{"id":12628,"date":"2026-06-01T13:03:34","date_gmt":"2026-06-01T13:03:34","guid":{"rendered":"https:\/\/www.vedprep.com\/exams\/?p=12628"},"modified":"2026-06-01T13:11:45","modified_gmt":"2026-06-01T13:11:45","slug":"synthesis-and-reactions-of-hydrides","status":"publish","type":"post","link":"https:\/\/www.vedprep.com\/exams\/iit-jam\/synthesis-and-reactions-of-hydrides\/","title":{"rendered":"Synthesis and reactions of Hydrides For IIT JAM 2027"},"content":{"rendered":"<p data-path-to-node=\"1\">If you are gearing up for the IIT JAM, you already know that the inorganic chemistry section can be a serious rank-booster if you play your cards right. Right in the middle of that syllabus sits a massive, high-yield topic: the <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>.<\/p>\n<p data-path-to-node=\"2\">Whether you are looking at main group elements or transition metals in <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>, how these compounds form and behave tells us a lot about bonding, periodic trends, and chemical reactivity.<\/p>\n<h2><strong>Understanding the Syllabus and Key Textbooks<\/strong><\/h2>\n<p data-path-to-node=\"5\"><b data-path-to-node=\"1\" data-index-in-node=\"228\">Synthesis and reactions of hydrides<\/b> falls squarely under the main block of Inorganic Chemistry in the <a href=\"https:\/\/jam2026.iitb.ac.in\/files\/syllabus_CY.pdf\" rel=\"nofollow noopener\" target=\"_blank\"><strong>IIT JAM official syllabus<\/strong><\/a>. If you want to crack top-tier competitive exams like IIT JAM, CSIR NET, or GATE, you really need to get a firm grip on this area.<\/p>\n<p data-path-to-node=\"6\">To build your foundation on <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>, you can dive into classic standard textbooks like <i data-path-to-node=\"6\" data-index-in-node=\"76\">Inorganic Chemistry<\/i> by J.D. Lee or <i data-path-to-node=\"6\" data-index-in-node=\"111\">Advanced Inorganic Chemistry<\/i> by Cotton and Wilkinson (and for specialized reactions, Johnson and Gilbert&#8217;s work is fantastic). These books layout everything you need to know about hydrides, breaking down how we make them and how they react.<\/p>\n<p data-path-to-node=\"7\">At <a href=\"https:\/\/www.vedprep.com\/online-courses\"><strong>VedPrep<\/strong><\/a>, we always tell our students that mastering the preparation methods and periodic properties of these compounds is the absolute secret weapon for scoring high in the exam.<\/p>\n<h2><strong>Overview: Synthesis and reactions of Hydrides For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"10\">Let&#8217;s break it down simply: <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides <\/b>are just compounds where hydrogen bonds with another element. But based on who hydrogen is partnering up with, we classify them into three main buckets: <b data-path-to-node=\"10\" data-index-in-node=\"190\">ionic (saline), covalent (molecular), and metallic (interstitial) hydrides<\/b>.<\/p>\n<ul data-path-to-node=\"11\">\n<li>\n<p data-path-to-node=\"11,0,0\"><b data-path-to-node=\"11,0,0\" data-index-in-node=\"0\">Ionic Hydrides:<\/b> Think of these as the pairing between hydrogen and highly electropositive metals, mostly from Group 1 and Group 2 (like <span class=\"math-inline\" data-math=\"\\text{NaH}\" data-index-in-node=\"136\">NaH<\/span>\u00a0or <span class=\"math-inline\" data-math=\"\\text{CaH}_2\" data-index-in-node=\"150\">CaH<sub>2<\/sub><\/span>). Here, hydrogen acts as the hydride ion (<span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"205\">H<sup>&#8211;<\/sup><\/span>).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"11,1,0\"><b data-path-to-node=\"11,1,0\" data-index-in-node=\"0\">Covalent Hydrides:<\/b> These happen when hydrogen shares electrons with non-metals or metalloids. Think of everyday gases like methane (<span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"132\">CH<sub>4<\/sub><\/span>) or ammonia (<span class=\"math-inline\" data-math=\"\\text{NH}_3\" data-index-in-node=\"157\">NH<sub>3<\/sub><\/span>).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"11,2,0\"><b data-path-to-node=\"11,2,0\" data-index-in-node=\"0\">Metallic Hydrides:<\/b> These form when hydrogen sneaks into the gaps or cavities inside the crystal lattices of transition metals (like <span class=\"math-inline\" data-math=\"\\text{LaNi}_5\" data-index-in-node=\"132\">LaNi<sub>5<\/sub><\/span> or <span class=\"math-inline\" data-math=\"\\text{TiH}_2\" data-index-in-node=\"149\">TiH<sub>2<\/sub><\/span>).<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"12\">When it comes to getting these compounds of <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides <\/b>ready in the lab, we usually rely on three main paths:<\/p>\n<ol start=\"1\" data-path-to-node=\"13\">\n<li>\n<p data-path-to-node=\"13,0,0\"><b data-path-to-node=\"13,0,0\" data-index-in-node=\"0\">Direct Synthesis:<\/b> Literally forcing hydrogen gas to react directly with another element. This usually needs a lot of heat and high pressure to get going.