Francium(Fr) is the most reactive element in Group 1A .
The least reactive is Lithium(Li)
The element become increasingly reactive 'down' Group 1A.
NB You will NOT find francium in a school lab. for two reasons. 1. It explosive when in contact with water. 2. It is 'Radio-active' and radio-active matter has to be kept in special conditions.
One example of a block element that is not located in group 1A or group 2A in the periodic table is carbon, which is a p-block element. Carbon is located in group 4A (14) of the periodic table and is known for its diverse bonding properties, forming a wide range of compounds.
This is a consequence of the law of periodicity of chemical elements.
Group 1A elements, also known as alkali metals, have one electron in their valence shell. This single valence electron is responsible for their high reactivity and tendency to lose that electron to form positive ions. As you move down the group, the number of electron shells increases, but the number of valence electrons remains the same at one.
The reactivity of the alkali metals increases as you go down column 1 (or 1A) in a periodic table. This occurs because the first ionization energy of the metals decreases, as a result of "shielding" the outermost electrons from the attraction of the positive nucleus by the inner electrons.
The reactivity of an element largely depends on its electronic configuration. All the 1st group elements have one electron each in the outer most s-orbital. Their reactivity is due to the loss of this electron and formation of a uni positive ion. The ease with which the element loses the electron dictates its activity. As we go down the group, the distance between the outer most orbital and nucleus increases and hence the ease with which the element loses the electron increases as we go down the group. So naturally the reactivity increases. However in the case of 7th group elements(halogens) the electronic configuration is s2p5. They acquire stability by acquiring another electron. This is called electron affinity. This increases as we go up a group. So we find the more reactive element at the top of the group. We can generalize this like this. The reactivity of an element depends on the ease with which it acquires the nearest iner gas electronic configuration.
Th reactivity of alkali metals increases from the top of Group 1A to the bottom
francium
penis
Any element in group 1
valence electrons and electronic configuration.
The element in Group 1A with a higher atomic number than chlorine but lower than bromine is iodine.
One example of a block element that is not located in group 1A or group 2A in the periodic table is carbon, which is a p-block element. Carbon is located in group 4A (14) of the periodic table and is known for its diverse bonding properties, forming a wide range of compounds.
Francium (Fr) has the largest atom among the group 1A elements. It has the highest atomic number and electron shells, resulting in a larger atomic size compared to other group 1A elements such as lithium, sodium, and potassium.
The ion of an element from group 1A on the periodic table will have a +1 charge. This is because elements in group 1A, also known as alkali metals, readily lose one electron to achieve a stable electron configuration, resulting in a positively charged ion.
Cesium is the most reactive Group 1A element because it has the lowest ionization energy and the largest atomic radius, making it more willing to donate its outermost electron in a chemical reaction compared to potassium, lithium, and sodium.
This is a consequence of the law of periodicity of chemical elements.
use your brain.