What is the predominant intermolecular force in the liquid state of each of these compounds: water (h2o), carbon tetrabromide (cbr4), and dichloromethane (ch2cl2)? drag the appropriate items to their respective bins. view available hint(s) dipole-dipole forces hydrogen bonding dispersion forces

Explanation:

It shows , Hydrogen bonding , Since ,

The molecule of water have a strong electronegative atom of oxygen and a hydrogen atom ,

So , the electronegative oxygen atom can interact with the other hydrogen atom of the other water molecule .

The molecule of Carbon tetrabromide have polar bonds of carbon and bromine atom , but overall the molecule is non - polar in nature , due to its tetraderal structure , hence ,

the molecule shows only dispersion forces .

The molecule of dichloromethane has Dipole Dipole forces due to difference in electronegativity between atoms .

answer; the numbers of valence electrons in the acetic acid molecule (ch3co2h) is 24;