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"13,1,0\"><b data-path-to-node=\"13,1,0\" data-index-in-node=\"0\">Indirect Synthesis:<\/b> Using a clever workaround, like reacting a metal halide with a strong reducing agent like <span class=\"math-inline\" data-math=\"\\text{LiAlH}_4\" data-index-in-node=\"110\">LiAlH<sub>4<\/sub><\/span>.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"13,2,0\"><b data-path-to-node=\"13,2,0\" data-index-in-node=\"0\">Disproportionation Reactions:<\/b> Where a compound essentially splits its own identity, oxidizing and reducing at the same time to leave you with a hydride.<\/p>\n<\/li>\n<\/ol>\n<p data-path-to-node=\"14\">Once you have them, their properties vary wildly. As per <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides, <\/b>their thermal stability changes drastically as you move down a group in the periodic table. Their electrical conductivity is totally different too\u2014some conduct electricity beautifully when melted, while others act as perfect insulators. They also show completely different chemical reactivity when you drop them into water or acids, often releasing a massive burst of hydrogen gas.<\/p>\n<p data-path-to-node=\"14\">Here is a quick cheat sheet to help you see the differences at a glance:<\/p>\n<table style=\"width: 100%; height: 222px;\" data-path-to-node=\"16\">\n<thead>\n<tr style=\"height: 24px;\">\n<td style=\"height: 24px;\"><strong>Property<\/strong><\/td>\n<td style=\"height: 24px;\"><strong>Ionic Hydrides<\/strong><\/td>\n<td style=\"height: 24px;\"><strong>Covalent Hydrides<\/strong><\/td>\n<td style=\"height: 24px;\"><strong>Metallic Hydrides<\/strong><\/td>\n<\/tr>\n<\/thead>\n<tbody>\n<tr style=\"height: 51px;\">\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,1,0,0\"><b data-path-to-node=\"16,1,0,0\" data-index-in-node=\"0\">Bonding Type<\/b><\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,1,1,0\">Primarily Ionic (<span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"17\">H<sup>&#8211;<\/sup><\/span>\u00a0ion)<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,1,2,0\">Covalent sharing<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,1,3,0\">Metallic \/ Interstitial<\/span><\/td>\n<\/tr>\n<tr style=\"height: 48px;\">\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,2,0,0\"><b data-path-to-node=\"16,2,0,0\" data-index-in-node=\"0\">Physical Appearance<\/b><\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,2,1,0\">Crystalline white solids<\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,2,2,0\">Gases, liquids, or volatile solids<\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,2,3,0\">Metallic solids, often non-stoichiometric<\/span><\/td>\n<\/tr>\n<tr style=\"height: 48px;\">\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,3,0,0\"><b data-path-to-node=\"16,3,0,0\" data-index-in-node=\"0\">Conductivity<\/b><\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,3,1,0\">Conducts in molten state<\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,3,2,0\">Insulators<\/span><\/td>\n<td style=\"height: 48px;\"><span data-path-to-node=\"16,3,3,0\">Excellent electronic conductors<\/span><\/td>\n<\/tr>\n<tr style=\"height: 51px;\">\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,4,0,0\"><b data-path-to-node=\"16,4,0,0\" data-index-in-node=\"0\">Reaction with <span class=\"math-inline\" data-math=\"\\text{H}_2\\text{O}\" data-index-in-node=\"14\">H<sub>2<\/sub>O<\/span><\/b><\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,4,1,0\">Vigorous, releases <span class=\"math-inline\" data-math=\"\\text{H}_2\" data-index-in-node=\"19\">H<sub>2<\/sub><\/span>\u00a0gas<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,4,2,0\">Mostly unreactive (except custom lewis acids)<\/span><\/td>\n<td style=\"height: 51px;\"><span data-path-to-node=\"16,4,3,0\">Generally inert at room temp<\/span><\/td>\n<\/tr>\n<\/tbody>\n<\/table>\n<h2 data-path-to-node=\"18\"><strong>Common Misconceptions in Synthesis and Reactions of Hydrides For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"19\">A huge trap that many JAM aspirants fall into is assuming that every single hydride out there is highly reactive and ready to blow up. It is easy to see why people think this\u2014most textbook questions show ionic hydrides reacting violently with air or water. But that is definitely not the whole story.