First 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.
Any Group 1 or Group 2 element will easily give up an electron. examples are: Sodium (Na) Potassium (K) Magnesium (Mg) Strontium (Sr)
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.
Elements that are in the same group of the periodic table have the same number of electrons in their outer energy level. In the case of lithium and sodium, they each have one electron in their farthest shell.
== == When metals react with other elements, the atoms of the metals give up their valence electrons.
The alkali-group elements (group I of the periodic table) H, Li, Na, K, Rb, Cs, Fr in period 1 to 7 respectively.
Metals are strong electron donors. They easily give their valence electrons.
When we say valence electron we mean the number of electron left it the outermost shell of element, valence electron can be positive of negetive. If an element need much electrons to be octet, that means that the element is not reactive than the one who will give out electrons, the the one who can give electrons much are less reactive than the one who can give a litle and the reaction will be normal as it is soppused to be, Eg lithium and berylium. Lithium is more reactive than berylium because lithuin has 1valence electron while berylium has 2....reactivity goes with the action of valence electron in an element
The force of attraction between the atom's nucleus and its valence electrons are the least. Hence valence electrons are lost easily.
it the smallest element with one valence electron and will bond to just about anything, theres no scenario in nature where hydrogen would not have another element around to bond to
Give the number of valence electrons for SBr4.
The positive ion, the one that took the electrons, should have a full shell while, the negative ion, the one that lost the electrons, should have an empty shell.
Any Group 1 or Group 2 element will easily give up an electron. examples are: Sodium (Na) Potassium (K) Magnesium (Mg) Strontium (Sr)
2 electrons
Metals, particularly the alkali metals- lithium, sodium, potassium, etc
Before : One electron in the valence shell After reaction w/ Cl gas: none electron in the valence shell
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.
give away its one valence electron