Flashcards
Chemistry unit 1
Cards in this deck (81)
- 11st Ionisation energyEnergy required to remove one electron from one moles of gaseous atomes (one off each) to produce 1 mole of 1+ gaseous ions
- 21st electron affinityThe energy released from 1 mole of gaseous atoms each aquire an electron to form 1 mole of gaseous 1- ions
- 3Relative atomic massThe weighted average of the masses of an atom's isotopes relative to 1/12 mass of a carbon 12 atom
- 4Isotopic massThe mass of the atoms of an isotope of an element relative to the mass of atoms of isotope carbon-12
- 5SubshellAny of the one or more orbitals making up an electron shell/ energy level of an atom
- 6OrbitalAn energy state in the atomic model which describes where an electron is likely to be
- 7MoleUnit of measurement- the amount of any substance that contains as many particles as there are atoms in 12 grams of pure carbon-12
(avagadro's constant- 6.02 * 10 ^23) - 8Empirical formulaGives the proportions of elements present in a compound in lowest wholes number ratio
- 9Molecular formulaThe number of atoms of each of the elements present in one molecule of a compound
- 10Electrostatic forceAttraction or repulsion due to electric charge
- 11Ionic bondingType of chemical bond that involves the electrostatic attraction between oppositely charged ions
- 12Covalent bondChemical bond that involves the sharing of electron pairs between atoms
- 13Metallic bondingType of chemical bond between atoms in a metallic element, formed by the valence electrons moving freely through the metal lattice
- 14Chemical bond(Electrostatic) attraction between two or more atoms
- 15Lone pairPair of valence electrons that are not shared with another atom
- 16Charge densityThe electric charge per unit area of a surface, or per unit volume of a field or body
- 17Standard enthalpy of formationEnthalpy change which occurs when one mole of the compound is formed from its elements under standard conditions, and with everything in its standard state
- 18Standard enthalpy change of combustionThe enthalpy change which occurs when one mole of the compound is burned completely in oxygen under standard conditions, and with everything in its standard state
- 19The standard enthalpy change of neutralisationThe enthalpy change when solutions of an acid and an alkali react together under standard conditions to produce 1 mole of water
- 20Standard enthalpy change of reactionThe enthalpy change that occurs in a system when one mole of matter is transformed by a chemical reaction under standard conditions
- 21Standard enthalpy of atomizationThe enthalpy change when 1 mole of gaseous atoms is formed from its element in its defined physical state under standard conditions
- 22Average bond enthalpyThe average amount of energy needed to break a specific type of bond, measured over a wide variety of different molecules
- 23Hess's lawThe change of enthalpy in a chemical reaction is independent of the pathway between the initial and final state/ route taken
- 24PressureThe force that a gas exerts on the walls of its container.
- 25ConcentrationThe number of molecules or ions in a given volume of a substance
- 26CatalystA substance that increases the rate of a chemical reaction without itself undergoing any permanent chemical change (provides alternative route)
- 27Functional groupA group of atoms responsible for the characteristic reactions of a particular compound
- 28Structural formulaA formula that shows the arrangement of atoms in the molecule of a compound
- 29Molecular formulaA formula giving the number of atoms of each of the elements present in one molecule of a specific compound.
- 30Standard conditions298 K / 25 degrees C
1 ATM pressure/ 100 kPa - 31IsomerSame formula but a different arrangement of atoms in the molecule and different properties
- 32StereoisomersSame molecular formula and sequence of bonded atoms (constitution), but that differ only in the three-dimensional orientations of their atoms in space
- 33GeometricDiffer from each other in the arrangement of groups with respect to a double bond, ring etc.
- 34Structural isomersMolecules with the same molecular formula have bonded together in different orders
- 35Chain isomersComponents of the (usually carbon) skeleton are distinctly re-ordered to create different structures
- 36Position isomersThe substituting atom or group occupies different positions
- 37Functional group isomersSame molecular formula but different functional groups. This means that functional isomers belong to different homologous series
- 38Homologous seriesSeries/ group of organic compounds that have similar chemical properties and the same general formula
- 39AlkanesSeries of saturated hydrocarbons
- 40AlkenesSeries of unsaturated hydrocarbons containing a double bond
- 41Carboxylic acidOrganic acid containing one or more carboxyl groups
- 42EsterCompound produced by the reaction between an acid and an alcohol with the elimination of a molecule of water replacing the hydrogen of an acid by an alkyl or other organic group
- 43AlcoholOrganic compound whose molecule contains one or more hydroxyl groups attached to a carbon atom
- 44AmideAn organic compound containing the group —C(O)NH2, related to ammonia by replacing a hydrogen atom by an acyl group.
