Table 2: Reaction of halogens with iron wool. An element X (atomic number 17) combines with an element Y (atomic number 20) to form a compound. The alkali metal electron configurations (group 1) always end with “s1” and the alkaline earth metals (group 2) always end with “s2”. Very few scientists handle fluorine because it is so dangerous. Thus, there are 7 electrons in the outermost shell of these elements. Therefore, astatine is a metalloid which prefers sharing or losing electrons to become an unstable and radioactive compound. Also write group number, period number and valency of ‘X’. The reaction is faster. The elements are Hydrogen and Helium with electronic configuration 1s 1 and 1s 2 This marks the complete filling of K shell. (adsbygoogle = window.adsbygoogle || []).push({}); © Copyright 2021 W3spoint.com. These 2 groups are know as “s block” elements . They share unpaired electrons to form covalent bonds as well. So these elements require only one electron to complete the octet. These 2 groups are know as “s block” elements. The members of this group 1 are as follows: 1. Sodium (Na) 4. The Same group elements have similar properties and reactivity. (ii) A common feature of the electronic configuration of the elements at the end of Period 2 and Period 3 is that the atoms have 8 electrons in their outermost shell. As all the elements in group 14 have 4 electrons in the outermost shell, the valency of Group-14 elements is 4. Table 1: Electronic configuration of group 17 elements. Although astatine is radioactive and only has short-lived isotopes, it behaves similar to iodine … 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. The halogens all have the general electron configuration ns2np5, giving them seven valence electrons. The electronic configurations of the elements in group 1: The atoms of all group 1 elements have similar chemical properties and reactions because they all have one electron in their outer shell. All rights reserved. The element misses out on the octet configuration by one electron. Reacts with almost anything instantly. (∵ Group no. The first example occurs in the case of the lanthanoids (elements having atomic numbers between 57 and 71).The lanthanoids have the general electron configuration [Kr]4d 10 4f i 5s 2 5p 6 5d 0 or 1 6s 2. where i is a number between 0 and 14. It will be helpful now to look at electron configurations also in the context of the periodic table. Group 1 elements are chemical elements having an unpaired electron in the outermost s orbital. Potassium (K) 5. They use these electrons in the bond formation in order to obtain octet configuration. The reaction is slow. There are seven electrons in the outermost shell. Properties of Halogens: Monovalency of Halogens: All halogen have shell electronic configuration is … The general electronic configuration is ns2np5 and the last electron occupies p orbital. p-Block Elements The p-Block Elements comprise those belonging to groups 13 to 18 and together with the s-block elements are called the Representative Elements or Main Group Elements. Properties and Trends in Element 14 1) Covalent Radius. Fluorine, on row 2, has a valence-shell configuration of 2s 2 2p 5; while that of chlorine is 3s 2 3p 5. Scandium would end in 3d1, titanium in 3d2, etc. The same goes for bromine (4s 2 4p 5 ), iodine (4s 2 4p 5 ), and astatine (5s 2 5p 5 ).Thus it is ironic that they are neighbors to the Group 8 noble gases, the least reactive among the elements. The alkali metal electron configurations (group 1) always end with “s 1 ” and the alkaline earth metals (group 2) always end with “s 2 ”. This results in the valence shell being shielded by more inner electron shells. 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? Note that only the energy level changes, but not the electron configuration at the highest energy level. Electrons: Electrons are negatively charged species that occupy a region of space outside the nucleus of an atom. All halogens have seven electrons in their outermost shell comprising completely filled s orbital and p orbital with 5 electrons. Hydrogen (H) 2. 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… (iii) If an element is in Group 17, it is likely to be non-metallic in character, while with one electron in its outermost energy level (shell), then it is likely to be metallic. Group-17 or VIIA Elements. 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. Actual configurations have not been verified. They can easily obtain a full octet by gaining one electron. Publish your article. Which group of elements has the valence configuration of {eq}ns^2np^2 {/eq}? Each group of elements having the same number of valence electrons. , 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. There is more attraction which makes it easier to gain an extra electron. Francium (Fr) Although hydrogen is in this group due to its electron configuration, it has characteristics distinct from alkali metals. Write the subshell electronic configuration of the element. So, they have an electronic configuration of s 2 p 2 in their valance shell. = 7 + 10 = 17) Question 11. The form of the periodic table is closely related to the electron configuration of the atoms of the elements. Electron Configuration Chart for All Elements in the Periodic Table. Forming compounds. The general electronic configuration is ns 2 np 5 and the last electron occupies p orbital. By sharing electrons in a covalent bond full outer electron shells are achieved. All the elements of group 17 have 7 electrons in its valence shell. For example, the all of the elements in group 3 beginning with