gen chem Flashcards by Justine Clark De los Santos

Proposes that matter is made up of particles that are always in motion.

KINETIC MOLECULAR THEORY

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a special type of dipole-dipole attraction between molecules, not a covalent bond to a hydrogen atom.

Hydrogen Bond

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is an attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole

Ion-dipole Force

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Are weak interactions between atoms or molecules where no chemical reaction takes place.

NON-COVALENT BOND

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It is generated by the complete transfer of valence electrons to achieve stability.

Ionic Bond

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Ions are fundamentally surrounded by delocalized electrons, which are responsible for processes such as conductivity.

Metallic Bond

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The particles in a liquid are attracted to one another, but they are not rigidly held together so they can always still move.

DIFFUSIBILITY

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It is an indication of the escape of molecules from the surface of the liquid. It is evidence of molecular motion.

EVAPORATION

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The molecules that escape are the ones with greatest velocity. Any surface that has an evaporating liquid on it is cooler than its surroundings.

COOLING EFFECT OF EVAPORATION

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A measure of its tendency to resist flowing motion.

VISCOSITY

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High fluid liquid is said to be free-flowing, mobile or “thin”

FLUIDITY

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Is the attraction of one kind of molecule to a different kind, and it can be quite strong for water, especially with other kinds of molecules bearing positive or negative charges.

ADHESION

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Refers to the attraction of molecules to other molecules of the same kind.

COHESION

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is odorless and tasteless liquid. It has a bluish tint.

PURE WATER

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TYPES OF CRYSTALLINE SOLID

Metallic Crystals, Ionic Crystals, Molecular Crystals, Covalent Network Crystals

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Are the simplest type of structure since the single metallic atoms are the constituent units.

Metallic Crystals

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Has ions as constituent particles

Ionic Crystals

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Are those which have molecules as constituent particles as well as structure units.

Molecular Crystals

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Are giant molecules or macromolecules

Covalent Network Crystals

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Is when heat is removed or cooling a liquid decreases the kinetic energy of the particles until they are unable to move and remain in fixed positions.

FREEZING

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It is the temperature at which the liquid freezes to form the solid

FREEZING POINT

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Is the process where the particles escape and enter the vapor or gas phase above the liquid

EVAPORATION OR VAPORIZATION

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Gas to Liquid
The reverse process of evaporation
This happens as particles in the vapor phase are cooled.

CONDENSATION

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Change from solid to gas without passing the liquid state.
Reverse of Deposition

SUBLIMATION

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Change from gas to solid phase without passing the liquid phase. The reverse of sublimation

DEPOSITION

show how the temperature changes as a substance is heated up.

HEAT CURVES

show how the temperature changes as a substance is cooled down.

COOLING CURVES

is a homogeneous mixture of one or more solutes dissolved in a solvent. Where one substance is dissolved into another. Uniform all throughout which makes it homogenous

SOLUTION

degree to which a substance dissolves in a solvent to make a solution (usually expressed as grams of solute per litre of solvent).

SOLUBILITY

Is when two liquids can be mixed to form a solution

MISCIBLE

Is when two liquids cannot be mixed to form a solution

IMMISCIBLE

Types of solutions

SOLVENT, SOLUTE, TYNDALL EFFECT,

The substance that does the dissolving. Any substance, generally liquid, which is capable of dissolving one or multiple substances, which produces a solution.

SOLVENT

Substance that is dissolved in a solution. The particles of solute in a solution cannot be seen by the naked eye. A solution does not allow beams of light to scatter.

SOLUTE

also known as the Tyndall phenomenon, is the scattering of a light beam by a medium containing microscopic suspended particles

TYNDALL EFFECT

is a solution in which a solvent is capable of dissolving any more solute at a given temperature.

Unsaturated Solution

comprises a large amount of solute at a temperature wherein it will be reduced, as a result the extra solute will crystallize quickly.

Supersaturated Solution

A solution containing a relatively large amount of dissolved solute

CONCENTRATED

A solution with a relatively small amount of dissolved solute.

