CHEM (II) First Quiz

Liquids

These are made up of particles that are close to each other and have kinetic energy.

Surface Tension, Capillary Action, Viscosity, Vapor Pressure, Molar Heat of Vaporization, Boiling Point

6 Physical Properties of Liquids

Surface Tension

it is the measure of the elastic force in the surface of a liquid. It is the property of the surface of a liquid that allows it to resist an external force, due to the cohesive nature of its molecules.

intermolecular force of attraction

The strength of surface tension depends on the\________

greater force

If the intermolecular force of attraction of a liquid
is strong, then there is a \______________ needed to
break through the surface, resulting to greater
surface tension.

hydrogen bond

Water has a high surface tension because of its
ability to form a \_______.

Surface Tension

The molecules look like thin elastic membrane of
slightly denser molecules. The geometry of the
legs of the water strider allows the insect to cross
the water without sinking.

Capillary Action

It is the tendency of a liquid to rise in narrow tubes or be drawn into small openings such as those between grains of a rock. Capillary action, also known as capillarity, is a result of intermolecular attraction between the liquid and solid materials.

Cohesion

it is the intermolecular attraction between like molecules (the liquid molecules).

Adhesion

It is an attraction between unlike molecules (such as those in water and in the particles that make up the glass tube).

Viscosity

It is the resistance of fluids to flow. In layman's term, it is defined as the measure of the thickness of a liquid.

slower

The greater the viscosity, the \________ the liquid flows.

Viscosity

It is expressed in units of centipoise (cP), also known as stoke. It is a metric system unit. The SI unit is Pascal-second (Pa-s) or Newton?second/meter2 (N-s/m2). 1 centipoise \= 0.001 Pa-s

inversely proportional

How does temperature affect the viscosities of substances? because Viscosity and temperature are i\_____________ with each other.

Viscosity

An increase in temperature causes kinetic energy to increase. Heat breaks the intermolecular forces causing the liquid molecules to move faster.

Vapor Pressure

It is the pressure at which a liquid and its vapor are in equilibrium at a given temperature.

volatile liquids

alcohol, gasoline, paint thinner and dry-cleaning solvents are what type of liquids

Vapor Pressure

It is the point at which equilibrium pressure is reached, in a closed container, between molecules leaving the liquid and going into the gaseous phase and molecules leaving the gaseous phase and entering the liquid phase.

lower

The stronger the intermolecular forces of attraction, the \______ the vapor pressure of a liquid.

Molar Heat of Vaporization

The relationship between vapor pressure and the strength of intermolecular forces is consistent with the trends in two other properties of liquids, the enthalpy or molar heat of vaporization, and the boiling point of the liquid.

Molar Heat of Vaporization

It is the energy required to vaporize 1 mole of a liquid at a given temperature. H is the symbol for enthalpy, which means heat content at a given standard condition.

Boiling Point

It is the temperature at which the liquid converts into a gas. A liquid boils when its vapor pressure equals the pressure acting on the surface of the liquid. The boiling point is the temperature at which the vapor pressure of a liquid is equal to the external pressure.

external pressure

The boiling point of a liquid depends on the \_________

100

The normal boiling point of water is \______ degrees Celsius.

Solids

They have fixed volume and fixed shape (regardless of size and shape of the container), high density, cannot be appreciably compressed, and their molecules vibrate in place.

Amorphous Solid

These are solids, like glass, that are formed rather rapidly that its constituent particles do not have time to align or organize into a more definite crystalline lattice.

Amorphous Solids, Crystalline Solids

Classes of Solids

Amorphous Solid

A type of solid who have Irregular Shapes?

Amorphous Solid

This solid do not have sharp melting points, instead they soften first and melt little by little over a wide temperature range.

Amorphous Solid

This solid (example: glass), like liquids, have short range order of regular shaped pattern of arrangement of constituent particles.

Amorphous Solid

A type of Solid that are pseudo or super cooled liquids.

Amorphous Solid

A type of solid that are isotropic in nature and do not have definite heat of fusion.

Crystalline Solid

Solid whose particles are arranged in regular geometric patterns. The representative particles exist in a highly ordered and repetitive pattern. This arrangement produces a beautiful regularly shaped crystal.

Ice, Sodium Chloride, Copper Sulfate, Diamond, Graphite, Sugar, Sand.

Example of Crystalline Solid?

Crystal lattices

These are structure of crystalline solids that are built from repeating units

Crystalline Solid

A type of solid who has a definite characteristic geometric shape

Crystalline Solid

A type of Solid who has sharp melting points and have a definite heat fusion.

Crystalline Solid

A type of Solid who has a long range order of regular pattern of arrangement of constituent particles.

Crystalline Solid

A type of solid where it is considered as true solids and they are anisotropic in nature.

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

4 Types of Crystalline Solids

Metallic Crystals

These are made of atoms that are readily lose electrons to form positive ions (cations), but no atoms in the crystal would readily gain electrons to the whole crystal, creating a structure made up of an orderly arrangement of cations surrounded by delocalized electrons that move around the crystal.

Ionic Crystals

These crystals have ions as constituents particles meaning they are made of ions (Cation and anions). These ions form strong electrostatic interactions that hold the crystal lattice together.

Molecular Crystals

These crystals are those which have molecules as constituent particles as well as structure units. The molecules present in the crystal are held by weak van der Waals forces of attraction.

Covalent Network Crystals

These are giant molecules of macromolecules which consist of very large numbers of atoms linked by a network of covalent bonds.

