3.1.1 Atomic Structure Flashcards

1
Q

Shrodinger idea of Atom

A

Cloud showing probabe location of electrons

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2
Q

Isotopes

Chemical and physical properties

A

Chemical reactions: same electron configuration so turns into same ion

Physical: different mass so greater force if attraction so higher m.p. and dencity

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3
Q

Stages of mass spectrometer

A
  1. Ionization
  2. acceleration
  3. ion drift
  4. In detection
  5. Data analasis
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4
Q

Electron impact ionization

A

Vaparised, electron fired from electron gun, electron knocked of atom, positively charged ion

  • used on low formula mass so no fragmentation from impact happens

(X + e- –> X+ + 2e-)

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5
Q

Electrospray ionization

A

Dissolved in volatile solvent, through hypodermic needle (attached to positive terminal with high volts), partical picks up proton from solvent

  • used for higher Mr (soft ionization techniques with fragmentation being rare)

(Xg + H+ –> XH+g) adds a H so +1 Mr

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6
Q

Acceleration

A

Plates of fixed electric feild strength push the ions giving them the the same Ek

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7
Q

Ion drift

A

Light particles are faster so reach detector first
Heavy particles are slower so reach later

Ek=½mv² (Ek is constant so m= k/v²)

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8
Q

Ion detection

A

Ion picks up e- from detector so current flows

Number of ions= k×current
Then converted into spectrometer
Time taken to hit detector also recorded to find speed

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9
Q

Data analasis

A

Sum of (% × Ar)/100

Find probability of having certain moleculeby
%1 × %2

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10
Q

Electron in sub levels for Chromium and Copper

A

Cr: [Ar] 4s¹ 3d⁵
Cu: [Ar] 4s¹ 3d¹⁰

Half full/ full 3d level gives atom more stability

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11
Q

Electronic configuration on Fe²+

A

Remove furthest s shell first

[Ar] (4d⁰) 3d⁶

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12
Q

Ionization energy definition

A

Enthalpy change to remove 1 mile of gaseous e- from 1 mile of gaseous atom to produce 1 mole of gaseous ions

Xg –> X+g + e-

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13
Q

1st Ionisation energies down the group

A

Ionisation energy decreases going down the group

Electrons further away from nucleus and more sheilded

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14
Q

1st ionization energies across the periodic table

A
  • overall all increase -Same quantum level but greater nuclear charge so stronger pull and smaller atomic radius
  • drop at start of p group and doubling in p group
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15
Q

2nd ionization energy

A

Enthalpy change to remove 1 mole of electrons from 1 mole of gaseous 1+ ion to make 1 mole of gaseous 2+ion

X+ –> X2+ + e-

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16
Q

Subsequent ionization energies

A

Xa+ –> X(a+1)+ + e-

17
Q

Rules for which particle has greater ionization energy

A
  • change in orbital/quantum level, larger atomic radius
  • greater nucleic charge, for same sheilding smaller atomic radius
  • p4 pairing of electron creating repulsion