Modules 1,2,3

Question 1

Matter has the ability to undergo _, the transformation of matter from one phase to another, as influence by varying physical conditions such as temperature and pressure.

Answer 1

phase changes

Question 2

A _ illustrates the changes in the phase of a matter under varying temperature and pressure conditions.

Answer 2

phase diagram

Question 3

This explains how gases behave. Also explains the properties of liquid and solid molecules, as well as the forces of attraction that account for such properties.

Answer 3

Kinetic Molecular Theory

Question 4

The word kinetic comes from the Greek word _, which means “to move”.

Answer 4

kinetin

Question 5

The energy needed to keep the articles moving.

Answer 5

kinetic energy (of a particle)

Question 6

What is kinetic energy dependent on?

Answer 6

temperature

Question 7

Phase changes are always accompanied by?

Answer 7

heat flow

Question 8

What is the strength of the
intermolecular forces of attraction dependent on?

Answer 8

• arrangement of the particles
• proximity of particles relative to one another
• nature of interacting particles

Question 8

This pertains to forces that hold individual particles such as atoms, molecules, or ions together.

Answer 8

intermolecular forces of attraction

Question 9

These are responsible for interactions within a molecule, such as covalent and ionic bonds. These are stronger than intermolecular attractions.

Answer 9

intramolecular forces of attraction

Question 10

Four types of intermolecular forces of attraction.

Answer 10

1. London dispersion force
2. Dipole-dipole interaction
3. Ion-dipole interaction
4. Hydrogen bond

Question 11

The four types of intermolecular forces of attraction are also known as?

Answer 11

Waals forces

Question 12

Who is Waals forces named after?

Answer 12

Dutch scientist Johannes Diderik van der Waals, 1837-1923

Question 13

This is the weakest among the intermolecular forces of attraction.

Answer 13

London dispersion force

Question 14

London dispersion force is caused by _, or the distortion of the electron cloud brought about by the presence of a highly charged particle.

Answer 14

Polarization

Question 14

London dispersion force is named after German-born physicist?

Answer 14

Fritz London

Question 15

The larger the electron cloud, the higher the chances of the atom getting attracted by a positively charged particle, which results to _, wherein one end of the atom is partially positive and the other end is partially negative?

Answer 15

temporary dipoles

Question 16

The London dispersion force occurs in all types of molecules, such as?

Answer 16

a. carbon dioxide (CO2)
b. gaseous diatomic molecules (hydrogen, oxygen, and nitrogen)
c. halogens (xenon or argon)

Question 17

How far an the London dispersion force reach?

Answer 17

3 x 10^9 meters

Question 18

London dispersion force is responsible for?

Answer 18

condensation and solidification of these molecules

Question 19

The _ of the oxygen atom, or the ability of the oxygen atom to draw an electro toward itself, contributes to the formation of a dipole.

Answer 19

electronegativity

Question 20

An intermolecular force of attraction that occurs between partially positive and partially negative ends/

Answer 20

Dipole-dipole interaction

Question 21

Dipole-dipole interaction is observed in _, such as amino acids, wherein the electrons are shared both by oxygen and carbon atoms.

Answer 21

polar covalent molecules

Question 22

This arises from the interaction between an ion and a polar molecule.

Answer 22

Ion-dipole interaction

Question 22

If the molecule is a _ (positively charged ion), it will be attracted to the partially negative end of the polar molecule.

Answer 22

cation

Question 23

If the molecule is an _ (negatively charged ion), it will be attracted to the partially positive end of the polar molecule.

Answer 23

anion

Question 24

The energy of the strength of the ion-dipole interaction is about _ (kJ/mol) for a _ (ppm) distance.

Answer 24

15 kilojoules per mole (kJ/mol) for a 500 parts per million (ppm)

Question 25

A special kind of dipole-dipole interaction, which is formed when hydrogen bonds with fluorine, oxygen, or nitrogen. Generally, they are still weaker than ionic or covalent bonds, but they are the strongest intermolecular force of attraction (when the _ is present between two atoms of two different molecules).

Answer 25

Hydrogen bond

Question 26

The distance needed to form a hydrogen.

Answer 26

2 x 10^-10m

Question 27

Properties of Liquids

Answer 27

1. Viscosity 2. Surface Tension 3. Vapor Pressure 4. Boiling Point

Question 28

This property refers to the measure of a liquid's resistance to flow.

Answer 28

Viscosity

Question 29

This refers to the amount of resistance needed to increase the surface area of liquids.

Answer 29

Surface Tension

Question 30

This is necessary to overcome surface tension. Must be proportional to the strength of the intermolecular forces.

