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Is CH4 a non polar molecule?
Yes.
Is ch4 bond a polar or non polar bond?
the molecule is non-polar the CH bonds are also non-polar
What type of molecular force is CH4?
It is a non polar compound.So it has london forces
Is CH4 non polar covalent bond?
Yes, CH4 has nonpolar covalent bonds because it consists of identical atoms (hydrogen and carbon) with similar electronegativities. In CH4, the electrons are shared equally between the carbon and hydrogen atoms, leading to a symmetrical distribution of charge and a nonpolar molecule.
Is ch4 molecule polar?
No. CH4 is nonpolar.
Is CH4 bond polar?
No, the CH4 molecule does not have a polar covalent bond because the carbon-hydrogen bonds are nonpolar. Since the four hydrogen atoms are symmetrically arranged around the central carbon atom, the molecule has a symmetrical shape and the individual bond dipoles cancel each other out.
Is CH4 a covelant or ionic Bond?
CH4 is a covalent compound.It is non polar
Does ch4 dissolev in water?
CH4 is non polar and water is polar.So they do not mix up
Does ch4 have London dispersion?
Yes, CH4 (methane) does exhibit London dispersion forces due to temporary fluctuations in electron distribution around the molecule. These dispersion forces are the weakest intermolecular forces and are responsible for the non-polar nature of methane.
Is CH4 symmetrical or not?
CH4, also known as methane, is a symmetrical molecule. It has a tetrahedral molecular geometry with carbon at the center and four hydrogen atoms arranged symmetrically around it.
Are NH3 and CH4 soluble in each other?
Ammonia (NH3) and methane (CH4) are not soluble in each other because they are both nonpolar molecules. Nonpolar molecules like these do not mix well with polar molecules like water, which is needed for molecules to dissolve in each other.
What is the intermolecular forces in compound ch4?
The intermolecular forces in CH4 (methane) are London dispersion forces. Methane molecules are non-polar, so the only type of intermolecular force present is the weak temporary dipole-induced dipole interactions between molecules.
