Unit 14 Vocab Flashcards
crystalline solids
Solids characterized by the regular arrangement of their components ex- salt, diamonds
ionic solids
Solids containing cations and anions that dissolve in water to give a solution containing the separated ions, which are mobile and thus free to CONDUCT an electric current
Held together by the strong forces that exist between oppositely charged ions. (PACKED)
HIGH melting pts.
molecular solids
(EX ice) Solids composed of small molecules
DO NOT conduct electricity when dissolved in water
LOW melting pts
intermolecular forces- weak.
dipole moment, dipole–dipole forces hold the solid together
nonpolar molecules- London dispersion forces hold the solid together.
Notice how covalent bonds and closer tg than the London dispersion in image
atomic solids
Solids that contain atoms at the lattice points (Only contain one type of atom, ex diamonds)
vary greatly different between each, b/c of how they can interact w each other
“a solid is classified as a molecular solid only if (like ice, dry ice, sulfur, and phosphorus) it contains small molecules. Substances like diamond that contain giant molecules are called network solids.”
what all the “solids” look like
In image
Bonding in metals
malleable, ductile, conducto, strong, high melting pts,
bonding in most metals is strong but nondirectional.
electron sea model
A model for metals postulating a regular array of cations in a “sea” of electrons
“all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electron:
alloy
A substance that contains a mixture of elements and has metallic properties
2 types
substitutional alloy
An alloy formed when some metal atoms are replaced by other metal atoms of similar size ex-brass
interstitial alloy
An alloy formed when some interstices (holes) in a metal lattice are occupied by smaller atoms
normal boiling point
The temperature at which the vapor pressure of a liquid is exactly one atmosphere; the boiling temperature under one atmosphere of pressure
heating/cooling curve
A plot of temperature versus time for a substance, where energy is added at a constant rate
normal freezing point
The melting/freezing point of a solid at a total pressure of one atmosphere
intramolecular forces
Interactions that occur within a given molecule
intermolecular forces
Relatively weak interactions that occur between molecules
molar heat of fusion
The energy required to melt 1 mole of a solid
molar heat of vaporization
The energy required to vaporize 1 mole of a solid
hydrogen bonding
Unusually strong dipole-dipole attractions that occur among molecules in which hydrogen is bonded to a highly electronegative atom
London dispersion forces
The relatively weak forces, which exist among noble gas atoms and nonpolar molecules that involve an accidental dipole that induces a momentary dipole in a neighbor
dipole–dipole attraction
The attractive force resulting when polar molecules line up such that the positive and negative ends are close to each other
vaporization/evaporation
The process in which a liquid is converted to a gas (vapor)
Differences between the types of solids
Ionic solids consist of oppositely charged ions packed together, molecular solids contain molecules, and atomic solids have atoms as their fundamental particles.
condensation
The process by which vapor molecules re-form a liquid
vapor pressure
The pressure of the vapor over a liquid at equilibrium in a closed container
