Chemistry Unit 1 Module 1 Atoms and reactions

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Atoms of the same element with different numbers of neutrons. Isotopes of the same element have; different masses, same no. of prtons & electrons and different no.s of neutrons in the nucleus.
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Atomic (proton) number
The number of protons in the nucleus of an atom
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Mass (nucleon) number
The number of particles (protons and neutrons) in the nucleus
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An ion
A positively or negatively charged atom or (covalently bonded) group of atoms (a molecular ion).
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Relative Isotopic Mass
The mass of an atom of an isotope compared with one twelfth of the mass of an atomof carbon-12.
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Relative Atomic Mass, Ar,
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, Mr
The weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12. You can find the relative molecular mass, Mr, by adding together the rwlative atomic masses of each atom making up a formula unit.
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Relative Formula Mass
The weighted man mass of a formula unit compared with one-twelfth of the mass of an atom of carbon-12. You can find the relative atomic masses by of each atom
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Avogadro constant, N
The number of atoms per mole odf the carbn-12 isotope (6.02x10 mol )
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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, M
the mass per mole of a substance. he units of molar mass are g mol
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Amount of substance
The quantity whose unit is the mole. Chemists use 'amount of substance' as a means of counting atoms. It is given the symbol n and is measured using a unit called the mole.
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Empirical formula
The simplest whole-number ratio of atoms of each element present in a compound.
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A small group of atoms held together by covalent bonds.
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Molecular formula
The actual number of atoms of each element in a molecule
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Molar volume
The volume per mole of a gas. the units of molar volume are dm mol . At room temperature and pressure, the molr volume is approximately 24.0dm mol .
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The Concentration of a Solution
The amount of solute, in mol, dissolved per 1dm (1000cm ) of solution. Measured in moles per cubic decimeter, mol dm .
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A Standard Solution
A solution of known concentration. Standard solutions are normally used in titrations to determine unknown information about another substance.
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A Species
Any type of particle that takes part in a chemical reaction.
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The molar relationship between the relative quantities of substances taking part in a reaction.
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An Acid
A species that is a proton donor.
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A Base
A species that is a proton acceptor.
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An Alkali
A type of base that dissolves in water forming hydroxide ions OH- (aq) ions:
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A Salt
Any chemical compound formed an acid when a H+ ion from the acid has been replaced by a metal ion or nother positive ion, such as the ammonium ion, NH
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Positively charged ion
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Negatively charged ion
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Refers to a crystalline compound containing water molecules.
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Refers to a subtance that contains no water molecules.
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Water of Crystallisation
Refers to water molecules that form an essential part of the crystalline structure of a compound.
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An Oxidation NUmber
A measure of the number of electrons that an atom uses to bond with atoms of another element. Oxidation numbers are derived from a set of rules.
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Is LOSS of electrons or an increase in oxidation number.
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Is GAIN of electrons or a decrease in oxidation number.
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A Redox reaction
Is a reaction in which both oxidation and reduction take place.
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A Reducing Agent
Is a reagent that reduces (adds electron to) another species.
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An Oxidising Agent
Is a reagant taht oxidises (takes electrons from) another species.
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Card 2


Atomic (proton) number


The number of protons in the nucleus of an atom

Card 3


Mass (nucleon) number


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Card 4


An ion


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Card 5


Relative Isotopic Mass


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