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Atomic Structure Flashcards

1
Q

Define the atomic no.

A

No. of protons in the nucleus

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2
Q

Define the mass no.

A

Total no. of protons + neutrons in the nucleus

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3
Q

Define isotopes

A

Atoms w/ same no. protons but diff no. of neutrons

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4
Q

What decides the physical properties of an element?

A

Mass of an atom

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5
Q

What decides the chemical properties of an element?

A

No. + arrangement of e-

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6
Q

Isotopes of an element have ____ physical properties

A

Diff

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7
Q

Why do isotopes have the same chemical properties?

A

Same e- configuration

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8
Q

Who discovered the 1st model of the atom + what was it?

A
  • John Dalton
  • Described atoms as solid spheres
  • Diff. spheres made up diff. elements
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9
Q

Who discovered the 2nd model of the atom + what was it?

A
  • JJ Thomson
  • Plum pudding model
  • Discovered e-
  • Showed atoms weren’t solid + indivisible
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10
Q

Who discovered the 3rd model of the atom + what was it?

A
  • Rutherford
  • Nuclear model - tiny +ve charged nucleus surrounded by cloud of -ve e- - most empty
  • Fired +ve charged a-particles at sheet of gold instead of being deflected, most passed straight through
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11
Q

Who discovered the 4th model of the atom + what was it?

A
  • Bohr proposed e- exist in shells of fixed energy
  • When e- move btw shells, electromagnetic radiation is emitted
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12
Q

Define the relative atomic mass (Ar)

A

Average mass of an atom of an element on a scale where an atom of carbon-12 is 12

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13
Q

Define the relative isotopic mass

A

Mass of an atom of an isotope of an element on scale where an atom of carbon-12 is 12

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14
Q

Define the relative molecular mass (Mr)

A

Average mass of a molecule on a scale where an atom of carbon-12 is 12

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15
Q

Describe how an ion is formed in a TOF mass spectrometer

A
  • Electronspray ionisation - high v applied in polar solvent, gains H+ ion
  • Electron impact ionisation - fire high energy e- at sample, knocks e- off, forming +1 ion
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16
Q

What happens in the 2nd stage of mass spectrometery?

A
  • Acceleration
  • +ve charged ions accelerated by electric field
  • Same kinetic energy
  • Lighter ions move faster
17
Q

What happens in the 3rd stage of mass spectrometery?

A
  • Ion drift
  • Ions enter region w/ no electric field, just drifts
  • Lighter ions drift faster
18
Q

Explain how ions are accelerated, detected + have their abundance determined in a TOF mass spectrometer

A
  • Accelerated by attraction to +ve charged plate
  • Detected by gaining e-
  • Abundance determinded by size of current flowing in detector
19
Q

Explain how a current is formed (3)

A
  • +ve ions hit +ve metal plate
  • E- flow to +ve ion
  • Current produced
  • Current proportional to abundance
20
Q

Suggest what might cause the relative atomic of a sample to be diff from the relative atomic mass given in the periodic table (1)

A

Some isotopes absent/takes into account other isotopes

21
Q

Why is it necessary to ionise molecules when measuring their mass in TOF mass spectrometer? (2)

A
  • Only ions will interact w/ + be accelerated by electric field
  • Only ions create current when hitting detector
22
Q

Explain how TOF mass spectrometery distinguishes btw ions w/ diff masses (3)

A
  • +ve ions accelerated by electric field
  • To constant kinetic energy
  • Lighter ions move faster
  • Faster ions arrive first at detector
23
Q

Outline how to work out relative atomic mass from a mass spectrum

A
  • Multiply abundance + x axis
  • Add up total
  • Divide by total abundance
24
Q

Give the full electronic configuration of chromium

A

[Ar] 4s13d5

25
Q

Give the full electronic configuration of copper

A

[Ar] 4s13d10

26
Q

What happens when a transition metal become ions?

A

Lose 4s e- before 3d

27
Q

Define the 1st ionisation energy

A

Energy needed to remove 1 e- from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

28
Q

What is the equation for the 1st ionisation energy?

A

x (g) → x+ (g) + e-

29
Q

What are the factors affecting ionisation energy?

A
  • Nuclear charge - more protons = stronger FOA
  • Distance from nucleaus - closer
  • Shielding - less e-
30
Q

Define high ionisation energy

A

High attraction btw e- + nucleus so more energy needed to remove e-

31
Q

Define the 2nd ionisation energy

A

Energy needed to remove 1 e- from each ion in 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions

32
Q

What is the equation for the 2nd ionisation energy?

A

x(n-1)+ (g) → xn+ (g) + e-

33
Q

Explain why the 2nd ionisation energy is higher than the 1st ionisation energy?

A
  • More energy needed to remove e- from more +ve ion
  • Less repulsion
  • Stronger FOA
34
Q

Explain the ionisation energy trend in group 2

A
  • Dec
  • Atom radius inc
  • More sheilding
35
Q

Explain the general trend in ionisation energy across period 3

A
  • Inc
  • More protons
  • Same shielding
  • Stronger FOA for outer e-
36
Q

Explain why a deviation occurs btw group 2 + 3 first ionisation energy in period 3 (3)

A
  • Al lower than Mg
  • Outer e- in 3p orbital
  • 3p is higher in energy
37
Q

Explain why a deviation occurs btw group 5 + 6 first ionisation energy in period 3 (3)

A
  • S lower than P
  • Outer e- in 3p orbital begin to pair
  • Electron pair repulsion

Chemistry Physical (11 decks)

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