Grade 11 Science Worksheets

Learning Objectives

• Use VSEPR electron-pair repulsion to predict molecular geometry from bonding and nonbonding pairs.
• Relate molecular shape to bond angles and predict relative polarity based on symmetry.
• Identify the electron-pair geometry vs. the molecular geometry for common VSEPR families.

Learning Objectives

• Use VSEPR to predict molecular shape and relate shape to polarity and dipole alignment
• Compare intermolecular forces (London dispersion, dipole-dipole, and hydrogen bonding) using molecular examples
• Explain how intermolecular forces affect melting and boiling points, including real-world regional phenomena

Learning Objectives

• Explain how intermolecular forces influence boiling point, vapor pressure, and phase changes.
• Interpret how molecular size, polarity, and temperature affect volatility and phase diagrams.
• Connect phase behaviour concepts to real-world examples such as petroleum fractions and atmospheric transport of organic compounds in Alberta.

Learning Objectives

• Explain how atomic radius, ionization energy, and electronegativity change across periods and down groups.
• Use periodic trends to predict whether atoms form cations or anions and how they bond.
• Connect periodic trends to real materials issues such as corrosion resistance and alloy selection.

Learning Objectives

• Draw Lewis structures showing valence electrons, bonding pairs, and lone pairs for common molecules.
• Use formal charge to select the most likely Lewis structure and minimize overall charge.
• Identify when resonance structures are needed to represent electron delocalization.+ Show more

Learning Objectives

• Explain how hydrogen bonding forms between a hydrogen atom and a lone pair on an acceptor atom
• Describe how hydrogen bonding affects physical properties such as melting and boiling points
• Connect hydrogen bonding to the behavior of water, ice, proteins, and polymers

Learning Objectives

• Explain what electronegativity measures and how it relates to electron attraction in a bond.
• Use electronegativity differences to predict bond polarity and identify polar vs. nonpolar covalent bonds.
• Describe periodic trends in electronegativity across periods and down groups.

Learning Objectives

• Explain how valence electron distribution relates to molecular polarity and dipole moments
• Use electronegativity and electron-density ideas to predict whether molecules are polar or nonpolar
• Connect molecular polarity to observable intermolecular interactions, such as hydrogen bonding and dispersion forces

Learning Objectives

• Explain how London dispersion forces arise from instantaneous electron fluctuations in nonpolar substances
• Describe how dispersion strength depends on molar mass and molecular surface contact
• Connect dispersion forces to macroscopic properties such as melting point, viscosity, and phase behavior

Learning Objectives

• Explain how dipole–dipole attractions form between polar molecules and how orientation affects intermolecular forces
• Predict how temperature changes dipole interactions and related physical properties in solutions and condensed phases
• Use dipole interactions to justify examples such as miscibility and boiling-point differences in Alberta-relevant contexts

Learning Objectives

• Compare ionic, covalent, and metallic bonding by describing electron transfer, electron sharing, and delocalized electron models.
• Link each bonding type to a characteristic structural motif (ionic lattice, covalent molecular pairs/framework, metallic electron sea).
• Use bonding models to predict and explain differences in electrical conduction, hardness, and solubility for real materials.

Learning Objectives

• Use stoichiometry with balanced dissociation/neutralization relationships to calculate unknown titrant or analyte concentrations.
• Compute equivalence volume and relate it to reaction mole ratios for strong acid–base and weak acid–base titrations.
• Interpret titration data, including endpoint and pH considerations, to explain how weak systems affect calculations.

Learning Objectives

• Compare ionic, covalent, and metallic bonding using particle-level ideas
• Predict physical properties such as melting point, conductivity, hardness, and solubility from bonding type
• Use real-world examples (e.g., salt for winter, steel in infrastructure, diamond/graphite materials) to justify property trends

Learning Objectives

• Explain how electronegativity differences create polar covalent bonds with partial charges.
• Distinguish polar bonds from polar molecules by using bond dipoles and molecular dipole vectors.
• Predict how molecular polarity affects interactions such as solubility and intermolecular forces.+ Show more

Learning Objectives

• Explain how protons, neutrons, and electrons determine atomic identity and charge
• Describe how electron arrangements (shells, subshells, and valence electrons) influence bonding and ion formation
• Connect atomic structure to common real-world examples such as sodium in road salt and carbon in hydrocarbons

Learning Objectives

• Explain how molecular orbital theory and band theory together describe delocalization and bonding in solids and transition-metal complexes.
• Relate orbital overlap and band structure to metallic conduction and semiconductor behavior.
• Use molecular symmetry and orbital/band models to predict spectroscopic features and reactivity trends.

