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Worksheetsgenchem
Total questions: 86
Worksheet time: 1hrs 7mins
Explains the properties of solids and liquids in terms of intermolecular forces of attraction and the kinetic energy of the individual properties.
Kinetic molecular theory
Intermolecular forces of attraction
Intramolecular Forces on Solids
Intramolecular Liquids
Matter in gas state has _____________ shape and volume
finite
indefinite
fix
fixed
Matter in the liquid state has _________ shape and ________ volume
Definite shape and definitive volume
Indefinite shape and indefinite volume
definite shape and indefinite volume
indefinite shape and definite volume
Matter in the solid state has ________ shape and _______ volume.
indefinite and definite
definite and definite
indefinite and indefinite
definite and indefinite
All matter is made up of _______
neutron
These particles are ______ in motion.
constant
inconsistent
continuous
discrete
The speed of particle is ________ to temperature means greater speed.
are attractive forces between molecules or particles in the solid and liquid state
-Weak
Intramolecular forces
Interstellar forces
holds atom together in a molecule
-strong
Intramolecular forces
Interstellar forces
are weak attractions between nonpolar molecules.
Ion-ion forces
London Dispersion Force (Van der Waals forces)
Ion-Dipole Forces
Dipole Forces
are an interaction forces between ions with positive sides.
Ion-ion forces
London Dispersion Force (Van der Waals forces)
Ion-Dipole Forces
Dipole Forces
it acts between an ion (either positive or negative) and a polar molecules.
Ion-ion forces
London Dispersion Force (Van der Waals forces)
Ion-Dipole Forces
Dipole Forces
exists between polar molecules. One end of a dipole attracts the oppositely charged end of the
other dipole.
Ion-ion forces
London Dispersion Force (Van der Waals forces)
Ion-Dipole Forces
Dipole-Dipole Forces
a special type of dipole-dipole force that exist between a hydrogen atom bound to a small and
highly electronegative non-metal atom.
Ion-ion forces
London Dispersion Force (Van der Waals forces)
Ion-Dipole Forces
Dipole-Dipole Forces
Hydrogen Bonding
Gases consist of ____________
These particles are so small, compared with the distances between
them, that the volume (size) of the individual particles can be assumed
to be negligible _______
Iesu
zero
indefinite
large
The particles are in ________________, colliding with the walls of
the container. These collisions with the walls cause the pressure exerted
by the gas.
proportional motion
constant random motion
The particles are assumed not to _____________ each other
:3
The average kinetic energy of the gas particles is ________________
to the Kelvin temperature of the gas
Gases are tiny molecules in mostly
empty space.
Evidence:
The compressibility of gases.
Gases do not clump.
Gases mix rapidly.
Gases exert pressure that does not diminish over time.
Charles’ Law
There are no attractive forces
between molecules.
Evidence:
The compressibility of gases.
Gases do not clump.
Gases mix rapidly.
Gases exert pressure that does not diminish over time.
Charles’ Law
The molecules move in constant,
rapid, random, straight-line motion.
Evidence:
The compressibility of gases.
Gases do not clump.
Gases mix rapidly.
Gases exert pressure that does not diminish over time.
Charles’ Law
The molecules collide classically
with container walls and one another.
Evidence:
The compressibility of gases.
Gases do not clump.
Gases mix rapidly.
Gases exert pressure that does not diminish over time.
Charles’ Law
The average kinetic energy of the
molecules is proportional to the Kelvin
temperature of the sample.
Evidence:
The compressibility of gases.
Gases do not clump.
Gases mix rapidly.
Gases exert pressure that does not diminish over time.
Charles’ Law
Object at rest tends to stay at rest, and object in motion tends to stay in motion at constant
velocity unless object is acted upon by an unbalanced, external force.
