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Catégorie :Category: nCreator TI-Nspire
Auteur Author: Hilo
Type : Classeur 3.0.1
Page(s) : 1
Taille Size: 2.16 Ko KB
Mis en ligne Uploaded: 01/05/2025 - 20:57:14
Uploadeur Uploader: Hilo (Profil)
Téléchargements Downloads: 1
Visibilité Visibility: Archive publique
Shortlink : http://ti-pla.net/a4614969
Type : Classeur 3.0.1
Page(s) : 1
Taille Size: 2.16 Ko KB
Mis en ligne Uploaded: 01/05/2025 - 20:57:14
Uploadeur Uploader: Hilo (Profil)
Téléchargements Downloads: 1
Visibilité Visibility: Archive publique
Shortlink : http://ti-pla.net/a4614969
Description
Fichier Nspire généré sur TI-Planet.org.
Compatible OS 3.0 et ultérieurs.
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1. Identify the atoms and bonds in the molecule Look at which atoms are present. Pay special attention to hydrogen attached to nitrogen (N), oxygen (O), or fluorine (F) . Identify types of bonds (single, double, etc.) and electronegativity differences (polar or nonpolar bonds). 2. Determine if any bonds are polar Use electronegativity values (approx): H = 2.1, C = 2.5, N = 3.0, O = 3.5, F = 4.0 A bond is polar if the difference is e 0.5 . For example, OH has EN = 3.5 2.1 = 1.4 very polar. 3. Determine the molecular geometry (shape) Use VSEPR theory : Count bonding and lone electron pairs on the central atom. Example: HO has 2 bonding pairs and 2 lone pairs bent shape. Geometry affects whether dipoles cancel out or not. 4. Determine molecular polarity If all polar bonds are symmetrically arranged (e.g. CO linear), the dipoles cancel nonpolar molecule . If polar bonds are asymmetrical (e.g. HO bent), dipoles dont cancel polar molecule . 5. Identify the types of IMFs present London Dispersion Forces (LDF) : Present in all molecules , especially nonpolar ones. Weak, caused by temporary electron shifts. Dipole-Dipole Forces : Only in polar molecules . Caused by attraction between permanent partial charges. Hydrogen Bonding : Only when H is directly bonded to N, O, or F . Strongest of the 3 main IMFs. 6. Finalize your IMF determination Nonpolar molecule only LDF Polar molecule LDF + dipole-dipole Polar + H bonded to N/O/F LDF + dipole-dipole + H-bonding Example: CH (methane) CH bonds: EN = 2.5 2.1 = 0.4 nonpolar Tetrahedral shape symmetrical Nonpolar molecule IMF: London Dispersion Forces only Want another example? Made with nCreator - tiplanet.org
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Compatible OS 3.0 et ultérieurs.
<<
1. Identify the atoms and bonds in the molecule Look at which atoms are present. Pay special attention to hydrogen attached to nitrogen (N), oxygen (O), or fluorine (F) . Identify types of bonds (single, double, etc.) and electronegativity differences (polar or nonpolar bonds). 2. Determine if any bonds are polar Use electronegativity values (approx): H = 2.1, C = 2.5, N = 3.0, O = 3.5, F = 4.0 A bond is polar if the difference is e 0.5 . For example, OH has EN = 3.5 2.1 = 1.4 very polar. 3. Determine the molecular geometry (shape) Use VSEPR theory : Count bonding and lone electron pairs on the central atom. Example: HO has 2 bonding pairs and 2 lone pairs bent shape. Geometry affects whether dipoles cancel out or not. 4. Determine molecular polarity If all polar bonds are symmetrically arranged (e.g. CO linear), the dipoles cancel nonpolar molecule . If polar bonds are asymmetrical (e.g. HO bent), dipoles dont cancel polar molecule . 5. Identify the types of IMFs present London Dispersion Forces (LDF) : Present in all molecules , especially nonpolar ones. Weak, caused by temporary electron shifts. Dipole-Dipole Forces : Only in polar molecules . Caused by attraction between permanent partial charges. Hydrogen Bonding : Only when H is directly bonded to N, O, or F . Strongest of the 3 main IMFs. 6. Finalize your IMF determination Nonpolar molecule only LDF Polar molecule LDF + dipole-dipole Polar + H bonded to N/O/F LDF + dipole-dipole + H-bonding Example: CH (methane) CH bonds: EN = 2.5 2.1 = 0.4 nonpolar Tetrahedral shape symmetrical Nonpolar molecule IMF: London Dispersion Forces only Want another example? Made with nCreator - tiplanet.org
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