ib chemistry atomic theory. atomic structure atoms are very small ~ 10 -10 meters all atoms are made...
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IB Chemistry
ATOMIC THEORY
Atomic Structure
Atomic StructureAtoms are very small ~ 10-10 metersAll atoms are made up of three sub-atomic particles: protons, neutrons and electrons
The protons and neutrons form a small positively charged nucleus
The electrons are in energy levels outside the nucleus
Atomic StructureThe actual values of the masses and charges of the sub-atomic particles are shown below:
A meaningful way to consider the masses of the sub-atomic particles is to use relative masses
Atomic Structure - Definitions
Atomic number (Z) is the number of protons in the nucleus of an atom. The number of protons equals the number of electrons in a neutral atom
N.B. No. of protons always equals the no. of electrons in any neutral atom of an element.
Mass number (A) is the sum of the number of protons and the number of neutrons in the nucleus of an atom.
No. of neutrons = Mass number – atomic number
So how can you work out the number of neutrons in an atom?
Atomic Structure - Example
No. of neutrons = Mass number – atomic number
No. of neutron = Mass No. – Atomic No.
= 23 – 11
= 12
So how can you work out the number of neutrons in an atom?
Example
Atomic Structure - Questions
1. What are the three sub atomic particles that make up the atom?
2. Draw a representation of the atom and labelling the sub-atomic particles.
3. Draw a table to show the relative masses and charges of the sub-atomic particles.
4. State the atomic number, mass number and number of neutrons of: a) carbon, b) oxygen and c) selenium.
5. Which neutral element contains 11 electrons and 12 neutrons?
Atomic Structure - Questions
5. Copy and complete the following table:
Summary Slide
All atomic masses are relative to the mass of carbon-12.
Eg one hydrogen atom weighs 1/12 the mass of a carbon-12 atom.
IsotopesIsotopes are atoms of the same element with the same atomic number, but different mass numbers, i.e. they have different numbers of neutrons.
Each atom of chlorine contains the following:
Cl Cl3517
3717
17 protons17 electrons18 neutrons
17 protons17 electrons20 neutrons
The isotopes of chlorine are often referred to as chlorine-35 and chlorine-37
IsotopesIsotopes of an element have the same chemical properties because they have the same number of electrons. When a chemical reaction takes place, it is the electrons that are involved in the reactions.However isotopes of an element have the slightly different physical properties because they have different numbers of neutrons, hence different masses.The isotopes of an element with fewer neutrons will have:
Lower masses • faster rate of diffusion Lower densities • lower melting and boiling points
Isotopes - Questions
1. Explain what isotopes are using hydrogen as an example.
2. One isotope of the element chlorine, contains 20 neutrons. Which other element also contains 20 neutrons?
3. State the number of protons, electrons and neutrons in:a) one atom of carbon-12b) one atom of carbon-14c) one atom of uranium-235d) one atom of uranium-238
Mass SpectrometerThe mass spectrometer is an instrument used:
To measure the relative masses of isotopes To find the relative abundance of the isotopes
in a sample of an element
When charged particles pass through a magnetic field, the particles are deflected by the magnetic field, and the amount of deflection depends upon the mass/charge ratio of the charged particle.
Mass Spectrometer – 5 Stages
Once the sample of an element has been placed in the mass spectrometer, it undergoes five stages.Vaporisation – the sample has to be in gaseous form. If the sample is a solid or liquid, a heater is used to vaporise some of the sample.
X (s) X (g)
or X (l) X (g)
Mass Spectrometer – 5 Stages
Ionization – sample is bombarded by a stream of high-energy electrons from an electron gun, which ‘knock’ an electron from an atom. This produces a positive ion: X (g) X + (g) + e-
Acceleration – an electric field is used to accelerate the positive ions towards the magnetic field. The accelerated ions are focused and passed through a slit: this produces a narrow beam of ions.
Mass Spectrometer – 5 Stages
Deflection – The accelerated ions are deflected into the magnetic field. The amount of deflection is greater when:
• the mass of the positive ion is less• the charge on the positive ion is greater• the velocity of the positive ion is less• the strength of the magnetic field is greater
Mass Spectrometer
If all the ions are travelling at the same velocity and carry the same charge, the amount of deflection in a given magnetic field depends upon the mass of the ion.For a given magnetic field, only ions with a particular relative mass (m) to charge (z) ration – the m/z value – are deflected sufficiently to reach the detector.
Mass Spectrometer
Detection – ions that reach the detector cause electrons to be released in an ion-current detectorThe number of electrons released, hence the current produced is proportional to the number of ions striking the detector.The detector is linked to an amplifier and then to a recorder: this converts the current into a peak which is shown in the mass spectrum.
Atomic Structure – Mass Spectrometer
Name the five stages which the sample undergoes in the mass spectrometer and make brief notes of what you remember under each stage.Complete Exercise 4, 5 and 6 in the handbook. Any incomplete work to be completed and handed in for next session.
Atomic Structure – Mass Spectrometer
Isotopes of boron
m/z value 11 10
Relative abundance %
18.7 81.3
Ar of boron = (11 x 18.7) + (10 x 81.3) (18.7 + 81.3)
= 205.7 + 813 100
= 1018.7 = 10.2 100
Mass Spectrometer – Questions
A mass spec chart for a sample of neon shows that it contains: 90.9% 20Ne 0.17% 21Ne 8.93% 22Ne
Calculate the relative atomic mass of neon
You must show all your working!
