Which is bigger fluorine or hydrogen

It is a nonmetal, and is one of the few elements that can form diatomic molecules F 2. It has 5 valence electrons in the 2p level. Its electron configuration is 1s 2 2s 2 2p 5. It will usually form the anion F - since it is extremely electronegative and a strong oxidizing agent. Fluorine is a Lewis acid in weak acid, which means that it accepts electrons when reacting. Fluorine has many isotopes, but the only stable one found in nature is F In the late 's minerals which we now know contain fluorine were used in etching glass.

The discovery of the element was prompted by the search for the chemical substance which was able to attack glass it is HF, a weak acid. The early history of the isolation and work with fluorine and hydrogen fluoride is filled with accidents since both are extremely dangerous. Eventually, electrolysis of a mixture of KF and HF carefully ensuring that the resulting hydrogen and fluorine would not come in contact in a platinum apparatus yielded the element.

Fluorine was discovered in by Georgius Agricola. He originally found it in the compound Fluorspar, which was used to promote the fusion of metals.

It was under this application until , when Schwanhard discovered its usefulness in etching glass. Pure fluorine from the Latin fluere, for "flow" was was not isolated until by Henri Moissan, burning and even killing many scientists along the way. It has many uses today, a particular one being used in the Manhattan project to help create the first nuclear bomb. The van der Waals radius gives an approximate idea of how closely atoms in different molecules can approach each other.

Note how these radii decrease across and increase down the periodic table. Also given are values for the covalent radius of each atom.

The covalent radius is one-half of this bond length, or pm. Covalent radii are approximately additive and enable us to predict rough values for the internuclear distances in a variety of molecules.

See: chemistry. Add a comment. Active Oldest Votes. Improve this answer. Sujay Ghosh Sujay Ghosh 9 9 bronze badges. Why does that not happen? And that is pretty regular in most cases. Note: If you calculate the Effective Nuclear Charge for each members of a group, you will get a clearer idea about why the size factor is getting dominated. Li has lesser ionization energy than H. But, along a period Ionization energy increases gradually, with some exceptions, and becomes the maximum at the Noble Gas element.

Pallas Pallas 1 1 silver badge 6 6 bronze badges. Sign up or log in Sign up using Google. Sign up using Facebook. Sign up using Email and Password. Each of the noble gases has their outermost electron shell completely filled, which means multiple noble gas atoms are held together by Van der Waals forces rather than through bonds.

Van der Waals forces aren't as strong as covalent bonds, so two atoms connected by Van der Waals forces don't get as close to each other as two atoms connected by a covalent bond.

This means the radii of the noble gases would be overestimated if we attempted to find their empirical radii, so none of the noble gases have an empirical radius and thus don't follow the atomic radius trends.

Below is a very simplified diagram of four atoms, all about the same size. The top two atoms are connected by a covalent bond, which causes some overlap between the atoms. The bottom two atoms are noble gas atoms, and they are connected by Van der Waals forces that don't allow the atoms to get as close together. The red arrows represent the distance between the nuclei.

Half of this distance is equal to atomic radius. As you can see, even though all four atoms are about the same size, the noble gas radius is much larger than the radius of the other atoms. Comparing the two radii would make the noble gas atoms look bigger, even though they're not. Including noble gas radii would give people an inaccurate idea of how big noble gas atoms are.

Because noble gas atoms bond differently, their radii can't be compared to the radii of other atoms, so they don't follow atomic radius trends. Other exceptions include the lanthanide series and actinide series at the bottom of the periodic table.

Neither series has a clear atomic radius trend. Once you understand each key atomic radius period trend, it makes it easier to understand other information about the elements.

For example, you can remember that noble gases are an exception to the atomic radius trends because they have a full outer electron shell.

These outer electron shells also make the noble gases inert and stable. That stability can be handy. For example, balloons are typically filled with helium, not hydrogen, because helium is much more stable and therefore less flammable and safer to use. You can also use atomic radii to estimate how reactive different elements will be.