Chemistry In Focus
6th Edition
ISBN: 9781305084476
Author: Tro, Nivaldo J., Neu, Don.
Publisher: Cengage Learning
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Question
Chapter 5, Problem 39E
Interpretation Introduction
Interpretation:
The effect of the structure of ozone on the amount of UV light hitting the earth is to be explained.
Concept Introduction:
Ozone is an atmospheric gas that absorbs UV light and thus, protects life on Earth from excessive UV exposure.
The reaction takes place as follows:
Ozone absorbs UV light and the oxygen-oxygen bond breaks.
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Part A - Describing o and Bonds in a Molecule
We have just arrived at a bonding description for the formaldehyde molecule. Which of the following statements about the molecule is or are true?
I. Two of the electrons in the molecule are used to make the T bond in the molecule,
II. Six of the electrons in the molecule are used to make the o bonds in the molecule
III. The C-O bond length in formaldehyde should be shorter than that in methanol, H3COH.
O Only one of the statements is true
O Statements I and II are true
O Statements I and III are true
O Statements II and III are true
O All three statements are true
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Chapter 5 Solutions
Chemistry In Focus
Ch. 5 - Drawing Lewis Structures for Ionic Compounds Draw...Ch. 5 - Using Lewis Structures to Determine the Correct...Ch. 5 - Prob. 5.3YTCh. 5 - Prob. 5.4YTCh. 5 - Drawing Lewis Structures for Covalent Compounds...Ch. 5 - Prob. 5.6YTCh. 5 - Prob. 5.7YTCh. 5 - Prob. 5.8YTCh. 5 - Prob. 5.9YTCh. 5 - Determining if a Molecule Is Polar Is SCl2 a polar...
Ch. 5 - Based on the Lewis structures for hydrogen and...Ch. 5 - Prob. 2SCCh. 5 - Prob. 3SCCh. 5 - Prob. 4SCCh. 5 - Prob. 5SCCh. 5 - Prob. 6SCCh. 5 - Prob. 7SCCh. 5 - Why is salt, NaCl, relatively harmless even though...Ch. 5 - If sodium is dropped into water, a loud fizzing...Ch. 5 - Explain ionic bonding according to Lewis theory.Ch. 5 - Prob. 4ECh. 5 - Prob. 5ECh. 5 - Prob. 6ECh. 5 - Draw electron dot structures for the following...Ch. 5 - Explain VSEPR theory. According to this theory,...Ch. 5 - Prob. 9ECh. 5 - Prob. 10ECh. 5 - In what ways is water unique? What about the water...Ch. 5 - What is the difference between a polar and a...Ch. 5 - Why do polar molecules have a greater tendency to...Ch. 5 - Prob. 14ECh. 5 - Lewis Structures for Atoms Draw Lewis structures...Ch. 5 - Draw Lewis structures for each of the following...Ch. 5 - Ionic Lewis Structures Draw a Lewis structure for...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Draw a Lewis structure for each of the following...Ch. 5 - Covalent Lewis Structures Draw a Lewis structure...Ch. 5 - Draw a Lewis structure for each molecular...Ch. 5 - General Lewis Structures Determine whether each...Ch. 5 - Determine whether each compound is ionic or...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - What is wrong with each Lewis structure? Fix the...Ch. 5 - Predicting the Shapes of Molecules Use VSEPR...Ch. 5 - Use VSEPR theory to determine the geometry of the...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - Draw a Lewis structure and use VSEPR theory to...Ch. 5 - CF2Cl2 is a chlorofluorocarbon implicated in ozone...Ch. 5 - Chlorofluorocarbons have been banned because they...Ch. 5 - Determining Molecular Polarity Determine whether...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Determine whether each molecule is polar:...Ch. 5 - Explain why water would be a gas at room...Ch. 5 - Prob. 38ECh. 5 - Prob. 39ECh. 5 - One of the observations that led G. N. Lewis to...Ch. 5 - G. N. Lewis developed a model for chemical bonding...Ch. 5 - The opening quote of this chapter states that Man...Ch. 5 - Draw a Lewis structure of the H2 molecule. If you...Ch. 5 - Prob. 44ECh. 5 - The Lewis structures for CH4,N2,andCO2, along with...Ch. 5 - CH3COCH3 (acetone) is a common laboratory solvent...
