create a quiz on inorganic chemistry exceptions to help me revise for my jee main exam.

If you are preparing for JEE Main, you already know that inorganic chemistry is full of rules. Electronic configuration rules, periodic table trends, bonding rules, and acid-base rules. But here is the real secret that toppers know: JEE loves to test the exceptions to these rules, not just the rules themselves.

Every year, a good number of questions in the JEE Main chemistry paper are based on something that does not follow the expected pattern. For example, why does chromium have the configuration 3d5 4s1 instead of 3d4 4s2? Why is the melting point of boron trichloride lower than expected? Why does fluorine not show a positive oxidation state when every other halogen does? These are exactly the type of twists that confuse students in the exam hall.

This blog is written in very simple English so that you can revise quickly, even a day before your exam. We have collected the most important exceptions in inorganic chemistry, topic by topic, in the same order that most JEE Main aspirants study them: atomic structure, periodic table, chemical bonding, s-block, p-block, d-block and f-block, and coordination compounds. At the end, there is a 25-question quiz with answers, so you can test yourself immediately after reading.

Keep a notebook beside you while reading this. Every time you see an exception, write it down in your own words. This simple habit is what separates students who score 90 plus in chemistry from students who lose marks on silly exceptions.

Why JEE Main Loves Exception-Based Questions

Before we go topic by topic, it helps to understand why the JEE Main paper setters are so fond of exceptions. The JEE Main exam is designed to check whether you have actually understood chemistry, or whether you have just memorised formulas without thinking about them. A question based on a straightforward rule can often be answered by guesswork or by pattern matching. But a question based on an exception forces you to think about the real reason behind a trend, not just the trend itself.

For example, almost every student knows that ionisation enthalpy increases across a period. But only a student who understands why beryllium has a higher ionisation enthalpy than boron can correctly answer a question that flips the expected order. This is exactly the kind of thinking JEE Main wants to test, and this is exactly why this blog focuses only on exceptions rather than repeating basic rules you already know.

Another reason exceptions are so popular in JEE Main is that they connect many chapters together. A single concept, such as the inert pair effect, can explain the behaviour of thallium in the boron family, tin and lead in the carbon family, and bismuth in the nitrogen family, all at once. Once you understand the underlying logic, you do not need to memorise three separate facts. You only need to remember one idea and apply it three times. This blog is structured so that you build this kind of connected understanding rather than disconnected, isolated facts.

Section 1: Exceptions in Electronic Configuration

The basic rules for filling electrons are the Aufbau principle, Pauli exclusion principle, and Hund’s rule. Most elements obey these rules in a straightforward way. But a few elements break the expected pattern because nature prefers extra stability from half-filled or fully filled subshells.

Chromium and Copper (3d series)

Based on the normal filling order, chromium (atomic number 24) should have the configuration [Ar] 3d4 4s2. But the actual configuration is [Ar] 3d5 4s1. This happens because a half-filled d-subshell (3d5) along with a half-filled s-subshell (4s1) gives extra stability through something called exchange energy.

Similarly, copper (atomic number 29) is expected to be [Ar] 3d9 4s2, but the actual configuration is [Ar] 3d10 4s1. A fully filled 3d10 subshell is more stable than a partially filled one, so one electron from 4s jumps into 3d.

Chromium (Cr): expected 3d4 4s2, actual 3d5 4s1
Copper (Cu): expected 3d9 4s2, actual 3d10 4s1
Molybdenum (Mo): similar to chromium, actual is 4d5 5s1
Silver (Ag): similar to copper, actual is 4d10 5s1

Exceptions in the Lanthanides and Actinides

In the f-block, you will find more such surprises. For example, in lanthanum (La), the electron goes into the 5d orbital instead of 4f, because at that point 5d is slightly more stable. This is why lanthanum is sometimes placed with the d-block, even though it is usually shown in the f-block table.

The same thing happens with gadolinium (Gd), where a half-filled 4f7 along with one 5d electron gives extra stability, similar to the chromium case.

Quick Tip

Whenever you see a question about “unexpected” electronic configuration, first check if a half-filled or fully filled subshell is involved. Nine times out of ten, that is the reason behind the exception.

Section 2: Exceptions in Periodic Properties

Ionisation Enthalpy: Why Some Trends Break

Normally, ionisation enthalpy increases as you move from left to right in a period because the nuclear charge increases. But there are clear exceptions you must remember.

