The strongest intermolecular interactions between hydrogen fluoride (HF) molecules arise from A) dipole dipole forces B) hydroge
n bonding C) ion dipole interactions D) ionic bondsE) London dispersion forces
2 answers:
Answer:
The answers are: A) dipole-dipole forces and B) hydrogen bonding
Explanation:
Hydrogen bonds are a class of bond that form from the attraction between a hydrogen atom and an atom that has a negative charge. This attraction is known by the name of dipole-dipole interaction.
In this case, since the hydrogen atom has a low electronegativity and since the fluorine atom has a high electronegativity, therefore, between them there will be a positive charge on the hydrogen atom and a negative charge on the fluorine atom. . In this way, they will have hydrogen bonds between the hydrogen atom and the fluorine atom.
The attached figure shows the bonds.
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The given question is incomplete. The complete question is:
Calculate the number of moles and the mass of the solute in each of the following solution: 100.0 mL of 3.8 × 10−5 M NaCN, the minimum lethal concentration of sodium cyanide in blood serum
Answer: The number of moles and the mass of the solute are and
respectively
Explanation:
Molarity of a solution is defined as the number of moles of solute dissolved per liter of the solution.
where,
n = moles of solute
= volume of solution in ml
n = moles of =
Thus the number of moles and the mass of the solute are and
respectively