Answer 30

Energy

Question 31

The work required to increase the surface area of a liquid by a unit area.

Answer 31

Surface free energy

Question 32

Vaporization is the transformation of a substance from a liquid to a gas. Vaporization is an endothermic process as it requires absorption of energy to break the intermolecular forces of attraction in a liquid.

Answer 32

Vapor Pressure

Question 33

The surface tension of water is _ and has a surface energy of _.

Answer 33

72.8 millinewtons per meter (mN/m); 72.8 millijoules per square meter (mJ/m^2)

Question 34

The condition at which there is a negligible net change.

Answer 34

Equilibrium

Question 34

The energy required to vaporize 1 mole of a liquid at a pressure of 101 325 pascals (Pa), which is equivalent to 760 millimeters of mercury (mmHg) or 1 atmosphere (atm).

Answer 34

standard heat of vaporization

Question 35

Liquid heated to transform into gas molecules. Then as the latter increases, some have the tendency to return to their liquid phase.

Answer 35

Condensation

Question 36

Defined as the pressuure of the vapor present at equilibrium.

Answer 36

vapor pressure of a liquid

Question 37

The ability to readily evaporate from an open vessel.

Answer 37

Volatility

Question 38

A liquid boils when its vapor pressure is equal to the prevailing atmospheric pressue.

Answer 38

Boiling Point

Question 39

An effective method in separating the components of a mixture or in the removal of impurities in solvents. Performed by heating mixture at a known temperature.

Answer 39

Distillation

Question 40

A molecule that contains a hydrogen proton.

Answer 40

Acid

Question 41

A molecule that contains hydroxide according to Arrhenius' definition.

Answer 41

Base

Question 42

Involves the transfer of protons from and to the same identical molecule, as given in the previous equation.

Answer 42

Autoprotolysis

Question 43

The ability to resist extreme pH changes.

Answer 43

Buffer

Question 44

These have a definite shape and volume due to the compact arrangement of their particles.

Answer 44

Solids

Question 45

Broad classifications of solids:

Answer 45

Crystalline and Amorphous

Question 46

_ have a regular, highly ordered arrangement.

Answer 46

Crystalline solids

Question 47

Examples of Crystalline solids:

Answer 47

amethyst fluorite pyrite

Question 47

Examples of Amorphous solids

Answer 47

glass charcoal plastic containers

Question 48

_ have a random, disordered arrangement. Gradually soften when heated and melt at a wide range of temperatures.

Answer 48

Amorphous solids

Question 49

This refers to the three-dimensional pattern formed by the points representing the location of these particles; it defines the basic structure of the lattice.

Answer 49

Space lattice

Question 50

This has spheres occupying all vertices.

Answer 50

simple cubic unit cell

Question 50

This has spheres occupying all vertices and faces.

Answer 50

face-centered cubic unit cell

Question 50

The smallest unit of the lattice.

Answer 50

unit cell

Question 51

This is characterized by spheres occupying the vertices and a sphere inside the cell.

Answer 51

body-centered unit cell

Question 52

Examples of body-centered crystal structures at 298K (25C):

Answer 52

Metals such as chromium, iron, and tungsten

Question 53

A rare and highly radioactive metal assumes a cubic crystal structure.

Answer 53

Polonium

Question 54

Examples of face-centered cubic structure:

Answer 54

Precious metals such as gold and platinum

Question 54

The number of particles present in a unit cell is systematically determined to quantify the _ or the number of the nearest neighboring particles, as well as to identify the physical properties of solids such as density and conductivity.

Answer 54

coordination number

Question 55

The crystal structure of a solid can be determined by _.

Answer 55

X-ray diffraction

Question 56

Who pioneered the work on X-ray crystallography and were both awarded the Nobel Prize in Physics in 1915.

Answer 56

William Henry Bragg and son William Lawrence Bragg

Question 57

The seven crystal systems:

Answer 57

1. cubic 2. tetragonal 3. orthorhombic 4. monoclinic 5. triclinic 6. hexagonal 7. rhombohedral (trigonal)

Question 58

Different substances that crystallize in the same lattice with the same atomic arrangements.

Answer 58

Isomorphous

Question 59

Substances that crystallize in several arrangements are?

Answer 59

polymorphous

Question 59

Crystals that are the same in two dimensions but different in the third.

Answer 59

Polytypes

Question 60

Polytypes can be either _ or _.

Answer 60

hexagonal or cubic close-packed

Question 61

This gives an ABAB pattern of layers, resembling a hexagonal unit cell.

