They're going to become positively charged. So before we look at this question, remember, we're gonna say that medals, they tend to lose electrons, so they're gonna lose electrons. It says, from what you know about ion formation in the periodic table, which ion would be unlikely to occur. In the next video, we'll see exactly how many electrons will we lose or gain for any particular element. So just remember, the whole reason elements gain and lose electrons is to become just like the noble gasses. I'm gaining negatively charged electrons, so I'm gonna become more negative as a result. So non metals tend to gain electrons to become negatively charged ions called an ions. If medals lose electrons, then non metals must be gaining electrons. Medals will go in greater detail on what types of metals are Type one medals and what other types of metals are. When metals have multiple charges, then they're referred to as type two. When a metal possesses one charge, we refer to them as type one medals. AT T could represent the positive charge that the ion gains, and it makes sense because if you're losing negatively charged subatomic particles in the form of electrons, you're going to become mawr positively charged Now, medals themselves medals can have either one type of positive charge or multiple types of positive charges. When it comes to medals, medals tend to lose electrons to become positively charged ions called cat ions. So if there number of electron matches one of the nearest noble gasses, now we're going to stay here. But just realize when it comes to the elements, the leader lose or gain electrons. ![]() What that means specifically will talk about several chapters from now. The reason these elements want to become the noble gas is because noble gasses themselves have the optimal number off outer shell electrons. Okay, so remember two different ways to describe the same column of the periodic table. Now, remember, your noble gasses are the elements that are found in Group eight A or Group 18. Therefore the distinguishing electron must occupy either the 5 s or 5 p subshell.Now the elements of the periodic table will either lose or gain electrons to become just like the noble gasses. For example, iodine is a representative element in the fifth period. The value of n, the principal quantum number for the distinguishing electron, can be quickly determined by counting down from the top of the periodic table. As a general rule, in the case of the representative elements, the distinguishing electron will be in an ns or np subshell. In the third period the 3 s subshell is filling for Na and Mg, and therefore Al, Si, P, S, Cl, and Ar. Across the second period Li and Be have distinguishing electrons in the 2 s subshell, and electrons are being added to the 2 p subshell in the atoms from B to Ne. In the first period the distinguishing electrons for H and He are in the 1 s subshell. The first three horizontal rows or periods in the modern periodic table consist entirely of representative elements. Formulas for chlorides of the first dozen elements that show the periodic variation of valence Element This agrees with the valence rules derived from the periodic table, and results in formulas for chlorides of the first dozen elements that show the periodic variation of valence. For representative elements the number of valence electrons is the same as the periodic group number, and the number needed to match the next noble-gas configuration is 8 minus the group number. That is, the valences of the representative elements may be predicted on the basis of the number of valence electrons they have, or from the number of electrons that would have to be added in order to attain the same electron configuration as an atom of a noble gas. Many of the chemical properties of the representative elements can be explained on the basis of Lewis diagrams. Most of the elements whose chemistry and valence we have discussed so far fall into this category. ![]() The representative elements are those in which the distinguishing electron enter an s or p subshell. The type of subshell ( s, p, d, f)into which the distinguishing electron is placed is very closely related to the chemical behavior of an element and gives rise to the classification shown by the color-coding on the periodic table seen here. ![]() This last electron is called the distinguishing electron because it distinguishes an atom from the one immediately preceding it in the periodic table. Since it is the outermost (valence) electrons which are primarily involved in chemical interactions between atoms, the last electron added to an atom in the building-up process is of far more interest to a chemist than the first. ![]() The commonly used long form of the periodic table is designed to emphasize electron configurations.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |