Some Important Terms. Flashcards
Atom
The smallest possible particle of an element.
Compound
A substance composed of two or more elements chemically bonded together.
Molecule
An arrangement of atoms covalently bonded together.
Covalent bond
A shared pair of electrons holding atoms together in a molecule.
Ions
Particle formed from an atom or group of atoms by loss or gain of electrons with, respectively, a positive or negative charge.
Ionic bonding
Electrostatic attraction between oppositely charged ions.
Atomic number
How many protons there are in an atom.
Mass
The number of protons and neutrons in an atom.
Isotopes
Atoms that are the same element with a different mass because of a different number of neutrons.
Element
A substance Taft cannot be broken down chemically into anything simpler.
Accurate result
A result that is close to the true answer
Acid
A substance that release hydrogen ions in an aqueous solution– a proton donor
Activation energy
The minimum amount of KE that particles need in order to react when they collide
Additional polymer
A long-chain molecule made by lots of small Alkene molecules adding together
Alcohol
A substance either the general formula CnH2nOH
Aldehyde
A substance with the general formula CnH2nO which has a hydrogen and one alkyl group attached to the carbonyl carbon atom
Alicyclic compound
An organic compound that contains carbon and hydrogen joined together in a non-aromatic ring.
Aliphatic compound
An organic compound that contains carbon and hydrogen joined together in straight chains, branches chains or a non-aromatic ring.
Alkali
A base that is soluble in water and release hydroxide ions in aqueous solution
Alkaline earth metal
An element in group 2 of the periodic table
Alkene
Hydrocarbon with the general formula CnH2n+2. Contains single bonds only.
Alkene
A hydrocarbon with the general formula CnH2n and containing at least one carbon-carbon double bond
Alkyl group
Hydrocarbon fragment with the general formula CnH2n+1
Anhydrous salt
A salts that doesn’t contain any water of crystallisation
Antacid
A substance that neutralises stomach acid
Aromatic compounds
And organic compound that contains the benzene ring
Atom economy
The proportion of reactant atoms that become part of the desired product expressed as a percentage
Proton number
The number of protons in the nucleus of an atom
Atomic radius
The distance between the nucleus of an atom and the outermost electrons
Average bond enthalpy
The energy needed to break one mole of a bond in the gas phase averaged over the different compounds that the bond is found in
Avogadro constant
6.02 x 10^23 The number of particles in one mole of a substance
Base
A substance that removes hydrogen ions from an aqueous solution- a proton acceptor
Biodegradable
A substance that naturally decomposes because organisms can digest it
Bohr model
A model for the structure of an atom proposed by Neils Bohr. He suggested that electrons only exist in fixed orbitals (shells) and not anywhere else
Bond enthalpy
The energy required to break the bonds between two atoms. Usually given as an average bond enthalpy.
Bond fission
The process of breaking a covalent bond
Carbocation
An organic ion containing a positively charged carbon atom
Carbonyl compound
And organic compound that contains a carbon oxygen double bond
Carboxylic acid
A substance that has a COOH Group attach the end of the carbon chain
Catalyst
A substance that increases the rate of reaction by providing an alternative reaction pathway with a lower activation energy. The catalyst is chemically unchanged at the end of the reaction.
Catalytic converter
A device fitted to a car exhaust system to remove pollutant gases such as carbon Monoxide, nitrogen monoxide and unburned hydrocarbons
Chain Isomer
A molecule that contains the same atoms is another molecule that has a different arrangement of the carbon skeleton
Charge density
The amount of charge in relation to the size of an ion
CFC
A Halo alkane containing fluorine and chlorine and no hydrogen. CFCs contributed ozone-depletion
Cis- teams isomerism
A special type of E/Z I summarise them were two of the groups attached to the carbon atoms around the carbon to carbon double bond are the same
Collision theory
The theory that a reaction will not take place between two particles unless they collide in the right direction and with at least a certain minimum amount of kinetic energy
Complete combustion
Burning a substance is completely in an access of oxygen. Complete combustion of a hydrocarbon will produce carbon dioxide and water only
Concentration
A measure of how many moles of a substance or dissolved in a volume of solution
Coordinates or dative covalent bond
A covalent bond formed when one atom provides both of the shared electrons
Covalent bond
Strong electrostatic attraction between a shared pair of electrons and the nucleus of bonded atoms
Curly arrow
And Aaron are used in a reaction mechanism to show the movement of the pair of electrons
Cyclo alkanes
A type of alkane which is one or more nonaromatic carbon rings
Dehydration reaction
A reaction in which water is eliminated from an organic molecule
Delocalised electrons
An electron that is not attached to a specific atom
Dipole
The difference in charge between two atoms caused by a shift in the electron density in the bond
Displacement reaction
I reaction where a more reactive element pushes out a less reactive element from an ionic solution
Disproportionation
When an element is both oxidised and reduced in a single chemical reaction
Displayed formula
I way of representing a molecule that shows how all the atoms are arranged and all the bonds between them
Distillation
A technique used to separate liquids with different boiling points. A mixture is gently heated so that substances are VAT rate and can be collected in order of increasing boiling point.
E/Z isomerism
A type of stereoisomerism that is caused by the restricted rotation about a carbon to carbon double bon. Each of the carbon atoms must be attached to 2 different groups.
Electron configuration
The number of electrons that an atom or ion has and how they are arranged
Electron shell
A region of an atom with a fixed energy that contains electrons orbiting the nucleus
Electron shell repulsion theory
The theory that in a molecule lone pair/ lone pair Bond angles are the biggest, lone pair/ bonding pair Bond angles are the second biggest, and bonding pair/ bonding pair bond angles are the smallest.
Electron shielding
Went into electrons affectively screen the other electrons from the pull of the nucleus
Electronegativity
The ability of an atom to attract the bonding electrons in a covalent bond
Electrophile
And electron pair exceptor
Electrophilic addition
A reaction mechanism where the double bond in an alkene opens and atoms are added to the carbon atoms
Elimination reaction
A reaction in which a pair of atoms or groups of atoms are removed from an organic molecule
Empirical formula
I thought you like giving the simplest whole number ratio of atoms of each element in a compound
Endothermic reaction
I reaction that absorbs energy in the form of heat (deltaH is positive)
Enthalpy change
Heat energy transferred in a reaction at a constant pressure(deltaH)
Enthalpy profile diagram
A graph showing how the enthalpy changes during a chemical reaction
Exothermic reaction
If reaction that gives out energy in the form of heat (deltaH is negative)
First ionisation energy
The energy needed to remove one mole of electrons from one mole of gaseous atoms
False positive
A result that suggests the presence of something eh ions that isn’t actually there
Functional group
Group of atoms that is responsible for the characteristic reactions of a molecule
Functional group isomers
A molecule that has the same molecular formula as another molecule that with atoms are arranged into different functional groups
General formula
An algebraic formula that can describe any member of a homologous series of compounds
Giant covalent lattice
A structure consisting of a huge network of covalently bonded atoms
Giant ionic lattice structure
A regular repeated structure made of oppositely charged ions strongly attracted to each other in all directions
Giant metallic lattice structure
A regular structure consisting of closely packed positive metal irons in a sea of delocalised electrons
Global warming
The warming of the planet due to an increased concentration of greenhouse gas in the troposphere which enhanced greenhouse effect
Greenhouse effect
The absorption and real mission of infrared rays creation by greenhouse gases in this troposphere
Greenhouse gas
Aigas absorbs and emits infrared radiation and so contributes to the greenhouse effect
Halide
A negative ion of a halogen
Haloalkane
An alkane with at least one halogen atom in the place of a hydrogen atom
Hesses law
The total entropy change of reaction is always the same no matter which route is taken
Heterolytic fission
When a covalent bond breaks unevenly with one of the bonding atoms receiving both of the electrons from the bonded pair resulting in the formation of a positively charged cation with a negatively charged anion
Homologous series
A family of organic compounds that have the same general formula and similar chemical properties
Homolytic fission
When a covalent bond breaks evenly with each bonding atoms receiving one electron from the bonding pair resulting in the formation of two electrically uncharged radicals
Hydrated salt
A salt that contains water of crystallisation
Hydrocarbon
A molecule that only contains hydrogen and carbon atoms
Hydrogen bond
The strongest intermolecular force it occurs when polarised covalent bonds cause hydrogen atoms to form weak bonds with lone pairs of electrons on the fluorine, nitrogen oxygen atoms of other molecules
Hydrolysis reaction
I reaction when molecules are split apart by water molecules the water molecules are also split into hydrogen ions and hydroxide ions
Incomplete combustion
Burning a substance in a poor supply of oxygen incomplete combustion of hydrocarbons and produces carbon monoxide water and sometimes carbon and carbon dioxide
Induced dipole dipole interactions
A type of intermolecular force close by temporary dipole is which causes all atoms and molecules to be attracted to each other
Infrared spectroscopy
And analytical technique used to identify the functional groups present in a molecule by measuring the infrared absorption frequencies of its bonds
Intermolecular forces
Forces between molecules
Ionic bond
Electrostatic attraction between positive and negative ions
Ionic equation
And equation which only shows the reacting particles of a reaction involving ions
Ionisation
The removal of one or more electrons from an atom or molecule, resulting in an ion forming
Isotopic abundance
The relative amount of a particular isotope occurring in a sample of an element
Ketone
A substance with the general formula CnH2nO which has two alkyl groups attached to the carbonyl-carbon atom
Lattice
A regular structure made of atoms or ions
Mass number
The total number of protons and neutrons in the nucleus of an atom
Mass spectrometry
And analytical technique used to find the structure of a molecule by measuring the masses of the ions it produces when it is bombarded with electrons
Mass spectrum
A chart produced by a mass spectrometer
Molar mass
Mass of one mole of something
Molar ratio
Ratio of the number of moles in each reactant and product in a balanced chemical equation
