Category: Chemistry Notes PPT

Chemistry Important Questions

Chemistry is important as well as a complicated subject for Science students. Many students find this subject easy whereas many do not. Board exams are near and it’s a very crucial time for preparation and revision. At this point, the Chemistry subject may seem scary. To help students with the upcoming board exams have brought for you the most important CBSE questions of Chemistry. These questions will not only help the lagging students in Chemistry but also will help in the proper revision for those whose preparation is completed. These CBSE important questions are a must for all the 12 Class students who are going to appear for their board exams this year.  

Marks wise Important Questions with Answers – Free pdf Download 

The CBSE important questions of Chemistry are available in pdf format. With being easily downloadable and available for free of cost these important questions become handy for students. These solutions are prepared by our experienced faculty who are well versed in their respective subjects so these questions are highly dependable and will help students to score the best in their exams. No matter how much you lack behind in Chemistry do give us a try at our CBSE important questions of Chemistry. 

Important Questions For Class 12 Chemistry CBSE With Answers

With proper focus on the syllabus of the Class 12th Chemistry as well as the pattern of the exams, we have prepared these most important questions of Chemistry for you all. This year CBSE has reduced a lot of syllabi. For scoring the best in exams knowing the syllabus is very important. We have shared the revised syllabus of Chemistry below-

There are a total of 16 Units divided into two books of NCERT of Chemistry as part1 and part 2.

Part 1

Unit 1 Solid-state

Unit 2 Solutions

Unit 3 ElectroChemistry

Unit 4 Chemical kinetics 

Unit 5 Surface Chemistry

Unit 6 removed

Unit 7  p block elements

Unit 8 d and f block elements

Unit 9 Coordination compounds

Part 2

Unit 10 Haloalkanes and haloarenes  

Unit 11 Alcohols, Phenols, and Ethers

Unit 12 Aldehydes ketones and carboxylic acids

Unit 13 Amines

Unit 14 Biomolecules

Unit 15   removed

Chapter Wise Questions Chemistry Class 12th  Weightage

Why Are Class 12 Chemistry Important Questions

• Marks wise important questions with their solutions help the students in a tension free preparation. Students can prepare better through these important questions.

• Time management is important for any exam preparation. Our important questions help in the same.

• Important questions also include those questions that are frequently asked in board exams.

• If a student has no time to do a detailed preparation of Chemistry subject then he/she can use our important questions bank and score well in the exams.

• Practicing from important questions is the best way to revise the concepts and do the proper practice.

Do you know from the rock salt we use to eat to the Kohinoor placed in the crown of England’s queen are all minerals!! More than 4000 naturally occurring minerals have been found on earth. Metals, precious gems such as ruby, sapphire, diamonds etc. many valuable products we get from the minerals. Even coal, natural gas and petroleum are also types of minerals which are known as energy minerals or fossil fuels.

Some minerals are valuable due to their usage in various fields while some are because of their beauty, rarity and durability. Almost 90% of the earth crust is composed of silicate minerals. You must remember here that minerals and rocks are different. Minerals have a definite chemical structure which is the same throughout that mineral. While rocks are composed of many minerals and are not consistent throughout their structure.

What are Minerals?

Minerals can be defined as naturally occurring chemical compounds which are inorganic in nature and have definite chemical composition and structure. They are generally found in all three forms solid, liquid and gaseous in nature. Iron ore, bauxite, hematite, mica, salt, potash, coal, petroleum, natural gas etc. are examples of minerals.

Classification of Minerals

Minerals can be classified into the following three types on the basis of their composition –

• Metallic Minerals

• Non-metallic Minerals

• Energy Minerals

Metallic Minerals

Metals are obtained by extraction of these minerals. These are very valuable as they provide metals in pure form. Examples of metallic minerals – iron ore, bauxite, hematite etc.

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Non-Metallic Minerals

Those minerals which do not contain metals are called non-metallic minerals. Examples of non-metallic minerals – diamond, mica, salt, potash etc. The Kohinoor diamond placed on the crown of England’s queen is an example of non-metallic mineral.

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Energy Minerals

Those minerals which provide energy are called energy minerals. These are also known as fossil fuels. Examples of energy minerals – Coal, petroleum, natural gas etc.

