This document discusses the atomic theory and properties of the three states of matter. It covers key scientists and their contributions, including Dalton formulating the atomic theory, Thomson discovering the electron, Rutherford naming the types of radiation, and Bohr proposing electron orbitals. The three states of matter - solid, liquid, gas - are compared in terms of particle motion and forces. Phase changes like melting, freezing and evaporation are explained. The development of the modern atomic model and discovery of subatomic particles like the proton and neutron are also summarized.

1. GROUP 3
MATTER AND THE
ATOMIC THEORY

2. PROPERTIES OF THE THREE STATES OF MATTER
PHASE CHANGES
MATTER

3. • The particulate matter is a well- accepted
description of matter. The basic principles of
the particulate model of matter are:
a) All matter is made up of tiny particles
b) There is empty spaces in between the particles.
c) The particles are in constant motion.
d) There are forces that act between the particles.
PROPERTIES OF THE THREE
STATES OF MATTER

4. PROPERTIES OF THE THREE
STATES OF MATTER
• This table shows the comparison between solids,
liquids and gases.

5. • The following picture shows the atoms in solid, liquid and
gas.
PROPERTIES OF THE THREE
STATES OF MATTER

6. • Matter, whether solid, liquid or gas, undergoes changes in
physical state, known as phase changes. Here are the phase
changes present in each of the three states of matter.
a) Melting- the solid absorbs energy which eventually increases the kinetic
energy of the particles, making them vibrate strongly and weakening the
attractive forces between the particles.
b) Evaporation- the particles of a liquid lose any order and become
completely free to form a gas. It involves absorption of energy and the
particles move faster and more able to overcome the alternative forces
between them.
c) Freezing- involves heat leaving the system. The particles lose kinetic energy
and become strongly attracted to each other and form a neat
arrangement.
PHASE CHANGES

7. PHASE CHANGES

8. HISTORY OF ATOMIC THEORY
POSTULATES OF JOHN DALTON’S THEORY
THE SUBATOMIC PARTICLES
ATOMIC THEORY

9. • Ancient Greek philosophers proposed
ideas about what matter was made of.
Almost 2,500 years ago, Leucippus and his
disciple, Democritus believed that nature
consisted of two things – “atoms and the
void that surround them” (Knieram, 1995 –
2013). They believed that “atoms are
physically, but not geometrically invisible”.
For Democritus, atoms are indestructible
and completely full, so there is no empty
space. Both Leucippus and Democritus
had the side of idea that there are many
different kinds of atom and each of them
had specific shape and size.
HISTORY OF ATOMIC THEORY

10. DEMOCRITUS
Democritus was an influential Ancient Greek pre-Socratic
philosopher primarily remembered today for his formulation
of an atomic theory of the universe.

11. LEUCIPPUS
Leucippus is reported in some ancient sources to
have been a philosopher that was the earliest Greek
to develop the theory of atomism — the idea that
everything is composed entirely of various
imperishable, indivisible elements called atoms.

12. • After more than 2000 years, the ancient
philosophers’ idea about atoms became a
theory when John Dalton put together
observation and results of several experiments
done by other scientists and formulated the
atomic theory. The postulates of his theory,
which is found in his book entitled “A New
System of Chemical Philosophy” published in
1808.
ATOMIC THEORY

13. a. All matter is made up of tiny particles
b. There is empty space in between the
particles.
c. The particles are in constant motion
d. There are forces that act between
the particles
POSTULATES OF JOHN DALTON’S
THEORY

14. JOHN DALTON
Chemist John Dalton was born September 6, 1766, in
Eaglesfield, England. During his early career, he
identified the hereditary nature of red-green color
blindness. In 1803 he revealed the concept of
Dalton’s Law of Partial Pressures. Also in the 1800s, he
was the first scientist to explain the behavior of
atoms in terms of the measurement of weight.
Dalton died July 26, 1844 in Manchester, England.

15. The cathode ray experiments in 1897 of various
scientist including Sir Joseph John Thomson led to the
discovery of the electron, the negatively charged particle
found in an atom. When high voltage electric current was
applied across electrically charged plates in a cathode ray
tube containing a small amount of gas, a ray coming from
the negatively charged electrode, the cathode, was
observed.
Thomson revised the atomic theory and proposed the
raisin bread model of the atom. According to him, an atom
is positively charged sphere with loosely embedded
electrons. This is similar to a bread with embedded raisins.
THE SUBATOMIC PARTICLES

16. JOSEPH JOHN THOMSON
J.J. Thomson was born on December 18, 1856, in
Cheetham Hill, England, and went on to attend Trinity
College at Cambridge, where he would come to head the
Cavendish Laboratory. His research in cathode rays led to
the discovery of the electron, and he pursued further
innovations in atomic structure exploration. Thomson won
the 1906 Nobel Prize in Physics, among many accolades.
He died on August 30, 1940.

17. The existence of subatomic particles is
further confirmed with the discovery of
radioactivity by Henri Becquerel. He found
out that the mineral pitch blend emitted high
penetrating rays, called Becquerel rays.
Furthermore, Pierre Curie and Marie Curie
discovered the elements Polonium and
Radium and found them to emit similar rays.
THE SUBATOMIC PARTICLES

18. HENRI BECQUEREL
Henri Becquerel was born in Paris, France, on
December 15, 1852. Born into a family of scientists,
Becquerel followed his father into the academic
field of physics. In 1896, he discovered radioactivity,
which was to be the focus of his work thereafter.
Becquerel won the Nobel Prize for Physics in 1903,
sharing the prize with Marie and Pierre Curie. He
died in Brittany, France, on August 25, 1908.

