definitions grade 11 chemistry

Got it! I'll break down all the definitions you need for the topics in each unit based on your uploaded photo. I'll provide clear definitions, followed by a memory aid (phrase or trick) for each one.

Unit 1: Matter, Chemical Trends, and Chemical Bonding

1. Atomic Radius

  • Definition: The distance from the nucleus to the outermost electron of an atom.

  • Memory Aid: "Big atoms are bulky; smaller ones are stingy."

    • Trick: As you go down a group, atoms get bigger (more shells). As you go left to right, atoms get smaller (stronger pull by nucleus).

2. Ionization Energy

  • Definition: The energy required to remove one electron from a neutral atom.

  • Memory Aid: "Stealing electrons is hard when the bond is strong."

    • Trick: Low ionization = metals (give up electrons easily). High ionization = non-metals.

3. Electronegativity

  • Definition: An atom's ability to attract electrons in a chemical bond.

  • Memory Aid: "Fluorine is the electron hog."

    • Trick: Fluorine has the highest electronegativity (3.98), while metals have low values.

4. Electron Affinity

  • Definition: The energy released when an atom gains an electron.

  • Memory Aid: "Non-metals LOVE gaining electrons."

    • Trick: Non-metals have high electron affinity (e.g., \ceCl\ce{Cl}). Metals don't.

5. Periodic Trends

  • Definition: Patterns in properties like atomic radius, ionization energy, and electronegativity across the periodic table.

  • Memory Aid: "Big, greedy, or stingy? Trends tell all."

6. Ionic Bond

  • Definition: Bond formed when one atom transfers electrons to another (metal + non-metal).

  • Memory Aid: "Opposites attract—metal donates, non-metal grabs."

7. Covalent Bond

  • Definition: Bond formed when atoms share electrons (non-metals).

  • Memory Aid: "Sharing is caring in covalent bonds."

8. Polar Covalent Bond

  • Definition: A covalent bond with unequal sharing of electrons.

  • Memory Aid: "The bully hogs the electrons (polar = uneven)."

9. Non-Polar Covalent Bond

  • Definition: A covalent bond with equal sharing of electrons.

  • Memory Aid: "Equal sharing = peace and harmony."

Unit 2: Chemical Reactions

10. Law of Conservation of Mass

  • Definition: Mass is neither created nor destroyed in a chemical reaction.

  • Memory Aid: "What goes in must come out."

11. Reactants and Products

  • Definition: Reactants are starting substances; products are what you end with.

  • Memory Aid: "React to start; produce to finish."

12. Endothermic Reaction

  • Definition: Reaction that absorbs energy.

  • Memory Aid: "Endo = enter energy."

13. Exothermic Reaction

  • Definition: Reaction that releases energy.

  • Memory Aid: "Exo = exit energy."

14. Types of Reactions

  • Definition:

    • Synthesis: Two elements → one compound.

    • Decomposition: One compound → two elements.

    • Single Displacement: Element + compound → new element + new compound.

    • Double Displacement: Compound + compound → two new compounds.

    • Combustion: Hydrocarbon + oxygen → \ceCO2+H2O\ce{CO2 + H2O}.

  • Memory Aid: "Sally Did Some Cool Dancing."

Unit 3: Quantities in Chemistry

15. Mole

  • Definition: The amount of substance containing 6.022×10236.022 \times 10^{23} particles.

  • Memory Aid: "A mole is a chemist’s dozen—but HUGE!"

16. Molar Mass

  • Definition: The mass of one mole of a substance (\ceg/mol\ce{g/mol}).

  • Memory Aid: "Mass for a mole—it’s on the periodic table."

17. Avogadro’s Number

  • Definition: 6.022×10236.022 \times 10^{23}, the number of particles in one mole.

  • Memory Aid: "Avo's giant number: 6.0226.022."

Unit 4: Solutions and Solubility

18. Solubility

  • Definition: The ability of a solute to dissolve in a solvent.

  • Memory Aid: "Dissolve and disappear!"

19. Concentration

  • Definition: The amount of solute in a solution (\cemol/L\ce{mol/L}).

  • Memory Aid: "Concentrated = more stuff in less space."

20. Dilution

  • Definition: Adding solvent to decrease concentration.

  • Memory Aid: "Dilution = dilute = less strength."

Unit 5: Gases

21. Kinetic Molecular Theory

  • Definition: Explains gas behavior: particles move randomly, collide, and have negligible forces.

  • Memory Aid: "Gases are wild, free, and bouncy!"

22. Boyle’s Law

  • Definition: Pressure and volume are inversely related.

  • Memory Aid: "Boyle bounces pressure down, volume up."

23. Charles’s Law

  • Definition: Volume and temperature are directly related.

  • Memory Aid: "Charles heats up = expands."

24. Ideal Gas Law

  • Definition: Relates pressure, volume, temperature, and moles (\cePV=nRT\ce{PV = nRT}).

  • Memory Aid: "Perfect gases obey \cePV=nRT\ce{PV = nRT}."

Would you like any more details or additional tricks for specific terms? 😊