OCR As Chemistry in-organic definitions

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  • Created by: Sanchia27
  • Created on: 30-01-18 10:03
Define Isotopes
Atoms of the same proton number with a different number of neutrons
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Define atomic number
Number of protons and neutrons of an atom
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Mass number
Number of protons and neutrons in the nucleus
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Ion
charged atom
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Relative isotopic mass
mass of an atom of an isotope compared to 1/12th of the mass of an atom of carbon-12
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relative atomic mass
weighted mean mass of an element compared with 1/12th of the masss of an atom of carbon-12
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Relative molecular mass
weighted mean mass of a molecule compared with 1/12th of an atom of carbon-12
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relative formula mass
weighted mean mass of a formula unit compared with 1/12th of an atom of carbon-12
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Avogadros constant, NA
number of atoms per mole of the carbon-1 isotope (6.02x 10^23mol^-1)
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Moles
Amount of any substance containing as many particles as there are carbon atoms in exactly 12g of carbon-12 isotope
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Molar mass
mass per mole of a substance (g mol^-1)
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concentration
Amount of solute in mol, disolved per 1 dm^3 of solution
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Species
Type of particle that takes part in chemical reaction.
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Stoichiometry
Molar relationship between relative quantities of substances taking part in a reaction
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Acid
species that is a proton donor
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Base
species that is a proton acceptor
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alkali
Type of base dissolved in water forming OH- ions
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Salt
any chemical compound formed from an acid, whose protons have been replaced by a metal or ammonium ions
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cation
positively charged ion
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Anion
negitively charged ion
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Hydrated
Crystaline compound containing water molecules
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anhydrous
substance that doesnt contain any water molecules
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water of crystallisation
water molecules that form an essential part of crystaline structure of a compound
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oxidation number
Measure of number of eletrons that an atom uses to bond with atoms of another element- derived from a set of rules
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Oxidation
Loss of electrons, increase of oxidation number
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reduction
gain of electrons, decrease in oxidation number
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reducing agent
reagant that reduces another species
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Oxidation agent
reagant that oxidises another species
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electron shielding
repulsion betweeen electrons in different inner shells
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successive ionisation energies
measure of energy required to remove each electron in turn
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1st ionisation energy
Energy required to remove one mole of electrons from one mole of gaseous atoms, forming one mole of uni-positive ions in the gaseous state. X (g) → X⁺ (g) + e⁻
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2nd ionisation energy
Energy required to remove one mole of electrons from one mole of unipositive ions in the gaseous state. X⁺ (g) → X²⁺ (g) + e⁻
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3rd ionisation energy
Energy required to remove one mole of electrons from one mole of X²⁺ ions in the gas phase. X²⁺ (g) → X³⁺ (g) + e⁻
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shell
Group of atomic orbitals with same orinciple quantum number, n.- energy levels
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Atomic orbital
Region within an atom that can hold up to two electrons, with opposite spins
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sub-shell
Group of same type of atomic orbitals (s, p, d, f) within a shell
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electron configuration
Arrangement of electrons in an atom
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Ionic bonding
Electrostatic attraction between oppositely charged ions
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Giant ionic lattice
3D structure of oppositely charged ions, held together by strong ionic bonds
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covalent bonding
Bond formed by a shared pair of electrons
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metallic bonding
Electrostatic attraction between positive metal ions & delocalised electrons
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Dative bonding
Shared pair of electrons provided by one of the bonding atoms only
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lone pair
Outer-shell pair of electrons that isn't involved in chemical bonding
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electronegativity
The ability of an atom to attract towards it the shared pair of electrons in a covalent bond
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Permenent dipole-dipole
Weak attractive force between permanent dipoles in neighbouring polar molecules
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intermolecular force
Attractive force between neighbouring molecules
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van der waals' forces
Attractive forces between induced dipoles in neighbouring molecules
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hydrogen bonds
A strong dipole-dipole attraction between an electron-deficient hydrogen atom (O−Hδ⁺, N−Hδ⁺) on one molecule; and a lone pair of electrons on a highly electronegative atom (H−Oδ⁻ or H−Nδ⁻) on a different molecule
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Giant metallic lattice
3D structure of positive ions and delocalised electrons, bonded together by strong metallic bonds
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simple molecular lattice
3D structure of molecules, bonded together by weak intermolecular forces
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Giant covalent lattice
3D structure of atoms, bonded together by strong covalent bonds
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Thermal decomposition
Breaking up of chemical substance with heat into at least two chemical substance
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displacement reaction
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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precipitation reaction
Formation of a solid from solution during chemical reaction- when 2 (aq) solutions are mixed together
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Other cards in this set

Card 2

Front

Define atomic number

Back

Number of protons and neutrons of an atom

Card 3

Front

Mass number

Back

Preview of the front of card 3

Card 4

Front

Ion

Back

Preview of the front of card 4

Card 5

Front

Relative isotopic mass

Back

Preview of the front of card 5
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