Concept explainers
(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 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.
(b)
Interpretation:
The molecular geometry prdicted by the valence shell electron-pair repulsion theory for each carbon atom in 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
- 1) The question screenshot has been attached down below answer step-by-step.arrow_forward< Complete the following structural formula for a neutral molecule by adding H atoms to complete the valence of each atom. Do not introduce any double or triple bonds. Then complete the Lewis diagram by adding any unshared electron pairs needed, so that each atom except H has a complete octet. [Review Topics] [References] Use the References to access important values if needed for this question. Br Br C—C— Write the molecular formula in the order CHX, where X stands for Cl or Br. Submit Answer The number of unshared pairs in the Lewis diagram unshared pair(s). Retry Entire Group 9 more group attempts remaining Previous Email Instructor Next Save and Earrow_forwardQuestion 14 of 28 A 0.02842 g sample of gas occupies 10.0 mL at 292.5 K and 1.10 atm. Upon further analysis, the compound is found to be 38.734% C and 61.266% F. What is the molecular formula of the compound? Draw the Lewis structure of the compound. molecular formula: Select Draw Rings More Erase / 切CBEGarrow_forward
- Question attachedarrow_forwardHow would you do this I’m stuck on the structurearrow_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. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar Ionic 5. C2Cl2 valence e-1 = shape= type of bonds = type of molecule = 6. AICI3 valence e-1 for one Cl-1 = shape= type of bonds = type of molecule = 7. K3PO3 valence e-1 = shape= type of bonds = type of molecule = 8. KH2PO3 valence e-1 = shape at the P= type of bonds = type of molecule = dicarbon dichloride aluminum chloride potassium phosphite potassium dihydrogen phosphitearrow_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. Shapes tetrahedral pyramidal bent trigonal planar linear diatomic monatomic ions Bond Types nonpolar covalent polar covalent nonpolar & polar covalent ionic ionic & covalent Type of molecule Nonpolar Polar lonic 1. HCC13 valence e-1 = shape= type of bonds = type of molecule = 2. SCI2 valence e-1 = shape= type of bonds = type of molecule = 3. P204 valence e-1 = shape= type of bonds = type of molecule = 4. N2O4 valence e-1 = shape= type of bonds = type of molecule = hydrogen carbon trichloride sulfur dichloride diphosphorus tetroxide dinitrogen tetroxidearrow_forwardClassify each of the following statements as true or false: a Molecular geometry around an atom may or may not be the same as electron-pair geometry around the atom. b Electron pair geometry is the direct effect of molecular geometry. c If the geometry of a molecule is linear, the molecule must have at least one double bond. d A molecule with a double bond cannot have trigonal pyramidal geometry around the double bonded atom. e A CO2 molecule is linear, but an SO2 molecule is bent. f A molecule is polar if it contains polar bonds. g A molecule with a central atom that has one lone pair of electrons is always polar. h A molecule with a central atom that has two lone pairs and two bonded pairs of electrons is always polar. i Carbon atoms normally form four bonds. j Hydrogen atoms never form double bonds.arrow_forwardMany free radicals combine to form molecules that do not contain any unpaired electrons. The driving force for the radical-radical combination reaction is the formation of a new electron-pair bond. Consider the formation of hydrogen peroxide. 2 OH(g) - H,O,(g) Write Lewis formulas for the reactant and product species in the chemical equation. Include nonbonding electrons. OH(g) H,O,(g) H H. : 0 H Question Source: MRG - General Chem about us privacy policy terms of use help contact us careers : :arrow_forward
- Write a correct Lewis structure for carbon monoxide.arrow_forwardPlease make a table with the answers.arrow_forwardDraw a Lewis structure that obeys the octet rule for each of the following ions. Assign formal charges to each atom. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all lone pairs of electrons. ClO3-arrow_forward
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