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Chemistry > 1.1 Atomic structure > Flashcards

1.1 Atomic structure Flashcards

1
Q

State two differences between plum pudding model and the model of the atomic structure

A
  1. Central nucleus contains protons and neutrons
  2. Electrons arranged in energy levels / shells / orbitals
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2
Q

Magnesium exists as three isotopes. State how if at all the chemical properties of these isotopes differ

A

No difference in chemical properties because they have the same electronic configuration

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3
Q

Which one of the following out of a proton, neutron and electron is not deflected by an electric field

A

Neutron

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4
Q

Helium particles were fired at a thin sheet of gold. Most of the particles were detected at a point P (to the right of the atom).A few particles were detcted at a point Q (top left of the atom) State what conclusion was made about the helium particles at point P and Point Q

A

P : Most of the gold atoms are mainly empty space.
Q : Gold atoms have a small positive nucleus

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5
Q

Define term mass number

A

Average mass of an element compared to one twelfth of the mass of an atom carbon - 12

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6
Q

Write an equation to represent second ionisation energy of strontium

A

Sr(g)^+ -> Sr(g)^2+ + e^-

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7
Q

Define first ionisation energy

A

The first ionisation energy is the energy needed to remove 1 mole of electrons from a mole of gaseous atoms in the gaseous state to form one mole of gaseous ions with a 1+ charge

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8
Q

Why is the first ionisation energy of strontium larger than the first ionisation energy of rubidium

A

Sr has more protons
They both have the same shielding
Sr has a greater nuclear attraction

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9
Q

Why is the second ionisation energy of rubidium stronger than the second ionisation energy of strontium

A

Second IE of rubidum involves removal of an electron closer to the nucleus
As it has less shielding it has a stronger attraction to the outer electrons

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10
Q

Explain why second ionisation energy of boron is higher than the first ionisation energy of boron

A

Outer electron is removed from a positive ion which requires more energy

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11
Q

Identify element in S block that has the highest first ionisation energy

A

Berylium

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12
Q

Deduce which is a smaller atom Lithium or Berylium

A

Berylium because they have same shielding but berylium has more protons

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13
Q

Deduce which is a smaller atom lithium or hydrogen

A

Hydrogen as it has less shielding

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14
Q

Complete full electron configuration of a chromium atom

A

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

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15
Q

Which of the following doesnt have a pair of s electrons in its highest orbital between magnesium and argon

A

Argon as its highest orbital is the d orbital

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16
Q

What is the elctronic configuration of Cu and Cu^+

A

Cu : (Ar) 4s1 3d10
Cu^+ : 3d10

17
Q

Deduce formula of ion that has same electron configuration of krypton and charge of 2+

A

Sr^2+

18
Q

Deduce formula of compound that contains 2+ charge and 3- ions that both have same electronic configuration of krypton

A

Ca3P2

19
Q

Explain why the first IE of sulfur is lower than the first IE of phosphorus

A

Sulfur has a pair of electron in one of its orbitals which repel each other

20
Q

State why the first IE of aluminium deviates from the general trend

A

Electron is removed from 3p orbital which is higher in energy than the 3s orbital

21
Q

Describe how molecules are ionised using electrospray ionisation

A

Sample is dissolved in a volatile solvent
Solvent injected ito mass spectrometry using a hypodermic needle
Tip of needle has a high voltage power supply
Each molecule gains a proton

22
Q

A mixture of 3 compounds is analysed using mass spectometry and are ionised by using electrospray ionisation. 3 compounds are : C3H5O2N, C3H7O3N, C3H7O2NS. Give formula of ion that reaches the detector first

A

C3H6O2N^+

23
Q

A sample of magnesium is analysed in a TOF mass spectometry using electron impact ionisation. Give an equation for process that occurs during ionisation of magnesium atom

A

Mg (g) -> Mg (g) ^+ + e^-

24
Q

Give an equation to represent ionisation of P in electrospray ionisation

A

P + H^+ -> PH^+

25
Q

M/Z vale of P when it undergoes electrspray ionisation is 556. What is the molecular mass of P

A

555

26
Q

Explain how ions are detected and relative abundance is measured in TOF mass spectrometer

A

Ion are accelerated using an electric field as it hits a negatively charged plate and gains an electron. Ion also hits the detector as relative abundance is proportional to the size of the current.

27
Q

How are ions formed in electron impact ionisation

A

Sample is bombarded by high energy electrons
From an electron gun which fires electrons at sample
Sample loses an electron forming a positive ion

28
Q

Why it is necessary to ionise molecules when measuring mass in TOF mass spectrometer

A

Ions will interact with and be accelerated using an electric field. Only ions will create a current when hitting the detector

29
Q

Bromine has two isotopes. 79Br and 81Br. State the peaks you would expect to see and their ratios.

A

158
160
162
25% : 50% : 25%

30
Q

Suggest what might cause relative atomic mass of a sample to be different to mass given in the periodic table

A

Other isotopes present / some isotopes may be absent

31
Q

Write equation for when nitrogen ion hits the detector

A

N^+ + e^- -> N

32
Q

Two peaks were observed at m/z = 107 & 109. Outline how TOF mass spectometry is able to seperate these two peaks

A

Positive ions accelerated using an electric field
To a constant kinetic energy
Ions with same m/z value of 107 move faster than ions with m/z value of 109. Therefore ions with m/z value of 107 arrive at detector first

33
Q

Which method between electron impact and electrospray ionisation is likely to break ions into fragments

A

Electron impact ionisation

34
Q

Why is a negatively chatged plate used in TOF mass spectrometry

A

Positive charged ions are attracted to negatively charged plate

35
Q

A sample containing isotopes are detected using mass spectometry. State why sample must be ionised

A

To accelerate ions in the sample
To detect ions in the sample

36
Q

How to calculate mass of magnesium

A

24 x 10^-3 Divided by 6.022 x 10^23

Chemistry (10 decks)

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