Hydrogen bonding usually occurs between molecules that have a hydrogen atom bonded to either Fluorine, Oxygen or Nitrogen. So technically CH4 cannot hydrogen bond certainly not between it's own molecules. CH4 is methane, or natural gas. This makes CH4 have a lower boiling point. Hydrogen fluoride HF has the strongest hydrogen bonding.
Water H2O and ammonia NH3 have the next strongest hydrogen bonding. Hydrogen bonding is when their is an electromagnetic attraction between the polar molecules in hydrogen and another atom.
Yes it has hydrogen bonding because the Nitrogen has lone pairs and it is bonded to a Hydrogen atom. Yes, Hydrogen bonding is a hydrogen bonded to any Fluorine, Nitrogen or Oxygen. Asked By Curt Eichmann. Asked By Leland Grant.
Asked By Veronica Wilkinson. Asked By Daija Kreiger. Asked By Danika Abbott. Asked By Consuelo Hauck. Asked By Roslyn Walter. All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply. Ask Login. Elements and Compounds.
Asked by Wiki User.Hydrogen bonding is about the propensity of H: to donate some of that pair of electrons to an atom usually that is more electronegative usually because of the way it is bonded to other atoms. The C:H bond is almost non-polar so ther is little tendency for the H to donate electron density. BUT if the other atom is very strongly electronegative then yes, I believe CH4 can form hydrogen bonds. But in general this would be very unusual in the typical conditions we study so its not something you'd predict to happen at or close to lab STP.
I'm thinking cold ionized plasmas CL-2 and CH4 say Extreme conditions. No, Hydrogen only occurs when hydrogen is bonded to an Oxygen, Nitrogen, or Fluorine because they are so electronegative it creates a partially positive and partially negative charge on the two bond components allowing for hydrogen bonding. Can methane CH4 participate in hydrogen bonding, please xplain or copy a link or something i dont understand? Methane is already stable.
There is no valence electron left as carbon's four valence electron has been filled with 4 hydrogens. Somemore, Hydrogen bonding is only formed when there is a valence Hydrogen electrons and oxygen's valence electrons.
NO, Hydrogen bonding is the intermolecular force that exists between an H atom of one molecule and an electronegative atom N, O, or F of another molecule. Normally molecules hydrogen bond when they have lone pairs of electrons. Since methane does not have any lone pair electrons it does not hydrogen bond. Trending News. Lucille Ball's great-granddaughter dies at A warning sign for Trump at The Villages in Florida. Virginia health officials warn of venomous caterpillars.
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Answer Save. Favorite Answer. How do you think about the answers? You can sign in to vote the answer. This Site Might Help You.Because methane is a non-polar molecule it is not capable of hydrogen bonding or dipole-dipole intermolecular forces. The electronegativities of C and H are so close that C-H bonds are nonpolar.
There are no bond dipoles and no dipole-dipole interactions. Even if the molecule had polar C-H bonds, the symmetry of molecule would cause the bond dipoles to cancel. The molecule would still be nonpolar. It is a blob with no positive or negative ends.
In a nonpolar molecule, electrons are always moving. At any instant, they might be at one end of the molecule. This would instantaneously create a temporary dipole, making that end negative and the other end positive.
The positive charge attracts the electrons in an adjacent molecule. This temporary attractive force is the London dispersion force. Feb 28, Just London dispersion forces.
Ernest Z. The only intermolecular forces in methane are London dispersion forces. The major intermolecular forces would be dipole-dipole forces and London dispersion forces. The only forces left to consider are London dispersion forces. Related questions How do functional groups affect intermolecular attractions? How do intermolecular forces affect evaporation rate?
How do intermolecular forces affect freezing point? How do intermolecular forces affect solubility? How do intermolecular forces affect solvation?
How do intermolecular forces affect surface tension and viscosity? When do intermolecular forces of attraction occur? How is melting point related to the intermolecular forces of attraction? How do intermolecular forces of attraction affect the evaporation of liquids? See all questions in Intermolecular Forces of Attraction.
Impact of this question views around the world. You can reuse this answer Creative Commons License.Hydrogen bonding usually occurs between molecules that have a hydrogen atom bonded to either Fluorine, Oxygen or Nitrogen. So technically CH4 cannot hydrogen bond certainly not between it's own molecules.
CH4 is methane, or natural gas. This makes CH4 have a lower boiling point.
Hydrogen fluoride HF has the strongest hydrogen bonding. Water H2O and ammonia NH3 have the next strongest hydrogen bonding. Hydrogen bonding is when their is an electromagnetic attraction between the polar molecules in hydrogen and another atom.
Yes it has hydrogen bonding because the Nitrogen has lone pairs and it is bonded to a Hydrogen atom. Yes, Hydrogen bonding is a hydrogen bonded to any Fluorine, Nitrogen or Oxygen. Asked By Curt Eichmann. Asked By Leland Grant. Asked By Veronica Wilkinson. Asked By Daija Kreiger. Asked By Danika Abbott. Asked By Consuelo Hauck.
Asked By Roslyn Walter. All Rights Reserved. The material on this site can not be reproduced, distributed, transmitted, cached or otherwise used, except with prior written permission of Multiply.
