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 therefore, they distribute themselves in positions around the central atoms that are as far away from one another. This arrangement of electron pairs is known as electron-pair geometry. The electron pairs may be shared in covalent bond, or they may be lone pairs.
Answer to Problem 19E
The Lewis diagrams for
The wedge-and-dash diagrams for
The electron pair geometry for
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,
In the molecule,
The atom which is least electronegative is the central atom. In
Figure 1
In
Figure 2
In
Figure 3
The electron-pair geometry depends on the number of electron pairs around the central atoms. In the molecule
In the molecule
In the molecule
The wedge-and-dash diagram for the molecule
Figure 4
The wedge-and-dash diagram for the molecules
Figure 5
The wedge-and-dash diagram for the molecules
Figure 6
The Lewis and wedge-and-dash diagrams for
(b)
Interpretation:
The molecular geometry predicted 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.
Answer to Problem 19E
The Lewis diagrams for
The wedge-and-dash diagrams for
The molecular geometry for
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,
In the molecule,
The atom which is least electronegative is the central atom. In
Figure 1
In
Figure 2
In
Figure 3
The molecular geometry depends on the number of electron pairs as well as number of unpaired electron on the central atoms. In the molecule
In the molecule
In the molecule
The wedge-and-dash diagram for the molecule
Figure 4
The wedge-and-dash diagram for the molecule
Figure 5
The wedge-and-dash diagram for the molecule
Figure 6
The Lewis and wedge-and-dash diagrams for
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Chapter 13 Solutions
Introductory Chemistry: An Active Learning Approach
- Which statements are true about electronegativity? (a) Electronegativity increases from left to right in a period of the Periodic Table. (b) Electronegativity increases from top to bottom in a column of the Periodic Table. (c) Hydrogen, the element with the lowest atomic number, has the smallest electronegativity. (d) The higher the atomic number of an element, the greater its electronegativity.arrow_forwardAnswer the questions in the table below about the shape of the bromine pentafluoride (BrF, molecule. How many electron groups are around the central bromine 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 bromine atom? (You may need to use the scrollbar to see all the choices.) (choose one)arrow_forwardQUESTION 5 Determine which compound should have a(n) linear 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 H3O+ B ClF2+ C IF2- D AsF5arrow_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_forwardMany organic compounds belong to a category of molecules called "hydrocarbons", meaning that they only contain hydrogen and carbons. An example of a simple hydrocarbon is shown below. Considering both the VSEPR shape of the molecule and electronegativity values of the elements and state whether you expect this simple hydrocarbon to be polar or nonpolar. Explain your answer. нн H-C-C-H ннarrow_forwardWrite 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_forward
- Answer the questions in the table below about the shape of the phosgene (COCI,) molecule. How many electron groups are around the central carbon 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 carbon atom? (You may need to use the scrollbar to see all the choices.) (choose one)arrow_forwardUse Lewis theory to determine the formula for the compound that forms between each of the following pairs of elements. Ca and I Express your answer as a chemical formula. Na and Se Express your answer as a chemical formula. Al and O Express your answer as a chemical formula.arrow_forwardQuestion 18 of 55 Draw the Lewis structure of HCIO, (by following the octet rule on all atoms) and then choose the appropriate pair of molecular geometries of the two central atoms. Your answer choice is independent of the orientation of your drawn structure. CI-O :0: H A) linear/planar B) pyramidal/trigonal pyramidal C) trigonal pyramidal / bent (109.5°) D) linear/trigonal E) bent (109.5%) / linear Click to edit molecule Submearrow_forward
- Use Lewis theory to determine the formula for the compound that forms between each of the following pairs of elements. Ca and Te Express your answer as a chemical formula. Mg and Br Express your answer as a chemical formula. Na and S Express your answer as a chemical formula. In and O Express your answer as a chemical formula.arrow_forwardDraw a Lewis structure for the following ions/molecules, including any resonance structures and/or formal charges. Place a box around any contributing resonance structures XeO4^-2, BrF5, CHF2CL What is the electron group geometry around the central atom for each of the above ions/molecules? For the above ions/molecules, what is the shape of the entire molecule/ion of the entire ion/molecule? Identify polar bonds with dipole arrows Indicate whether each of the ions/molecules is POLAR or NON-POLARarrow_forwardWrite a Lewis structure for each of the following molecules. H2O2 Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.arrow_forward
- Introductory Chemistry: An Active Learning Approa...ChemistryISBN:9781305079250Author:Mark S. Cracolice, Ed PetersPublisher:Cengage LearningOrganic ChemistryChemistryISBN:9781305580350Author:William H. Brown, Brent L. Iverson, Eric Anslyn, Christopher S. FootePublisher:Cengage Learning