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Chemistry > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

Name the 3 subatomic particles

A

Proton, neutron, electron

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2
Q

What is the relative mass of an electron

A

1/2000 or 1/1840

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3
Q

What letters do we use to represent mass number and atomic number

A

Mass number = M and Atomic number = Z

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4
Q

How is a positive ion formed

A

By losing electrons

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5
Q

What ion would be expected to be formed by an element in group 6

A

2- ion

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6
Q

What is the formula of the sulfate ion

A

SO42-

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7
Q

Write the chemical formula of calcium nitrate

A

Ca(NO3)2

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8
Q

Define isotope

A

Isotopes are atoms of the same element (same number of protons) with different numbers of neutrons

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9
Q

Calculate the number of neutrons in C12 and C14

A

6 in C12 and 8 in C14

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10
Q

Why do isotopes have the same chemical properties

A

Same number of electrons

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11
Q

Describe the atomic model proposed by JJ Thompson

A

Plum pudding model, sphere of positive charge with electrons dotted around

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12
Q

Describe the experiment of Rutherford where he discovered the nucleus

A

Fired alpha particles at gold foil and some deflected and a few bounced back showing small centers of positive charge

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13
Q

Describe the atomic model proposed by Bohr

A

Positive nucleus surrounded by electrons in defined shells

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14
Q

How could you calculate the mass of one atom of oxygen using its Ar of 16

A

16 divided by the Avagadro’s constant (6.022 x 10^23)

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15
Q

What is meant by relative atomic mass

A

Mean mass of atoms of an element relative to the mass of 12g of carbon 12

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16
Q

What are the 5 main stages in mass spectrometer

A

Vaporisation, Ionisation, acceleration, drift, detection

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17
Q

Write generic equations to show the ionisation of X in a mass spectrometer by electron impact and proton absorbtion.

A

e- +X (g) –> X+ (g) + 2e-

X + H+ ——> XH+

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18
Q

Write a generic equation to show the ionisation of X in a TOF mass spectrometer

A

H+ +X (g) –> XH+ (g)

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19
Q

What are the two methods of ionisation that could be used in a mass spectrometer?

A

electron impact and electrospray

20
Q

Describe what happens during electrospray ionisation

A

Particles gain a proton

21
Q

Compare the speed and kinetic energy of a lithium and potassium atom in TOF mass spectrometry

A

Speed of lithium faster than potassium. Both have same KE

22
Q

What is meant by the molecular ion peak

A

The highest m/z value on the spectrum of a molecule, formed when the molecule does not break up

23
Q

How do you work the RMM in a TOF mass How do you work the RMM in a TOF mass spectometer

A

Subtract one from the mass of the molecular ion

24
Q

Why is m/z used in a mass spectrum not just mass

A

Because atoms can be doubly ionised and would be accelerated more quickly

25
Q

How are ions detected in a mass spectrometer?

A

ions hit the detector and gain electrons, which causes a current to flow

26
Q

How can you determine the number of ions hitting the detector at a m/z value?

A

The size of the current indicates how many ions of that m/z ratio are hitting the detector

27
Q

Calculate the Ar of an element sample which is made up of 75% C12 and 25% C14

A

12.5

28
Q

How many electrons can the s, p and d subshells each hold

A

s = 2, p = 6, d = 10

29
Q

Write the electronic configuration of an element with 20 electrons

A

1s2,2s2,2p6,3s2,3p6,4s2

30
Q

Write the electronic configuration of an elements with 24 electrons

A

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

31
Q

Which two transition metal elements do not have a full 4s orbital

A

Chromium and copper

32
Q

As a general rule which energy levels do electrons fill first?

A

Electrons fill orbitals in order from lowest energy to highest energy

33
Q

Which subshell fills first 4s or 3d?

A

4s

34
Q

From which subshell are electrons removed first during ionisation 4s or 3d?

A

4s

35
Q

Into what orbitals would two electrons in a p subshell go?

A

Electrons fill orbitals singularly before pairing up

36
Q

Fe has electron configuration [Ar] 4s2 3d6. what is the electron configuration of the Fe3+ ion

A

[Ar] 3d5

37
Q

Define first ionisation energy

A

The energy required to remove one mole of electrons from one mole of atoms in the gaseous state

38
Q

Write an equation to show the 1st ionisation energy of sodium

A

Na(g) ——> Na+(g) + e-

39
Q

Write an equation to show the 4th ionisation energy of calcium

A

Ca3+(g) ——> Ca4+(g) + e-

40
Q

Is ionisation energy exothermic or endothermic

A

Endothermic - requires energy

41
Q

How does nuclear charge affect ionisation energy

A

Increasing nuclear charge increase ionisation energy as electrons harder to remove

42
Q

How does 1st ionisation energy change down the group and give 2 reasons why

A

Decreases down group. Electrons further from nucleus so less attraction and more shielding so less attraction

43
Q

Write an equation to show the third ionisation energy of nitrogen

A

N2+ –> N3+ + e-

44
Q

Why do group 3 elements eg. Al, not fit the trend in increasing first ionisation energy across the period

A

Electrons removed from a p orbital which is further from the nucleus so less attraction so ionisation energy decreases

45
Q

Why do group 6 elements eg. O, not fit the trend in increasing first ionisation energy across the period

A

Electrons removed from an orbital which contains two electrons which gives some repulsion so easier to remove. So ionisation energy decreases

Chemistry (21 decks)

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