Flashcards
Atomic structure and Electronic configuration AS
Cards in this deck (20)
- 1AtomThe smallest part of an element that can take part in chemical reactions.
- 2ElementA substance that consists of only one type of atom.
- 3ProtonA positively charged particle in the nucleus of an atom
- 4NeutronAn uncharged particle found in the nucleus of an atom with the same relative mass as a proton.
- 5ElectronA negatively charged particle found in orbitals outside the nucleus; it has negligible mass in comparison to a proton.
- 6Atomic numberThe number of protons found in the nucleus of an atom.
- 7Mass numberThe number of protons and neutrons found in the nucleus of an atom.
- 8IsotopeAtoms of the same element with the same number of protons and electrons but a different number of neutrons.
- 9Energy levelsThe specific distances from the nucleus corresponding to the energy of the electron.
- 10SubshellsRegions of the principal quantum shells where electrons exist in defined areas of space.
- 11OrbitalA region of space outside the nucleus of an atom that can be occupied by a maximum of two electrons.
- 12s, p and d orbitals
- 13Atomic Radius and trendsHalf the distance between the nuclei of two covalently bonded atoms.
Increases down the group because an additional shell is added and shielding increases.
Decreases across a period because nuclear charge and nuclear attraction increase and shielding remains the same. - 14Ionic radius and trendsHalf the distance between the nuclei of two ions.
Same trends as atomic radius - 15ShieldingThe ability of inner shell electrons to reduce the effect of nuclear charge on outer electrons.
- 16Ionisation energyThe amount of energy required to remove one mole of electrons from one mole of gaseous atoms to form one mole of gaseous ions.
- 17Trends in Ionisation energiesDown the group, IE decreases because:
The distance between the nucleus and the valence shell increases.
Atomic radius increases.
Nuclear attraction decreases.
The shielding effect increases. - 18Trends in Ionisation energiesAcross a period, IE increases because:
Nuclear charge increases.
Nuclear attraction increases.
Atomic radius decreases.
Distance between the nucleus and the valence shell decreases.
The shielding effect remains the same. - 19Spin-pair repulsionWhen a pair of electrons in the same orbital repel each other. This decreases IE.
- 20Electronic configuration
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- A-level Chemistry Flashcards on Atomic structure and Electronic configuration AS, created by Fatima Conteh on 15/12/2022.
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- Fatima Conteh
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