Chapter One - Intro to Chemistry Essential Questions: How does the work of chemists impact scientific research and everyday life?
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1 The science of chemistry affects all aspects of life and most natural events. Chapter One - Intro to Chemistry How does the work of chemists impact scientific research and everyday life? Why studying chemistry is important to them. The steps and processes of the scientific method. How the use of various deliberate techniques will assist them in both numeric and conceptual problem solving. Discuss examples of current research in chemistry. Apply each step of the scientific method to chemical research examples. Implement specific strategies for solving numeric and conceptual problems. Use a consistent method to track and document the inquiry process (lab notebook) Physical and chemical properties as determined through an investigation can be used to identify a substance How properties used to describe matter can be classified. The differences among the 3 states of matter The differences between physical and chemical properties. What occurs during a chemical reaction How the law of conservation of mass applies to all physical and chemical changes Chapter Two- Matter and Change How does matter tend to behave, react and change? Distinguish between extensive and intensive properties Differentiate among the 3 states of matter Discuss reversible and irreversible physical changes Classify mixtures as homogeneous or heterogenous Discuss various ways to separate mixtures Describe the differences among elements, substances, mixtures, and compounds Describe what happens during a chemical change Identify 4 possible clues that a chemical change has taken place Apply the law of conservation of mass to chemical reactions
2 Accuracy and precision in measurement are fundamental to experimental science. Conversion methods for scientific notation and unit conversion How density relates to temperature, mass and volume. Rules for significant figures and calculations using significant figures. Chapter 3- Measurement and Uncertainty How do measurement techniques, accuracy and precision impact experimental science? Chapter 4- Atomic Structure of atomic structure and functions has changed and developed over time, and continues to do so. How Democritus, Dalton, Rutherford and others impacted atomic theory. How modern technology and instrumentation allows us to visualize the nature of individual atoms. How subatomic particles influence the identity and mass of elements. The basic information about atoms and elements contained in the periodic table Convert measurements to scientific notation Distinguish among accuracy, precision, and error of a measurement Determine the number of significant figures in a measurement and in a calculated answer Distinguish between mass and weight Convert between temperature scales Use dimensional analysis to convert convert simple and complex units Calculate density from experimental data Describe how density varies with temperature How does our understanding of the structure of atoms affect our ability to explain the structure and behavior of matter? Discuss changes over time in atomic theory. Describe the structure of atoms according to the Rutherford model. Explain what makes elements and isotopes different from each other Given partial information, calculate numbers of protons, neutrons, electrons and atomic mass of atoms of various elements.
3 Energy level changes and the positions of electrons in atomic orbitals are key factors in the behavior of atoms, elements, and all matter. How inadequacies in the Rutherford model led to Bohr s new proposals. How the quantum mechanical model describes energies and positions of electrons How shapes of electron orbitals relate to different orbital sublevels. The Aufbau principle, Pauli Exclusion priniciple, and Hund s rule. How the movement of electrons into higher and lower energy levels impacts energy absorption and light emission. The relationship between wavelength and frequency. How quantum mechanics describes the motions of subatomic particles and atoms as waves, and differs from the ways in which classical mechanics describes the motions of larger bodies. Chapter 5- Electrons in Atoms How do the Bohr and Quantum Mechanical models help explain the impact of electrons on the behavior of matter? Relate energy levels and orbits to the behavior of electrons. Explain how the quantum mechanical model further explains the probable location and behavior of electrons. Chart the principle energy levels, sublevels and number of possible electrons found in orbitals as described by the quantum mechanical model. Explain how the shapes of p and s orbitals relate to the probable location of electrons. Use an Aufbau diagram to determine the electron configuration of representative elements. Describe how the Aufbau principle, Pauli exclusion principle and Hund s rule drive electron configurations. Explain why some elements have electron configurations that differ from those determined by using the Aufbau principle. Explain the main concept of the Heisenberg Uncertainty principle. Given 2 out of 3 quantities, calculate the energy, frequency, or wavelength of photons. Use the concept of the atomic emission spectrum to explain why each element emits a particular color spectrum of light.