Newton's First Law of Motion (Law of Inertia)
Newton’s First Law of Motion (Law of Inertia)
Inertia ∞ Mass
Motion ∞ Volume
Volume ∞ Mass
Mass ∞ Inertia
The objects involved remain separate
(a)
the objects become one mass
(a)
in Model Gas Behavior all collisions must be (a)
Particles in an ideal gas…
have no volume
have elastic collisions
are in constant, random, straight line motion
dont attract or repel each other
directly proportional
Particles in a REAL gas…
have their own volume
attract each other
at low pressures
at high temperatures
in nonpolar atoms/molecules
Gas behavior is most ideal…
have their own volume
attract each other
at low pressures
at high temperatures
in nonpolar atoms/molecules
Characteristics of Gases
Gases expand to fill any container.
Gases are fluids (like liquids).
Gases have very low densities.
Gases can be compressed.
Gases undergo diffusion & effusion.
Liquid Properties Affected by Intermolecular Forces
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
Resistance of a liquid to flow
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
It is related to the ease with which molecules can move past each other.
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
Water acts as if it has a “skin” on it due to extra inward forces on its surface.
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
The rise of liquids up narrow tubes
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
Conversion from one state of matter to another
Boiling Point / Melting Point
Viscosity
Surface Tension
Capillary Action
Phase Change
A plot of temperature vs. heat added
Heating Curve
Viscosity
Surface Tension
Capillary Action
Phase Change
Viscosity increases with stronger intermolecular forces and decreases
with _____________
Viscosity increases with stronger intermolecular forces and decreases
with _____________
Intermolecular forces that bind similar molecules to one another are called
(a)
Intermolecular forces that bind a substance to a surface are called
(a)
attract the liquid to the wall of the tube.
(a)
attract the liquid to itself.
(a)
Water has stronger adhesive forces with (a)
(a) has stronger cohesive forces with itself
is either added or released in a phase change.
(a)
energy change and change of state
three heats
(a)
Gases liquefies when pressure is applied.
(a)
The temperature beyond which a gas cannot be compressed is called
(a)
The pressure needed to compress the liquid at critical temperature
(a)
The state beyond this temperature is called
(a)
As the temperature _____, the fraction of molecules that have
enough energy to break free ________.
drop, decreases
rises, increases
drop, increases
r
As _______ molecules escape the liquid, the pressure they exert ________.
less, decreases
more, increases
more, decreases
less, increases
liquid molecules evaporate and vapor molecules condense at the same rate.
(a)
is the temperature at which its vapor pressure equals atmospheric
pressure.
(a)
is the temperature at which its vapor pressure is 760 torr.
(a)
The natural log of the vapor pressure of a liquid is inversely proportional to its temperature.
(a)
is a graph of pressure vs. temperature for a substance.
(a)
Some substances do not go directly from the
solid state to the liquid state.
(a)
molecules are only ordered in
one dimension, along the long axis.
(a)
molecules are ordered in two dimensions, along the long axis
and in layers.
(a)
nematic-like crystals are layered at angles to each other.
(a)
-is the temperature at which a solid changes into a liquid.
(a)
can be defined as the pressure at which the rate of sublimation of a solid matches the rate of deposition of its vapor phase.
(a)
-are non-crystalline solid in which the atoms and molecules are not organized in a definite lattice pattern.
(a)
-are arranged in a regular repeating pattern.
(a)
Two properties of solid
(a)
Types of solid
(a)
-consist of metal cations surrounded by a “sea” of mobile valence electrons.
(a)
two types of metallic crystals
(a)
consists of alternating positively-charged cations and negatively-charged anions
(a)
-consist of molecules at the lattice points of the crystal, held together by relatively weak intermolecular forces
(a)
-consists of atoms at the lattice points of the crystal, with each atom being covalently bonded to its nearest neighbor atoms.
(a)
-is the property shown by substances which have molecules or ions that can assume more than one stable arrangement in the solid state.
(a)
two types of solution
(a)
The substance will dissolve in a liquid
(a)
The substance will not dissolve in a liquid and formed precipitate
(a)
three types of solubility
(a)
is a mixture of two or more substances, but it’s not just any mixture. A solution is a homogeneous mixture.
(a)
two classifications of solution
(a)
are ionic compounds that dissolves to form ions in solution completely.
(a)
are the solutions that contain neutral molecules and do not dissociate into ions in solution.
(a)
three energy of solution formation
(a)
