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Key Terms 2 Flashcards

(61 cards)

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1
Q

Oxidising Agent

A

Causes something else to be oxidised therefore is itself reduced and gains electrons

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2
Q

Reducing Agent

A

Causes something else to be reduced therefore is itself oxidised losing electrons.

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3
Q

Disproportionation

A

Where an element is both reduced and oxidised in a reaction

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4
Q

In what order does the positive and negative ion go when naming a molecule?

A

Positive first then negative

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5
Q

How do you name a transition metal in a molecule

A

Metal(Oxidation state in Roman Numerals)

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6
Q

For oxoanions, how do you name them in a molecule?

A

Their Name (Oxidation state of element that’s NOT oxygen)

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7
Q

For compounds with H+ acids, how do you name them in a molecule?

A

Their Name(Oxidation state of element(s) that are NOT oxygen)

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8
Q

Oxoanion

A

Negative ion with oxygen in

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9
Q

Orbital

A

Region of space in which electrons can be found

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10
Q

What shape is the p-orbital?

A

Dumbbell

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11
Q

What shape is the s-orbital?

A

Spherical

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12
Q

Chromium electron config

A

4s1 3d5

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13
Q

Copper electron config

A

4s1 3d10

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14
Q

Metallic Bonding

A

Positive atoms bonded by electrostatic attraction in a sea of delocalised electrons

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15
Q

Ionic bonding

A

Electrostatic attraction between a positive and negative ion

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16
Q

Malleable

A

be able to be pressed or hammered into shape without breaking

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17
Q

Ductile

A

To be able to be made or bent into a wire without breaking

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18
Q

Periodicity

A

A trend within the periodic table

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19
Q

How does a salt form?

A

When the hydrogen in an acid is replaced by a positive metal ion in a neutralisation reaction

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20
Q

Exothermic

A

A reaction in which releases energy

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21
Q

Endothermic

A

A reaction in which takes in energy

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22
Q

Enthalpy

A

The measure of the total internal energy of a chemical system

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23
Q

Conditions for Standard Enthalpy Change

A

To be at standard conditions and all reactants must be at 1 moldm

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24
Q

Standard conditions

A

298K and 100kPa

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25
Standard Enthalpy Change of Formation
When 1moldm of substance is formed from it's constituent elements in their standard states in standard conditions
26
Standard Enthalpy Change of Combustion
When 1 mole of a substance is completely combusted in excess oxygen under standard conditions
27
Standard Enthalpy Change of Neutralisation
When an acid and a base in their standard states react to form 2 mole of water under standard conditions
28
Standard Enthalpy Change of Reaction
When molar quantities as stated in a chemical equations react together under standard conditions
29
Bond enthalpy
The average energy required to break 1 mole of bonds in gaseous molecules
30
Hess' Law
Hess' Law states that the enthalpy change of a reaction is the same whatever route is taken from reactants to products
31
Heterogenous Catalysts
Where reactants and catalysts are in different states
32
Homogenous Catalysts
Where reactants and catalysts are in the same state
33
Adsorb
To stick to the surface
34
Maxwell Boltzmann Distribution
The effect of different conditions on the activation energy of molecules
35
Maxwell Boltzmann Distribution - Higher Temp
The peak (number of molecules) is lower and it is more to the right (higher energy)
36
Maxwell Boltzmann Distribution - Higher Conc.
It is higher at every point (more molecules)
37
Maxwell Boltzmann Distribution - Catalysts
Activation energy is more to the left (less energy required)
38
Catalyst Poisoning
Occurs in heterogenous catalysts - when poisoned by an impurity binding to the surface of the catalyst. These impurities bond irreversibly to catalysts however can be cleaned by oxidising chemicals with hot air.
39
Dynamic Equilibrium
Where the rate of the forward and backward reactions are equal and the concentrations of the reactants and products are constant.
40
Le Chatelier's Principle
If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change.
41
Saturated Hydrocarbons
Compounds that only contain single carbon bonds (every other bond hydrogen)
42
Unsaturated hydrocarbons
Compounds that do contain a C=C or triple carbon bond equivalent
43
Aliphatic
A compound containing carbon and hydrogen joined together in straight chains, branched chains, or non aromatic rings (so no benzenes)
44
Alicyclic
An aliphatic compound arranged in a non aromatic ring with or without side chains
45
Aromatic
Compounds that do contain a benzene (arene) ring
46
Homologous series
A family of organic compounds with the same functional group - same reactivity but different physical properties
47
Sigma Bond
A single covalent bond - end to end overlap of electron orbitals
48
Pi Bond
A covalent bond with sideways overlaps only occurring in p orbitals - they are either above or below the centre of the atom - has to already be a sigma bond to occur.
49
Structural Isomer
Same molecular formula but different structural formula
50
Chain isomer (structural isomer)
The length of the chain varies and therefore the chain varies
51
Position isomer (structural isomer)
Same functional/side group but different place
52
Functional group isomer (structural isomer)
Where functional group is different but same formula
53
Breaking bonds: exo or endothermic
Endothermic
54
Forming bonds: exo or endothermic
Exothermic
55
Polar Bond
A covalent bond where the shared pair of electrons is shared unequally between the bonding atoms
56
Dipole
A dipole is the separation of partial charges in a molecule
57
I.E drop between groups 2 and 3
In group 3, the electron is lost in the p-subshell which is further away as opposed to the s-subshell
58
I.E drop between groups 5 and 6
Group 6 takes an electron from a paired bond which is repelled more and therefore lost easier
59
Hess Law (Combustion)
reactants - products
60
Hess Law (Formation)
products - reactants
61
Maxwell-Boltzmann Axis
X - Amount of energy Y - Number of molecules (with that amount of energy)

Chemistry (6 decks)

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