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London dispersion force occurs betwen all molecules but is the only intermolecular bond exhibited in NON polar molecules. since glucose (C6H12O6) is a polar molecule, the strongest force present is hydrogen bonding. hydrogen bonding occurse in between the hydrogen of one molecule and the oxygen, flourine, or nitrogen of another molecule.
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What are the intermolecular forces present in C2H5OH?
The intermolecular forces present in C2H5OH (ethanol) are hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
What are the intermolecular forces present in diethyl ether?
The intermolecular forces present in diethyl ether are primarily London dispersion forces and dipole-dipole interactions.
What intermolecular forces are present in cl2?
London forces are present in chlorine molecules.
How do the strengths of the intermolecular forces vary from CO2 to CS2 to CSe2?
Of CO2, CS2 and CSe2, CO2 is the smallest molecule whereas CSe2 is the largest molecule. The same pattern exists in the strength of the intermolecular forces. All three are linear, non polar molecules.
What intermolecular forces are present in SiF4?
In SiF4, the intermolecular forces present are London dispersion forces. These forces arise due to temporary fluctuations in electron distribution within the molecule, leading to weak attractions between neighboring molecules.
What are the intermolecular forces present in C2H5OH?
The intermolecular forces present in C2H5OH (ethanol) are hydrogen bonding, dipole-dipole interactions, and London dispersion forces.
What are the intermolecular forces present in diethyl ether?
The intermolecular forces present in diethyl ether are primarily London dispersion forces and dipole-dipole interactions.
What intermolecular forces are present in cl2?
London forces are present in chlorine molecules.
What kind of intermolecular forces present in Ar?
Dipole forces and London forces are present between these molecules.
How do the strengths of the intermolecular forces vary from CO2 to CS2 to CSe2?
Of CO2, CS2 and CSe2, CO2 is the smallest molecule whereas CSe2 is the largest molecule. The same pattern exists in the strength of the intermolecular forces. All three are linear, non polar molecules.
What intermolecular forces are present in SiF4?
In SiF4, the intermolecular forces present are London dispersion forces. These forces arise due to temporary fluctuations in electron distribution within the molecule, leading to weak attractions between neighboring molecules.
What substances would exhibit dipole-dipole intermolecular force bcl2 cf4 co2 cl2 nh3?
BCl3 and NH3 would exhibit dipole-dipole intermolecular forces, as they have polar bonds. CF4, CO2, and Cl2 would not exhibit dipole-dipole forces, as they are nonpolar molecules.
What is the intermolecular forces present in C3H8?
The only intermolecular forces in this long hydrocarbon will be dispersion forces.
What intermolecular forces are present in a molecule with no dipoles?
Van der Waals forces, specifically London dispersion forces, would be present in a molecule with no dipoles.
What are the intermolecular forces present in HI?
The intermolecular forces present in hydrogen iodide (HI) are dipole-dipole interactions and London dispersion forces. Hydrogen bonding is not a significant interaction in HI due to the large size of the iodine atom.
What is the stronger intermolecular force between CO2 and COS?
The stronger intermolecular force between CO2 (carbon dioxide) and COS (carbonyl sulfide) is found in COS. While CO2 is a nonpolar molecule and primarily exhibits London dispersion forces, COS is polar and can engage in dipole-dipole interactions in addition to dispersion forces. The presence of a polar bond in COS contributes to stronger intermolecular attractions compared to the nonpolar CO2.
How can one determine the strongest intermolecular force present in a substance?
To determine the strongest intermolecular force in a substance, you need to consider the types of molecules present. Look for hydrogen bonding, which is the strongest intermolecular force. If hydrogen bonding is not present, then consider dipole-dipole interactions and London dispersion forces in determining the strength of intermolecular forces.
