Matter in Our Surroundings

Blocks

Layers

Particles

Waves

A stone is heavy

Water is wet

Diluting a colored solution still leaves it colored

Air can be felt

Newton

Pascal

Kilogram

Metre

Ether

Earth

Plastic

Steel

The fact that solids have a high density

The fact that a single drop of water contains about $10^{21}$ particles

The fact that gases can be compressed

The fact that liquids can flow

Magnetic force

Inter-particle or intermolecular force

Gravitational force

Nuclear force

Evaporation and condensation

Diffusion of gas particles in air

Chemical reaction of smoke with oxygen

High pressure in the corner of the room

Substance A is more likely to be a gas than substance B.

Substance A is more likely to be a solid or liquid than substance B.

Substance B will have a higher density than substance A.

Substance B will have a higher boiling point than substance A.

A piece visible to a magnifying glass.

A single atom of copper.

A single electron from a copper atom.

Copper cannot be divided because it is continuous.

Gas particles have more mass than solid particles.

Gas particles have higher kinetic energy and negligible forces of attraction compared to solid particles.

Solid particles are not matter.

Solid particles are too large to move.

$0^\circ C$

$100^\circ C$

$273^\circ C$

$37^\circ C$

Ice has more energy

Water has more energy

Ice absorbs latent heat from the surroundings to melt

Water absorbs latent heat from the surroundings

Particles of matter are very small

Particles of matter have spaces between them

Particles of matter are constantly moving

Particles of matter are visible to the naked eye

$3.34 \times 10^5 J/kg$

$2.25 \times 10^6 J/kg$

$100 J/kg$

$0 J/kg$

1 and 2

3 and 4

2 and 3

1 and 4

Wind speed

Surface area

Insoluble impurities in the liquid

Humidity

Definite shape

Fluidity

Incompressibility

Fixed volume

It would still sublimate directly into a gas at the same temperature.

It would remain a solid indefinitely and could not be converted to any other state.

It would first melt into a liquid state before eventually boiling into a gas.

It would immediately transition into the plasma state due to the high pressure.

Evaporation requires the entire liquid to reach the same kinetic energy, whereas boiling only affects the top layer.

Boiling occurs only when the vapor pressure of the entire bulk matches the atmospheric pressure, while evaporation involves only high-energy surface molecules escaping.

Evaporation is an exothermic process that heats the surroundings, while boiling is an endothermic process.

Atmospheric pressure only exerts force on the liquid during evaporation and becomes zero during the process of boiling.

The density and inter-particle space of the liquid and gas phases have become identical.

The particles have lost all kinetic energy and are in a state of absolute rest.

The substance has transitioned into a Bose-Einstein Condensate.

The inter-molecular forces have become infinitely strong, turning the substance into a solid.

Substance A

Substance B

Substance C

All three substances have equal forces of attraction

Liquid to Gas

Gas to Liquid

Solid to Liquid

Liquid to Solid

Solid

Liquid

Gas

Ice

Solid

Liquid

Gas

Plasma

Melting Point

Boiling Point

Critical Temperature

Sublimation Point

$273\ K$

$373\ K$

$0\ K$

$100\ K$

Have less energy than particles in ice.

Have more energy than particles in ice.

Move slower than particles in ice.

Are closer together than particles in ice.

$2.25 \times 10^6 J/kg$

$3.34 \times 10^5 J/kg$

$4.18 \times 10^3 J/kg$

$2.73 \times 10^5 J/kg$

Melting and Boiling

Sublimation and Deposition

Vaporization and Condensation

Fusion and Solidification

Weaker

Stronger

Equal

Negligible

From a heater only

From the surrounding air or the liquid itself

From the bottom of the container only

Energy is not required

Mass

Energy

Volume

Color

Kinetic energy decreases

Kinetic energy remains the same

Kinetic energy increases

Kinetic energy becomes zero

It has a higher boiling point

It has a lower boiling point

It is denser than water

It does not evaporate at all

Beaker B will have a higher rate of evaporation because it contains more water molecules.

Beaker A will have a higher rate of evaporation because the water level is lower.

Both beakers will have the same rate of evaporation because they have the same surface area.

The rate of evaporation cannot be determined without knowing the exact humidity.

It increases the rate of evaporation to keep the plant cool during the day.

It decreases the rate of evaporation by reducing the exposed surface area.

It allows the plant to absorb more moisture from the air through the spines.

It increases the kinetic energy of the water molecules within the plant.

Water

Ether

Alcohol

Cooking oil

From the sunlight only.

From the bulk of the liquid and the surroundings.

Only from the air above the liquid.

The molecules create their own energy.

Increases the temperature of the surroundings.

Decreases the humidity of the air around the clothes.

Increases the surface area of the clothes.

Decreases the kinetic energy of the water molecules.

Increase in surface area

Increase in temperature

Increase in wind speed

Increase in humidity