Difference Between Metallic and Non-Metallic Minerals

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Energy minerals are studied under the category of fossil fuels. They are quite visibly different from metallic and non-metallic minerals. But generally, students get confused between metallic and non-metallic minerals so for your clear understanding we are providing here key differences between metallic and non-metallic minerals

This was a brief about metallic and non-metallic minerals, if you are looking for detailed study material on the topic then register yourself on or download learning app for class 6-10, IIT JEE and NEET.

Conclusion

Minerals are the country’s natural resources, which can be used in a variety of ways. Mineral formation and concentration take hundreds of years, making it a finite and non-renewable resource. As a result, it is critical to save resources, which can be accomplished through recycling metals.

Non-metallic minerals, such as limestone, mica, and gypsum, do not contain any metals, according to the difference between metallic and non-metallic minerals. Metallic minerals, on the other hand, contain metal in its unprocessed form.

The Michaelis Menten hypothesis or Michaelis Menten kinetics is a model that is designed to explain generally the velocity of enzyme-catalyzed reactions and their gross mechanism. Among the best-known models in biochemistry to determine catalyst kinetics, the Michaelis Menten hypothesis is used. 

 

The Michaelis Menten kinetics was first proposed in 1913, assuming that enzymes and their substrate are able to form a reversible complex as soon as they react. Substrates are the substances that catalysts react with in order to produce the desired product. A second assumption is that the concentration of the product (p) directly relates to the rate of its formation.

 

Michaelis Menten Equation

Whenever enzyme active sites are filled with substrates, the rate of such a reaction is maximum. In other words, the reaction kinetics increase as the concentration of substrates increases. Kinetic studies of enzymes have been based on this relationship. Thus, the Michaelis Menten hypothesis or the kinetics theory has been reduced to a mathematical formula relating the concentration of the substrate S to the rate of formation of product P or reaction rate v. The formula is stated below that is known as the Michaelis-Menten equation. 

[{V = frac {dPP} {dt}}] = [{V_{max} = frac {SS} {K_m + SS}}]

In this equation, Vmax represents the maximum reaction rate achieved by the system at saturation of the substrate concentration. KM  equals the concentration of the substrate when the value of the rate of reaction is half of Vmax. When the reaction rate and concentration of the substrate of an enzyme-catalyzed reaction are plotted together, the hypothesis becomes clearer.

 

Enzyme-catalyzed Reactions: Mechanism

An enzyme-catalyzed reaction happens when it attracts substrates to its active site and catalyzes them into a desired product. At the end of the reaction process, the product dissociates from the enzyme’s active site. A substrate complex is a result of the interaction between the active enzyme and the substrate. 

 

Binary complexes, which involve only one enzyme in the reaction, and ternary complexes, which involve two enzymes and two substrates, are called so. They are connected by electrostatic forces or by hydrophobic forces, not chemical bonds. So, bonding has a physical nature and is noncovalent. 

 

It has been observed that applications of enzymes to biochemical reactions actually increase their rate by a large fraction, approximately 106 times greater than when enzymes are not utilized as catalysts. Additionally, it has been observed that the mechanism of enzyme-catalyzed reactions has the capability of separating very similar substrates and greatly enhancing the rate of reaction of one without having much impact on the other substrate.

 

There is a simple lock and key model popularly known to explain the mechanism behind enzyme-catalyzed reactions. By visualizing the enzyme as three-dimensional and the substrate as three-dimensional, the kinetic model can be clarified. Both the substrates and enzymes are complemented in such a way that their structures can fit tightly with one another and their active catalytic sites are in close proximity to those chemical bonds which are altered during the reaction. As in the case of keys, their active sites are designed to fit perfectly into the keyholes of the locks. Likewise, their active sites are tailored to fit perfectly with the chemical structure of their substrates.

 

Michaelis Menten Kinetics Application

 

A catalyst’s efficiency is measured by Kcat / KM, a measure of how efficiently it transforms the substrate into a product. So, diffusion enzyme catalysts, such as fumarase, whose upper limit is 10⁸-10¹⁰ M^-1 S^-1, actually diffuse the substrate into the active site of the enzyme catalyst. Apart from biochemical reactions, it has been applied to a wide variety of other areas such as alveolar dust clearance, clearance of blood-alcohol, bacteriophage infection, and photosynthesis-irradiance relationships.

