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Transcript
Mr. Shields Learning Objectives - Unit 9 Ionic and Metallic Bonding Regents Chemistry Know the definition of a Chemical Bond Know what the most abundant metal and non-metal is in the earth’s crust Recognize that the driving force of chemical bond formation is the formation of the octet o Know the definition of an ionic bond o Know that the attraction of opposite charges is the force of attraction in an ionic bond Be able to describe ionic bond formation in term of an electron transfer process o Metals transferring electrons to non-metals o Draw Lewis dot structures to show how electrons are transferred to form ionic compounds Given 2 elements be able to determine the chemical formula of the ionic compound formed when they react o Be able to use oxidation numbers to help explain the formula o Be able to show how electrons are transferred between all the atoms Be able to draw and explain key points on the PE Curve for bond formation o Filled s and p orbitals in the valence shell Know that PE is stored in a chemical Bond Be able to explain why energy is absorbed when a bond is broken & energy is released when a bond is formed. o Ionic reactions are exothermic o Bond breaking is endothermic Know that metals tend to form Cations (pos. ions) and non-metals tend to form Anions (neg. ions) and together they form ionic compounds Know that binary ionic compounds contain 2 different elements (but not necessarily only 2 atoms) Know that ionic compounds form crystal lattice structures and be able to explain in general terms how these are arranged in terms of alternating positive and negative charge Be able to Calculate which of several compounds is more ionic than the others based on electronegativity differences Know that bonds having an electronegativity difference greater than 1.7 are considered to be ionic o The higher the EN difference the greater the ionic character o Less than 1.7 the compound is not considered ionic Be able to discuss the physical properties of IONIC compounds Be able to explain why Ionic compounds will not conduct electricity in the solid (crystalline) phase but will conduct electricity if molten or in solution Be able to draw Lewis Dot structures for ions and Ionic compounds Define the term oxidation number 1 Mr. Shields o Learning Objectives - Unit 9 Ionic and Metallic Bonding Regents Chemistry Know the Typical oxidation numbers for Group 1,2, 13-18 Know the Crisscross method for determining the subscripts in binary ionic compound formulas Know how to name ionic compounds using the stock system when given the chemical formula (ex. Cr(NO3)3 = Chromium (III) nitrate) Know how to write ionic compound formulas when given their stock system name for example Chromium (III) nitrate = Cr(NO3)3 Know that the names of binary ionic compounds end in –ide (ex. Calcium sulfide) Know polyatomic ions are groups of atoms covalently bonded that have a positive or negative charge that enables them to form ionic compounds Recognize in a chemical formula the presence of a polyatomic ion o Memorize the names, formula and charge of the Polyatomics in the list given you o Be able to use TABLE E to determine names, formulas and charge whne needed Know that the endings of polyatomic ions end in –ite, -ate, and –ide. o Polyatomic ions ending in –ate have more oxygen than those ending in –ite (ex. SO4 = sulfate, SO3 = sulfite) Know the definition of a metallic bond Be able to explain how metallic bonds are formed in terms of valence electrons and temporary cations o Freely flowing valence electrons moving from one overlapping valence shell to the next Be able to explain verbally and visually what is meant by the term “sea of electrons” Be able to discuss the physical properties of METALS Know that metals conduct electricity and are good conductors of heat o Be Explain these properties of metals in terms of delocalized electrons Know that as the possible number of delocalize electrons increases strength and hardness of the metal also increases Be able to explain why metals are malleable and ductile whereas ionic compounds are not o Ionic compounds form crystals that will shatter if struck hard 2