Describe the intermolecular forces that must be overcome to convert each of the following from a liquid or solid to a gas.

so2, h2se

check all that apply.

a. ion-dipole bonding.
b. hydrogen-bonding.
c. london dispersion forces.
d. dipole-dipole bonding.

Answers

i just learnt this recently but i need to look through my notes again

8

explanation:

each principal energy level above the first contains one s orbital and three p orbitals. a set of three p orbitals, called the p sublevel, can hold a maximum of six electrons. therefore, the second level can contain a maximum of eight electrons - that is, two in the s orbital and 6 in the three p orbitals.

mark brainliest and have a great day!

SO₂ would require to overcome dipole-dipole bonding and London dispersion forces

H₂Se would require to overcome hydrogen-bonding

Explanation:

Both of these molecules are gaseous but are liquid under pressure

Ion-dipole bonding is present when there are ions present in the liquid. In both the cases, ions are not present hence this bonding is not present in the given molecules.

Hydrogen bonding is present in H₂Se, because there is a more electronegative element present than hydrogen. This develops partial charges on both the atoms and consequently attracts hydrogen atom of one molecule to the selenium atom of the other molecule.

London dispersion forces are present between all type of molecules, atoms and ions. These forces are weak but are dominant in molecules having large size. SO₂ is a large molecule so it will be dominant in it

Dipole-dipole bonding is present in molecules that have polar ends. SO₂ have polar ends, so this bonding will be present in it



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