Each period has one more energy level than the last: lets look at group 1 the alkaline metals as an example
H - 1 - one energy level
Li - 2,1 - two energy levels
Na - 2, 8, 1 - three energy levels
K - 2, 8, 8, 1 - four energy levels
ect
every column is a family and they each have the same number of electrons to begin with. but the to become stable, they need to take, or give away electrons to have 8 electrons on there outter shell
They are related because the principal energy level of the valence electron is equal to the period number its located in.
its not the energy level that changes but its the number of electrons of protons, the number its assigned to is the amount of electrons or neutrons it has
it depends on how close it is to the noble gas
The period number is the same as the highest energy level containing electrons for the atoms in that period.
In which it was found
The halogen family elements have 7 valence electrons. This is because they have 7 electrons in their outermost energy level.
Neon
The valence electrons are the electrons that undergo chemical bonding in the main group or representative elements.
An atom can have a maximum of 8 valence electrons, except for hydrogen and helium, which can have a maximum of 2 valence electrons. Valence electrons are the electrons in the outermost energy level of an atom.
Oxygen atoms have 6 electrons in the highest occupied energy level. They are two 2s electrons and four 2p electrons. All elements in Group 16 have 6 valence electrons. For Groups 13-18, subtract 10 from the group number and that gives you the number of valence electrons (the electrons in the highest energy s and p orbitals). The Group 1 elements have one valence electron and the Group 2 elements have two valence electrons. The transition metals can vary in the number of valence electrons. You can't necessarily go by group number for them.
When these elements have five electrons on the outermost shell of electrons.
Neon
The valence electrons are the electrons that undergo chemical bonding in the main group or representative elements.
Elements within the same period have the their valence electrons in the same principle energy level. For example, those elements in period 2, have their valence electrons in the 2nd energy level.
That, or they, would be the outer most shell electrons. The one(s) that get shared when elements bond. The one that moves out and up when struck by a photon. The one that makes light when it falls back down (gives up its' energy) to its' original shell. ADD: It is a valence electron.
The period number is the same as the energy level containing the valence electrons. For example, in period 4, the valence electrons are the 4s and 4p electrons.
Boron is located in group 3A. It is group 13 in modern notation. This set of elements have three valence electrons.Boron is in the 13th group in the periodic table. Elements in this group has 3 electrons in the outermost energy level. That means they have 3 valence electrons.
The number of electrons of both atoms and its valence number.
Oxygen atoms have 6 electrons in the highest occupied energy level. They are two 2s electrons and four 2p electrons. All elements in Group 16 have 6 valence electrons. For Groups 13-18, subtract 10 from the group number and that gives you the number of valence electrons (the electrons in the highest energy s and p orbitals). The Group 1 elements have one valence electron and the Group 2 elements have two valence electrons. The transition metals can vary in the number of valence electrons. You can't necessarily go by group number for them.
The energy of the valence electrons is greater than the energy of the core electrons.
The energy of the valence electrons is greater than the energy of the core electrons.
There are different numbers of valence electrons in different elements.