Class 9 Science: Chemistry, Physics, Biology

Introduction

• Exams are near, Prashant bhaiya is here to help.

Session Overview

• Complete class 9th science in 3-4 hours covering chemistry, physics, and biology.
• Intended for students who haven't started studying and those needing revision.
• It's the last selfie for Class 9th students before they transition to Class 10th.

Matter in Our Surroundings

• Matter: Anything with mass that occupies space.
• Focus on physical properties in this chapter; chemical properties will be covered later.
• Matter consists of tiny particles (atoms) too small to see even with a microscope.
• Experiment: Potassium Permanganate in Water: Crystals of potassium permanganate are dissolved in water, turning it pink; the water remains slightly pink even after multiple dilutions.
• Conclusion: Matter comprises extremely small particles.
• Particles Have Space Between Them: Demonstrated by adding sugar to water, where it dissolves and seems to disappear as it fills spaces between water molecules.
• Diffusion: Mixing of substances, illustrated by potassium permanganate in water.
• Temperature Dependence: Diffusion increases with temperature.
• Diffusion is highest in gases, then liquids, then solids.
• Constant Motion: Particles are in constant motion, most in gases, less in liquids, least in solids.
• Particles Attract Each Other: Attraction is strong in solids, less in liquids, and very weak in gases.

States of Matter: Solid, Liquid, Gas

• Solid: Atoms are close with no space, very strong attraction, fixed shape and volume, cannot be compressed, and have low kinetic energy.
• Liquid: Atoms have space between them with some attraction, fixed volume but no fixed shape, little compression, and more kinetic energy.
• Gas: Atoms have the most space between them with very weak attraction, no fixed shape or volume, highly compressible, and high kinetic energy.

Gases

• Properties: Large spaces, weak attraction, high kinetic energy, no fixed shape/volume, easily compressed.

Conversion of Temperature: Celsius and Kelvin

• Celsius to Kelvin: Add 273.
• Kelvin to Celsius: Subtract 273.
• SI Unit of Temperature: Kelvin.

Change of State

• Solid to Liquid: Heat increases the melting point, causing fusion.
• Liquid to Gas: Heat increases the boiling point, causing vaporization.
• Gas to Liquid: Cooling the temperature causes condensation.
• Liquid to Solid: Cooling the temperature causes solidification.
• Solid to Gas: Sublimation.
• Gas to Solid: Deposition.
• Pressure Impact: Increasing pressure causes gas to turn into a liquid, and then a solid.

Melting and Boiling

• Melting Point: The minimum temperature at which a solid converts to a liquid.
• Latent Heat of Fusion: Heat needed to convert 1 kg of solid into liquid at the same temperature.
• Boiling Point: Temperature at which liquid converts to gas.
• Latent Heat of Vaporization: Heat required to convert 1 kg of liquid into gas at the same temperature

Evaporation

• A surface phenomenon where a liquid turns into vapor below its boiling point.

Evaporation Facts

• Reason for Process: Evaporation causes cooling.
• Factors: Temperature, wind speed, surface area, and humidity.
• Summer in Cotton: Cotton absorbs sweat and cools the body.
• Water drop on Glass: Indicates a cool temperature in the environment.
• Evaporation vs Boiling:
  • Evaporation happens at any temperature, while boiling occurs at a fixed temperature.
  • Evaporation is a surface phenomenon; boiling involves the entire liquid and causes cooling, while boiling does not.

Is Matter Around Us Pure

• Types: Matter is divided into pure and impure substances.
• Elements of Matter: Elements and Compounds are sub-categorized into Metals, Non-Metals, and Metalloids. Impure substances are Mixtures, classified as Homogeneous and Heterogeneous.
• Pure Substance: Made up of only one type of matter or atom.
• Properties of Pure Atoms: C: Consistent Physical Properties, I: Inseparable, D: Defined Composition.
  • Elements: Basic form of matter.
  • Compounds: Combination of different elements of matter.

Elements

• Metals: Lusterous (shiny), silver/gray, conduct electricity.
• Non-Metals: Non-lustrous, colorful, and do not conduct electricity.
• Metalloids: Intermediate physical properties, can be both metallic and non-metallic.

Compound

• The ratio of hydrogen to oxygen in water is 1:8.
• Mixture: Combination of different matters.
• Homogeneous mixtures are mixed properly, while heterogeneous are not.

Factors

• Factors affect each part of a mixture by physical and chemical means.
• Difference between Compound.
• Mixtures can be Homogeneous or Heterogeneous, while Compounds are Homogeneous.

Solutions

• Solution of True Mixture, and its small particle size.
• No Seperation.
• Scatter the light.

Colloidal Solution

• Big Particical but can't be seperated in filtration.
• They scatter light.
• Ex: Milk, the solutions are semi-see-through. Surface Area increases to increases Evaporations. Humidity affects the speed of what can be absorbed.
• Solutions = Solute (Small Mixture) + Solvent (Big Mixture).

Concentration of Solution Calculation

• Formula: Mass of Solute / Mass of Solution x 100.
• Solubility: Maximum amount of solute that can dissolve in a solvent.
• Temperature increase by increases.
• Saturated Solution/ Solution increases to reach the the highest point of saturation.