Be vs B: Beryllium has a higher ionisation enthalpy than boron, even though boron comes after beryllium. This is because beryllium has a fully filled 2s2 configuration, which is more stable and harder to remove an electron from. Boron’s electron is in the 2p orbital, which is slightly higher in energy and easier to remove.
N vs O: Nitrogen has a higher ionisation enthalpy than oxygen. Nitrogen has a half-filled 2p3 configuration (one electron in each of the three p orbitals), which gives extra stability. Removing an electron from oxygen’s 2p4 is comparatively easier because it relieves some electron-electron repulsion.
Mg vs Al and P vs S: The same pattern repeats in period 3, exactly like Be-B and N-O, because the underlying reason (half-filled and fully filled stability) is the same.

Electron Gain Enthalpy: Why Fluorine Is Not the Most Negative

You may expect fluorine to have the most negative electron gain enthalpy in its group, since it is the smallest halogen. But chlorine actually has a more negative electron gain enthalpy than fluorine.

The reason is the small size of the fluorine atom. When an extra electron enters the already small 2p subshell of fluorine, there is strong electron-electron repulsion, which reduces the energy released. Chlorine is bigger, so the new electron experiences less repulsion, and more energy is released overall.

Order of electron gain enthalpy (more negative to less negative) for halogens: Cl > F > Br > I
Notice that fluorine is second, not first, which surprises many students.

Atomic and Ionic Radius Exceptions

Lanthanide contraction is a very important exception-based topic. Because of poor shielding by 4f electrons, the atomic radii of elements after the lanthanides (such as hafnium) are almost the same as the elements just above them in the d-block (such as zirconium). This is why zirconium and hafnium have almost identical chemical properties and are difficult to separate.

Another point to remember is that the size of a cation is always smaller than its parent atom, while the size of an anion is always larger than its parent atom. This is true without exception and is often used to test if you understand basic radius concepts.

Section 3: Exceptions in Chemical Bonding

Bond Angle and Shape Exceptions

VSEPR theory predicts shapes based on the number of bond pairs and lone pairs. But real bond angles are often slightly different from the ideal value because lone pairs repel more strongly than bond pairs.

NH3 vs PH3: Ammonia has a bond angle of about 107 degrees, while phosphine has a bond angle close to 93 degrees. This is unexpected if you assume all hydrides behave the same way. The reason is that nitrogen is more electronegative and pulls bonding electrons closer, which reduces lone pair to bond pair repulsion less than you would think, and the smaller size of nitrogen also matters. As you go down the group (PH3, AsH3, SbH3), bond angles keep decreasing.
H2O bond angle: Water has a bond angle of about 104.5 degrees, less than the ideal tetrahedral angle of 109.5 degrees, because of two lone pairs on oxygen pushing the bonded hydrogen atoms closer together.

Why BF3 and BCl3 Do Not Behave the Same

Boron trifluoride (BF3) is a weaker Lewis acid than boron trichloride (BCl3), which seems strange because fluorine is more electronegative than chlorine. You would expect BF3 to want electrons more, not less.

The exception is explained by back bonding. In BF3, the small fluorine atoms can donate their lone pair electrons into the empty p-orbital of boron, partially filling it and reducing boron’s tendency to accept electrons from outside. Chlorine is larger, so this back bonding is weaker in BCl3, making BCl3 a stronger Lewis acid.

Order of Lewis acidic strength: BI3 > BBr3 > BCl3 > BF3
This order is the exact reverse of what electronegativity alone would suggest, which is exactly why JEE likes to test it.

Diagonal Relationship: When Elements Break Their Own Group Pattern

Some elements behave more like an element diagonally placed in the periodic table rather than the elements in their own group. This is called a diagonal relationship, and it is an important exception to normal group trends.

Lithium and Magnesium: Lithium behaves more like magnesium than like sodium or potassium. Both lithium and magnesium form covalent bonds more easily, both have lower solubility for their carbonates, and both decompose their nitrates to give the oxide.
Beryllium and Aluminium: Beryllium shows several properties similar to aluminium rather than to magnesium or calcium, such as forming amphoteric oxides and covalent halides.

Section 4: Exceptions in s-Block Elements

Lithium: The Odd One in Group 1

Lithium is the smallest alkali metal, and its small size and high charge density make it behave differently from sodium, potassium, and the other alkali metals.

