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Concept explainers
(a)
Interpretation:
The electron-pair geometry for the molecules,
Concept introduction:
The electron pairs in Lewis diagrams repel each other in real molecule and thus they distribute themselves in positions around the central atoms that are as far away from one another. This arrangement of electron pairs is called electron-pair geometry. The electron pairs may be shared in covalent bond, or they may be lone pairs.
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Answer to Problem 22E
The Lewis diagrams for
and
The wedge-and-dash diagrams for
and
The electron pair geometry for both molecules is tetrahedral.
Explanation of Solution
To write the Lewis diagram for a compound first the number of valence electrons is to be calculated. In the molecule,
Similarly, in the molecule,
The atom which is least electronegative is the central atom. In
Figure 1
In
Figure 2
The electron-pair geometry depends on the number of electron pairs around the central atoms. In both the molecules
The wedge-and-dash diagram for the molecules
Figure 3
The wedge-and-dash diagram for the molecules
Figure 4
The Lewis and wedge-and-dash diagrams for
(b)
Interpretation:
The molecular geometry prdicted by the valence shell electron-pair repulsion theory for the molecules
Concept introduction:
Molecular geometry is the precise term that is used to describe the shape of molecules and arrangement of atoms around the central atom. The molecular geometry of a molecule is predicted by valence shell electron-pair repulsion theory or in short VSEPR theory. VSEPR theory applies to substances in which a second period element is bonded to two, three, four, or other atoms.
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Answer to Problem 22E
The Lewis diagrams for
and
The wedge-and-dash diagrams for
and
The molecular geometry for both molecules is trygonal pyramidal.
Explanation of Solution
To write the Lewis diagram for a compound first the number of valence electrons is to be calculated. In the molecule,
Similarly, in the molecule,
The atom which is least electronegative is the central atom. In
Figure 1
In
Figure 2
The molecular geometry depends on the number of electron pairs around the central atoms and the number of lone pairs present on the central atom. In the both of the molecules,
The wedge-and-dash diagram for the molecules
Figure 3
The wedge-and-dash diagram for the molecules
Figure 4
The Lewis and wedge-and-dash diagrams for
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Chapter 13 Solutions
Introductory Chemistry: An Active Learning Approach
- Answer the questions in the table below about the shape of the perchlorate (CIO,) anion. How many electron groups are around the central chlorine atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central chlorine atom? (You may need to use the scrollbar to see all the choices.) (choose one)arrow_forwardQUESTION 4 Give the molecular geometry and number of electron groups for BrF5. square planar, 6 electron groups T-shaped, 5 electron groups seesaw, 5 electron groups octahedral, 6 electron groups O square pyramidal, 6 electron groups QUESTION 5 Place the following in order of decreasing X-A-X bond angle, where A represents the central atom and X represents the in each molecule. CS₂ CF4 O CS2 > CF4> SC12 CF4 > SC12 > CS2 CF4> CS2 > SC1₂ ⒸCS₂ = SC12 > CF4 SC12 > CF4 > CS₂ QUESTION 6 How many of the following molecules are polar? KrBr2 SC³6 OCCl2 PBr5 2 00000 0 01 SC1₂arrow_forwardQUESTION 4 Determine which compound should have a(n) trigonal pyramidal molecular geometry. Key Concept: Lewis structures are drawn from a knowledge of the total number of electrons from all the atoms involved in the structure. The element with the lowest electronegativity is the central atom. Fulfill octet of outside atoms first. Molecular shape depends upon the number of atoms and lone pair electrons around the central atom. A BrCl3 B IF4+ C BCl3 D NCl3arrow_forward
- Write the Lewis structure for the following molecule. State the electronic structure (shape based on electron pairs or bonds) AND the geometric structure (shape based on the atoms only). Include all valence electrons in your structure. State how many electrons are used to form covalent bonds in the molecule. Is the molecule polar? O2arrow_forwardAnswer the questions in the table below about the shape of the sulfur hexabromide (SBr) molecule. How many electron groups are around the central sulfur atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central sulfur atom? (You may need to use the scrollbar to see all the choices.) (choose one) X Ś Um 0 Garrow_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
- NO3 Sketch the proper Lewis structure for this substance. Be sure to follow octet/duet rules for each atom and use the total number of valence electrons available. Use your drawing to answer the following questions. Count the total number of electron domains surrounding the central atom. Enter the value only. Enter the name corresponding to the electron domain geometry. Choices are: linear, trigonal planar, or tetrahedral. Enter the name corresponding to the molecular geometry. Choices are: linear, trigonal planar, tetrahedral, bent, or trigonal pyramidal. Predict the bond angle. Enter the value without units. Use a "<" if needed.arrow_forwardAnswer the questions in the table below about the shape of the phosphorus trifluoride (PF3) molecule. How many electron groups are around the central phosphorus atom? Note: one "electron group" means one lone pair, one single bond, one double bond, or one triple bond. What phrase best describes the arrangement of these electron groups around the central phosphorus atom? (You may need to use the scrollbar to see all the choices.) (choose one) X Śarrow_forwardFor the molecule CHCl3, draw its Lewis Structure and then answer the following questions based on that structure. (The central atom in each case is the atom with the lowest electronegativity). How many valence electrons are in the molecule? (Remember to add an electron for each negative charge or to subtract one for each positive charge). How many lone pairs of electrons are in the central atom of the molecule? What is the electron pair geometry of the molecule? Tetrahedral Octahedral Triangular planar Trigonal Pyramidal Which of these structures could represent the three dimensional molecular shape of the molecule CHCl3? (Rotate the structures to perceive 3D shape. Pay attention to the angles!) What is (are) the bond angle(s) at the central atom of the molecule CHCl3? 104.5° 109.5° 90° 180° Would the molecule's structure be polar, nonpolar, or ionic? polar nonpolar ionicarrow_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_forward
- General, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage Learning
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