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How many valence electrons does a bromine anion contain?
A bromine anion has 8 valence electrons. This is because bromine, with 7 valence electrons, gains one extra electron when it forms an anion to achieve a full octet and become stable.
If an atom has four valence electrons is it an anion?
No, having four valence electrons does not determine whether an atom is an anion. An anion is formed when an atom gains electrons to have a negative charge. If the atom with four valence electrons gains four more electrons, it would become an anion.
How many valence electrons does anion of OCl?
The anion of OCl (hypochlorite ion) has 8 valence electrons. This is because oxygen contributes 6 valence electrons and chlorine contributes 7 valence electrons. The overall negative charge of the anion adds one more electron, totaling 8 valence electrons.
How many valence electrons does br- have?
The anion is Br+; bromine has 7 valence electrons.
How many electrons does an oxygen anion have?
An oxygen anion has 10 electrons, because it gains two electrons to achieve a full valence shell of 8 electrons.
How many valence electrons does a bromine anion contain?
A bromine anion has 8 valence electrons. This is because bromine, with 7 valence electrons, gains one extra electron when it forms an anion to achieve a full octet and become stable.
How many valence electrons does HBr have?
Hydrogen has 1 valence electron. Bromine has 7 valence electrons. When hydrogen and bromine react, the bromine atom 'steals' the hydrogen atom's only electron. The hydrogen atom then has no electrons and the bromine atom has 8 valence electrons. The two atoms are now ions because their number of protons does not equal their number of electrons. The bromine atom is now a bromide anion and the hydrogen atom is now a hydrogen cation (a proton). The two ions remain together, ionicly bonded and together are called hydrogen bromide.
How do you determine which halogen has an anion with 36 electrons?
There is no halogen that will become anionic. All of the valence electrons in halogens are filled, thus halogens will not react with any other compound or element. Bromine is an element that will form and anion with 36 electrons.
How many electrons does (anion) CL have?
Chloride anion has 8 valence electrons.
If an atom has four valence electrons is it an anion?
No, having four valence electrons does not determine whether an atom is an anion. An anion is formed when an atom gains electrons to have a negative charge. If the atom with four valence electrons gains four more electrons, it would become an anion.
How many valence electrons does anion of OCl?
The anion of OCl (hypochlorite ion) has 8 valence electrons. This is because oxygen contributes 6 valence electrons and chlorine contributes 7 valence electrons. The overall negative charge of the anion adds one more electron, totaling 8 valence electrons.
How many valence electrons does br- have?
The anion is Br+; bromine has 7 valence electrons.
How many electrons does an oxygen anion have?
An oxygen anion has 10 electrons, because it gains two electrons to achieve a full valence shell of 8 electrons.
What is the valence number of bromide?
in the valence shell of bromide 7 electrons are present. So the valency of bromide is 1
How many valence electrons does cl- have?
Cl- has 8 valence electrons. This is because chlorine, in its neutral state, has 7 valence electrons (group 17), and the -1 charge of the chloride ion indicates the addition of an extra electron.
How many valence electrons do the anions have when they bond?
This number is different for each anion.
How many electrons does a fluoride anion contain?
flouride atoms are part of the halogen group and so have 7 valence electrons. however a flouride ion is a different story. firstly it depends if the ion is an anion or a cation. if the ion is F- then it is an anion and has 1 extra electron and so has 8 valence electrons. if it is F+ is is a cation and has lost an electron and so has only 6 valence electrons. if the ion is F2- this means it has gained two electrons and so on.
