compare the properties of element in group 1 and group 17
Answers
Answer:
The general electronic configuration of Group 1 elements is ns1. They have a strong tendency to donate their valence electron in the last shell to form strong ionic bonds. They have the least nuclear charge in their respective periods. As we move down the group, the atomic radius increases. Therefore, the nuclear charge decreases. Caesium is the most metallic element in the group.
In order to prevent the elements from coming in contact with oxygen, they are stored in jars that contain oil. The melting points of these elements are quite low, which is 180° Celsius in the case of Lithium, while it is 39° Celsius in the case of Rubidium. When it comes to the density of the metal, group one elements display a very low level of density of up to 1 gcm-3 which means that they can easily float on the surface of the water.
Therefore, if we decide to cut these metals, we will be able to do so, without much trouble. Upon being cut into two halves, we can observe that their surface is as shiny as any other metal but even after they are stored in oil, they undergo tarnishing. As a conductor of heat and electricity, they are excellent.
Learn more about Group 14 Elements here.
The Reaction of Alkali Metals with Water
Alkali metals derive their classification because of the results of their reaction with water. It is known upon the reaction with water that alkali metals produce an alkaline solution, along with the release of hydrogen gas. The following chemical equations demonstrate how various metals react with water:
The halogens are located on the left of the noble gases on the periodic table. These five toxic, non-metallic elements make up Group 17 of the periodic table and consist of: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). Although astatine is radioactive and only has short-lived isotopes, it behaves similar to iodine and is often included in the halogen group. Because the halogen elements have seven valence electrons, they only require one additional electron to form a full octet. This characteristic makes them more reactive than other non-metal groups.
Explanation: