3.1.1 Atomic Structure

Question 1

Shrodinger idea of Atom

Answer 1

Cloud showing probabe location of electrons

Question 2

Isotopes

Chemical and physical properties

Answer 2

Chemical reactions: same electron configuration so turns into same ion

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

Question 3

Stages of mass spectrometer

Answer 3

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

Question 4

Electron impact ionization

Answer 4

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-)

Question 5

Electrospray ionization

Answer 5

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

Question 6

Acceleration

Answer 6

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

Question 7

Ion drift

Answer 7

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

Ek=½mv² (Ek is constant so m= k/v²)

Question 8

Ion detection

Answer 8

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

Question 9

Data analasis

Answer 9

Sum of (% × Ar)/100

Find probability of having certain moleculeby
%1 × %2

Question 10

Electron in sub levels for Chromium and Copper

Answer 10

Cr: [Ar] 4s¹ 3d⁵
Cu: [Ar] 4s¹ 3d¹⁰

Half full/ full 3d level gives atom more stability

Question 11

Electronic configuration on Fe²+

Answer 11

Remove furthest s shell first

[Ar] (4d⁰) 3d⁶

Question 12

Ionization energy definition

Answer 12

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-

Question 13

1st Ionisation energies down the group

Answer 13

Ionisation energy decreases going down the group

Electrons further away from nucleus and more sheilded

Question 14

1st ionization energies across the periodic table

Answer 14

• 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

Question 15

2nd ionization energy

Answer 15

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-

Question 16

Subsequent ionization energies

Answer 16

Xa+ –> X(a+1)+ + e-

Question 17

Rules for which particle has greater ionization energy

Answer 17

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