<\/p>\n<p data-path-to-node=\"19\"><b data-path-to-node=\"20,0\" data-index-in-node=\"0\">Reality Check:<\/b> While ionic hydrides like lithium hydride (<span class=\"math-inline\" data-math=\"\\text{LiH}\" data-index-in-node=\"58\">LiH<\/span>) or sodium hydride (<span class=\"math-inline\" data-math=\"\\text{NaH}\" data-index-in-node=\"89\">NaH<\/span>) are incredibly aggressive because they want to shed that extra electron, covalent hydrides are a completely different story. The methane (<span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"239\">CH<sub>4<\/sub><\/span>) in your kitchen stove or the ammonia (<span class=\"math-inline\" data-math=\"\\text{NH}_3\" data-index-in-node=\"290\">NH<sub>3<\/sub><\/span>) in a lab bottle is perfectly stable at room temperature and won&#8217;t react unless you give it a major spark.<\/p>\n<p data-path-to-node=\"21\">The main takeaway here is that hydride reactivity depends entirely on the type of bond it holds. Don&#8217;t paint them all with the same brush. For example, while <span class=\"math-inline\" data-math=\"\\text{LiH}\" data-index-in-node=\"158\">LiH<\/span> is super reactive, aluminum hydride (<span class=\"math-inline\" data-math=\"\\text{AlH}_3\" data-index-in-node=\"206\">AlH<sub>3<\/sub><\/span>) is actually less stable structurally but isn&#8217;t quite as violent as you might expect. Keeping these subtle differences straight in your head is what separates a top ranker from the rest of the pack.<\/p>\n<h2 data-path-to-node=\"23\"><strong>Real-World Applications of Synthesis and Reactions of Hydrides For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"24\">To make this concrete, let&#8217;s step out of the exam hall for a second. Imagine a giant industrial oil refinery. They handle heavy crude oil that is packed with messy impurities like sulfur and nitrogen. To clean it up and turn it into the clean petrol or diesel we put in cars, engineers pump in hydrogen gas under intense conditions to create temporary hydride intermediates on metal catalysts. This process strips away the bad stuff, leaving behind high-quality, environmentally friendly fuel.<\/p>\n<p data-path-to-node=\"25\">Out in the commercial world, these reactions show up everywhere:<\/p>\n<ul data-path-to-node=\"26\">\n<li>\n<p data-path-to-node=\"26,0,0\"><b data-path-to-node=\"26,0,0\" data-index-in-node=\"0\">Catalytic Reactions and Fuel Cells:<\/b> In pharma labs, chemists use sodium borohydride (<span class=\"math-inline\" data-math=\"\\text{NaBH}_4\" data-index-in-node=\"85\">NaBH<sub>4<\/sub><\/span>) as a go-to reducing agent to build complex drug molecules. Meanwhile, clean energy cars run on proton-exchange membrane fuel cells that use hydrogen to generate electricity, leaving nothing behind but pure water vapor.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"26,1,0\"><b data-path-to-node=\"26,1,0\" data-index-in-node=\"0\">Hydrogen Storage:<\/b> Storing gas is incredibly tough because it takes up too much space. Instead, scientists use alloys like <span class=\"math-inline\" data-math=\"\\text{LaNi}_5\" data-index-in-node=\"122\">LaNi<sub>5<\/sub><\/span> to soak up hydrogen gas like a sponge, packing it tightly into a solid form (<span class=\"math-inline\" data-math=\"\\text{LaNi}_5\\text{H}_6\" data-index-in-node=\"213\">LaNi<sub>5<\/sub>H<sub>6<\/sub><\/span>) that is perfectly safe to transport.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"26,2,0\"><b data-path-to-node=\"26,2,0\" data-index-in-node=\"0\">Green Energy Production:<\/b> Teams are using solar energy and custom catalysts to split water apart, capturing hydrogen directly through photocatalysis.<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"27\">Of course, doing this in real life means balancing tight constraints like extreme pressures, sensitive temperatures, and tricky pH levels. But mastering these materials is paving the way for sustainable industrial operations worldwide.<\/p>\n<h2 data-path-to-node=\"29\"><strong>Strategies for Exam Preparation: Synthesis and Reactions of Hydrides For IIT JAM<\/strong><\/h2>\n<p data-path-to-node=\"30\">If you want to clear the IIT JAM chemistry cutoff and aim for the IITs, you need a strategy that goes beyond just memorizing reactions. You need to understand the <i data-path-to-node=\"30\" data-index-in-node=\"163\">why<\/i> behind the chemical behavior.<\/p>\n<p data-path-to-node=\"31\"><strong>Key Subtopics to Focus On:<\/strong><\/p>\n<ul data-path-to-node=\"32\">\n<li>\n<p data-path-to-node=\"32,0,0\">The exact preparation methods for ionic, covalent, and metallic hydrides (watch out for the reagents!).<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"32,1,0\">Reactions of hydrides with water, acids, organic functional groups, and Lewis bases.<\/p>\n<\/li>\n<li>\n<p data-path-to-node=\"32,2,0\">Periodic trends in the thermal stability and reducing power of covalent hydrides (especially Groups 14 to 17).