Types of Solution: Dispersed Medium, and Dispersed Phase

• Dispersed Medium: The liquid base or solvent.
• Dispersed Phase: The material being solute.

Suspension

• Big Particles.
• Opaque so that lights cant see throw.
• Can be sperated in filtratation.
• They cant also scatter light.
• Examples: Emulsion liquid and liquid mixed togeather.

Physical and Chemical Change

• Physical Changes: Changes in physical property.
• Chemical Changes: Changes in physical/chemical properties resulting in a change in the element.

Atoms Molecules

Atom

• Maharishi Kanad discovered that atoms are the smallest indivisible particles.
• Elements always have the same properties.

Dalton

• Dalton's Atomic Theory: All matter is made of tiny, indivisible particles called atoms.
• Atomic number can not be dived.
• Given same identical Atoms as chemcial.

Modern Day Symbols

• Symbols represent elements (e.g., H for Hydrogen, O for Oxygen).
• Some symbols are derived from different names (e.g., K for Potassium, from Kalium).
• Use tricks to memorize the elements.

Atomic Number Calculation

• Tricks on Even Mulitply by 2, when odd Muttiply yby 2 and add 1.
• EX Carbon is 6.. so 6x2 is 12 the Atomic.

Exceptions

• H one Hydrogen.
• 35. 5 Chlorine.
• 40 Argan.
• 14 Nightrogen.

Amu

• Mass of An Atom Carbon.. mass of the atoms of of the Carbon.

Atom Types

• Ion and Molecules.
• Atoms want to stay alone so they stay as a inert Atom.
• If they combined to one atom they can be two types as ion molecule types.
• Ions are group of atoms and Negative charages.
• Caion Positvely Charage. Anion Negative Charge.

Table

• Memorize table when need too. plus 1 plus and so.
• Module is A atom.
• Eleents stay in two types Element and Compound.
• Element stays in two types same 2o0.
• Atmotcy number in number of element in a same group.
• How Calculate is you count the amount in formula.

Formula Unit Mass

• For ionic compoud used and what ever the calculation results is the ammount needed.
• Combine capabitiy capacity is known as valency.

Chemical Formula

• Easy process on how to make chemical formulas.
• Then do Cross Moltiplication.

Structure Atom

• JJ Tomoson did Cad Ray expeirment.
• He found cadhode ray. Experiment.
• There was a Cadthode Ray and An node rate. Eletron moves from negative to positve.

Cadode

• Hich volage.
• Low Preasses. Goldestine - Proton Found.

Chadwick

• 1932- Neutral.
• Atmoic mass in protone number.
• Mass elctron.

JJ Tomsom Modle

Plum Poding.

• Red water, Black seeds. elelcrton embedding.
• negative chargeds is what that equal.

Rother Food

• He is a liar.
• Gold flah expeirment. All are alpha partricals to the foil.

He used Gold Fal because its more maliuable. to move the atmoic ray on the metal.

• He tested out Atoms.
• Most light atms to all. Alpha.
• He had to come up with solution which is to the core there is atom. which has core to it.
• the Atom is positve and its center there is mass in the mucleus.
• Electron revovle. and mucleis is small.

Draw Backs

• Bor then explain, the rutherford modual is fales and cant to expain how it woks in a proper moddel.
• Bor explain electorn around nyclaus it does not releases a stainblle.

electron abosorves atmoic at each space level

• K-Shell.
• L-Shell.
• M shell then and last is N-Schell.
• Formula is 2n2 so u calculate from that. if its going to be postives charges and is then goes from higehr position , when negative is on lower position.

Atomic Numbers

• Elements is numbers.
• Proton nuetron that same to the electric current , Electrically neutral.

Electrons Ditributed

• you cant have more then 8 on most schll. if you have the. that same to electric current.
• Valnce electron, vaalnve 1.
• Isotopes: top Change. mass change.
• Isopro Mass change. Example of Hydron gen Protum, and deteriating.

Usea of Uranium

• Uranium and pultuium is reactor planer.
• Coblad has Cancer Treament.
• and Lodine for throid.

Structure of life

• Cell all Organims.
• History Robert Hoke is call, Cell. Liviving is LUN howck and.
  • Sleiden and shown all of cell theroy.
  • cells must be in cell division.
  • Unicellalruer same, multicelula or same.
  • largest cell is austruuch.
  • smalelst myscoplanma.
  • Longe st is neuro. Plasma Membran - Proctetion outside of cell. selectively perimble. to make things.
  • Lipds proteins.

Ectosomis high low to low.

Hpper tonice : when cells swwells.

Cell wall

• Protects the tree.
• Nuclus. DNA. and Protients. chromo. prokartic and ukartuic. Prokaratic:. does has enulcus

Qkayotic has enuluicas and well dine

• Citoplam : Cell with liquid.
• Organs: tiny organs in the cells.

endosplasm reticulum. iFatory the place where all action are

• Rough protiens. libd are smooth .
• Packaging and transport. = Galogy apapturus. = lysosome
• suisisde bags or redyce materal. cels.vaqious
• Storage = vaqious mitcoiendra.
• Have dna powers huse. placttids
• animals cant have pladtifids. crloplats colurles ryosymz protiene

A comprehensive session to cover the entire Class 9th science syllabus which includes chemistry, physics and biology. Suitable for revision of important concepts. Focus on matter, its properties and composition.