Learning Objectives

• Describe how pH changes as titrant is added during a titration and identify key features of titration curves (initial pH, buffer region, inflection point, equivalence point).
• Compare the shapes of titration curves for strong acid–strong base, weak acid–strong base, and weak base–strong acid systems.
• Use curve features to select appropriate endpoints and interpret titration data in real samples (e.g., natural waters and industrial effluents).

Learning Objectives

• Distinguish strong acids/bases from weak acids/bases based on how completely they ionize in water
• Relate the strength of an acid or base to the concentration of free H+ or OH− ions in solution
• Use equilibrium ideas to explain why weak species only partially dissociate

Learning Objectives

• Explain how polyprotic acids dissociate in steps and how each dissociation constant affects pH.
• Interpret titration curves by identifying equivalence points and buffer regions for systems like carbonate and phosphate.
• Calculate cumulative acidity and use stepwise dissociation information to predict pH trends across concentration ranges.

Learning Objectives

• Explain what pH means and how it relates to hydrogen ion concentration and acidity/basicity.
• Use the pH–pOH relationship (at 25°C, pH + pOH = 14) to solve or check chemistry problems.
• Connect pH to real-world effects such as mineral solubility, chemical speciation, and aquatic organism suitability.

Learning Objectives

• Explain how neutralization produces salt and water and relate this to molar stoichiometry.
• Use balanced chemical equations to calculate moles and solve titration/equivalence problems.
• Identify the limiting reagent and determine how it affects the amount of product formed.

Learning Objectives

• Match an indicator’s color-change pH range to the expected equivalence pH for an acid–base titration.
• Select an appropriate indicator for different titration types using expected steepness and pH region of the equivalence point.
• Explain why indicator transition intervals must align with the titration’s buffering and endpoint region.

Learning Objectives

• Explain what the Henderson–Hasselbalch equation describes in terms of pH, pKa, and concentration ratios.
• Use the Henderson–Hasselbalch equation to predict how changing acid/base concentrations affects buffer pH.
• Interpret buffer behavior in real environmental or industrial water systems.

Learning Objectives

• Explain how acid and base dissociation constants (Ka and Kb) describe proton-transfer equilibria
• Use Ka, Kb, and Kw relationships to reason about pKa and pKb and predict relative acid/base strength
• Apply equilibrium and buffering ideas to estimate or interpret pH changes in real aqueous systems

Learning Objectives

• Analyze how acid–base reactions and buffering influence environmental pH in Alberta contexts.
• Use stoichiometry and titration ideas to estimate neutralization requirements for contaminated water.
• Explain how dissociation and equilibrium affect remediation decisions and compliance targets.

Learning Objectives

• Explain what degree of dissociation (α) means for weak acids and weak bases in solution.
• Predict how initial concentration and equilibrium effects change percent dissociation.
• Describe how the common-ion effect influences ionization of dissociated species.+ Show more

Learning Objectives

• Determine hydrogen ion concentration from pH and hydroxide ion concentration from pOH using logarithmic relationships
• Use Kw to interrelate [H+], [OH-], and pH/pOH in water samples
• Apply correct significant figures, units, and conversions when reporting aqueous concentration results

Learning Objectives

• Explain how a conjugate acid-base pair resists changes in pH when small amounts of acid or base are added.
• Relate buffer effectiveness to the proximity between pKa and target pH and to the relative amounts of acid and base forms.
• Apply buffer concepts to real-world systems such as agricultural soils and water treatment.

Learning Objectives

• Explain what buffer capacity means and how it relates to pH change after adding acid or base
• Identify factors that increase or decrease buffer capacity using buffer concentration and component ratio
• Use carbonate and organic system examples to reason about environmental buffering in real settings+ Show more

Learning Objectives

• Explain how molecular structure factors influence acid strength in water.
• Use trends such as bond polarity, electronegativity, atom size, resonance stabilization, and oxidation state to predict acidity.
• Relate electron-withdrawing groups in oxyacids and halogen-substituted acids to acidity trends.+ Show more

Learning Objectives

• Describe the vertical structure of the atmosphere and relate temperature changes to layers such as the troposphere and inversion conditions.
• Explain how pressure gradients and temperature differences drive horizontal and vertical atmospheric circulation.
• Interpret representations like sounding profiles and pressure maps to connect thermodynamics with observable weather and climate patterns.

Learning Objectives

• Explain how carbon moves among the atmosphere, ocean, terrestrial biosphere, and sediments using reservoirs and fluxes.
• Use mass-balance reasoning to describe how natural processes and human activities change atmospheric CO2.
• Interpret isotopic tracer ideas to distinguish natural carbon cycling from anthropogenic contributions.+ Show more

Learning Objectives

• Explain how momentum, buoyancy, and the Coriolis effect shape atmospheric and oceanic circulation patterns.
• Interpret streamfunction plots and velocity-field descriptions to infer where air or water rises and sinks.
• Connect major circulation systems (jet streams, trade winds, thermohaline circulation) to heat redistribution and climate teleconnections such as ENSO.

