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Published byEric McKenzie Modified over 8 years ago
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مادسیج، شبکه آموزشی پژوهشی دانشجویان ایران Madsg.com مادسیج یعنی دهکده علم و دانش ایران !!
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پیوند کوالانسی و بررسی مولکول ها تنظیم از : ابولفضل احمدی دبیر شیمی ناحیه 2 قزوین
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Overlapping orbitals Draw orbital diagrams for F + F, H + O, Li + F 1s2s2p 1s2s2p 1s2s2p 1s F2F2 H2OH2O 2s1s2s2p LiF is ionic (metal + non-metal)
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تشکیل پیوند گرمازا است
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Why do covalent bonds form? Lower P.E. = More stable
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Bond Energy (B.E.) – aka Bond Enthalpy or Bond Strength Covalent Bond Strength – depends on strength of attraction between nuclei and shared electrons Bond Energy – energy needed to overcome attraction and break the bond
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Strength of Bond different than E required to pull atoms apart (B.E.) Weaker Bonds = Higher Energy “Shallow Energy Well” Stronger Bonds = Lower Energy “Deeper Energy Well” Less E needed to break. Lower B.E. More E needed to break. Higher B.E.
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Section 9.3: Covalent Bonding Bond Type (Single, Double, Triple) also matters Nuclei more attracted to 2 shared pairs of e- than one shared pair of e-. Higher bond order = Shorter bond length = Higher Bond Energy Same two elements, different B.E.
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Section 9.3: Covalent Bonding Periodic Table Trends Without Detailed Bond Lengths The closer the atoms, the stronger the bond. Bond Energy: C—F > C—Cl > C—Br
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پیوند کووالانسی قطبی و پیوند ناقطبی Polar & nonpolar Covalent Bonds
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مقایسه قطبیت پیوند
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مقایسه خصلت پیوند
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رفتار مولکول قطبی دو اتمی در میدان الکتریکی
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Writing Lewis Formulas: The Octet Rule رسم ساختار لوویس و قاعده 8 تایی
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Lorem ipsum dolor sit amet, consectetuer adipiscing elit. Vivamus et magna. Fusce sed sem sed magna suscipit egestas. Title
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