NATS 1870 Lecture Notes - Lecture 8: Ph Indicator, Hydronium, Chemical Polarity

• School: York University
• Department: Natural Science
• Course: NATS 1870
• Professor: Robin Kingsburgh

Document Summary

Recall: bonds: ionic o(cid:374)e ato(cid:373) do(cid:374)ates its e(cid:859) to a(cid:374)othe(cid:396) Fully shared: non-polar: h2: h-h: equally sharing between h-atoms. Partially shared: polar: h20o o- h h: o att(cid:396)a(cid:272)ti(cid:448)e e(cid:859) slightly (cid:373)o(cid:396)e tha(cid:374) h. Fact that water h2o has polar bond many substances can dissolve n it: example of acidic solution: hydrochloric acid, h2o + hci ------------------------ h3o + ci- Hydrochloric acid hydronium responsible for acidic characteristics. H+ or proton becomes disassociated + attracted to h2o negative o end of molecule. The concentration of hydronium (h3o+) in a solution measures the acidity of that solution: high h30+ concentration ---very acidic. An acid can be considered a proton donor or electron acceptors (cid:858) Form chemical bonds with material (paper, fabric) become physically attached to material. Colour: arises from selective absorption by the dye molecules remaining wavelengths are reflected to eye by underlying material. Pai(cid:374)e(cid:396)s a(cid:396)e suspe(cid:374)ded i(cid:374) a (cid:862)(cid:373)ediu(cid:373)(cid:863) (cid:894)oil, a(cid:272)(cid:396)yli(cid:272) poly(cid:373)e(cid:396)s(cid:895)