Draw the molecule. It is a selenium atom with two bonds to hydrogen atoms and two lone pairs. There is a definite polar bond here: Selenium is more electronegative than hydrogen so electrons will tend to go towards the selenium atom, causing a dipole.

However, it is not polar enough to be considered a hydrogen bond.

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The answer is that dipole-dipole causes most of the intermolecular forces although london dispersion forces always exist.

It's just in this case they are insignificant compared to dipole-dipole.

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The electronegativity of H is 2. So the boomerang-shaped H2Se molecule has a charge separation within it. Trending News. Witness to executions hears haunting last words.

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what intermoleculare force is H2se? dipole dipole, dispersion,h-bond,covalent,or interionic?

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Volume 55, Previous Article Next Article. From the journal: Transactions of the Faraday Society. Calculations of dipole moments of H 2 Se and AsH 3.If you can't find the dipole moment online then you can get a pretty good approximation using the following method though it is a bit involved. You will need the following two pieces of information before you begin, which I have obtained from Chemistry, The Central Science by Theodore Brown 11e:. To find the dipole moment you must first find the partial charge of the Se and H atoms.

This is the amount by which the bonding electrons are shared unequally:. Se holds a partial charge of Finally, we multiply the separated charge by the distance of separation, where the displacement vector d is directed from the negative to positive charge, to obtain the dipole moment:. The molecular dipole moment of H2Se is the sum of the individual Se-H dipole moments.

If we place the Se atom at the center of an xy plane, i. The y components of the two vectors, however, are in the same direction so they add and because they are the same magnitude their sum is simply twice the magnitude of one of them and its direction exactly bisects the molecule.

Ammonia has a dipole moment of 1. Its dipole moment is the net dipole moment resulting from three individual bond moments. How many times does Justin Bieber say 'baby' in his song 'Baby'? Is best defined as the total weight of persons gear equipment stores fuel and motor assembly found on a vessel? All Rights Reserved.

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Organic Chemistry. Inorganic Chemistry. Top Answer. Wiki User The bonding radii of the Se and H atoms: 1. Related Questions. Does ammonia have a dipole moment? Why is the dipole moment of HI less than the dipole moment of HCl? Does CHCl3 have a dipole moment? Does CH3NH2 have a dipole moment? No, CH3NH2 does not have a dipole moment. Does SF6 have dipole moment? SF6 does not have a dipole moment. Trending Questions. Hottest Questions. Previously Viewed.

Unanswered Questions.By using our site, you acknowledge that you have read and understand our Cookie PolicyPrivacy Policyand our Terms of Service. Chemistry Stack Exchange is a question and answer site for scientists, academics, teachers, and students in the field of chemistry. It only takes a minute to sign up. In other words, it seems to me the intermolecular forces should be induced-dipole induced-dipole making the molecule non-polarnot dipole dipole.

I should clarify, I first saw this statement in the answers to a high school chemistry exam. I then googled it, and got the same answer i. Information in this question is all over the place and often out of context. Let me get a few things straight:. Van der Waals forces, also known as London interactions, occur between every pair of molecules regardless of polarity. They are explained by induced and spontaneous dipoles at a molecular level and femtosecond timescale.

Dipole interactions are present between macroscopic dipoles and account for the boiling point difference between e. For strong dipoles, these interactions are orders of magnitude larger than the underlying van der Waals forces.

Electronegativities are, of course, atomic properties and also depend on things like oxidation state if one is truly accurate. For no two different elements is the electronegativity difference ever zero. Calling van der Waals forces dipole interactions is usually considered wrong although they build up upon the same principles: electrostatic interaction.

I tried to stick to a high-school level as well as possible. Hence a number of simplifications in this answer.

the boiling point of H2Te > H2Se > H2S, explain this trend in terms of intermolecular force.?

Thus, every molecule of that type will display dipole-dipole interactions however weak they may be. The electron cloud is not stationary in time, but dynamic.

This means that the electron cloud is subject to fluctuations in its distribution. So, at some point in time, the electron cloud will be shifted in one direction. Hence, the molecule has become slightly polar. These fluctuations take place on a very, very, very short timescale, and basically the "non-polar" molecule is not really non-polar although it may be close.

