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Atomic Structure
AQA A Level Chemistry
| Question | Answer |
|---|---|
| Name the 3 subatomic particles | Proton, neutron, electron |
| What is the relative mass of an electron | 1/2000 or 1/1840 |
| What letters do we use to represent mass number and atomic number | Mass number = M and Atomic number = Z |
| How is a positive ion formed | By losing electrons |
| What ion would be expected to be formed by an element in group 6 | 2- ion |
| What is the formula of the sulfate ion | SO42- |
| Write the chemical formula of calcium nitrate | Ca(NO3)2 |
| Define isotope | Isotopes are atoms of the same element (same number of protons) with different numbers of neutrons |
| Calcualte the number of neutrons in C12 and C14 | 6 in C12 and 8 in C14 |
| Why do isotopes have the same chemical properties | Same number of electrons |
| Describe the atomic model proposed by JJ Thompson | Plum pudding model, sphere of positive charge with electrons dotted around |
| Describe the experiment of Rutherford where he discovered the nucleus | Fired alpha particles at gold foil and some deflected and a few bounced back showing small centres of positive charge |
| Describe the atomic model proposed by Bohr | Positive nucleus surrounded by electrons in defined shells |
| How could you calculate the mass of one atom of oxygen using its Ar of 16 | 16 divided by the avagadro constant (6.022 x 10^23) |
| What is meant by relative atomic mass | Mean mass of atoms of an element relative to the mass of 12g of carbon 12 |
| Whate are the 5 main stages in mass spectrometry | Vaporisation, Ionisation, acceleration, drift, detection |
| Write generic equations to show the ionisation of X in a mass spectrometer by electron impact and proton absorbtion. | e- +X (g) --> X+ (g) + 2e- X + H+ ------> XH+ |
| Write a generic equation to show the ionisation of X in a TOF mass spectrometer | H+ +X (g) --> XH+ (g) |
| What are the two methods of ionisation that could be used in a mass spectrometer? | electron impact and electrospray |
| Describe what happens during electrospray ionisation | Particles gain a proton |
| Compare the speed and kinetic energy of a lithium and potassium atom in TOF mass spectrometry | Speed of lithium faster than potassium. Both have same KE |
| What is meant by the molecular ion peak | The highest m/z value on the spectrum of a molecule, formed when the molecule does not break up |
| How do you work the RMM in a TOF mass spectometer | Subtract one from the mass of the molecular ion |
| Why is m/z used in a mass spectrum not just mass | Because atoms can be doubly ionised and would be accelerated more quickly |
| How are ions detected in a mass spectrometer? | ions hit the detector and gain electrons, which causes a current to flow |
| How can you determine the number of ions hitting the detector at a m/z value? | The size of the current indicates how many ions of that m/z ratio are hitting the detector |
| Calculate the Ar of an element sample which is made up of 75% C12 and 25% C14 | 12.5 |
| How many electrons can the s, p and d subshells each hold | s = 2, p = 6, d = 10 |
| Write the electronic configuration of an element with 20 electrons | 1s2,2s2,2p6,3s2,3p6,4s2 |
| Write the electronic configuration of an elements with 24 electrons | 1s2,2s2,2p6,3s2,3p6,4s13d5 |
| Which two transition metal elements do not have a full 4s orbital | Chromium and copper |
| As a general rule which energy levels do electrons fill first? | Electrons fill orbitals in order from lowest energy to highest energy |
| Which subshell fills first 4s or 3d? | 4s |
| From which subshell are electrons removed first during ionisation 4s or 3d? | 4s |
| Into what orbitals would two electrons in a p subshell go? | Electrons fill orbitals singularly before pairing up |
| Fe has electron configuration [Ar] 4s2 3d6. what is the electron configuration of the Fe3+ ion | [Ar] 3d5 |
| Define first ionisation energy | The energy required to remove one mole of electrons from one mole of atoms in the gaseous state |
| Write an equation to show the 1st ionisation energy of sodium | Na(g) ------> Na+(g) + e- |
| Write an equation to show the 4th ionisation energy of calcium | Ca3+(g) ------> Ca4+(g) + e- |
| Is ionisation energy exothermic or endothermic | Endothermic - requires energy |
| How does nuclear charge affect ionisation energy | Increasing nuclear charge increase ionisation energy as electrons harder to remove |
| How does 1st ionisation energy change down the group and give 2 reasons why | Decreases down group. Electrons further from nucleus so less attraction and more shielding so less attraction |
| Write an equation to show the third ionisation energy of nitrogen | N2+ --> N3+ + e- |
| Why do group 3 elements eg. Al, not fit the trend in increasing first ionisation energy across the period | Electrons removed from a p orbital which is further from the nucleus so less attraction so ionisation energy decreases |
| Why do group 6 elements eg. O, not fit the trend in increasing first ionisation energy across the period | Electrons removed from an orbital which contains two electrons which gives some repulsion so easier to remove. So ionisation energy decreases |
Created by:
davenantchemistry
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