DILUTE

Is the weakest intermolecular force. Temporary attractive force defined as a temporary attractive force caused by the creation of temporary dipoles in a nonpolar molecule.

London Dispersion Forces

occurs when the partial charges formed within one molecule are attracted to an opposite partial charge in a nearby molecule.

Dipole-dipole Force

Occurs when pairs of electrons are shared by atoms. Atoms will covalently bond with other atoms in order to gain more stability, which is gained by forming a full electron shell.

Covalent Bond

Why does ice float on water?

Density

Is the force that causes the molecules on the surface of the liquid to “tighten their hold to one another” Creating the thin membrane on the surface. the property of the surface of a liquid that allows it to resist an external force, due to the cohesive nature of the water molecules.

SURFACE TENSION

Refers to the spontaneous rising of a liquid in a narrow tube. This action results from the cohesive forces (intermolecular forces) within the liquid and the adhesive forces between the liquid and the walls of the container.

CAPILLARY ACTION

Incapable of being compressed or condensed.

INCOMPRESSIBILITY

a measure of the tendency of a material to change into the gaseous or vapor state, and it increases with temperature.

VAPOR PRESSURE

Is the temperature at which the vapor pressure of a liquid is equal to the external pressure (atmospheric pressure above the liquid) Heat of vaporization, expressed in cal/g, kcal/g-atom, kJ/kg, is the energy required to change exactly 1 gram of liquid to vapor at its normal boiling point.

BOILING POINT

BOILING POINT degree celsius and fahrenheit

100 Celsius 212 Fahrenheit

FREEZING POINT degree celsius and fahrenheit

0 Celsius 32 Fahrenheit

State of Matter : SOLID

Structures Properties Classification

Is the temperature at which a solid melts to form a liquid

MELTING POINT

Is the amount of heat required to completely melt a solid once it has reached its melting point

HEAT OF FUSION

the change from solid to gas without passing through the liquid state

SUBLIMATION

Is the pressure exerted by the vapor when in equilibrium with the solid, at a given temperature.

VAPOR PRESSURE OF A SOLID

It is a solid in which the constituent particles such as atoms, ions, or molecules have an orderly arrangement It has regularly arranged structure units with characteristic geometric forms. Quartz, Calcite , Sugar, Mica, Diamonds, Snowflakes, Rock, Calcium fluoride, Silicon dioxide, Alum

Crystalline Solid

The constituent particles are randomly arranged Do not have sharp melting point

Amorphous Solid

Is the phase change involves a gain or absorption of heat by the substance from the environment. Examples: Evaporation of Water, Baking Bread, Frying Eggs, Photosynthesis

ENDOTHERMIC

It involves loss or release of heat by the substance to the environment Examples: Formation of Snow, Burning Candle, Burning Wood, Gas Burner in Use

EXOTHERMIC

Temperature at which the solid melts to form a liquid

MELTING POINT

Temperature at which the liquid starts to boil

BOILING POINT

Basis of Water as Solvent (Two Forms of Solutions)

Aqueous Solutions, Non- Aqueous Solutions

When a solute is dissolved in water the solution Example: salt in water, sugar in water and copper sulfate in water.

Aqueous Solutions

When a solute is dissolved in a solvent other than water Example: iodine in carbon tetrachloride, sulphur in carbon disulfide, phosphorus in ethyl alcoho

Non- Aqueous Solutions

can be defined as a solution in which a solvent is not capable of dissolving any more solute at a given temperature.

Saturated Solution

is any external solution that has the same solute concentration and water concentration compared to body fluids. In an isotonic solution, no net movement of water will take place.

Isotonic Solutions

is any external solution that has a high solute concentration and low water concentration compared to body fluids. In a hypertonic solution, the net movement of water will be out of the body and into the solution.

Hypertonic Solutions

is any external solution that has a low solute concentration and high water concentration compared to body fluids. In hypotonic solutions, there is a net movement of water from the solution into the body.

Hypotonic Solutions

three types of matter

solid, liquid, gas