Answer 61

hexagonal close-packed polytype

Question 62

This gives an ABCABC pattern of stacking.

Answer 62

cubically close-packed polytype

Question 63

Unoccupied spaces in the crystal?

Answer 63

Holes

Question 64

Size of the octahedral hole?

Answer 64

0.414r

Question 65

Size of the tetrahedral hole?

Answer 65

0.225r

Question 66

Classifications of solid:

Answer 66

1. ionic 2. molecular 3. network 4. metallic

Question 67

Ions occupy the unit cell. These are hard, brittle, and poor conductors of heat and electricity.

Answer 67

Ionic solids

Question 68

An example of ionic solid.

Answer 68

Sodium chloride (NaCl)

Question 69

The unit cell of a _ is made up of molecules or atoms. High melting points ranging from 673 to 3273K (400-3000C). These are soft and poor conductors of heat and electricity.

Answer 69

Molecular Solids

Question 70

The coordination number of molecular solids:

Answer 70

four

Question 71

The coordination number of ionic solids:

Answer 71

six

Question 71

Allotropes of carbon.

Answer 71

Diamond and graphite

Question 72

Polymetric materials, diamond, and quartz are classified as _. These are large or "giant" molecules in which atoms are covalently bonded in a highly cross-linked, rigid network. Are very hard and have high melting points, ranging from (1473 to 4273K)/(1200-4000C). Poor thermal and electrical conductors.

Answer 72

Network or Covalent Solids

Question 73

These are different physical forms of the same element in the same physical state.

Answer 73

Allotropes

Question 74

These are bound by metallic bonding, a type of bond in which the metal atoms "Swim" in a sea of electrons. Thus, intermolecular attraction exists between nucleus of metal atom and the negatively charged electrons. Excellent thermal and electrical conductor. Also possess malleability, ductility, luster (interaction of light with the surface of the metal), and hardness.

Answer 74

Metallic solids

Question 75

The coordination number of metallic solids:

Answer 75

eight or 12

Question 76

Examples of metals:

Answer 76

Copper nickel chromium

Question 76

These do not conduct electricity or heat due to thelarge band gap between empty MO and conduction band.

Answer 76

Insulators

Question 77

_, or simply the band theory of metals, accounts for the most properties of metals.

Answer 77

molecular orbital (MO) theory

Question 78

This movement of electrons in the MOs occupied by the conducting electrons called _ enable the conduction of heat through a metal.

Answer 78

conducting bands

Question 79

A process of introducing a filled MO from a dopant, which is either electron-deficient or electron-rich, in between the empty MO and the conduction band.

Answer 79

Doping

Question 80

Involve transition from one phase to another. Occurs when a substance is subjected to different temperature and pressure conditions.

Answer 80

Phase changes

Question 81

Phase changes include:

Answer 81

1. Melting 2. Vaporization 3. Sublimation

Question 82

A solid may turn into liquid if it is heated.

Answer 82

Melting

Question 82

Continuing the heating process will eventually cause the liquid to boil and eventually vaporize, or turn to gas.

Answer 82

Vaporization

Question 83

The temperature at which a solid changes to a liquid.

Answer 83

melting point

Question 84

The energy required to melt 1 mol of solid at its melting point.

Answer 84

latent heat of fusion

Question 84

At what temperature further increases and water bpils?

Answer 84

373 K (100C)

Question 85

A system in which no exchanges of matter take place.

Answer 85

Closed system

Question 85

This represents pressure-temperature relationships at equilibrium, as the pure substance undergoes phase changes in a closed system.

Answer 85

phase diagram

Question 85

The process at which a solid is vaporized at atmospheric pressure without transforming to a liquid.

Answer 85

Sublimation

Question 85

Matter goes into the system and goes out into the surroundings, or vice versa.

Answer 85

Open system

Question 86

The critical temperature of water.

Answer 86

674 K (374C)

Question 86

Formed when the temperature of a substance is above its critical temperature.

Answer 86

Supercritical fluid

Question 86

The critical temperature of carbon dioxide

Answer 86

304K (31C)

Question 87

The temperature in which the vapor cannot be liquefied regardless of the pressure applied.

Answer 87

Critical temperature

Question 87

Gives the combinaation of the critical pressure and critical temperature.

Answer 87

Critical point

Question 87

The pressure at which liquefaction occurs at the critical temperature.

Answer 87

Critical pressure

Question 88

The critical point of water.

Answer 88

647 K and 2.21 X 10^7 Pa (218 atm)

Question 88

The critical point of carbon dioxide.

Answer 88

304 K and 7.40 X 10^6 Pa (73 atm)