MARK KENETH C. SUMBILLO
Special Science Teacher I
Subject Teacher
Around 460 B.C., Greek philosopher Democritus
thought of the idea of atoms.
He asked this question:
If you break a piece of matter in half, and then
break it in half again, how many breaks will you
have to make before you can break it no further?
Democritus thought that it ended at some point,
a smallest possible bit of matter. He called these
basic matter particles, “
.”
academic
requirements
Natural
disasters
Poor internet
connection
If you will be a
poverty solid matter, what
are the things that
you?
School Year
misunderstanding
Distracting
chores
Life is never a smooth road to take.
Situations sometimes go against our favor.
We cannot always have what we want.
People are sometimes unfriendly.
There are times we are
,
there are also times we are
.
What matters is what we are composed of.
When we are in our most basic
,
we can never be broken further.
-Mark Sumbillo
“Everywhere man
blames nature and
fate, yet his fate is
mostly but the echo
of his
and
, his
and
.”
-
Democritus, known in
antiquity as the 'laughing
philosopher' because of
his emphasis on the
value of '
,'
was one of the two
founders of ancient
. He
elaborated a system
originated by his teacher
Leucippus into a
materialist account of
the natural world.
to
460 years (460 B.C.)
1,803 years (1803)
2,263 years
were made in 1907.
According to the official recipe, the previous
day’s Tootsie Roll batch is mixed into the new
batch each day, so theoretically, this means
there’s
of the very first Tootsie
Rolls in every new roll made today.
The English meteorologist,
chemist, mathematician, and
philosopher, John Dalton
formulated the first modern
description of atom as the
fundamental building block of
chemical structures.
He developed the law of
multiple proportions (first
presented in 1803) by studying
and expanding upon the works
of Antoine Lavoisier and
Joseph Louis Proust.
All matter is composed of atoms,
indivisible and indestructible building
blocks. While all atoms of an element
were identical, different elements had
atoms of differing size and mass.
The first breakthrough in
the study of chemical
reactions resulted from
the work of the French
chemist and nobleman
Antoine Lavoisier
between
1772 and 1794.
Lavoisier found that
in a chemical reaction.
Atoms cannot be created, destroyed, or
transformed into atoms of another element.
This statement is true for
is not true, however, for
. It
.
are composed of
.
The smallest possible
amount of matter that
still
as a chemical element,
now known to consist of
a nucleus surrounded
by electrons.
Au
element
Au
atoms
Atoms of different
elements are
;
however, atoms of a given
element are of the same
size, shape, mass, and
chemical properties.
Relative sizes for atoms of the Noble Gases.
This image from
John Dalton’s
published in 1808,
depicts various
atoms and
molecules.
All compounds are composed of
combinations of atoms in
defined ratios.
Proust, a French chemist,
published papers on urine,
phosphoric acid and alum.
During his stay in Spain, Proust
studied Spanish minerals.
In 1806 he articulated the
,
one of the bases of chemical
atomism, and which receives
its name. The law is formulated
in 1808 by John Dalton, but it is
the work of Proust that provides
the
that
determined its acceptance.
Proust had studied tin oxides and found that their
masses were either 88.1% Sn and 11.9% O or
78.7% Sn and 21.3% O (these were tin (II) oxide
and tin (IV) oxide respectively).
Dalton noted from these percentages that
100 g of Sn will combine either with 13.5 g or 27 g
of O; 13.5 and 27 form a ratio of 1:2.
Dalton found an atomic theory of
matter could elegantly explain this
in chemistry – in
the case of Proust’s tin oxides, one
tin atom will combine with either
one or two oxygen atoms.
Sn2O2
Sn2O4
states that a pure compound is made up of
elements in the
by mass.
Examples:
Sodium carbonate
Ammonium chloride
Silicon dioxide
Sodium Chloride
Na2CO3
NH4Cl
SiO2
NaCl
states that two elements combine to form
, the ratio of the
mass of the other element is a whole number
or a simple fraction.
Examples:
H2O2
H2O
OH-
NO
NO2-
NO3-
SO2
SO32-
SO42-
Chemical reactions resulted in
the rearrangement of the
reacting atoms.
A
only involves separation,
combination, or rearrangement of atoms.
6CO2 + 6H2O
C6H12O6 + 6O2
Atomic theory has been
revised over the years to
incorporate the existence
of atomic isotopes and
the interconversion of
mass and energy.
In addition, the discovery
of subatomic particles
has shown that
can be
.
Dalton’s importance in the development
of
has been
recognized by the designation of the
atomic mass unit as a Dalton.
The standard unit that is used for
indicating mass of an atom.
amu
µ
Da
Subatomic
particles
Symbol
Mass (g)
Charge
(coulomb)
neutron
n0
1.6749 x 10-27
0
proton
p+
1.6726 x 10-27
1.6022 x 10-19
electron
e-
9.1094 x 10-31
- 1.6022 x 10-19
Element
p+
e-
n0
𝟏
𝟏𝐇
1
1
0
𝟏𝟐
𝟔𝐂
6
6
6
𝟒𝟎
𝟏𝟖𝐀𝐫
18
18
22
𝟑𝟗
𝟏𝟗𝐊
19
19
20
𝟑𝟐 𝟐−
𝟏𝟔𝐒
16
18
16
𝟐𝟒
𝟐+
𝐌𝐠
𝟏𝟐
12
10
12
𝟓𝟔
𝟑+
𝐅𝐞
𝟐𝟔
26
23
30
Element
p+
e-
n0
𝟑𝟐 𝟐−
𝟏𝟔𝐒
16
18
16
𝟑𝟓 −
𝟏𝟕𝐂𝐥
17
18
18
means having the same
number of electrons. Atoms should be
adjacent periodically and bear different
charge.
neutral to cation
neutral to anion