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Chemistry Dictionary > Unit 1 > Flashcards

Unit 1 Flashcards

1
Q

Oxidation Number

A

The number of electrons that need to be added to (or taken away from) an element to make it neutral

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2
Q

Atomic Number

A

The number of protons in the nucleus of an atom

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3
Q

Mass Number

A

Is the number of protons + the number of neutrons in the nucleus of an atom

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4
Q

Isotopes

A

Are atoms having the same number of protons but a different number of neutrons

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5
Q

Ion

A

Is a particle where the number of electrons does not equal the number of protons

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6
Q

Positive Ions (Cations)

A

Form when an atom loses one or more electrons
Eg: K —> K(+) + e-

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7
Q

Negative Ions (Anions)

A

Form when an atom gains one or more electron
Eg: F + e- —> F(-)

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8
Q

Alpha Particles

A

They are a cluster of two protons and two neutrons and are therefore positively charged

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9
Q

Beta Particles

A

Fast moving electrons and therefore are negatively charged

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10
Q

Gamma Rays

A

High energy electromagnetic radiation therefore no charge

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11
Q

Half-life

A

Time taken for half the atoms in a radioisotope to decay

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12
Q

Atomic Orbital

A

Is a region within an atom that can hold up to two electrons with opposite spins

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13
Q

Electronic Configuration

A

Arrangement of electrons in an atom

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14
Q

First Ionisation Energy

A

The energy required to remove one electron from each atom in one mole of its gaseous atoms
X (g) ——> X+ (g) + e-

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15
Q

Nuclear Energy

A

The greater the nuclear charge, the greater the attractive force on the outer electron

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16
Q

Electron Shielding

A

The repulsion between electrons in different shells. Inner shell electrons repel outer shell electrons.
Therefore the more filled inner shells or sub-shells there are, the smaller the attractive force on the outer electron

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17
Q

Distance of outer electron from the nucleus

A

The greater the distance, the smaller the attractive force on the outer electron

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18
Q

Successive Ionisation Energy

A

The measure of energy needed to remove each electron in turn until all the electrons are removed from an atom

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19
Q

Convergence Limit

A

When spectral lines become so close together they have a continuous band of radiation and separate lines cannot be distinguished

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20
Q

Relative Atomic Mass

A

Average mass of one atom of the element relative to one-twelfth the mass of one atom of Carbon-12

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21
Q

Relative Isotopic Mass

A

Mass of one atom of an isotope relative to one-twelfth the mass of one atom of Carbon-12

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22
Q

Relative Formula Mass

A

Of a compound is the sum of the relative atomic masses of all atoms present in it’s formula

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23
Q

Mass Spectrometer

A

Used to calculate the average mass of an atom of an element, the mass of the isotopes of the element together with their relative abundances known

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24
Q

Molecular Ion

A

Positive ion formed in a mass spectrometer from a whole molecule

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25
Fragmentation
Splitting of molecules, in a mass spectrometer, into smaller parts
26
One Mole
Is the amount of any substance that contains the same number of particles as there are atoms in exactly 12g of Carbon-12
27
Avogadro’s Constant
The number of atoms per mole (6.022 X 10 power of 23 mol-1)
28
Molar Mass
The mass of one mole of a substance
29
Stoichiometry
Molar relationship between the amounts of reactants and product in a chemical reaction
30
Empirical Formula
The simplest formula showing the simplest whole number ratio of the number of atoms of each present element
31
Molecular Formula
Shows the actual number of atoms of each element present in the molecule. It is a simple multiple of the EF
32
Molar Volume
The volume per mole of a gas, Vm
33
Atom Economey
Mass of required product ———————————- X 100 Total mass of reactants
34
Percentage Yield
Mass of product obtained ———————————— X 100 Max theoretical mass of product
35
Ionic Bond
Is a bond formed by the electrical attraction between positive and negative ions
36
Covalent Bond
Has a pair of electrons with opposed spin shared between two atoms with each atom giving one electron
37
Coordinative Bond
Covalent bond in which both shared electrons come from one of the atoms
38
Electronegativity
Measure of the ability of an atom in a covalent bond to attract the electron bonding pair
39
Polar Bond
Has one end of the bond with a slightly positive charge and the other end with a slightly negative charge I.E, a dipole (neutral)
40
Dipole
Separation of charge within a molecule
41
Intermolecular Bonding
Weak bonding holding the molecules together Eg: a liquid and governs the physical properties of a substance
42
Intramolecular Forces
Strong bonding between the atoms in a molecule and governs its Chemistry
43
Van Der Waals Forces
Weak intermolecular forces made up of dipole-dipole and induced dipole-induced dipole forces of attraction
44
Hydrogen Bond
Relatively strong intermolecular bond having a hydrogen atom joined to a very electronegative element in a a molecule and bonding to another electronegative element in another molecule
45
Bond Pair
Two electrons having opposed spins that bond two atoms in a molecule together by a covalent or coordinate bond
46
Lone Pair
Two electrons having opposite spins that belong to one atom only and are not involved in bonding to other atoms
47
Solute
Substance that dissolves in the solvent (can be solid, liquid or gas)
48
Solvent
Liquid medium in which the solute dissolves, commonly water
49
Saturated
Solution that cannot dissolve any more solute under the existing conditions
50
Polar
Molecule with separation of delta positive and delta negative charge
51
Crystal Coordination Number
The number of anions around each cations in an ionic lattice and vice versa
52
Delocalised
Means that an electron is not attached to a particular atom - it can move around between other atoms
53
Reducing Agent
Gives the electron to another species that is therefore oxidised by its loss
54
Oxidising Agent
Remove an electron from another species and it is therefore reduced
55
Redox
A chemical reaction in which an electron is transferred from one species - the reducing agent - to another species, which is reduced by the receiving the electron
56
Volatility
Describes how readily a substance vaporises
57
Electronegative Element
Having a strong affinitive for an electron in this acting as an oxidising agent
58
Dynamic Equilibrium
When the forward and reverse reactions occur at the same rate
59
Revirsible Reaction
One that can go in either direction, depending on the condition
60
Position of Equilibrium
The proportion of product to reactants in an equilibrium mixture
61
Le Chatelier’s Principle
States that other system are equilibrium is subjected to a change. The equilibrium tends to shift as to minimise the effect of change.
62
Acid
Is a proton (H+) donor
63
Base
Is a proton (H+) accepter
64
A Strong Acid
Fully disassociates in aqueous solution Eg: HCL
65
A Weak Acid
Partially disassociates an aqueous solution Eg: CH3COOH
66
pH
-log10[H+]
67
A Salt
Compound that forms on a metal ion replaces the hydrogen ion in an acid
68
Standard Solution
The concentration is accurately known

Chemistry Dictionary (2 decks)

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