19. Born Maria Sklodowska on November 7, 1867, in Warsaw,
Poland, Marie Curie became the first woman to win a
Nobel Prize and the only woman to win the award in two
different fields (physics and chemistry). Curie's efforts, with
her husband Pierre Curie, led to the discovery of polonium
and radium and, after Pierre's death, the development of
X-rays. She died on July 4, 1934.
MARIE CURIE

20. PIERRE CURIE
French physicist Pierre Curie was one of the founding
fathers of modern physics and is best known for
being a pioneer in radioactive studies. He and his
wife, Marie Curie, won the Nobel Prize in Physics in
1903, and the curie, a unit of radioactivity, was
named after him. Curie died in 1906 after being run
over by a horse-drawn carriage in Paris.

21. •Ernest Rutherford named the three
kinds of Becquerel rays as alpha (a)
particles, beta (B) particles, and
gamma (y) radiation. He was also
considered the Father of Nuclear
Physics.
THE SUBATOMIC PARTICLES

22. Chemist and physicist Ernest Rutherford was born August
30, 1871, in Spring Grove, New Zealand. A pioneer of
nuclear physics and the first to split the atom, Rutherford
was awarded the 1908 Nobel Prize in Chemistry for his
theory of atomic structure. Dubbed the “Father of the
Nuclear Age,” Rutherford died in Cambridge, England, on
October 19, 1937 of a strangulated hernia.
ERNEST
RUTHERFORD

23. Niels Bohr assumed that electrons move in
orbits around the nucleus but only orbits of certain
radii are allowed. The present model is based on a
theory which says that electrons are not confined in
fixed orbits around the nucleus. The positive charge
of the nucleus comes from the proton. Its charge
has the same magnitude as the electron but
opposite in sign.
THE SUBATOMIC PARTICLES

24. NIELS BOHR
Born on October 7, 1885, in Copenhagen, Denmark,
Niels Bohr went on to become an accomplished
physicist who came up with a revolutionary theory on
atomic structures and radiation emission. He won the
1922 Nobel Prize in physics for his ideas and years later,
after working on the Manhattan Project in the United
States, called for responsible and peaceful applications
of atomic energy across the world.

25. Eugene Goldstein discovered its existence
when he experiment with tubes containing gasses
at low temperature or pressures and a tube with
perforated cathode. He observed rays passing the
holes on the cathode and moving away from the
positive electrode, which are left after electrons
have been removed. This was called proton.
THE SUBATOMIC PARTICLES

26. German physicist known for his work on electrical phenomena in
gases and on cathode rays; he is also credited with discovering
canal rays. In 1886 he discovered what he
termed Kanalstrahlen, or canal rays, also called positive rays; these
are positively charged ions that are accelerated toward and
through a perforated cathode in an evacuated tube. He also
contributed greatly to the study of cathode rays; in 1876 he
showed that these rays could cast sharp shadows, and that they
were emitted perpendicular to the cathode surface.
EUGENE
GOLDSTEIN

27. THE SUBATOMIC PARTICLES
The following shows the proposed model of atoms by different scientists.

28. The positive charge of the nucleus comes from the
proton. Eugene Goldstein discovered its existence when he
performed experiments with tubes containing different
gases at very low pressures and a tube with a perforated
cathode.
The protons account for only part of the mass of the
nucleus. In 1932, Sir James Chadwick discovered the
neutron, also found in the nucleus of the atom. It has almost
the same mass as the protons but neutral. The charge of the
electron is measured in coulombs (c). In chemistry, the
charge of a particle is usually expressed in charge units or as
multiples of the charge of the electron.
THE SUBATOMIC PARTICLES

29. THE SUBATOMIC PARTICLES
• The mass of the particles is commonly expressed in
atomic mass unit (amu) instead of grams. One
amu is equivalent to 1.66053892 × 10 to the
negative 24 grams. Therefore, the alpha particle,
which is the helium nucleus and which contains
two protons and two neutrons, has a mass of
around 4 amu.

30. One of the assumptions of Dalton’s atomic theory states that
atoms of the same element are alike and are different from the
atoms of other elements. We will now see how the atom is
identified and that the atoms of the same elements are not
identical in all aspects.
• Atomic number: the number of protons in their nuclei. The atomic
number is the identity number of an element. It provides several
information regarding the characteristics of the atoms of the
elements.
• Isotope: Isotopes are variants of a particular chemical element
such that while all isotopes of a given element have the same
number of protons in each atom, they differ in neutron number.
IDENTITY OF AN ATOM

31. • Ion: If electrons are removed from or added to a neutral
atom, a charged particle of the same particle, called ion,
is formed. Ions have two different charges and they are as
what follows.
a) Cation: An ion with positive charge and is formed when
an electron is removed from the atom.
b) Anion: A negatively charged ion and is formed when an
electron is added to the atom.
IDENTITY OF AN ATOM

33. • G5 Cariño, Ma. Fatima
• G10 Javier, Ma. Sarah
• G15 Moralejo, Ski
• G17 Reyes, Joanna Ysabella
• G21 Samson, Claire Erika
• G26 Ty, Trizsa Jasmin
• B7 Da Silva, John Julius
• B12 Francisco, James Harvey
• B16 Oamil, Ken Edward
8- Mitochondrion Group 3 Members