Q3

Question 1

Kinetic Molecular Theory

Answer 1

all matters are made up of atoms and molecules that are always moving.

These particles hold kinetic energy and move around in random directions.

Question 2

force that hold atoms together in a metallic substance.

Answer 2

Metallic bond

Question 3

formed between two or more atoms by transfer of one or more electrons between atoms
- electrons are transferred

Answer 3

Ionic bond

Question 4

particle with unequal number of protons and electrons

Answer 4

Ions

Question 5

negative ions

Answer 5

Anions

Question 6

postively charged

Answer 6

Cations

Question 7

consists of the mutual sharing of one or more pairs of electrons between two atoms.

Answer 7

Covalent bond

Question 8

2 types of covalent bonds

Answer 8

Polar covalent, non-polar covalent bonds

Question 9

forces within ionic compounds and simply the attraction between negative and positive ions (anions and cations attract).

Answer 9

Ion-ion forces

Question 10

attraction between two polar molecules

Answer 10

Dipole-dipole

Question 11

is a principle/idea/model that is used to explain the behavior, movement of particles/molecules for every states of matter from a microscopic point of view.

Answer 11

KMT

Question 12

This theory explains the states of matter, and is based on the idea that matter is composed of tiny particles that are always in motion. This theory helps explain observable properties and behaviors of solids, liquids, and gases

Answer 12

KMT

Question 13

KMT states that:

Answer 13

1. Matter is made up of particles that are constantly moving.
2. All particles have energy, but the energy varies depending on the temperature the sample of matter is in.
3. The temperature of a substance is a measure of the average kinetic energy of the particles.
4. A change in phase may occur when the energy of the particles is changed.
5. There are spaces between particles of matter. The average amount of empty space between molecules gets progressively larger as a sample of matter moves from the solid to the liquid and gas phases.
6. There are attractive forces between atoms/molecules, and these become stronger as the particles move closer together. These attractive forces are called intermolecular forces.

Question 14

region of space where all physical and chemical properties are uniform.

Answer 14

Phase

Question 15

Liquids and solids

Answer 15

Condensed phase

Question 16

A state change of any material due to temperature or pressure change is a phase transition. It is a physical change (or reaction).

Answer 16

Phase transition

Question 17

solids whose particles are arranged in regular geometric patterns.

• Rigid and incompressible
• Sharp melting point

Answer 17

Crystalline solids

Question 18

have fixed shape and volume but their particles are not arranged in a regular geometric pattern.

• also referred to as “supercooled” liquids because these solids appear to have been cooled at very low temperatures and their viscosities are very high.
• No definite heat of fusion

Answer 18

Amorphous solid

Question 19

Glass is an example of

Answer 19

Amorphous solid

Question 20

lattice points are occupied by molecules, molecules are packed closely as their size and shape allow , IMF may be LDF in the case of non-polar crystals, dipole-dipole for polar crystals, and some cases such as ice have hydrogen bonding.

Answer 20

Molecular solids

Question 21

the constitution particles are ions
- formed by the arrangement of cations and anions by strong coulombic forces
- atoms are held together by electrostatic force
- held firmly and no large space for the ions to move around

Answer 21

Ionic solids

Question 22

positive metal ions in a sea of delocalized electrons. These electrons are evenly spread out throughout the crystal
- held together by electrostatic force between cations and delocalized electrons (metallic bonds)

Answer 22

Metallic solids

Question 23

a covalent network crystal consists of atoms at the lattice points of the crystal

Answer 23

Covalent solids

Question 24

is a graph that relates pressure and temperature to the state of matter.
The diagram can help us identify what is the state of a substance at a given temperature and pressure.

Answer 24

Phase diagram

Question 25

is the point where at a certain pressure and temperature at equilibrium all three phases of a substance co-exist.

Answer 25

Triple point

Question 26

is a point where temperature and pressure at which gas and liquid merge together to form a supercritical fluid.

Answer 26

Critical point

Question 27

is any substance at a temperature and pressure above its critical point, where distinct liquid and gas phases do not exist.

Answer 27

Supercritical fluid

Question 28

is where a substance is impossible to liquefy no matter how you increase or compress the substance.

Answer 28

Critical temperature

Question 29

is a plot where it shows how the addition of heat (x-variable) can affect the temperature change (y-variable) and phase change of a substance.