All matter whether metals, nonmetals, or inert substances are principally composed of atoms, molecules, and/or ions but their distribution in the matter depends upon the state it is representing, that is, either solid, liquid, or gaseous. Depending on the state, the molecular structures of solid, liquid, and gases are geometrically and structurally different. This difference in structure is primarily due to the variation of the arrangement of molecules in liquid, solid, and gases.

The particles in the gases are far away from each other and thus are well separated and do not have a definite shape.  Because of the large distance between the molecules of gases, they move quite easily and very fast causing vibration, therefore, possessing high kinetic energy.

On the other hand, liquid molecules are close together but are not tightly packed; they do not show any definite molecular arrangements and have no definite shape of their own. The liquid vibrates and slides across each other with lesser speed as compared to gases and therefore shows less kinetic energy.

In solid matters, the molecules are tightly  packed with each other in a definite arrangement and thus have a defined structure, shape, and size. Solid vibrates but its molecules do not move from place to place. The molecular structure of solid, liquid, and gas is represented by the following diagram.

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Characteristics of Solid, Liquid, and Gases

Properties Based on Molecular Structure of Solid, Liquid, and Gas

1. Molecular Structure of Solid

There are two types of solid structure based on the molecular arrangements of solid, namely, crystalline solid and amorphous solid.

In crystalline solids, the molecules that make up the solids are in definite and regular arrangements which gives them a well-defined structure. Crystalline solids are made up of cell units that are the smallest repeating pattern of solid and are the building blocks of crystalline solid. They are identical in nature and repeating.

Whereas amorphous solids do not have a definite structural pattern and order of themselves. Though the molecules are closely and tightly packed and have very little mobility, the arrangements of the molecules are not regular and in asymmetrical order. A few common examples of these types of solids are plastic and gases.

Further on the basis of the molecular structure of crystalline solid, it is divided into four categories, namely, ionic solid, molecular solid, atomic solid also known as covalent network, and metallic solid.

• Ionic Solid: These solids are made up of positive as well as negative ions that are held together closely by electrostatic force. They have high melting points, high brittle crystals and are bad conductors in their solid forms, for example, salt and sodium chloride (NaCl).

• Molecular Solid: The atoms or molecules of these solids are held closely by strong bonding forces like London Dispersion forces, dipole–dipole force as well as hydrogen bonding. They have usually low melting points with very low conductivity, for example, molecular solid in sucrose.

• Atomic (or Covalent) Solid: This type of solid is usually up with atoms that are held together by a covalent bond and share a covalent force between them as well. They are usually hard and have high melting points but poor conductors of heat and electricity (with exceptions). Common examples of this type of solid are graphite and diamond. Now graphite has a 2D hexagonal structure unlike diamond and is therefore held together by weak London dispersion Force. Thus, graphite is not as strong as diamonds. 

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• Metallic Solids: They are made up of metal atoms and are held together strongly by metallic bonds. Thus, they range from soft and malleable to hard solids with high melting points as well as high electrical conductivity.

Particles of solid are arranged in unit cells that have different patterns. Now the molecules, atoms, or ions that are together are known as particles that always have some voids in whichever way the particles are arranged. Thus, the quantitative aspect of the solid-state can be expressed numerically as packing efficiency that is expressed as a percentage. Thus, the equation of packing efficiency can be expressed as, 

[text{Packing Efficiency} = frac{text{Number of Atoms} times text{Volume obtained by 1 share}}{text{Total Volume of Unit Cell}} times 100%]

Alternatively, [text{Packing Efficiency}] (%) = [frac{text{Volume of Atoms in Unit Cell} }{text{Total Volume of Unit Cell}} times 100%]

2. Molecular Structure of Liquid

Liquid molecules, much like solid and unlike gases, are closer to each other and can glide across each other easily. But in solids, as the particles are held strongly by the intermolecular forces, liquids possess too much thermal energy and thus cannot be held at a certain position by these forces and thus move around easily within the liquid mass.

Although liquid has a much greater cohesion force as compared to that of gas, this force cannot prevent a few molecules of the liquid from bonding with each other. On the other hand molecules at the surface of the liquid experience a cohesive force with the molecules that are within the surface and near to liquid mass. Because of this cohesive force, the liquid molecules on the surface of the liquid act as the stretching membrane. Thus, the liquid molecules of the liquid surface tend to draw inwards towards the centre of mass and hence forms a sphere. This is called the surface tension of the liquid.

