Month September October Content/Essential Quest lab equipment lab safety states of matter physical vs. chemical change element names and symbols graph construction and interpretation classifying matter conservation of energy EQ-What are the differences between pure substances and mixtures? EQ-How are changes in matter accompanied by changes in energy? metric system measurement convers temperature temperature convers density heat specific heat EQ- In what ways has the theory of the atom changed over time due to technological improvements? Skills/Activities Resources Assessments know names and funct of lab equipment demonstrate safe and proper lab technique explain similarities and differences of solids, liquids, and gases at the atomic level define and distinguish between physical and chemical change; list 3 indicat of chemical change know element names and atomic symbols; identify elements as metals, nonmetals, and metalloids construct graphs of experimental data by hand and spreadsheet software classify matter as elements,, homogeneous mixtures, or heterogeneous mixtures know matter and energy are conserved in all chemical and physical change know metric units of fundamental units of the metric system perform convers for measurements of length, mass, volume, time, and density define and distinguish between temperature and heat convert temperature measurements between degrees Celsius, degrees Fahrenheit, and Kelvin experimentally determine the density of solid and liquid matter define and distinguish between endothermic 1 Temperature probes Temperature probes lab equipment test lab safety test atomic symbol test lab: conservation of mass lab: classifying matter lab: physical and chemical change lab - measure volume lab - measuring length; calculation of volume and density lab: density of solids lab: density of Assessment Anchors and Eligible Content Chem.A.1.1.1 Chem.A.1.1.2 Chem.A.1.1.4 Chem.A.1.2.2 Chem.A.1.1.3 PA Standards Reading, Writing, Speaking, and Listening
and exothermic calculate the heat lost and gained in heat transfer events describe the accuracy and precision individual measurements and sets of measurements liquids lab: heat transfer lab: determining the Cp value of an unknown metal November atomic structure + and ion atomic structure isotopes isotope designation types of radiation the mole and molar mass arrangement of e- in atoms electron configuration notation; orbital notation; electron dot notation; periodic law EQ-How does the distribution of electrons in atoms affect the formation of a compound? describe the atomic structure of atoms in terms of protons, neutrons, and electrons know that atoms of the same element may only differ in their number of neutrons represent the atomic structure of isotopes using nuclear symbol notation and hyphen notation define and distinguish between alpha, beta, and gamma radiation perform convers between moles and number of atoms and between moles and grams of atoms know that the chemical and physical properties of elements are determined by their electron configurat lab: rxn rate and electron configurat lab: gravity filtration lab: vacuum filtration lab: half-life lab: radioactive decay and C-14 dating Chem.A.2.1.1 Chem.A.2.1.2 Chem.A.2.2.1 Chem.A.2.2.2 Chem.A.2.2.3 Chem.A.2.2.4 Chem.A.2.3.1 Chem.A.2.3.2 December chemical bonding covalent bonding Lewis structures and structural formulas ionic bonding atomic structure of + and - polar and nonpolar molecules intermolecular forces of attraction EQ- What factors determine the types of chemical bonds that form between particles? define and distinguish between ionic, covalent, and metallic chemical bonds predict type of bonding between elements by type model covalent bonding with Lewis structures and structural formulas determine the atomic structure of positive and negative classify molecules as polar or nonpolar; list and define three types of intermolecular forces of attraction; know relative strengths of intermolecular forces of attraction; explain melting point and boiling point trends in terms of intermolecular forces of lab: Lewis structures and structural formulas lab: boiling point and evaporation rate lab: like dissolves like Chem.B.1.3.1 Chem.B.1.3.2 Chem.B.1.3.3 Chem.B.1.4.1 Chem.B.1.4.2 2
January monatomic ; polyatomic binary ionic types 1 and 2 ionic of binary molecular acids and bases writing chemical equat balancing equat classifying equat EQ- What factors identify the types of chemical react? EQ- According to the collision theory, what factors affect the rate of a chemical reaction? attraction memorize formulas of common monatomic name and write formulas type 1 and 2 binary ionic name and write formulas of ionic of name and write formulas of binary molecular name and write formulas of common acids and bases write word equat, formula equat and chemical equat to represent chemical change balance chemical equat classify chemical equat as synthesis, decomposition, single replacement, double replacement, or combustion react - monatomic - - binary ionic - ionic of - binary molecular lab: types of chemical react lab: single replacement react and the activity series Chem.A.1.1.5 Chem.B.2.1.3 Chem.B.2.1.4 Chem.B.2.1.5 January motion acceleration motion in one dimension produce and interpret graphs of position versus time produce and interpret graphs of velocity versus time calculate the speed and velocities of objects convert units of velocity. calculate the acceleration of objects. zes 3.3.12.B2 February motion in one dimension objects in free-fall terminal velocity weight distinguish between average and instantaneous velocity calculate distance traveled by an object in free-fall calculate time of an object in free-fall zes project gear car design 3.3.12.B2 3
March April two-dimensional motion projectile motion forces and laws of motion Newton s 1 st law of motion Newton s 2 nd law of motion Newton s 3 rd law of motion calculate the weight of objects. know objects accelerate vertically at the same rate produce and interpret graphs of projectile motion distinguish between contact and field forces draw free-body diagrams to illustrate forces acting on objects know that frictional forces always oppose motion. know that an object accelerates when a net force acts upon it know that acceleration is directly proportional to the magnitude of applied force. know that acceleration is inversely proportional to mass. define normal force. identify action-reaction paired forces. zes project catapult design zes 3.2.10.B2 3.2.10.B2 May work kinetic energy potential energy momentum and collis electricity convert masses between units of grams and kilograms. calculate the potential energies of objects. calculate the kinetic energies of moving objects. calculate momentum of moving objects. know momentum is conserved. define and distinguish between oxidation and reduction. labelectroplating project rocketry design and competition 3.2.12.A4 3.2.10.B4 3.2.10.B5 3.2.12.B3 3.2.12.B6 3.4.12.A1 4
June Final Exam Final Exam Final Exam 5