<\/p>\n<\/li>\n<\/ul>\n<p data-path-to-node=\"33\">The best way to prepare is to stop staring at the theory and start solving actual problems. Practicing numerical questions and structural prediction problems is what makes the theory stick. At <a href=\"https:\/\/www.vedprep.com\/online-courses\/iit-jam\"><strong>VedPrep<\/strong><\/a>, we spend a lot of time walking students through the exact question patterns and marking schemes seen in previous years. If you focus your energy on these high-weightage areas and practice consistently, you will feel completely confident when exam day rolls around.<\/p>\n<h2 data-path-to-node=\"35\"><strong>Worked Example: Synthesis and Reaction of a Covalent Hydride<\/strong><\/h2>\n<p data-path-to-node=\"36\">Let&#8217;s look at how covalent hydrides act when we put them to work. Take methane (<span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"80\">CH<sub>4<\/sub><\/span>) as our model covalent hydride. Unlike ionic hydrides, it doesn&#8217;t have an eager <span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"172\">$\\text{H}^-$<\/span> ion waiting to jump out. Instead, it relies on radical pathways to swap its atoms.<\/p>\n<p data-path-to-node=\"37\"><strong>Question:<\/strong><\/p>\n<p data-path-to-node=\"38\">Explain the synthesis and reaction of methane (<span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"47\">CH<sub>4<\/sub><\/span>) when treated with chlorine gas (<span class=\"math-inline\" data-math=\"\\text{Cl}_2\" data-index-in-node=\"92\">Cl<sub>2<\/sub><\/span>) under sunlight.<\/p>\n<p data-path-to-node=\"39\"><strong>Solution:<\/strong><\/p>\n<p data-path-to-node=\"40\">When you mix methane with chlorine gas in the presence of ultraviolet (UV) light, you trigger a free-radical substitution reaction. The light snaps the chlorine molecule apart into highly reactive chlorine radicals, which then attack the stable <span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"245\">CH<sub>4<\/sub><\/span>\u00a0bonds.<\/p>\n<p><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-20302 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/ultraviolet-UV-300x50.png\" alt=\"ultraviolet (UV)\" width=\"300\" height=\"50\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/ultraviolet-UV-300x50.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/ultraviolet-UV.png 438w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p>In this process, we swap a hydrogen atom out for a chlorine atom, giving us chloromethane (<span class=\"math-inline\" data-math=\"\\text{CH}_3\\text{Cl}\" data-index-in-node=\"91\">CH<sub>3<\/sub>Cl<\/span>) and hydrogen chloride (<span class=\"math-inline\" data-math=\"\\text{HCl}\" data-index-in-node=\"136\">HCl<\/span>) gas. This classic reaction is a favorite in the <b data-path-to-node=\"42\" data-index-in-node=\"196\">synthesis and reactions of hydrides<\/b> question bank because it perfectly highlights how stable covalent hydrides need a high-energy pathway to react.<\/p>\n<h2 data-path-to-node=\"44\"><strong>Deeper Dive into Ionic and Metallic Hydrides<\/strong><\/h2>\n<p data-path-to-node=\"45\">Let&#8217;s look closer at how we make ionic hydrides in <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>. We can pull this off using direct reactions, indirect pathways, or even disproportionation tricks.<\/p>\n<p data-path-to-node=\"46\">For the direct route, you heat up an alkali metal with hydrogen gas under high pressure. For example, if you want to make lithium hydride (<span class=\"math-inline\" data-math=\"\\text{LiH}\" data-index-in-node=\"139\">LiH<\/span>), you react pure lithium metal with hydrogen gas:<\/p>\n<p data-path-to-node=\"46\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-full wp-image-20303 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Metallic-Hydrides.png\" alt=\"Metallic Hydrides\" width=\"282\" height=\"83\" \/><\/p>\n<p data-path-to-node=\"48\">On the other hand, indirect synthesis might involve reacting a metal compound with an existing hydride or reducing agent to get what you need.<\/p>\n<p data-path-to-node=\"49\">Once you form these ionic hydrides from <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>, they behave like classic salts. They form beautiful crystalline solids and have high melting points. While they won&#8217;t conduct electricity as a solid, the moment you melt them down, the ions can move freely, allowing them to conduct electricity efficiently.<\/p>\n<p data-path-to-node=\"50\">And if you drop an ionic hydride like sodium hydride (<span class=\"math-inline\" data-math=\"\\text{NaH}\" data-index-in-node=\"54\">NaH<\/span>) into water, it reacts violently, pulling a proton from the water to create a massive release of hydrogen gas and leaving a basic solution behind:<\/p>\n<p data-path-to-node=\"50\"><img loading=\"lazy\" decoding=\"async\" class=\"alignnone size-medium wp-image-20304 aligncenter\" src=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Transition-metals-300x53.png\" alt=\"Transition metals\" width=\"300\" height=\"53\" srcset=\"https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Transition-metals-300x53.png 300w, https:\/\/www.vedprep.com\/exams\/wp-content\/uploads\/Transition-metals.png 405w\" sizes=\"(max-width: 300px) 100vw, 300px\" \/><\/p>\n<p data-path-to-node=\"50\">Transition metals handle things differently in <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>. Metallic hydrides form when transition metals simply absorb hydrogen gas into the empty pockets of their metal structures. These materials still conduct electricity just like regular metals and are the ultimate candidates for safe hydrogen storage tech.