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35 Cards in this Set
- Front
- Back
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Relative mass of an electron |
1/1840 |
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What is the atomic number of an element |
The number of protons in the nucleus |
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What is the mass number of an atom |
The sum of the protons and neutrons |
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What is an isotope |
Atoms of the same element with different masses |
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What is relative atomic mass |
The weighted mean mass of an atom of an element compared to 1/12 of an an atom of carbon12 |
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What is relative isotopic mass |
The mass of an individual atom of a particular isotope relative to 1/12 of the mass of an atom of carbon12 |
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What is the molecular ion peak? |
The peak with te highest m/z ratio in the mass spectrum |
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What is an M peak also known as? |
A molecular ion peak |
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First stage of a mass spectrometer? |
Sample bombarded by electrons and becomes + charged |
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What happens in a mass spectrometer |
+ sample Deflected by a magnetic field according to their m/z ratio Detected |
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What can be calculated from a mass spectrometer? |
Relative abundance |
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Who first put forward the quantum theory that described shells? |
Max Planck |
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In which shell do electrons have the most energy |
The last shell |
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Shape on an s orbital? |
Sphere |
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Shape of a p orbital |
Figure of 8 |
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How many electrons per orbital (all) |
2 |
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How many electrons in the s subshell? |
2 |
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How many electrons in the p subshell? |
6 |
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How many electrons in the d subshell |
10 |
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How many electrons in the f subshell? |
14 |
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How many electrons in the first quantum shell? |
2 |
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How many electrons in the third quantum shell |
18 |
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What is a quantum shell? |
The energy level of an electron |
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What is an orbital? |
The region within an atom that can hold up to 2 electrons with opposite spins |
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What is Hund’s rule? |
That electrons will occupy the orbitals singly before taking pairs |
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What does the Pauli exclusion principal state? |
That 2 electrons can’t occupy the same orbital unless they have opposite spins |
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How is electron spin usually shown? |
Arrows up and down |
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How if te first ionisation energy represented? |
A(g)—>A+(g) +e- |
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How is the second ionisation energy represented? |
A+(g)—> A2+(g)+e- |
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How can we tell what group an element is in from its ionisation energies? |
Big jump when the electron is being removed from an outer shell |
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What is the first ionisation energy? |
The energy required to remove on electron from each atom in one mole of atoms in a gaseous state |
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What happens to ionisation energies across a period? |
General increase |
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What happens to ionisation energies down a group? |
Generally decreases |
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What is periodicity? |
A regularly repeating pattern of atomic,physical and chemical properties with increasing atomic number |
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What happens to te radius across each period? |
Decreases due to stronger attraction |
