3.1.1 Atomic Structure Flashcards

1
Q

Mass number definition

A

Total number of protons and neutrons in an atom. Known as A

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2
Q

Proton/atomic number definition

A

Number of protons in an atom. Known as Z.

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3
Q

Mass of a proton, neutron and electron

A

Proton: 1
Neutron: 1
Electron: 1/1840

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4
Q

Charge of a proton, neutron and electron

A

Proton: +1
Neutron: 0
Electron: -1

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5
Q

5 steps of TOF

A
  1. Ionisation
  2. Acceleration
  3. Ion drift
  4. Ion detection
  5. Data analysis
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6
Q

What information does TOF give

A

Relative isotopic mass
Relative isotopic abundance

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7
Q

Two methods of ionisation for TOF

A

Electron impact
Electrospray ionisation

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8
Q

Electrospray ionisation + equation

A
  1. Sample is dissolved in volatile solvent
  2. Injected through hollow needle connected to positive terminal of high voltage supply
  3. Each molecule gains a proton
    M(g) + H+ –> MH+(g)
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9
Q

Electron impact + equation

A
  1. Sample is vaporised
  2. Electron fired at sample
  3. Electrons collide with sample and knock off an electron, forming positive ions
  4. Can cause fragmentation with large molecules
    M+(g) e- –> M+(g) + 2e-
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10
Q

Why is it necessary to ionise samples in TOF

A
  1. Ions will interact with and be accelerated by an electric field
  2. Ions will create a current when they hit the detector
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11
Q

Detection stage of TOF

A
  1. Ions are accelerated towards a negatively charged metal plate
  2. Speed at which they reach the plate depends on their mass
  3. Positive ion picks up an electron from the detector, inducing a current
  4. The greater the abundance or charge the greater the current
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12
Q

First Ionisation energy

A

The amount of energy needed to remove one mole of electrons from one mole of gaseous atoms, forming a mole of gaseous 1+ ions

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13
Q

Ionisation energy trends

A
  1. Along the period ionisation energy increases as atomic radius decreases, meaning the electrons are more attracted to the nucleus and less easily lost
  2. Down the group ionisation energy decreases as shielding and atomic radius increases, so electrons are less attracted to the nucleus and more easily lost
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14
Q

Explain the pattern in the first ionisation energies of the elements from lithium to
neon. (6)

A

General trend
1. Ionisation energy generally increases along the period
2. Due to smaller atomic radius
3. And similar shielding

Deviation Be to B
4. B lower than Be
5. 2p sub shell is of higher energy than 2s sub shell

Deviation N to O
6. O lower than N
7. As it has paired electrons which repel each other

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15
Q

Relative atomic mass definition

A

Average mass of an atom of an element compared to 1/12 the mass of a carbon 12 atom

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16
Q

Relative molecular mass definition

A

Average mass of a molecule compared to 1/12 the mass of a carbon 12 atom.

17
Q

Relative formula mass definition

A

Average mass of an ionic compound compared to 1/12 the mass of a carbon 12 atom.

18
Q

What is Avogadro’s constant

A

The number of particles in a mole
6.022x10^23

19
Q

How are moles calculated

A

Moles = Mass/Mr
Moles = concentration x volume

20
Q

Ideal gas equation

21
Q

Ideal gas equation units

A

P- Pa
V - m^3
n - mol
R - 8.314
T - K

22
Q

Empirical formula definition

A

The simplest whole number ratio of atoms of each element in a compound.

23
Q

Molecular formula definition

A

The actual number of atoms of each element in a compound

24
Q

Percentage atom economy equation

A

(Mr of desired product ÷Mr of reactants) x 100

25
Advantages of high atom economy
Less waste More environmentally friendly More cost effective Greater efficiency
26
Give two difference between the modern model of the atom and the Thomson model
Protons in centre of atom Electrons in shells around nucleus Neutron in the centre of the atom Most of the atom is empty space