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The liquid wets a solid surface only when the intermolecular force of attraction between the molecules of liquid on the liquid surface to the molecules on the solid surface is greater. For example, wetting of clothes where water is retained on the surface of the fabric. But when the intermolecular force is not that high, the liquid is not retained on the solid surface, for example, when mercury is run through a glass capillary.

Also, the molecules in the liquid state exhibit properties of diffusion. That is when two miscible liquids are poured into a container, the molecules in liquid states due to greater intermolecular force start diffusing into each other unit, they form a uniform mixture.

Liquid also has a very unique property called buoyant force in which the substance immersed into the liquid experiences an upward force that is equal to the weight of the liquid displaced by the substance. 

3. Molecular Structure of Gases

As the molecules of the gases are at very high kinetic energy and are separated by large distances, they can easily slide and cross each other and don’t possess any particular shape, size, or volume.

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Based on its molecular arrangements, few of the properties of gases are listed below:

• Particles are in constant random motion.

• Particles often collide with each other and with the wall of the container but due to its high elasticity, there is no net loss of energy from the particles of gas.

• There is no force of attraction or repulsion between the molecules of the gas.

• Since the molecules of the gases are very small, thus the volume occupied by the gas molecules is negligible as compared to the total volume of the container.

• The kinetic energy of the gas molecules depends on the absolute temperature of the gas and all the gas molecules with the same absolute temperature will have the same kinetic energy.

Now since the molecules or the atoms of the gases are very tiny and therefore have a lot of empty space between them, the particles are constantly in motion. Now as the volume of the gaseous is very small, hence, its density is also minimal due to which a gas can be compressed or expanded according to the condition.

As the particles are in constant motion, therefore, the two gases in one container will mix with each other as their molecules will move constantly and will collide with each other. Thus, the no. of particles colliding with the surface of the container and the force with which they are colliding on the wall is determined as the pressure of that particular gas. 

As different gases have different particle motions, and hence, they collide with various speeds giving rise to the different kinetic energy distribution of various gases. The graph represents the same.

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Molecular Model of Solid, Liquid, and Gas

The molecular model of the solid, liquid, and gas helps in determining the kinetic molecular theory of matter as these two factors are closely related to one another. Various molecular arrangements and their motion kinetics give rise to the force with which one molecule will collide with another in the  same substance or intermolecular interaction for different substances giving rise to the kinetic molecular theory. The kinetic molecular theory explains the interaction between atoms and their microscopic properties that in turn give rise to the macroscopic properties of the matter such as pressure, temperature, and volume. This theory was developed to explain the existence of various states of matter and the way by which matter converse from one state to another.

Thus, the key points of kinetic molecular theory that can clarify the molecular model of solid, liquid, and gas are given below: 

• Matters are made up of particles that are in constant motion, that is, they are continuously moving.

• The temperature of matter is measured by the average kinetic energy of the moving particles.

• The change in phase occurs when the change in the kinetic energy of the molecules of matter changes.

All particles of the matter have energy and the energy of the particles varies with the temperature of the matter. This in turn determines if the matter should be in a solid, liquid, or gaseous state. The matter in the solid-state has the least kinetic energy followed by liquid and gaseous particles have the highest kinetic energy.

Even if the particles are closely packed with each other, there is still some space between the particles which are called voids. These voids start becoming larger and larger as the matter changes from solid to liquid and finally to a gaseous state.

There are always attractive forces between particles that are called intermolecular attractive forces and it starts getting bigger and bigger as the particles come closer to one another.

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Conclusion

Here, our discussion on the molecular structure of solids, liquids, and gases completes. You should now be able to differentiate between the arrangements of molecules in different states of matter: solid, liquid, and gas. You should also be able to relate the arrangement of the molecules at a microscopic level and their inference on the macroscopic properties of the matter.

The C in the C–X bond is carbon while the halogen is denoted as X. The high electronegativity of halogen makes the electron cloud attract more towards itself and therefore gains a slight negative charge, while the carbon attains a slight positive charge. As the halogens need only one electron to achieve their nearest inert gas configuration, that is, their octet state, so between one carbon and one halogen atom, only one sigma bond is formed. The C–X bond length in haloarenes increases due to the increase in atomic size from fluorine to astatine and the bond dissociation strength decreases.

