7A. The electron affinity values for the halogens are large in magnitude. Some sources list the values as large negative numbers, while others list them as large positive numbers.
Group 17, halogens
Group 17, (group VIIb), the halogens
An excited electron releases a photon as it returns to ground state.
If an electron transits to a lower energy level, it releases a quantum of energy which is equivalent to the energy difference between the states. If the electron travels to upwards, it absorbs a similar quantum of energy.
Elements on the right side of the periodic table require large amounts of energy to remove an electron from the outermost energy level of their atoms. It is much easier for them to gain rather than lose electrons.
On the periodic table there is no such order of first and second as asked in the question.
The first ionization energy is the energy that is required in order to remove the first electron from an atom in the GAS phase, the second ionization energy is the energy required to remove the second electron from an atom, etc. Ionization energy generally increases for every electron that is removed, and increases from left to right in the periodic table or if moving up the periods. In this case, from the periodic table (or according to Mastering Chemistry) Bromine (Br) has a larger sixth ionization energy than Selenium (Se).
An excited electron releases a photon as it returns to ground state.
Ionization energy increases to the right and up on the periodic table. Ionization energy is the energy required to remove an electron. It can be conceptualized as the opposite of electron affinity, though this is not precisely true.
When an electron is acquired by a neutral atom, the energy change is called electron affinity. Neutral atoms with an s2p6 electron configuration in the highest energy level are best classified as gases.
To get excited, it must absorb energy. To get back to its ground state, it releases energy.
Electrons move to a lower energetic state within an atom or molecule when they release energy.
If an electron transits to a lower energy level, it releases a quantum of energy which is equivalent to the energy difference between the states. If the electron travels to upwards, it absorbs a similar quantum of energy.
This is a chemical element. You can find the how many electron in a single atom by using a periodic table.
It releases the same amount of energy that it absorbed when it was excited to a higher energy state.
The ionization energy is the energy needed to extract an electron from an atom.The value of the ionization energy increase from left to right in a period of the periodic table and decrease in a group from the above to down.
exothermic oxidation, is where a molecule loses an electron(s), and releases heat energy in the process
the alkali metals
The ionization energy increases because the energy required to remove a valence electron will increase. The atoms want to keep their valence electrons because as you move more towards the right of the Periodic Table towards the noble gases. To write an abbreviation for electron configuration, it requires a noble gas and the valence electron configuration.