<\/p>\n<h2 data-path-to-node=\"54\"><strong>Advanced Materials and the Hydrogen Economy<\/strong><\/h2>\n<p data-path-to-node=\"55\">When we talk about the future of clean energy, we are talking about the hydrogen economy. The <b data-path-to-node=\"55\" data-index-in-node=\"94\">synthesis and reactions of hydrides<\/b> play a massive role in making this a reality.<\/p>\n<p data-path-to-node=\"56\">Special hydrogen storage alloys, like <span class=\"math-inline\" data-math=\"\\text{TiFe}\" data-index-in-node=\"38\">TiFe<\/span> or<span class=\"math-inline\" data-math=\"\\text{LaNi}_5\" data-index-in-node=\"53\">LaNi<sub>5<\/sub><\/span>, can safely store and release massive amounts of hydrogen gas at normal temperatures. As per <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides, <\/b>This lets engineering teams design highly efficient hydrogen fueling stations and compact fuel cell systems. By storing the gas inside a solid metal lattice, we achieve incredible volumetric storage density without needing dangerously high-pressure gas tanks.<\/p>\n<p data-path-to-node=\"57\">In the world of catalysis in <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides<\/b>, complex hydrides are excellent chemical carriers. Take sodium borohydride (<span class=\"math-inline\" data-math=\"\\text{NaBH}_4\" data-index-in-node=\"102\">NaBH<sub>4<\/sub><\/span>) again\u2014it acts as a predictable, safe donor of hydrogen for turning unsaturated organic bonds (like aldehydes or ketones) into clean alcohols through hydrogenation.<\/p>\n<p data-path-to-node=\"58\">On top of that, material scientists are now using metal hydrides as stepping stones to build advanced nanostructures. For instance, they use titanium hydride (<span class=\"math-inline\" data-math=\"\\text{TiH}_2\" data-index-in-node=\"159\">TiH<sub>2<\/sub><\/span>) as a starting material to synthesize high-purity titanium dioxide nanoparticles, which are used in solar panels and cutting-edge electronics.<\/p>\n<h2 data-path-to-node=\"58\"><strong>Final Thoughts\u00a0<\/strong><\/h2>\n<p data-path-to-node=\"58\">Mastering the <b data-path-to-node=\"0\" data-index-in-node=\"26\">synthesis and reactions of hydrides<\/b> comes down to recognizing patterns rather than raw memorization. Once you can connect the type of chemical bonding to how a hydride behaves in the lab, predicting products and identifying periodic trends becomes second nature. Based on <b data-path-to-node=\"1\" data-index-in-node=\"228\">synthesis and reactions of hydrides, <\/b>these concepts are the building blocks of real-world green energy technologies and advanced materials. Keep working through practice problems, stay consistent with your revision, and don&#8217;t hesitate to lean on expert resources. At VedPrep, we are always here to help you clear up any confusion and turn tricky inorganic chemistry topics into your biggest scoring strengths on exam day.<\/p>\n<p data-path-to-node=\"58\">To know more in detail from our faculty, watch our YouTube video:<\/p>\n<p class=\"responsive-video-wrap clr\"><iframe title=\"Reagents and Name Reaction in Organic Chemistry | CSIR NET | GATE | IIT JAM | DU | BHU |Chem Academy\" width=\"1200\" height=\"675\" src=\"https:\/\/www.youtube.com\/embed\/1mZUlluWaoQ?list=PLdZcCa6mtW233hnUC42MCJjOFuX4_LTWv\" frameborder=\"0\" allow=\"accelerometer; autoplay; clipboard-write; encrypted-media; gyroscope; picture-in-picture; web-share\" referrerpolicy=\"strict-origin-when-cross-origin\" allowfullscreen><\/iframe><\/p>\n<h2><strong>Frequently Asked Questions<\/strong><\/h2>\n<style>#sp-ea-20308 .spcollapsing { height: 0; overflow: hidden; transition-property: height;transition-duration: 300ms;}#sp-ea-20308.sp-easy-accordion>.sp-ea-single {margin-bottom: 10px; border: 1px solid #e2e2e2; }#sp-ea-20308.sp-easy-accordion>.sp-ea-single>.ea-header a {color: #444;}#sp-ea-20308.sp-easy-accordion>.sp-ea-single>.sp-collapse>.ea-body {background: #fff; color: #444;}#sp-ea-20308.sp-easy-accordion>.sp-ea-single {background: #eee;}#sp-ea-20308.sp-easy-accordion>.sp-ea-single>.ea-header a .ea-expand-icon { float: left; color: #444;font-size: 16px;}<\/style><div id=\"sp_easy_accordion-1780317969\">\n<div id=\"sp-ea-20308\" class=\"sp-ea-one sp-easy-accordion\" data-ea-active=\"ea-click\" data-ea-mode=\"vertical\" data-preloader=\"\" data-scroll-active-item=\"\" data-offset-to-scroll=\"0\">\n\n<!