GEN CHEM 3rd Quarter

Covalent bond

________- one or more pairs of electron are shared by two atoms.

KMT

________- model word to explain the behavior used of matter.

Johannes Van Der Waals

________ (1837- 1923)- working on the theory of ideal gases of close recognized the existence of some type of weak force or particles that are very close to each other.

Viscosity

________- measure of fluid resistance to flow.

Effusion

________- process in which gas through a small hole in its current container into another container.

Phase diagrams

\- are plots of pressure (usually in atmospheres) versus temperature (usually in degrees celcius or Kelvin)

Supercritical fluid

________- Beyond the temperature of the critical point, the merged single phase.

IMF

________- molecules interact and have a great influence on one another.

1atm

Boiling Point- the boiling point of a liquid when the external pressure is ________ is called the normal boiling point.

Sublimation (or deposition) curve

________ - The curve on a phase diagram which represents the transition between the gaseous and solid states.

Fluid

________- gas or a liquid, a substance that can flow.

Vaporization

________- change of phase from liquid to vapor (gaseous phase)

Capillary Action

________- tendency of a liquior to rise in narrow tubes or to be drawn into small openings.

Ethyl Alcohol

________- water have very low vapor pressures, both liquid have the strong dipole- dipole interaction called hydrogen bonding.

Pentane

________- nonpolar substance, and its vapor pressure is high compared to those of water and ethyl alcohol.

Phase diagram

________ - is a graphical representation of the physical states of a substance under different conditions of temperature and pressure.

Network solid or covalent

\- ________ crystal solid that may be a chemical compound in which atom are bonded by covalent bond.

Diffusion

________- process which a gas, enters a container w /another gas and two mix to form a uniform mixture.

Vapor

________- gaseous substance that exist naturally as a liquid or solid of normal temperature.

Normal melting

________ and boiling points- Melting and boiling points when the pressure is 1 atm.

Green line

________- divides the solid and liquid phases, and represents melting (solid to liquid) and freezing (liquid to solid) points.

Electrostatic bonding

________ - attraction between oppositively charged ions in a chemical compound.

Melting (or freezing) curve

\- The curve on a phase diagram which represents the transition between the liquid and solid states.

Super Saturated

________- more than the maximum amount of salute.

Molecular Crystal

________- solid composed of molecules held together by Vander Waals forces.

Blue line

________- divides the liquid and gas phases, and represents vaporization (liquid to gas) and condensation.

Intramolecular forces

________- forces that holds atoms together in a molecule.

Saturated Solution

\- there is maximum amount of solute that can be dissolved in a given amount of solvent in a given temperature.

Vaporization (or condensation) curve

________ - The curve on a phase diagram which represents the transition between the gaseous and liquid states.

Phase

________- homogenous part of a system in contact w /other parts of the system.

Melting (or freezing) curve

The curve on a phase diagram which represents the transition between the liquid and solid states

Vaporization (or condensation) curve

The curve on a phase diagram which represents the transition between the gaseous and liquid states

Sublimation (or deposition) curve

The curve on a phase diagram which represents the transition between the gaseous and solid states

Triple point

The point on a phase diagram at which the three states of matter coexist, combination of pressure and temperature at which all three phases of matter are at equilibrium

Critical point

The point in temperature and pressure on a phase diagram where the liquid and gaseous phases of a substance merge together into a single phase

critical temperature and critical pressure

The temperature and pressure corresponding to the critical point

Normal melting and boiling points

Melting and boiling points when the pressure is 1 atm

Liquefied petroleum gas or liquid petroleum gas (LPG or LP gas)

also referred to as simply propane or butane, are flammable mixtures of hydrocarbon gases used as fuel in heating appliances, cooking equipment, and vehicles

phase diagram

is a graphical representation of the physical states of a substance under different conditions of temperature and pressure