Lithium carbonate decomposes on heating to give lithium oxide and carbon dioxide, but sodium and potassium carbonates are stable to heat and do not decompose easily.
Lithium nitrate on heating gives lithium oxide, while sodium and potassium nitrates give the nitrite on heating.
Lithium forms a stable covalent bond character in many of its compounds because of its high polarising power, unlike the more ionic compounds of the other alkali metals.
Lithium is the only alkali metal that reacts directly with nitrogen gas to form lithium nitride (Li3N), something sodium and potassium do not do under normal conditions.

Beryllium: The Odd One in Group 2

Just like lithium in group 1, beryllium does not behave like the rest of group 2 (magnesium, calcium, strontium, barium).

Beryllium does not react with water, while the other group 2 elements do, especially calcium, strontium and barium.
Beryllium oxide and beryllium hydroxide are amphoteric, meaning they react with both acids and bases, while the oxides and hydroxides of the rest of the group are basic.
Beryllium forms mostly covalent compounds because of its small size and high charge density, while the rest of group 2 forms predominantly ionic compounds.

Quick Tip

Remember this pattern: the very first member of almost every group in the periodic table behaves a little differently from the rest of the group. This is sometimes called the “anomalous behaviour of the first member” and it is one of the most repeated exception themes in JEE Main.

Section 5: Exceptions in p-Block Elements

Boron Family Exceptions

Boron does not form B3+ ions easily because the sum of the first three ionisation enthalpies is too high. So boron compounds are mostly covalent, even though boron is in the same group as aluminium, which does form ionic compounds more readily in many of its salts.

Another classic exception is the melting and boiling point trend in the boron family. You would expect boiling points to decrease smoothly down the group, but boron itself has an unusually high melting point because of its strong covalent network structure, much higher than aluminium, which is a metal with a lower melting point.

Carbon Family Exceptions

Carbon shows catenation (the ability to form long chains with itself) much more strongly than silicon, germanium, tin, or lead, even though they are all in the same group. This is because the carbon-carbon bond is much stronger than silicon-silicon or other heavier bonds in the group.

Carbon also does not show a stable +2 oxidation state easily, while lead actually prefers the +2 state over +4, which is the reverse of what you might expect moving down a group where the lower oxidation state usually becomes more stable for heavier elements. This effect, where the lower oxidation state becomes more stable down the group, is called the inert pair effect, and it is itself an exception you must remember clearly for tin and lead, and also for thallium in the boron family.

Nitrogen Family Exceptions

Nitrogen cannot form a five-coordinate compound like PCl5 because nitrogen does not have d-orbitals available in its valence shell. Phosphorus, arsenic, and antimony, which do have accessible d-orbitals, can form such five-coordinate compounds.

Nitrogen also exists as a stable diatomic gas (N2) with a strong triple bond, while phosphorus exists as P4 molecules. This is an exception in molecular structure that often confuses students who assume all group 15 elements form similar simple molecules.

Oxygen Family and Halogen Family Exceptions

Oxygen shows a maximum covalency of 4, while sulfur and the heavier elements in the group can show covalency of 6, again because oxygen lacks accessible d-orbitals while sulfur has them.

In the halogen family, fluorine never shows a positive oxidation state, while chlorine, bromine and iodine commonly show positive oxidation states such as +1, +3, +5 and +7. This happens because fluorine is the most electronegative element of all and also has no d-orbitals to use for expanding its bonding.

Fluorine also forms only one type of oxoacid (HOF), while chlorine forms several oxoacids (HOCl, HOClO, HOClO2, HOClO3). This is directly connected to the same reason: lack of d-orbitals and extremely high electronegativity in fluorine.

Noble Gas Exceptions

Noble gases were once believed to be completely unreactive. But xenon, and to a smaller extent krypton, actually do form real compounds, such as XeF2, XeF4, and XeF6. Helium, neon, and argon still do not form any known stable compounds, but xenon’s reactivity itself was a huge exception when discovered, since it broke the old belief that group 18 elements never react.

There is a simple reason why xenon reacts while helium and neon do not. Xenon is a much larger atom, so its outer electrons are held less tightly by the nucleus and are easier to remove or share. Helium and neon are too small and their electrons are held too strongly, so they almost never take part in bond formation. This size-based reasoning is the same type of logic you should apply whenever a question asks you to compare reactivity within any single group of the periodic table.