-- Start accordion card div. -->\n<div class=\"ea-card ea-expand sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203080\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203080\" aria-controls=\"collapse203080\" href=\"#\"  aria-expanded=\"true\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-minus\"><\/i> Why are ionic hydrides also called \"saline\" hydrides?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse collapsed show\" id=\"collapse203080\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203080\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>\"Saline\" just means salt-like. Because alkali and alkaline earth metals are highly electropositive, they completely transfer their valence electrons to hydrogen. This forms a crystalline, high-melting solid with an ionic lattice (<span class=\"math-inline\" data-math=\"\\text{M}^+\" data-index-in-node=\"230\">M<sup>+<\/sup><\/span><sup>\u00a0<\/sup>and <span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"245\">H<sup>-<\/sup><\/span> ions) that looks and behaves a lot like standard table salt (<span class=\"math-inline\" data-math=\"\\text{NaCl}\" data-index-in-node=\"317\">NaCl<\/span>).<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203081\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203081\" aria-controls=\"collapse203081\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does the thermal stability of covalent hydrides change down a group?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203081\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203081\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It decreases drastically. As you move down a group (like Group 15 from <span class=\"math-inline\" data-math=\"\\text{NH}_3\" data-index-in-node=\"71\">NH<sub>3<\/sub><\/span>\u00a0to <span class=\"math-inline\" data-math=\"\\text{BiH}_3\" data-index-in-node=\"86\">BiH<sub>3<\/sub><\/span>), the central atom gets much larger. Because the atom is so big, its orbital overlap with the tiny <span class=\"math-inline\" data-math=\"1s\" data-index-in-node=\"198\">1s<\/span>\u00a0orbital of hydrogen becomes incredibly weak. A weaker bond means it takes far less heat to break it apart.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203082\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203082\" aria-controls=\"collapse203082\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why is {LiH} exceptionally stable compared to other alkali metal hydrides?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203082\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203082\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It boils down to lattice energy. Both lithium (<span class=\"math-inline\" data-math=\"\\text{Li}^+\" data-index-in-node=\"47\">Li<sup>+<\/sup><\/span>) and hydride (<span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"73\">H<sup>-<\/sup><\/span>) ions are exceptionally small. Because they are similar in size, they pack together incredibly tightly in a crystal lattice. This high lattice energy makes <span class=\"math-inline\" data-math=\"\\text{LiH}\" data-index-in-node=\"240\">LiH<\/span>\u00a0stable up to nearly <span class=\"math-inline\" data-math=\"900^\\circ\\text{C}\" data-index-in-node=\"271\">900\u00b0C<\/span>\u00a0before it decomposes.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203083\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203083\" aria-controls=\"collapse203083\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can metallic hydrides conduct electricity as well as the parent metals?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203083\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203083\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Yes, they can! Because hydrogen atoms sit inside the interstitial gaps of the transition metal lattice without disrupting the mobile \"sea of electrons,\" metallic hydrides maintain excellent electronic conductivity. Sometimes, the absorption of hydrogen even alters the magnetic properties of the metal.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203084\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203084\" aria-controls=\"collapse203084\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why do ionic hydrides liberate hydrogen gas at the anode during electrolysis?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203084\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203084\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>In a molten ionic hydride, hydrogen exists as the negatively charged hydride ion (<span class=\"math-inline\" data-math=\"\\text{H}^-\" data-index-in-node=\"82\">H<sup>-<\/sup><\/span>). When you pass an electric current through the melt, these negative ions migrate toward the positive electrode (the anode), where they lose electrons (get oxidized) and pair up to form <span class=\"math-inline\" data-math=\"\\text{H}_2\" data-index-in-node=\"279\">H<sub>2<\/sub><\/span>\u00a0gas.