Side by side dot structures of two water moleculs are given below. Draw structures like that on your paper. Put partial positive and partial negative charges where appropriate. Show two hydrogen bonds by connecting the partial positive charge on one molecule to the partial negaive charge on the other molecule using a dotted line. Upload your answer here. H-O-H H-O-H

Side by side dot structures of two water moleculs are given below. Draw structures like that on your paper. Put partial positive and partial negative charges where appropriate. Show two hydrogen bonds by connecting the partial positive charge on one molecule to the partial negaive charge on the other molecule using a dotted line. Upload your answer here. H-O-H H-O-H

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Draw resonance formulas for this molecule. Clearly indicate where any delta negative and delta positive charges should go.
Use the notes on the green page to help. Use CER, Claim-answer to the question, reasoning-why its drawn correctly, evidence- to show why the others are incorrect. Answer completely.
Use the following information to determine the Lewis structure, find the electron and molecular geometry of the molecule, determine the angle of the molecule, and determine the polarity. If the atoms are not the same, you may assume that the difference in their electronegativities are between 0.4 and 2.0. Atom information: A: 6 valence electrons, CANNOT exceed the octet. Further from fluorine on the periodic table than X. X: 6 valence electrons, CANNOT exceed the octet. Closer to fluorine on the periodic table than A. Molecule: AX,2- Electron Geometry: [Select] Molecular Geometry: [Select ] Bond Angle: [ Select] Polarity: [Select]
Please send the answer by typing only. I don't want handwritten.
Arrange the elements in the chart above in order of increasing electronegativity. Place the element with the LOWEST electronegativity value at the beginning of your list.
Please answer them. Thanks!
CONCEPT MAPPING Marvin started a concept map to demonstrate the properties of water. He lost the map on campus, but luckily you found it. Save the day and complete his map. You'll notice that in the bottom left the document says "paste drawing here." As part of this task, you will be creating a drawing of a molecule of water. Be sure to label the molecule with the types of atoms and the charges that make this molecule polar. ?????
Can u explain this one with an answer thank you
Write the electron dot structure for hydroxide ion, [OH]-a. What is the total number of available valence electrons?______Remember that hydroxide has a -1 charge, so an extra valence electron must be added to the total.b. In the space below, arrange the atomic symbols, then add bonding electron pairs. Distribute non-bonding electron pairs. Don’t forget to indicate the charge on the finished structure.
For the following molecule, indicate the positive and negative ends of the dipole, using the symbol →→→→→→→. Refer to a table of the Pauling electronegativity scale as needed. Select the single best answer. CO The arrow points to the left. The arrow points to the right.
Following is a molecule with polar bonds whose shape was obtained using the VSEPR theory. Specify the molecular shape of this molecule, and whether the molecule is polar or nonpolar. (Hint: In terms of polarity, see whether the dipoles in the molecule cancel or not. A molecule containing polar bonds can be nanpolar if the dipoles cancel each other. You can imagine the dipoles as ropes pulling on the central atom–If the pulls cancel each other, that is, the central atom cannot move, then the molecule is nonpolar. If on the other hand the opposite is true, then the molecule is polar.) O trigonal pyramidal shape, nonpolar O trigonal planar shape, nonpolar O tetrahedral shape, polar O trigonal pyramidal shape, polar O trigonal planar shape, polar
Draw the attraction between a water molecule and a molecule of NF3 First, draw one molecule and add the partial charges where needed - use the ΔEN to determine the types of bonds. Then, draw the second molecule so that the δ+ on one molecule lines up across from the δ- on the other. Since we can't draw the molecules here you will answer questions about the drawings that you made on the homework worksheet. NF3 has ____________ bonds with a ΔEN = ____________ . NF3 has 4 REDs and is symmetrical/asymmetrical (answer is ________ ) making it a polar/nonpolar (answer is __________ ) molecule. Each F has a ______________ charge and the N has a ________ charge. H2O has 2 ___________ bonds with a ΔEN = ___________ . H2O has 4 REDs and is symmetrical/asymmetrical (answer is ___________ . ) making it a polar/nonpolar (answer is _________ ) molecule. Each H has a _____________ charge and the O has a ____________ charge. The strongest possible attractive force between these two…