gaining 1 electron
An atom of chlorine and an atom of bromine will form a covalent bond. Since both atoms are nonmetals, they will share electrons to complete their outer electron shells and achieve a more stable electron configuration.
A bromine atom typically has seven electrons in its outer shell, which means it only needs one more electron to have a full octet of eight electrons. Bromine can achieve an octet by gaining one electron to form a stable bromide ion with a -1 charge.
When a bromine atom gains an electron to form the bromide ion (Br-), it becomes negatively charged. The added electron gives the ion a full outer shell of electrons, making it stable. The bromide ion will be attracted to positively charged ions or molecules.
If a bromine atom underwent alpha decay, the result would be an arsenic atom with a mass number four lower than the original bromine atom. I did a little research on this, however, and it appears that there are no bromine isotopes that undergo alpha decay. I have provided a link to the interactive table of nuclides.
Francium would likely form an ionic bond with bromine by transferring its single valence electron to bromine in order to achieve a stable electron configuration. This would result in the formation of francium bromide (FrBr).
The Lewis Dot Diagram of KBr would show potassium (K) with one valence electron and bromine (Br) with seven valence electrons. The potassium atom would donate its electron to the bromine atom to form an ionic bond, resulting in a stable octet for each atom.
Bromine becomes stable by acquiring a full outer shell of electrons through bonding with other atoms or molecules. It can achieve stability by forming a single covalent bond, sharing one electron with another atom or molecule. Alternatively, bromine can form a diatomic molecule by sharing two electrons with another bromine atom.
An atom of chlorine and an atom of bromine will form a covalent bond. Since both atoms are nonmetals, they will share electrons to complete their outer electron shells and achieve a more stable electron configuration.
Bromine has seven electrons in its outermost energy level. It can get the stable electron configuration by getting one electron from another atom which makes the -1 charge.
A bromine atom typically has seven electrons in its outer shell, which means it only needs one more electron to have a full octet of eight electrons. Bromine can achieve an octet by gaining one electron to form a stable bromide ion with a -1 charge.
When a bromine atom gains an electron to form the bromide ion (Br-), it becomes negatively charged. The added electron gives the ion a full outer shell of electrons, making it stable. The bromide ion will be attracted to positively charged ions or molecules.
CBr (carbon monobromide) is a covalent compound. It is composed of a carbon atom bonded to a bromine atom via a covalent bond, where they share electron pairs to form a stable molecule.
The chemical symbol for the element bromine is Br. The elemental form of bromine is theoretically in the diatomic form (Br2), but it is not found in that form freely. Most of the bromine on earth exist as bromide salts in crustal rock.Chemical symbol for stable bromine is Br2. The state of matter of it is liquid. It is red-brown in colour.
When lithium reacts with bromine to form the compound LiBr, each lithium atom loses one electron to attain a stable electron configuration. This results in the formation of Li+ ions. The bromine atoms gain one electron each to form Br- ions. The ionic attraction between the Li+ and Br- ions then leads to the formation of the ionic compound LiBr.
The combining ratio of potassium and bromine is 1:1, meaning that one atom of potassium combines with one atom of bromine to form potassium bromide (KBr).
"Bromine" is the name of an atom or an element. The corresponding ion is named "bromide".
If a bromine atom underwent alpha decay, the result would be an arsenic atom with a mass number four lower than the original bromine atom. I did a little research on this, however, and it appears that there are no bromine isotopes that undergo alpha decay. I have provided a link to the interactive table of nuclides.