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203085\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203085\" aria-controls=\"collapse203085\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How does the reducing power of group 16 hydrides vary?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203085\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203085\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Reducing power increases down the group: <span class=\"math-inline\" data-math=\"\\text{H}_2\\text{O} &lt; \\text{H}_2\\text{S} &lt; \\text{H}_2\\text{Se} &lt; \\text{H}_2\\text{Te}\" data-index-in-node=\"41\">H2O &lt; H2S &lt; H2Se &lt; H2Te<\/span>. Because the <span class=\"math-inline\" data-math=\"\\text{M-H}\" data-index-in-node=\"138\">M-H<\/span>\u00a0bond strength plummets as the central atom gets larger, it becomes much easier for the molecule to give up its hydrogen atoms to reduce something else.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203086\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203086\" aria-controls=\"collapse203086\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Are there any covalent hydrides that act as Lewis acids?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203086\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203086\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>es, elements from Group 13 form electron-deficient covalent hydrides. Borane (<span class=\"math-inline\" data-math=\"\\text{BH}_3\" data-index-in-node=\"79\">BH3<\/span>) and alane (<span class=\"math-inline\" data-math=\"\\text{AlH}_3\" data-index-in-node=\"103\">AlH3<\/span>) don't have a full octet of valence electrons around their central atoms, which makes them eager to accept electron pairs from Lewis bases like ammonia or ethers.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203087\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203087\" aria-controls=\"collapse203087\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Why are transition metal hydrides used for hydrogen storage rather than ionic hydrides?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203087\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203087\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Ionic hydrides react irreversibly with moisture and require chemical destruction to get the hydrogen back. Transition metal alloys (like <span class=\"math-inline\" data-math=\"\\text{LaNi}_5\" data-index-in-node=\"137\">LaNi5<\/span>), however, act like a physical sponge. They absorb hydrogen gas at mild pressures and release it cleanly when you slightly raise the temperature or lower the pressure, making them perfectly reusable.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203088\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203088\" aria-controls=\"collapse203088\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> What is the main product when silane {SiH4) is exposed to air?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203088\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203088\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Silane is pyrophoric, meaning it spontaneously bursts into flames when it hits the air. It reacts rapidly with oxygen to form solid silicon dioxide (<span class=\"math-inline\" data-math=\"\\text{SiO}_2\" data-index-in-node=\"149\">SiO2<\/span>) and water vapor, a stark contrast to methane (<span class=\"math-inline\" data-math=\"\\text{CH}_4\" data-index-in-node=\"209\">CH4<\/span>), which requires an ignition source to burn.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-203089\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse203089\" aria-controls=\"collapse203089\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> How do you prepare sodium hydride {NaH) in an industrial setting?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse203089\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-203089\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>It is prepared via direct synthesis. Molten sodium metal is reacted directly with pure hydrogen gas at temperatures around <span class=\"math-inline\" data-math=\"300^\\circ\\text{C}\" data-index-in-node=\"123\">300\u00b0C<\/span>\u00a0to <span class=\"math-inline\" data-math=\"400^\\circ\\text{C}\" data-index-in-node=\"144\">400\u00b0C<\/span>\u00a0under high pressure to force the formation of the ionic solid lattice.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2030810\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2030810\" aria-controls=\"collapse2030810\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i> Can VedPrep materials help me predict structural anomalies in complex hydrides?