Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Cfe Higher Chem > Random Mix (units 1 And 2) > Flashcards

Random Mix (units 1 And 2) Flashcards

You may prefer our related Brainscape-certified flashcards:
AP® Chemistry flashcards Periodic Table flashcards Chemistry 101 flashcards Organic Chemistry 101 flashcards
1
Q

What are the three types of Van der Waals forces?

A

London Dispersion Forces
Hydrogen Bonding
Permanent-dipole interactions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What type of intermolecular interactions occur in Ammonia (NH3)

A

Hydrogen bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Why does the first ionisation energy decrease as a group is descended?

A

There are added electron shells which increase shielding and decrease attraction for electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Why are the intermolecular forces in carbon tetrachloride (CCl4) only London dispersion forces?

A

The molecule although containing polar bonds is symmetrical, hence its polarity cancels each other out.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Why does propan-1-ol have a lower boiling point than ethan1,2diol

A

Ethan1,2diol has two hydrogen bonds per molecule whilst propan-1-ol only has one

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Which element would have the strongest metallic bonding; sodium, magnesium or calcium

A

Magnesium as it only has 3 electron shells (calcium has 4) and the outer shell contains 2 electrons per atom instead of the 1 in sodium (has greater nuclear charge)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

In terms of collision theory, explain the effect of temperature on reaction rate

A

Greater proportion of reactant particles will have sufficient activation energy and the rate of collisions will increase due to particles moving faster

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What effect does a catalyst have on a potential energy diagram?

A

Lowers the activation energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

In terms of bonds explain what is meant by an endothermic reaction

A

Product bonds can store more energy than reaction bonds

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the activated complex look like for the following reaction
H2 + Cl2 -> 2HCl

A

H—-H
| |
| |
Cl—Cl

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What formula is used to calculate reaction rate

A

Change in conc/volume/mass
Over
Change in time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Name a compound in which the solid is less dense than the liquid

A

Water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

A mixture of sodium sulphate and sodium phosphate contains 10 moles of sodium and 2 moles of phosphate ions. How many sulphate ions are present?

A

Na has a valency of 1, SO4 a valency of 2
2NaSO4 is sodium sulphate
The ratio is 2:1.
Na has a valency of 1, PO4 a valency of 3
3NaPO4 is sodium phosphate
Ratio is 3:1.
So if this has 2 moles of phosphate then there is 6 moles of sodium.
As there is 10 moles of sodium altogether then there is 4 moles of sodium in the sodium sulphate, meaning there is 2 moles of sulphate

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Why is there a large jump between the second and third ionisation energies of of calcium?

A

The third electron is being removed from a very stable full electron she’ll arrangement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What is the equation for the 2nd ionisation enthalpy of Oxygen?

A

O+(g) —> O2+(g) + e

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Name the reactants required to make ethylbutanoate

A

Ethanol and butanoic acid

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Esters can be used as flavourings. What other use do esters have?

A

Solvents

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What method is used to hydrolyse an ester?

A

Reflux

19
Q

What type of reaction is used to make soap molecules?

A

Alkaline hydrolysis

20
Q

What is the traditional name for propan-1,2,3-triol?

A

Glycerol

21
Q

Which types of molecules have a tuning fork shape?

A

Fats and oils

22
Q

What change in physical properties occur when a fat is dehydrogenated?

A

The melting point lowers and it turns into a liquid at room temperature (this is due to the formation of double bonds- making it more unsaturated)

23
Q

What chemical process occurs in the manufacture of margarine

A

Hydrogenation

24
Q

What is meant by hydrophobic

A

‘Water hating’

25
Q

Amide link

A

C=O-N-H

26
Q

What is the molecular formula of glycerol

A

C3H8O3

27
Q

What part of a soap molecule is hydrophilic and hydrophobic

A

Ionic Hydrophilic head (dissolves in water, not oil)

Non polar hydrophobic tail (doesn’t dissolve in water, oil soluble)

28
Q

What type of bonding holds alpha helixes together in proteins?

A

Hydrogen bonding

29
Q

What is the pattern of oxidation in alcohols?

A

Primary and secondary alcohols can be oxidised

Tertiary cannot

30
Q

Why is there a large jump in ionisation energy between the 2nd and third ionisation energies of magnesium?

A

The third electron is being removed from a very stable full electron arrangement

49
Q

What is formed at the highest potential energy point in a reaction

A

Activated complex

50
Q

Which factor is changed that allow particles to collide with greater energy?

A

Temperature

51
Q

The relative rate of a reaction is found to be

0.002 s-1 How long was the reaction timed for ?

A

500 seconds

52
Q

What is an activated complex?

A

An unstable intermediate structure formed by product bonds partially forming and reactant bonds partially breaking

53
Q

What is eA used for

A

To form an activated complex

54
Q

Why is energy absorbed in an end other,it reaction?

A

Because the products can store more energy than the reactants

55
Q 
What is the rate of reaction in the last 20 s before the reaction stops.
Mass(g)
4   2   0.5  0.5
Time (s)
0  20  40  60
A

0.075gs-1

56
Q

Which of the following could be a unit of measurement for a rate of reaction
0C\min, mg\0C, mg\hr

A

Mg/hr

57
Q

What would prevent a collision by reactant particles which have the sufficient activation energy

A

Incorrect collision geometry

58
Q

Explain the pattern of atomic size as a group is descended

A

Atomic size gets bigger as the number of shells increase decreasing attraction due to increased shielding effect

59
Q

Explain the pattern of ionisation energy as a period is crossed

A

Ionisation energy increases as atomic number increases due to increasing attractive forces.

60
Q

What is the intermolecular force of attraction found in oxygen gas

A

London dispersion forces

61
Q

How are London dispersion forces caused

A

The transient displacement of moving electrons within the electron cloud causes slightly momentary dipoles

62
Q

Why does phosphorous have a higher melting point than chlorine

A

Phosphorous is a larger molecule P4. Whilst Chlorine is diatomic. Hence larger London dispersion forces

Cfe Higher Chem (9 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions