What is the electron affinity of Br?
What is the electron affinity of Br?
324.5371
A7: Electron Affinities
| Z | Element | Electron affinity (kJ/mol) |
|---|---|---|
| 35 | Br | 324.5371(3) |
| 36 | Kr | – |
| 37 | Rb | 46.884(2) |
| 38 | Sr | 5.023(6) |
What is 2nd electron affinity?
The second electron affinity is the energy required to add an electron to each ion in 1 mole of gaseous 1- ions to produce 1 mole of gaseous 2- ions. This is more easily seen in symbol terms. X−(g)+e−→X−2(g) It is the energy needed to carry out this change per mole of X−.
What is the second ionization energy of bromine?
BROMINE
| First ionization energy / kJ mol-1: | 1139.87 |
|---|---|
| Second ionization energy / kJ mol-1: | 2103.40 |
| Third ionization energy / kJ mol-1: | 3473.50 |
What is 1st and 2nd electron affinity?
There are two types of electron affinity, first and second. The first involves the addition of an electron to a neutral atom. Because this exothermic process releases energy, first electron affinities are negative values. The second pertains to the addition of an electron to a negative ion.
Does BR have a positive electron affinity?
When electron affinity is negative, it implies that adding an electron to an atom actually requires energy. So if you go by the sign convention, the electron affinity of bromine is actually positive because energy is being released when you add an electron to bromine.
Why is the 2nd electron affinity of oxygen positive?
The second electron affinity of oxygen is positive because after adding two electrons to its neutral oxygen atom, it attains a noble gas configuration. A noble gas configuration being most stable, releases energy to decrease the total energy of the configuration.
Is second electron affinity positive?
Second electron affinity is always negative.
How do you find electron affinity?
The amount of energy released when a neutral atom in its gaseous state accepts an electron and gets converted into a negatively charged ion is known as electron affinity. X ( g ) + e − → X − ( g ) + E . A . Therefore, the electron affinity of chlorine is – 349 KJ/mol.
What is the equation for electron affinity?
The electron affinity is the difference of the energies of the system without an electron and that of the anion, E G – E – = – ε 2 . It is equal approximately to the negative energy of the virtual orbital on which the electron lands (if ε 2 < 0 attaching an electron means energy lowering).
Why is the 2nd electron affinity endothermic?
2nd electron affinity is always endothermic (positive) because the electron is added to an ion which is already negative therefore it must overcome the repulsion.
What is the electron affinity of bromine?
Electron affinity of Bromine is 324.6 kJ/mol. In chemistry and atomic physics, the electron affinity of an atom or molecule is defined as: the change in energy (in kJ/mole) of a neutral atom or molecule (in the gaseous phase) when an electron is added to the atom to form a negative ion.
What is the symbol for bromine in chemistry?
| references. Bromine is a chemical element with symbol Br and atomic number 35. It is the third-lightest halogen, and is a fuming red-brown liquid at room temperature that evaporates readily to form a similarly coloured gas. Its properties are thus intermediate between those of chlorine and iodine.
What is the Order of electrons in each shell of bromine?
Therefore, the bromine atom will have two electrons in the first shell, eight in the 2nd orbit, eighteen electrons in the 3rd shell, and the remaining seven electrons will be in the fourth shell. Therefore, the order of the number of electrons in each shell of the bromine atom is 2, 8, 18, 7.
What is the electron configuration of the bromide ion?
The electron configuration of bromide ion (Br –) is 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s 2 4p 6. The electron configuration of bromide ion (Br –) shows that the bromide ion acquired the electron configuration of krypton. Bromine atom exhibit -1, +1, +3, +5 oxidation states. The oxidation state of the element changes depending on the bond formation.
