This document discusses isotopes and atomic structure. It defines isotopes as atoms of the same element that have the same number of protons but different numbers of neutrons. Isotopes have the same chemical properties but slightly different physical properties. The document also discusses nucleon number, which is the total number of protons and neutrons in an atom's nucleus. The mass number equals the nucleon number. Radioactive isotopes are unstable and undergo nuclear decay over time into stable daughter isotopes.

1. THE NATURE OF MATTER
Chapter # 02
Topic :ISOTOPES
Objective
Define nucleon number
Define and state isotope of same atoms with
different nucleon number

2. ATOMIC STRUCTURE
Nucleus
Electron
Orbit
Energy Levels

3. ATOMIC STRUCTUREATOMIC STRUCTURE
the number of protons in an atom
the number of protons and
neutrons in an atom
HeHe
22
44Atomic mass
Atomic number
number of electrons = number of protons

4. 4
O
16
8
chemical symbol
mass number
(nucleon number)
proton number
(atomic number)
P=E
No. of
protons= no.
of electrons
atomic number (proton number) is the number of
protons in an atom.
Each oxygen atom has 8 protons.
As the number of electrons is equal to the number of
protons in an atom, each oxygen atom contains 8
electrons.
Mass=P+N
mass number is the total number
of protons and neutrons in an
atom.
Number of neutrons in the
oxygen atom is: 16 – 8 = 8.
Interpreting Chemical Symbol

5. Definition of Isotopes
Isotopes are atoms of the same
element which contains the same
number of protons but different
number of neutrons.

6. Isotopes
O
16
8
mass
number
proton
number
Oxygen-16 Oxygen-17 Oxygen-18
O O
17
8
18
8
n = 8 n = 17 – 8
= 9
n = 18 – 8
= 10

7. Isotopes
Isotopes have the same chemical
properties but slightly different
physical properties

8. Q. Do all isotopes of the same element have the
same mass?

9. Isotopes of Some Elements and Their
Atomic Mass

10. 10
The atomic mass of an element
• is listed below the symbol of each element on
the periodic table.
• Gives the mass of an “average” atom of each
element compared to 12C.

11. 11
The calculation for atomic mass requires the
• percent(%) abundance of each isotope.
• atomic mass of each isotope of that element.
• sum of the weighted averages.
mass of isotope(1)x (%) + mass of isotope(2) x (%) =Ar
100 100
Ar=(Average atomic mass)

12. 12
24Mg = 23.99 amu x 78.70/100 = 18.88 amu
25Mg = 24.99 amu x 10.13/100 = 2.531 amu
26Mg = 25.98 amu x 11.17/100 = 2.902 amu
Atomic mass (average mass) Mg = 24.31 amu

14. I know the answer……..

15. RADIO ISOTOPES
Parent isotope
Radioactive decay
heat
Daughter isotope

16. Stable vs. Unstable
• A stable isotope does NOT
undergo radioactive (or nuclear)
decay.
• An unstable isotope undergoes
radioactive (or nuclear) decay.
Unstable isotopes are also known
as radioisotopes or radionucleides

17. Uses of Radioactive Isotopes
• Food irradiation
• Archaeological dating (carbon-dating)
• Smoke detectors
• Radioactive tracers

19. NUCLEON NUMBER
electr
ons

20. • Process of emitting energy in the forms of
waves or particles.

21. • In nucleus there are two types of forces

22. • Stable isotopes:
• They do not naturally decay but exist in
natural materials in differing proportions
• Unstable iso tope
• Isotopes that continously break down into
lower atomic weight isotopes