Mole
The unit of amount of substance
Molecular formula
A way of representing molecules that shows the actual number of atoms of each element in a molecule
Molecular ion
And I on made up of a group of atoms with an overall charge
Monomer
A small molecule which is used to make a polymer
Neutralisation reaction
A reaction between an acid and a base to produce a salt and water
Noble gas
An element in group 0 of the periodic table. These elements are extremely stable because they have a full outer shell of electrons
Nomenclature
Naming organic compounds
Nucleophile
An electron-pair donor
Nucleus
Central part of an atom ion only made up of protons and neutrons
Orbital
Region of a sub shell that contains a maximum of two electrons with opposite spins
Oxidation
Loss of electrons
Oxidation number
The total number of electrons an element has donated or excepted
Oxidising agent
Something that accepts electrons and gets reduced
Percentage yield
Amount of product that is actually obtained during a reaction expressed as a percentage of the amount of product that should form
Permanent dipole dipole interactions
Intermolecular forces that exist because the difference in electronegativity is in a polar bond causes week electrostatic forces of attraction between molecules
Pi bond
A type of bond formed when 2P orbitals overlap sideways
Polar bond
A true they don’t bond were difference in electronegativity has cause a shift in electron density in the bond
Polar molecule
Emily still containing polar bonds that are arranged so that the dipoles don’t cancel each other out causing an overall dipole to be created across the molecule
Polymer
A long molecule formed from lots of small molecules joined together
Radical
A particle with an unpaired electron
Redox reaction
A reaction where reduction and oxidation happen simultaneously
Reducing agent
Something that donates electrons and gets oxidised
Reduction
Gain of electrons
Refluxing
Heating a reaction mixture in such a way that you boil it without losing volatile solvents reactants or products. Any vaporised compounds call condense and get back into the reaction mixture
Relative atomic mass
The average mass of an atom Auger and elements compare to 1/12 of the mass of an atom of carbon 12
Relative formula mass
The average mass of a molecule or formula unit compared to 1/12 of the mass of an atom of carbon 12
Relative isotopic mass
The mass of an atom of an isotope of an element compared to 1/12 of the mass of an atom of carbon 12
Relative molecular mass
The average mass of a molecule compared to 1/12 of the mass of an atom of carbon 12
Salt
A compound formed when hydrogen in an acid molecule is replaced by a metal ion or ammonium ion
Saturated hydrocarbon
A hydrocarbon where all the carbon carbon bonds are single bonds
Sigma bond
Type of bond formed when two orbitals overlap directly between the bonded atoms
Silver nitrate test
A test that uses silver nitrate to identified halide ions in the solution
Simple molecular structure
A compound with strong covalent bonds with in its molecules but weak forces between is molecules
Skeletal formula
A simplified organic formula which only shows the carbon skeleton and associated functional groups
Specific heat capacity
The amount of heat energy it takes to raise the temperature of 1 g of given substance by 1K
Spin
The type of momentum possessed by an electron spin can either be down or up
Standard conditions
100kPa 298K
Standard enthalpy change of combustion
The ends of the change one month one mole of substance is completely burned in oxygen under standard conditions we all reactants and products in their standard states
Standard enthalpy change of formation
The Exelby change when one mole of a compound is formed from its elements in the standard states under standard conditions
Standard entropy change of neutralisation
The answer will be change when an acid and alkali react together to form one mole of water under standard conditions
Standard enthalpy change of reaction
The answer be change when a reaction occurs in the molar quantities shown in the chemical equation under standard conditions
Stereoisomer
A molecule that has the same structural formula as another molecule but it’s atoms are arranged differently in space
Strong acid or base
And acid or base that almost completely ionises in aqueous solution
Structural formula
Away representing molecules that shows the items carbon by carbon with the attached hydrogens and functional
Structural isomer
A molecule with the same molecular formula is another molecule but with the atoms connected in a different way
Sub shell
The subdivision of an energy level subshells may be SPDF
Substitution reaction
A reaction were some items from one react in a swap with atoms from another reactant
Successive ionisation energy
The energy needed to remove one mole of each subsequent electron from each ion in one mole of positively charged gaseous ions
Titration
A type of experiment used find the concentration of a solution that involves gradually adding one solution to a known volume of another until the reaction between the two is complete
Unsaturated hydrocarbon
A hydrocarbon with one or more carbon to carbon double bond is carbon to carbon triple bonds or an aromatic group
Van der Waals forces
Term referring to both and do you induced dipole dipole interactions and permanent dipole dipole interactions
Volatility
Substances tendency to evaporate
Water of crystallisation
The water contained in an ionic lattice
Weak acid or base
Said or base that only slightly ionises in aqueous solution
Yield
Amount products you get from a reaction
