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fluid
any substance that flows
when the change of state or phase change occurs…
intermolecular attractions (forces) are either breaking or forming
The strength of the intermolecular forces of the substance determines…
the amount of energy needed for the phase change
If a substance has very strong intermolecular forces
then more energy is needed to change state/phase and a higher temperature is needed for the change as well
with stronger intermolecular forces
higher melting points and higher boiling points are observed
heating and cooling curves
show the temperature changes as heat (energy) is added or removed over time.
the slopped parts of the graph occur when
a substance is only changing temperature and not changing state. Ex. solids getting warmer and gaining kinetic energy, speeding up, and spreading out
ionic compounds don’t
sublime
the pressure formed from the evaporating gas/vapor. (the pressure of gas above the liquid when liquid is sealed in a closed container)
vapor pressure
the lower the boiling point…
the easier it is to evaporate and the higher the vapor pressure.
at 1 atm
carbon dioxide sublimes and water does not
the stronger the attraction
the greater the energy needed to make/break the attraction
the stronger the intermolecular forces
the higher the melting point, the higher the boiling point, and the lower the vapor pressure (harder to evaporate)
Intermolecular forces, strongest to weakest
ion-dipole, hydrogen bonding, dipole-dipole, ion-induced dipole, dipole-induced dipole, induced dipole-induced dipole
an ion-dipole interaction is formed when
a cation or anion is attracted to the partial positive or partial negative of a polar molecule. these often form as a result of an ionic compound dissociating/dissolving in water
a dipole-induced dipole interaction is formed when
the partial positive or partial negative of a polar molecule causes the electron cloud of a nonpolar molecule to distort and creates a temporary induced dipole in the nonpolar molecule
an ion-induced dipole if formed when
a cation or anion causes the electron cloud of nonpolar molecule to distort and creates a temporary induced dipole in the nonpolar molecule
the mass of the atoms or molecules impacts the strength of the induced dipoles. the more electrons an atom or molecule the more those electrons…
can move in the cloud and generate less temporary/stronger induced dipoles and stronger interactions
solubility
how much of a given substance dissolves in another substance at a given temperature and can also be described as MIXING
The rule for dissolving
LIKE dissolves LIKE
CHARGES dissolves CHARGES
POLAR dissolves POLAR / NONPOLAR dissolves NONPOLAR
IMF dissolves IMF
the tension on the surface of the water drop is known as
surface tension
a surfactant
a substance that reduces surface tension and increases wetting
any dissolving medium is called the
solvent
the dissolved particles are called the
solute
solvation
the process of ion capture by the solvent
aqueous solution
defined as a solution where water IS the solvent
Soluble
has the ABILITY to dissolve
Electrolytes are
metals and nonmetals - ions
nonelectrolytes are
nonmetals and nonmetals - covalent compounds
dissociation
the separation of ions that occurs when an ionic compound dissolves and involves aquious solutions
Anhydrous
a substance that contains no water or water has been removed
4 factors determine how quickly something dissolves
the identity of the solute (the identity tells you about the properties of substance like bonding, intermolecular forces, solubility, ect.
changing the temperature
agitating (stirring, shaking, mixing)
changing the surface area (breaking up chunks, crushing, grinding, spreading solute by adding slowly)
solution
homogeneous mixtures with uniform appearance and composition - transparent and doesn’t separate
colloid
heterogenous mixture containing particles, called the dispersed phase, that are spread throughout the substance - cloudy and doesn’t separate
suspension
a heterogeneous mixture from which particles settle upon standing - can be separated and is also cloudy
brownian motion
the random motion of particles due to the collisions of rapidly moving particles
tyndall effect
the scattering of light by particles in a mixture that are of a certain size
as gas solubility goes up
so does the pressure, with the opposite also being true
precipitate
a solid that forms from a chemical reaction
when OH- (hydroxide) is on one side of the balencing equations
use hoh
when determining if it can actually happen with single replacement
use the activity series
the more reactive metals in the actvity series are towards the top
and the least reactive are below that, then the halogns
a reactive metal will replace any metals
below it
the net ion equation
an equation for a reaction in solution that shows only those particles hat are directly involved in the chemical change
alkali metals and what do they mean for solubility
Li, Na, K, Rb, Cs, Fr - these and the ammonium ion (NH4+) are generally soluble, as well as the acetate ion, nitrate ions and the sulfate ion
halide ions
F-, Cl-, B-, I-
generally insoluble ions include
carbonate ion, chromate ion, phosphate ion. sulfide ion (S-2), and the hydroxide rule
Note 
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