84219
Description
Flashcards by siobhan.quirk, updated more than 1 year ago
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Created by siobhan.quirk
over 11 years ago
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| Question | Answer |
| Define first ionisation energy | the energy required to remove the first electron from each atom in one mole of gaseous atom to form one mole of gaseous 1+ ions |
| Define electron shielding | the repulsion between electrons in different inner shells. Shielding reduces the net attractive force from the positive nucleus on the outer-shell electrons |
| Define successive ionisation energies | a measure of energy required to remove each electron in turn |
| Define second ionisation energy | the energy required to remove one electron from each ion in one mole of gaseous 1+ ions to form one mole of gaseous 2+ ions |
| Define shell | a group of atomic orbitals with the same prinicipal quantum number |
| Define principal quantum number | a number representing the relative overall energy of each orbital, which increases with distance from the nucleus |
| Define atomic orbital | a region within an atom that can hold up to two electrons with opposite spins |
| Define sub-shell | a group of the same type of atomic orbitals |
| Define electron configuration | the arrangement of electrons in an atom |
| Define compound | a substance formed from two or more chemically bonded elements in a fixed ratio, usually shown by a chemical formula |
| Define ionic bond | the electrostatic attraction between oppositely charged ions |
| Define giant ionic lattice | a 3D structure of oppositely charged ions held together by strong ionic bonds |
| Define group | a vertical column in the Period Table. Elements have similar properties and their atoms have the same number of outer-shell electrons |
| Define covalent bond | a bond formed by a shared pair of electrons |
| Define lone pair | is an outer-shell pair of electrons that are not involved in chemical bonding |
| Define dative covalent bond | (or coordinate bond) is a shared pair of electrons which has been provided by one of the bonding atoms only |
| Define electronegativity | a measure of the attraction of a bonded atom for the pair of electrons in a covalent bond |
| Define permanent dipole | a small charge difference across a bond that results from a difference in electronegativites of the bonded atoms |
| Define polar covalent bond | has a permanent dipole |
| Define polar molecule | has an overall dipole when you take into account any dipoles across the bonds |
| Define intermolecular force | an attractive force between neighbouring molecules |
| Define permanent dipole-dipole force | a weak attractive force between permanent dipoles in neighbouring polar molecules |
| Define van der Waals' forces | arractive forces between induced dipoles in neighbouring molecules |
| Define hydrogen bond | a strong dipole-dipole attractoin between an electon deficient hydrogen atom on one molecule and a loe pair of electrons on a highly electronegative atom on a different molecule |
| Define metallic bonding | electrostatic attraction between positive metal ions and delocalised electrons |
| Define delocalised electrons | electrons shared between more than two atoms |
| Define giant metallic lattice | is a 3D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds |
| Define simple molecular lattice | a 3D structure of molecules bonded together by weak intermolecular forces |
| Define giant covalent lattice | a 3D structure of atoms, bonded together by strong covalent bonds |
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