ATOMIC MASS AND MASS NUMBER
ATOMIC NUMBER
- number of protons in the nucleus of an atom.
eg. oxygen - 8
sodium - 11
MASS NUMBER
sum of protons and neutrons in an atom.
eg.
sodium- 23
number of protons=11
number of neutrons = 12
thus mass number=23
All atoms of one element have the same number of protons
but may have different number of neutrons
thus different mass numbers.
MASS NUMBER IS WRITTEN ON THE TOP LEFT SIDE OF THE ELEMENT
eg. 23
Na
ISOTOPES
atoms of an element having different number of neutrons and thus different mass numbers
Most isotopes are stable which means that their nuclear structure doesnot change over.
eg.
The stable isotopes of oxygen are designated as 16 17 18
O, O, O
or O-16, O-17, 0-18
Although the isotopes of an element have different number of neutrons, they have identical chemical properties because they have the same number of electrons.
RADIO ACTIVE ISOTOPES
Isotopes that are unstable
their nuclei decay or spontaneously charge into a stable configuration
eg.
H-3
C-14
O-15
O-19
As they decay
they emit radiation
either subatomic particles or packets of energy
and in this process often transforms into a different element.
eg.
C-14 ,the radio active isotope of carbon, decays into N-14
The decay of a radio isotope may be as fast as a fraction of a second
OR as slow as millions of years.
HALF LIFE OF AN ISOTOPE
Time required for half of the radioactive atoms in a sample of that isotope to decay into a stable form
eg. The half life of C-14 = 5600 years
The half life of I-131=8 days.
Some uses of radio active isotopes
a. C-14 -
used to determine the age of organic samples.
RADIO ISOTOPES AS TRACERS
1. Thalium- 201
used to monitor blood flow through the heart during an exercise stress test.
2. I-131
used to detect cancer of the thyroid gland
to assess its size nad activity.
to destroy part of na overactive thyroid gland.
3. Cesium-n 137
used to treat advanced cervical cancer
4. Iridium
used to treat prostate cancer.
ATOMIC MASS / ATOMIC WEIGHT OF AN ELEMENT
IS THE AVERAGE MASS OF ALL ITS NATURALLY OCCURING ISOTOPES
Typically the atomic mass of an element is close to the mass number of its abundant isotope.
UNIT
The standard unit for measuring the mass of atoms and their subatomic particles is a dalton or atomic mass unit. (amu)
Mas of a neutron = 1.008 daltons.
Mass of a proton = 1.007 daltons.
Mass of an electron = 0.0005 daltons.
= 2000 times smaller than the mass of a neutron or proton.
eg.
sodium
number of neutrons= 12
number of protons= 11
atomic number= 11
mass number= 23
atomic mass= 22. 99
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