PLEASE GIVE HANDWRITTEN ANSWERS TO ALL PARTS
Posted: Fri May 06, 2022 7:38 am
PLEASE GIVE HANDWRITTEN ANSWERS TO ALL PARTS
35. Copy the table below onto another piece of paper. Then, using the procedure outlined in the feature on page 424, fill in the blank spaces in this table. Electro- negativity Sub- stance difference type formula Bond Structural Particle type NaBr N₂ nonpolar molecule SO₂ CaCl₂ ionic C₂H6 2.5 2.1 0.4 s=0 Solu- bility in water yes
AN How To Predict solubility 1. Determine bond type by calculating. electronegativity difference and selecting range. 2. Indicate charges as needed on a structure of the substance. Check for dipoles if needed. 3. Identify parti- cle types and charges. Deter- mine solubility. 424 Chapter 11 IF the difference in electronegativities for bonded atome is between. 0.4 and 2.1, THEN the bonds are polar covalent. LF the effective poles... ..0.0 and 0.4, THEN the bonds are nonpolar covalent, as in CH₁. ..2.1 and 1.0, THEN the bonds are ionic. And THEN.... ... are not in the same position, THEN the molecule. will be a dipole with effective charges, as in H₂O. 188 Pr 11D Anal mol ...the particles are ions with full charges in a crystal lattice, as in NaCl ... are in the same position, THEN the molecule has no molecular dipole and no effective charges. And THEN, the molecule be- haves as if it were nonpolar, as in CCL₂ And THEN, because there is no net separation of charge on the particles, the substance will be And THEN, because there is a net separation of charge on the particles, the substance will be • soluble in nonpolar solvents insoluble in polar solvents • soluble in polar solvents • insoluble in nonpolar solvents. Overall polarity of molecules determines solubility In this chapter you have focused on three types of substances: nonpolar molecules, molecular dipoles, and ionic crystals. Nonpolar molecules with either polar or nonpolar bonds carry no overall charge. When it comes to sol- ubility, the full charges of ions and the partial charges of dipoles are grouped le together because they attract each other. You can use the presence or ab- sence of charges to predict whether one chemical will dissolve in another. Chemists sometimes summarize this rule by saying "like dissolves like." • Many charged substances (ions and dipoles) will dissolve in other charged substances. (Some exceptions are described in Table 11-1 on page 410.) • A nonpolar substance will dissolve in another nonpolar substance. • A polar or charged substance will not dissolve in a nonpolar substance. These principles are summarized in the feature above, which can be used to help predict a substance's solubility. 1.Dete by nes 406
- Please Give Handwritten Answers To All Parts 1 (207.23 KiB) Viewed 38 times
- Please Give Handwritten Answers To All Parts 2 (148.74 KiB) Viewed 38 times
AN How To Predict solubility 1. Determine bond type by calculating. electronegativity difference and selecting range. 2. Indicate charges as needed on a structure of the substance. Check for dipoles if needed. 3. Identify parti- cle types and charges. Deter- mine solubility. 424 Chapter 11 IF the difference in electronegativities for bonded atome is between. 0.4 and 2.1, THEN the bonds are polar covalent. LF the effective poles... ..0.0 and 0.4, THEN the bonds are nonpolar covalent, as in CH₁. ..2.1 and 1.0, THEN the bonds are ionic. And THEN.... ... are not in the same position, THEN the molecule. will be a dipole with effective charges, as in H₂O. 188 Pr 11D Anal mol ...the particles are ions with full charges in a crystal lattice, as in NaCl ... are in the same position, THEN the molecule has no molecular dipole and no effective charges. And THEN, the molecule be- haves as if it were nonpolar, as in CCL₂ And THEN, because there is no net separation of charge on the particles, the substance will be And THEN, because there is a net separation of charge on the particles, the substance will be • soluble in nonpolar solvents insoluble in polar solvents • soluble in polar solvents • insoluble in nonpolar solvents. Overall polarity of molecules determines solubility In this chapter you have focused on three types of substances: nonpolar molecules, molecular dipoles, and ionic crystals. Nonpolar molecules with either polar or nonpolar bonds carry no overall charge. When it comes to sol- ubility, the full charges of ions and the partial charges of dipoles are grouped le together because they attract each other. You can use the presence or ab- sence of charges to predict whether one chemical will dissolve in another. Chemists sometimes summarize this rule by saying "like dissolves like." • Many charged substances (ions and dipoles) will dissolve in other charged substances. (Some exceptions are described in Table 11-1 on page 410.) • A nonpolar substance will dissolve in another nonpolar substance. • A polar or charged substance will not dissolve in a nonpolar substance. These principles are summarized in the feature above, which can be used to help predict a substance's solubility. 1.Dete by nes 406