F gains 1 e - and Ogains 2 e -'s, and O gain e -'s to attain theconfiguration of Ne thus, the halogens tend to -1 charges and theoxygen family tends to a -2 charge. The charge of elements in the periodic table can be determined by looking at the groups they belong to. On the other side of the periodic table elements gain electrons toresemble the next higher noble gas. Thus, the group 2 metals tend tohave a +2 charge. The alkali earth metals (group 2), such as, Mg or Sr lose two e-'sto attain the configuration of Ne. Since K loses one electron (1 negative charge)it is no longer neutral it now has a +1 charge. Kloses an electron so that it will have the same electronconfiguration as Ne.
The alkali metals will lose anelectron to resemble the next lowest noble gas thus, all the alkalimetals form +1 ions. For example, potassium atoms do this to form ions with the same electron configuration. Two (or more elements) can share electrons so that each attains the electron configuration of the nearest noble gas. All Group 1 atoms can lose one electron to form positively charged ions.The most simple atom to describe is the hydrogen atom. An element can attract additional electrons to achieve the electron configuration of the next highest noble gas. Protons have a positive electrical charge, neutrons are neutral, and electrons have a negative charge.An element can give up electrons to achieve the electron configuration of the next lowest noble gas.Achieving a Noble Gas Electron Configurationįor reasons we will discuss later, elements react until theelement achieves an electron configuration of a noble gas.Įlements can achieve a noble gas electron configuration threeways.
0 kommentar(er)
