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module 6 aromatic test > Definitions (Understand) > Flashcards

Definitions (Understand) Flashcards

1
Q

Atomic number

A

the number of protons in the nucleus of an atom

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2
Q

Relative formula mass

A

the weighted mean mass of a formula unit compared with one-twelth of the mass of an atom of carbon 12

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3
Q

Relative molecular mass

A

the weighted mean mass of a molecule compared with one-twelfth of the mass of an atom of carbon-12.

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4
Q

Mole

A

the amount of substance containing as many particles as there are carbon atoms in exactly 12g of carbon-12 isotope

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5
Q

Molar mass

A

The mass of one mole of any substance, expressed in grams per mole.

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6
Q

Empirical formula

A

the simplest whole number ratio of atoms of each element in a compound

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7
Q

Molecular formula

A

the number of atoms of each element in a molecule

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8
Q

Lone pair

A

an outer-shell pair of electrons that is not involved in chemical bonding

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9
Q

Bonded pair of electrons

A

A pair of electrons shared between two atoms to make a covalent bond.

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10
Q

Permanent dipole

A

a small charge difference across a bond resulting from a difference in the electronegativities of the bonded atoms

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11
Q

Polar bond

A

A covalent bond with a permanent dipole

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12
Q

Polar molecule

A

a molecule with an overall dipole, taking into account any dipoles across bonds

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13
Q

Alkyl group

A

an alkane with a hydrogen atom removed, e.g. CH3, C2H5; alkyl groups are often shown as R

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14
Q

Alicyclic

A

Contains carbon atoms joined together in a ring that is not aromatic.

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15
Q

Aliphatic

A

Contains carbon atoms joined together in straight or branched chains.

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16
Q

Aromatic

A

Containing one or more benzene rings

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17
Q

Saturated

A

Containing single bonds only

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18
Q

Unsaturated

A

Containing a multiple carbon-carbon bond

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19
Q

Structural isomers

A

molecules with the same molecular formula but with different arrangements of atoms

20
Q

Homolytic bond fission

A

the breaking of a covalent bond with one of the bonded electrons going to each atom, forming two radicals.

21
Q

Heterolytic bond fission

A

the breaking of a covalent bond with both the bonded electrons going to one of the atoms, forming a cation (+ve ion) and an anion (-ve ion)

22
Q

Radical

A

a species with an unpaired electron

23
Q

Stereoisomers

A

compounds with the same structural formula but with a different arragement of atoms in space.

24
Q

General formula

A

the simplest algebraic formula for a member of a homologous series.

25
Q

Structural formula

A

a formula showing the minimal detail for the arrangement of atoms in a molecule

26
Q

Skeletal formula

A

a simplified organic formula, with hydrogen atoms removed from alkyl chains, leaving just a carbon skeleton and associated functional groups

27
Q

Displayed formula

A

a formula showing the relative positioning of all the atoms in a molecule and the bonds between them.

28
Q

Addition reaction

A

a reaction in which a reactant is added to an unsaturated molecule to make a saturated molecule.

29
Q

Electrophilic addition reaction

A

a type of addition reaction in which an electrophile is attracted to an electron-rich centre or atom, where it accepts a pair of electrons to form a new covalent bond

30
Q

Alkane

A

the homologous series with the general formula CnH2n+2

31
Q

Alkene

A

The hydrocarbon homologous series with one carbon-to-carbon and the general formula CnH2n

32
Q

Structural isomers

A

molecules with the same molecular formula but with different arrangements of atoms

33
Q

Elimination reaction

A

the removal of a molecule from a saturated molecule to make an unsaturated molecule

34
Q

Dehydration

A

an elimination reaction in which water is removed from a saturated molecule to make an unsaturated molecule.

35
Q

Carbocation

A

An ion that contains a positively charged carbon atom.

36
Q

Average bond enthalpy

A

the average enthalpy change that takes place when breaking by homolytic fission 1 mol of a given type of bond in the molecules of a gaseous species.

37
Q

Standard conditions

A

a pressure of 100kPa (1 atmosphere), a stated temperature, usually 298 K (25degrees C), and a concentration of 1 mol dm^-3 (for reactions with aqueous solutions).

38
Q

Standard state

A

the physical state of a substance under the standard conditions of 100kPa (1 atmosphere) and 298 K (25 degrees C).

39
Q

Enthalpy change of reaction

A

the enthalpy change that accompanies a reaction in the molar quantities expressed the chemical equation under standard conditions, all reactants and products being in their standard states

40
Q

Homogenous catalyst

A

a reaction in which the catalyst and reactants are in the same physical state, which is most frequently the aqueous or gaseous state

41
Q

Heterogenous catalyst

A

a reaction in which the catalyst has a different physical state from the reactants; frequently, reactants are gases whilst the catalyst is solid.

42
Q

Hydrogen bond

A

a strong dipole-dipole attraction between an electron-deficient hydrogen atom (O-H, F-H or N-H) and a lone pair of electrons on a highly electronegative atom (H-O: H-F: or H-N:) on a different molecule

43
Q

Oxidation

A

loss of electrons or increase in oxidation number

44
Q

Substitution

A

a reaction in which an atom or group of atoms is replaced with a different atom or group of atoms

45
Q

Volatility

A

the ease with which a liquid turns into a gas. Volatility increases as boiling point decreases.

46
Q

Hydrolysis

A

a reaction with water or aqueous hydroxide ions that breaks a chemical compound into two compounds

module 6 aromatic test (29 decks)

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