Brainscape's Knowledge GenomeTM

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


See full index

Chemical Systems > Revision > Flashcards

Revision Flashcards

1
Q

What is Atomic Number?

A

Number of protons which is the same of the number of electrons.

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

What is mass number?

A

Number of protons and neutrons.

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

Isotopes?

A
  • Have a different number of neutrons.
  • Same chemical properties because same number and structure of electrons.
  • Different physical properties.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Mass Spectrometry is used to?

A
  • Find the relative atomic mass of elements.
  • Find the relative molecular mass of molecular compounds.
  • Identify elements and chemical compounds.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

TOF

A

Sample is converted into positive ions which are accelerated at high speeds in an electric field. Separation based on fact that the speed of an ion depends on its mass to charge ratio.

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

2 exceptions to electron configuration?

A
  • Chromium= 4s1, 3d5.
  • Copper= 4s1, 3d10.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Elements are classified into:

A
  • Metals- Lose e- to become positive ions.
  • Non- metals- Gain (share) e- to become negative ions.
  • Metalloids- Chemical behaviour of metalloids is between metallic and non- metallic.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Ionic Bonding?

A
  • Electrostatic force of attraction between oppositely charged ions.
  • Between metals (cations) and non- metals (anions).
  • Ions formed so they form a lattice.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Main physical properties of Ionic bonding?

A
  • Solid at room temperature.
  • High melting point.
  • Good conductors when dissolved/ melted.
  • Brittle.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Covalent Bonding?

A
  • Between 2 non- metals.
  • Dative Covalent is where one stone provides both e- to form the bond.
  • Atoms that provide the electron pair must have a pair which is not involved in bonding.
  • Simple covalent consists of small molecules.
  • Covalent bonds are strong but attraction forces is relatively weak.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

Main Physical Properties of covalent bonding?

A
  • Gases/ liquids at room temperature.
  • Low melting and boiling points.
  • Poor conductors of electricity.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What is electronegativity?

A

Measure of relative ability of an atom to attract the shared pair of e- in a covalent bond.

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

What does electronegativity depend on and is favoured by?

A
  • Large nuclear charge.
  • Small atomic radius.
  • Low shielding.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Across a period, electronegativity?

A
  • Increases.
  • Atomic radius decreases.
  • Nuclear charge increases.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Down a group, electronegativity?

A
  • Decreases.
  • Atomic radius increases.
  • Higher shielding.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

3 IMF?

A
  • VDW- non- polar molecules, the bigger the molecule the stronger the VDW.
  • Dipole- Dipole forces- Polar molecules, the bigger the difference the stronger the force.
  • Hydrogen bonding- HN, HO, HF.
    Lone pairs strongly attract the hydrogen, high boiling points, small enough so accessible by hydrogen atoms.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

Particle?

A

Building unit of a substance.

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

Empirical formula?

A

Simplest ratio of atoms present in a compound.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Molecular formula?

A

Actual number of atoms present in a compound.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Energy is needed to?

A

Break bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

Energy is released when?

A

Forming bonds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Energy Change=

A

Bonds breaking- Bonds forming.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

If you increase temperature?

A
  • Particles are faster.
  • Average kinetic energy increases.
  • Heat energy depends on amount of substance.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

Enthalpy Change=

A

Heat energy per amount of reactant given out/ taken in as the reaction proceeds.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Q

Collision theory?

A
  • A reaction can only occur when the energy of the collision has sufficient energy.
    Minimum energy a particle should have in order to become overcome the barrier is called the activation energy.
    At the beginning of the reaction, a large number of reactant particles leads to a large number of collisions which means a fast reaction rate.
    As the reaction takes place, reactant particles are consumed and the number of collisions decreases so the reaction rate slows down and eventually stops.
26
Q

Factors affecting reaction rate?

A
  • Temperature= High temperature, increased the frequency of collisions and energy of collisions, increasing reaction rate.
  • Catalyst- A catalyst does not change the frequency/ energy of collisions but reduces the activation energy. Catalyst provides and alternative pathway so increases number of successful collisions so faster reaction.
27
Q

Rate Expression?

A
  • K= rate constant.
  • To work out the overall order , add up indices.
  • H+ is a catalyst.
  • Units= Moldm-3s-1
28
Q

Initial rate method?

A

Start of reaction, tangent at 0.

29
Q

Different Orders?

A
  • Zero Order- No effect on initial rate.
  • First order- Same multiplication.
  • Second order- If something is multiplied by 2 other thing is multiplied by 4.
30
Q

Bronsted Lowry?

A
  • Acid= H+ (Proton) donor.
  • Base= H+ acceptor.
31
Q

Kw=

A
  • Kw= [H+][OH-].
  • At 298k for all aqueous solutions:
    Kw= 1*10^-14.
32
Q

For strong acid?

A

Use pH= -log(H+).

33
Q

For strong base?

A
  • Do Kw divided by [OH-].
  • Then sub the number into -log[H+].
34
Q

For weak acid?

A
  • [H+]= square root of Ka*c.
  • Then sub into -log.
35
Q

Larger Ka=

A

Stronger the weak acid.

36
Q

Smaller the PKa=

A

Stronger the weak acid.

37
Q

Le Chateliers Principle?

A

States a reaction at equilibrium will oppose a change in order to return to equilibrium.

38
Q

Action of buffers?

A
39
Q

When the word equimolar comes up, this means?

A

pH= the value of PKa.

40
Q

To work out a buffer calculation?

A

pH= pKa + log([A-]/[HA]).

41
Q

Blood buffering?

A
42
Q

Al3+ means that?

A

3 electrons have been lost.

43
Q

Cl- means that?

A

1 electron has been gained.

44
Q

Exceptions to oxidation states?

A

NaH
H2O2
OF2

45
Q

To work whether it is a reductive or oxidation half equation?

A

If the oxidation state decrease it is a reduction reaction.
If the oxidation state increases it is an oxidation reaction.

46
Q

Displacement reaction?

A

REDOX

47
Q

Metal displacement?

A

Most reactive metal will displace the least reactive metal.

48
Q

Reducing agent?

A

It is oxidised.
It is and electron donor.

49
Q

Oxidising agent?

A

It is reduced.
It is and electron acceptor.

50
Q

Vitamin C?

A

Known as ascorbic acid.
It is a reducing agent.
It oxidises cells.

51
Q

Bonding in organic molecules is predominantly?

A

Covalent.

52
Q

Structural Isomer?

A

They have the same molecular formula but different structural formulas.

53
Q

3 types of structural isomer?

A
  • Chain.
  • Position.
  • Functional group.
54
Q

Isomer may have?

A

Different physical and chemical properties.

55
Q

Stereoisomerism?

A

Have the same molecular and structural formula but atoms have different 3D spatial arrangement.

56
Q

2 types of stereoisomerism?

A
  • E/Z (geometric).
  • Optical.
57
Q

Chiral carbon is one that?

A

Has 4 different groups attached to it.

58
Q

Element?

A

Pure substance made of only one kind of atom.

59
Q

Chemical compound?

A

Made up of two or more types of atoms which are chemically bonded.

60
Q

The bigger that maintains the pH of human blood involves?

A

Carbonic acid and bicarbonate ion.

Chemical Systems (1 decks)

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