structure of atom gcse chemistry model of atom

structure of atom gcse chemistry model of atom

1. Model of
the Atom
GCSE Chemistry

2. One
Name the three types
of subatomic particle.
Two
Describe key
properties of the
three subatomic
particles.
Three
Explain what an
isotope is and provide
an example.
Learning Points

3. What are atoms?
Atoms make up everything in the world. Elements are
made up of only one type of atom. Each element has
specific, unique atoms. All atoms are neutral, meaning
that they have no overall charge.

4. Nucleus
The nucleus is the centre of
the atom. It is where all of the
mass of the atom is
contained.
-
-
+ +
Nucleus

5. Subatomic
Particles
Atoms are made up of
three subatomic particles:
Protons
Neutrons
Electrons
-
-
+ +

6. -
Protons
Protons are positively charged
subatomic particles. They can
be found in the nucleus and
have a relative weight of 1.
-
+ +

7. Neutrons
Neutrons are subatomic
particles that have no charge.
They are neutral. They can be
found in the nucleus and have
a relative weight of 1.
-
-
+ +

8. Electrons
Electrons are negatively
charged subatomic particles.
They are located in shells (or
energy levels) around the
nucleus. Electrons have a
relative weight of 0, because
the weight is negligible.
-
-
+ +

9. Location in
the atom
Charge
Relative
weight
Proton Nucleus + 1
Neutron Nucleus 0 1
Electron Shells - 0
Summary

10. Electron Configuration
Atoms can have multiple shells of electrons. The electrons
are arranged in a specific way:
The first shell can hold 2 electrons
The second shell can hold 8 electrons
The third shell can hold 8 electrons
The earlier shells must be filled before the next shell
can be occupied

11. Looking at Electron Configuration
Ne
Neon atoms have 10 electrons. The
electron configuration of neon is 2,8.
Chlorine atoms have 17 electrons. The
electron configuration of chlorine is 2,8,7.
Cl

12. Relative Atomic Mass
Li
3
7
Elements can be found in the periodic table. The numbers next to
the chemical symbols in the periodic table, provide information
about the numbers of subatomic particles. A lithium atom has 3
protons, 4 neutrons and 3 electrons.
Atomic (proton) number = the number of
protons (also the number of electrons).
Relative atomic mass = the total mass of
the nucleus (protons and neutrons).
+
+
+
-
-
-

13. Isotopes
Isotopes are atoms of the same
element with different numbers
of neutrons. For example,
hydrogen has three isotopes with
the same number of protons and
electrons, but different numbers
of neutrons.
Hydrogen-1
Hydrogen-2
Hydrogen-3

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Model of the Atom

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