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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Answer:
Phosphorus makes 5 bonds with other atoms
Explanation:
has total 32 number of valence electrons (P has 5 , O has 6 and Cl has 7 valence electrons).
These valence electrons are used to draw Lewis structure of .
Formal charge on an atom = (no. of valence electrons of the atom)-(no. of covalent bonds attached to the atom)-(no. of electrons in lone pair of the atom)
Applying octet rule (atoms have eight electrons in their valence shell) and minimizing formal charge of , it has been found that P makes total 5 bonds with rest of the atoms.
Lewis structure of along with formal charge (in parentheses) has been given below.
