Why is fluoride more stable than chloride?

Fluorine is having outermost Second orbital but Chlorine has outermost third orbital. hence , Fluorine is more stable than Chlorine. also , there is a rule that states , more negative charge on more electronegative atom is always a stable atom.

Why is the fluoride ion stable?

However, most ions form when atoms transfer electrons to or from other atoms or molecules. In the case of nonmetals such as fluorine, which has seven electrons in the outermost energy level, a more stable state can be achieved by gaining one electron and filling up the outer energy level.

Why iodide ion is more stable than chloride ion?

I- is larger in size as it belongs to the 5th period, the negative charge will be more dispersed or spread in the I- compared to Cl-, thus making I- more stable than Cl-.

Why is a fluoride ion smaller than a chloride ion?

Actually, Fluorine ion is smaller than chlorine ion. This is because the radius of fluorine ion is smaller than chlorine ion. Fluorine Ion has 2 shells and Chlorine Ion has 3 shells.

Is fluoride ion unstable?

The counter arguement is that fluoride ion has four lone pairs and a small size which makes it least stable. Down the group , since atomic size increases the extra electron is stabilized.

Which is more stable fluoride ion or chloride ion?

The answer lies in the fact that F is a smaller atom than Cl. When an electron adds to F, the electrons are closer to each other than in Cl, so there is stronger electron-electron repulsion. This is why chloride formation is easier than fluoride formation.

Is fluoride positive or negative ion?

Ion Charge?

Fluorine Atom
9 p+	to complete	Protons are identical in the atom and ion. Negative charge is caused by excess electrons
10 n	octet
9 e-	add 1 electron
0 charge

Which is more stable chlorine atom or chloride ion?

With additional electron in the outer shell, chloride ion tends to expand due to the electron repulsion between each other. Chloride has achieved the Argon electron configuration, therefore, stable than the chlorine atom.

Is iodide more stable than bromide?

Bromine has 4 shells, whereas iodine has 5. Positively charged protons are found in the nucleus of the atom. For bromine or iodine to react, each atom needs to gain an electron to fill up its shell so that it is in a more stable state.

Why are fluoride ions larger than sodium ions?

Fluoride ion has very high lone pair repulsion as compared to other halide thus its size increases more than usual. Both F-&Na+ have same electronic configuration but due to increased nuclear pull radius of Na+ decreases while in F- it increases due to repulsion.

Is fluoride ion reactive?

Unlike other hydrogen halide acids, the anion (fluoride ion) is quite reactive, and can form fairly insoluble salts with alkaline earth metals such as calcium and magnesium. Since the fluoride ion can react with calcium and magnesium, it can be dangerous to living organisms.

Why is fluoride more basic than iodide?

Fluoride anion is a stronger base because it’s the salt of a weaker acid. Sodium iodide is the salt of a very strong acid and thus it’s salt is essentially neutral. On the other hand because HF is a relatively weak acid, so sodium fluoride, a salt of HF is weakly basic.

Why is fluorine ion more stable than iodine ion?

Thermodynamic stability is sometimes a tricky beast, but in general a fluoride ion is more stable than an iodide ion which is prone to oxidation to give iodine or iodate. This is connected to the oxidising ability of fluorine (strong) versus iodine (weak), not to the strengths of the acids, though.

Why is fluoride more soluble than chloride?

For a substance to be soluble, there should be a release of energy as only then the system would turn into a more stable one (having less energy). Now H.E. for fluoride ion is more than that of chloride as both carry the same charge but due to smaller size of fluoride ion, it is able to bond with a larger number of water molecules.

Which anion is less stable than iodide?

Flouride anion is less stable than iodide anion due to the repulsion of electrons in the outermost octet of fluoride. But this rule is not absolute as chloride has the highest stability (in the gaseous state) though it is above bromine and iodine. Edit: Considering some confusion in the comments I shall put this here.

Why is fluorine not an oxidising agent?

The fluoride anion is not an oxidising agent. If it were, it would take up electrons to become a fluoride dianion ( F X 2 − ), inserting an electron into the 3s level—not happening. What you probably meant is fluorine (the element; the diatomic molecule) being the strongest oxidising agent out there.