Answer 29

Heating curve

Question 30

Types of Solutions

Answer 30

Saturated Unsaturated Super saturated

Question 31

Solvent holds as much solute as is possible at that temperature.

Answer 31

Saturated

Question 32

Less than the maximum amount of solute for that temperature is dissolved in the solvent.

Answer 32

Unsaturated

Question 33

Solvent holds more solute than is normally possible at that temperature.

Answer 33

Super saturated

Question 34

These solutions are unstable; crystallization can usually be stimulated by adding a “seed crystal” or scratching the side of the flask.

Answer 34

Super saturated

Question 35

refers to the amount of solute present in a given quantity of solvent or solution.

Answer 35

Concentration of solution

Question 36

if less than or equal to 0.1g of solute dissolves in 100g of solvent

Answer 36

Insoluble solute

Question 37

- if the amount of solute that dissolves in 100g of solvent is greater than 0.1g but less than 10g.

Answer 37

Slightly soluble solute

Question 38

if less than or equal to 0.1g of solute dissolves in 100g of solvent

Answer 38

Insoluble solute

Question 39

if the amount of solute that dissolves in 100g of solvent is greater than or equal to 10g.

Answer 39

A soluble solute

Question 40

What type of IMF must be predominantly overcome when a molecule of ammonia (NH3) escapes from liquid ammonia?

Answer 40

H-bond

Question 41

Consider a list of liquids that have only London Forces as intermolecular interactions. What happens to the boiling point, vapour pressure and surface tension, respectively, as the molecular weight of these liquids increases? Increases, decreases, increases Increases, decreases, decreases Decreases, increases, decreases Decreases, increases, increase

Answer 41

Increase, decreases, increases

Question 42

Tendency of molecules of the same kind to stick one another.

Answer 42

Cohesion

Question 43

Which of the following changes would increase the vapor pressure of a liquid? A decrease in temperature A decrease in the intermolecular forces in the liquid. An increase in the size of the open vessel containing the liquid.

Answer 43

A decrease in the intermolecular forces in the liquid.

Question 44

Humans have physiologically adapted to sweat if the body temperature rises past ideal levels. The ability to do so helps cool the body down. Water’s ___________ allows us to maintain homeostasis – body regulating itself to maintain balance like body temperature – and survive as we are today.

Answer 44

High specific heat

Question 45

Water molecules bond in a crystalline form as the temperature of water drops. The molecules rearrange to form hexagonal ring. This creates more space between molecules and expansion of water molecules. What characteristic of water does this change describe?

Answer 45

Density

Question 46

H2S

Answer 46

Hydrosulfuric acid or Hyrogen Sulfide

Question 47

Mg3N2

Answer 47

Magnesium nitride

Question 48

NaHCO3

Answer 48

Sodium Bicarbonate

Question 49

Cu3(PO4)2

Answer 49

Copper (II) phosphate

Question 50

Cl2O7

Answer 50

Dichlorine heptoxide

Question 51

1. Capillary Action is caused by adhesion and cohesion forces. 2. CO2 has higher vapor pressure than NaCl. 3. Liquid water has a specific heat of 4.18 J/g-Co and iron has 0.45 J/g-Co, this data shows that liquid water gets hotter faster than the iron. 4. As temperature gets higher, average kinetic energy of molecules increases. 5. Liquids and gases are the phases we considered as fluids. 6. According to KMT, all particles are always in constant motion. 7. The stronger the adhesive force, surface tension also gets stronger. 8. Fluids with high fluidity flows slowly. 9. As the average kinetic energy of your molecules increases, molecules tend to move away from each other. 10. KCl which is a salt is a polar molecule and cannot be dissolve in water.

Answer 51

1.

Question 52

interaction between molecules

Answer 52

Intermolecular force

Question 53

Hard and brittle, have high melting point and a poor thermal and electrical conductor like table salts.

Answer 53

Ionic crystalline

Question 54

Solids occupied by molecules whose forces between may be LDF, dipole-dipole or H-bond.

Answer 54

Molecular crystalline

Question 55

Glass is an example.

Answer 55

Amorphous solid

Question 56

The hardest of the substance belong to this type.

Answer 56

Network covalent

Question 57

Crystalline solid that is used as electric wires.

Answer 57

Metallic crystalline