4 Chapter 6- The Periodic Table Physical and chemical properties of most elements can be predicted from information and position in the periodic table. Mendeleev and other chemists used the properties of elements to sort them into groups The basic, identifying properties of metals, nonmetals and metalloids What information about elements in shown in each square, group and period of the periodic table How elements can be classified based on their electron configurations How and why cations and anions form Trends in atomic size, ionic size, ionization energy, and electronegativity occurring in the periodic table How does the periodic table allow prediction of the chemical and physical properties of elements? Classify elements based on their position in the periodic table Determine atomic mass and numbers of protons, neutrons and electrons in an element based on information available in the periodic table Use the periodic table to determine and track the number of electrons in highest occupied energy levels of different elements Given shorthand electron configurations, determine the symbols for elements represented by these configurations Differentiate between ionization energy and electronegativity Explain the reasons for trends in atomic size, ionic size, ionization energy and electronegativity in the periodic table
5 Valence electrons and the octet rule drive the properties, electrical charges, and bonding systems of ionic compounds and metals The number of valence electrons in atoms of each representative element How cations and anions form The electrical charge of ions and ionic compounds Properties of ionic compounds How valence electrons behave in metallic bonding Why metal alloys have different properties than their component elements Chapter 7- Ionic and Metallic Bonding How do the octet rule and numbers of valence electrons explain the formation and electrical charge of ions and bonding patterns of ionic compounds and metals? Find the number of valence electrons in an atom of a representative element Explain why different elements gain or lose electrons to become ions Determine the correct chemical formula for ionic compounds Explain how melting points, crystalline solid structure and electrical conductivity relate to ionic bonding Explain how electron configuration and position connects to the malleability, ductility and crystalline structure of metals
6 Chapter 8- Covalent Bonding Electron sharing patterns affects bond strength, molecular shape and chemical properties. Molecular compounds tend to have lower melting and boiling points. A molecular formula shows how many atoms of each element a molecule contains. Single, double or triple covalent bonds form so that atoms can attain the configurations of noble gases. How coordinate covalent bonds form. How covalent bond strength corresponds with bond dissociation energy. When and why the octet rule cannot be satisfied. How VSEPR theory connects to molecular shapes. How intermolecular forces and polarity affect the behavior of molecules. How does electron sharing vs. electron transfer affect the properties of covalently bonded molecules and substances? Explain why molecular compounds have lower melting and boiling points than ionic compounds. Draw/write structural and molecular formulas for various molecular compounds. Use the octet rule and electron dot structures to determine bonding patterns. Explain how a coordinate covalent bond differs from a more typical covalent bond. Draw an electron dot (Lewis) structure for molecules with single, double and triple covalent bonds. Use molecule kits to model the bonding patterns and shape of various molecules. Show 2 or more electron dot structures for molecules showing resonance. Explain why some molecules cannot satisfy the octet rule. Differentiate between sigma and pi bonds in molecular orbitals. Use VSEPR theory to predict the shape of various molecules. Explain the difference between polar and nonpolar covalent bonds. Compare Van der Walls forces to Hydrogen bonds. Describe how the covalent bonds in network solids result in very high melting points.
7 Molecular compounds can be named and interpreted based on a system of rules and scientific laws. Chapter 9- Chemical Names and Formulas How to name and identify monoatomic and polyatomic ions. Rules for naming binary ionic and polyatomic ion compounds, binary molecular compounds and acids and bases. How the laws of definite and multiple proportions apply to chemical formulas and reactions. What rules and laws govern the naming and interpretation of molecular formulas? Name ions of representative and transition metals Compare the stock and classical systems for naming metal ions with more than one ionic charge Name and write formulas for common polyatomic ions Given names, write formulas for binary ionic compounds, polyatomic ion compounds, binary molecular compounds, and acids and bases. Given formulas, name binary ionic compounds, polyatomic ion compounds, binary molecular compounds, and acids and bases Given the masses of reacting elements, calculate mass ratios using the law of multiple proportions.