Mass Spectrometer – Questions
90.9% 20Ne 0.17% 21Ne 8.93% 22Ne
(90.9 x 20) + (0.17 x 21) + (8.93 x 22)
100
Ar= 20.18
Mass Spectrometer – Questions
Calculate the relative atomic mass of lead
You must show all your work!
m/e
204 206 207 208
52.3
23.622.61.5
Mass Spectrometer – Questions
1.5% 204Pb 23.6% 206Pb 22.6% 207Pb 52.3% 208Pb
(1.5 x 204) + (23.6 x 206) + (22.6 x 207)+(52.3 x 208)
100306 + 4861.6 + 4678.2 +
10878.4100
20724.2100
Ar= 207.24
Ionization Energy
Ionization of an atom involves the loss of an electron to form a positive ion.The first ionization energy is defined as the energy required to remove one mole of electrons from one mole of atoms of a gaseous element.The first ionization energy of an atom can be represented by the following general equation:
X(g) X+ + e- ΔH > 0Since all ionizations requires energy, they are endothermic processes and have a positive enthalpy change (ΔH) value.
Ionization EnergyThe value of the first ionization energy depends upon two main factors:The size of the nuclear chargeThe energy of the electron that has been removed (this depends upon its distance from the nucleus)
Ionization EnergyAs the size of the nuclear charge increases the force of the attraction between the negatively charged electrons and the positively charged nucleus increases.
+ +Small
nuclear charge
Large nuclear charge
Small force
of attraction
Smaller ionization
energy
Large force of
attractionGreater
ionization energy
Ionization energy
As the energy of the electron increases, the electron is farther away from the nucleus. As a result the force of attraction between the nucleus and the electron decreases.
+Electrons closer
to positive nucleus
Large force of attraction
Greater ionizati
on energy
Electrons further away from positive
nucleusSmall force of
attraction
Smaller ionizati
on energy
+
Ionization energy - Questions
Write an equation to represent the first ionization of:
a) aluminiumb) lithiumc) sodium
Trends across a PeriodGoing across a period, the size of the 1st ionisation energy shows a general increase.This is because the electron comes from the same energy level, but the size of the nuclear charge increases.
+ + + +
Going across a Period
Trends across a Period (2 exceptions)
The first ionisation of Al is less than that of Mg, despite the increase in the nuclear charge. The reason for this is that the outer electron removed from Al is in a higher sub-level: the electron removed from Al is a 3p electron, whereas that removed from Mg is a 3s.
Electronic structureIonisation energy/kJ mol-1
Na 1s2, 2s2, 2p6, 3s1 494
Mg 1s2, 2s2, 2p6, 3s2 736
Al 1s2, 2s2, 2p6, 3s2, 3p1 577
Si 1s2, 2s2, 2p6, 3s2, 3p2 786
P 1s2, 2s2, 2p6, 3s2, 3p3 1060
S 1s2, 2s2, 2p6, 3s2, 3p4 1000
Cl 1s2, 2s2, 2p6, 3s2, 3p5 1260
Ar 1s2, 2s2, 2p6, 3s2, 3p6 1520
Trends across a Period (2 exceptions)
The first ionisation energy of S is less than that of P, despite the increase in the nuclear charge. In both cases the electron removed is from the 3p sub-level. However the 3p electron removed from S is a paired electron, whereas the 3p electron removed from P is an unpaired electron. When the electrons are paired the extra mutual repulsion results in less energy being required to remove an electron, hence a reduction in the ionisation energy.
3s
3p
Phosphorus
3s
3p
Sulphur
Trends across a Period - Questions
Now take a look at the graph below:
a) Explain what the graph shows in as much detail as possible
b) There is one other break in the general pattern going across a Period. What is it and explain why that is.
0
500
1000
1500
2000
2500
3000
0 5 10 15 20 25
Atomic number (Z)
Fir
st io
nis
atio
n
en
erg
y/kJ
mo
l-1
H
He
Li
Be
B
CN
O
F
Ne
Na
Mg
AlSi
P
S
ClAr
K
Ca
Trends down a Group+
+
+
+
Dow
n th
e G
rou
p
Ionization energy decreases going down a Group.Going down a Group in the Periodic Table, the electron removed during the first ionization is from a higher energy level and hence it is further from the nucleus.The nuclear charge also increases, but the effect of the increased nuclear charge is reduced by the inner electrons which shield the outer electrons.
Ionization energy - Questions
1. Explain why sodium has a higher first ionization energy than potassium.
2. Explain why the first ionization energy of boron is less than that of beryllium.
3. Why does helium have the highest first ionisation energy of all the elements?
4. Complete Tasks
Successive Ionization energy
Definition: 2nd i.e.The energy per mole for the process X+
(g) X2+(g) +e-
And so on for further successive ionisation energies
Successive Ionization energy
Successive i.e’s increases because electrons are being removed from increasingly positive ions.
Therefore, nuclear attraction is greater.
Large jumps seen when electron is removed form a new sublevel closer to the nucleus
Successive Ionization energy
Succesive ionisation energies of Calcium
0
1
2
3
4
5
6
0 2 4 6 8 10 12 14 16 18 20
Number of electron removed
2nd i.e higher than first – electron has greater pull from nucleus
Large increase between 4th and 3rd shells – electron closer to nucleus
Electron Affinity
Energy Change per mole for:
X (g) + e-
X-(g)
That is, for the gaseous atoms to gain an electron to form anions
Electron Affinity
The first e.a is negative (exothermic) because the electron is attracted to the positive charge on the atom’s nucleus.
The second e.a is positive (endothermic) because an electron is being added to an ion which is already negative : repulsion occurs