IB Chemistry Definitions - Standard Level
Practise and master the definitions that correspond to the command terms define or distinguish used through out the IB Chemistry course.
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- Chemistry
- Quantitative ChemistryAtomic StructurePeriodicityBondingEnergeticsKineticsEquilibriumAcids and BasesOrganic ChemistryMeasurement and Data Processing
- International Baccalaureate
- Other
- Created by: Venandah Madanhi
- Created on: 09-02-15 20:50
The mass of one mole of any substance, expressed in grams per mole.
Molar Mass
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The average mass of an atom, taking into account the relative abundances of all the naturally occurring isotopes of the element, relative to one atom of C-12
Relative Atomic Mass
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The average mass of a molecule, calculated by adding the relative atomic masses of the constituent atoms
Relative Molecular Mass
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The simplest whole number ratio of the atoms a compound contains.
Empirical Formula
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The actual number of atoms of each element in the compound
Molecular Formula
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The substance dissolved in a solvent forming a solution
Solute
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The liquid that dissolves another substance or substances to form a solution
Solvent
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A homogeneous mixture of a solvent with a solute - there is usually some interaction between the solvent and solute molecules
Solution
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The amount of solute in a known volume of solution - is often represented by square brackets around the substance
Concentration
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The sum of the protons and neutrons in the atom's nucleus
Mass Number
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The number of protons in its nucleus. Its is also equal to the number of electrons the atom contains. - this also defines the element and its position in the Periodic Table.
Atomic Number
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Atoms of the same element but have different number of neutrons.
Isotopes
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Shows an unbroken sequence of frequencies, such as the spectrum of visible light
Continuous Spectrum
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An emission spectrum that only has certain frequencies of light. It is produced by excited atoms and ions as they fall back to a lower energy level
Line Spectrum (Discontinuous Spectrum)
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A vertical column of elements in the Periodic Table. The atoms of the elements all have the same outer shell structure by an increasing number of inner shells.
Group
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A horizontal row of elements in the Periodic Table. The atoms of the elements have the same number of shells but with an increasing number of electrons in the outer shell.
Period
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The minimum energy required to remove one mole of electrons from one mole of atoms in a gaseous state.
First Ionization Engergy
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The tendency of an atom in a molecule to attract a shared pair of electrons towards itself.
Electronegativity
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A reaction that releases heat to the surroundings as a result of forming products with stronger bonds than the reactants.
Exothermic Reaction
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A reaction that absorbs heat from the surroundings as a result of forming products with weaker bonds than the reactants.
Endothermic Reaction
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The heat transferred during a reaction carried out under standard conditions.
Standard Enthalpy of Reaction
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The energy required to break a mole of covalent bonds in the reactant, all reactants and products being in a gaseous state.
Average bond enthalpy
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The increase in concentration of products (or the decrease in concentration of reactants) per unit time.
Rate of Reaction
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The minimum energy required for a chemical reaction to take place.
Activation Energy
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Acid is a proton donor
Bronsted-Lowry Acid
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Base is a proton donor
Bronsted-Lowry Base
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Acid is an electron-pair acceptor
Lewis Acid
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Base is an electron-pair donor
Lewis Base
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Acids and bases that are almost completely dissociated
Strong Acids and Bases
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Acids and bases that are only partially dissociated
Weak Acids and Bases
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The loss of electrons
Oxidaion
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The gain of electrons
Reduction
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Accept electrons and become reduced.
Oxidising Agent
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Donate electrons and become oxidised.
Reducing Agent
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Measurements that have small random errors.
Precision
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Measurements that have small systematic errors.
Accuracy
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Other cards in this set
Card 2
Front
The average mass of an atom, taking into account the relative abundances of all the naturally occurring isotopes of the element, relative to one atom of C-12
Back
Relative Atomic Mass
Card 3
Front
The average mass of a molecule, calculated by adding the relative atomic masses of the constituent atoms
Back
Card 4
Front
The simplest whole number ratio of the atoms a compound contains.
Back
Card 5
Front
The actual number of atoms of each element in the compound
Back
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