Module 3 Flashcards

1
Q

Define first ionisation energy

A

the energy required to remove one electron from each atom in one mole of gaseous atoms of an element

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2
Q

Which factors affect ionisation energy across a Period?

A
Atomic Radius Decreases
Nuclear Charge Increases
Electron Shielding Remains Similar
(Greater Charge Density)
First Ionisation Energy Increases
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3
Q

Which factors affect ionisation energy down a Group?

A

Atomic Radius Increases
Nuclear Attraction Decreases
Electron Shielding Increases
First Ionisation Energy Decreases

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4
Q

Describe Metallic Bonding

A

The electrostatic attraction between positive metal ions and a sea of delocalised electrons

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5
Q

What is the pattern in melting points across the period table?

A

It increases from groups 1 to 14 (giant structures) and then decreases from groups 15 to 18 (simple molecules with IM-forces) ((After Si))

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6
Q

Why does the reactivity of group 2 elements increase down the group?

A

Group 2 elements react by losing electrons, further down the group the attraction between the outer-electron and the nucleus decreases

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7
Q

Describe the trend in the solubility of group 2 hydroxides?

A

As you descend the group, solubility of the group 2 hydroxide increases and hence, pH increases also

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8
Q

How does the reactivity of the Halogens change down the group?

A

It decreases, because the atomic radius is increasing and so is the shielding

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9
Q

What is a disproportionation reaction?

A

One where the same species is both oxidised and reduced

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10
Q

State a concern associated with putting chloride ions in the water to sterilise it

A

It might react with alkanes, to form carcinogenic haloalkanes

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11
Q

What is the correct order to carry out the qualitative negative ion tests?

A

1) Carbonate (add nitric acid, makes carbon dioxide)
2) Sulphate (add barium nitrate, makes a white ppt)
3) Halide (add silver nitrate, makes coloured ppts)
(‘4’) add ammonia to coloured ppts, only iodine will not dissolve)

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12
Q

Define enthalpy change of reaction

A

the enthalpy change that accompanies a reaction in the molar quantities in the equation

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13
Q

Define enthalpy change of formation

A

the enthalpy change that accompanies the formation of one mole of a compound from its elements

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14
Q

Define enthalpy change of combustion

A

the enthalpy change that takes place when one mole of a substance reacts completely with oxygen

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15
Q

Define enthalpy change of neutralisation

A

the enthalpy change that accompanies the reaction of an acid by a base to produce one mole of water

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16
Q

What is the equation for energy change (involving specific heat capacity)?

A

q=mc Δt

17
Q

What can cause inaccuracies in the experimental enthalpy change value compared to the standard one?

A

It was measured in non-standard conditions
Incomplete combustion occurred
Heat was lost (transferred) to the surroundings

18
Q

What is the bond enthalpy of a bond?

A

The energy required to break one mole of the bond in its gaseous state

19
Q

What factors can affect the rate of a reaction?

A

Concentration / Pressure
Temperature
Use of a catalyst
Surface area (if solid)

20
Q

What defines whether or not a collision is effective in a reaction?

A

If it has or not collided in the correct orientation, and with enough energy, to actually react

21
Q

What are the key features of catalysts?

A

They lower activation energy, without undergoing any permanent change themselves (always regenerated)

22
Q

What is the difference between Homogenous and Heterogeneous catalysts?

A

Homogenous catalysts are in the same state as the reactants, and often form intermediates. Heterogeneous catalysts are in a different state to the reactants and work by adsorption and desorption

23
Q

What is autocatalysis?

A

When the product of a reaction acts as a catalyst for that reaction

24
Q

What does the area under the curve resemble in the Boltzmann Distribution?

A

The total number of particles

25
Q

What effect does increasing temperature have on the Boltzmann curve?

A

It stretches the curve horizontally, lowering the maximum point, but the total area remains the same

26
Q

What is Le Chatelier’s Principle?

A

When a system is in a dynamic equilibrium and is subjected to an external change, the system will readjust itself to counteract the change

27
Q

In a dynamic equilibrium, what effect will increasing the temperature have?

A

It will encourage the endothermic direction, to oppose the increase

28
Q

In a dynamic equilibrium, what effect will increasing the pressure have?

A

It will encourage the reaction that produces fewer moles of gas, to oppose the increase