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NEED MORE EMPHASIS ON ISOTOPES C4.10c Calculate the average atomic mass of an element given the percent abundance and mass of the individual isotopes. C4.10d Predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table C4.10 e Write the symbol for an isotope in nuclear notation C4.8h Describe the shape and orientation of s and p orbitals. ___ Orbital (S, P, D, F) ___ Noble Gas Configuration ___ WS – Electron and Noble Gas Configurations ___ Activity – Electron Configuration Battleship. ___ Quiz – Electron Configurations Student Expectations – Changing the Electrons and Neutrons within Atoms Big Idea / Question(s): 1. What types of changes can occur to atoms without altering the atom’s elemental identity? 2. How do the changes that occur to atoms effect the properties of those atoms? Overview: In this short unit we will see how the periodic table can be used to deepen our understanding of atom models. We will see that even atoms of the same element can be different. Isotopes are atoms of the same element with different masses. Isotopes are created when atoms of the same element do not have the same number of neutrons. Atoms of the same element may also have different numbers of electrons. If an atom changes its number of electrons and the atom has an unequal number of protons and electrons then the atom will be charged. Charged atoms are called Ions. Even though atoms of the same element may have different numbers of neutrons or electrons we need to remember that they are still the same element. Only changing protons (or atomic number) changes the element. The concepts and terms learned in this unit will be important to us throughout the rest of chemistry. Perhaps the most important of these concepts are valence electrons, ions and isotopes. Vocabulary Terms: ___ Ion ___ Electron Configuration ___ Average Atomic Mass ___ Charge ___ Isotope ___ Element Symbol ___ Atomic Number ___ Mass Number ___ Metallic Character ___ State of Matter ___ Valence Electrons ___ Hyphen Notation ___ Nuclear Notation Resources: Section 3.3 (pages 77 through 82) – Subatomic Particles, Atomic Mass, Mass Number and Atomic Number Assignments: ___ Outline (pages 77 through 82) and Section Review 3.3 # 1 a-d, h, 2, 3 (Subatomic Particles, Atomic Mass, Mass Number and Atomic Number) ___ WS – SubAtomic Particles and Periodic Table Basics ___ Quiz - SubAtomic Particles, Electron Configurations and Periodic Table Basics CONCEPTS TO KNOW (BOLDED ARE MORE IMPORTANT) Introduced: _______ Basic: _________ Mastered: _________ the differences between charged and neutral atoms. I can identify and describe What is the difference between a neutral fluorine atom and a fluoride atom which is an atom of fluorine with a 1_ charge? Introduced: _______ Basic: _________ Mastered: _________ of each subatomic particle in any given atom. I can find out the number Introduced: _______ Basic: _________ Mastered: _________ element in question from the number of subatomic particles. I can determine the If an element has 25 protons what is the element? If an element has a 2+ charge and 10 electrons what is the element? What subatomic particle cannot be use to identify an element? Introduced: _______ Basic: _________ Mastered: _________ I can describe how an atom becomes charged and how to determine the exact numerical charge of the ion. I can describe ions as either anions (negative atoms) or cations (positive atoms). Describe how sodium (Na) becomes a 1+ ion? Is Na1+ a cation or anion? Why would Na become a positive ion and fluorine (F) would be a 1-? Introduced: _______ Basic: _________ Mastered: _________ I can define an isotope. Compare and contrast isotopes of Uranium – 234, Uranium – 235 & Uranium – 238? C4.10c Introduced: _______ Basic: _________ Mastered: _________ I can calculate the average atomic mass of an element given the percent abundance and mass of the individual isotopes. Calculate the atomic mass of rubidium. The two isotopes of rubidium have atomic masses and relative abundancies of 84.91 amu (72.16%) and 86.91 amu (27.84%). C4.10d Introduced: _______ Basic: _________ Mastered: _________ I can predict which isotope will have the greatest abundance given the possible isotopes for an element and the average atomic mass in the periodic table Which isotope of lithium is more abundant Lithium – 6 or Lithium – 7? Explain C4.10 e Introduced: _______ Basic: _________ Mastered: _________ for an isotope in nuclear notation I can write the symbol Write the nuclear notation for isotopes of uranium 235 and 238. Introduced: _______ Basic: _________ Mastered: _________ among isotopes of the same element. I can describe the differences Introduced: _______ Basic: _________ Mastered: _________ get metallic character and state of matter. I can read the periodic table to Describe the basic trend for metallic character within the periodic table. Give examples that support your trend. Describe the basic trend for state of matter within the periodic table. Give examples that support your trend. C4.8x Introduced: _______ Basic: _________ Mastered: _________ energy levels and orbital blocks within the periodic table. I can identify the What block and energy level do the following elements belong: K, V, C, U? C4.8e Introduced: _______ Basic: _________ Mastered: _________ I can construct the electron configuration and the noble gas configuration for S and P block elements. Write the electron configuration and noble gas configuration for I. C4.8x Electron Configuration - Electrons are arranged in main energy levels with sublevels that specify particular shapes and geometry. Orbitals represent a region of space in which an electron may be found with a high level of probability. Each defined orbital can hold two electrons, each with a specific spin orientation. The specific assignment of an electron to an orbital is determined by a set of 4 quantum numbers. Each element and, therefore, each position in the periodic table is defined by a unique set of quantum numbers.; C4.8e Write the complete electron configuration of elements in the first four rows of the periodic table. C4.8f Write kernel structures for main group elements. C4.8h Describe the shape and orientation of s and p orbitals. Include! Demo - Mind Reading Game; Lecture on the Reading Periodic Table, WS - Periodic Table Basics Quiz - Periodic Table Basics Plan - SubAtomic Particles, Electron Configurations and Periodic Table Basics Day 1 and 2 – Assign Out (pages 77 through 82) and SR 3.3 # 1 a-d, h, 2, 3 – Subatomic Particles, Atomic Mass, Mass Number and Atomic Number. This assignment will be due Day 4. Use the C4.10 A – D. WS – SubAtomic Particles and Periodic Table Basics as the means of learning how to determine the number of each subatomic particle in the atom, whether the atom is charged, difference between isotopes, and how to read the periodic table to get metallic character and state of matter. Day 2 and 3 – Students will learn how to construct an electron and noble gas configuration using WS – Electron and Noble Gas Configurations and Activity – Electron Configuration Battleship. Day 4 – Check-In and Review Out and SR 3. 3 (pages 77 through 82). Quiz - SubAtomic Particles, Electron Configurations and Periodic Table Basics Teach students how to write the electron configurations for main group elements, Finish with Electron Configuration Battleship; WS - Electron Configurations (or do H thru K, Ga, Br, Te, Cs, Pb, Rn); Quiz – Electron Configurations