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a.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
b.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
c.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
d.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
e.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
f.
To determine:
The attractive forces present in the given compound.
Concept introduction:
The type of attractive forces relies upon the type of functional group and atoms of the molecule. London forces, ionic attractions, dipole-dipole attractions and hydrogen bonding are the main attractive forces present in pure compounds. Out of these forces, dispersion forces are the weakest forces present in almost all compounds and hydrogen bonding is stronger than dipole-dipole attractions.
The presence of opposite and equal charges lead to the formation of ionic attractions. The molecules that are polar in nature possess dipole-dipole attractions due to the presence of dipoles. Hydrogen bonding occurs in a molecule if hydrogen atom is attached with more electronegative atom.
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Chapter 7 Solutions
EBK GENERAL, ORGANIC, AND BIOLOGICAL CH
- List the major intermolecular forces of attraction (IMFs) which exists for the following molecules: A. NH3B. C2H6C. CO2arrow_forwardSelect the compound with the lowest freezing point: a. SnH4 b. They all have the same freezing point. c. SiH4 d. GeH4 e. CH4arrow_forwardThere are five pure substances. The molecular component is shown per substance. Based on this information, answer items 56 to 65. Substance Molecular Component Substance Molecular Component O Substance A Substance D Substance B Substance E Substance C OH 56. The physical properties of the substances are influenced by intermolecular forces of attraction. Which substance(s) are predominantly influenced by the intermolecular association of the molecules via hydrogen bonding? A. Substance A only B. Substance A and C C. Substance A, B, and C D. Substance A, B, C, and D 57. Which substance is expected to turn blue litmus paper into red color? A. Substance A B. Substance B C. Substance C D. Substance D OH Harrow_forward
- When LiCl dissolves in water, aqueous Li+ and Cl- ions result. The force of attraction that exist between Cl- and H2O is called a ____ interaction. a. ion-dipole b. ion-ion c.dipole-dipole d. london dispersion forces.arrow_forward34. What is the property of water which makes it possible for autoionization of water? O a. Ambidextrous b. Amphoteric c. Surface tension d. Liquid phase O O O Oarrow_forwardWhat kinds of attractive forces, including chemical bonds, would be present between the particles in: (d) BrCl(l ) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bonding (e) NaCl(s) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bonding (f) Na2SO4(s) a. dipole-dipole b. London forces c. covalent bonding d. H-bonding e. ionic bondingarrow_forward
- London forces are forces of attraction between what molecules. a. polar b. nonpolar c. slightly polararrow_forwardPOLAR molecules does not easily evaporate due to strong intermolecular force acting on it. * Determine if the CAPITALIZED WORD(S) make the statement correct. Choose TRUE if it does, choose FALSE if otherwise. A. TRUE B. FALSEarrow_forward1. sketch a few water molecules and label the polar covalent bonds and show where the hydrogen bonds are locatedarrow_forward
- Based off the molecular polarity of water, which of the following molecules would be soluble in water? A.glucose, carbon dioxide, ethanol B.glucose, methanol, and ethanol C.carbon dioxide, methane, methanolarrow_forward4. Air is 78% nitrogen. If the Henry's law constant for nitrogen is 7x10 4 molar/atm, what is the solubility of nitrogen in water at sea level where the air pressure is 1.00 atm? A. 2x104 M B. 3x10 M C. 4x104 M D. 5x10 4 M E. 6x10 4 Marrow_forward51. Molecular nitrogen (N2) is sparingly soluble in water due to a. dispersion forces. b. dipole-induced dipole forces. c. dipole-dipole forces d. hydrogen bonding.arrow_forward
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