What you should know and be able to do (learning outcomes)
Be able to give a definition of the science of chemistry. Understand what is meant by the kinetic theory of matter. Be able to offer explanations for events on the macroscale in terms of behavior of atoms and molecules on the microscale. Know what is meant by a chemical process and a chemical reaction and why energy is given out or taken in by them. Know about the quantum structure of the atom. Be able to explain how atoms form bonds in molecules. Know the basic principles of spectroscopy. Understand how atoms are held together in molecules. Be able to write structural formula for compounds, containing more than 4 atoms, of C, H, N and O.
Be able to suggest strategies for solving problems.
Know what chemists mean by the following terms: atom, electron, proton, neutron, molecule, compound, mixture, ion, isotope, atomic weight, mole, molar mass, metal, non-metal, metalloid, periodic table, accuracy, precision, Avogadro’s number.
Be able to convert from mass (in g) to number of moles (mol) and vice versa.
Know the names of elements and their symbols (inside front cover, 2.7). Not lanthanides or actinides or 104-109. Know the physical form of elements at room temperature and pressure.
Know the chemical formulae of some common molecules.
Know that chemical composition is important and that an important application of chemistry is to the analysis of materials. Be able to calculate a formula from percent composition data.
The charges on the ions that common elements form when they form ions in solids or solution (Fig 3.7).
The formulae of common anions and the ammonium cation (Table 3.1).
The rules for solubility (Fig 5.1). The rules for oxidation states (p. 171).
The common acids and bases, and which are strong and which are weak (Table 5.2).
You should be able to:
Covert moles to grams and grams to moles (p. 59)
Write formulae from names (3.3 and 3.4),
Calculate an empirical formula and a molecular formula from analytical data (3.6).
Write chemical expressions and balance them to make equations (4.2); write a net ionic equation (p. 155, 164, 167).
Calculate the mass of reactants or products from the reaction stoichiometry (4.3).
Round the results of calculations to the appropriate number of significant figures.
Chapters 6 - 8.
Distinguish between energy and power.
Be able to calculate the amount of heat given out or taken in by a system.
Use Hess’s law to calculate an enthalpy change for a reaction.
Be able to calculate a standard enthalpy of reaction from standard enthalpies of formation.
Understand the relationship between wavelength, frequency and speed for wave motion.
Be able to name the various regions of the electromagnetic spectrum.
Be able to calculate the energy of a photon.
Be able to calculate a wavelength of an emission or absorption line in the H spectrum on the basis of the Bohr theory.
Know the three quantum numbers arising from the solutions of Schrodinger’s equation and the relationship between them.
Know the shapes of s, p and d orbitals.
Be able to explain the phenonema of diamagnetism, paramagnetism and ferromagetism and be able to predict the first two from electron structure (understand the relationship with electron spin)
Be able to write the electronic structure of any element in the periodic table using either the spectroscopic notation or the orbital box notation (know the order in which orbitals are filled).
Be able to write the electronic structure of common ions (cations and anions) of common elements.
Be able to explain periodic trends in properties of elements (size, ionization energy, electron affinity) in terms of electronic structure.
Be able to place atoms and ions in order of size.
Be able to predict the relative values of ionization energies and electron affinities of elements.
Be able to correlate chemical characteristics of elements with electronic structure.
Explain what ionic and covalent bonds are.
Draw Lewis structures for molecules and ions.
Account for bond order, lengths and strengths
Explain the concept of resonance (as it applies to chemical bonding)
Estimate DH of a reaction from the individual bond enthalpies of the reactants and products.
Explain the concept of electronegativity, know the trends in this parameter in the periodic table and be able to predict the polarity of bonds and molecules.
Describe and predict the shape of molecules and estimate bond angles.
Explain the concept of hybridization of atomic orbitals and propose hybridization schemes to account for molecular geometry.
Explain the formation of sigma and pi bonds and how they differ, and how a molecule with a double bond can have geometrical isomers.
Explain the basic concepts of molecular orbital theory with the production of bonding and antibonding orbitals.
Use molecular orbital theory to predict bond orders and relative strengths of bonds in simple molecules.
Chapters 12 and 13.
Know the relationship between pressure, volume, temperature and number of mol of a gas. Know how gas density relates to these parameters.
Be able to solve problems in which one unknown in the general gas equation is to be found.
Understand how the components of gas mixtures exert partial pressures.
Be able to explain the behavior of gases in terms of the kinetic theory. This behavior includes diffusion and effusion.
Be able to explain the properties and behavior of liquids (and vapor in contact with liquids) in terms of the interactions between molecules and ions. Be able to predict trends in properties (such as boiling point, vapor pressure, surface tension, viscosity) in terms of the interactions between molecules.
Be able to explain behavior and properties of liquids on the basis of the kinetic-molecular theory.
Chemical Analysis
Understand how chemistry can be applied to obtain information about chemical composition. Know what is meant by qualitative and quantitative analysis, analyte, and matrix. Calculate the amount of analyte present based on the results of titrimetric or gravimetric procedures. Understand how chemical analysis can be achieved by spectroscopic measurements.