The deuteron is bound by nuclear forces just as H-atom is made up of p and e bound by electrostatic forces.
The deuteron is bound by nuclear forces just as H-atom is made up of p and e bound by electrostatic forces. If we consider the force between neutron and proton in deuteron as given in the form of a Coulomb potential but with an effective charge e′ :

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estimate the value of (e’/e) given that the binding energy of a deuteron is 2.2 MeV.
The binding energy in H atom

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If proton and neutron had charge e' each and were governed by the same electrostatic force, then in the above equation we would need to replace electronic mass m by the reduced mass m' of proton-neutron and the electronic charge e by e' .

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a) he helium (he) is an element by itself. he atom can only exhibit dispersion forces.b) hclh          1a                   1 × 1 e– = 1 e–cl         7a                   1 × 7 e– = 7 e–   total: 8 valence e–[readmore]cl is more electronegative than h, so hcl is a polar covalent compound. hcl exhibits dipole-dipole interaction.c) h2oh          1a                   1 × 2 e– = 2 e–o          6a                   1 × 6 e– = 6 e–   total: 8 valence e– since hydrogen is bonded directly to oxygen.h2o exhibits hydrogen bonding.d) cl2cl         7a                   1 × 7 e– = 14 valence e–composed of the same atom. there's no electronegativity difference.cl2 can only exhibit dispersion forces. hydrogen gas in its natural state consists of molecules of h2, where two hydrogen atoms are bound together by a 100% covalent bond.

the h2 molecules are attracted to each other by london dispersion forces. london dispersion forces result from the formation of temporary dipoles. a) van der waals (present, all molecule/atoms contain it)[readmore](b) dipole-dipole (present, c=o creates a partial charge on c and o)(c) hydrogen bonding (not present, h-bonds are only present in compounds with h attached on o, n or f)(d) ion-ion (not present, only appears on compound with full charges) coulomb's law:f=kq1q2r2, where k is the coulomb's constant and r is the separation between the two charges. the magnitude of the net force:fnet=fx2+fy2k = 9 × 109 n·m2/c2the force due to charge q1 is:f1a=kq1qar1a2=(9×109)(21.4×10-6)(13.5×10-6)(80.1×10-2)2[readmore]f1a = 4.05 nthe force due to charge, q2:f2a=kq2qar2a2=(9×109)(30.6×10-6)(13.5×10-6)[(80.1×10-2)2+(80.1×10-2)2]2f2a = 2.9 nforce due to charge, q3:f3a=kq3qar3a2=(9×109)(57.3×10-6)(13.5×10-6)(80.1×10-2)2f3a = 10.9 nthe net force along the x-axis:fx=f1a-f2acos(45°)=4.05-(2.9)cos(45°)fx = 2.0 nthe net force in the y-direction:fy=f3a-f2acos(45°)=10.9-(2.9)cos(45°)fy = 8.85 nthe magnitude of the net force:fnet=fx2+fy2=2.02+8.852fnet = 9.07 nthe magnitude of the net force on the charge at point a is 9.07 n. recall that there are several types of intermolecular forces:1. ion-dipole interaction – occurs between an ion and a polar covalent compound2. hydrogen bonding – occurs in compounds where hydrogen is directly connected to an electronegative element such as n, o, or f3. dipole-dipole interaction – occurs between two polar covalent compounds4. induced-dipole interaction – occurs when a nonpolar compound interacts with a polar compound5. dispersion forces – occurs in all compounds. this is the primary intermolecular force exhibited by nonpolar compounds.[readmore]although hcl is a polar molecule, it still exhibits dispersion forces because it occurs in all compounds since, atomic number of an atom = the number of protons.hence, the number of protons is 17.now, the number of protons = the number of electrons.∴ the number of electrons is also 17.given: mass number = 35we know that mass number = number of protons + number of neutrons.∴ number of protons + number of neutrons = 35⇒ 17 + number of neutrons = 35⇒ number of neutrons = 35 – 17⇒ number of neutrons = 18 because of the small size of boron atom and presence of only six electrons in its valence shell, b(oh)3 accepts a pair of electrons from oh- ion of h2o, releasing a proton.the reaction mechanism is: Answer  
Atoms prefer to have a filled outermost shell because this makes them more stable.  
Atoms react with each other to get the most stable state possible. A filled outermost shell (a  
complete octet for s- and p-elements) is very stable because all orbitals are filled with  
electrons. Stability of an atom is connected with its energy. Atoms with greater stability have  
less energy. We can see this in chemical reactions: a reaction that increases the stability of the  
atoms will release energy in the form of heat or light. chapter 5 key: electron: e                         number: # ­                 valence electron: ve   three­dimensional: 3d molecular: molec               with: w/ chemical: chem                 different: diff positive: pos negative: neg i. bonding theories ­ a. valence shell e pair repulsion (vsepr)  valence shell e pair repulsion: model predicting the arrangements of ve  ­ pairs around a central atom that minimizes their mutual repulsion  electron pair geometry: 3d arrangements of bonding pairs andn lone pairs  of e about a central atom  molecular geometry: 3d arrang answer: the molecular mass of an element is defined as the sum of the masses of the elements present in the molecule. molecular mass is obtained by multiplying the atomic mass of an element with the number of atoms in the molecule and then adding the masses of all the elements in the molecule. o2 is a diatomic molecule. the mass of an oxygen atom = 16 amu. ∴ mass of o2 molecule = 2 × 16 = 32 amu. mass of one molecule of oxygen → 32/ avogadro constant ( 6.023 × 1023) → 5.31 × 10-23g.