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gen chem Flashcards

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1
Q

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

A

KINETIC MOLECULAR THEORY

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2
Q

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

A

Hydrogen Bond

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3
Q

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

A

Ion-dipole Force

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4
Q

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

A

NON-COVALENT BOND

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5
Q

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

A

Ionic Bond

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6
Q

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

A

Metallic Bond

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7
Q

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

A

DIFFUSIBILITY

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8
Q

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

A

EVAPORATION

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9
Q

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

A

COOLING EFFECT OF EVAPORATION

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10
Q

A measure of its tendency to resist flowing motion.

A

VISCOSITY

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11
Q

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

A

FLUIDITY

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12
Q

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.

A

ADHESION

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13
Q

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

A

COHESION

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14
Q

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

A

PURE WATER

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15
Q

TYPES OF CRYSTALLINE SOLID

A

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

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16
Q

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

A

Metallic Crystals

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17
Q

Has ions as constituent particles

A

Ionic Crystals

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18
Q

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

A

Molecular Crystals

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19
Q

Are giant molecules or macromolecules

A

Covalent Network Crystals

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20
Q

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.

A

FREEZING

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21
Q

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

A

FREEZING POINT

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22
Q

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

A

EVAPORATION OR VAPORIZATION

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23
Q

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

A

CONDENSATION

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24
Q

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

A

SUBLIMATION

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25
Q

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

A

DEPOSITION

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26
Q

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

A

HEAT CURVES

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27
Q

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

A

COOLING CURVES

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28
Q

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

A

SOLUTION

29
Q

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

A

SOLUBILITY

30
Q

Is when two liquids can be mixed to form a solution

A

MISCIBLE

31
Q

Is when two liquids cannot be mixed to form a solution

A

IMMISCIBLE

32
Q

Types of solutions

A

SOLVENT, SOLUTE, TYNDALL EFFECT,

33
Q

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

A

SOLVENT

34
Q

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.

A

SOLUTE

35
Q

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

A

TYNDALL EFFECT

36
Q

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

A

Unsaturated Solution

37
Q

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

A

Supersaturated Solution

38
Q

A solution containing a relatively large amount of dissolved solute

A

CONCENTRATED

39
Q

A solution with a relatively small amount of dissolved solute.

A

DILUTE

40
Q

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.

A

London Dispersion Forces

41
Q

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

A

Dipole-dipole Force

42
Q

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.

A

Covalent Bond

43
Q

Why does ice float on water?

A

Density

44
Q

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.

A

SURFACE TENSION

45
Q

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.

A

CAPILLARY ACTION

46
Q

Incapable of being compressed or condensed.

A

INCOMPRESSIBILITY

47
Q

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

A

VAPOR PRESSURE

48
Q

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.

A

BOILING POINT

49
Q

BOILING POINT
degree celsius and fahrenheit

A

100 Celsius
212 Fahrenheit

50
Q

FREEZING POINT degree celsius and fahrenheit

A

0 Celsius
32 Fahrenheit

51
Q

State of Matter : SOLID

A

Structures
Properties
Classification

52
Q

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

A

MELTING POINT

53
Q

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

A

HEAT OF FUSION

54
Q

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

A

SUBLIMATION

55
Q

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

A

VAPOR PRESSURE OF A SOLID

56
Q

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

A

Crystalline Solid

57
Q

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

A

Amorphous Solid

58
Q

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

A

ENDOTHERMIC

59
Q

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

A

EXOTHERMIC

60
Q

Temperature at which the solid melts to form a liquid

A

MELTING POINT

61
Q

Temperature at which the liquid starts to boil

A

BOILING POINT

62
Q

Basis of Water as Solvent (Two Forms of Solutions)

A

Aqueous Solutions, Non- Aqueous Solutions

63
Q

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

A

Aqueous Solutions

64
Q

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

A

Non- Aqueous Solutions

65
Q

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

A

Saturated Solution

66
Q

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.

A

Isotonic Solutions

67
Q

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.

A

Hypertonic Solutions

68
Q

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.

A

Hypotonic Solutions

69
Q

three types of matter

A

solid, liquid, gas

gen chem (2 decks)

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