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Chemistry > Definitions > Flashcards

Definitions Flashcards

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1
Q

The enthalpy of formation

A

The standard enthalpy change when one mole of a compound is formed from its constituent elements under standard conditions, and all reactants and products in their standard states.

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2
Q

The enthalpy of combustion

A

The standard enthalpy change when one mole of a substance is burned completely in oxygen.

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3
Q

The enthalpy of atomization

A

The standard enthalpy change which accompanies the formation of one mole of gaseous atoms from the element in its standard state.

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4
Q

The first ionisation energy

A

The enthalpy change when one mole of gaseous atoms is converted into a mole of gaseous ions each with a single positive charge

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5
Q

The second ionisation energy

A

The enthalpy change when one mole of positively charged gaseous ions loses a mole of electrons.

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6
Q

The first electron affinity

A

The enthalpy change when a mole of gaseous atoms is converted to a mole of gaseous ions, each with a negative charge.

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7
Q

The second affinity

A

The enthalpy change when a mole of electrons is added to a mole of gaseous ions each with a single negative charge to form ions each with two negative charges.

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8
Q

Lattice enthalpy of formation

A

The standard enthalpy change when one mole of a solid ionic compound is formed from its gaseous ions.

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9
Q

Lattice enthalpy of dissociation

A

The standard enthalpy change when one mole of solid ionic compound dissociated into its gaseous ions.

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10
Q

Enthalpy of hydration

A

The standard enthalpy change when water molecules surround one mole of gaseous ions

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11
Q

Enthalpy of solution

A

The standard enthalpy change when one mole of solute dissolves completely in solution in sufficient solvent to form a solution in which molecules or ions are far enough apart to not interact with each other.

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12
Q

Mean bond enthalpy

A

The enthalpy change when one mole of gaseous molecules each breaks a covalent bond to form two free radicals averaged over a range of compounds.

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13
Q

Define Brønsted-Lowry acid

A

Proton Donor

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14
Q

Define Lewis acid

A

Electron pair acceptor

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15
Q

Define Acid derivative

A

Organic compound related to a carboxylic acid with the formula RCOZ where RCO represents an acyl group and Z = Cl, NHR, OR, or OCOR.

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16
Q

Define activation energy

A

The minimum energy that a particle needs in order to react; the energy difference between the reactants and the transition state.

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17
Q

Define aldehyde

A

An organic compound containing the general formula

RCHO

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18
Q

What are the alkaline earth metals

A

The metals in Group 2 of the periodic table

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19
Q

Define alkane

A

A hydrocarbon with C-C and C-H single bonds only with the general formula CnH2n+2

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20
Q

Define allotropes

A

Pure elements which can exist in different physical forms in which their atoms are arranged differently. for example, diamond, graphite, and buckminsterfullerene are allotropes of carbon.

21
Q

Define anaerobic respiration

A

The process by which energy is released and new compounds are formed within living organisms in the absence of oxygen.

22
Q

Define Atom Economy

A

Describes the efficiency of the reaction by comparing the total number of atoms in the product with the total number in starting materials.

23
Q

Define Atomic orbital

A

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

24
Q

Define Avogadro constant

A

Number of particles in a mole

6.022x1023

25
Q

Define Brønsted-Lowry base

A

Proton acceptor

26
Q

Define Lewis Base

A

Electron pair donor

27
Q

Define Base peak

A

The ion with the greatest abundance (tallest peak) in a mass spectrum

28
Q

Define Bond dissociation enthalpy

A

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

29
Q

Define Buffer

A

A solution which resists changes to the pH when small amounts of acid/base are added to it.

In the image, only solution B is the buffer.

30
Q

Define Calorimeter

A

An instrument for measuring the heat changes that accompany chemical reactions

31
Q

Define Carbocation

A

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

32
Q

Define Carbon-neutral

A

A process, or series of processes, in which as much carbon dioxide is absorbed from the air as is given out.

33
Q

Define Catalyst

A

A substance that alters the rate of a chemical reaction but is not used up in the reaction.

34
Q

Define Catalytic Cracking

A

The breaking, with the aid of a catalyst normally a zeolite of long-chain alkane molecules (obtained from crude oil) into shorter hydrocarbons. The reaction forms an ionic indeterminate. It also may produce some alkenes.

35
Q

Define Chelation

A

The process by which a multidentate ligand replaces a monodentate ligand in forming co-ordinate (dative) bonds to a transition metal ion.

36
Q

Define Chemical feedstock

A

The starting materials in an industrial chemical process.

37
Q

Define Chiral

A

This means ‘handed’. A chiral molecule exists in two mirror-image forms that are not superimposable.

38
Q

Define Chiral Centre

A

An atom to which 4 different atoms or groups are bonded.

39
Q

Define Co-ordinate bond

A

A covalent bond in which both electrons in the bond come from one of the atoms. (Also known as a dative bond)

40
Q

Define Co-ordination number

A

The number of ligand molecules bonded to a metal ion.

41
Q

Define Covalent bonding

A

A chemical bond where two atoms share a pair of electrons between them.

42
Q

Define Delocalisation

A

The process by which electrons are spread over several atoms and help bond them.

43
Q

Define Dipole-dipole forces

A

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

44
Q

Define displacement reactions

A

A chemical reaction in which one atom replaces another atom in a compound.

45
Q

Define displayed formula

A

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

46
Q

Define Disproportionation

A

Redox Reaction in which the oxidation number of an element both increases and decreases.

47
Q

Define Dynamic Equilibrium

A

Constant concentration as forward reaction rate = bascward reaction rate.

48
Q
A

Chemistry (37 decks)

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