IB Chemistry S2.2.6 Molecular Polarity Flashcards

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S1.1.1 Elements, Compounds and Mixtures

S1.1.2 The Kinetic Molecular Theory

S1.1.3 Temperature and Kinetic Energy

S1.2.1 Atomic Structure

S1.2.2 Isotopes

S1.2.3 Mass Spectrometry (HL only)

S1.3.1 Emission spectra and energy levels

S1.3.2 Hydrogen emission spectrum

S1.3.3 Main energy levels

S1.3.4 Sublevels and orbitals

S1.3.5 Orbital configurations and rules

S1.3.6 Ionization energy (HL only)

S1.3.7 Successive ionization energies (HL only)

S1.4.1 The mole and Avogadro constant

S1.4.2 Relative atomic and formula masses

S1.4.3 Molar mass

S1.4.4 Empirical and molecular formulas

S1.4.5 Molar concentration

S1.4.6 Avogadro's law

S1.5.1 The ideal gas model

S1.5.2 Deviations from ideal gas behavior

S1.5.3 Molar volume of an ideal gas

S1.5.4 The ideal gas equation

S2.1.1 Formation of ions

S2.1.2 Ionic bonds and binary compounds

S2.1.3 Lattice structures and properties

S2.2.1 Formation of covalent bonds

S2.2.2 Single, double and triple bonds

S2.2.3 Coordination bonds

S2.2.4 VSEPR theory

S2.2.5 Bond polarity

S2.2.6 Molecular polarity

S2.2.7 Covalent network structures

S2.2.8 Intermolecular forces

S2.2.9 Intermolecular forces and physical properties

S2.2.10 Chromatography

S2.2.11 Resonance structures (HL only)

S2.2.12 Benzene (HL only)

S2.2.13 Expanded Octet of Electrons (HL only)

S2.2.14 Formal Charge and Lewis Formulas (HL only)

S2.2.15 Sigma and Pi Bonds (HL only)

S2.2.16 Hybridization and Bonding (HL only)

S2.3.1 Metallic bonding and properties of metals

S2.3.2 Strength of metallic bonds

S2.3.3 Transition elements and delocalized d-electrons (HL only)

S2.4.1 Bonding as a continuum

S2.4.2 Position in the bonding triangle

S2.4.3 Alloys

S2.4.4 Polymers

S2.4.5 Addition polymers

S2.4.6 Condensation polymers (Higher Level)

S3.1.1 The structure of the periodic table

S3.1.2 Electron configuration and group trends

S3.1.3 Periodicity of properties

S3.1.4 Trends in chemical reactivity

S3.1.5 Metallic and non-metallic oxides

S3.1.6 Oxidation states

S3.1.7 Discontinuities in ionization energy trends (HL only)

S3.1.8 Properties of transition elements (HL only)

S3.1.9 Oxidations states of transition elements (HL only)

S3.1.10 Color of transition metal complexes (HL only)

S3.2.1 Representation of organic compounds

S3.2.2 Functional groups

S3.2.3 Homologous series

S3.2.4 Physical trends in homologous series

S3.2.5 IUPAC nomenclature

S3.2.6 Structural isomers

S3.2.7 Stereoisomers (HL only)

S3.2.8 Mass spectrometry (HL only)

S3.2.9 Infrared spectra (HL only)

S3.2.10 Proton nuclear magnetic resonance spectroscopy (HL only)

S3.2.11 H NMR spectra interpretation (HL only)

S3.2.12 Structural analysis (HL only)

R1.1.1 Energy transfer in chemical reactions

R1.1.2 Endothermic and exothermic reactions

R1.1.3 Energy profiles

R1.1.4 Standard enthalpy change

R1.1.5 Practical considerations

R1.2.1 Bond enthalpy

R1.2.2 Hess’s Law

R1.2.3 Standard enthalpy changes of combustion and formation (HL only)

R1.2.4 Hess's Law with combustion and formation data (HL only)

