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88 Cards in this Set

  • Front
  • Back

Activation energy

The minimum energy a particle needs in order to react. The energy (enthalpy) difference between the reactants and the transition state

Aldehyde

An organic compound with the general formula RCHO in which there is a c=o bond (carbonyl group)

Alkaline earth metals

Metals in group 2

Alkane

A hydrocarbon with single c-c and c-h bonds only. General formula of CnH2n+2

Allotrope

A pure element which can exist in different physical forms. Eg- diamond, graphite and buckminsterfullerene are all allotropes of carbon

Anaerobic respiration

Process by which energy is released and new compounds fomed in living things without oxygen

Atom economy

Describes the efficiency of a chemical reaction by comparing the total number of atoms in the product to those in the starting materials.


%atom economy= mass desired product/mass of reactants X100

Atomic orbital

A region of space around an atomic nucleus where there is a high probability of finding an electron

Avogadro constant

Total number of particles in 1 mole.

Avogadro's number

6.022X10^23

Bond disassociation enthalpy

The enthalpy change required to break a covalent bond with all species in gaseous state

Calorimeter

An instrument for measuring the heat changes that accompany chemical reactions

Catalyst

Substance that alters the rate of a chemical reaction but is not used up in the reaction

Catalytic cracking

The breaking, with the aid of a catalyst, of long chain molecules from crude oil into shorter chained mixed hydrocarbons

Carbocation

An organic ion in which one of the carbon atoms has a positive charge.

Carbon-neutral

A process, or series of processes in which as much CO2 is absorbed from the site as is given out.

Chemical feedstock

The starting materials in an industrial chemical process

Co-ordinate bonding

Covalent bonding in which both the electrons in the bond come from one of the atoms in the bond

Covalent bonding

Describes a chemical bond in which electrons are shared between two atoms

Cracking

The breaking of long chain hydrocarbons into shorter chain hydrocarbons

Delocalised

Electrons that are spread over several atoms and help to bond them together

Dipole-dipole force

An intermolecular force that results from the attraction between molecules with permanent dipoles

Displacement reaction

A chemical reaction in which one atom or a group of atoms replaces another in a compound

Displayed formula

The formula of a compound drawn out so that each atom and each bond is shown

Disproportionation

Describes a redox reaction in which the oxidation number of some atoms of a particular element increases and that of other atoms of the same element decreases

Dynamic equilibrium

A situation in which the composition of a reaction mixture does not change because of both forward and backward reactions are proceeding at the same rate

Electron density

The probability of an electron being found in a particular volume of space.

Election pair repulsion theory

A theory which explains the shapes of simple molecules by assuming that pairs of electrons around a central atom repel racketeer and thus take up positions as far away as podunk from another in 3D space

Electronegativity

The power of one atom to attract the pair of electrons in a covalent bond

Electrophile

An electron-deficient atom, ion or molecule that takes part in an organic reaction by attacking areas of high electron density in another reactant

Electrophilic addition

A reaction in which a c=c bond is saturated and in which the initial reaction is an attack by an electrophile

Electrostatic forces

The forces of attraction and repulsion between electrically charged particles

Elimination

A reaction in which an atom or group of atoms is removed from a reactant

Empirical formula

The simplest whole number ratio in which the atoms in a compound combine

Endothermic

A reaction where heart is taken in

Enthalpy change

A measure of heat energy given out or taken in when a chemical or physical change occurs at a constant pressure

Enthalpy diagram

A diagram on which the enthalpies of the products and reactants are plotted on a vehicle scale to show their relative levels

Equilibrium mixture

The mixture of products and reactants formed when a reversible reaction is allowed to proceed in a closed container until no further change occurs. The forward and backward reactants are still processing but at the same rate

Exothermic

Describes a reaction in which heat is given out. (Heat EXits)

Fingerprint region

The area of infrared spectrum below about 1500cm^-1. It is caused by complex vibrations of the whole molecule and is characteristic of a particular molecule

Fraction

A mixture of hydrocarbons collected over a particular range of boiling points during the fractional distillation of crude oil.