scandium, all end in “d1”. All of the elements in group 16, beginning with oxygen, end with “p4”. Unlike the lighter group 17 elements, tennessine may not exhibit the chemical behavior common to the halogens. Answer: a. It contains hydrogen and alkali metals. Must be heated strongly and so does the iron wool. The ns2np6 electron configuration, known as the octet configuration, contains eight electrons and generally has the lowest energy and is the most stable. They are one electron short of having full outer s … Table 1: Electronic configuration of group 17 elements. The elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) are called the halogens. Hence they are kept in group VII-A (17) of a periodic table, before inert gases. When one looks at the Group 16 elements, the electronic configuration of all the elements in that group is categorized by the presence of six electrons in their last shell or the valence shell. Likewise, the outer shell moves further from the nucleus. An element ‘X’ has mass number 35 and number of neutrons 18. There are 118 elements … To form a compound in a chemical reaction, electrons must be exchanged. As we learned earlier, each neutral atom has a number of electrons equal to its number of protons. Its group number is 17 as it has 7 valence electrons. As the outer shell moves further from the positive attraction of the nucleus, attraction towards incoming electron decreases due to overall reduced negative charge on the atom. google_ad_client = "pub-0644478549845373"; The elements in group eighteen are Helium, Neon, Argon, Krypton, Xenon, and Radon. The rows in the periodic table show increasing energy levels and the levels rise as one moves up the list of halogens. The electron when reaching the fluorine octet stays intact due to closeness to the nucleus. The electronic configuration of any element determines its physical state and reactivity with other elements. Three shells are K, L, M. For example, fluorine, chlorine, bromine, and iodine routinely accept an electron to achieve the more stable electronic configuration of a noble gas, obtaining eight electrons in their valence shells instead of seven. Hence, they are monovalent with common valency of -1.Fluorine is the most reactive halogen because the electron it is attracting is coming into a shell closest to the positive nucleus. google_ad_height = 60; Atomic radius increases down Group 17 from top to bottom. The “f  block” elements are those at the bottom of the periodic table that we call the lanthanide and actinide groups. These elements are all in all alluded to as noble gasses. Reacts with heated iron wool very quickly. (b) This element is a non-metal as it gains one electron to complete its outermost shell and elements which gain electrons … Fluorides of Krypton and compounds of xenon, such as Oxides, fluorides, and oxyfluorides, are well known. The transition elements are called “d block” elements and always end with 1 or more “d electrons”. Electron configurations are the summary of where the electrons are around a nucleus. Learn more about Group 17 Elements here. These elements’ electron configurations always end with one or more “f  electrons.”. Example: If the electronic configuration of an element is 2, 8, 7. In group 4A or 14, all elements end in p2. Therefore, these are very reactive non-metals. Halogens gain an electron in reactions to form negative ions with a -1 charge and they are 1 electron less than a full octet. How to Find Electron … All the Group 17 elements are molecules containing two atoms. Caesium (Cs) 7. They can easily obtain a full octet by gaining one electron. It is the first column of the s block of the periodic table. The periodic table can be broken into “blocks” that show what the last electron added to the electron configuration is. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. google_ad_slot = "2147476616"; google_ad_width = 468; All halogens have seven electrons in their outermost shell comprising completely filled s orbital and p orbital with 5 electrons. For instance, hydrogen exists as a gas, while other ele… They obtain the octet by accepting one electron to produce a univalent anion, X– (F–, Cl–, Br– and I–). (AI 2016) Answer: Atomic number of X = Mass number of X – No of neutrons = 35 – 18 = 17 Therefore Electronic configuration of X = 2, 8, 7 Group number =17 What we will do now is place those electrons into an arrangement around the nucleus that indicates their energy and the shape of the orbital in which they are located. 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). The element X in group 17 has 3 shells. The expression "noble gases" infers that these elements have a tendency to be chemically inert or un-reactive. They can complete their octet either by picking up an electron or sharing an electron. And so it goes. The general rule is that the element's electron configuration ends in d and whatever place they are in. The s-, p- and d-block elements of the periodic table are arranged into these columns or groups. The general electronic configuration of group 17 is: ns2np5. For the transition metals, groups 3-12, there are many exceptions. All Group 17 (group VIIA or halogen) elements have 7 valence electrons (7 electrons in the valence shell or highest energy level ). For example, all the elements in group 13, beginning with boron, end with “p1”. Fig 1: Arrangement of electrons in the first three elements of the halogen family. 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. The elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) are called the halogens. 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