Definitions Flashcards

1
Q

Define an isotope

A

atoms which have the same number of protons but different numbers of neutrons

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2
Q

Define relative isotopic mass

A

The mass of an atom of the isotope compared with 1/12th of the mass of an atom of carbon-12

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3
Q

Define relative atomic mass

A

The weighted mean mass of an atom of an element compared with 1/12th of the mass of an atom of carbon-12

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4
Q

Define relative molecular mass

A

The weighted mean mass of a molecule of that substance compared to 1/12th of the mass of an atom of carbon-12

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5
Q

Define relative formula mass

A

The average mass of a formula unit of that substance compared to 1/12th of the mass of an atom of carbon-12

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6
Q

Define a mole

A

The amount of substance that contains 6.02 x 10^23 particles

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7
Q

Define molar mass

A

The mass (in grams) of 1 mole of a substance. The units of molar mass are g mol ^-1

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8
Q

Define an orbital

A

A region of space that can hold up to 2 electrons, with opposite spins

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9
Q

Define an ion

A

An atom or group of atoms that has lost or gained one or more electrons

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10
Q

Define molecular formula

A

Shows the number of atoms of each element in one molecule of the substance

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11
Q

Define empirical formula

A

Shows the simplest whole number ratio of atoms of each element present in a substance

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12
Q

Define an acid

A

A compound that releases H+ ions in aqueous solution

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13
Q

Define a base

A

A compound that neutralises an acid to form a salt

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14
Q

Define an alkali

A

A type of base that dissolves in water to release hydroxide ions, OH-

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15
Q

Define a salt

A

A compound formed when the H+ ion from an acid is replaced by a metal ion or an ammonium ion

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16
Q

Define ionic bonding

A

The electrostatic attraction between positive and negative ions

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17
Q

Define a giant ionic lattice

A

A regular array of alternating positive and negative ions

18
Q

Define a covalent bond

A

The attraction of a shared pair of electrons for the nuclei of the bonded atoms

19
Q

Define a dative covalent bond

A

One in which both of the electrons in the covalent bond are provided by the same atom

20
Q

What does the electron pair repulsion theory state

A

That the electron pairs in the outer shell of the central atom in a molecule repel each other and therefore arrange themselves to be as far away from each other as possible

21
Q

Define electronegativity

A

The ability of an atom to attract the bonding electrons in a covalent bond

22
Q

Define induced dipole-dipole forces

A

Attractive forces between molecules that arise when random electron movements in one molecule cause an instantaneous dipole which in turn causes an induced dipole in the other molecule

23
Q

Define permanent dipole-dipole forces

A

Electrostatic attraction forces between polar molecules. The positive pole of one molecule is attracted to the negative pole of a neighbouring molecule

24
Q

Define a hydrogen bond

A

The intermolecular attraction between hydrogen covalently bonded to N, O, or F of one molecule and the LONE PAIR on N,O, or F in another molecule

25
Define metallic bonding
The attraction between a lattice of positive ions and a sea of delocalised electrons
26
Define oxidation
Loss of electrons or an increase in oxidation number
27
Define reduction
Gain of electrons or a decrease in oxidation number
28
Define oxidising agent
The substance that contains the element that is reduced
29
Define reducing agent
The substance that contains the element that is oxidised
30
Define functional group
An atom or group of atoms that gives a compound its characteristics chemical reactivity
31
Define homologous series
A series of compounds that have the same functional group and the same general formula, and in which successive members of the series differ by an extra CH2 unit
32
Define hydrocarbons
Compounds which contain only carbon and hydrogen
33
Define saturated
Compounds which contain single bonds between carbon atoms
34
Define isomer
Different compounds that have the same molecular formula
35
Define structural isomers
Compounds that have the same molecular formula but different structural formula
36
Define a radical
An atom or group of atoms which has an unpaired electron
37
Define homolytic fission
The breaking of a covalent bond with one of the bonded electrons going to each atom, forming 2 radicals
38
Define heterolytic fission
The breaking of a covalent bond forming a cation and an anion
39
Define stereoisomers
Compounds with the same structural formula but with a different arrangement in space
40
Define an electrophile
An electron pair acceptor
41
What is meant by the term standard solution
A solution of known concentration