REVIEWER FOR 1ST QUARTER EXAM (GC2) Flashcards
explains the properties of liquids in term of the intermolecular forces of attraction and the kinetic energy of the individual particles
KINETIC MOLECULAR MODEL
refers to attractive forces between particles, it pull the particles together
INTERMOLECULAR FORCES
keep the particles at a distance and/or moving around
KINETIC ENERGY
PROPERTIES OF SOLID
- Have definite shape and volume
- Do not flow
- Virtually incompressible
- Expand when heated but to a lesser extent
PARTICLES OF SOLIDS
- Strongly attached to each other
- Vibrate in fixed positions
- Vibrate faster when heated
PROPERTIES OF LIQUID
- Have definite volume but no definite shape
- Flow and take the shape of its container
- Very difficult to compress
- Slightly expand when heated
PARTICLES OF LIQUIDS
- Weakly attached to each other; break their interaction easily
- Move more freely that those in solids
- Move faster when heated
Giving/taking electron, formula unit, force of attraction between two opposite charges (ions), keep the compound solid at room temperature
Ionic bond
sharing electrons, weaker only involves partial charges, molecules
Covalent Bond
Intermolecular Forces of Attraction in a pure substance include…
- DIPOLE-DIPOLE FORCES
- HYDROGEN BONDING
- ION-DIPOLE
- LONDON DISPERSION FORCES
Dipole-dipole and London dispersion forces are collectively known as
VAN DER WAALS FORCE
exists between two polar molecules or a molecule in which one end of the molecule is slightly positive, while the other end is slightly negative
DIPOLE-DIPOLE FORCES
A special type of dipole-dipole interaction that exist only in molecules that contain H atom bonded to a small, highly electronegative atom such as N, O, or F
HYDROGEN BONDING
Acts between an ion (either positive or negative) and a polar molecule. The degree of this interaction depends on the a size and charge of the ion and on the size and dipole moment of the polar molecules; Cations (positively charged ions) interact more strongly with dipoles than anions (negatively charged ions)
ION-DIPOLE FORCES
The weakest IMF or simply dispersion forces are attraction that exist between all atoms and molecules
LONDON DISPERSION FORCES
The ease when they move within the atom is called?
Polarization
GENERAL PROPERTIES OF LIQUIDS
- SURFACE TENSION
- VISCOSITY
- VAPOR PRESSURE
- BOILING POINT
- HEAT VAPORIZATION
It is the property of a liquid to resist an external force and thus assume a lesser surface area.
This attributed to the strong attractive and cohesive forces between and among the molecules, particularly at the surface of the liquid.
SURFACE TENSION
This is the resistance of a liquid to flow. It is loosely referred to as the thickness and thinness of a liquid.
The greater the intermolecular forces, the more viscous the substance
Example: Oil and honey
VISCOSITY
the pressure exerted by its vapor when in equilibrium wit its liquid or solid. This means that when a solid substance is made to evaporate in a close container, the gas exerts a pressure above the liquid.
Substances with relatively strong IMF will have low vapor pressure because the particles will have difficulty escaping as a gas.
VAPOR PRESSURE
temperature at which its vapor pressure is equal to the external atmospheric pressure. It is also influenced by the strength of its IMF. The greater the attractive forces, the higher the energy needed to increase the kinetic energy of the molecules to break these forces
BOILING POINT
The temperature at which a liquid boils under an ______ of ________ is referred to as its normal boiling point
atmospheric pressure, of 760 mmHg (1 atm)
The normal boiling point of water is ?
100 degree Celsius
the amount of heat required to vaporize one mole of a substance at its boiling point.
The application of heat disrupts the intermolecular forces of attraction of the liquid molecules and allow them to vaporize.
MOLAR HEAT OF VAPORIZATION