Ask Login. Elements and Compounds. Asked by Wiki User. Top Answer. Wiki User Answered A hydrogen bond is an intermolecular force IMF that forms a special type of dipole-dipole attraction when a hydrogen atom bonded to a strongly electronegative atom exists in the vicinity of another electronegative atom with a lone pair of electrons.
Intermolecular forces IMFs occur between molecules. Other examples include ordinary dipole-dipole interactions and dispersion forces. Hydrogen bonds are are generally stronger than ordinary dipole-dipole and dispersion forces, but weaker than true covalent and ionic bonds. Many elements form compounds with hydrogen. If you plot the boiling points of the compounds of the group 14 elements with hydrogen, you find that the boiling points increase as you go down the group.
The increase in boiling point happens because the molecules are getting larger with more electrons, and so van der Waals dispersion forces become greater. If you repeat this exercise with the compounds of the elements in groups 1516, and 17 with hydrogen, something odd happens. Although the same reasoning applies for group 4 of the periodic table, the boiling point of the compound of hydrogen with the first element in each group is abnormally high.
These relatively powerful intermolecular forces are described as hydrogen bonds. If you are not familiar with electronegativityyou should follow this link before you go on. It doesn't go that far, but the attraction is significantly stronger than an ordinary dipole-dipole interaction. Hydrogen bonds have about a tenth of the strength of an average covalent bond, and are constantly broken and reformed in liquid water.
If you liken the covalent bond between the oxygen and hydrogen to a stable marriage, the hydrogen bond has "just good friends" status. Water is an ideal example of hydrogen bonding. Notice that each water molecule can potentially form four hydrogen bonds with surrounding water molecules: two with the hydrogen atoms and two with the with the oxygen atoms. This is why the boiling point of water is higher than that of ammonia or hydrogen fluoride. In the case of ammonia, the amount of hydrogen bonding is limited by the fact that each nitrogen only has one lone pair.
In a group of ammonia molecules, there are not enough lone pairs to go around to satisfy all the hydrogens. In hydrogen fluoride, the problem is a shortage of hydrogens. In water, two hydrogen bonds and two lone pairs allow formation of hydrogen bond interactions in a lattice of water molecules.
Water is thus considered an ideal hydrogen bonded system. When an ionic substance dissolves in water, water molecules cluster around the separated ions. This process is called hydration. Water frequently attaches to positive ions by co-ordinate dative covalent bonds. It bonds to negative ions using hydrogen bonds. If you are interested in the bonding in hydrated positive ions, you could follow this link to co-ordinate dative covalent bonding. The diagram shows the potential hydrogen bonds formed with a chloride ion, Cl.
Although the lone pairs in the chloride ion are at the 3-level and would not normally be active enough to form hydrogen bonds, they are made more attractive by the full negative charge on the chlorine in this case. However complicated the negative ion, there will always be lone pairs that the hydrogen atoms from the water molecules can hydrogen bond to.Hydrogen bondinginteraction involving a hydrogen atom located between a pair of other atoms having a high affinity for electrons ; such a bond is weaker than an ionic bond or covalent bond but stronger than van der Waals forces.
Hydrogen bonds can exist between atoms in different molecules or in parts of the same molecule. The other atom of the pair, also typically F, N, or O, has an unshared electron pair, which gives it a slight negative charge.
Mainly through electrostatic attraction, the donor atom effectively shares its hydrogen with the acceptor atom, forming a bond.
Because of its extensive hydrogen bonding, water H 2 O is liquid over a far greater range of temperatures that would be expected for a molecule of its size. Water is also a good solvent for ionic compounds and many others because it readily forms hydrogen bonds with the solute. Hydrogen bonding between amino acids in a linear protein molecule determines the way it folds up into its functional configuration.
Hydrogen bonds between nitrogenous bases in nucleotides on the two strands of DNA guanine pairs with cytosineadenine with thymine give rise to the double-helix structure that is crucial to the transmission of genetic information. Hydrogen bonding. Article Media. Info Print Cite.
What intermolecular forces are present in #CH_4#?
Submit Feedback. Thank you for your feedback. Home Science Chemistry. The Editors of Encyclopaedia Britannica Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree See Article History.
Read More on This Topic. The interactions described so far are not limited to molecules of any specific composition. However, there is one important intermolecular Learn More in these related Britannica articles:. However, there is one important intermolecular interaction specific to molecules containing an oxygen, nitrogen, or fluorine atom that is attached to a hydrogen atom.
This dominance is especially important in those solutions that involve hydrogen bonding. Whenever a solution contains molecules with an electropositive hydrogen atom and with an electronegative atom such as nitrogen, oxygen, sulfur, or fluorinehydrogen bonding may occur and, when it does,…. Hydrogen bonding is important in a few crystals, notably in ice. With its lone electron, a hydrogen atom usually forms a single covalent bond with an electronegative atom.
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That's great, but many of those predictions will be hopelessly wrong by the end of March. That's why it's so fascinating that Ray Kurzweil, one of the leading thinkers when it comes to the future of technology, has had such a strong track record in making predictions about technology for nearly two decades.
So how does he do it. The fact is, Ray has a system and this system is called the Law of Accelerating Returns. In his new book How to Create a Mind: The Secret of Human Thought Revealed, Kurzweil points out that "every fundamental measure of information technology follows predictable and exponential trajectories.