Fluorides of Krypton and compounds of xenon, such as Oxides, fluorides, and oxyfluorides, are well known. Group-17 or VIIA Elements. There are 118 elements … Unlike the lighter group 17 elements, tennessine may not exhibit the chemical behavior common to the halogens. There are seven electrons in the outermost shell. There is more attraction which makes it easier to gain an extra electron. Therefore, these are very reactive non-metals. The ns2np6 electron configuration, known as the octet configuration, contains eight electrons and generally has the lowest energy and is the most stable. The general electronic configuration is ns 2 np 5 and the last electron occupies p orbital. Therefore, astatine is a metalloid which prefers sharing or losing electrons to become an unstable and radioactive compound. The elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) are called the halogens. The valence shell electronic configuration of these electrons is ns2np5. Francium (Fr) Although hydrogen is in this group due to its electron configuration, it has characteristics distinct from alkali metals. An element ‘X’ has mass number 35 and number of neutrons 18. The oxidation states of all the elements belonging to this group are -1. The electron when reaching the fluorine octet stays intact due to closeness to the nucleus. The members of this group 1 are as follows: 1. Properties of Halogens: Monovalency of Halogens: All halogen have shell electronic configuration is … Lithium (Li) 3. Write the period number, c. What will be the chemical formula of the compound formed if the element X reacts with element Y of the third period which contains one electron in the p subshell? By sharing electrons in a covalent bond full outer electron shells are achieved. The s-, p- and d-block elements of the periodic table are arranged into these columns or groups. Write the subshell electronic configuration of the element. Table 2: Reaction of halogens with iron wool. These elements are all in all alluded to as noble gasses. The atoms of each element gain more shells and increase in size going down the group. All halogens have seven electrons in their outermost shell comprising completely filled s orbital and p orbital with 5 electrons. The compounds of the s-block elements, with the exception of those of beryllium are predominantly ionic. The alkali metal electron configurations (group 1) always end with “s1” and the alkaline earth metals (group 2) always end with “s2”. The element misses out on the octet configuration by one electron. It will be helpful now to look at electron configurations also in the context of the periodic table. Learn more about Group 17 Elements here. For the transition metals, groups 3-12, there are many exceptions. All of the elements in group 16, beginning with oxygen, end with “p4”. Electron configurations are the summary of where the electrons are around a nucleus. The general electronic configuration of group 17 is: ns2np5. (adsbygoogle = window.adsbygoogle || []).push({}); © Copyright 2021 W3spoint.com. An element X (atomic number 17) combines with an element Y (atomic number 20) to form a compound. , Electrons and Sublevels  Electron Configurations and the Periodic Table  Writing Electron Configurations  Box and Arrow Configurations using Pauli Exclusion Principle and Hund's Rule   Quantum Numbers, Electron Configurations and the Periodic Table, Electron configurations and the periodic table. Reacts with almost anything instantly. Which group of elements has the valence configuration of {eq}ns^2np^2 {/eq}? This results in the valence shell being shielded by more inner electron shells. Atomic radius increases down Group 17 from top to bottom. They use these electrons in the bond formation in order to obtain octet configuration. Write atomic number and electronic configuration of ‘X’. For example, the all of the elements in group 3 beginning with scandium, all end in “d1”. The periodic table can be broken into “blocks” that show what the last electron added to the electron configuration is. They share unpaired electrons to form covalent bonds as well. b. The rows in the periodic table show increasing energy levels and the levels rise as one moves up the list of halogens. The element X in group 17 has 3 shells. Then its period number is 3 as it has three electrons shells. Here is a summary of the types of orbitals and how many electrons each can contain: So based on what we know about the quantum numbers and using the char… “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. All halogens have seven electrons in their outermost shell comprising completely filled s orbital and p orbital with 5 electrons. The penultimate shell of carbon contains the s 2 electrons, silicon has s 2 p 6 electrons and germanium contains the s 2 p 6 d 10 electrons and is unsaturated. All the elements of group 17 have 7 electrons in its valence shell. They can complete their octet either by picking up an electron or sharing an electron. If so, a. Table 1: Electronic configuration of group 17 elements. The transition elements are called “d block” elements and always end with 1 or more “d electrons”. The electronic configuration of any element determines its physical state and reactivity with other elements. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. The reaction is slow. Therefore fluorine is the most reactive and it produces stable ionic salts and covalent compounds due to highest electronegativity. Its group number is 17 as it has 7 valence electrons. For example, all the elements in group 13, beginning with boron, end with “p1”. 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