For the following compounds: Draw the dot structure (please draw out all of the shells) Use an arrow to indicate electrons that are being transferred (or color-code the atom's electrons) a. b. C. Show the ionic bonds d. Indicate which is the cation and which is the anion. Lithium + Fluorine Magnesium + Oxygen

For the following compounds: Draw the dot structure (please draw out all of the shells) Use an arrow to indicate electrons that are being transferred (or color-code the atom's electrons) a. b. C. Show the ionic bonds d. Indicate which is the cation and which is the anion. Lithium + Fluorine Magnesium + Oxygen

Introductory Chemistry: An Active Learning Approach

6th Edition

ISBN:9781305079250

Author:Mark S. Cracolice, Ed Peters

Publisher:Mark S. Cracolice, Ed Peters

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 45E

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In a covalent bond between two atoms, the more electronegative atom will attract more electron density toward itself, causing a polar bond. The more electronegative element is the negative pole, whereas the less electronegative element is the positive pole. The direction of the dipole is always toward the more electronegative element. This is often inflicated by an arrow, as shown in the figure. (Figure 1) The magnitude of the bond polarity is the difference in electronegativity values of the atoms. For example, in the molecule Cl2, the CICI bond is nonpolar because there is no difference in electronegativity between two atoms of the same element. In the CIBr molecule, However, the C1 Br bond is polar because Cl and Br have different electroneaativitv values. A CI I bond would be more polar than a C1 Br bond because there is a greater electronegativity difference between Cland I than between CI and Br.
Part c draw the molecule by placing atoms on the grid and connecting them with bonds include all hydrogen atoms
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CH3COCH3 (acetone) is a common laboratory solvent that is often used in nail polish remover. Its Lewis structure and space-filling molecular image are shown here: Acetone is a polar molecule; the oxygen end has a slightly negative charge (oxygen is more electronegative), whereas the carbon and hydrogen end has a slightly positive charge. In liquid acetone, the molecules are attracted to each other via these polar ends-the positive end of one molecule is attracted to the negative end of its neighbor-and therefore align as shown here: Draw a Lewis structure and space-filling molecular image for CH2Cl2 (dichloromethane), another common laboratory solvent. Is the molecule polar? Which end of the molecule has a slightly negative charge? Which end has a slightly positive charge? Draw several space-filling molecular images of CH2Cl2 showing how they align in liquid dichloromethane.
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use differences in electronegativity to account for certain properties of bonds. What if all atoms had the same electronegativity values? How would bonding between atoms be affected? What are some differences we would notice?
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