Learning Objectives

• Explain how coupled Earth system models link atmosphere, ocean, cryosphere, and biosphere processes to simulate climate behavior.
• Describe common model boundary conditions, forcings, and diagnostics such as ensemble means and uncertainty ranges.
• Evaluate model skill and limitations using examples like volcanic forcing and land-use change.

Learning Objectives

• Explain how global energy balance links incoming solar energy, outgoing radiation, and climate change
• Interpret radiative forcing and feedbacks using simple energy budget ideas and diagrams
• Describe how albedo and polar amplification affect seasonal and long-term temperature patterns+ Show more

Learning Objectives

• Explain how land-use change, resource extraction, and emissions alter Earth systems (land, water, air).
• Use the idea of measurement and data (spatial patterns and time series) to connect local actions to regional impacts.
• Describe heat and trace gases as components of the human footprint and discuss trade-offs with resilience.

Learning Objectives

• Explain how geologic maps, geophysical surveys, and basin models reveal where mineral, water, and energy resources form and accumulate.
• Distinguish renewable versus nonrenewable resource reservoirs and describe how extraction changes fluxes into and out of those reservoirs.
• Connect resource occurrence to tectonic settings and sedimentary processes, and evaluate sustainability using reserve quality and extraction-rate ideas.

Learning Objectives

• Describe how rocks form, transform, and break down across geologic time within the rock cycle.
• Explain how plate tectonics control metamorphism, magma generation, and sedimentation.
• Use stratigraphic and tectonic ideas to trace material pathways and discuss residence time concepts.+ Show more

Learning Objectives

• Explain major causes of sea-level variability, including thermal expansion, ice-sheet mass loss, and local subsidence.
• Describe how satellite altimetry and tide-gauge records complement each other for understanding sea-level change.
• Interpret stratigraphic and coastal geomorphology evidence to infer past sea-level rates over time scales.+ Show more

Learning Objectives

• Identify Earth’s major subsystems (atmosphere, hydrosphere, lithosphere, biosphere) and describe how they act as reservoirs.
• Explain how mass and energy move among subsystems using fluxes and conceptual box-and-arrow models.
• Use evidence and key terminology to describe interactions such as ocean–atmosphere coupling and watershed transfers.

Learning Objectives

• Explain the roles of protons, neutrons, and electrons in determining atomic identity and behavior
• Use emission spectra and mass spectrometry evidence to support discrete energy levels and isotopic composition
• Calculate average atomic mass from isotopic abundances and interpret basic ion formation patterns

Learning Objectives

• Distinguish ionic, covalent, and metallic bonding using electronegativity difference and formal charge ideas.
• Use potential-energy diagrams and electron-sharing/electron-transfer concepts to justify bond strength trends.
• Relate lattice considerations to lattice energy, melting point, and conductivity predictions.

Learning Objectives

• Use Lewis structures and VSEPR models to predict bond angles and molecular shapes.
• Explain how hybridization and orbital overlap relate to bonding geometry and bond order.
• Use resonance and molecular orbital ideas to account for polarity and spectroscopic/reactivity trends.

Learning Objectives

• Apply the Aufbau, Pauli exclusion, and Hund’s rules to write correct electron configurations for atoms and ions.
• Connect valence electron patterns to common oxidation states and periodic trends.
• Explain how orbital shapes and nodal structure relate to electron probability and energy concepts.

Learning Objectives

• Use reaction quotient Q and compare it to the equilibrium constant K to predict the direction of shift in both homogeneous and heterogeneous systems.
• Calculate equilibrium concentrations or partial pressures using Kc and Kp expressions, including the role of stoichiometric coefficients.
• Explain Le Châtelier’s principle for concentration, pressure, and temperature perturbations and connect it to thermodynamic tendencies.

Learning Objectives

• Characterize dispersion, dipole–dipole, and hydrogen-bonding interactions and relate them to phase behavior.
• Explain how molecular polarity and intermolecular attractions influence boiling point, vapor pressure, and solubility.
• Use potential-energy ideas and property trends to connect microscopic forces to macroscopic observations like cohesive versus adhesive behavior.

Learning Objectives

• Determine reaction order from initial-rate data and connect it to rate laws
• Use integrated rate expressions to interpret concentration–time and initial-rate representations
• Explain how collision theory and transition-state ideas relate to temperature dependence and activation energy

Learning Objectives

• Explain how effective nuclear charge helps predict trends in atomic radius, ionization energy, electron affinity, and electronegativity.
• Use periodic trends to predict the likely ionic charges and simple compound formation for main-group elements.
• Compare relative reactivity across periods and groups using electron structure and periodic patterns.