Asbestos, Mica, Graphite

Example of Covalent Network Crystals

Covalent network crystals

The Atoms in these solids are held together by a network of covalent bonds. To break or to melt a CNS, covalent bonds must be broken.

intramolecular forces

a type of forces holds atoms together in a molecule and forces stabilize individual molecules.

Intermolecular forces

a type of forces that are attractive forces between molecules.

Ionic bond, Covalent bond

What are the two types of Intramolecular Forces?

Ionic bond

it is formed by the complete transfer of valence electron(s) between atoms.

Covalent bond

It is formed between atoms that have similar electronegativities—the affinity or desire for electrons.

polar covalent bond, nonpolar covalent bond

What are the 2 types of covalent bond?

nonpolar covalent bond

a type of bond that is formed between the same atoms or atoms with very similar electronegativities.

polar covalent bond

a type of bond that is formed when atoms of slightly different electronegativities share electrons.

covalent bond

What is the intramolecular force of attraction that forms when atoms share electron?

Ionic bond

What is the intramolecular force of attraction that generates two opposite-charged ions?

polar covalent bond

What kind of covalent bond is formed when atoms of slightly different electronegativities share electrons?

nonpolar covalent bond

What kind of covalent bond is formed between atoms or atoms with very similar electronegativities?

Intermolecular forces

These forces are much weaker than the intramolecular forces of attraction but are important because they determine the physical properties of molecules like their boiling point, melting point, density, and enthalpies of fusion and vaporization.

Van der Waals forces

forces that are electrical in nature; that is, they result in the attraction between centers of opposite charge in two molecules close to each other.

dipole-dipole, hydrogen bond, ion-dipole, london dispersion

Types of Intermolecular Forces

dipole-dipole forces

forces that are attractive forces between the positive end of one polar molecule and the negative end of another polar molecule.

ion-dipole

it is an attractive force that results from the electrostatic attraction between an ion and a neutral molecule that has a dipole. It is most commonly found in solutions(water)(solution or solvent).

Hydrogen Bonding

This is a special kind of dipole- dipole interaction that occurs specifically between a hydrogen atom bonded to either an oxygen, nitrogen, or fluorine atom.

London Dispersion Forces

These are the weakest of the intermolecular forces and exist between all types of molecules, whether ionic or covalent— polar or nonpolar. The more electrons a molecule has, the stronger the London dispersion forces are.(pataasan ng atomic number sa periodic table).

Ion-dipole, hydrogen bonding, dipole-dipole, london dispersion

arrangement of intermolecular forces from strongest to weakest.

Dipole-dipole

What is the attractive force that exist between the positive end of one polar molecule and the negative end of another polar molecule?

Ion-dipole

It is an attractive force that is commonly found in solutions, especially ionic compounds in polar liquids?

C

Which of the following compounds will
not have hydrogen bond? a. NH3, b. H20, c. H2S, d, HS

C

Which of the following exhibits dipole- dipole attraction between molecules? a. O2, b. H2, c. H2O, d. F2

D

Which of the following diatomic molecules will have the strongest London dispersion forces? a. F2 b. Br2, c. Cl2, d. I2

Phase Diagram

a graph showing the conditions at which a substance exists as a solid, liquid, or gas. It is also a graph that relates Pressure and Temperature to the state of matter.

Phase Diagram

It is a graphic summary of the physical state of a substance as a function of temperature and pressure in a closed system.

vapor pressure curve for solid

A curve between solid and gas

sublimation and deposition

process involved on the curve between solid and gas

vapor pressure curve for liquid

A curve between liquid and gas

boiling point

a point at 100 degrees Celsius @ 101.325 KPa

condensation and vaporization

process involved on the curve between liquid and gas

Freezing point

process involved on the negative slope or a curve between solid and liquid

solid, liquid, gas

Triple point has what elements?

triple point

what point is this in water 0.01 degrees Celsius @ 0.00604 atm

Solution

It is used to describe a homogeneous mixture in which at least one substance (the solute) is dissolved in another substance (the solvent).

solute, solvent

2 parts of a solution

Solvent

It is the substance in which a solute is dissolved in to produce a homogeneous mixture

Solute

It is the substance that dissolves in a solvent to produce a homogeneous mixture

Dilute, Concentrated

solution can be qualitatively described as:

Dilute

a solution that contains a small proportion of solute relative to solvent,

Concentrated

a solution that contains a large proportion of solute relative to solvent.

Unsaturated, Saturated

Semi-Quantitative Expressions of Concentration

Unsaturated

a solution in which more solute will dissolve

Saturated

a solution in which no more solute will dissolve.

unsaturated, saturated, supersaturated

Saturated Solutions

Unsaturated

dissolved solute is below saturation point. More can dissolve

Saturated

dissolved solute is at saturation point. No more can dissolve

Supersaturated

dissolved solute is above saturation point. Additional solute gathers at the bottom

Percent by mass, mole fraction, molarity, molality, percent by volume, parts per million

Quantitative Expressions of Concentration

percent by mass

(also called percent by weight or weight percent) it is the ratio of the mass of a solute to the mass of the solution, multiplied by 100 percent

Percent by volume

It is a common expression used for expressing concentration. It is used for reporting concentration of liquid solutes in solution.

Parts per Million

It is a term used in chemistry to denote a very, very low concentration of a solution. One gram in 1000 ml is 1000 ppm and one thousandth of a gram (0.001g) in 1000 ml is one ppm.

Parts per Million

It is a measurement of the concentration of a solution.