In general, which is more polar, the stationary phase or the mobile phase?The stationary phase is always more polarThe mobile phase is always more polarIt depends on our choices for both stationary and mobile phaseTheir polarity doesn't really matter so we never consider it

Generally, in normal phase chromatography, stationary phases are usually more polar, while mobile…

Answered: In general, which is more polar, the…

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter6: Covalent Bonding

Section: Chapter Questions

Problem 40QRT: Acrolein is the starting material for certain plastics. (a) Which bonds in the molecule are polar...

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Similar questions

hat does it mean to say that a bond is polar? Give two examples of molecules with polar bonds. Indicate in your examples the direction of the polarity.
Successive substitution of F atoms for H atoms in the molecule CH4 produces the molecules CH3F, CH2F2, CHF3, and CF4. a. Draw Lewis structures for each of the five molecules. b. Using VSEPR theory, predict the geometry of each of the five molecules. c. Specify the polarity (polar or nonpolar) for each of the five molecules.
According to the VSEPR model, what are the arrangements of two, three, four, five, and six valence-shell electron pairs about an atom?
Which one of the following bonds is polar? a. a bond between two identical atoms b. a bond between two atoms with the same electronegativity c. a bond between two atoms with different electronegativities
Successive substitution of F atoms for H atoms in the molecule NH3 produces the molecules NH2F, NHF2, and NF3. a. Draw Lewis structures for each of the four molecules. b. Using VSEPR theory, predict the geometry of each of the four molecules. c. Specify the polarity (polar or nonpolar) for each of the four molecules.
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.
Identify the coordinate covalent bond(s) present, if any in each of the following molecules by listing the two atoms involved in the bond. Name the atom on the left or the bottom in the bond first.
Indicate whether each of the following triatomic molecules is polar or nonpolar. The molecular geometry is given in parentheses. a. ONBr (angular with N in the center position) b. OF2 (angular with O in the center position) c. SO2 (angular with S in the center position) d. H2S (angular with S in the center position)
Is the Cl2BBCl2 molecule polar or nonpolar?
Determining Molecular Polarity Determine whether each molecule is polar: a.HBrb.IClc.I2d.CO
7.30 The bond in HF is said to be polar, with the hydrogen carrying a partial positive charge. For this to be true, the hydrogen atom must have less than one electron around it. Yet the Lewis dot structure of HF attributes two electrons to hydrogen. Draw a picture of the electron density distribution for HF and use it to describe how the hydrogen atom can carry a partial positive charge. How can these two models of the HF bond (the electron density and the Lewis structure) seem so different and yet describe the same thing?
What is the most polar bond in the molecule?

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In general, which is more polar, the stationary phase or the mobile phase? The stationary phase is always more polar The mobile phase is always more polar It depends on our choices for both stationary and mobile phase Their polarity doesn't really matter so we never consider it