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Chemistry A-Level > 3.1.1 Atomic structure > Flashcards

3.1.1 Atomic structure Flashcards

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1
Q

What is the relative mass, relative charge and location in the atom of a proton?

A
  • 1.
  • 1+.
  • Nucleus.
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2
Q

What is the relative mass, relative charge and location in the atom of a neutron?

A
  • 1.
  • 0.
  • Nucleus.
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3
Q

What is the relative mass, relative charge and location in the atom of an electron?

A
  • 1/1840.
  • -1.
  • Energy levels.
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4
Q

What happens due to the extremely high density in the nucleus?

A
  • Particles within are drawn together by extremely powerful forces.
  • Overcome the repulsion protons have for each other.
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5
Q

What is the atomic number (Z)?

A
  • No. protons in nucleus.
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6
Q

What is the mass number (A)?

A
  • No. protons + neutrons in nucleus.
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7
Q

What are isotopes?

A
  • Same element but have different mass number but same atomic number.
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8
Q

What are the three isotopes of hydrogen?

A
  • Protium.
  • Deuterium.
  • Tritium.
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9
Q

Do isotopes have the same chemical and physical properties?

A
  • Same chemical bc same electron arrangement.
  • Diff physical bc diff masses.
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10
Q

What are the two isotopes of chlorine?

A
  • Chlorine-35.
  • Chlorine-37.
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11
Q

What are the two important isotopes of carbon?

A
  • Carbon-12.
  • Carbon-13.
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12
Q

What is the carbon-12 standard?

A
  • Relative mass is measured against 1/12 of a carbon-12 atom.
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13
Q

What is the relative isotopic mass?

A
  • Mass of single isotope of element relative to 1/12 mass of carbon-12
  • Same as mass number for particular isotope of an element.
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14
Q

Where is the relative isotopic mass derived from?

A
  • Mass spectroscopy where mass of individual isotopes can be determined.
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15
Q

What is the relative atom mass (Ar)?

A
  • Average mass of an atom of an element relative to 1/12 of mass of carbon-12.
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16
Q

What are the 5 steps of mass spectroscopy?

A
  • Ionisation.
  • Acceleration.
  • Ion drift.
  • Ion detection.
  • Data analysis.
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17
Q

What is mass spectroscopy used for (elements)?

A
  • Determine information about elements and compounds.
  • Determines relative isotopic masses and abundances.
  • This is used to calculate Ar.
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18
Q

How does mass spectroscopy help to identify compounds?

A
  • Identify unknown purified compounds by comparing mass spectrum to those in database.
  • Gives relative molecular mass (Mr).
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19
Q

What are the two methods of ionisation for mass spectroscopy?

A
  • Electron spray ionisation.
  • Electron impact ionisation.
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20
Q

How is the process of electron impact ionisation carried out?

A
  • Sample vapourised then bombarded w e-.
  • E- gun –> hot wire that emits e-.
  • E- knocks e- off particle leaving molecular ion/ M+ ion.
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21
Q

What is the equation for electron impact ionisation?

A
  • X(g) –> X+(g) + e-.
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22
Q

What type of substances is electron impact ionisation used for?

A
  • Elements + substances w lower molecular mass.
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23
Q

What type of substance is electrospray ionisation used for?

A
  • Substances w higher molecular mass.
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24
Q

What type of technique is electrospray ionisation?

A
  • Soft ionisation technique.
  • Fragmentation is unlikely.
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25
Q

How is the process of electrospray ionisation carried out?

A
  • Sample dissolved in polar, volatile solvent.
  • Pumped through hypodermic needle to create charged droplets.
  • Mononuclear ions (single +ive charge).
  • Ionised by gaining proton.
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26
Q

What is the equation for electrospray ionisation?

A
  • X(g) + H+ –> XH+(g).
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27
Q

What happens during acceleration during mass spectroscopy?

A
  • Negative electrical field attracts ions + give constant KE.
  • KE=1/2mv^2.
  • All same KE so heavier particles travel slower than lighter particles.
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28
Q

What happens during ion drift during mass spectroscopy?

A
  • Region where no electrical field –> flight tube.
  • Ions separated based on diff velocities.
  • Small travel fast through flight tube + arrive at detector first.
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29
Q

What happens during data analysis during mass spectroscopy?