R1.2.5 Born-Haber Cycle (HL only)

R1.3.1 Combustion fuels

R1.3.2 Incomplete combustion

R1.3.3 Fossil fuels

R1.3.4 Biofuels

R1.3.5 Fuel cells

R1.4.1 Entropy (S) (HL only)

R1.4.2 Gibbs free energy (ΔG) (HL only)

R1.4.3 Spontaneity and Gibbs free energy (HL only)

R1.4.4 Gibbs free energy and equilibrium (HL only)

R2.1.1 Chemical equations and stoichiometry

R2.1.2 Using the mole ratio

R2.1.3 Limiting and excess reactants

R2.1.4 Percentage yield

R2.1.5 Atom economy

R2.2.1 Rate of reaction

R2.2.2 Collision theory

R2.2.3 Factors affecting the rate of reaction

R2.2.4 Activation energy

R2.2.5 Catalysts

R2.2.6 Reaction mechanisms and rate-determining steps (HL only)

R2.2.7 Energy profiles and transition states (HL only)

R2.2.8 Molecularity (HL only)

R2.2.9 Rate equations (HL only)

R2.2.10 Order of a reaction (HL only)

R2.2.11 Rate constant (HL only)

R2.2.12 Arrhenius equation (HL only)

R2.2.13 Arrhenius factor (HL only)

R2.3.1 Dynamic equilibrium

R2.3.2 The equilibrium law and constant

R2.3.3 Magnitude of K and temperature dependence

R2.3.4 Le Châtelier’s principle

R2.3.5 Reaction quotient (Q) (HL only)

R2.3.6 Quantifying equilibrium concentrations (HL only)

R2.3.7 Gibbs free energy and equilibrium (HL only)

R3.1.1 Brønsted–Lowry acid-base theory

R3.1.2 Conjugate acid-base pairs

R3.1.3 Amphiprotic species

R3.1.4 pH and the hydrogen ion concentration

R3.1.5 The ion product of water (Kw)

R3.1.6 Strong and weak acids and bases

R3.1.7 Neutralization reactions

R3.1.8 pH curves for neutralization

R3.1.9 pOH scale (HL only)

R3.1.10 Acid and base strength and constants (HL only)

R3.1.11 Conjugate Acid-Base pair (HL only)

R3.1.12 The pH of a salt solution (HL only)

R3.1.13 pH curves of Acid-Base combinations (HL only)

R3.1.14 Acid-Base indicators and pH changes (HL only)

R3.1.15 Appropriate indicators for titration (HL only)

R3.1.16 Buffer solutions (HL only)

R3.1.17 The pH of a buffer solution (HL only)

R3.2.1 Oxidation and reduction definitions

R3.2.2 Redox half-equations

R3.2.3 Reactivity of elements based on periodic trends

R3.2.4 Acid-metal reactions

R3.2.5 Electrochemical cells: Oxidation and reduction

R3.2.6 Primary (voltaic) cells

R3.2.7 Secondary (rechargeable) cells

R3.2.8 Electrolytic cells

R3.2.9 Oxidation of organic compounds

R3.2.10 Reduction of functional groups

R3.2.11 Reduction of unsaturated compounds

R3.2.12 Standard electrode potentials (HL only)

R3.2.13 Standard cell potential (HL only)

R3.2.14 Gibbs free energy and cell potential (HL only)

R3.2.15 Electrolysis of aqueous solutions (HL only)

R3.2.16 Electroplating (HL only)

R3.3.1 Radicals

R3.3.2 Homolytic fission

R3.3.3 Substitution reactions with alkanes

R3.4.1 Nucleophiles

R3.4.2 Nucleophilic substitution reactions

R3.4.3 Heterolytic fission

R3.4.4 Electrophiles

R3.4.5 Electrophilic attack

R3.4.6 Lewis acid (HL only)

R3.4.7 Lewis acid-base reaction (HL only)

R3.4.8 Ligands and coordination bond (HL only)

R3.4.9 SN1 and SN2 mechanisms (HL only)

R3.4.10 Rate of the substitution reactions (HL only)

R3.4.11 Electrophilic addition (HL only)

R3.4.12 The relative stability of carbocations (HL only)

R3.4.13 Reactions between benzene and electrophiles (HL only)

IB Chemistry S2.2.6 Molecular Polarity Flashcards

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Each card focuses on S2.2.6 Molecular polarity and is aligned with the IB Chemistry syllabus, ensuring focused revision on atomic structure, chemical reactions, and organic chemistry.

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Why can a molecule containing polar bonds be non-polar overall?

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The molecule has a symmetrical geometry . The individual bond dipoles cancel each other out .

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S2.2.6 Molecular polarity

IB Chemistry S2.2.6 Molecular Polarity Flashcards

Structure 1. Models of the particulate nature of matter

S1.1 Introduction to the particulate nature of matter3 subtopics

S1.2 The nuclear atom3 subtopics

S1.3 Electron configurations7 subtopics

S1.4 Counting particles by mass: The mole6 subtopics

S1.5 Ideal gases4 subtopics

Structure 2. Models of bonding and structure

S2.1 The ionic model3 subtopics

S2.2 The covalent model16 subtopics

S2.3 The metallic model3 subtopics

S2.4 From models to materials6 subtopics

Structure 3. Classification of matter

S3.1 The periodic table: Classification of elements10 subtopics

S3.2 Functional groups: Classification of organic compounds12 subtopics

Reactivity 1. What drives chemical reactions?

R1.1 Measuring enthalpy change5 subtopics

R1.2 Energy cycles in reactions5 subtopics

R1.3 Energy from fuels5 subtopics

R1.4 Entropy and spontaneity (HL)4 subtopics

Reactivity 2. How much, how fast and how far?

R2.1 How much? The amount of chemical change5 subtopics

R2.2 How fast? The rate of chemical change13 subtopics

R2.3 How far? The extent of chemical change7 subtopics

Reactivity 3. What are the mechanisms of chemical change?

R3.1 Proton transfer reactions17 subtopics

R3.2 Electron transfer reactions16 subtopics

R3.3 Electron sharing reactions3 subtopics

R3.4 Electron-pair sharing reactions13 subtopics

IB Chemistry S2.2.6 Molecular Polarity Flashcards

Structure 1. Models of the particulate nature of matter

S1.1 Introduction to the particulate nature of matter3 subtopics

S1.2 The nuclear atom3 subtopics

S1.3 Electron configurations7 subtopics

S1.4 Counting particles by mass: The mole6 subtopics

S1.5 Ideal gases4 subtopics

Structure 2. Models of bonding and structure

S2.1 The ionic model3 subtopics

S2.2 The covalent model16 subtopics

S2.3 The metallic model3 subtopics

S2.4 From models to materials6 subtopics

Structure 3. Classification of matter

S3.1 The periodic table: Classification of elements10 subtopics

S3.2 Functional groups: Classification of organic compounds12 subtopics

Reactivity 1. What drives chemical reactions?

R1.1 Measuring enthalpy change5 subtopics

R1.2 Energy cycles in reactions5 subtopics

R1.3 Energy from fuels5 subtopics

R1.4 Entropy and spontaneity (HL)4 subtopics

Reactivity 2. How much, how fast and how far?

R2.1 How much? The amount of chemical change5 subtopics

R2.2 How fast? The rate of chemical change13 subtopics

R2.3 How far? The extent of chemical change7 subtopics

Reactivity 3. What are the mechanisms of chemical change?

R3.1 Proton transfer reactions17 subtopics

R3.2 Electron transfer reactions16 subtopics

R3.3 Electron sharing reactions3 subtopics

R3.4 Electron-pair sharing reactions13 subtopics

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Flashcards for S2.2.6 Molecular polarity - IB