Untitled Flashcards Set

Main similarity, the bonds occur to satisfy the octet or fulfill its outer shell.
Ionic bonds = metals (cation) giving up valence electrons to non-metal (anion) which
receives the valence electrons.
Covalent bonds = non-metals (anions) bonding with each other by sharing valence
electrons
Metallic bonds = metals (cations) attracted to delocalized valence electrons which are
shared in a sea of electrons by the surrounding metal atoms.
2. Properties of Ionic Compounds = forms crystal lattices, hard, brittle, conducts electricity
when it dissolves in water, high melting and boiling points.
3. Properties of Covalent Compounds = forms crystal structures but not uniform, does not
conducts electricity if dissolved, low melting and boiling points, soft when it’s a solid,
flammable.
4. Properties of Metallic compounds = durable, ductile, malleable, conducts electricity and
heat, moderate to high melting and boiling points.
5. Synthesis, Decomposition, Combustion, Single and Double Replacement
6. Lattice Energy = the energy required to break an ionic bond.
Bond Dissociation = the energy required to break a covalent bond.
7. Single bond = requires 2 VE, long in length, weak in strength, sigma.
Double bond = requires 4 VE, medium in length and strength, one sigma, one pi.
Triple bond = requires 6 VE, short in length, strongest in strength, one sigma, two pi.
8. Polar Covalent = unequal sharing of valence electrons.
Non-Polar Covalent = equal sharing valence electrons.
9. London dispersion force is the weakest intermolecular force. The London dispersion
force is a temporary attractive force that results when the electrons in two adjacent
atoms occupy positions that make the atoms form temporary dipoles. This force is
sometimes called an induced dipole-induced dipole attraction.
Dipole-Dipole Forces. Dipole-dipole forces are attractive forces between the positive
end of one polar molecule and the negative end of another polar molecule.
A hydrogen bond is the attractive force between the hydrogen attached to an
electronegative atom of one molecule and an electronegative atom of a different
molecule. Usually the electronegative atom is oxygen, nitrogen, or fluorine, which has a
partial negative charge.