Haloarenes Nature of C–X Bond

The chemical compounds containing arenes are known as haloarenes, where one or more hydrogen atoms bonded to an aromatic ring are replaced with halogens. It contains halogen atoms attached to sp2 hybridized carbon atom(s) of an aryl group. The C–X bond’s nature depends on both the halogen of the compound and the nature of carbon in the benzene ring. The alphabet “X” generally denotes halogen. Halogens are group 17 elements that have very high electronegativity. Going down the group, the elements are namely, fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). The highest electronegativity is of fluorine (F). The elements in this group need one more electron to complete the nearest noble gas configuration.

The carbon in haloarenes which is a 14th group element has lesser electronegativity as compared to that of the halogens which have higher electronegativity.

Salient Points on the Nature of C–X Bonds in Haloarenes

The salient points on the nature of C–X bonds in haloarenes are as follows: 

• We know that the halogens are more electronegative than carbon and due to this high electronegativity, it makes the electron cloud attract more towards itself and therefore gains a slight negative charge, while the carbon attains a slight positive charge. Thus, the C–X bond in haloarenes is polarised.

• Between one carbon atom and one halogen atom, only one sigma bond is formed because halogens need only one electron to reach the nearest inert gas configuration, that is, the octet state.

• The atomic size increases from fluorine to astatine; therefore, as a result, the C–X bond length in haloarenes also increases, and the bond dissociation strength decreases.

• Moving down the group, the electronegativity decreases, and we know that dipole moment depends on the difference in electronegativity of carbon and halogens. Therefore, the dipole moment also decreases down the group. Although, there is an exception of C–Cl and C–F dipole moments., Cl has less electronegativity than F, but the dipole moment of C–Cl bond is more than C–F. 

Solved Examples

1. Which C–X bond is strongest?

Answer: Carbon–fluoride bond.

Except for the carbon–iodine bond, the carbon–halogen bonds are polar, because the electron pair is pulled closer to the halogen atom than the carbon. This is because the halogens are more electronegative than carbon apart from iodine. Fluorine is the most electronegative that pulls the electron pair more strongly than the other halogens. Therefore, the carbon–fluorine bond is the strongest. 

2. Which of the following orders is correct regarding the bond enthalpy ε(C−X) in an alkyl halide (RX)?

(a) ε(C−I) < ε(C−Br) < ε(C−Cl)

(b) ε(C−I) < ε(C−Br) > ε(C−Cl)

Answer: Bond enthalpy C−X (where X is Cl, Br, I) decreases with increase in the atomic number of X. Hence, the correct order is option a.

3. What are the factors responsible for low reactivity of aryl halides towards nucleophilic substitution?

Answer: The following factors are responsible for the low reactivity of aryl halides towards nucleophilic substitution:

1. The bond length of C–X in haloarene is smaller than C–X bond length in alkyl halide.

2. By any nucleophile, it is difficult to displace halogen in haloarenes.

3. A nucleophile easily replaces halogen.

4. Attack of nucleophiles on aryl halides becomes an electron-rich molecule due to the presence of pi bonds.

is the platform that has a solution for all your educational queries, you can connect with a professional advisor to get a solution for all your academic problems. Students can get benefits of by getting expert tips to clear their examination with flying colors. 

In Chemistry, nitride is defined as the compound of nitrogen in which nitrogen has a formal oxidation state of three. A large class of compounds that has a wide range of properties and applications is called nitrides. 

Nitride is composed of different classes of chemical compounds which are combined with an element of equal or lower electronegativity , like boron, silicon and other such metals. 

It contains the nitrite ion  (N3−).  also like carbides, we can divide nitrides into three general categories , that are :

• Ionic

• Interstitial and

• Covalent

There are few metal nitrides that are unstable and most of them react with water to form ammonia and oxide or hydroxide the metal. Some nitrides are very refractory like the nitrite of boron, vanadium, silicon, titanium and tantalum . These nitrides are also resistant to chemical attack, and therefore they are useful as abrasives and creating crucibles.

Chemistry is a very tricky subject and some students may find it difficult but if they choose the right pattern to study then they will see that the topics will be easy for you. Mainly the revision notes which the student prepares to play a very important role as in Chemistry there are numerous formulas and equations which students need to learn so the revision notes must be prepared accordingly to help students to go through it multiple times.

What is Nitride Ion?

