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Grade 11 Chemistry: WE CAN DO IT! - Coggle Diagram
Grade 11 Chemistry: WE CAN DO IT!
Atomic Structure
Calculating the relative atomic mass using spectrometry
Deducing the electron configuration of atom or ion
Explaining the box diagrams, with parallel orbits, etc
Describing the absorption spectrum of hydrogen atom
Describing the emission spectrum of hydrogen atom with valence shells and arrows to indicate electron movement
Calculating the first ionization energy of hydrogen using E=hv and c=v*(wavelength) and UV emission spectrum
Describing the trend in ionization energy graphs
Bonding
Covalent bonding: electrostatic attraction between a shared pair of electrons and the positively-charged nucleus
Deduce the Lewis structure of a given compound
Note the incomplete octets (e.g. Be, B)
Note the expanded octets (Period 3 or below)
Examine the properties of bond: Bond length, bond strength, and bond polarity which is due to electronegativity (discuss the extent of polarity, in comparison to ionic compounds)
Deduce the geometry of molecules based on VSEPR theory (repulsion between e- domains and bond angle)
Determine the following:
1) molecular polarity using geometry (VSEPR) and bond polarity
2) resonance structure by proposing Lewis structures (average)
Know how resonance influences bond length and strength, affecting the overall reactivity.
3) formal charge that can be compared to electronegativity
Describe the atomic orbitals (s, p, d, f) with axis
Describe the formation of molecular orbitals due to the overlap between atomic or hybrid orbitals
so forms sigma and pi bonds
Describe the formation of hybridization of orbitals (ground, excited, then mixed state that produces degenerate orbitals)
Outline how sp3, sp2, and sp hybridization have certain shapes, which form certain bonds
Define three types of intermolecular forces, and compare them, to determine the relative properties of compounds: LDF, Dip-dip, H
Explain the mechanism of penicillin, and compare it to aspirin
+Know that aspirin forms salt by added NaOH, to be absorbed
Explain the properties and structure of penicillin and aspirin (D2)
in reference to benzene ring and *beta-lactam ring•
Compare
the structure of morphine, codeine, and diamorphine
thus explain why diamorphine is better to cross blood-brain barrier than morphine
Outline the trends in melting points for oxides
or Period 3
Know different types of
macromolecules
and how their reactivity differ due to different structures: graphite, C60, diamond, SiO2, etc
Metallic bonding: electrostatic attraction between metal cations and a sea of delocalized electrons
Explain the properties of metals with the strength of metallic bond: ionic radii, charge on cation, # of electrons, ...
Explain the physical and chemical properties of alloys
Ionic bonding: electrostatic attraction between oppositely-charged ions
Explain the properties of ionic compounds with the strength of ionic bonds: ionic radii, charge on cation, shape ...
Know that the ionic compounds only conduct electricity when it is dissolved or molten, because only then, charged particles become free to move carrying charge.
Name ionic compounds or deduce its formula from name
Energetics
Hess's law
Born-Haber cycle
Bond enthalpy
Transfer of energy in form of heat:
q=mc*(change in T)
Types of enthalpies
Electron affinity:
First ionization energy: energy required to remove one mole of electrons from one mole of substance in gaseous state
*Have different orders (not exact word)
Enthalpy of atomization
Enthalpy of hydration
Enthalpy of solution
Lattice enthalpy
Entropy
Gibbs free energy: ΔG=ΔH-TΔS
If the ΔG is negative, then the reaction is spontaneous.
If the change in enthalpy and the change in entropy are both positive or both negative, then the spontaneity depends on temperature.
Entropy is the measurement of disordered-ness
(Is always positive).
