Second Semester Chemistry Study Guide

Transcription

1 Second Semester Chemistry Study Guide All of the information on this review is fair game for the final Some information will be more prevalent on the test (Think about which topics we spent more time on through class ) Everything included has been covered in your notes The final will include a variety of question types from multiple choice to matching, completion, illustration, calculations, and problem solving The final may also include up to three short answer questions that will be expected to contain a 3+ sentence response for potential full credit Chapter 1 1. Scientific Method Identify the six components of the scientific method Chapter 2 2. Properties of matter Contrast extensive & intensive properties of matter Contrast physical & chemical properties of matter Identify the three main states of matter Identify key properties of each state of matter Contrast physical changes & chemical changes 3. Mixtures Contrast homogeneous & heterogeneous mixtures Identify methods that separate mixtures Chapter 3 4. Measurement Be able to write numbers in scientific notation Be able to calculate the error of an experimental value Be able to calculate the percent error of an experimental value Be able to determine the significant figures of a value Be able to determine significant figures of a calculated value (after +, -, x, ) Be able to use conversion factors to convert between metric prefixes

2 Chapters 4 & 5 5. Structure & Models of the Atom What is an atom? Illustrate and describe each key scientist s model of the atom i. Dalton ii. Thomson iii. Rutherford iv. Bohr v. Schrodinger Describe Thomson s Cathode Ray Tube Experiment and what he was able to conclude Describe Rutherford s Gold-Foil Experiment and what he was able to conclude Differentiate between the properties of the three subatomic particles (actual mass will not be on the test, but all else may be) Describe the idea of a quantum Describe what defines an element s atomic number Describe what defines an isotope s mass number Be able to determine an element s atomic mass by using mass numbers and relative abundance 6. Electron Arrangement Be able to use the Aufbau diagram, Pauli Exclusion Principle, and Hund s Rule to correctly place electrons in an electron configuration Be able to write an element s electron configuration in both the long and short forms 7. Atomic Orbitals Identify the number of electrons that may fit into each energy level Identify the number of sublevels that may fit into each energy level Identify the number of electrons that may fit into each sublevel Identify the number of orbitals each sublevel has present 8. Atomic Spectra Identify and describe the relationship shown in the equation c=λν Use the above equation to determine an unknown wavelength or frequency Explain how and why light is emitted from an excited gas Explain why light emitted from gases has very specific emission spectra that is unique to each element Chapter 6 9. Organizing & Classifying Describe how the modern periodic table is arranged (there are many possible correct answers) Differentiate between the three classes of element by their properties Be able to identify groups with special names (alkali metals, alkaline earth metals, halogens, noble gases) Relate an element s position on the periodic table (noble gases, representative elements, transition metals, and inner transition metals) to its electron configuration Be able to identify blocks on the periodic table Be able to use the periodic table to determine an element s electron configuration

3 10. Trends Define atomic size Define atomic attraction Define the shielding effect Identify how an ion forms Contrast cations and anions (be sure to compare each to its neutrally-charged atom) Define ionization energy Define electronegativity Describe the group & periodic trends of atomic size Be able to determine which element would have a greater or lesser atomic size Describe the group & periodic trends of ionization energy Be able to determine which element would have a greater or lesser ionization energy Describe the group & periodic trends of ionic size Be able to determine which element would have a greater or lesser ionic size Describe the group & periodic trends of electronegativity Be able to determine which element would have a greater or lesser electronegativity Chapter Ions Describe valence electrons Be able to illustrate an atom or ion using Lewis Dot Structures Be able to use the octet rule to determine the number of electrons gained or lost by an atom Identify which atoms will become cations, and which will become anions 12. Ionic Bonds & Compounds Describe an ionic bond Describe why ionic compounds are neutrally charged Be able to write the chemical formula & formula unit of an ionic compound Identify the three key characteristics (properties) of ionic compounds Describe why ionic compounds are able to conduct an electric current when dissolved in water 13. Bonding in Metals Describe the structure of metals at the atomic level Describe a metallic bond Describe how the sea of electrons model supports the metallic properties of being a good conductor, having high malleability, and high ductility Explain why alloys are often better than the element alone Chapter Molecular Compounds Describe a covalent bond Describe a molecule Identify the properties of molecular compounds Contrast a molecular formula from a chemical formula of an ionic compound

4 15. Covalent Bonding Differentiate between single, double, & triple covalent bonds Be able to write the structural formula of a compound Explain how a coordinate covalent bond is formed Be able to illustrate a coordinate covalent bond Define a polyatomic ion Explain how a polyatomic ion is formed Be able to illustrate a polyatomic ion 16. Bonding Theories Define VSEPR theory Explain why VSEPR theory is important in chemistry Explain the importance of unshared electron pairs in VSEPR theory Describe a domain Be able to determine the number of domains for a given atom Be able to determine the proper VSEPR shape for a given central atom Contrast a molecular orbital from an atomic orbital Identify the two types of molecular orbitals that may form from a bond Be able to identify the proper number and type of bond(s) between any two atoms Define orbital hybridization Be able to determine the orbital hybridization of an atom 17. Polarity & Attraction Contrast nonpolar & polar covalent bonds Explain what causes polar bonds Be able to illustrate the presence of a polar bond Describe how the shape of a molecule may determine its polarity Describe what causes hydrogen bonding Chapter Ionic Compounds Know the polyatomic ions provided on your polyatomic ion list Be able to correctly write the name of binary and polyatomic ionic compounds Be able to correctly write the formula of binary and polyatomic ionic compounds 19. Molecular Compounds Be able to correctly write the name of binary molecular compounds Be able to correctly write the formula of binary molecular compounds

5 Chapter The Mole Define a mole and the value associated with it Be able to convert a number of particles to moles Be able to convert moles to a number of particles Be able to determine the molar mass of an element or compound 21. Other Mole Relationships Be able to convert mass, in grams, to moles Be able to convert moles to mass, in grams Identify the volume of any gas at STP Be able to convert volume of a gas, in liters, to moles Be able to convert moles to volume of a gas, in liters 22. Composition of Compounds Be able to determine the percent composition of a compound by calculating the percent mass of each element from mass data Be able to determine the percent composition of a compound by calculating the percent mass of each element using the chemical formula Be able to use percent composition as a conversion factor Define empirical formula Be able to determine the empirical formula of a compound from percent composition Define molecular formula Be able to determine the molecular formula of a compound from percent composition Chapter Describing Reactions Be able to write a word equation for a chemical reaction Be able to convert a word equation to a skeleton equation Be able to properly balance a chemical equation for a chemical reaction 24. Types of Reactions Identify the five general types of chemical reactions from a provided chemical equation Predict the products of any given reactants Be able to use the Activity Series of Metals to identify if a single-replacement reaction will occur Be able to use the Activity Series of Halogens to identify if a single-replacement reaction will occur Be able to use the Solubility Chart to identify if a double-replacement reaction will occur May be on final dependent on if we get to the content in class Chapter Chemical Calculations Be able to use a balanced chemical equation to write and use a mole ratio Be able to use a mole ratio to convert from moles of one substance to moles of another substance Be able to use a mole ratio to convert from units (mass, volume, particles) of one substance to units (mass, volume, particles) of another substance