A
  • Flight times analysed + recorded by data analyser.
  • Mass spectrum obtained as plot of relative abundance against mass to charge ratio (m/z).
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30
Q

What does a trace from a mass spectrum show (axis)?

A
  • Series of peaks vertically which show relative abundance.
  • Horizontal axis - mass to charge ratio.
  • relative abundance - how many of each ion is present.
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31
Q

What can sometimes be seen on a trace from mass spectroscopy when electron impact ionisation has been used?

A
  • Cause diff peaks due to fragmentation caused by impact.
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32
Q

What is really important to remember when calculating an Ar from a mass spectrum (esp electro spray ionisation)?

A
  • Take an average from the abundance.
  • Also element - take off a proton that was added during mass spec!!!
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33
Q

How to read a trace from mass spec of a molecular elememt?

A
  • Some exist as diatomic molecules so divide by 2.
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34
Q

How to read a trace from mass spec of a compound?

A
  • Last major peak is molecular ion.
  • M/z value for this peak is Mr of the compound.
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35
Q

What is the largest peak on a mass spec trace called?

A
  • Base peak.
  • Most stable ion produced as molecules is broken up.
36
Q

How are elements (and compounds) detected from mass spectra?

A
  • m/z values entered into computer.
  • Compared to database.
  • This requires pure sample.
37
Q

What is an energy level and what is it split into?

A
  • E- shells.
  • Split into sub-shells.
38
Q

What happens to the distance between energy levels as you move away from the nucleus?

A
  • Energy levels get closer together.
39
Q

What is an energy level split into?

A
  • Sub-shells.
40
Q

What is a sub-shell made up of?

A
  • Orbitals or a combination of orbitals.
41
Q

What is an orbital?

A
  • 3D space that can hold up to 2 e-.
42
Q

What happens in an orbital to minimise repulsion?

A
  • e- in same orbital spin in different directions.
43
Q

What are the 4 types of orbitals?

A
  • s, p, d and f.
44
Q

How many s, p and d orbitals are there at each energy level?

A
  • s –> 1.
  • p –> 3.
  • d –> 5.
45
Q

What are important features of filling sub-shells?

A
  • Distance between sub-shells decreases further away from nucleus –> causes overlap.
  • e- fill sun-shells closer to the nucleus first.
46
Q

What do the up and down arrows in e- configuration represent?

A
  • Direction of spin of e- in orbitals.
47
Q

What is the ground state?

A
  • When e- are in their lowest possible energy levels.
48
Q

Why do e- prefer not to be in orbitals together?

A
  • Because this causes a repulsion between the e-.
49
Q

What are the two elements which are exceptions to e- configuration?

A
  • Copper + Chromium.
50
Q

What happens when metals form ions?

A
  • When the loose e- loose from outermost level except d-block elements.
51
Q

How do you name a non-metal ion?

A
  • Use atom as stem and ‘-ide’ on end.
52
Q

What are the two ions that can be formed from hydrogen?

A
  • H+ –> hydrogen ion.
  • H- –> hydride ion.
53
Q

What does isoelectronic mean?

A
  • Particles which have the same e- configuration.
54
Q

What will elements in the main groups usually form ions of?

A
  • The nearest noble gas.
55
Q

What is the process of ionisation?

A
  • Process of removing e- from atoms and ions.
56
Q

What is the definition of the first ionisation energy?

A
  • Energy required to remove 1 mole of e- from 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions.
57
Q

How is the first ionisation of sodium represented?

A
  • Na(g) –> Na+(g) + e-.
58
Q

How is the second ionisation of sodium represented?

A
  • Na+(g) –> Na2+(g) + e-.
59
Q

How is the third ionisation of sodium represented?

A
  • Na2+(g) –> Na3+(g) + e-.
60
Q

How does ionisation in plasma televisions happen?

A
  • Electrical current runs through.
  • +ively charged ions collide w e- causing them to release ultraviolet photons that react to release visible light.
61
Q

What are the units for ionisation energy?

A
  • Kj mol-1.
62
Q

Is ionisation an endothermic or exothermic reaction?

A
  • Endothermic as energy is required to remove an electron from attractive power of nucleus.
63
Q

How are the existence of energy levels proven?