Change in entropy is always negative as it gets more disordered
but spontaneity must consider other elements too
Acids & Bases
Different theories: Arrhenius, Bronsted-Lowry, Lewis
Distinguish definitions
Identify conjugate pairs
Know amphoteric and/or amphiprotic species
3.2 Periodity: Trend in acidity/alkalinity and pH for Period 3 oxides
Acid deposition of sulfur and nitrogen oxides
effects of acid rain on materials
chemically-justified strategies against acid rain
Mechanism of antacids that neutralize HCl
Use of pH scale for pH = -log[H+ (aq)]
Equilibrium
Description of equilibrium state in physical and chemical systems
Use of equilibrium law: Deduce equilibrium expression that gives the equilibrium constant (Kc), given the chemical expression
at a constant temperature
Compare reaction quotient (Q) to Kc
Le Chatelier's principle: concentration, pressure, temperature, catalyst
-->
can do calculation given initial concentrations and Kc
Kw: ionic product constant of water
Kw = [H+][OH-] for in every solution, H2O ⇋ H+ + OH-
and pH + pOH = pKw at every temperature
For any conjugate pair, Ka*Kb=[H+][OH-]=Kw
Henderson-Haseslbalch equation: pH = pKa + log10([A⁻]/[HA]) to determine the pH of a weak acid solution
Deduction of acid and base dissociation constants
Weak acids and bases have reversible dissociation ('weak')
Deduce the chemical equation for acid dissociation and base ionization.
Compare strengths by e- conductivity, rate, and pH
pH curve and buffer
Mechanism of buffer (something and its conjugate salt)
Use of pKa and pKb, neutralization, etc to make a buffer solution
Consideration how salt hydrolysis may influence the equivalence point
Factors that influence buffer: dilution (buffering capacity), temperature (Ka or Kb, so pH)
How is buffer region seen in the pH curve of neutralization btw acid and base?
Kinetics
Radioactivity (follows first order kinetics)
Nuclear application
Nuclear imagingL uses radionuclide as a tracer in the radiopharmaceuticals that target dif't parts of the body
Technitium-99m
PET (positron emission tomography) with F-18
Nuclear therapy
External radiotherapy e.g. using Co-60 in teletherapy
Internal radiotherapy: e.g. Lu-177, Yt-90
Targeted alpha therapy(TAT) (Pb-212)
Boron neutron capture therapy (BNCT): B-10 to 11 to decay
Side effects or radiotherapy: fatigue, nausea, etc
Wastes: LLW and HLW - cooled then stored
Deduction of equations for alpha, beta, gamma radiation
Comparison of their
ionizing density and effect
Calculate half-life of medicine using different equations.
NOTE
: rate of decay = λ[A] where λ is the decay constant (or rate constant) -- only difference from rate expression is that this is not a chemical reaction and it does
not depend on temperature
Rates
Kinetic theory of gases --> Maxwell-Boltzmann distribution curve*
collisions must happen with KE greater than Ea, and in correct orientation
Initial rates of each reaction by using gradient calculation (conc over time)
Measuring rates in different methods
Deduce the rate law (rate expression): rate = k [A]^2[B] for example
Does not rely on the chemical equation
Must determine the order in respect to each reactant
Can consider the rate mechanism for this
Deduce the order by drawing graphs
Does it has a constant half-life?
Propose reaction mechanism (usually unimolecular or bimolecular steps) and also determine the RDS
SHOULD be able to draw energy profiles
Outline the nucleophilic substitution of halogenoalkanes, both SN2 and SN1 mechanisms considering the order of alkanes.
can consider the solvent choice
can consider the inversion
can consider the leaving order
Enantiomers can be used to determine the optical activity and determine if the reaction goes SN2 and SN1 (in what ratio)
racemic mixture for SN1 (with some inversions) - 50%/50% L/R
Identify chiral centers and molecules that have no plane of symmetry
Free radical substitution of alkanes (halogenation) in stages of initiation, propagation, and termination
Relationships of rate with temperature, concentration, particle size, pressure (for gas), catalyst
Calculate the activation energy using different forms of Arrhenius equation (16.2) -- Ea in the unit of J mol-1
Extra: Ideal Gas Theory
PV = nRT
be minded of the units (K, Pa, m3)
Ideal gas volume (molar volume)
by Avogadro's law
Gas laws: Relationships between volume, pressure, and temperature
Know the deviation from ideal behaviors, for the real gases
(More ideal at lower pressure at high temperature)
Interpreting NMR, IR graphs, with HDI
Infrared graph -- show the radiation that is absorbed as peak?
NMR
Hydrogen deficiency index