8 Atomic and molar masses can be used to determine particle counts, mass, volume, percent composition and chemical formulas of substances and compounds. How to use dimensional analysis to complete unit and molar conversions. How Avogadro s number relates to the count of representative particles in substances. How the mole is used to represent quantities in chemistry. How to convert among molar mass, moles, number of particles, mass and volume. How to calculate the percent by mass of an element in a compound. The relationship between empirical and molecular formulas. Chapter 10- Chemical Quantities How can the count, mass and volume of a substance be measured? Identify numbers of representative particles in atoms, molecules and formula units of various substances. Given a chemical formula, calculate the molar mass of a substance. Use dimensional analysis to convert among mole-mass and mole-volume relationships. Calculate percent composition of each element in a given compound. Use percent composition information to calculate gram amounts of each element in a given mass of a compound. Given percent composition information, determine the empirical formula of a compound. Given molar mass and empirical formula, determine the molecular formula of a compound. Relate drug testing technology to the separation and identification of chemical components.
9 Five general types of chemical reactions obey the law of conservation of mass and represent the behavior of most substances as they combine and break down. How to write word and skeleton equations using appropriate symbols. Why the law of conservation of mass controls the balancing of chemical equations. How to follow steps and use coefficients to balance chemical equations. The differences among combination, decomposition, single-replacement, double-replacement and combustion reactions. How the activity series of metals can be used to predict the products of singlereplacement reactions. The conditions under which doublereplacement reactions are likely to occur. The products of a hydrocarbon combustion reaction. Why many ionic reactions occur in aqueous solution. How to write and balance complete ionic and net ionic equations. How to use solubility rules to predict the formation of a precipitate in an aqueous ionic reaction. Chapter 11- Chemical Reactions How can the behavior of chemical reactants and products be described and predicted? Given a skeleton equation, write a word equation and vice-versa. Explain how the law of conservation of mass requires the balancing of chemical equations. Translate word equations to skeleton equations, and then balance these equations. Differentiate between the meaning of subscripts and coefficients in chemical equations. Label and describe a given chemical equation as combination, decomposition, single-replacement, double-replacement or combustion. Describe the conditions under which double- replacement reactions are likely to occur. Use the activity series of metals to predict the products of singlereplacement reactions. Use the solubility rules to predict the formation of precipitates in aqueous ionic reactions. Write complete ionic equations and then convert these reactions to balanced net ionic equations.
10 Chapter 12- Stoichiometry Balanced chemical equations provide information about chemical quantities and ratios, and can be used to calculate quantities of products and reactants. How to determine mole ratios from a chemical equation Steps to follow in solving mole-mole, mass-mass and volume problems using stoichiometry. What factors result in limiting and excess reagents in chemical reactions. The difference between theoretical and actual percent yield in chemical reactions. How can quantities of chemical products and reactants be determined using the information available in a balanced chemical reaction? Write mole ratios of products and reactants from a balanced chemical equation. Calculate moles and mass of products and reactants using stoichiometry techniques and dimensional analysis. Calculate molecules of a product given mass of a reactant. Calculate volume of gaseous reactants and products formed at STP. Determine the limiting and excess reagants in a reaction. Use a limiting reagent to find the quantity of a product. Calculate theoretical and percent yield of reactions.
11 The compressibility of gases allows specific relationships among pressure, temperature and volume. Why gases are easier to compress than solids or liquids. How amount, temperature and volume affect the pressure of gases. How to use Boyle s, Charles s, Gay- Lussac s and the Combined Gas Law to calculate gas variables. What is needed to calculate the amount of gas in a sample at given conditions of volume, temperature and pressure The conditions under which real gases are most likely to differ from ideal gases. How Dalton s Law of Partial Pressures relates to mixed gases. How Graham s Law explains the relationship between molar mass and diffusion and effusion rates in gases. Chapter 14- The Behavior of Gases How do the temperature, pressure, amount and volume of gases affect each other? Describe the relationships among amount, volume, temperature and pressure of gases. Use Boyle s law to calculate pressure or volume when temperature is constant. Use Charles s law to calculate temperature or volume when pressure is constant. Use Gay-Lussac s law to calculate pressure or temperature when volume remains constant. Use the Combined Gas Law with a constant volume of gas. Explain how Charles s law can be derived from the combined gas law. Use the Ideal Gas Law to find the amount of a gas in moles or mass. Use the kinetic theory of gases to explain why no gas exhibits ideal behavior at all temperatures and pressures. Explain how dissolved nitrogen may lead to nitrogen narcosis and decompression sickness in scuba divers. Use Dalton s Law of Partial Pressures to determine the total and partial pressures of mixed gases. Compare the diffusion and effusion rates of gases with different molar masses.
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