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Physical Chemistry And Transition Metals Flashcards

1
Q

What is half life?

A

The time taken for half of a reactant to be used up.

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2
Q

What is the equation for calculating the rate constant from half life?

A

k= ln(2)/t1/2

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3
Q

What is the rate determining step?

A

The slowest step in a multi-step reaction.

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4
Q

How do you identify the rate determining step?

A

The rate equation only includes the reacting species involved in the rate determining step.
The orders of the rate equation match the number of species involved in the rate determining step.

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5
Q

What factors affect the rate constant?

A

Increasing the temperature shifts equilibrium to the right which increases the proportion of particles that exceed Ea.
When the temperature increases, the particles move faster and collide more frequently.

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6
Q

What is homogeneous equilibrium?

A

When equilibrium species all have the same state or phase.

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7
Q

What is heterogeneous equilibrium?

A

When the equilibrium species all have different states or phases.

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8
Q

What is a mole fraction?

A

The proportion by volume to the total volume of gases in a mixture.

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9
Q

What is partial pressure?

A

The contribution that a gas makes towards the total pressure.

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10
Q

Why must Kp only include gases?

A

Because only gases have partial pressures.

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11
Q

What effect does an exothermic reaction have on the equilibrium constant?

A

The equilibrium constant will decrease with increasing temperature.
Raising the temperature will decrease the equilibrium yield.

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12
Q

What effect does an endothermic reaction have on the equilibrium constant?

A

The equilibrium constant increases with increasing temperature.
Raising the temperature increases the equilibrium yield.

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13
Q

How do changes in concentration and pressure affect the equilibrium constant?

A

Kc and Kp are unaffected by changes in concentration and pressure.

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14
Q

How do catalysts affect the equilibrium constant?

A

It is unaffected by the equilibrium constant.

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15
Q

What is Kw?

A

The ionic product of water and its value is 1x10^-14.

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16
Q

What is a buffer solution?

A

A system that minimises pH changes when small amounts of acids or base are added.

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17
Q

What happens when more acid is added to a buffer solution?

A

-The concentration of acid increases.
-The acid ions react with the conjugate base.
-Equilibrium shifts to the left to remove most of the acid ions.

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18
Q

What happens when more base is added to a buffer solution?

A

-The concentration of alkali increases.
-The little acid ions left react with the alkali ions.
-The weak acid dissociates which shifts equilibrium to the right to restore most of the acid ions.

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19
Q

pKa= ?

A

—logKa

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20
Q

What is a Brønstead-Lowry acid?

A

A species which donates protons.

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21
Q

What is a Brønstead-Lowry base?

A

A species with accepts protons.

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22
Q

pH= ?

A

—log[H+]

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23
Q

[H+]= ?

A

10^—pH

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24
Q

Ka= ?

A

10^—pKa

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25
What is a weak acid?
A species which only partially dissociates in a solution.
26
What is a strong acid?
A species which fully dissociates in a solution.
27
What is the relationship between Ka and strong acids?
Ka is higher and pKa is smaller.
28
What is the relationship between Ka and weak acids?
Ka is smaller and pKa is larger.
29
What is lattice enthalpy?
The measure of the strength of an ionic bind in a giant ionic lattice.
30
What is the standard enthalpy of formation?
The enthalpy change that takes place when one mole of a gaseous atoms from the element in its standard state under standard conditions.
31
What is the standard enthalpy of atomisation?
The enthalpy change that takes place for the formation of one mole of gaseous atoms from the element in its standard state under standard conditions.
32
What is the first ionisation energy?
The enthalpy change required to move one electron from each atom in one mole of gaseous atoms to form one mole of gaseous +1 ions.
33
What is the first electron affinity?
The enthalpy change that takes place when one electron is added to each atom in one mole of gaseous atoms to form one mole of gaseous -1 ions.
34
What is the standard enthalpy change of solution?
The enthalpy change that takes place when one mole of a solute dissolves in a solvent.
35
What is the enthalpy change of hydration?
The enthalpy change the comes with dissolving gaseous ions in water to form one mole of aqueous ions.
36
What are the properties of ionic compounds?
- High melting and boiling points. -Soluble in polar solvents. -Conduct electricity when molten or dissolved.
37
How does increasing ionic size affect lattice enthalpy?
-Ionic radius increases. -Attraction between ions decreases. -Lattice energy becomes less negative. -The melting point decreases.
38
How does increasing ionic charge affect lattice enthalpy?
-Ionic charge increases. -Attraction between ions increases. -Lattice energy becomes more negative. -The melting point increases.
39
How does increasing ionic size affect hydration?
-The ionic radius increases. -The attraction between the ion and water molecules decreases. -The hydration energy becomes less negative.
40
How does increasing ionic charge affect hydration enthalpy?
-Ionic charge increases. -The attraction between ions and water molecules increases. -The hydration enthalpy become more negative.
41
What is entropy?
A measure of the dispersal of energy in a system, which increases as the system is more disordered.
42
What is the standard entropy?
The entropy of one mole of a substance under the standard conditions.
43
What is reduction?
The gain of electrons or the decrease in oxidation number.
44
What is oxidation?
The loss of electrons or the increase in oxidation number.
45
What is an oxidation number?
It takes electrons from the species being oxidised and it contains the species that is reduced.
46
What is a reducing agent?
It adds electrons to the species being reduced and it contains the species that is oxidised.
47
Why is a salt bridge used when making an electrode?
It allows the ions to flow.
48
When the electrode potential value is more negative…?
-The greater the tendency to lose electrons and undergo oxidation. -They have less tendency to gain electrons and reduction. -The greater the reactivity of a metal in losing electrons.
49
When the electrode value is more positive…?
-It has a greater tendency to gain electrons and undergo reduction. -It has a less tendency to lose electrons and undergo oxidation. -The greater the reactivity of a non-metal in gaining electrons.
50
Where are d-block elements located?
Between groups 2 and 13.
51
What is the end of the electronic configuration of chromium?
3d5 4s1
52
What is the end of the electronic configuration of copper?
3d10 4s1
53
When d-block elements form ions and atoms…?
The 4s orbital is the first to fill and the first to empty.
54
What are the properties of transition metals and their compounds?
-They form compounds where the transition element has different oxidation states. -They form coloured compounds. -The elements and their compounds can act as catalysts.
55
What is a ligand?
A complex ion formed when one or more molecules or negatively charged ions bond to a central metal ion.
56
What is a dative covalent bond?
When one of the bonded atoms provides both of the electrons for the shared pair.
57
What is a monodentate ligand?
A ligand that donates one pair of electrons to a central metal ion.
58
What is a bidentate ligand?
Ligands that donate two lone pairs to the central metal ion.
59
What is ligand substitution?
When one ligand is replaced by another ligand.
60
What is the test and result for ammonium ions?
Damp red litmus paper will turn blue.
61
What is the test and result for a carbonate ion test?
Add dilute nitric acid and effervescence is produced.
62
What is the test and result for sulfate ions?
Add barium ions and a white precipitate of barium sulfate is formed.
63
What is the test and result for halide ions?
Add aqueous silver ions. Chlorine forms a white precipitate and is soluble

Chemistry (5 decks)

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