An element's reactivity is influenced by its ability to gain or lose electrons to achieve a stable electron configuration. Elements with incomplete outer electron shells are generally more reactive as they can easily form bonds with other elements to gain stability. Reactivity can also be affected by factors such as atomic size and electronegativity.
Group 1 elements, also known as alkali metals, tend to give up electrons and become positive ions due to their low ionization energy and affinity to lose an electron to achieve a stable electron configuration.
Oh, dude, elements that gain 2 electrons when they combine with another element are found in Group 16 of the periodic table, also known as the oxygen group. This includes elements like oxygen, sulfur, and selenium. So, like, when these elements bond with others, they're all like, "I'll take two electrons, thanks!"
These are electrically positive objects.
The elements in group one and two react so easily because they have only one or two valence electrons, and the non metals, want those electrons. These group elements loose 1 or 2 electron to be stable instead of gaining 6 or 7 to complete the outer shell attain stable electronic configuration of a noble gas.
Thede are unreactive elements.
Carpets and balloons both give up electrons easily.
easily gain electrons
The elements that typically give up electrons are the ones which have the lowest ionization energy. The valence electron which holds on loosely will be the one to be given out easily.
Carpets and balloons both give up electrons easily.
no
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
The force of attraction between the atom's nucleus and its valence electrons are the least. Hence valence electrons are lost easily.