PHYS1006 Lecture Notes - Lecture 19: Mass Spectrometry, Electronvolt, Hydrogen Atom

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indigozebra538

25 Jun 2018

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Zia Palmer

19130064

PHYS1006

Atomic and Nuclear Radiation

Learning outcomes:

Structure of the nucleus

Binding energy

Nuclear force

Radioactivity

Types of nuclear radiation

Structure and Properties of the Nucleus

Nucleus: densely packed centre of an atom composed of PROTONS and NEUTRONS.

PROTONS have a positive charge:

NEUTRONS are essentially neutral:

Collectively, neutrons and protons are called nucleons.

Different nuclei are referred to as nuclides.

Nuclides are symbolised as follows:

where ‘X’ is the chemical symbol for the element.

Isotopes: nuclides that have the same atomic number, but a different mass number.

Radius of a Nucleus

Where is the Mass number

Diameter of a Nucleus

Where is the Mass number

Example 1

Find the diameter of the following

= 1

1 femotometer =



= 56

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Document Summary

Nucleus: densely packed centre of an atom composed of protons and neutrons. Nuclides are symbolised as follows: where x" is the chemical symbol for the element. Isotopes: nuclides that have the same atomic number, but a different mass number. Nuclear mass is measured using a mass spectrometer and is expressed with reference to the mass of a carbon-12 atom, which is assigned a mass of exactly 12u, where 1u is an atomic mass unit defined as: Atomic mass expressed in grams is called molar mass. Masses can also be expressed in terms of their energy equivalent. The total mass of a nucleus is always less than the mass of the protons and neutron in it. The mass difference is a measure of the be that holds the nucleus together. A helium nucleus is made up of two protons and two neutrons. Calculate the be of the helium nucleus using the following atomic masses.

Related Questions

Which of the following statements are true about nuclei and thenuclear force?

1)The nuclear force is a short-range repulsive force.
2)The nuclear force is weaker than the electric (Coulomb)force.
3)The mass number (A) indicates the number of nucleons in anucleus.
4)Isotopes are nuclei that have the same number of neutrons, butdifferent numbers of protons.
5)There are Z protons in a nucleus (where Z is atomicnumber).
6)The chemical symbol is determined by the atomic mass number, A.

A nuclear reaction is represented by an equation similar to theequation for a chemical reaction. An example of a nuclear reactionis the decay of radium into radon by the emission of an alphaparticle (a helium nucleus). The equation for this reactionis

^{226}_{\ 88}{\rm Ra}\; \rightarrow \, ^{222}_{\ 86}{\rmRn}+\;^4_2{\rm He}.

The superscript preceding each element indicates the nucleon numberof that particular nucleus (total number of protons and neutrons).The subscript indicates the charge of the nucleus, which is equalto the atomic number for nuclei. Nuclear reactions frequentlyinvolve electrons (sometimes called beta rays) and photons(sometimes called gamma rays). Electrons, which have nucleon number0 and charge -1, are represented in equations as either ^{\ \;0}_{-1}\beta or ^{\ \; 0}_{-1}{\rm e}. Photons are represented as^{0}_{0}\gamma to emphasize that they have no nucleon number andcarry no charge.

In nuclear reactions, several conservation laws are usuallysufficient to determine the products or reactants. One of these isconservation of nucleon number. The total number of neutrons andprotons in all of the reactants must be the same as the totalnumber of protons and neutrons in the products. Although protonsand neutrons sometimes change into one another, neither can simplydisappear. Another important conservation law is conservation ofcharge. The net charge of the reactants must be the same as that ofthe products.

Notice that, in our equation for the decay of radium, the sum ofthe nucleon numbers on each side is 226 and the sum of the chargeson each side is 88. If you knew everything in this equation exceptthe isotope of radon produced, you could simply subtract 4 from 226to find the nucleon number required to make the nucleon number ofthe products equal the nucleon number of the reactants. Similarly,if you knew everything in this equation except for the identity ofthe product element, you could simply subtract 2 from 88 and thenlook in a periodic table to find that the element with atomicnumber 86 is radon.

In parts A and B consider the decay of radon by alpha particleemission:

^{222}_{\ 86}{\rm Rn}\;\rightarrow\;X +\,^{4}_{2}{\rm He}.

a. What is the nucleon number of the element X?
Express your answer as an integer.

b. What is the atomic number (nuclear charge) of the elementX?
Express your answer as an integer.

n parts C and D consider the decay of Potassium-43 into calcium-43via the following reaction:

^{43}_{19}{\rm K} \rightarrow ^{43}_{20}{\rm Ca}+\,X.

c. What is the charge of the emitted particle X?
d. is not visible yet

E. An isotope of potassium with a half-life of roughly one billionyears is often used in radioactive dating. This isotope decaysthrough electron capture, the process of drawing an electron intothe nucleus. What is the chemical symbol for the element thatresults from this process? The equation for the reaction is

^{40}_{19}{\rm K}+\,^{\ \;0}_{-1}{\rm e}\rightarrow \,?.
Express your answer as a chemical symbol (e.g., Na forsodium).

f. The reaction energy of a reaction is the amount of energyreleased by the reaction. It is found by determining the differencein mass between the reactants and products and then using E=mc^2 toconvert the lost mass into the released energy.

Look again at the equation for the decay of radium (Ra), given inthe introduction. Use the following table of masses to determinethe reaction energy of this reaction.
Nucleus or particle Mass in atomic mass units
radium-226 226.025402
radon-222 222.017571
alpha particle 4.002602
Express your answer in joules to three significant figures.

please answer fully... thank you

PHYS1006 Lecture Notes - Lecture 19: Mass Spectrometry, Electronvolt, Hydrogen Atom

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