the valence electron of lithium that is easily removed is the 1s2 electron
Both francium and lithium have 1 electron in their outer electron shell and have a partially filled s-orbital. Both metals easily lose this outer shell electron.
LiBr would be the chemical formula. Lithium has +1 electron and Bromine has -1 electron so they combine easily.
No, because it has only on electron on it's outer shell, it loses it far to easily to other elements to be found pure, such as chlorine to make lithium chloride.
Let me start off by saying that the Lithium ion is not less reactive than the Lithium atom. In fact, Li+ is far more reactive than the Lithium atom, which is why it does not exist in its free state. Lithium ions tend to combine with anything it comes into contact with. However, it has a more stable electronic configuration than the Lithium atom, resembling that of a Noble gas(in the case of Li, it is Helium), which is why 1+ is the preferable oxidation state of Lithium.
lithium is IA group element .As lithium is basic it should give its electron easily but it is not that effecient in this as sodium.As it has small radius and high nuclear attraction towards its electrons.but sodium has larger atomic radii than the lithium less nuclear attraction towards its electrons.thus sodium is more reactive than lithium.
Of the metals listed, lithium is the most reactive. Lithium is an alkali metal with only one valance electron. This electron is easily lost in order to give lithium a stable noble gas configuration. Because of this tendency to lose an electron, lithium is quite reactive.
I think lithium should be more reactive as it has only 1 valance electron wheres Boron has 3 valance electrons. The electro positivity(tendency to lose electrons) of Lithium is greater then Boron, therefore more reactive.
Both francium and lithium have 1 electron in their outer electron shell and have a partially filled s-orbital. Both metals easily lose this outer shell electron.
LiBr would be the chemical formula. Lithium has +1 electron and Bromine has -1 electron so they combine easily.
Potassium. This can be seen by the potassium setting itself on fire in water. Can lithium, carbon or hydrogen do that?
Atomic number of Lithium is three. It has got two electrons in the first orbit. The third electron is free and in the outermost orbit. The atomic number of Sodium is 11 and that of potassium is 19. Sodium and potassium one electron in the outermost orbit. This outermost electron can be easily donated to have stable configuration. That is like Neon and Argon, respectively. So sodium and potassium can conveniently give up the last electron, rather than taking seven electrons to complete the outermost orbit. When sodium gives an electron, it loses about ten percent of charge. If potassium loses an electron, it loses about 5.5 percent charge. But if Lithium loses an electron, it loses 33.33 percent electrical charge. It will become grossly electrically positive in that case. Lithium feels uncomfortable to lose that much electrical charge. If Lithium forms the covalent bond, it does not have to become grossly electrically positive. Rather the electrical charge remains same, as the electrons are shared up in case of covalent bond. That is the reason as the why Lithium forms covalent bond, unlike other alkaline metals.
Lithium is in Group 1A and is a metal, therefore it forms +1 ions in order to achieve a noble gas configuration. For 1A and 2A metals, cation charge = group number or valence number. (they are the same thing).Lithium atom loses one electron to form the cation Li+
It is difficult to remove electron from He than Li. LI easily loses electron and reach stable state.
No, because it has only on electron on it's outer shell, it loses it far to easily to other elements to be found pure, such as chlorine to make lithium chloride.
Let me start off by saying that the Lithium ion is not less reactive than the Lithium atom. In fact, Li+ is far more reactive than the Lithium atom, which is why it does not exist in its free state. Lithium ions tend to combine with anything it comes into contact with. However, it has a more stable electronic configuration than the Lithium atom, resembling that of a Noble gas(in the case of Li, it is Helium), which is why 1+ is the preferable oxidation state of Lithium.
Due to low ionisation enthalpy, metals easily lose an electron and attain positive charge. eg. Na+, K+
Potassium can loose electron easily . Comparatively Lithium have high ionisation energy and low level of loosing electron while absorbing light energy.