The first question is, what is nitride and its properties. When nitrogen combines with elements such as silicon, boron, any other metals, or any element with lower or similar electronegativity than nitrogen, it is known as a nitride. It is a separate class of compounds altogether. Nitride, just like carbides, can be separated into three general categories known as interstitial, ionic, and covalent nitrides. Nitride compounds generally contain the nitride ion. Now questions such as what is the formula for nitride, what is the charge of nitride, what is the symbol of nitride are bound to arise. We will answer these questions a bit later. Such compounds usually react with water to turn into the hydroxide or oxide of the metal and ammonia gas.

Nitride Ion Overview

The question of what is nitride can be explained better by saying that it never comes through an aprotic solution. It is mainly a nitrogen compound. The Ionic radius of nitrides is 140 pm approximately. The oxidation state of nitrogen is -3. Nitride ion is the main iron present in nitrides along with the metal cation. Another question that comes is what is the formula for nitride Ion. The formula for nitride Ion is N-3. Some metal nitrates are very unstable. At the same time, some metal nitrides like those of vanadium, boron, silicon, tantalum, titanium and more are refractory. These are also resistant to earth chemical interactions and are very hard. Uses of nitride are seen in crucibles and abrasives due to hardness.

Preparation of Nitrides

There are three methods for the preparation of nitrides. The first method is where elements directly combine or reaction proceeds at higher temperatures. Calcium nitride synthesis is shown below with the direct combination method.

[ 3C_{a} + N_{2} rightarrow Ca_{3}N_{2} ]

The second method is a much more feasible one and is by loss of ammonia or NH₃. It is done by the thermal breakdown of decomposition of barium amide or any metal amides available.

[ 3Ba(NH_{2})_{2} rightarrow B{a}_{3}N_{2} + 4NH_{3} ]

The method is also an easy one to proceed with in the future. During the surface hardening of metal objects, preferably steel, nitride is also formed. Ammonia when heated to high temperatures between 950 to 1050 Fahrenheit or 500 to 570 Celsius for almost 100 hours starting from a minimum of 5 hours gives out nitride. But it also depends on the desired hardening form or case’s depth.

Reduction of metal oxides is metal halides that also produce nitride. It is another method to prepare nitrides and know exactly what is a nitride. The process takes place in the presence of gaseous nitrogen. Let’s take an example and prepare aluminum nitride with this method.

[ Al_{2}O_{3} + N_{2} rightarrow 2AIN + 3CO ]

Uses of Nitride

There are many uses of nitride, but mainly they are used as insulators. One of the lubricants at high temperatures is hexagonal boron nitride which is extremely hard. The lubricating nature is due to its layered structure. It is akin to molybdenum disulfide. Nitrides are also used for cutting materials and hard coatings. For example, titanium nitride and silicon nitride are used for the same. It is because similar to carbides, nitride has high lattice energy and hence are generally refractory substances. The N-3 ions have a strong attraction with the metal cations. Owing to the large band gaps, nitride behaves like insulators. Blue light emitted from LED lights is due to the excessive bandgap in gallium nitride. Some nitrides like lithium nitride are also used for hydrogen storage purposes as they can absorb hydrogen-like metal oxides.

 

Ionic Nitrides

The only alkali metal that does form a nitride is Lithium. Every alkaline Earth metal forms nitrides. The formula they have is M3N2. These nitrides react with water (hydrolysis) and produce metal hydroxide and ammonia. Ionic Nitrides have a wide range of stability. Be3N2 has a melting point of 220⁰ degrees Celsius, and Mg3N2 at 27⁰ degrees Celsius decomposes completely.

Interstitial Nitrides

Transition metals with nitrogen form interstitial Nitrides. Nitrogen atoms occupy holes or spaces in the closely packed lattice of the metal. The formula they have is M2N, M4N and MN. These have a metallic luster and are opaque with high conductivity, melting point and are extremely hard. Interstitial Nitrides are inert and prepared by heating the metal in ammonia. One of the characteristics reaction is giving below:

[ 2VN + 3H_{2}SO_{4} rightarrow V_{2}(SO_{4})_{3} + N_{2} + 3H_{2} ]

Covalent Nitrides

Examples are Cyanogen, boron nitride, disulfur dinitride, tetrasulfur tetranitride and phosphorus nitride. They have a wide range of properties.

Solved Examples

1. What is the Formula for Nitride?

Answer: What is the formula of nitride ion is a very common question. The formula is (N-3).

2. What is the Symbol for Nitride?

Answer: The symbol of the nitride ion is N-3 while metal Nitrides are of many symbols and notations.