CHCl3 exist in liquid state due to:
Correct answer: A. Dipole-dipole and London dispersion forces
- A. Dipole-dipole and London dispersion forces
- B. Dipole induced dipole forces
- C. Dipole-dipole forces
- D. Hydrogen bonding
Explanation
Chloroform exhibits both dipole-dipole forces (between the positive end of one molecule and the negative end of another) due to its polar bonds, as well as London dispersion forces (van der Waals forces) due to temporary fluctuations in electron distribution. These combined forces contribute to its liquid state.
Report an error
The more specific you are, the faster it gets fixed. A source beats an opinion.
Prefer email? [email protected]
About Properties of Liquids
Liquid behavior depends on intermolecular forces, which produce surface tension, viscosity, capillary action and a definite volume without a fixed shape. The topic also covers vapor pressure, evaporation, boiling point and the effect of temperature and external pressure, while distinguishing evaporation at the surface from boiling throughout the liquid.
Practise Liquids
350 free Liquids MCQs from Chemistry, each with the correct answer and an explanation. Unlimited attempts, no account needed.
Discussion
Stuck on an option, or know a faster way to get there? Ask or explain it here.
No comments yet. Be the first to explain this one.
Exams that ask Chemistry questions like this
Chemistry is on 14 papers prepared for on TestUstad, and all of them draw the same bank, so this question is worth knowing for every one of them.
More Properties of Liquids questions
If N2 gas is bubbled through water at 20°C, how many ml (at STP) of N2 gas would dissolve in a litre of water? Partial pressure of N2 gas is equal to 742.5 torr and Hennery's law constant for it is 5.75 x 10^7 torr at 20°C.
Which of the following pairs is an example of completely immiscible liquids?
The density of liquids are _ than gases but _ to solids.
The highest boiling point among the following is for:
Liquids have no definite shape; it is because:
Strong dipole-dipole forces among the liquid molecules are responsible for: