20 imp topic chemistry series start

What is a Solution?
A homogeneous mixture of: ✔️ Solute (less amount)
✔️ Solvent (more amount)
📌 Examples:
Sugar in water
Salt in water
⭐ Types of Solutions (Based on Raoult’s Law)
🔹 #IdealSolution
📌 Obeys Raoult’s law at all concentrations
✔️ ΔHmix = 0
✔️ ΔVmix = 0
✔️ A–A ≈ B–B ≈ A–B interactions
📌 Examples:
Benzene + Toluene
n-Hexane + n-Heptane

#NonIdealSolution
📌 Does NOT obey Raoult’s law
✔️ ΔHmix ≠ 0
✔️ ΔVmix ≠ 0
✔️ A–B ≠ A–A or B–B interactions
⭐ Types of Non-Ideal Solutions

1️⃣ #PositiveDeviation
✔️ A–B interactions weaker
✔️ Vapour pressure ↑
✔️ Endothermic mixing (ΔH > 0)
📌 Examples:
Ethanol + Acetone
Acetone + CS₂

2️⃣ #NegativeDeviation
✔️ A–B interactions stronger
✔️ Vapour pressure ↓
✔️ Exothermic mixing (ΔH < 0)
📌 Examples:
Chloroform + Acetone
HNO₃ + Water

⭐ Azeotropes
📌 Constant boiling mixture
📌 Vapour composition = Liquid composition
✔️ Positive deviation → Minimum boiling azeotrope
✔️ Negative deviation → Maximum boiling azeotrope

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#ColligativeProperties
Properties depending on number of solute particles, not nature

⭐ 4 Colligative Properties

1️⃣ Relative Lowering of Vapour Pressure
📌 ΔP / P° = n₂ / n₁
📌 Raoult’s law based

2️⃣ Elevation of Boiling Point
📌 ΔTb = Kb · m
✔️ Boiling point ↑
✔️ Kb → Molal elevation constant
3️⃣ Depression of Freezing Point
📌 ΔTf = Kf · m
✔️ Freezing point ↓
✔️ Kf → Molal depression constant
4️⃣ Osmotic Pressure
📌 π = CRT
✔️ Most reliable colligative property
✔️ Used to find molar mass


⭐ #Van’tHoffFactor (i)
📌 i = Actual number of particles / Expected number
✔️ Association → i < 1
✔️ Dissociation → i > 1
✔️ Non-electrolyte → i = 1
📌 Modified formulas:
ΔTb = iKb m
ΔTf = iKf m
π = iCRT

#NEETHOTPOINTS
✔️ Ideal solution → ΔHmix = 0
✔️ Positive deviation → Weak A–B attraction
✔️ Negative deviation → Strong A–B attraction
✔️ Azeotrope → Constant boiling mixture
✔️ Most accurate colligative property → Osmotic pressure

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#ElectrochemicalCell
Device that converts chemical energy → electrical energy
📌 Components:
Anode → Oxidation
Cathode → Reduction
📌 Electron flow: Anode → Cathode
🔋 EMF of Cell
📌 E°cell = E°cathode − E°anode
✔️ Standard conditions: 1 M, 1 atm, 298 K

#NernstEquation (Very High Yield )
🌱 Used to calculate cell potential at non-standard conditions
⭐ General form:

E=E°-RT/NF LN Q

At 298K

E=E°-0.0591/n LogQ

Where
E = Cell potential
E° = Standard potential
n = Number of electrons transferred
Q = Reaction quotient

#Specialcases (Direct MCQ)
✔️ For concentration cell:

E=0.059/n log C2/C1

✔️ At equilibrium:
E = 0
Q = K
E°=0.059/n logK

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Conductivity
🌱 Electrical Conductance (G)
📌 Reciprocal of resistance
G=1/R
Unit: Siemens (S)

⭐ Specific Conductivity (κ)
Conductance of solution of: ✔️ 1 cm length
✔️ 1 cm² area
Depends on:
Concentration
Temperature
Nature of electrolyte

⭐ Molar Conductivity (Λm)
(Λm)=k×1000/C
Unit: S cm² mol⁻¹

📌 C = molarity
✔️ Increases on dilution
✔️ Maximum value at infinite dilution → Λ°m

Strong vs Weak Electrolyte
Feature :Strong :Weak
Ionisation :Complete :Partial
Λm with dilution :Slight ↑ :Sharp ↑
Kohlrausch law :✔️ Applicable
: ✔️ Applicable

#Kohlrausch’s Law
At infinite dilution:
Λm°=(Λm°+) + ((Λm°_)

✔️ Helps calculate:
Λ°m of weak electrolytes
Degree of dissociation
Ka, Kb

#NEETHOTPOINTS
✔️ Nernst eqn at 298 K → 0.0591/n
✔️ At equilibrium → E = 0
✔️ Unit of κ → S cm⁻¹
✔️ Λm increases with dilution
✔️ Maximum conductivity → Infinite dilution

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#ChemicalKinetics

⭐ First Order Reaction
🌱 Definition
Reaction whose rate depends on concentration of one reactant raised to power 1

📌 Rate law:
Rate =k(A)

🔢 Integrated Rate Equation
K=2.303/t log (A)•/(A)
📌 Where:
� = rate constant
� = time
� = initial concentration
� = concentration at time t

#Halflife (t½)
Time for concentration to become half
t1/2=0.693/k

⭐Independent of initial concentration (#veryimp )
Units
✔️ Rate constant (k) → s⁻¹
Graph (Direct MCQ)
✔️ log[A] vs t → Straight line
✔️ Slope → –k/2.303

Examples
✔️ Radioactive decay
✔️ Decomposition of N₂O₅
✔️ Acid hydrolysis of esters (pseudo-first order)

#NEETHOTPOINTS (1st Order)
✔️ Half-life independent of concentration
✔️ Unit of k → s⁻¹
✔️ Straight line graph → log[A] vs t
✔️ Pseudo-first order → One reactant in excess

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#Arrhenius Equation
🌱 Shows effect of temperature on rate constant
⭐ Equation

K=Ae^-ea/Rt
📌 Where:
� = rate constant
� = Arrhenius factor / frequency factor
� = Activation energy
� = Gas constant
� = Temperature (K)

⭐ Log Form (Most Used)
LogK=logA-Ea/2.303RT

⭐ Two Temperature Form
Log K2/K2=Ea/2.303R(T2-T1/T2•T1)

#Graph
✔️ log k vs 1/T → Straight line
✔️ Slope → –Ea / 2.303R
✔️ Intercept → log A

#Effect of Catalyst
✔️ Lowers Ea
✔️ Does NOT change ΔH
✔️ Increases rate

#NEETHOTPOINTS
✔️ Higher Ea → Slower reaction
✔️ Catalyst → lowers Ea
✔️ Temperature ↑ → k ↑
✔️ Straight line → log k vs 1/T
✔️ Unit of Ea → J mol⁻¹

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General Physical Properties (d-Block)
⭐ Atomic & Ionic Size
✔️ Size decreases from left → right (↑ nuclear charge)
✔️ After middle → almost constant (poor shielding by d-electrons)

⭐ Density
✔️ Increases from 3d → 4d → 5d
📌 Reason:
Increase in atomic mass
Lanthanide contraction (5d elements smaller → higher density)

⭐ Melting & Boiling Points
✔️ Very high
📌 Reason:
Strong metallic bonding
Involvement of d-electrons
📌 Exceptions:
Zn, Cd, Hg → low m.p.
✔️ Hg → liquid (weak metallic bonding)

⭐ Variable Oxidation States
✔️ Due to similar energy of (n−1)d & ns electrons
📌 Example:
Fe → +2, +3
Mn → +2 to +7

⭐ Magnetic Properties
✔️ Paramagnetic → unpaired electrons
✔️ Diamagnetic → all paired
📌 Magnetic moment:
U=√n(n+2)

⭐ Colour
✔️ Due to d–d transitions
✔️ Zn²⁺, Cd²⁺ → colourless (d¹⁰)
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🌟 Lanthanide Contraction (VERY HIGH YIELD 🔥)
🌱 Definition
Gradual decrease in atomic & ionic radii of lanthanides from La → Lu
#Reason
✔️ Poor shielding effect of 4f-electrons
✔️ Effective nuclear charge increases
🔥 Consequences of Lanthanide Contraction
1️⃣ Similar size of 4d & 5d elements
📌 Zr ≈ Hf
📌 Chemical properties similar
2️⃣ High density of 5d elements
📌 Reason:
Smaller size
Higher mass
3️⃣ Difficulty in separation of lanthanides
📌 Very similar radii & properties
4️⃣ Basic strength of hydroxides decreases
📌 La(OH)₃ > Lu(OH)₃
5️⃣ Decrease in ionic radii of Ln³⁺ ions
📌 Affects coordination number & complex formation
#NEETHOTPOINTS
✔️ Poor shielding → 4f electrons
✔️ Cause of Zr–Hf similarity → Lanthanide contraction
✔️ Colour in d-block → d–d transition
✔️ Colour in f-block → f–f transition
✔️ Most stable oxidation state of lanthanides → +3
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#CoordinationCompounds
Valence Bond Theory (VBT) & Isomerism (NCERT • NEET)

🌱 Coordination Compound
A compound in which: ✔️ Central metal atom/ion
✔️ Surrounded by ligands
✔️ Linked by coordinate bonds
📌 Example: [Co(NH₃)₆]Cl₃

⭐ #ValenceBondTheory (VBT)
🌱 Explains: ✔️ Geometry
✔️ Magnetic behaviour
✔️ Hybridisation

🔹 Postulates of VBT
✔️ Metal ion provides empty orbitals
✔️ Ligands donate lone pair
✔️ Overlap → coordinate bond
✔️ Paired/unpaired electrons decide magnetic nature

⭐ #Hybridisation&Geometry
Hybridisation :Geometry
d²sp³ / sp³d² :Octahedral
sp³ : Tetrahedral
dsp² : Square planar

#InnerOrbitalvsOuterOrbitalComplex
⭐ Inner Orbital Complex (Low spin)
✔️ Uses (n−1)d orbitals
✔️ Pairing of electrons occurs
✔️ Strong field ligands
📌 Example:
[Co(NH₃)₆]³⁺ → d²sp³ (octahedral)

⭐ Outer Orbital Complex (High spin)
✔️ Uses nd orbitals
✔️ No pairing
✔️ Weak field ligands
📌 Example:
[FeF₆]³⁻ → sp³d² (octahedral)

#MagneticNature (VBT)
✔️ Unpaired e⁻ → Paramagnetic
✔️ Paired e⁻ → Diamagnetic
📌 Example:
[Ni(CN)₄]²⁻ → Diamagnetic (dsp²)
[NiCl₄]²⁻ → Paramagnetic (sp³)
⚠️ Limitations of VBT
❌ Cannot explain colour
❌ Cannot explain strong vs weak ligands clearly
❌ No quantitative explanation of spectra

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Isomerism in Coordination Compounds
🌱 Compounds with same formula but different arrangement

⭐ #Structural Isomerism
1️⃣ Ionisation Isomerism
✔️ Exchange between ligand & counter ion
📌 Example:
[Co(NH₃)₅SO₄]Br
[Co(NH₃)₅Br]SO₄

2️⃣ Solvate (Hydrate) Isomerism
✔️ Water inside or outside coordination sphere
📌 Example:
[Cr(H₂O)₆]Cl₃
[Cr(H₂O)₅Cl]Cl₂·H₂O

3️⃣ Linkage Isomerism
✔️ Ambidentate ligands
📌 Example:
NO₂⁻ → nitro / nitrito
SCN⁻ → thiocyanato / isothiocyanato

4️⃣ Coordination Isomerism
✔️ Between cationic & anionic complexes
📌 Example:
[Co(NH₃)₆][Cr(CN)₆]
[Cr(NH₃)₆][Co(CN)₆]

⭐ #Stereoisomerism
1️⃣ Geometrical Isomerism
✔️ cis–trans
📌 Examples:
[Pt(NH₃)₂Cl₂]
[Co(NH₃)₄Cl₂]⁺

2️⃣ Optical Isomerism
✔️ Non-superimposable mirror images
✔️ d & l forms
📌 Example:
[Co(en)₃]³⁺

#NEETHOTPOINTS
✔️ Square planar → dsp²
✔️ Strong ligand → pairing → inner orbital
✔️ Ambidentate ligand → linkage isomerism
✔️ cis–trans in square planar & octahedral
✔️ Optical isomerism → no plane of symmetry

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#Haloalkanes
Alkanes in which H is replaced by halogen (F, Cl, Br, I)
📌 General formula: R–X
🔄 Nucleophilic Substitution Reactions
⭐ SN1 Reaction (Unimolecular)
🌱 Rate depends on only one species
📌 Rate = k[R–X]
🔹 Mechanism (2 Step)
1️⃣ R–X → R⁺ + X⁻ (Slow, RDS)
2️⃣ R⁺ + Nu⁻ → R–Nu (Fast)
⭐ Key Features
✔️ Formation of carbocation
✔️ Rearrangement possible
✔️ Racemisation occurs
✔️ Favoured by polar protic solvents
⭐ Order of Reactivity
3° > 2° > 1° > CH₃
📌 Reason: Carbocation stability
⭐ SN2 Reaction (Bimolecular)
🌱 Single step reaction
📌 Rate = k[R–X][Nu⁻]
🔹 Mechanism
✔️ Backside attack
✔️ Transition state formation
✔️ Simultaneous bond making & breaking
⭐ Key Features
✔️ No carbocation
✔️ No rearrangement
✔️ Inversion of configuration (Walden inversion)
✔️ Favoured by polar aprotic solvents
⭐ Order of Reactivity
CH₃ > 1° > 2° >> 3°
📌 Reason: Steric hindrance

SN1 vs SN2 (Direct MCQ)
Feature :SN1 :SN2
Steps :2 :1
Rate depends on :R–X :R–X & Nu⁻
Intermediate :Carbocation :None
Rearrangement :✔️ :❌
Stereochemistry :Racemisation
: Inversion
Favoured by ;3° haloalkane
: 1° haloalkane

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#PreparationofHaloalkanes
⭐ 1️⃣ From Alcohols
✔️ Using HX
📌 Reactivity:
3° > 2° > 1°
✔️ Using PCl₃ / PCl₅ / SOCl₂
📌 SOCl₂ best → gaseous by-products
⭐ 2️⃣ From Alkenes
✔️ Addition of HX (Markovnikov rule)
✔️ Anti-Markovnikov (HBr + peroxide)
⭐ 3️⃣ From Alkanes
✔️ Free radical halogenation
✔️ Less selective
⭐ 4️⃣ Finkelstein Reaction
✔️ R–Cl / R–Br + NaI (acetone) → R–I
⭐ 5️⃣ Swarts Reaction
✔️ R–Cl / R–Br → R–F
✔️ Using AgF / Hg₂F₂
#NEETHOTPOINTS
✔️ SN1 → Carbocation intermediate
✔️ SN2 → Walden inversion
✔️ 3° haloalkane → SN1 favoured
✔️ SOCl₂ → best for R–Cl
✔️ Anti-Markovnikov → HBr + peroxide

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#Alcohols
Organic compounds containing –OH group attached to sp³ carbon
📌 General formula: R–OH

⭐ #PreparationofAlcohols
1️⃣ From Alkenes
✔️ Acid-catalysed hydration
RCH=CH2+H+/H20 = RCH(OH) -CH3
📌 Follows Markovnikov’s rule

Hydroboration–Oxidation
RCH=CH2+BH3/THF, H2O2/OH^- = RCH2-CH2OH
📌 Anti-Markovnikov, no rearrangement

2️⃣ From Haloalkanes
R-X+Aq KOH= ROH

3️⃣ From Aldehydes & Ketones
✔️ Reduction using:
NaBH₄
LiAlH₄
📌 Aldehyde → 1° alcohol
📌 Ketone → 2° alcohol

4️⃣ From Grignard Reagent
RMGX+ HCHO=1° alcohol
RMGX+ RCHO=2°alcohol
RMGX+R2CO=3°alcohol


#NEETHOTPOINTS (Alcohol)
✔️ Hydroboration → Anti-Markovnikov
✔️ NaBH₄ milder than LiAlH₄
✔️ Grignard reagent + HCHO → 1° alcohol

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Ethers
Organic compounds with –O– linkage
📌 General formula: R–O–R′

Williamson Ether Synthesis (Very High Yield 🔥)
📌 Best method to prepare ethers
RONA+R'X = ROR' + Nax
✔️ Involves SN2 mechanism
✔️ Best with 1° haloalkane
❌ 3° haloalkane → Elimination occurs
📌 For unsymmetrical ether:
Use bulky group as alkoxide
Smaller group as haloalkane

⭐ Reaction of Ether with HI
📌 Ether cleavage by HI / HBr
🔹 Mechanism
✔️ Protonation of ether oxygen
✔️ I⁻ attacks alkyl group

#CaseWiseReaction

1️⃣ Symmetrical Ether
R-O-R+ 2HI = 2RI + H20

2️⃣ Unsymmetrical Ether
✔️ If one group is 3° → Cleavage at 3° carbon (SN1)
✔️ If both are 1° → I⁻ attacks less hindered carbon (SN2)
📌 Example:

CH3-O-C2H5 + HI = Ch3I + C2H5OH

NEETHOTPOINTS (Ether)
✔️ Williamson → SN2 reaction
✔️ Best haloalkane → 1°
✔️ Ether cleavage → HI > HBr
✔️ 3° ether → SN1 cleavage
✔️ Unsymmetrical ether → less hindered side breaks

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Aldehyde Ketone & Carbohydrates

1️⃣ Important Name Reactions & Tests
✅ #Aldehydes
⭐Tollens’ Test
Aldehyde + [Ag(NH3) 2}^+→ Silver mirror
👉 Ketone ❌ (except α-hydroxy ketone

⭐Fehling’s Test 🔵➡️🔴
Aliphatic aldehyde → Red ppt (Cu₂O)
👉 Aromatic aldehyde ❌

⭐Benedict’s Test
Similar to Fehling’s (for reducing sugars)

⭐Schiff’s Test
Pink colour → Aldehyde present


#Ketones
⭐Iodoform Test 🟡
Group present: –COCH₃
Positive for:
Acetone
Ethanol
2° alcohol with –CHOH–CH₃

⭐ 2,4-DNP Test
Orange / yellow ppt → Carbonyl present (Ald/Ket)

#ImportantNameReactions

⭐Aldol Condensation
Aldehyde/Ketone with α-H → β-hydroxy aldehyde → α,β-unsat compound

⭐ Cannizzaro Reaction
Aldehyde without α-H → Alcohol + Acid (base medium)

⭐Clemmensen Reduction
Zn-Hg /HCL - C=O → –CH₂–

⭐Wolff–Kishner Reduction
NH2NH2/KOH→ C=O → –CH₂–

#CarbohydratesImportantTests
Molisch Test → Violet ring (general test)
Fehling / Benedict → Red ppt (reducing sugar)
Barfoed Test → Monosaccharide (+ fast)
Iodine Test → Blue colour (starch)
Osazone Test → Needle shaped crystals (glucose = fructose)

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2: #NucleophilicAdditionReactions
📌 General Reaction
RCHO/R-CO-R'+NU^- = Additional product

📌 Reactivity Order
Aldehyde > Ketone
(H- > CH₃- > bulky alkyl)

#ImportantNucleophiles
HCN → Cyanohydrin
NaHSO₃ → Bisulphite compound
RMgX (Grignard)
HCHO → 1° alcohol
Aldehyde → 2° alcohol
Ketone → 3° alcohol
NH₂OH → Oxime
NH₂NH₂ → Hydrazone
2,4-DNP → Orange ppt

#NCERTDirectPoints
Aldehydes oxidise easily ✔️
Ketones resist oxidation ❌
Formaldehyde is most reactive
Benzaldehyde ❌ Fehling test

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#AMINES Topic : 9

1️⃣ Important Name Reactions & Tests
#NameReactions

Hoffmann Bromamide Reaction

1⭐ Amide → 1° amine (one C less)
RCONH2+ BR2+KOH = RNH2

2⭐Gabriel Phthalimide Synthesis
Alkyl halide → 1° aliphatic amine only
👉 Aromatic ❌

3⭐ Carbylamine Reaction (Confirmatory for 1° amine)
(bad smell)
R-NH2+CHCl3+KOH=R-NC
Hinsberg Test
1° amine → soluble sulphonamide
2° amine → insoluble
3° amine → no reaction
Diazotisation Reaction
Aromatic 1° amine + Nano2/HCL(0°-5°)→ Diazonium salt

#Tests

⭐Nitrous Acid Test
1° aliphatic → N₂ gas
1° aromatic → diazonium salt
2° → nitrosoamine
3° → salt formation

⭐Acetylation Test
1° & 2° amines react; 3° ❌

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2️⃣ Basic Nature of Amines
📌 #ReasonofBasicity
Due to lone pair on N
Electron donating groups ↑ basicity
Electron withdrawing groups ↓ basicity
📊 Basic Strength Order (NCERT)

⭐Gas phase:
3°>2°>1°>NH3

⭐Aqueous solution:
2°>1°>3°>NH3
👉 Due to solvation + steric hindrance

⭐Aromatic 🆚 Aliphatic

⭐Aliphatic amines > NH₃ > Aromatic amines

⭐Aniline less basic due to resonance (lone pair delocalisation)

⚠️ #ImportantNCERTPoints

⭐Aniline reacts with HNO₂ at low temp
⭐Basicity increases with +I effect
⭐Ortho substituted aniline → less basic (steric + H-bonding)

#NEETTrapLines
⭐Carbylamine test → only 1° amine
⭐Gabriel synthesis → only 1° aliphatic amine
⭐Aromatic amines form diazonium salts

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#BIOMOLECULES
⭐1️⃣ CARBOHYDRATES
Definition
Polyhydroxy aldehydes or ketones or substances which give them on hydrolysis

📌 General formula: Cₙ(H₂O)ₙ
⭐ Classification of Carbohydrates

⭐ 1️⃣ Monosaccharides
✔️ Cannot be hydrolysed further
✔️ Sweet, crystalline
📌 Examples:
Glucose (Aldohexose)
Fructose (Ketohexose)
Ribose

⭐ 2️⃣ Oligosaccharides
✔️ 2–10 monosaccharide units
📌 Examples:
Sucrose (Glucose + Fructose) ❌ reducing
Maltose (Glucose + Glucose) ✔️ reducing
Lactose (Glucose + Galactose) ✔️ reducing


⭐3️⃣ Polysaccharides
✔️ High molecular weight
✔️ Non-sweet
📌 Examples:
Starch → plant storage
Glycogen → animal storage
Cellulose → structural (

Reducing 🆚 Non-Reducing Sugars
✔️ Free aldehyde / ketone group → Reducing
📌 Reducing: Glucose, Fructose, Maltose, Lactose
📌 Non-reducing: Sucrose

#ImportantNCERTConcepts
⭐ D & L Configuration
Based on position of –OH on penultimate carbon
Glucose → D-glucose

⭐ Anomers
Differ at anomeric carbon (C-1 in glucose)
α-glucose & β-glucose

⭐ Epimers
Differ at one carbon (except anomeric)
Glucose & Galactose (C-4)

⭐ Glycosidic Bond
Link between two monosaccharides
In sucrose → α-1,β-2

#RemeberGuys
Tollen’s / Fehling’s → reducing sugars
Iodine test → starch (blue-black)

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#PROTEINS
⭐ Definition
Polymers of α-amino acids joined by peptide bonds
📌 Peptide bond: –CO–NH–

⭐ Amino Acids
📌 General formula:
NH₂–CH(R)–COOH
✔️ Zwitterion in aqueous solution
✔️ 20 standard amino acids

#Classificationof AminoAcids
⭐ Based on Nutrition
Essential → Diet required
Non-essential → Synthesised in body

⭐Based on Charge
Acidic: Aspartic, Glutamic
Basic: Lysine, Arginine
Neutral: Glycine, Alanine

#ProteinStructureLevels
⭐ 1️⃣ Primary
✔️ Sequence of amino acids
✔️ Most specific

⭐ 2️⃣ Secondary
✔️ α-helix
✔️ β-pleated sheet
📌 Stabilised by H-bonds

⭐ 3️⃣ Tertiary
✔️ 3D folding
✔️ Stabilised by:
Disulfide bonds
Ionic bonds
H-bonds

⭐ 4️⃣ Quaternary
✔️ More than one polypeptide chain
📌 Example: Haemoglobin

#TypesofProteins
⭐Fibrous → Structural (Keratin, Collagen)

⭐Globular → Functional (Enzymes)

⭐Denaturation
✔️ Loss of biological activity
❌ Primary structure unchanged
📌 Causes:
Heat
pH change

📌 Example:
Boiled egg white

#NEETHOTPOINTS
✔️ Disulfide bond → Cysteine
✔️ Enzymes → globular proteins
✔️ Sucrose → non-reducing
✔️ Cellulose → β-glucose polymer

@Ayano1me @Neetugpoll @Neetugquiz