-1 state of halogens is common and stable but -1 of Hydrogen is rare and extremely reactive. But they hydrogen atoms can also gain one electron similar to halogens. Hydrogen is the first element in the periodic table of Mendeleev - atomic number 1. Similarities to Metals. it has le, IP in nucleus. The two hydrogens are the same, but some periodic tables show hydrogen in both places to emphasize that hydrogen isn't really a member of the first group or the seventh group. Some reasons why hydrogen was placed in the group 1A elements are as follows: It has a valence electron of 1. H has 1 e- in the outer ring such as those in column 1, and likes to give it away forming H+, positive ion. Astatine should react very slowly with hydrogen, even when heated. Hydrogen is also found in a wide range of compounds throughout the earth including hydrocarbons, acids, and hydroxides. Thus it can lose an electron to achieve a stable configuration like alkali metals and hence can be placed in group 1 … Similarly, it can gain one electron to achieve stability.Like Group 17 elements,it can gain electron. Hence, it can also be placed above the halogen group. It forms covalent compounds like halogens unlike alkali metals. Hydrogen is a chemical element with atomic number 1 which means there are 1 protons and 1 electrons in the atomic structure.The chemical symbol for Hydrogen is H. With a standard atomic weight of circa 1.008, hydrogen is the lightest element on the periodic table. Each water molecule (H 2 O) contains two hydrogen atoms. Use the information to predict the reaction of astatine with hydrogen. Find an answer to your question give reason why hydrogen can be placed in group 1 (1a) and group 17 (7a) sahebrambani sahebrambani 5 minutes ago Chemistry Secondary School Give reason why hydrogen can be placed in group 1 (1a) and group 17 (7a) 2 See answers sahebrambani is waiting for your help. the main groups are numbered from 1 to 7 going from left to right, and the last group on the right is Group 0 the block in between Group 2 and Group 3 is where the transition metals are placed In others, you might find hydrogen placed independently of any group; somewhere at the top of the Periodic Table. Like group I elements, hydrogen has only one electron in its valence shell. Let us see how this plays out. Hydrogen also resembles halogens in many ways. Hydrogen can be placed in both group 1 and group 17 because its electronic configuration is similar to both the groups. Resemblance with alkali metals no. hi.. well hydrogen IS NOT in group 1 of the periodic table.. That is why position of hydrogen is still undecided. The most common place to find hydrogen on earth is in water. Where do you think should hydrogen be placed in the Modern periodic table? Add your answer and earn points. It can both lose as well as gain an electron. There are many reasons for including hydrogen among the elements in Group IA. As a result it can be placed in group 1, as it usually is, or with the halogens in group 17 (fig 4). Its +1 oxidation state is much stable like the others. First and foremost reason being that it is similar to alkali metals in electronic configuration(1s1) i.e. 3) In some hydrogen differs from both alkali metals and halogens. State the electronic configuration of hydrogen [at. Example. Hydrogen's Placement in the Periodic Table. Finally, hydrogen is sometimes placed separately from any group; this is based on its general properties being regarded as sufficiently different from those of the elements in any other group. There has been considerable discussion as to the placement of Hydrogen. 1) In some properties it resembles alkali metals.As such, it can be placed in group 1 of the periodic table along with alkali metals. this is because the electronic configaration of h2 is similar to alkali metal. Hydrogen is considered to be in a group of its own. The valance electronic configuration of hydrogen is the same with the group 1A elements. This leads to lower … Hydrogen can be placed in group number 1 or (but not normally) in group number 17 because it has some properties similar to both groups.. On one hand , it exhibits the property of alkali metals by losing one electron to get a positive charge ( H --> H + + e-). Still, If I'd be Moseley I'd place it above the alkali metals. THESE PROPERTIES LEAD TO THE UNEXPLAINED POSITION OF HYDROGEN Li (Z=3): K 2, L 1 have 1 valency. Group number indicates the number of valence electrons or outer electronic configuration. why Hydrogen could be placed in group I or group VII of the periodic table.? Actually, in most Periodic Tables, you shall find Hydrogen placed above Group 1 (but detached from it vertically). Element Hydrogen (H), Group 1, Atomic Number 1, s-block, Mass 1.008. single electron in outermost shell. Like group I elements, hydrogen has only one electron in its valence shell. Oxygen has an oxidation state of -2, so for this compound it is -6 (-2 charge x 3 atoms= -6). Hydrogen can be placed in group 1[1A] as it forms a positive ion as in HC1 like alkali metals H. Question 2. Group 1 metals are referred to as alkali metals and have a charge of +1 Group 2 metals are referred to as alkaline earth metals and have a charge of +2. IT IS JUST PLACED ABOVE group 1 of th table as it has valency one and cannot be placed with halogens as it has just one valence electron. It can get rid of one electron to attain noble gas configuration. Hydrogen can also be placed in Group 17, because it can acquire a second electron to form a hydride ion, H-, just as the other elements in Group 17 can form 1- ions. Like halogens, hydrogen is a gas, and exists as a diatomic molecule (H2). Hydrogen gas is made up of diatomic molecules designated as H 2. H can also be in column 17, because it only takes 1 e- to fill that outer ring, forming a H- ion, hydride. Answer: Electronic configuration of hydrogen is 1 i.e. it has le, IP in nucleus. Other properties are much similar. Electronic configuration of hydrogen is 1 i.e. atish1 atish1 13.03.2016 Chemistry Secondary School ... *but it is placed at the top of group 1 above the alkali metal. These s-block elements are found in Group 1 and Group 2 of the periodic table and are the most active metals. One electron in its valence shell substance in the Modern periodic table 75! 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