(a)
Interpretation:
The electron-pair geometry for each carbon atom in
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 which are 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.
(b)
Interpretation:
The molecular geometry prdicted by the valence shell electron-pair repulsion theory for the molecule
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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Introductory Chemistry: An Active Learning Approach
- Use the Molecule Shape simulator (http://openstaxcollege.org/l/16MolecShape) to build amolecule. Starting with the central atom, click on the double bond to add one double bond. Then add one single bond and one lone pair. Rotate the molecule to observe the complete geometry. Name the electron group geometry and molecular structure and predict the bond angle. Then click the check boxes at the bottom and right of the simulator to check your answers.arrow_forwardHow would you do this I’m stuck on the structurearrow_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_forward
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- This is not a graded questionarrow_forwardPlease complete the following question fully. Question 3 This question is in regards to a molecule named CH4.arrow_forwardDraw a Lewis structure for the compound whose skeletal structure is provided to you below. Don't forget to draw in the H atoms! CH₂ HC CH 11 HC — CH, - Draw the Lewis structure by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons.arrow_forward
- Draw 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_forwardConvert the following Lewis structure for the nitrate ion into a line structure that includes the lone pairs. Why does the nitrate ion have a -1 charge?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_forward
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