A compound derived from ammonia by replacement of a hydrogen atom by a metal, containing the anion NH2– - 45KetoneAn organic compound containing a carbonyl group =C=O bonded to two hydrocarbon groups, made by oxidizing secondary alcohols
- 46AldehydeAn organic compound containing the group —CHO, formed by the oxidation of alcohols
- 47Crude oilUnrefined petroleum
- 48Homolytic fissionChemical bond dissociation of a molecule by a process where each of the fragments retains one of the originally-bonded electrons
- 49Heterolytic fissionBoth of the electrons involved in the original bond remain with only one of the fragment species
- 50Free radicalAn uncharged molecule (typically highly reactive and short-lived) having an unpaired valence electron
- 51Free radical substitutionSubstitution reaction involving free radicals as a reactive intermediate. The reaction always involves at least two steps, and possibly a third
- 52Electrophilic additionAddition reaction between electrophile and nucleophile where a π bond is broken and two new σ bonds are formed.
The substrate of an electrophilic addition reaction must have a double bond or triple bond - 53ElectrophileIn general, electrophiles are positively charged species that are attracted to an electron rich centre. It participates in a chemical reaction by accepting an electron pair in order to bond to a nucleophile
- 54NucleophileDonates an electron pair to an electrophile to form a chemical bond in relation to a reaction.
All molecules or ions with a free pair of electrons or at least one pi bond can act as nucleophiles. - 55General formulaType of empirical formula that represents the composition of any member of an entire class of compounds
- 56Fractional distillationSeparation of a liquid mixture into fractions differing in boiling point (and hence chemical composition) by means of distillation
- 57ValenceElectrons involved in or available for chemical bond formation
- 58Atomic radiusSize of its atoms, usually the mean or typical distance from the center of the nucleus to the boundary of the surrounding cloud of electrons
- 59Metallic characterHow readily an atom can lose an electron
- 60Thermometric titrationTitration in which the end point is determined by measuring the temperature of a solution.
Yielding a plot of temperature over volume of titrant. Used for neutralization, precipitation, redox, organic condensation etc. - 61Lattice enthalpyMeasure of the strength of the forces between the ions in an ionic solid. The greater the lattice enthalpy, the stronger the forces
- 62Electrostatic theoryLike charges repel, unlike charges attract
- 63Polar moleculeAsymmetric molecule with a dipole. A polar molecule has a partial positive charge in one part of the molecule and complementary negative charge in another part
- 64Soluble/ insolubleAble to be dissolved, especially in water, or not.
- 65AtomThe basic unit of a chemical element
- 66ElementA substance that cannot be broken down into simpler substances by chemical means.
An element is composed of atoms that have the same atomic number - 67Ionan atom or molecule with a net electric charge due to the loss or gain of one or more electrons.
- 68MoleculeA group of atoms bonded together.
The smallest fundamental unit of a chemical compound that can take part in a chemical reaction - 69CompoundA substance formed when two or more chemical elements are chemically bonded together
- 70Double saltcomposition of a mixture of two simple salts but with a different crystal structure from either
more than one cation or anion, and is obtained by combination of two different salts which were crystallized in the same regular ionic lattice - 71Displacement reactionmore reactive element displaces a less reactive element from its compound
- 72BasepH of more than 7. When bases are dissolved in water, they are known as alkalis e.g. metal hydroxides, oxides and carbonates
- 73Relative molecular massThe sum of all the relative atomic masses of the atoms in a molecule
- 74Polarisation of an ionThe distortion of its electron cloud away from being spherical
Cation distorts anion - 75Organic compoundThe compounds containing carbon that are typically found in living systems
- 76HazardExisting situation/ condition that could cause harm
- 77RiskThe probability that the hazardous event/ something bad will happen
- 78Pi bondSide to side overlap of two p orbitals
- 79Thermochemical equationA balanced chemical equation which includes enthalpy change
- 80IsoelectronicSame electronic structure
- 81ElectronegativityTendency of an atom to attract bonding electron pair in a covalent bond
Information
- Description
- Flashcards on Chemistry unit 1, created by rose.begg on 19/05/2015.
- Created by
- rose.begg
- Views
- 2
- Rating