0
Why is it easier to remove an electron from bromine then it is to remove an electron from fluorine?
Wiki User
∙ 11y ago
The reason why fluorine has a higher ionization energy level than oxygen is because it is closer to the nucleus than is oxygen, therefore, it will take more energy to pull electrons from the nucleus.
Wiki User
∙ 15y ago
Wiki User
∙ 14y agoBecause fluorine has 3 more protons than the carbon, so it pulls the electrons towards the nucleus with more force.
Wiki User
∙ 11y agoBecause of the large size, the valence electrons in bromine is less attracted by the nucleus and hence can be removed easily.
Add your answer:
Earn +20 pts
What is the formula for bromine gas?
Electron affinity is that energy released when one electron is added to a gaseous atom of an element. For MgMg(g) + e- -> Mg- (g) ; Energy = 0 kJ/molIt is different from ionization potential which is the energy required to remove one electronMg(g)-> Mg+(g)+2e-
How can remove the bromine from hexane solvent?
By solvent extraction with water. By fractional distillation.
Why is it harder to remove an electron from Magnesium than it is to remove an electron from Calcium?
Zinc has more electrons in its outer energy level than Calcium. Because of this, itsnucleus is more attracted to this energy level and pulls it more the nucleus in Calcium. Because of this greater attraction it is harder to remove the electron from Zinc.
If enough energy was added to remove an electron for calcium which energy level would the electron be removed?
The 3s.
Why is fluorine most electronegative than oxygen?
Electronegativity is an atoms relative ability to remove an electron pair in the formation of a covalent bond. I.e. an atoms ability to steal a pair of electrons from the outer ring of another atom to make a covalent bond, (like a contract to share electons in order to fill there outer shells and become stable) Across the periodic table (left to right) this gets harder to do due to an increase in attraction forces between the nuclear charge and the outer electons. Therefore across the periodic table 'more' electronegativity energy is required to remove those electrons. Down the periodic table, from top to bottom attraction forces between the electrons in the outer shell and the central nuclear charge decreases (shielding effect of sub levels and increased atomic radius), this make it easier for the electrons to be stolen, so there is less electronegativity required. Fluorine is the highest and furthest to the right, making it the most electronegative. (Helium and Neon etc have full outer shells so arent involved in covalent bonds)
What is the third ionization energy for fluorine?
Second ionization energy of fluorine is the amount of energy needed to remove an electron from a unipositive fluorine atom (F+)to form F2+,in all the gaseous state
Why does bromine have higher ionization energy then lead?
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Is it easier to remove an electron from the outer energy level than one closer to the nucleus?
Yes
Is it easier to remove an electron from the outside shell of a K atom than from the outside shell of a Na atom?
Yes.
How does electron shielding explain why it is easier to remove an electron from rubidium than from lithium?
In rubidium, having a larger atomic radius, the attraction force between the atomic nucleus and and the electron from outermost shell is lower.
Does bromine remove gum from hair?
well maybe because coca-cola remove gum from hair and well their is bromine in their
Why is Cs more electropositive than Rb?
The single outer electron is further away from the nucleus and thus is less tightly bound and thus it is energetically easier to remove that electron
Why is it easier to remove electrons from metals than non metals?
because metals have excess of electrons while non metals are electron deficient
Why it is difficult to remove an electron from halogens?
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
Why is it difficult to remove electron from halogens?
In their outer electron shell, halogens have 7 valence electrons, one less than the number needed for a full shell. Therefore, it is much, much easier for the halogen to gain an electron in bonding than for it to lose 7 - the ionization energy (energy required to remove an electron from an atom) is quite high.
Is it easier to remove an electron from and iodide ion or a bromide ion?
Electrons are affected by the protons in the nucleus. They have a positive charge that attracts the electrons. The further away the electron is, the lower the attractive power. It's like trying to get your mate to leave a bar when there's an attractive woman there. If he's at a table by the door just looking at her it'll be much easier than if he's sat next to her, talking! Iodide ions have their electrons a full energy shell further away from the nucleus than the bromide ions do. So they are the table by the door, and easier to remove. Bromides are the next easiest in the group, then Chlorine and Fluorine is the hardest. That's like he's got her room number and a promise!
What is the most chemically active non-metal in the periodic table?
The most chemically active non-metal, and the most reactive element overall, is fluorine. Fluorine has an extremely high electronegativity, meaning that it will remove an electron form almost anything. Therefore, it is amazingly reactive, and it even reacts with glass.
