Midterm: Open Ended

Today’s Agenda Midterm – Open Ended Silently read – Chapter 13: States of Matter Answer Section Assessment Questions throughout chapter Take Home Assignment: Finish Reading Chapter 13, and answering Section Assessment Questions

Goals Complete the Open Ended section of the Chemistry Midterm. Give examples of substances that exist in the solid, liquid, and gas states at room temperature.

Big Idea: Chemistry is the study of matter and the changes it undergoes. Concept: Observations can be quantitative, qualitative, direct, or indirect Concept: Atoms are made up of smaller particles including protons, neutrons, electrons, quarks, etc. Concept: Chemical periodicity is the basis for the arrangement of the periodic table. Concept: Mixtures can be separated by physical means because the different components have different properties. Concept: The use of significant figures assures that quantitative observations are both accurate and precise.

Big Idea: Changes in matter are accompanied by changes in energy. Concept: All matter is made up of atoms. Concept: Atoms are the smallest pieces of an element that still retain the properties of that element. Concept: Average atomic masses of the elements are reported on the periodic table. Concept: Electrons are found in quantized energy levels within the atom. Concept: The electronic structure within atoms is predicted by the Aufbau Principle, the Pauli Exclusion Principle, and Hund’s Rule, giving the atom its most stable arrangement. Concept: Energy is absorbed or emitted when electrons move from one energy level to another within the atom. Concept: Isotopes are atoms of the same element with different numbers of neutrons.

Big Idea: Atomic theory is the foundation for the study of chemistry. Concept: Energy is absorbed or emitted when electrons move from one energy level to another within the atom.

Big Idea: Periodic trends in the properties of atoms allow for the prediction of physical and chemical properties. Concept: Physical properties of matter can be described as intensive (like density) or extensive (like mass). Concept: Trends in the periodic table can predict the properties and behaviors of elements.

Big Idea: Chemical bonding occurs as a result of attractive forces between particles. Concept1: Electrons are found in quantized energy levels within the atom. Concept 2: The electronic structure within atoms is predicted by the Aufbau Principle, the Pauli Exclusion Principle, and Hund’s Rule, giving the atom its most stable arrangement. Concept 3: The type of bonding that occurs between atoms is related to the valence electrons of those atoms. Concept 4: Chemical bonding can be covalent, polar covalent, or ionic. Concept 5: lewis dot diagrams are useful for studying the structure and bonding nature of atoms.

PA Standards 3.2.C.A1 “Differentiate between pure substances and mixtures; differentiate between heterogeneous and homogeneous mixtures.” 3.2.C.A2 “Relate the position of an element on the periodic table to its electron configuration and compare its reactivity to the reactivity of other elements in the table,” and “Compare the electron configurations for the first twenty elements of the periodic table.” and “Explain how atoms combine to form compounds through both ionic and covalent bonding.” 3.2.C.A5 “Recognize discoveries from Dalton (atomic theory), Thomson (the electron), Rutherford (the nucleus), and Bohr (planetary model of atom), and understand how each discovery leads to modern theory. Describe Rutherford’s “gold foil” experiment that led to the discovery of the nuclear atom.” 3.2.C.A6 Science as Inquiry A2: Distinguish among the isotopic forms of elements. Explain the probabilistic nature of radioactive decay based on subatomic rearrangement in the atomic nucleus.