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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an isotope?

A

An atom with the same no. of protons but a different no. of neutrons

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2
Q

Define relative atomic mass

A

The average mass of an atom of an element relative to 1/12 the mass of a Carbon-12 atom

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3
Q

What is mass spectroscopy used to find?

A

Abundance and mass of each isotope of an element

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4
Q

What are the 2 types of ionisation for TOF mass spectroscopy?

A

Electron Impact, Electrospray Ionisation

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5
Q

Explain how electron impact ionisation works

A
  • Sample is vaporised
  • Electron gun fires high energy electrons
  • One electron from each particle is knocked off, forming +1 ions
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6
Q

Explain how electrospray ionisation works

A
  • Sample is dissolved in volatile solvent
  • Sample is injected through hypodermic needle
  • Positive needle tip ionises particles by gaining a proton
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7
Q

Which type of ionisation is better for biological molecules and why?

A

Electrospray, no fragmentation

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8
Q

Describe how positive ions are accelerated in TOF mass spectroscopy

A
  • Using an electric field until all particles have the same kinetic energy
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9
Q

Explain how the flight tube stage of TOF mass spectroscopy

A
  • Positive ions travel through hole in negative plate and into tube
  • TOF depends on velocity which depends on mass alone
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10
Q

How does the detection phase of TOF mass spectroscopy work?

A
  • Positive ions hit negative plate
  • Positive ions are discharged by gaining electrons
  • Current is generated
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11
Q

How does the detection phase of TOF mass spectroscopy work?

A
  • Positive ions hit negative plate
  • Positive ions are discharged by gaining electrons
  • Current is generated
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12
Q

What are energy levels divided into?

A

Sub shells

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13
Q

How many electrons can a sub-shell hold?

A

2 electrons

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14
Q

How many d-orbitals are there per energy level?

A

5

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15
Q

What is the 1st ionisation energy?

A

The energy required to remove 1e- from an atom of 1mol of gaseous atoms of an element

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16
Q

Why should an element be gaseous?

A

So energy isn’t used breaking bonds between atoms of that element

17
Q

Give the 3 factors affecting ionisation energy

A

Nuclear Charge, Distance from Nucleus, Shielding Effect

18
Q

Explain how nuclear charge affects ionisation energy

A

Stronger positive charges attracts electrons more powerfully

19
Q

How does shielding affects ionisation energy?

A

Electrons on inner shells reduce the effect of proton charge

20
Q

Describe how ionisation energy is affected across the periods

A
  • General increase due to increase in nuclear charge
  • Shielding and nucleus distance are similar
21
Q

How is ionisation energy affected down the group?

A
  • General decrease as shielding and nucleus distance increases
  • Causes weaker attraction to nucleus so ionisation energy decrease
22
Q

Describe the solid sphere model

A
  • Small, hard spheres called atoms
  • Couldn’t be divided
  • Different atoms are different sizes
23
Q

What discovery did Becquerel make?

A

Atoms were divisible as particles are emitted from an unstable nucleus

24
Q

Describe the plum pudding model

A

A sphere of positive charge with negative electrons embedded in it

25
Q

What was the main discovery from the Alpha Scattering Experiment?

A

Most of the atom was empty space

26
Q

Describe the nuclear model

A

A small, concentrated, positive ball of mass surrounded by electrons

27
Q

What did Bohr discover that differed with the nuclear model?

A

Electrons orbit in shells

28
Q

What did Chadwick prove and what did this account for?

A
  • Presence of neutrons
  • Accounted for discrepancy in atomic weights of elements
29
Q

How did Schrodinger affect the previous model of the atom?

A

He realised that electrons orbit at similar energy levels but with different quantities of energy

Chemistry (3 decks)

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