о С — Н н н н н H. С — Н - - - .. н н Н — N — н H н — С — с3 с н н н :0 : :0 :arrow_forward
- Name the highlighted chemical group in each molecule. Lewis structure name of highlighted group H olo Н— С —Н .. .. 0=C - N- H H н н Н— С —N: H H H H H Н— N— С — С— 0 H :0:arrow_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? 3. Draw the Lewis structure of ozone, O3. Describe why ozone has a bent shape instead of a linear shape.arrow_forward4. CHCl3 a. Lewis structure Electronic geometry_ C. d. Molecular shape_ e. Bond angle? b. Draw the different bonds and label their polarity. inorpelt b Soigns broff 02 8arrow_forward
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