Examius
🇮🇳 KCET · flashcards
KCET Chemistry Flashcards
51 question-and-answer cards covering Chemistry as it is examined in KCET. 24 of them are printed below, taken from across the deck — no signup, no paywall on the preview.
24 sample cards from the Chemistry deck
Sampled from the end of the deck, so these are different cards from the ones shown on the syllabus page.
Write the Nernst equation for an electrode at 298 K.
E = E° − (0.0591/n) log Q, where n = number of electrons transferred and Q = reaction quotient.
State Faraday's first law of electrolysis.
The mass of a substance deposited or liberated at an electrode is directly proportional to the quantity of electric charge passed (m ∝ Q); 1 Faraday = 96500 C = 1 mole of electrons.
What is the relationship between standard cell potential and Gibbs energy?
ΔG° = −nFE°cell, where n = moles of electrons, F = Faraday constant (96500 C/mol).
Define the rate law and order of a reaction.
The rate law expresses rate as rate = k[A]^x[B]^y; the order is the sum (x + y) of the exponents of concentration terms.
Give the integrated rate equation and half-life for a first-order reaction.
k = (2.303/t) log([A]₀/[A]); half-life t₁/₂ = 0.693/k (independent of initial concentration).
State the Arrhenius equation and what it describes.
k = A·e^(−Ea/RT), relating the rate constant to activation energy (Ea) and temperature; A is the pre-exponential factor.
Define oxidation and reduction in terms of electrons and oxidation number.
Oxidation = loss of electrons / increase in oxidation number; Reduction = gain of electrons / decrease in oxidation number.
What is a disproportionation reaction? Give an example.
A reaction in which the same element is simultaneously oxidised and reduced. Example: 2H₂O₂ → 2H₂O + O₂ (oxygen goes from −1 to −2 and 0).
State the modern periodic law.
The physical and chemical properties of elements are periodic functions of their atomic numbers.
How do atomic radius and ionization enthalpy vary across a period and down a group?
Across a period: atomic radius decreases, ionization enthalpy increases. Down a group: atomic radius increases, ionization enthalpy decreases.
Why is hydrogen placed with both group 1 and group 17 in some periodic tables?
Like group 1 it has one valence electron and forms H⁺; like group 17 it needs one electron to complete its shell and forms H⁻ (hydride), so it shows resemblance to both.
What is the trend in reactivity and atomic size down group 1 (alkali metals)?
Down group 1, atomic size increases and reactivity increases because the outer electron is more easily lost (lower ionization enthalpy).
What is the inert pair effect in p-block elements?
The reluctance of the ns² electrons to participate in bonding for heavier p-block elements, making lower oxidation states more stable down the group (e.g., Pb²⁺ more stable than Pb⁴⁺).
What are interhalogen compounds? Give the general types.
Compounds formed between two different halogens, of types XX', XX'3, XX'5, XX'7 (e.g., ClF, BrF₃, IF₅, IF₇).
Why do transition (d-block) elements show variable oxidation states and form coloured compounds?
Variable oxidation states arise from similar energies of (n−1)d and ns electrons; colour arises from d-d electronic transitions when partially filled d-orbitals absorb visible light.
What are lanthanoid contraction and its consequence?
The steady decrease in atomic/ionic radii across the lanthanoids due to poor shielding by 4f electrons; it causes second and third row transition elements to have similar sizes (e.g., Zr and Hf).
State Werner's coordination theory: primary and secondary valencies.
Primary valency = oxidation state, satisfied by negative ions, ionizable. Secondary valency = coordination number, satisfied by ligands, non-ionizable and directional, giving the complex its geometry.
Define ligand, coordination number, and denticity.
A ligand is an ion/molecule that donates a lone pair to the central metal. Coordination number = number of donor atoms bonded to the metal. Denticity = number of donor sites a ligand uses (mono-, bi-, polydentate).
What does crystal field theory say causes colour and magnetism in complexes?
Ligands split the metal d-orbitals into different energy levels (Δo for octahedral). d-d transitions across this gap give colour; the number of unpaired electrons (high vs low spin) determines magnetic behaviour.
What are electrophiles and nucleophiles?
Electrophiles are electron-deficient species that accept electron pairs (e.g., NO₂⁺, H⁺); nucleophiles are electron-rich species that donate electron pairs (e.g., OH⁻, CN⁻, NH₃).
Distinguish inductive effect, resonance effect, and hyperconjugation.
Inductive: permanent polarization of σ bonds due to electronegativity difference. Resonance: delocalization of π/lone-pair electrons over the molecule. Hyperconjugation: delocalization of σ(C-H) electrons into an adjacent empty p or π orbital.
State Markovnikov's rule and the anti-Markovnikov (peroxide) effect.
Markovnikov: in addition of HX to an unsymmetrical alkene, H adds to the carbon with more hydrogens. Peroxide effect: with HBr and peroxides, addition is anti-Markovnikov (free-radical mechanism).
Distinguish SN1 and SN2 mechanisms in haloalkanes.
SN1: two-step, carbocation intermediate, first-order, favoured by tertiary halides and polar protic solvents, gives racemization. SN2: one-step, single transition state, second-order, favoured by primary halides, gives inversion of configuration (Walden inversion).
Name the functional-group test to distinguish aldehydes from ketones.
Tollens' reagent (ammoniacal AgNO₃) gives a silver mirror with aldehydes but not ketones; Fehling's solution gives a red-brown Cu₂O precipitate with aliphatic aldehydes only.
What this deck covers
The Chemistry deck follows the KCET Chemistry syllabus — 6 chapters and 25 topics — so questions land on material that is genuinely examinable rather than trivia around it. That works out to roughly 8.5 cards per chapter.
Answers are written to be recallable, not just readable — averaging about 160 characters, which is long enough to carry the reasoning and short enough to say out loud.
A deck like this earns its keep on the second and third pass. Read the syllabus first so you know the shape of the subject, then use the cards to find the specific facts that have not stuck.
Chemistry flashcards FAQ
How many Chemistry flashcards are in this KCET deck?
51 cards. This page previews 24 of them, sampled evenly across the deck so you can judge the difficulty before installing anything.
Are these KCET flashcards free?
Yes. The preview here is free to read with no signup, and the full 51-card deck is free inside the Examius app.
What do the Chemistry cards cover?
They follow the KCET Chemistry syllabus — 6 chapters and 25 topics — so the questions track what is actually examinable.
How should I use these flashcards?
Read the syllabus first so you know the shape of the subject, then drill the deck. Examius schedules each card with spaced repetition, so cards you keep missing come back sooner and ones you know drift further apart.