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2030810\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-2030810\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>At VedPrep, we break down molecular orbital theory and periodic trends using clean visualization tools. We don't just ask you to memorize structures like diborane or lithium borohydride\u2014we show you the electron density maps and symmetry principles so you can intuitively predict shapes and reactivity patterns on your exam.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<!-- Start accordion card div. -->\n<div class=\"ea-card  sp-ea-single\">\n\t<!-- Start accordion header. -->\n\t<h3 class=\"ea-header\">\n\t\t<!-- Add anchor tag for header. -->\n\t\t<a class=\"collapsed\" id=\"ea-header-2030811\" role=\"button\" data-sptoggle=\"spcollapse\" data-sptarget=\"#collapse2030811\" aria-controls=\"collapse2030811\" href=\"#\"  aria-expanded=\"false\" tabindex=\"0\">\n\t\t<i aria-hidden=\"true\" role=\"presentation\" class=\"ea-expand-icon eap-icon-ea-expand-plus\"><\/i>  How can you distinguish between {NaH} and {HCl} gas reactions with water?\t\t<\/a> <!-- Close anchor tag for header. -->\n\t<\/h3>\t<!-- Close header tag. -->\n\t<!-- Start collapsible content div. -->\n\t<div class=\"sp-collapse spcollapse \" id=\"collapse2030811\" data-parent=\"#sp-ea-20308\" role=\"region\" aria-labelledby=\"ea-header-2030811\">  <!-- Content div. -->\n\t\t<div class=\"ea-body\">\n\t\t<p>Both reactions look energetic, but they yield opposite chemical environments. <span class=\"math-inline\" data-math=\"\\text{NaH}\" data-index-in-node=\"78\">NaH<\/span>\u00a0reacts with water to give a strong base and hydrogen gas (<span class=\"math-inline\" data-math=\"\\text{NaH} + \\text{H}_2\\text{O} \\rightarrow \\text{NaOH} + \\text{H}_2\" data-index-in-node=\"147\">NaH + H2O \u2192NaOH + H2<\/span>). <span class=\"math-inline\" data-math=\"\\text{HCl}\" data-index-in-node=\"218\">HCl<\/span>\u00a0gas simply dissolves in water to form highly acidic hydrochloric acid (<span class=\"math-inline\" data-math=\"\\text{H}_3\\text{O}^+ + \\text{Cl}^-\" data-index-in-node=\"300\">H3O<sup>+<\/sup> + Cl<sup>-<\/sup><\/span>) without producing <span class=\"math-inline\" data-math=\"\\text{H}_2\" data-index-in-node=\"354\">H2<\/span>\u00a0gas.<\/p>\n\t\t<\/div> <!-- Close content div. -->\n\t<\/div> <!-- Close collapse div. -->\n<\/div> <!-- Close card div. -->\n<\/div>\n<\/div>\n\n","protected":false},"excerpt":{"rendered":"<p>Synthesis and reactions of hydrides are crucial topics in inorganic chemistry, essential for IIT JAM aspirants. Understanding the Syllabus and Key Textbooks This topic falls under Inorganic Chemistry, a unit in the official CSIR NET \/ NTA syllabus. Students preparing for IIT JAM and other competitive exams like CSIR NET and GATE should focus on mastering this area.<\/p>\n","protected":false},"author":11,"featured_media":12627,"comment_status":"open","ping_status":"open","sticky":false,"template":"","format":"standard","meta":{"_acf_changed":false,"footnotes":"","rank_math_seo_score":89},"categories":[23],"tags":[2923,7567,7568,7569,7570,2922],"class_list":["post-12628","post","type-post","status-publish","format-standard","has-post-thumbnail","hentry","category-iit-jam","tag-competitive-exams","tag-synthesis-and-reactions-of-hydrides-for-iit-jam","tag-synthesis-and-reactions-of-hydrides-for-iit-jam-notes","tag-synthesis-and-reactions-of-hydrides-for-iit-jam-questions","tag-synthesis-and-reactions-of-hydrides-for-iit-jam-study-materials","tag-vedprep","entry","has-media"],"acf":[],"_links":{"self":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12628","targetHints":{"allow":["GET"]}}],"collection":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts"}],"about":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/types\/post"}],"author":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/users\/11"}],"replies":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/comments?post=12628"}],"version-history":[{"count":7,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12628\/revisions"}],"predecessor-version":[{"id":20311,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/posts\/12628\/revisions\/20311"}],"wp:featuredmedia":[{"embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media\/12627"}],"wp:attachment":[{"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/media?parent=12628"}],"wp:term":[{"taxonomy":"category","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/categories?post=12628"},{"taxonomy":"post_tag","embeddable":true,"href":"https:\/\/www.vedprep.com\/exams\/wp-json\/wp\/v2\/tags?post=12628"}],"curies":[{"name":"wp","href":"https:\/\/api.w.org\/{rel}","templated":true}]}}