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Neither of these metals hold onto their outer electron (singular, as they are alkali metals) very strongly. Relatively speaking though, lithium holds onto its outer-most electron more strongly than Sodium does.
1 electron in the s orbital
nope.
the alkali metals have 1 electron in their outer most shell. in order to obtain a full outer shell they have to lose this electron. so when they react with another metal they lose this electron and the outer most shell.
The farther an electron is from the nucleus, the greater its energy.
There is only one electron in the outer most electron shell. With the lighter (less massive) alkali metals, there are less electron shells, between the outer most electron and the nucleus. Since the nucleus is positive(Protons) it more strongly holds the outer most electron. However, when going down the Alkali (Group 1) metals there are more electron shells, so the outer most electron is further away from the nucleus, and thereby less strongly held. This is evidenced by Lithium (The least massive) which only slowly effervesces in water. At the bottom of the group Francium ( The most massive) is explosive in water. NB Francium is not used in the open laboratory because it is also radio-active.
Neither of these metals hold onto their outer electron (singular, as they are alkali metals) very strongly. Relatively speaking though, lithium holds onto its outer-most electron more strongly than Sodium does.
It has a relatively high positive charge on its nucleus, a small atomic radius, only one electron shell between its nucleus and its outer electron shell, and is one electron short of a full outer shell.
Darmstadtium has seven electron shells around the nucleus.
It's because as atomic radius increases, so do the number of electron shells. The full electron shells closer to the nucleus act like a barrier or shield that reduces the pulling force exerted by the Nucleus on the outer electron. Since the nucleus's pulling force is reduced, an electron on the outer shell can escape much more easily.
1 electron in the s orbital
The distance from the center of the nucleus to the outer "edge" of the electron cloud.
alkali metal
Neon. The closer electrons are to the nucleus, the greater the pull the nucleus has on the electrons.
The electron outside the shell donate its electron to the one inside the shell
Because the force of attraction between the nucleus and the outer most electron is less. In addition, most metals (but not all) will gain the stable electronic configuration of the nearest noble gas if they lose electron.
Yes