1. Introduction to Atoms
Holt: Chapter 11
Fusion: Unit 5

2. SOL PS. 3
• The student will investigate and understand the
modern and historical models of atomic structure. Key
concepts include
A) The contributions of Dalton, Thomson, Rutherford and
Bohr in understanding the atom; and
B) The modern model of atomic structure

3. Section 1: Development of Atomic Theory
• Democritus (440 BC)
• The word atom is from the Greek atomos, meaning “not
able to be divided.”
• He thought atoms were small hard particles made of a
single material formed into different shapes.
• Aristotle disagreed, but Democritus was right!
• Matter is made of tiny particles we call atoms.
• Atom- the smallest unit of an element that maintains the
properties of that element.

4. Dalton
• 1700s- scientists realized that elements could combine in specific ratios to
form compounds.
• John Dalton, a British chemist and teacher, wanted to know why
• The results of his experiments were the basis for this atomic theory
published in 1803.
• His theory stated:
• All substances are made of atoms. Atoms are small particles that cannot be created,
divided or destroyed.
• Atoms of the same element are exactly alike, and atoms of different elements are
different.
• Atoms join with other atoms to make new substances.
• He wasn’t 100% correct…

5. Thomson
• 1897, British scientist J.J. Thomson showed that there was a mistake
in Dalton’s theory.
• He discovered there are small particles INSIDE the atom! This means
that atoms can be divided into smaller parts.
• He experimented with a cathode-ray tube. (page 314 Holt)

6. Thomson’s findings
• Due to beam attraction to the positive plate, there must be negative
electric charges.
• Negatively charged particles are present in every kind of atom.
• These negative particles are now called electrons.
• Proposed a new model of the atom: plum-pudding
• Plum-pudding model suggests that electrons are mixed throughout an
atom like plums in a pudding.

7. Rutherford
• 1909, Ernest Rutherford tested Thomson’s theory
• Gold foil experiment- he aimed a beam of positively charged particles
at a sheet of gold foil; he expected the beam to go straight through
the foil, but some particles were deflected or bounced straight back
• He explained that atoms are mostly empty space, with a tiny part
made of highly dense matter.
• 1911- He proposed that the center of the atom is a tiny, extremely
dense, positively charged part called a nucleus.

8. Bohr
• 1913- Niels Bohr, a Danish scientist, studied the way atoms react to
light.
• He concluded that electrons move around the nucleus in certain
paths, or energy levels. Also known as the planetary model.

9. Modern Atomic Theory
• Erwin Scrodinger and Werner Heisenberg further explained the
nature of electrons in the atom. Electrons DO NOT travel in definite
paths. There are regions inside the atom where electrons are likely to
be found. These are called electron clouds.
• 1932- James Chadwick discovers the neutron.

10. Section 2: The Atom
• Atoms are made of protons, neutrons and electrons
• Protons- positively charged particles in the nucleus
• Neutrons- no electrical charge or neutral, located in the nucleus
• Electrons- negatively charged particles found around the nucleus in
electron clouds
• Protons and neutrons are more massive than electrons. The majority
of the mass of an atom is located in the nucleus.
• Atomic mass units are used to describe the mass of atoms or
molecules.

12. • Atoms are neutral. This is due to the protons (+) and electrons (-)
“canceling” each other.
• If the number of protons and neutrons are not equal, the atom
becomes a charged particle called an ion. Losing electrons creates a
positive ion. Losing protons creates a negative ion.
• Atoms of different elements differ.

13. Atomic number
• Atomic number is the number of protons in the nucleus of an atom;
the atomic number is the same for all atoms of an element