Section 6: Exceptions in d-Block and f-Block Elements

Why Zinc, Cadmium, and Mercury Are Often Excluded from Transition Metals

Zinc, cadmium, and mercury have a completely filled d10 configuration in both their atomic and common ionic forms. Because a transition element is defined as one with a partially filled d-subshell, these three elements do not strictly qualify as transition metals, even though they are placed in the d-block of the periodic table. This single fact is asked again and again in JEE Main.

Irregular Trends in Atomic Size and Density

In the d-block, atomic radius does not decrease smoothly across a period like it does in the s and p blocks. The radius first decreases, then becomes almost constant in the middle of the series, and may even increase slightly near the end. This happens because the added d-electrons shield the nuclear charge from the outer electrons, balancing out the increasing nuclear pull.

Similarly, density increases gradually across the 3d series but does not always increase perfectly in order, since atomic size and atomic mass both change at slightly different rates.

Variable Oxidation States and the Stability of +2 vs +3

Most transition metals show variable oxidation states, but the relative stability does not always follow a simple pattern. For example, Mn2+ is unusually stable compared to its neighbours because it has a half-filled 3d5 configuration. Similarly, Fe3+ (3d5) is more stable than Fe2+ (3d6) for the same half-filled stability reason, even though Fe2+ might seem like the simpler, lower-energy option.

Cu2+ is more stable in aqueous solution than Cu+, even though Cu+ has a fully filled 3d10 configuration which should be more stable on its own. This apparent contradiction exists because Cu2+ has a much higher hydration enthalpy in water, which compensates for the loss of that extra stability, making Cu2+ the commonly seen ion in solution.

Lanthanides and Actinides: Oxidation State Surprises

Although +3 is the most common and expected oxidation state for lanthanides, some of them also show +2 or +4 states when it leads to a half-filled or fully filled f-subshell. For example, cerium commonly shows +4 (reaching a stable f0 configuration) and europium commonly shows +2 (reaching a stable f7 half-filled configuration).

Actinides show a much wider range of oxidation states compared to lanthanides because the 5f, 6d, and 7s orbitals are closer in energy to each other, so more electrons are available for bonding. This greater variability in actinides compared to the more limited variability in lanthanides is itself a commonly tested exception.

Catalytic Behaviour and Magnetic Exceptions

Transition metals are well known for their catalytic activity, and this too is connected to an exception-based idea. Most transition metals and their compounds work well as catalysts because they can change their oxidation state easily and provide a surface where reactant molecules can temporarily bond. But this is not equally true for every transition metal. Scandium, for instance, is a poor catalyst compared to manganese or iron, because scandium has very few stable oxidation states to switch between.

Magnetic behaviour also has its own exceptions worth remembering. The magnetic moment of a transition metal ion usually depends only on the number of unpaired electrons, and this works well for most 3d ions when calculated using the simple spin-only formula. However, for some 4d and 5d series ions, and for several lanthanide ions, the experimental magnetic moment does not match the simple spin-only value, because orbital motion of electrons also contributes to the magnetism in these cases. This is why JEE Main sometimes specifically asks about 3d series ions when testing the spin-only formula, since it is most reliable there.

Section 7: Exceptions in Coordination Compounds

Coordination chemistry has its own set of surprises that depend on the strength of the ligand field, and these are slightly more advanced but still appear in JEE Main.

Pairing of electrons depends on ligand strength: A metal ion with the same charge can show different magnetic behaviour depending on whether the ligand is strong field or weak field. For example, [Fe(CN)6]4- is diamagnetic (low spin) because CN- is a strong field ligand that forces electron pairing, while [FeF6]4- is paramagnetic (high spin) because F- is a weak field ligand.
Same metal, same oxidation state, different geometry: Nickel(II) complexes can be square planar or tetrahedral depending on the ligand, even though the metal and its oxidation state stay the same. This goes against the simple idea that geometry depends only on the central metal ion.
Colour exceptions: Zinc and scandium complexes are usually colourless, even though most transition metal complexes are coloured, because Zn2+ has a fully filled d10 configuration and Sc3+ has an empty d0 configuration. Colour in transition metal complexes comes from d-to-d electron transitions, and these need a partially filled d-subshell, which neither zinc nor scandium has.

Revision Quiz: Test Yourself on Inorganic Chemistry Exceptions

Now it is time to check how much you remember. This quiz has 25 multiple choice questions, written in the same style as JEE Main. Try to attempt every question without looking back at the blog first. Write your answers on a rough sheet, then check them against the answer key given right after the quiz.

