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IB Chemistry ATOMIC THEORY

IB Chemistry ATOMIC THEORY. Atomic Structure. Atomic Structure. Atoms are very small ~ 10 -10 meters All atoms are made up of three sub-atomic particles: protons, neutrons and electrons. The protons and neutrons form a small positively charged nucleus

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IB Chemistry ATOMIC THEORY

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  1. IB Chemistry ATOMIC THEORY

  2. Atomic Structure

  3. Atomic Structure • Atoms are very small ~ 10-10 meters • All 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

  4. Atomic Structure • The 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

  5. 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. • So how can you work out the number of neutrons in an atom? No. of neutrons = Mass number – atomic number

  6. Atomic Structure - Example • So how can you work out the number of neutrons in an atom? • Example No. of neutrons = Mass number – atomic number No. of neutron = Mass No. – Atomic No. = 23 – 11 = 12

  7. Atomic Structure - Questions • What are the three sub atomic particles that make up the atom? • Draw a representation of the atom and labelling the sub-atomic particles. • Draw a table to show the relative masses and charges of the sub-atomic particles. • State the atomic number, mass number and number of neutrons of: a) carbon, b) oxygen and c) selenium. • Which neutral element contains 11 electrons and 12 neutrons?

  8. Atomic Structure - Questions 5. Copy and complete the following table:

  9. 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.

  10. 35 17 37 17 Cl Cl Isotopes • Isotopes 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: 17 protons 17 electrons 18 neutrons 17 protons 17 electrons 20 neutrons The isotopes of chlorine are often referred to aschlorine-35andchlorine-37

  11. Isotopes • Isotopes 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

  12. Isotopes - Questions • Explain what isotopes are using hydrogen as an example. • One isotope of the element chlorine, contains 20 neutrons. Which other element also contains 20 neutrons? • State the number of protons, electrons and neutrons in: a) one atom of carbon-12 b) one atom of carbon-14 c) one atom of uranium-235 d) one atom of uranium-238

  13. Mass Spectrometer • The 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.

  14. 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)

  15. 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.

  16. 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

  17. 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.

  18. Mass Spectrometer • Detection – ions that reach the detector cause electrons to be released in an ion-current detector • The 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.

  19. 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.

  20. Atomic Structure – Mass Spectrometer • Isotopes of boron Ar of boron = (11 x 18.7) + (10 x 81.3) (18.7 + 81.3) = 205.7 + 813 100 = 1018.7 = 10.2 100

  21. 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!

  22. (90.9 x 20) + (0.17 x 21) + (8.93 x 22) • 100 Mass Spectrometer – Questions • 90.9% 20Ne • 0.17% 21Ne • 8.93% 22Ne Ar= 20.18

  23. 52.3 23.6 22.6 1.5 m/e 204 206 207 208 Mass Spectrometer – Questions Calculate the relative atomic mass of lead You must show all your work!

  24. (1.5 x 204) + (23.6 x 206) + (22.6 x 207)+(52.3 x 208) • 100 • 306 + 4861.6 + 4678.2 + 10878.4 • 100 • 20724.2 • 100 Mass Spectrometer – Questions • 1.5% 204Pb • 23.6% 206Pb • 22.6% 207Pb • 52.3% 208Pb Ar= 207.24

  25. 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 > 0 • Since all ionizations requires energy, they are endothermic processes and have a positive enthalpy change (ΔH) value.

  26. Ionization Energy • The value of the first ionization energy depends upon two main factors: • The size of the nuclear charge • The energy of the electron that has been removed(this depends upon its distance from the nucleus)

  27. + + Ionization Energy • As 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  Large force of attraction  Smaller ionization energy Greater ionization energy

  28. + + 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 further away from positive nucleus  Electrons closer to positive nucleus  Large force of attraction  Small forceof attraction  Greater ionization energy Smaller ionization energy

  29. Ionization energy - Questions • Write an equation to represent the first ionization of: a) aluminium b) lithium c) sodium

  30. + + + + Trends across a Period • Going 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

  31. 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.

  32. Sulphur Phosphorus 3p     3p    3s   3s   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.

  33. He Ne F Ar N Cl C P Be H O Mg Ca S Si B Li Na Al K Trends across a Period - Questions • Now take a look at the graph below: • Explain what the graph shows in as much detail as possible • There is one other break in the general pattern going across a Period. What is it and explain why that is.

  34. + + + + Trends down a Group 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. Down the Group

  35. Ionization energy - Questions • Explain why sodium has a higher first ionization energy than potassium. • Explain why the first ionization energy of boron is less than that of beryllium. • Why does helium have the highest first ionisation energy of all the elements? • Complete Tasks

  36. 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

  37. 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

  38. Successive Ionization energy Large increase between 4th and 3rd shells – electron closer to nucleus 2nd i.e higher than first – electron has greater pull from nucleus

  39. 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

  40. 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

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