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