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Chemical Bonding
- 2. Biological, chemical, and physical properties of matter result from the ability of atoms to form bonds from electrostatic forces between electrons and protons and between atoms and molecules. As a basis for understanding this concept:
- a. Students know atoms combine to form molecules by sharing electrons to form covalent or metallic bonds or by exchanging electrons to form ionic bonds. Ch. 8, Ch. 9
- b. Students know chemical bonds between atoms in molecules such as H2, CH4, NH3, H2CCH2, N2, Cl2, and many large biological molecules are covalent. Ch. 9
- c. Students know salt crystals, such as NaCl, are repeating patterns of positive and negative ions held together by electrostatic attraction. Ch. 8.2, p. 217-220
- d. Students know the atoms and molecules in liquids move in a random pattern relative to one another because the intermolecular forces are too weak to hold the atoms or molecules in a solid form. Ch. 13.3
- e. Students know how to draw Lewis dot structures. Ch. 9
- f.* Students know how to predict the shape of simple molecules and their polarity from Lewis dot structures. Ch. 9.4
- g.* Students know how electronegativity and ionization energy relate to bond formation. Ch. 6.3
- h.* Students know how to identify solids and liquids held together by Van der Waals forces or hydrogen bonding and relate these forces to volatility and boiling/melting point temperatures. Ch. 13.4
- The standards marked with an asterisk need to be learned by the honors chemistry class only. All other standards need to be learned by all chemistry students.
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