The form of the periodic table is closely related to the electron configuration of the atoms of the elements. google_ad_height = 60; Learn more about Group 17 Elements here. Physical and Chemical Properties of Aldehydes and Ketones, Oxidation states of d and f Block Elements, Electronic Configuration of Group 14 Elements, Physical and chemical properties of Group 16 elements. For example, the s sublevel can only hold two electrons, so the 1s is filled at helium (1s 2).The p sublevel can hold six electrons, the d sublevel can hold 10 electrons, and the f sublevel can hold 14 electrons. b. For instance, hydrogen exists as a gas, while other ele… There are seven electrons in the outermost shell. Fluorine (F), Chlorine (Cl), Bromine (Br), Iodine (I), Astatine (At) in the periodic table belong to group-17, or VIIA with the general electronic configuration of valence electron ns 2 np 5, where n = 2 to 6. Electrons: Electrons are negatively charged species that occupy a region of space outside the nucleus of an atom. The reaction is slow. The oxidation states of all the elements belonging to this group are -1. Login, Best Place for Technologies and Academics Tutorial, p-Block Elements: Group 17 (Electronic configuration). If so, a. All Group 17 (group VIIA or halogen) elements have 7 valence electrons (7 electrons in the valence shell or highest energy level ). All the Group 17 elements are molecules containing two atoms. An element ‘X’ has mass number 35 and number of neutrons 18. To form a compound in a chemical reaction, electrons must be exchanged. The electronic configuration of any element determines its physical state and reactivity with other elements. The periodic table can be broken into “blocks” that show what the last electron added to the electron configuration is. These 2 groups are know as “s block” elements. The halogens all have the general electron configuration ns2np5, giving them seven valence electrons. Table 1: Electronic configuration of group 17 elements. The atoms of each element gain more shells and increase in size going down the group. For example, all the elements in group 13, beginning with boron, end with “p1”. = 7 + 10 = 17) Question 11. Halogens gain an electron in reactions to form negative ions with a -1 charge and they are 1 electron less than a full octet. The expression "noble gases" infers that these elements have a tendency to be chemically inert or un-reactive. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. The elements are Hydrogen and Helium with electronic configuration 1s 1 and 1s 2 This marks the complete filling of K shell. google_ad_client = "pub-0644478549845373"; This results in the valence shell being shielded by more inner electron shells. An element X (atomic number 17) combines with an element Y (atomic number 20) to form a compound. Group 17 elements [non-metals] gain 1 electron and from an ion N⁻ ... Group 18 elements do not react and form ions because they already have a stable electron configuration. (adsbygoogle = window.adsbygoogle || []).push({}); © Copyright 2021 W3spoint.com. Answer: a. Likewise, the outer shell moves further from the nucleus. These elements’ electron configurations always end with one or more “f  electrons.”. They share unpaired electrons to form covalent bonds as well. So these elements require only one electron to complete the octet. The general electronic configuration is ns 2 np 5 and the last electron occupies p orbital. The transition elements are called “d block” elements and always end with 1 or more “d electrons”. The valence shell electronic configuration of these electrons is ns2np5. Fig 1: Arrangement of electrons in the first three elements of the halogen family. Each group of elements having the same number of valence electrons. These elements require one electron to finish their octet. There are 118 elements … Must be warmed and the iron wool heated. Hence they are kept in group VII-A (17) of a periodic table, before inert gases.