Free radical

A chemical species with an unpaired electron-usually highly reactive

Functional group

An atom or group of atoms in an organic molecule which is responsible for the characteristic reactions of that molecule

Group

A vehicle column of the elements in the periodic table. They have similar properties as they all have the same outer electron arrangement.

Half equation

An equation for a redox reaction which considers just one of the species involved and shows explicitly the electrons transferred to or from it

Heterogeneous catalyst

A catalyst which is in a different phase from the reactants. Eg: iron in the haber process

Homogenous catalyst

A catalyst which is in the same phase as the reactants

Homologous series

A set of organic compounds with the same functional group. The compounds differ in the length of their hydrocarbon chains

Hydrogen bonding

Strongest IMF where a hydrogen atom covalently bonded to a NOF interacts with another NOF

Incomplete combustion

a combustion reaction where there is insufficient oxygen for all the carbon to form carbon dioxide so carbon monoxide is produced or just carbon

Ionic binding

A chemical bond where electron(s) are transferred from one atom to another resulting in the formation of oppositely charged ions joined by strong electrostatic forces of attraction

Ionisation energy

The energy required to remove a mile of electrons from a mole of isolated gaseous ions or atoms

Isomer

One or two compounds with the same molecular formula but different structural formula

Ketone

An organic compound with the general formula R2CO in which there is a C=O carbonyl group

Lattice

A regular three dimensional arrangement of atoms ions or molecules

Leaving group

In an organic substitution reaction, the leaving group is an atom or group of atoms that is ejected from the starting material, normally taking an electron pair and forming a negative ion

Lone pair

A pair of electrons in the outer shell of an atom that is not involved in bonding

Maxwell-Boltzmann distribution

The distribution of energies (and speeds) of the molecules in a had our liquid

Mean bond enthalpy

The average value of the bond disassociation enthalpy for a given type of bond taken from a range of different compounds.

Metallic binding

Describes a chemical bonds in which outer electrons are spread over a lattice of metal ions in a delocalised system

Mole

A quantity of substance

Molecular formula

A formula that treks us the numbers of atoms of each different element that make up a molecule in a compound

Molecular ion

In mass spec this is a molecule of the sample which has been ionised and not broken up

Monomer

A small molecule that combines with many other monomers to form a polymer

Nucleons

Protons and neutrons

Nucleophile

An ion or group of atoms with a negative charge or partially negative charged area that participates in an organic reaction by attacking an electron deficient area in another reactant

Nucleophilic sub

Organ reaction where a molecule containing a partially charged positive carbon atom is attacked by a reagent with a negative charge

Oxidation

Loss of electrons

Oxidation state

The number of electrons lost or gained by an atom in a compound composite to an atom

Oxidising agent

Reduces another species

Percentage yield

Actual amount of product/theoretical amount X100

Periodicity

Regular reoccurrence of the properties of elements when they are arranged in the periodic table

Polar

A molecule in which the charge is not symmetrically distributed

Positive induction effect

Tendency of some atoms to release electrons via covalent bond

Redox reaction

Electrons transferred from one species to another

Reduction

Gain of electrons

Reducing agent

Oxidises other reactant

Relative atomic mass

Average mass of an atom / 1\12 mass of C12 atom

Relative formula mass

Average mass of an entity / 1\12 mass C12 atom

Relative molecular mass

Average mass of a molecule / 1\12 mass of C12 atom

Saturated hydrocarbon

Only contains hydrogen and carbon with only single bonds

Specific heat capacity

The amount of heat needed to raise the temperature of 1g of substance by 1k

Spectator ions

Ions that are unchanged during the chemical reaction

Enthalpy change of combustion

The amount of heat energy given out when 1 mile of a substance is completely burned in oxygen with all reactants and products in their standard states and conditions.

Enthalpy of formation

Heat change when 1 mole of substance is formed from its elements in its standard states and conditions

Nuclear forces

Forces that hold together protons and neutrons in the atoms nucleus

Structural formula

A way of writing the formula of an organic compound in which bonds aren't shown but each carbon is written separately with the groups of atoms attached to it

Van der waals force

An IMF that is caused by instantaneous dipoles and acts between All atoms and molecules