Chem Unit 1
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- Created by: Emily Hotson
- Created on: 23-03-13 19:48
Isotopes
Atoms of the same element with different numbers of neutrons.
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Atomic Number
The number of protons in the nucleus of an atom.
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Mass Number
The number of particles in the nucleus.
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Relative Isotopic Mass
The mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12.
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Relative Atomic Mass
The weighted mean mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12.
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Relative Molecular Mass
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12.
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Relative Formula Mass
The weighted mean mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12.
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A Mole
The amount of any substance containing as many particles as there are carbon atoms in exactly 12g of the carbon-12 isotope.
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Molar Mass
The mass per mole of a substance.
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Empirical Formula
The simplest whole number ratio of atoms of each element present in a compound.
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Molecular Formula
The actual number of atoms of each element in a molecule.
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Standard Solution
A solution of known concentration.
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Species
Any type of particle that takes place in a chemical reaction.
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Stoichiometry
The molar relationship between the relative quantities of substance taking part in a reaction.
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A Salt
Any chemical compund formed from an acid when an H+ ion from the acid has been replaced by a metal ion or another positive ion.
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A Cation
A positively charged ion.
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An Anion
A negatively charged ion.
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Hydrated
A crystalline compound containing water molecules.
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Anhydrous
A substance that contains no water molecules.
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Water of Crystallisation
Water molecules that form an essential part of the crystalline structure of a compound.
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Oxidation Number
Measure of the number of electrons that an atom uses to bond with atoms of another element.
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First Ionisation Energy
The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.
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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
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Successive Ionisation Energies
A measure of the energy required to remove each electron in turn.
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A Shell
A group of atomic orbitals with the same principal quantum number,n. Also known as a main energy level.
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Atomic Orbital
A region within an atom that can hold up to two electrons, with opposite spins.
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A Sub-Shell
A group of the same type of atomic orbitals.
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An Ionic Bond
The electrostatic attraction between oppositely charged ions.
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A giant-ionic Lattice
3D structure of oppositely charged ions, held together by strong ionic bonds.
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A Covalent Bond
A bond formed by a shared pair of electrons.
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A Lone pair
An outer-shell pair of electrons that is not involved in chemical bonding.
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A Dative Covalent Bond
A shared pair of electrons which has been provided by one of the bonding atoms only.
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Electronegativity
A measure of the attraction of a bonded atom for the pair of electron in a covalent bond.
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A Permanent Dipole
A small charge difference across a bond that results from a difference in the electronegativities of the bonded atoms.
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A Polar Covalent Bond
A covalent bond with a permanent dipole.
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An Intermolecular Force
An attractive force between neighbouring molecules.
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A Permanent Dipole-Dipole Force
A weak attractive force between permanent dipoles in neighbouring polar molecules.
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Van der Waals' Forces
Attractive forces between induced dipoles in neighbouring molecules.
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A Hydrogen Bond
A strong dipole-dipole interaction between an electron-deficient hydrogen atom on molecule and a lone pair of electrons on a highly electronegative atom on a different molecule.
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Metallic Bonding
The electrostatic attraction between positive metal ions and delocalised electrons.
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A Giant Metallic Lattice
A 3D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds.
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A Simple Molecular lattice
A 3D structure of molecules bonded together by weak intermolecular forces.
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A Giant Covalent Lattice
A 3D structure of atoms, bonded together by strong covalent bonds.
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Periodicity
A regular periodic variation of properties of elements with atomic number and position in the Periodic table.
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A Displacement Reaction
A reaction in which a more-reactive element displaces a less-reactive element from an aqueous solution of the latter's ions.
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Disproportionation
The oxidation and reduction of the same element in a redox reaction.
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A Precipitation Reaction
The formation of a solid from a solution during a chemical reaction. Often formed when two aqueous solutions are mixed together.
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Other cards in this set
Card 2
Front
The number of protons in the nucleus of an atom.
Back
Atomic Number
Card 3
Front
The number of particles in the nucleus.
Back
Card 4
Front
The mass of an atom of an isotope compared with one-twelfth of the mass of an atom of carbon-12.
Back
Card 5
Front
The weighted mean mass of an atom of an element compared with one-twelfth of the mass of an atom of carbon-12.
Back
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