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3 years ago

What intermolecular forces are present in each of the substances?

2 answers:

4 0

What intermolecular forces are present in each of the substances? CH4,C3H8,CH3F,HF, C6H5OH (dispersion forces<span>, </span>dipole-dipole forces<span>, or </span>hydrogen bonding<span>);A sample of ideal gas at room temperature occupies a volume of 34.0L at a pressure of 782torr .</span>

pochemuha3 years ago

3 0

What intermolecular forces are present in each of the substances? (1) Chloroform, CHCl3, (2)Oxygen, O2, (3)Polyethylene, CnH2n+2, and (4)Methanol, CH3OH.

<h3>Explanation: </h3>

Intermolecular forces are the forces that mediate interaction between molecules including forces of attraction or repulsion act between molecules and other types of neighboring particles, atoms or ions. The four intermolecular forces are: Ionic bonds, Hydrogen bonding, Van der Waals dipole-dipole interactions, Van der Waals dispersion force. The characteristics are Ionic bonds > Hydrogen bonding > Van der Waals dipole-dipole interactions > Van der Waals dispersion force

An ionic bond is chemical bond type where one or more electrons are transferred from one atom to another. Hydrogen bond is attractive (dipole-dipole) interaction between an electronegative atom and a hydrogen atom bonded to another electronegative atom. Whereas Van der Waals is distance-dependent interaction between atoms or molecules. There are two kinds of Van der Waals forces: weak London Dispersion Forces and stronger dipole-dipole forces.

(1) Chloroform, CHCl3, are intermolecular forces that present in each of the substances
(1) Chloroform, CHCl3: Dipole-dipole intermolecular forces are most important.
(2)Oxygen, O2: London dispersion forces are most important.
(3)Polyethylene, CnH2n+2: London dispersion forces are most important.
(4)Methanol, CH3OH: Dipole-dipole intermolecular forces and hydrogen bounds are important

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Bob measured out 1.60 grams of sodium. He calculates that 1.60 g of

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Explanation:

Step 1: Given data

Bob measured out 1.60 g of Na. He forms NaCl according to the following equation.

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Step 2: Calculate the percent yield.

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