How to use this quiz

Give yourself exactly 20 minutes for all 25 questions, just like a mini exam. This builds your speed along with your concept. After checking your score, go back and re-read only the sections where you made a mistake.

Q1. Which of the following shows the correct electronic configuration exception?

(A) Cr: 3d4 4s2

(B) Cu: 3d9 4s2

(D) Fe: 3d5 4s3

Q2. The first ionisation enthalpy of nitrogen is higher than that of oxygen because of:

(A) Larger atomic size of oxygen

(B) Half-filled stability in nitrogen’s 2p3

(D) Oxygen being a gas at room temperature

Q3. Among the halogens, which one has the most negative electron gain enthalpy?

(A) Fluorine

(B) Chlorine

(D) Iodine

Q4. Which is the correct order of Lewis acid strength for boron trihalides?

(A) BF3 > BCl3 > BBr3 > BI3

(B) BI3 > BBr3 > BCl3 > BF3

(D) All boron trihalides have equal acidic strength

Q5. The bond angle in PH3 is smaller than in NH3 mainly because:

(A) Phosphorus has more lone pairs than nitrogen

(B) Nitrogen is less electronegative than phosphorus

(D) PH3 does not have any lone pair

Q6. Lithium shows a diagonal relationship with which element?

(A) Sodium

(B) Beryllium

(D) Boron

Q7. Which oxide and hydroxide of group 2 is amphoteric, unlike the rest of the group?

(A) Magnesium oxide and hydroxide

(B) Beryllium oxide and hydroxide

(D) Barium oxide and hydroxide

Q8. Why does lithium nitrate decompose differently from sodium nitrate on heating?

(A) Lithium nitrate is more ionic than sodium nitrate

(B) Lithium has a smaller size and higher polarising power

(D) Lithium nitrate does not contain oxygen

Q9. Which p-block exception explains why lead prefers the +2 oxidation state over +4?

(A) Catenation

(B) Lanthanide contraction

(D) Back bonding

Q10. Why can phosphorus form PCl5 but nitrogen cannot form NCl5?

(A) Nitrogen is more reactive than phosphorus

(B) Nitrogen does not have accessible d-orbitals

(D) PCl5 is an ionic compound

Q11. Fluorine does not show a positive oxidation state mainly because:

(A) It has the smallest atomic radius among halogens

(B) It is the most electronegative element and has no available d-orbitals

(D) It is a liquid at room temperature

Q12. Which noble gas was the first to be shown to form real chemical compounds?

(A) Helium

(B) Neon

(D) Xenon

Q13. Zinc, cadmium, and mercury are usually excluded from the typical definition of transition metals because:

(A) They are radioactive

(B) They have a fully filled d10 configuration

(D) They are found only in liquid form

Q14. Mn2+ is unusually stable among the 3d series ions because of:

(A) Its large ionic size

(B) A half-filled 3d5 configuration

(D) Strong covalent bonding

Q15. Cu2+ is more commonly found in aqueous solution than Cu+, even though Cu+ has a fully filled d-subshell, because:

(A) Cu2+ has a higher hydration enthalpy that compensates for lost stability

(B) Cu+ is radioactive

(D) Copper does not form Cu+ at all

Q16. Cerium commonly shows the +4 oxidation state among lanthanides because reaching +4 gives it:

(A) A half-filled f7 configuration

(B) An empty f0 configuration

(D) No change in electronic configuration

Q17. Which statement about actinides versus lanthanides is correct?

(A) Actinides show fewer oxidation states than lanthanides

(B) Lanthanides show more variable oxidation states than actinides

(D) Both show exactly the same range of oxidation states

Q18. [Fe(CN)6]4- is diamagnetic while [FeF6]4- is paramagnetic. This is an example of:

(A) Lanthanide contraction

(B) Effect of ligand field strength on electron pairing

(D) Inert pair effect

Q19. Zn2+ and Sc3+ complexes are usually colourless because:

(A) They do not form complexes at all

(B) They have either completely filled or completely empty d-orbitals, so no d-to-d transition is possible

(D) They do not have any ligands attached

Q20. Hafnium and zirconium have almost the same atomic radius mainly due to:

(A) Diagonal relationship

(B) Inert pair effect

(D) Back bonding

Q21. Which of the following correctly shows why carbon shows strong catenation compared to silicon?

