Notes on Particulate Nature of Matter

Particulate Nature of Matter

  • Page 1: PARTICULATE NATURE OF MATTER

Matter

  • Definition: Anything that has mass and can occupy space.
  • Composition: It is composed of baryonic materials.

Common Phases of Matter

  • Solid
  • Liquid
  • Gas
  • Plasma (note: page 3 shows a broken spelling as 'Plasm a')

Phase Changes

  • Energy input/output drives phase changes:
    • Solid → Liquid: Melting
    • Liquid → Solid: Freezing
    • Liquid → Gas: Vaporization
    • Gas → Liquid: Condensation
    • Solid → Gas: Sublimation
    • Gas → Solid: Deposition
  • Ionization/Deionization related to plasma state:
    • Ionization: Gas → Plasma (atoms become free-floating ions and free electrons)
    • Deionization: Plasma → Gas (recombination to neutral gas)
  • Plasma: A special state where some atoms are free-floating ions and free electrons (high-energy, ionized gas).

Extreme Phases of Matter

  • Supercritical Fluid
  • Degenerate Matter

SUPERCRITICAL FLUID

  • Definition: Highly compressed gases that combine properties of gases and liquids.
  • Characteristics: They possess the density of a liquid and the mobility of a gas.

DEGENERATE MATTER

  • Also known as the collapsed state of matter.
  • Condition: Occurs when the usual atomic structure breaks down because electromagnetic forces are overcome by gravity.

PROPERTIES OF MATTER

PROPERTIES OF MATTER

  • Physical properties
    • Intensive properties
    • Extensive properties
  • Chemical properties

1.1 PHYSICAL PROPERTIES

  • These are qualities of matter that are observable and measurable without changing its composition.

INTENSIVE/ INTRINSIC PROPERTY OF MATTER

  • These are the physical properties that remain constant regardless of the amount of matter present.
  • Examples: boiling point, melting point, density, color, odor, and texture.

Some examples of intensive properties

  • Luster (t) / Lustre
  • Color
  • Hardness
  • Boiling point
  • Temperature
  • Refractive index
  • Melting point

EXTENSIVE/ EXTRINSIC PROPERTY OF MATTER

  • These vary with the amount of matter present.
  • Examples: shape, size, length, mass, and volume.

Some examples of extensive properties

  • Size
  • Volume
  • Mass
  • Length
  • Weight
  • Entropy
  • Energy

1.2 CHEMICAL PROPERTIES OF MATTER

  • Characteristics of matter that it exhibits when it undergoes a change in composition.
  • They also describe the behavior of substances in the presence of other substances.

Chemical and Physical Changes

  • Chemical change: A chemical reaction forms new products.
  • Physical change: Matter changes form but not chemical identity.
  • Examples of changes (as listed):
    • Combustion, Rotting, Melting, Shredding, Rusting, Digestion, Boiling, Chopping

CLASSIFICATIONS OF MATTER

Pure substance vs Mixture

  • Pure substance
  • Matter
  • Mixture
  • Element
  • Compound
  • Homogeneous mixture
  • Heterogeneous mixture

A. PURE SUBSTANCES

  • A pure substance is matter with definite chemical composition and distinct properties.
  • Cannot be separated into components by physical separation techniques.

A.1 ELEMENTS

  • Elements are pure in nature.
  • They are made up of atoms and cannot be decomposed into simpler substances by ordinary chemical means.
  • Elements can be a metal, non-metal, or metalloid.

A.1.1 METALS

  • Metals are good conductors of heat and electricity.
  • They have properties of ductility, malleability, exhibit metallic luster, have a high melting point, and high density.

ALKALI METALS

  • These are metals found in Group IA of the Periodic Table.
  • Highly reactive and do not occur freely in nature.
  • Readily lose one electron to form ionic bonds with other elements.
  • Can explode if exposed to water.

[Periodic Table excerpt from the transcript]

  • H, Li, Na, K, Rb, Cs, Fr

ALKALI METALS (summary, as per transcript)

  • Found in group IA; very reactive; do not occur freely in nature.
  • Readily lose one electron to form ionic bonds; can explode when contacted with water.

ALKALI METALS (re-iteration)

  • These are found in group IA of the periodic table.
  • Very reactive and do not occur freely in nature.
  • Readily lose one electron to form ionic bonds with other elements.
  • Can explode if exposed with water.

ALKALINE EARTH METALS

  • Belong to group IIA of the periodic table.
  • The two outer electrons are easily shed to form cations with a charge +2.
  • They are naturally occurring in nature.

TRANSITION METALS

  • They have a lot of electrons that are distributed in different ways.
  • Located at the center of the periodic table.

RARE EARTH METALS

  • LANTHANIDES: All found in nature; not radioactive; all naturally occurring except promethium.
  • ACTINIDES: Located below the lanthanides; all radioactive; all man-made except uranium and thorium.

A.1.2 NON-METALS

  • Non-metals are dull and poor conductors of heat and electricity.

HALOGENS

  • Non-metallic elements; name derives from salt-former (halogen).
  • Compounds containing halogens are called salts.
  • Halogens include fluorine, chlorine, bromine, iodine, and astatine.

NOBLE GASES

  • Elements with a full outer electron shell; highly stable and not readily forming compounds.

A.1.3 METALLOIDS

  • Have characteristics of both metals and non-metals.

A.2 COMPOUNDS

  • Compounds are pure substances made from two or more elements that have reacted chemically with each other.

A.2 COMPOUNDS ORGANIC / INORGANIC

  • ORGANIC: Compounds containing carbon with other elements.
  • INORGANIC: Compounds made up of elements other than carbon.

ORGANIC COMPOUNDS

  • Examples: carbon-containing compounds such as acetic acid, methane, glucose, toluene, and acetone.
  • Formulas (as examples):
    • CH_{3}COOH
    • CH_{4}
    • C{6}H{12}O_{6}
    • C{6}H{5}CH_{3}
    • C{3}H{6}O

INORGANIC COMPOUNDS

  • Salts formed when an acid is neutralized by a base.
  • Acids produce H+ ions in aqueous solution.
  • Bases contain OH- ions in aqueous solution.

Acid–Base–Salt illustration (from the transcript)

  • Acid: HCl
  • Base: NaOH
  • Salt: NaCl
  • Ion representation in solution: Cl-, Na+, OH-, Na+ (example of ions involved)
  • Overall reaction example (neutralization):
  • ext{HCl} + ext{NaOH}
    ightarrow ext{NaCl} + ext{H}_{2} ext{O}

B. MIXTURES

  • Mixtures are formed when two or more substances are mixed together.
  • There are no chemical bonds formed between the substances.
  • They can be separated by physical methods; not requiring chemical reaction.

B.2 HOMOGENEOUS MIXTURE

  • These are perfectly uniform in composition.
  • When two or more substances are mixed and the final substance appears to have the same chemical composition, it is a homogeneous mixture.

Homogeneous Mixture Examples

  • Coffee
  • Wine
  • Air
  • Brass
  • Vinegar
  • Steel
  • Natural Gas
  • Blood

B.3 HETEROGENEOUS MIXTURE

  • Result when the phases mixed are distinguishable from each other.
  • The boundary between phases is usually observable with the naked eye.

Heterogeneous Mixtures Examples

  • Chocolate Chip Cookies
  • Pizza
  • Soda with Ice
  • Tossed Salad
  • Sandwich