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VSEPR, intermolecular forces, and intramolecular forces

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Section 1

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INTERmolecular forces

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6 years ago

Date created

Mar 1, 2020

Cards (14)

Section 1

(14 cards)

INTERmolecular forces

Front

forces of attraction between separate molecules -weaker than intramolecular forces -when broken/formed a physical phase change occurs

Back

hydrogen bonding forces

Front

a strong interaction between a partial positive h atom and a partial negative FON atom IN ANOTHER MOLECULE

Back

effect of lone pairs on shape and angles of molecule

Front

lone pairs repel other electrons pairs more strongly which compresses the angles between bonding pairs

Back

steric number

Front

# of lone pairs on central atom + number of atoms bonded to central atom

Back

H20, HF, and NH3

Front

have significantly higher boiling points because they have a much stronger attraction which means it requires more energy to break

Back

bonding electrons vs lone pairs

Front

lone electron pairs influence the shape in a similar manner as bonded electron pairs

Back

compound that exhibits hydrogen bonding

Front

water

Back

compound that exhibits only London dispersion forces

Front

carbon dioxide and methane

Back

INTRAmolecular forces

Front

very strong forces between atoms of a SINGLE molecule -include ionic, covalent and metallic bonds -when broken, a chemical change occurs

Back

what defines a molecule as polar?

Front

an uneven distribution of charge (based on electronegativity differences between bonded atoms and the 3-D interaction of ALL the bonds)

Back

compound that exhibits dipole-dipole attraction

Front

hydrogen Chloride (HCl)

Back

dipole-dipole forces

Front

occur between polar molecules -partially positive end of a polar molecule is attracted to the partially negative end of another polar molecule -only exist between nearby molecules -more polar = stronger force and higher boiling/melting points because it takes more energy to break IMFs

Back

London dispersion forces

Front

form between all molecules and the only force acting upon nonpolar molecules -temporary partial charges are developed because electrons are constantly in motion -these tiny instantaneous differences cause attractions between nonpolar molecules -strength in dispersion forces = higher molecular weight

Back

VSEPR theory

Front

Valence-shell electron-pair repulsion theory; because electron pairs repel, molecules adjust their shapes so that valence electron pairs are as far apart as possible

Back