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Understanding Bonding and Nomenclature: Ionic and Covalent Compounds

In this three-week unit, we will explore the different types of bonds formed by elements and learn how to name the resulting compounds. Students will memorize essential rules and procedures through consistent practice, including regular homework assignments and quizzes. We will cover topics such as ionic and covalent bonding, the transfer and sharing of electrons, and the significance of chemical formulas. Students will also engage in drawing Lewis dot diagrams to visualize these concepts. Key concepts will include solubility, the octet rule, and the properties of various compounds.

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Understanding Bonding and Nomenclature: Ionic and Covalent Compounds

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  1. Bonding and Nomenclature Unit • About 3 weeks • Will discuss the bonds that elements form and how to name the compounds formed • There are many rules and procedures that simply must be memorized and practiced • Therefore, there will be small amounts of homework regularly and several quizzes

  2. Ionic Bonding Covalent Bonding Transfer of Electrons (e-) Sharing Electrons (e-) Cmpds shown as a formula with chemical symbols and numbers Between (b/w) cations & anions B/w two nonmetals Weaker than Ionic bonding B/w metals & nonmetals Therefore, lower melting point (mp), boiling point (bp) and hardness Stronger than covalent bonding Both follow Octet Rule: Cmpds form so that each atom has an octet of ve-. Can lose, gain or share to reach 8. Except H which is full with 2. Therefore, higher melting point (mp), boiling point (bp) and hardness Can be soluble or insoluble depending on polarity Sometimes referred to as a molecular compound (cmpd) Soluble: ability to be dissolved Example: Na+ Cl- NaCl Sodium Chloride Example: CO Carbon Monoxide Chemical bond: mutual electrical attraction between the nuclei and valance electrons of atoms which binds the atoms together.

  3. Covalent Bonding • Can be either polar or non-polar • Polar: uneven distribution of charge caused by two different nonmetals bonding together. If there is a large enough difference, they can be soluble. Ex: C-O • Nonpolar: An even distribution of charge caused by the same non-metal bonded to one another. These are insoluble. Ex: Cl-Cl

  4. Homework tonight! Define the key terms: Chapter 6, Sections 1, 2, and 3 (page 208—21 words) • Tomorrow we will be drawing compounds as Lewis Dot Diagrams. You do not need your book.

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