Phase diagrams

are plots of pressure (usually in atmospheres) versus temperature (usually in degrees Celsius or Kelvin)

green line

divides the solid and liquid phases, and represents melting (solid to liquid) and freezing (liquid to solid) points

blue line

divides the liquid and gas phases, and represents vaporization (liquid to gas) and condensation

red line

divides the solid and gas phases, and represents sublimation (solid to gas) and deposition

supercritical fluid

Beyond the temperature of the critical point, the merged single phase

Phase

homogenous part of a system in contact w/ other parts of the system

Intramolecular forces

forces that holds atoms together in a molecule

Intermolecular forces

attractive forces between molecule

Diffusion

process which a gas, enters a container w/ another gas and two mix to form a uniform mixture

Effusion

process in which gas through a small hole in its current container into another container

KMT

model word to explain the behavior used of matter

Johannes Van Der Waals (1837-1923)

working on the theory of ideal gases of close recognized the existence of some type of weak force or particles that are very close to each other

IMF

molecules interact and have a great influence on one another

Fluid

gas or a liquid, a substance that can flow

Surface

measure of the elastic force in the surface of a liquid, amount of energy required to Stretch or increase the surface of a liquid by a unit area,

Capillary Action

tendency of a liquior to rise in narrow tubes or to be drawn into small openings

Viscosity

measure of fluid resistance to flow

Vapor

gaseous substance that exist naturally as a liquid or solid of normal temperature

Vaporization

change of phase from liquid to vapor (gaseous phase)

vapor pressure of a liquid

equilibrium pressure of vapor above its liquid, pressure exerted by the vapor above the surface of the liquid in a closed temperature

Boiling Point

the boiling point of a liquid when the external pressure is 1atm is called the normal boiling point

Molar Heat of Vaporization (AH Vap)

energy required to vaporize, 1 mole of a liquid at given temperature

Ethyl Alcohol

water have very low vapor pressures, both liquid have the strong dipole-dipole interaction called hydrogen bonding

Acetone

popular but does not have H-bonding, it's vapor pressure is of Intermediate value

Pentane

nonpolar substance, and its vapor pressure is high compared to those of water and ethyl alcohol

Crystal or crystalline solid

solid material whose components, such as atom molecules or ions

Ion

atom or group of atoms that has a net positive or negative charge

ionic Crystal

solid that consists of positively and negatively charge ion held together by electrostatic forces

Electrostatic bonding

attraction between oppositively charged ions in a chemical compound

Ionic bond

electrostatic force that hold ions together in an ionic compound

Network solid or covalent

network crystal solid that may be a chemical compound in which atom are bonded by covalent bond

Molecular Crystal

solid composed of molecules held together by Vander Waals forces

Covalent bond

one or more pairs of electron are shared by two atoms

Nature of solute and Solvent

general rule of solutions -like dissolve like"

Polar liquids

dissolve polar compound and nonpolar liquids dissolve nonpolar compounds

Polar Compound

compound either ionic or Covalent, that have a permanent dipole moment

Nonpolar Compound

covalent compound have no permanent dipole moment

Saturated Solution

there is maximum amount of solute that can be dissolved in a given amount of solvent in a given temperature

Super Saturated

more than the maximum amount of salute

Unsaturated

less than maximum amount of solute

percent by mass

(mass of solute/mass of solution) x 100

percent by volume

(volume of solute/volume of solution) x 100

percent by mass/volume

(mass of solute/100 of solution) x 100

parts per million/ppm

(mass of solute/mass of solution) x 1mil

parts per billion/pbb

mg of solute/L of solution

\

moles of solute/moles of solution

mole fraction(solvent)

moles of solvent/moles of solution

Molarity/M

moles of solute/L of solution

molality/m

**moles of solute/kg of solvent**

normality/X

no. of equivalent solute/L of solutions

Osmotic pressure

a certain pressure exerted on the solution which can stop osmosis. just

Raoult's law

the partial pressure of a solvent over a solution is given by the vapor pressure of the pure solvent, multiplied by the mole fraction of the solvent in the solution