This more detailed way of describing the arrangement of electrons in atoms is reflected in a representation of the Periodic Table (below) that shows the elements grouped in blocks: the s-block, the p-block, the d-block and the f-block. This type of sublevel is found from the fourth energy level. any fsubshell can hold up to 14 electrons.Energy levels higher than two have a d sub-shell. any dsubshell can hold up to 10 electrons.All energy levels except the first one have a p sub-shell. any psubshell can hold up to 6 electrons.any ssubshell can hold a maximum of 2 electrons.To differentiate between them, each type of subshell is denoted by a letter. Sublevels differ by the shape of the maximum number of electrons they can hold. The relationship is that there are as many sublevels per level as its number.Ĭurrently, there are four types of subshells known to be used by electrons in atoms up to element 118, the heaviest atom ever produced. The first shell or energy level is made up of only one subshell, the second shell consists of two subshells, the third shell has three subshells, and so on for higher energy levels. The valence electrons will determine how many electrons are shared or transferred between atoms.Each electron shell consists of subshells.When there is a large imbalance of electronegativity and ionization energy between atoms, an ionic bond will form.If we have a meta/nonmetal pairing then the nonmetal atom will pull strongly on the metal's weakly held (low ionization energy) electron and the metal atom will not pull very strongly (low electronegativity) on the strongly held (high ionization energy) electrons of the nonmetal atom.When both atoms in the pair have a similar pull on the other's electrons (electronegativity) and resist the removal of an electron (ionization energy) in a similar way, then they will share electrons forming a covalent bond.In that situation the atoms will attract the other's electrons with about the same strength, and it will take a similar amount of energy to remove an electron from each atom. If we have a metal/metal or a nonmetal/nonmetal pairing then each atom in the pair will have a similar electronegativity and ionization energy as the atom it is bonded with.If two atoms are going to bond together we have three possible categories:.Non-Metals (high ionization energy and high electronegativity).Metals (low ionization energy and low electronegativity).The periodic table can be divided into two broad groups:.Basically, atoms are most stable when they can achieve an outer electron structure similar to the closest Noble gas.This can be done by either sharing electrons between atoms, taking electrons from other atoms, or giving electrons away to other atoms. If atoms don't have 8 valence electrons (or two if they are close to He), then they will react with other atoms in order to have 8 valence electrons.One exception is He which has a full principle energy level with 2 electrons. All of these elements have 8 valence electrons in their highest principle energy level. One simple piece of evidence for this is the Noble Gases which form the last column on the right of the periodic table.Experimental evidence shows us that atoms are most stable when they have full s and p orbitals (8 valence electrons) in their highest principle energy level.Pick two elements from any column and determine how many valence electrons those atoms have.Bromine has 7 valence electrons: 1s 22s 22p 63s 23p 6 4s 23d 10 4p 5.Sodium has 1 valence electron: 1s 22s 22p 6 3s 1.Oxygen has 6 valence electrons: 1s 2 2s 22p 4.It is these electrons that primarily interact with other atoms. Valence electrons are those electrons that are in the highest principle energy level.
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