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Chemistry > Atomic structure > Flashcards

Atomic structure Flashcards

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1
Q

What is Ionisation Energy?

A

The minimum amount of energy required to remove a mole of electrons from a mole of atoms in a gaseous state

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2
Q

What are the 3 factors that affect ionisation energy?

A
  • Distance of outer electron to nucleus
  • Shielding
  • Nuclear charge
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3
Q

State the general trend in Ionisation Energy across a period

A
  • General increase
  • Same shielding
  • Increase in protons, which increases nuclear charge, meaning there is a stronger nuclear attraction on the outer electron which requires more energy to lose
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4
Q

State the trend of ionisation energies down a group

A
  • Decrease
  • More shells between nucleus and outer electron shell, increases shielding so there is a weaker nuclear attraction on outer electron which requires less energy to lose
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5
Q

State the trend in atom sizes across a period

A
  • Decrease in size
  • Same shielding
  • Increase in protons so higher nuclear charge, so a greater nuclear attraction on outer electron which pulls the outer shell closer
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6
Q

How many electrons and orbitals are in each block?

A
  • s: 1 orbital and 2 electrons
  • p: 3 orbitals and 6 electrons
  • d: 5 orbitals and 10 electrons
  • f: 7 orbitals and 14 electrons
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7
Q

Which orbitals do electrons fill first?

A
  • Fill orbitals with the lowest energy levels
  • The further away from the nucleus the higher the energy
  • Fill empty orbitals on that energy level first
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8
Q

What is the general rule for electrons in the 4s subshell?

A

First in, first out

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9
Q

What are the exceptions in the 3d subshells and why?

A
  • Chromium: An electron from the 4s subshell goes into the empty orbital in 3d to make it half-full since that is more stable than a partially full subshell
  • Copper: An electron from the 4s subshell goes into the last half full orbital to make the subshell completrely full since that is more stable than a partially full subshell
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10
Q

State the full electronic configuration of Chromuim

A

1s2 2s2 2p6 3s2 3p6 4s1 3d5

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11
Q

State the full electronic configuration of Copper

A

1s2 2s2 2p6 3s2 3p6 4s1 3d10

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12
Q

State the full electronic configuration of Fe2+

A

1s2 2s2 2p6 3s2 3p6 3d6

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13
Q

State the full electronic configuration of Silver

A

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s1 4d10

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14
Q

Which element has the electronic configuration [Kr] 5s1 4d5 ?

A

Molybdenum

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15
Q

How and why does the IE of Boron deviate from the general trend in period 2?

A
  • IE is lower than Beryllium’s
  • The electron to be removed from Be is in 2s subshell whereas the electron from B is in 2p subshell
  • 2p subshell is higher in energy than 2s subshell so less energy is needed to remove the electron from boron
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16
Q

How and why does the IE of Oxygen deviate from the general trend in period 2?

A
  • IE is lower than Nitrogen’s
  • Outer electron in N is unpaired, whereas electron in O is paired
  • Paired electrons repel therefore less energy is needed to remove the electron from Oxygen
17
Q

What are the 2 factors that are measured in Mass Spectrometry?

A
  • Relative abundance of isotopes
  • Mass/charge ratio
18
Q

Why is the inside of a Mass Spectrometer a vacuum?

A

To prevent collision with air particles

19
Q

Why are sample particles ionised?

A
  • So they can be accelerated towards the negatively charged plate
  • So they can generate a current when they hit the detector
20
Q

How is the ion accelerated?

A
  • Positive ions are attracted to the neratively charged plate
  • All ions have the same KE
21
Q

How are ions sperated in the flight tube?

A

Smaller, lighter ions travel faster than larger, heavier ions and move ahead

22
Q

How are ions detected?

A
  • Each ion hits the detector and gains an electron
  • This generates a current
  • The size of this current is proportional to the abundance of the ion
23
Q

How are molecules ionised in electron impact?

A
  • High energy electron
  • From an electron gun is fired at the sample
  • One electron from each particle is knocked off
  • Forms a 1+ ion/ positively charged
24
Q

What is the general formula of an ion which has been ionised by electron impact?

(Use M as your element)

A

M(g) -> M+(g) + e-

25
Q

How are molecules ionised in electro spray?

A
  • Sample dissolved in volatile solvent
  • Passed through hypodermic needle
  • Connected to high voltage power supply to create a fine mist
  • Each particle gains a proton (H+) to form a positive charge
26
Q

What is the formula for kinetic energy?

A

KE = ½ x m x v²

27
Q

What are the 2 formulas for velocity?

A

v = √2KE ⁄ m
v = d ⁄ t

28
Q

What is the formula for mass?

(in terms of KE)

A

m = 2KE ⁄ v²

29
Q

What is Avagadros constant?

A

6.022 x 10^23

30
Q

What is the formula for finding the mass?

(Using the mass number)

A

mass in Kg = mass no. x 10^-3 ⁄Avagadros constant

31
Q

What is the definition of relative atomic mass?

A

A weighted average of all isotopes of an element taking into account their abundance

32
Q

How, if at all, do isotopes of the same elements differ in terms of chemical properties and why?

A
  • They don’t since they have the same electronic configuration
33
Q

What are 2 differences between the plum pudding model and the current model?

A
  • Nucleus contains protons and neutrons
  • Electrons in shells orbiting the nucleus
34
Q

What is the period 3 element witht the highest second ionisation energy?

A

Sodium

- Has full outer shell

35
Q

Explain why a fluoride ion is larger than a sodium ion

(2 marks)

A
  • Same electronic configuration and shielding
  • Fluoride ion has less protons/ lower nuclear charge
  • Weaker attraction between nucleus and outer electrons
36
Q

Why is the second ionisation energy of calcium lower than that of potassium?

(2 marks)

A
  • Outer electron in Ca is further from nucleus/ removed from a higher energy level
  • More shielding in Ca+

Chemistry (13 decks)

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