2.1: 1. MAT- States of Matter, Interactions, Bonding, and Energy
- Page ID
- 436096
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Summary:
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To gain a fundamental understanding of the composition of atoms with an emphasis on the atom’s nucleus.
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To develop chemical literacy regarding isotopes, nuclear stability, radioactive decay, fission, fusion, and applications involving nuclear transformation.
- To develop chemical literacy regarding phases of matter including gases, liquids, and solids with an emphasis on:
- the gas phase and the origins and relative strengths of different contributions to intermolecular forces in the condensed phases,
- phase changes and phase diagrams,
- the properties of liquids and especially how they reflect intermolecular forces,
- the properties of solids, especially crystal structures and metallic conduction.
- To gain a fundamental understanding of the gaseous state of matter and the ideal and non-ideal behavior of gases.
Review of Key Concepts in Periodic Trends, Bonding, and Concentrations
- Determine whether the force of interaction is positive or negative for a pair of charged particles.
- Use Coulomb’s Law to arrange a series of charged particle systems from the most attractive system to the most repulsive system.
- Describe the difference between the actual nuclear charge, Z, and the effective nuclear charge, Zeff, experienced by a particular electron in an atom. Explain the reason for the periodic trend observed in the Zeff for the outermost electron in the elements. Calculate Zeff for the outermost electrons in the elements.
- Rank atoms and/or ions in order of increasing electronegativity, ionization energy, and/or atomic radius.
- Describe an ionic bond, which particular attention to the location of the electrons. Describe a covalent bond. Judge whether a covalent bond is polar or nonpolar.
- Determine if the bonding in a molecule would be best categorized as ionic, polar covalent, or nonpolar covalent. (This requires a synthesis of analyzing the position of the elements on the periodic table and applying knowledge of electronegativity trends, definitions of bond types, and recognition of polyatomic ions).
- Write chemical formulae from the names of ionic and molecular compounds and vice versa using chemical nomenclature conventions.
- Predict how to combine ions to make neutral ionic compounds by analyzing the charges and determining the number of each type of species needed.
Atomic Structure and Nuclear Reactions
- Describe atomic structures using the sub-atomic particles most relevant to chemists (protons, neutrons, and electrons), including charges, normal relative locations, and approximate masses of all species.
- Define the word isotope and provide examples of important radioactive isotopes in environmental chemistry, carbon-14 dating, and other applications.
- Calculate relative abundances of isotopes, exact isotopic masses, and/or average atomic mass from provided data.
- Write balanced chemical reaction equations for nuclear reactions.
- Define and provide symbols for some species that can be emitted in nuclear reactions: positron, neutron, alpha particle, beta particle, gamma ray.
- Define and be able to calculate binding energy and mass decrement or mass defect.
- Define fission and fusion and describe similarities and differences between these processes.
- Perform quantitative calculations for the half-life involved in radioactive decay.
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Gases
- Explain Boyle’s Law, Charles’ Law and Avogadro’s Law as empirical descriptions of the behavior of gases under certain conditions.
- Understand what is meant by an ideal gas, the assumptions made in describing an ideal gas, and the ideal gas equation as a combination of Boyle’s Law, Charles’ Law and Avogadro’s Law.
- Adeptly convert between units of pressure if given the conversion factors.
- Relate pressure, volume, and/or temperature for a gas sample in a closed container using the ideal gas law.
- Define standard temperature and pressure (STP).
- Apply Dalton’s Law of partial pressures to problems that involve mixtures of gases. (moved to SOL)
- Define mole fraction. Apply mole fraction in calculations. (moved to SOL)
- Synthesize previous knowledge of density, reaction stoichiometry, and gram-mole conversions with new knowledge about ideal gas behavior and partial pressures to construct solutions to quantitative problems that combine these concepts.
- Explain the key differences between real gases and the ideal gas.
- Explain the difference between effusion and diffusion, and apply knowledge to quantitative problems.
- Describe the differences between gases, liquids, and solids, both in terms of their macroscopic properties and molecular scale structure and dynamics.
- Describe the different kinds of intermolecular forces in terms of their origins and relative strengths.
- Describe the effect of intermolecular forces on a substance’s properties like the boiling point or heat of vaporization. Rank substances by these properties.
- Recall and define 3 types of intermolecular forces. Apply this knowledge to various substances, and then combine this knowledge with that of phase changes to arrange those substances by increasing boiling point.
- For a given molecule or set of molecules, identify which intermolecular forces are most important.
- Apply the Clausius-Clapeyron equation to problems involving the vapor pressures of liquids. (moved to SOL)
Liquids, Solids, and Transitions
- Describe the differences between gases, liquids, and solids, both in terms of their macroscopic properties and molecular scale structure and dynamics.
- Describe the different kinds of intermolecular forces in terms of their origins and relative strengths.
- Describe the effect of intermolecular forces on physical properties like the boiling point or heat of vaporization. Rank substances by these properties.
- For a given molecule or set of molecules, identify which intermolecular forces are most important.
- Interpret heating curves and how they relate to phase diagrams. (moved to SOL)
- Use heat capacities and the enthalpies of vaporization and fusion to calculate the heat necessary to raise the temperature of a substance a given amount. (moved to SOL)
- Read and interpret a phase diagram, and identify special points on the diagram like the triple and critical points. (moved to SOL)
- Use a phase diagram to identify the sequence of phases that would be observed when changing temperature and/or pressure. (moved to SOL)
- Apply the Clausius-Clapeyron equation to problems involving the vapor pressures of liquids and solids. (moved to SOL)
- Explain how phase equilibria and phase transformations reflect the rate of transfer of molecules between different phases. (moved to SOL)
- Explain how intermolecular forces affect the microscopic and macroscopic properties of liquids, including boiling point, \(\Delta H_{vap}^\circ\), surface tension, capillary action, and viscosity.
- Distinguish between the different classes of solids (atomic, molecular, ionic, metallic, and network), and describe the kinds of attractive forces and properties that are characteristic of each.
- Identify and describe the essential features of cubic unit cells (scc, bcc, and fcc) and closest packing structures (hcp and ccp).
- Relate densities and atomic radii using geometrical parameters for cubic unit cells.
- Identify the stoichiometry of crystalline compounds given information on the kinds of sites occupied by the atoms or ions in the unit cell.
- Rank the relative melting points of ionic solids using knowledge about atomic radius trends and the force of attraction between charge particles.
Matter and Energy
- Predict energy changes that result from the interaction of charged particles at different distances.
- Explain the essence of each of the following thermodynamic terms: enthalpy, entropy, and free energy.
- Calculate the amount of energy given off in a nuclear reaction.
- Understand and explain the difference between a law and a theory.
- Understand the Kinetic Molecular Theory (KMT) as a scientific theory and how it “explains” the behavior of ideal gases.
- Explain the meaning of root mean square speed for a collection of gas molecules.
- Understand what is meant by the temperature of a gas and its relationship to the average kinetic energy of a collection of gas molecules.
- Construct a Born Haber cycle to calculate lattice energies of ionic compounds. (moved to SOL)