CHEM 14C Study Guide - Midterm Guide: Atomic Orbital, Covalent Bond, Electronegativity

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tealmoose892

23 Mar 2020

School

UCLA

Department

Chemistry and Biochemistry

Course

CHEM 14C

Professor

Castillo

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Document Summary

Non - covalent forces (identify non - covalent molecular interactions and relate them to physical properties) Boiling point requires more heat energy ) stronger non - covalent - is attraction causes to disrupt - $ interactions higher. * when one or moreforces operates , strongest force dominates. London forces ( lf ) (momentarily induced dipole) Polarizability : ability to distort electron cloud. Y" electronegativity (cid:195) iv polarizability c. harder to distort e- cloud , T aofomto radius csize) (cid:195) t polarizability ( easier to distort e- cloud ) T surface area (cid:195) t stronger lf e. g - krs x vs m ( across aperiod ) (down a group ) Dipole is formed when there is an uneven sharing between atoms in covalent bond (cid:195) creation of partial -14 - charges. * hydrogen bonding (donor ) w (acceptor ) t s - x - h - - - - - - a hashrghdeotrondensitytoatrowtsttl.

Related Questions

I don't understand how to compare these forces to the around binding forces mentioned above

Phase changes always associate with change of enthalpy. For the following situations, name the phase transition and indicate whether the process is exothermic or endothermic.

. Dry ice (solid carbon dioxide) turns to gaseous carbon dioxide. Answer:

. Water vapor turns to liquid water. Answer:

. Solid iron turns to liquid iron. Answer:

. Iodine vapor turns to solid iodine. Answer:

. Liquid helium turns to helium gas. Answer:

True or false

. Intermolecular forces are stronger than ionic and covalent bonds. Answer:

. For molecules with similar size and molar mass, those with higher polarity would have higher boiling point. Answer:

. Ion-dipole forces exist between ionic potassium bromide and polar water. Answer:

. Dispersion forces exist between argon and helium. Answer:

. Instantaneous dipoles exist in all molecules and atoms. Answer:

. The strength of dispersion forces depends on the molar mass but the shape of the molecules have no effect on dispersion forces. Answer:

. Ice has a higher density than water because ice has an ordered cagelike structure. Answer:

. Liquids with weaker intermolecular interactions have lower viscosity. Answer:

. Viscosity decreases with increasing temperature. Answer:

. For any molecules, the heat of vaporization is always lower than the heat of fusion because it takes more energy to make molecules to move past one another in a solid lattice. Answer:

Which of the following accounts for the difference in phase observed at room temperature?

CHEM 14C Study Guide - Midterm Guide: Atomic Orbital, Covalent Bond, Electronegativity

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