group 17 elements electronic configuration

google_ad_width = 468; They can easily obtain a full octet by gaining one electron. It is the first column of the s block of the periodic table. Please contribute and help others. Electronegativity decreases down group 17 from top to bottom. The reaction is faster. The element misses out on the octet configuration by one electron. The elements are Hydrogen and Helium with electronic configuration 1s 1 and 1s 2 This marks the complete filling of K shell. Which group of elements has the valence configuration of {eq}ns^2np^2 {/eq}? The general electronic configuration is ns2np5 and the last electron occupies p orbital. An element X (atomic number 17) combines with an element Y (atomic number 20) to form a compound. These 2 groups are know as “s block” elements . Fluorides of Krypton and compounds of xenon, such as Oxides, fluorides, and oxyfluorides, are well known. Thus, these elements look out to either lose one electron and form a covalent bond or gain one electron and form an ionic bond. Likewise, the outer shell moves further from the nucleus. 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. If so, a. 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. 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. Reacts with heated iron wool very quickly. The general electronic configuration of the d-block elements is (n − 1)d 1–10 ns 0–2.Here "(noble gas)" is the configuration of the last noble gas preceding the atom in question, and n is the highest principal quantum number of an occupied orbital in that atom. Table 1: Electronic configuration of group 17 elements. The atoms of each element gain more shells and increase in size going down the group. 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 general rule is that the element's electron configuration ends in d and whatever place they are in. Actual configurations have not been verified. Group 1 elements are chemical elements having an unpaired electron in the outermost s orbital. (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 google_ad_client = "pub-0644478549845373"; 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). They can easily obtain a full octet by gaining one electron. Note that only the energy level changes, but not the electron configuration at the highest energy level. Then its period number is 3 as it has three electrons shells. (b) This element is a non-metal as it gains one electron to complete its outermost shell and elements which gain electrons … The halogens all have the general electron configuration ns2np5, giving them seven valence electrons. (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. All Group 17 (group VIIA or halogen) elements have 7 valence electrons (7 electrons in the valence shell or highest energy level ). The electronic configuration of any element determines its physical state and reactivity with other elements. Login, Best Place for Technologies and Academics Tutorial, p-Block Elements: Group 17 (Electronic configuration). google_ad_slot = "2147476616"; Learn more about Group 17 Elements here. They can complete their octet either by picking up an electron or sharing an electron. The oxidation states of all the elements belonging to this group are -1. So, they have an electronic configuration of s 2 p 2 in their valance shell. 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. Hydrogen (H) 2. Although astatine is radioactive and only has short-lived isotopes, it behaves similar to iodine … Fig 1: Arrangement of electrons in the first three elements of the halogen family. 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. They are one electron short of having full outer s … Publish your article. These elements are a part of the p block. The halogens all have the general electron configuration n s 2n p 5, giving them seven valence electrons. Lithium (Li) 3. Sodium (Na) 4. Table 2: Reaction of halogens with iron wool. The form of the periodic table is closely related to the electron configuration of the atoms of the elements. Write the subshell electronic configuration of the element. The general electronic configuration is ns 2 np 5 and the last electron occupies p orbital. As we learned earlier, each neutral atom has a number of electrons equal to its number of protons. Answer: a. For example, all the elements in group 13, beginning with boron, end with “p1”. And so it goes. The element X in group 17 has 3 shells. All of the elements in group 16, beginning with oxygen, end with “p4”. The reaction is slow. Therefore fluorine is the most reactive and it produces stable ionic salts and covalent compounds due to highest electronegativity. Thus, there are 7 electrons in the outermost shell of these elements. This results in the valence shell being shielded by more inner electron shells. There are seven electrons in the outermost shell. Must be heated strongly and so does the iron wool. There is more attraction which makes it easier to gain an extra electron. The elements of Group 17 (fluorine, chlorine, bromine, iodine, and astatine) are called the halogens. The Same group elements have similar properties and reactivity. 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. Therefore, astatine is a metalloid which prefers sharing or losing electrons to become an unstable and radioactive compound. Must be warmed and the iron wool heated. 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. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. Fluorine, on row 2, has a valence-shell configuration of 2s 2 2p 5; while that of chlorine is 3s 2 3p 5. The rows in the periodic table show increasing energy levels and the levels rise as one moves up the list of halogens. Three shells are K, L, M. 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? As all the elements in group 14 have 4 electrons in the outermost shell, the valency of Group-14 elements is 4. Caesium (Cs) 7. (∵ Group no. The valence shell electronic configuration of these electrons is ns2np5. Example: If the electronic configuration of an element is 2, 8, 7. 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. The members of this group 1 are as follows: 1. All halogens have seven electrons in their outermost shell comprising completely filled s orbital and p orbital with 5 electrons. Very few scientists handle fluorine because it is so dangerous. Write atomic number and electronic configuration of ‘X’. All the Group 17 elements are molecules containing two atoms. Each group of elements having the same number of valence electrons. Its group number is 17 as it has 7 valence electrons. All the elements of group 17 have 7 electrons in its valence shell. These elements are all in all alluded to as noble gasses. 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 “f  block” elements are those at the bottom of the periodic table that we call the lanthanide and actinide groups. google_ad_height = 60; Electron configurations are the summary of where the electrons are around a nucleus. “P block” elements are all those in groups 13-18 and always end with 1 or more “p” electrons. These 2 groups are know as “s block” elements. So these elements require only one electron to complete the octet. To form a compound in a chemical reaction, electrons must be exchanged. //-->, 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. Francium (Fr) Although hydrogen is in this group due to its electron configuration, it has characteristics distinct from alkali metals. For the transition metals, groups 3-12, there are many exceptions. They are one electron short of having full outer s … = 7 + 10 = 17) Question 11. All rights reserved. These elements tend to show patterns in atomic radius, ionization energy, and electronegativity. Electron Configuration Chart for All Elements in the Periodic Table. Rhubidium (Rh) 6. They share unpaired electrons to form covalent bonds as well. They use these electrons in the bond formation in order to obtain octet configuration. For example, all the elements of group 2 have an electron configuration of [E] ns 2 (where [E] is an inert gas configuration), and have notable similarities in their chemical properties.

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