When hydrogen and fluorine atoms bond, a permanent net dipole forms resulting from hydrogen being covalently bonded to the fluorine as hydrogen bonds form.
the hydrogen bond is the strongest type of intermolecular force since the hydrogen nucleus is extremely small and positively charged and fluorine is very electronegative so that the electron on the hydrogen atom is strongly attracted to the fluorine. this leaves a highly localised positive charge on the hydrogen atom and highly negative localised charge on the fluorine.
this means the electrostatic attraction between these molecules will be greater than for the polar molecules that do not have hydrogen covalently bonded to either fluorine.
because the fluorine atom is unstable, as is the hydrogen, because they have not filled up their valence shell, they bond together quickly, and because of their opposing charges, very strongly.
have a look at some online animations, with will become very clear to you.
(-) (-) (-) (strong hydrogen bonds)
(-) F ----------------------------------------… H (+)
(-) (-)
it looks a little bit like that, the (-) negative charges on the fluorine attract the positive (+) charge on the hydrogen, forming in hydrogen bonds (----). The fluorine has 7 electrons and the (---) is where both H and F share the electron.
Potassium (K) has 1 valence electron which is loses to become K^+. Fluorine has 7 valence electrons and picks up the 1 electron lost by K, and it becomes F^-. They attract each other to become KF.
this is because a fluorine ion is one electron short of a full valence shell,which makes getting another electron to fill the shell very favourable,filling the shell makes the molecule much more stable
[He] 2s2 3p5 is the electronic configuration of a neutral Fluorine atom. It's -1 ion (F-, fluoride ion), however is: [He] 2s2 3p6, or [Ne].
Fluorine is a halogen. All halogens have 7 valence electrons. There are thus 7 valence electrons for Fluorine, 2 in the 2s orbital, and 5 in the 2p orbitals.
Fluorine has 7 valence electrons, however, Fluoride (F-) is an anion with a negative charge, giving it one more electron, bumping the number of valence electrons to 8.
Fluorine has 7 valence electrons. 2 In the first electron shell, and 5 in the second electron shell.
Potassium (K) has 1 valence electron which is loses to become K^+. Fluorine has 7 valence electrons and picks up the 1 electron lost by K, and it becomes F^-. They attract each other to become KF.
I believe you are talking about fluorine. If you are, F needs one more electron to gain a full shell.If you go to WikiAnswers for this information, that is counterproductive, because there is a much better way to do it. Look at the periodic table. Groups IA through VIIIA tell you what you need to know. IA has one valence electron, IIA has two valence electrons etc. Fluorine is in group VIIA and therefore has seven valence electrons. All atoms want eight, and thus fluorine is in need of one more.
I believe there is 8 electrons in the outer valence
Fluorine is a chemical element in the halogen group. It's electron structure is 1s2 2s2 2p5. That means that it has 6 valence electrons.
Both fluorine and chlorine have seven valence electrons. In the case of fluorine they're in n=2 and in the case of fluorine they're in n=3, but other than that they're the same.
this is because a fluorine ion is one electron short of a full valence shell,which makes getting another electron to fill the shell very favourable,filling the shell makes the molecule much more stable
Any element in the halogen group will have seven valence electrons. These elements include fluorine, chlorine, bromine, iodine, and astatine.
ONE (apex)
it has 7 valence electrons, which is the number of electrons on the outer energy level, so it needs 7.
Fluorine has 7 valence electrons and should gain 1 more electron.
Yes it does. Each fluorine shares one electron with oxygen. So fluorine as well as oxygen will have 8 valence electrons.