When this slightly polar molecule approaches a non-polar one, the small dipole moment induces a shift in the other molecule's electron distribution due to electron-electron repulsion. The slightly negative part of molecule A will be attracted to the slightly positive part of molecule B, and a lower-energy state is achieved. This is called induced dipole-dipole interactions, and is a simple explanation of how certain melting-point trends can be observed for groups in the periodic table.

See this youtube video for an introduction to various dipole-dipole interactions skip to to start on the induced dipole-dipole interactions. More generally, the symmetry of the molecule should be first considered to decide if the molecule has a dipole moment. Someone could argue that these could still hypothetically have no dipole moment at some particular state, such as a specific rotational and vibrational state, but realistically these molecules will have a dipole moment.

Then the specific elements and electronegativities could be considered to quantify the dipole moment. Sign up to join this community.Dipole moments occur when there is a separation of charge. They can occur between two ions in an ionic bond or between atoms in a covalent bond; dipole moments arise from differences in electronegativity.

The larger the difference in electronegativity, the larger the dipole moment. The distance between the charge separation is also a deciding factor into the size of the dipole moment. The dipole moment is a measure of the polarity of the molecule.

When atoms in a molecule share electrons unequally, they create what is called a dipole moment. This occurs when one atom is more electronegative than another, resulting in that atom pulling more tightly on the shared pair of electrons, or when one atom has a lone pair of electrons and the difference of electronegativity vector points in the same way.

dipole moment of h2se

One of the most common examples is the water molecule, made up of one oxygen atom and two hydrogen atoms. The differences in electronegativity and lone electrons give oxygen a partial negative charge and each hydrogen a partial positive charge. When two electrical charges, of opposite sign and equal magnitude, are separated by a distance, an electric dipole is established. The dipole moment acts in the direction of the vector quantity.

Hence, water is polar. The vector points from positive to negative, on both the molecular net dipole moment and the individual bond dipoles. Table A2 shows the electronegativity of some of the common elements.

The larger the difference in electronegativity between the two atoms, the more electronegative that bond is. To be considered a polar bond, the difference in electronegativity must be large.

The dipole moment points in the direction of the vector quantity of each of the bond electronegativities added together. Consider a simple system of a single electron and proton separated by a fix distance. When proton and electron close together, the dipole moment degree of polarity decreases.

However, as proton and electron get farther apart, the dipole moment increases. The Debye characterizes size of dipole moment.Monoatomic Ions. Determine the rate law and the value of the rate constant for this reaction. Table 1 is an alphabetical listing of the elements, according to the symbol of the elements. The chemistry of H2S has been studied since the s.

dipole moment of h2se

Sulfur is more electronegative than selenium. A polar molecule is one in which there is a difference in electronegativity between the atoms in the molecule, such that the shared electron pair. Colorless, flammable, poisonous and corrosive, H2S gas is. HCrO4 aq 2.

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It is a selenium atom with two bonds to hydrogen atoms and two lone pairs. Hydrogen selenide is a metabolite of selenium which could have potential antiangiogenic effect in the chemoprevention of cancer. The chemical name for P 4 O 6 is "tetraphosphorus hexoxide.

dipole moment of h2se

Iodine oxidation by hydrogen peroxide in acidic solutions, Bray-Liebhafsky reaction and other related reactions April Physical Chemistry Chemical Physics 12 25 Eau of molecule in a gas at equilibrium. Thats what I would think under testing. The half-cell potential is the potential developed at the electrode of a half cell due to the process of oxidation or reduction. So the repulsion of the lone pairs cancel off each other. A weak acid is one that only partially dissociates in water or an aqueous solution.

There are total of 20 valence electrons for the ClO2- Lewis structure. Se is oxidized, therefore H2Se g is the reducing agent. CN- does not have the proton, HCN has the proton. Why does H2Se have a bent shape? It has 6 valence electrons. Read our article on how to balance chemical equations or ask for help in our chat.

B Electron pair donor.

Dipole Moments

So I used the other and the answe. As the number of oxygens increases, so does the acid strength; again, this has to do with electronegativity.But last week Michael Arrington at TechCruch reported on a rumor which hints at a more clever plan: a free Kindle for every Prime customer of Amazon. It turns out that was just a test run for a much more ambitious program. A reliable source tells us Amazon wants to give a free Kindle to every Amazon Prime subscriber.

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