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Alevel > Steers Chem > Flashcards

Steers Chem Flashcards

1
Q

What happens to first ionisation energies down a group

A

Decreases

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2
Q

Causes of change in ionisation energy down a group

A

Atomic radius increases, shielding increases, nuclear attraction decreases- ionisation energy decreases

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3
Q

Trend in first ionisation energy across a period

A

Increases

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4
Q

Causes of trend in ionisation energy across a period

A 
Nuclear charge increases
Same shell-similar shielding
Nuclear attraction increases
Atomic radius decreases
Ionisation energy increases
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5
Q

Trends down group 2

A

Reactivity inc
Ionisation energy dec
Solubility inc
pH inc- more alkaline down group

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6
Q

Why does boiling point increase down group 7

A

More electrons
Stronger London forces
more energy necessary to break forces
Boiling point increases

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7
Q

Why does reactivity decrease down group 7

A

Atomic radius increases
More shielding
Less nuclear attraction to attract electron to get full outer shell
Reactivity decreases

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8
Q

Why does reactivity increase down group 2

A

Atomic radius increases
Nuclear attraction decreases
Shielding increases
Less energy needed to lose electrons

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9
Q

G2+O2

A

MgO

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10
Q

Mg h20

A

Mg(oh)2 and h2

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11
Q

Mg hcl

A

Salt and water

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12
Q

MgO h20

A

Mg(oh)2

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13
Q

Solubility of group 2 hydroxides

A

Increases down group as has more OH- ions

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14
Q

Risks of chlorine in water

A

React with hydrocarbons ch4 from decaying veg to produce chlorinated hydrocarbons suspected of causing cancer

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15
Q

First electron affinity vs second

A

First=exo

2nd=endo

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16
Q

Why are second electron affinities endo

A

Second electron being gained by a negative ion which repels which needs energy to force it on

17
Q

Enthalpy change of solution

A

The enthalpy change that takes place when one mole of solute dissolves in a solvent

(NaCl—–> Na+. Cl-

18
Q

Enthalpy change of hydration

A

The enthalpy change that accompanies the dissolving of gaseous ions in water to form one mole of aqueous ions

19
Q

Effect of ion size on lattice enthalpy

A

Ionic radius increases
Attraction between ions dec
Lattice energy less exothermic
Mp decreases

Smaller ions attract more easily. More energy given off

20
Q

Effect of charge on lattice enthalpy

A

Charge increases
Ions more attraction
More negative lattice energy
Mp increases

Ions attract more easily give off more energy

21
Q

Effect of ion size on hydration

A

Ionic radius increases
Attraction between ion and water decrease
Hydration enthalpy less -ve (increases)

22
Q

Effect of ionic charge on hydration

A

Ionic charge increases
Attraction with water increase
Become more -ve
More energy given off

23
Q 
Cu2+
Fe2+
Fe3+
Mn2+
Cr3+
A 
Add sodium hydroxide to metal sulfate 
Cu2+ blue ppt of caoh 
Fe2+ green ppt 
Fe3+ brown ppt
Mn2+ off white ppt 
Cr3+ forms dark green solution
24
Q

Standard entropy

A

Entropy of one mile of substance under standard conditions

Alevel (8 decks)

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