(A) Carbon has more valence electrons than silicon

(B) The carbon-carbon bond is much stronger than the silicon-silicon bond

(D) Carbon has d-orbitals available for bonding

Q22. The maximum covalency of oxygen is 4 while sulfur can show a covalency of 6 because:

(A) Oxygen is more reactive than sulfur

(B) Sulfur has accessible d-orbitals while oxygen does not

(D) Sulfur has a smaller atomic radius

Q23. Beryllium does not react with water under normal conditions, unlike the rest of group 2, mainly because of its:

(A) Large atomic size

(B) Strong covalent character and protective oxide layer

(D) Position in the f-block

Q24. Which pair correctly shows the anomalous behaviour of the first member of a group?

(A) Sodium and Magnesium

(B) Lithium and Beryllium showing different behaviour from their own groups

(D) Caesium and Barium having identical properties

Q25. Nickel(II) complexes can be either square planar or tetrahedral with the same oxidation state because:

(A) Geometry depends only on the metal, never on the ligand

(B) Geometry can depend on the nature of the ligand attached, not on the metal alone

(D) Square planar geometry is impossible for nickel

Answer Key

Check your answers below. For every wrong answer, go back to the related section above and read it one more time before moving to the next topic.

Q1: C Q2: B Q3: B Q4: B Q5: C

Q6: C Q7: B Q8: B Q9: C Q10: B

Q11: B Q12: D Q13: B Q14: B Q15: A

Q16: B Q17: C Q18: B Q19: B Q20: C

Q21: B Q22: B Q23: B Q24: B Q25: B

Final Revision Tips Before Your JEE Main Exam

Make a single page of only exceptions, not full topics. This page becomes your most valuable revision tool in the last few days before the exam.
Whenever you learn a new topic in inorganic chemistry, immediately ask yourself, “Is there an exception to this rule?” This habit alone can improve your accuracy a lot.
Group exceptions by their root cause. Most of them come from only a few reasons: half-filled or fully filled stability, lack of d-orbitals, inert pair effect, lanthanide contraction, back bonding, and anomalous behaviour of the first group member. If you remember these five or six root causes, you can explain almost every exception in this blog without memorising each one separately.
Retake this quiz after two or three days. If your score improves without looking at the blog again, you know the concept is now permanently in your memory.
Practice previous year JEE Main questions on these exact topics, since the examiners often repeat the same type of exception-based question with just the elements changed.

Inorganic chemistry exceptions may feel like a long list to remember, but once you understand the small number of reasons behind them, the whole topic becomes much easier. Keep practising, keep revising this quiz, and you will feel much more confident handling exception-based questions on your JEE Main exam day. All the best for your preparation!

Frequently Asked Questions on Inorganic Chemistry Exceptions

Why does JEE Main ask so many exception-based questions in inorganic chemistry?

JEE Main wants to test real understanding, not just memorised rules. Exceptions check whether you understand the reason behind a trend, such as half-filled stability or the inert pair effect, rather than just remembering the trend itself.

What is the most common reason behind inorganic chemistry exceptions?

Most exceptions in this topic come from only a handful of root causes: half-filled or fully filled subshell stability, the inert pair effect, lanthanide contraction, the absence of d-orbitals in second period elements, and back bonding. If you understand these five ideas well, you can explain almost every exception listed in this blog.

Is it necessary to memorise every single exception separately?

No. It is much more efficient to understand the small number of root causes mentioned above. Once you know why an exception happens, you can apply that same logic to a new element or compound you have never seen before, which is exactly what JEE Main often expects you to do.

How many marks can exception-based questions affect in JEE Main chemistry?

It varies from year to year, but inorganic chemistry exceptions regularly appear in multiple questions across periodic properties, chemical bonding, and d-block and f-block chapters. Since each question carries equal weight, even two or three exception-based questions can meaningfully change your score, so they are worth revising carefully.

What is the best way to revise these exceptions just before the exam?

Make a single summary page that lists only the exceptions, grouped by their root cause rather than by chapter. Read this page on the morning of your exam, and retake the quiz in this blog a day or two before the exam to confirm that the concepts have actually stayed in your memory.

Poonam Pareek

Poonam Pareek is the Founder, CEO, and Lead Writer of StudentsTalk.in, an education-focused platform dedicated to helping students stay informed about the latest academic updates, scholarships, entrance exams, career opportunities, government schemes, and study resources. With a passion for education and student success, she creates informative, easy-to-understand content.