INTRODUCTION TO PS:

PHYSICAL SCIENCE

  • is a branch of natural science that is concerned with the study of nonliving materials

  • includes Chemistry, Physics and Earth Science

CHEMISTRY

  • deals with the study of composition, structure, properties, and changes in matter

PHYSICS

  • deals with the properties and interaction of matter and energy

EARTH SCIENCE

  • is concerned with the study of Earth and the universe around it

  • it is divided into four namely: geology, oceanography, meteorology and astronomy

Matter

  • anything that occupies space and has mass.

States of Matter

  • Solid

  • Liquid

  • Gas

  • Plasma

  • Bose-Einstein Condensate

Solid

  • where atoms or molecules are in contact

  • force of attraction are strongest

  • crystalline sugar, salt, and metals

Solid object

  • occupies definite shape and volume and is independent of its container. It can no longer compressed because its particles are tightly packed

Types of Solid

Crystalline

  • solids that have well-defined shape

  • Their particles exist in highly ordered arrangement.

  • calcite, quartz, sugar, diamonds, etc

Amorphous

  • solids whose particles are organized in random patterns.

  • charcoal, rubber, glass

Liquid

  • state of matter where particles cohere but are not so rigid

  • molecules are usually separated with greater distance compared to that of the solids

  • has a fixed volume but no definite shape. Particles are held together strongly by attractive forces and are in close contact with another.

  • are free to move past one another

  • motion of particles passing one another causes it to take the shape of its container.

Movement of atoms

  • gives a liquid its distinctive property which is the ability to flow

Viscosity

  • measure of a fluid’s resistance to flow

  • shampoo, soda, oil and gasoline

Gases

  • has no definite volume and shape.

  • distance of atoms or molecules is much greater than in liquid.

  • expands to fill its container.

  • its particles move independently of one another and they have enough energy to overcome the attractive forces that hold them together

  • it bounces and presses continuously in all directions against the walls of its container

Plasma

  • state of matter is only under extreme condition

  • matter is changed into an aggregate of positively charged particles

  • These particles move very rapidly in a cloud of negatively charged electrons

  • stars, lightning, welding arc, auroras, neon signs

Bose Einstein Condensate

  • only developed in laboratories

  • occurs in temperature close to absolute zero

  • particles here move closer, but stopping when temperature is absolute 0.

  • made up of bosons

  • BEC

Eric Cornell & Carl Weiman

  • were the ones who proved the theory of two physicist, Albert Einstein & Satyendra Nath Bose.

Atom

  • came from the Greek word “atomos” which means “indivisible” or “uncuttable”.

  • smallest particle that makes up matter

  • fundamental building blocks of matter.

Structure of atoms

Subatomic particles of an atom

Proton

  • positively charged particle

  • Ernest Rutherford

Electron

  • negatively charged particle

  • J.J. Thomson

Neutron

  • neutral in charged

  • James Chadwick

Matter can be classified into two categories:

Pure Substances

  • are either elements or compounds.

  • Elements and Compounds

Mixtures

  • can either be homogeneous or heterogeneous.

  • Homogeneous and Heterogeneous

Element

  • type of matter which cannot be broken down into two or more pure substances

In chemistry

  • elements are identified by their symbols

  • consists of one or two letters usually derived from the name of the elements

118 recorded

  • elements in the periodic table

Compound

  • is a pure substance that contains more than one element

Example:

Water

  • contains hydrogen and oxygen

Table salt

  • contains sodium and chlorine

Mixtures

  • contains two or more pure substances combined in such a way that each substance retains its identity

Two types of mixtures:

Homogenous

  • or uniform mixtures.

  • The composition of the mixtures are the same throughout.

Heterogeneous

  • or non uniform mixtures

  • those composition varies throughout.

Solution

  • common type of homogeneous mixture

Solute

  • is the substances that gets dissolved

Solvent

  • dissolving medium

Several methods in the chemical laboratory can be used to separate components of a mixture:

Filtration

  • passing the solution using a filter medium with fine pores.

Distillation

  • applying heat vaporizing the liquid leaving a residue behind

  • liquid can be recovered in pure form

Chromatography

  • this is more complex, but more versatile separation of liquids based on their solubility and affinity or adsorption on a solid surface in case of paper chromatography or through the gas chromatography for mixtures of volatile solutions.

Properties of Matter

Physical property

  • those that you can find is by direct use of your senses and by weighing and measurement.

  • inherent characteristics of a substance that can be determined, observed, and measured without changing its composition.

  • Example: color, shape, hardness, luster, ductility, malleability, conductivity, density, solubility roughness, smoothness, sweetness, saltiness, elasticity, tensile and more

Physical properties of matter fall into two categories:

Intensive properties

  • do not change whether the amount of substance is small or large.

Color

  • if we add a 5 kg of water to a 10 kg of water, it is still blue.

BP/MP

  • when a 5 kg of water and 10 kg of water are boiled at 100˚C.

Extensive properties

  • depends on how much matter

  • mass, length, volume, internal energy, heat, enthalphy, entropy, time, circumference, diameter, distance, area, width, and thickness

Richard C. Tolman in 1917

  • Intensive and extensive properties were introduced by

Chemical property

  • those that when you do observation, chemical change must be carried out.