Dalton's Atomic Theory

1. Oxygen atoms Hydrogen atoms
DALTON’S ATOMIC THEORY

1) All matter is composed of tiny, indivisible particles called atoms.
For example, atoms of oxygen.

2) All atoms of a particular element are identical, but the atoms
of one element differ from the atoms of any other element. Each
element has unique atoms.

3) Atoms of different elements combine with each other in
certain whole-number proportions to form compounds. For
example, water (H2O) is a combination of one atom of oxygen
and two atoms of hydrogen.

4) In a chemical reaction, atoms are rearranged to form new compounds;
they are not created, destroyed, nor changed into atoms of any other
element.

There were three fundamental laws established by Dalton and other
scientists of his time to support the atomic theory. These laws are the:
a) Law of Conservation of Mass
The law of conservation of mass states that in a chemical reaction, matter is
neither created nor destroyed, or, more accurately, there is no detectable change
in mass during an ordinary chemical reaction.

b) Law of Definite Proportions
The law of definite proportions states that different samples of any pure
compound contain the same elements in the same proportions by mass.

c) The Law of Multiple Proportions
The law of multiple proportions states that the mass of one element that
can combine with a fixed mass of another element are in a ratio of small whole
numbers.

• Oxygen•Carbon•Hydrogen