explain
The electron configuration in the outer shell is the same for all of the elements in the same column. This results in some similar chemical properties between these elements in the same group (column).
Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine All the above seven elements have same core-electron configuration as that of neon.
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
A full outer electron shell, the so-called valence shell, creates an inert gas in those elements (the inert or noble gases). In other elements, what is called "inert gas configuration" will apear in the Halogens (the Group 17 elements) and some Group 16 elements. When they "borrow" an electron or electrons in an ionic bond, they do so to achieve "inert gas configuration" by "filling" their valence shell with the borrowed electrons.
There are some elements that would get placed in an order that would not be correct for their electronic configuration.
We can predict the electron configuration, some chemical and physical properties, the atomic weight, etc.
The electron configuration in the outer shell is the same for all of the elements in the same column. This results in some similar chemical properties between these elements in the same group (column).
Sodium Magnesium Aluminium Silicon Phosphorus Sulphur Chlorine All the above seven elements have same core-electron configuration as that of neon.
There are specific factors that can contribute to a the properties of chemical elements. Some of these factors include the amount of valance electrons in the element.
Iodine accepts one electron to achieve noble gas configuration. Strontium loses two electrons to achieve noble gas configuration. Nitrogen accepts three electrons to achieve noble gas configuration. Krypton already has a noble gas configuration.
By using the activity series (sometimes called reactivity series) which orders metals by their reactivity with other metals, one can determine the reactivity of a metal
Electronegativity is, to some extent, a subjective value (though based on a composite of actually measurable physical properties). The highest electronegativity is usually assigned to fluorine. The electron configuration of fluorine's outermost shell is 2s2 2p5.
Chlorine is a nonmetal. It is only one electron short of a noble gas electron configuration and is much more likely to abstract an electron from some other element than to donate one to some other element.
A full outer electron shell, the so-called valence shell, creates an inert gas in those elements (the inert or noble gases). In other elements, what is called "inert gas configuration" will apear in the Halogens (the Group 17 elements) and some Group 16 elements. When they "borrow" an electron or electrons in an ionic bond, they do so to achieve "inert gas configuration" by "filling" their valence shell with the borrowed electrons.
electrons
Group 1 elements are metallic in nature. They have 1 electron in their outermost octet.
Hydrogen is placed in the group 1 because has some chemical similarities and electron configuration (one electron).