Forces.

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Presentation transcript:

Forces

Types of Bonds

Intramolecular Bonding __________ - metal + non metal __________ - non metal + non metal __________ - metal + metal

Intermolecular Intermolecular bonds – Bonding __________ Network Covalent bonding Ionic bonding Metallic bonding Hydrogen bonding Dipole – Dipole bonding London Dispersion forces

Network Covalent Continuous network of covalent bonds Examples: quarts, diamond, graphite, SiO2 Extremely __________ melting points Generally __________ in all solvents __________ conductors of electricity

Ionic Strong bonds due to __________ forces __________ melting points Good conductors of electricity when __________ or in __________ Usually soluble in __________ or __________ solvents

Metallic __________ of valence electrons __________ melting points Electrons free to move around __________ conductor of electricity

Hydrogen bonding Occurs when H is bonded to _____, _____, or _____ They are VERY strong leading to High boiling points Viscous

Polarity In order for a substance to be polar, the bonds within the molecule must carry different charges and cannot cancel out due to symmetry

Polar or non polar CHF3 CO2 BCl3 CH4 H2O

Rule for solubility __________ dissolves __________ Polar will dissolve in polar Non polar will dissolve in non polar

Van der Waals Forces Dipole – Dipole Dipole - partial __________ & a partial __________ charges at one end The partial positive and partial negative will __________ These attractions are called dipole - dipole attractions These come from polar molecules ONLY!!!

London Dispersion forces Small electrostatic forces caused by the __________ of the electron in molecules In all molecules More electrons  stronger LDF because more polarizable

What type of intermolecular forces are present? HCl HF CaCl2 CH4 CO NaNO3

Which will have the … Highest boiling point… HBr, Kr, Cl2 Highest freezing point…H2O, NaCl, HF Lowest freezing point…N2, CO, CO2 Lowest boiling point…CH4, CH3CH3, CH3CH2CH3 Highest boiling point…HF, HCl, HBr

More examples At 25C ONF is a gas where H2O is a liquid. Why? At 25C Br2 is a liquid when Cl2 is a liquid. Why?