An atom of bromine-82 has 35 protons, 35 electrons and 47 neutrons. All electrically neutral atoms of bromine have 35 electrons.
Bromine has 4 electron shells.
A bromine atom with a mass number of 79 loses one electron to become a bromine ion with a negative 1 charge. This occurs when the atom gains an extra electron, giving it a full outer electron shell of 8 electrons, thus forming the Br- ion.
The bromine electron configuration is 4s23d104p5.
Bromine loses an electron and forms a bromide ion by gaining one electron in the reaction with sodium. Sodium donates its electron to bromine, making the bromine atom gain one electron and become a bromide ion during the reaction.
Bromine gains an electron to achieve a stable electron configuration and forms the bromide ion with a negative charge. This process is called reduction as bromine is gaining an electron.
Bromine tends to gain one electron to achieve a stable electron configuration, making it an electron acceptor (accepts one electron).
l = 1
The electron geometry of bromine pentafluoride is trigonal bipyramidal. This is because there are five regions of electron density around the central bromine atom.
The oxidation number of Br- is -1. Bromine typically has an oxidation state of -1 when it forms an ion by gaining one electron.
Bromine has a higher electron affinity than iodine. This is because bromine has a smaller atomic size, resulting in a stronger attraction for electrons compared to iodine.
An iodine atom has the same number of electrons as a bromine ion. Both elements belong to the halogen group and have seven valence electrons. When bromine gains one electron to become an ion, it will have a full outer shell with eight electrons, the same electron configuration as iodine.
Both. Bromine gains one electron in ionic compounds. Bromine will share electron in covalent compounds.