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∙ 11y agoFirst of all this is a lot more than just one element. All the alkali metals are like this, all having one valence electron. They are Hydrogen, Lithium, Sodium, Potassium, Rubidium, Cesium, and Francium. Yes they have elements named after countries.
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∙ 11y agoThe alkali-group elements (group I of the periodic table) H, Li, Na, K, Rb, Cs, Fr in period 1 to 7 respectively.
Except hydrogen, elements in group 1 are very reactive at they can give away their only electron in their valence shell easily to be ionized.
An element that is a metal is more likely to give away its electrons because metals tend to lose electrons in chemical reactions to achieve a stable electron configuration. Sodium and potassium are common examples of metals that readily give away electrons.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
To be stable it would need to be A2B (2 of element A would give a total of 6 valence electrons + the 1 element B would give a total of 8 electrons in the covalent bond. The bond is now stable and you have a compound.)
Metals are strong electron donors. They easily give 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.
The number of valence electrons in an element determines its reactivity. Elements with few valence electrons tend to be more reactive as they are more likely to gain or lose electrons to achieve a stable electron configuration. Elements with full valence shells are generally stable and less reactive.
Francium gives away electrons very easily due to its location in the alkali metal group, which makes its outer electron very loosely bound. This makes Francium highly reactive and likely to form ions by losing its single valence electron.
The alkali-group elements (group I of the periodic table) H, Li, Na, K, Rb, Cs, Fr in period 1 to 7 respectively.
Yes, hydrogen gives up its valence electron easily because it has only one electron in its outer shell. This makes it highly reactive and willing to donate its electron to form a positive ion.
An element that is a metal is more likely to give away its electrons because metals tend to lose electrons in chemical reactions to achieve a stable electron configuration. Sodium and potassium are common examples of metals that readily give away electrons.
Give the number of valence electrons for SBr4.
If an atom has one valence electron, it will typically form a +1 cation by losing that electron to achieve a stable electron configuration.
Cesium has one valence electron. To achieve a noble gas electron configuration like xenon, cesium would need to give up that one valence electron, therefore losing one electron.
In the calculation of valence electron counts using the 18-electron rule, phosphine (PH3) contributes 5 valence electrons. Since each hydrogen atom contributes 1 electron, the total valence electron count for PPh3 (Ph = phenyl group) would be 5 (from phosphorus) + 3x1 (from hydrogen) = 8 electrons.
Except hydrogen, elements in group 1 are very reactive at they can give away their only electron in their valence shell easily to be ionized.