A
  • Large gaps between successive ionisation energies.
  • Correspond to removal of e- from energy levels closer to nucleus so more energy required to remove.
64
Q

What is effective nuclear charge?

A
  • General increase in successive ionisation energies caused by increase in ratio of protons to e- as e- are removed.
65
Q

What can successive ionisation energies be used for?

A
  • Can be used as indicator of the group the element belongs to.
66
Q

What are the 3 trends in ionisation energies?

A
  • Ionisation energy decreases down the group.
  • Ionisation energy generally increases across the period.
  • Within short periods (2+3) there is a zig-zag pattern.
67
Q

Which elements cause a zig-zag in the ionisation energies?

A
  • Group 3 –> boron + aluminium.
  • Group 6 –> oxygen + sulphur.
68
Q

What are the three factors that can be used to explain trends in ionisation energies?

A
  • Atomic radius.
  • Nuclear charge.
  • Shielding by inner e-.
69
Q

What is atomic radius and how does this vary down a group and across a period?

A
  • How far the outer e- are from the attractive power of the nucleus.
  • Increase down group.
  • Decrease across period.
70
Q

How does atomic radius affect ionisation energy?

A
  • The further the outermost e- is from attractive power of nucleus, the less energy is required to ionise it.
71
Q

What is nuclear charge and how does this affect ionisation energy?

A
  • How many protons are attracting the outer e-.
  • Greater nuclear charge leads to a stronger attraction to the outer e- so more energy is required to ionise it.
72
Q

What is shielding and how does this affect ionisation energy?

A
  • How many e- are between outer e- and attractive power of nucleus.
  • More inner e- means more shielding + less energy is required to ionise outer e-.
73
Q

What happens to ionisation energy down the group?

A
  • Decreases.
  • Atomic radius - increases so easier to loose outer e-.
  • Shielding by inner e- - more shells so more shielding so easier to loose outer e-.
  • Nuclear charge - increases so works against other 2 factors.
74
Q

What happens to ionisation energy across the period?

A
  • Increases.
  • Atomic radius - decreases outer e- has more protons to attract.
  • Shielding - constant due to same energy level.
  • Nuclear charge - increases due to more protons.
75
Q

Why is there a dip in ionisation energy at aluminium?

A
  • 3p1 e- is further from the nucleus + has additional shielding from 3s2 so requires less energy for ionisation.
76
Q

Why is there a dip in ionisation energy at sulphur?

A
  • Due to paring of e- in p sub-shell.
  • 3p4 means that 2 e- are paired in 1st p orbital.
  • Repulsion between e- lowers ionisation energy required to move an e-.
77
Q

What provides evidence that 2nd + 3rd energy levels are divided into 2 sub-shells?

A
  • Atoms in group 3 + 6 w lower ionisation energies show that 1st sub-shell has 1 orbital and 2nd has 3 orbitals.
78
Q

Why do group 1 elements have the lowest first ionisation energy in each period?

A
  • Greatest atomic radius + lowest nuclear charge in each period.
79
Q

Why do group 0 elements have the highest first ionisation energy in each period?

A
  • Smallest atomic radius.
    • highest nuclear charge in period.
80
Q

What is the general pattern for ionisation energy down the group?

A
  • Decreases.
  • Atomic radius increases.
  • Shielding by inner e- increases.
  • Less energy required to remove e-.
81
Q

What is the general pattern for ionisation energy across the period?

A
  • Increases.
  • Atomic radius decreases.
  • Nuclear charge increases.
  • Shielding by inner e- stays the same.
  • More energy required to remove e-.
82
Q

Why are there lower 1st ionisation energies than expected in group 3?

A
  • Group 3 have s2p1 arrangement.
  • Outer p1 further from nucleus.
  • Inner s2 e- increase shielding so less energy required to ionise outer p1 e-.
83
Q

Why are there lower 1st ionisation energies than expected in group 6?

A
  • Group 6 have p4 arrangement.
  • Repulsion between 2 e- in p orbitals leads to less energy being required to ionise the outer e-.
84
Q

What are the patterns in 2nd ionisation energies?

A
  • Shifted one to the left.
  • Group 1 element would have lowest 1st ionisation but would have highest 2nd ionisation energy.
85
Q

Why do group 1 elements have the highest 2nd ionisation energies?

A
  • 2nd e- is being removed from an energy level closer to the nucleus.

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