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- Complete a Lewis structure for the compound shown below, then answer the following questions. What are the predicted bond angles about the carbon and nitrogen atoms? How many lone pairs of electrons are present in the Lewis structure? How many double bonds are present?arrow_forwardescribe the type of bonding that exists in the Cl2(g)molecule. How does this type of bonding differ from that found in the HCl(g)molecule? How is it similar?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_forward
- 10.) The structural formula of a certain aldehyde (related to formaldehyde) is H3C-CH2-CHO. Draw a Lewis structure for this aldehyde and determine the number of bonds present. Note that a single or a double or a triple bond counts as one bond. Write the number, not the word.arrow_forwardHow does adding an atom affect the position and angles of existing atoms or lone pairs? How does adding a lone pair affect the position and angles of existing atoms and lone pairs? Is the effect of adding bonded atoms and lone pairs to the central similar? Explain your answer. Describe what is meant by the "Steric #". Explain the difference between the terms "Electron Geometry" and "Molecule Geometry". How does changing a bond to a double or triple bond affect the shape of the molecules? List the molecules in Part III where the real bond angles differ from the theoretical model values. Why do you think the values differ?arrow_forward- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 9. Na3P valence e = REDs = shape= bond angles = 10. AI(NO3)3 valence e = REDs = shape = bond angles = sodium phosphide aluminum nitrate For nitratearrow_forward
- - Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 6. OCI2 valence e = REDS = shape= bond angles = oxygen dichloride 7. P2S4 valence e = REDs at each central atom = shape at each central atom = bond angles = diphosphorus tetrasulfide dicarbon tetrachloride 8. C2C14 valence e = REDs at each central atom = shape at each central atom = bond angles =arrow_forward- Draw Lewis structures for each of the following. Give the total number of valence electrons, select from the lists the number of Regions of Electron Density (REDs) around the central atom, the molecular shape, and the bond angles. - Do not put covalent bonds between metals and nonmetals. - Put brackets around anions to show both charge and quantity REDS 0, no central atom 2 3 4 Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Angles 109.5° 120° 180° none, no central atom 1. H2CCI2 valence e = REDS = shape= bond angles = 2. NC13 valence e = REDs = shape= bond angles = 3. CS2 valence e = REDS = shape= bond angles = dihydrogen carbon dichloride nitrogen trichloride carbon disulfidearrow_forwardThe element vibranium (Vb) reacts with pandemonium (Pn) to generate a covalent PnVb4 molecule. If a pandemonium atom has 8 valence electrons and each vibranium atom has 7 valence electrons, draw the Lewis structure of PbVb4. What is the molecular geometry of the PbVb4 molecule? Pn is the central atom.arrow_forward
- Column I: Draw the best Lewis structure. Label any atoms with nonzero formal charge. Column II: List the total number of major resonance contributors and draw at least two (if they exist). Column III: How many electron groups are around the central atom? Column IV: What is the electron geometry? Column V: What is the molecular geometry? Possible answers: linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral, bent, trigonal pyramidal, see-saw, T-shaped, square pyramidal, square planar). Column VI: Give values of the bond angles around the central atom. (for example, 109.5°, less than 109.5°, 120°, less than 120°, etc.). Column VII: Give the hybridization of the central atom. Column VIII: State how many sigma bonds and pi bonds are present in the molecule or ion. Column IX: Is the molecule polar or non-polar?arrow_forward♥ Draw Lewis structures for each of the following. Use the DEN and the number of REDs around thecentral atom to select the type of bonds, the molecular shape, and type of molecule from the lists.♥ Do not put covalent bonds between metals and nonmetals♥ Put brackets around anions to show both charge and quantity.arrow_forwardStep 1 – Write the Lewis structure from the molecular formula.Step 2 – Assign an electron-group arrangement by counting all electron groups (bonding plus nonbonding) around the central atom (or around each centralatom, if more than one central atom in structure).Step 3 – Predict the ideal bond angle from the electron-group arrangement and the effect of any deviation caused by lone pairs or double bonds.Step 4 – Name the molecular shape by counting bonding groups and nonbonding groups separately.Step 5 – Predict whether the molecule is polar or nonpolarStep 6 – Describe the hybridization around the central atom and identify the total number of σ and π bonds in the structurearrow_forward
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Types of bonds; Author: Edspira;https://www.youtube.com/watch?v=Jj0V01Arebk;License: Standard YouTube License, CC-BY