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intermolecular forces in nh3

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Answers:dispersion forces; ionic bonding; NaCl. hydrogen bonding dispersion forces; NH3. metallic bonding; dispersion forces; Fe. Explaination Three types of force can operate between covalent molecules: Dispersion Forces also known as London Forces (named after Fritz London who first described these forces theoretically 1930) or as Weak Intermolecular Forces or as van der Waal's Forces (namd after the person who contributed to our understanding of non-ideal gas behaviour). Dipole-dipole interactions Hydrogen bonds Relative strength of Intermolecular Forces: Intermolecular forces (dispersion forces, dipole-dipole interactions and hydrogen bonds) are much weaker than intramolecular forces (covalent bonds, ionic bonds or metallic bonds) dispersion forces are the weakest intermolecular force (one hundredth-one thousandth the strength of a covalent bond), hydrogen bonds are the strongest intermolecular force (about one-tenth the strength of a covalent bond). dispersion forces < dipole-dipole interactions < hydrogen bonds Dispersion Forces (London Forces, Weak Intermolecular Forces, van der Waal's Forces) are very weak forces of attraction between molecules resulting from: momentary dipoles occurring due to uneven electron distributions in neighbouring molecules as they approach one another the weak residual attraction of the nuclei in one molecule for the electrons in a neighbouring molecule. The more electrons that are present in the molecule, the stronger the dispersion forces will be. Dispersion forces are the only type of intermolecular force operating between non-polar molecules, for example, dispersion forces operate between hydrogen (H2) molecules, chlorine (Cl2) molecules, carbon dioxide (CO2) molecules, dinitrogen tetroxide (N2O4) molecules and methane (CH4) molecules.

Question:I need to predict which types of intermolecular forces would be on each of these molecules (dipole-dipole, hydrogen, or dispersion). 1. NH3 I thought it might be dipole-dipole, hydrogen, and dispersion, but I'm not sure if it is a polar molecule. 2. C3H4 I thought it would be all of them once again, but I'm not sure if it is polar or if it's hydrogen since it's bonded to carbon and not a halogen, nitrogen, oxygen, etc. Thanks for your help!

Answers:Hydrogen bonding occurs when you have hydrogen bonded to O,N, or F, which are very electronegative. The large difference between the electronegativity of hydrogen and O,N or F produces a highly polar covalent bond where H is partially positve and O, N or F is partially negatve. So now you have an electrostatic attraction between the partially positive hydrogen in one atom and the partially negative of the O,N or F in another molecule which makes a strong dipole dipole attraction called a hydrogen bond. That being said.... NH3 has hydrogen bonding. The second one is nonpolar, no hydrogen bonding since H is not bonded to O,N or F. So it is dispersion forces.

Question:I'm currently studying AS Chemistry and this topic is really confusing me: can someone please briefly explain permanent dipole-dipole, van der Waals and hydrogen bonding to me? also, i don't get how polar molecules (i.e. with permanent dipole-dipole forces can have van der Waals forces as well). someone please help!!! thanks!

Answers:ALL moleucles has weak van der Waals - it is a momentary elctron correlation dipole-dipole only in molecules like H2O, NH3 H-bond a sharing of a hydrogen between two molcules so that the H can "take" part of an electron

Question:What kind of intermolecular force helps make the fatty acid C9H16O2 soluble in oil? And also, what kind of intermolecular attraction exists between soap and biodiesel that accounts for high solubility?

Answers:you see, the inermolecular force helps the fatty acid to lose weight nd be thin , its goal is to reach a size C9H16O2 and by doing that , it puts oil on it self to make it easier for the terroist to get to. and what the soap does is, it actully cleans the oil and the blemishes for the pimples to be more clean and clearer.

From Youtube

Intermolecular Forces :A video demonstration and explination on one of the types of intermolecular force, hydrogen bonding.

Intermolecular Forces :Professor Mark Buntine revises important relevant info from the Bonding and Polarity videos, and then addresses the different types of intermolecular forces, including dispersion forces and dipole-dipole forces hydrogen bonding, ion-dipole interactions, and the physical attributes of these and other intermolecular forces. He also goes into detail regarding the properties one of our most important molecules: water.