Brainscape's Knowledge GenomeTM

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


See full index

Advanced Higher Chemistry > Inorganic Chemistry > Flashcards

Inorganic Chemistry Flashcards

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

What way can electromagnetic radiation be characterized

A

In terms of frequency and or wavelength

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

What is the order of the electromagnetic spectrum

A

Gamma, X-Rays, Ultraviolet, visible, infrared, radio

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

What units are wavelengths given in

A

Nano meters

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

What property is electromagnetic radiation said to have and why

A

It is said to have dual nature because it can behave as a wave or as a particle

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

Photon

A

A stream of particles that is given off when electromagnetic radiation is absorbed or emitted.

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

What happens when a photon is absorbed or emitted

A

Energy is gained or lost by electrons within the substance.

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

Energy associated with one mole of photons formula

A

E=Lhf or E=Lhc/wavelength

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

What happens when energy is transferred to atoms

A

Electrons may be promoted to higher energy levels

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

When is a photon emitted

A

When an excited electron moves from a higher energy level to a lower energy level.
This light energy emitted produces a spectrum made up of a series of lines at discrete energy levels.

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

What can the atomic emission spectrum be used for

A

Used to quantify and identify specific elements as each produces a specific absorption and emission soectra

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

Absorption spectroscopy

A

When EM radiation is directed at an atomized sample. Radiation is absorbed as electrons are promoted to higher energy levels.

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

Emission Spectroscopy

A

High temperatures are used to excite th electrons within atoms. As the electrons drop to lower energy levels photons are emitted. An emission spectrum is produced by measuring the intensity of light emitted at different wavelengths.

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

Different orbital shapes

A

S,P,D,F

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

Quantum number n

A

Indicates the main energy level for an electron and related to the size of the orbital

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

Angular momentum quantum number l

A

Determines the shape of the sub shell and have values from 0 to n-1

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

The magnetic quantum number m1

A

Determines the orientation of the orbital and can have values between -l and +l

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

The spin magnetic quantum number ms

A

Determines the direction of spin and can have a value of +1/2 or -1/2

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

Aufbau Principle

A

Electrons fill orbitals in order of increasing energy

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

Hunds Rule

A

When degenerate orbitals are available electrons fill singly keeping their spins parallel before spin pairing occurs.

20
Q

Pauli Exclusion Principle

A

No two electrons in one atom can have the same 4 set of quantum numbers therefore no orbital can hold more than two electrons and these two electrons must have opposite spins.

21
Q

Degenerate

A

Degenerate means of the same energy, all orbitals within each sub shell are degenerate

22
Q

S block

A

Groups 1 and 2

23
Q

P block

A

Groups 3-7

24
Q

D block

A

Transition metals

25
Q

What is associated with half full or full sub shells

A

Stability so they have higher ionisation energies

26
Q

VESPR Shapes

A

Linear-2
Trigonal Planar-3
Tetrahedral-4
Trigonal Bipyramidal-5
Octahedral-6

27
Q

Pair repulsion continuum

A

Non bonding/non bonding > Non bonding/bonding > bonding/bonding

28
Q

Transition metal definition

A

Metals with incomplete d sub shells in at least one of their ions

29
Q

Exceptions to the aufbau principle

A

Chromium and copper atoms

30
Q

What happens when atoms from the first row of transition metals form ions

A

4s orbitals are lost first then 3d

31
Q

What happens when oxidation number increases

A

Oxidation is taking place

32
Q

What happens when there is a decrease in oxidation number

A

Reduction is taking place

33
Q

What compounds are used as oxidising agents

A

Compounds containing metals with high oxidation states

34
Q

What compounds are used as reducing agents

A

Compounds containing metals with low oxidation states

35
Q

Ligands

A

Negative ions or molecules with non bonding pairs of electrons that they have to donate to a central metal atom forming dative covalent bonds

36
Q

How can ligands be classified

A

Monodentate, bidentate and hexadentate

37
Q

Coordination number

A

The amount of bonds from the central atoms to ligands

38
Q

What happens when metals form complexes

A

Their d orbitals are no longer degenerate

39
Q

How do d orbitals split

A

Occurs when electrons present in approaching ligands cause the electrons lying along axes to be repelled

40
Q

Strong field ligands

A

Ligands that cause a large difference in energy between subsets of d orbitals

41
Q

Weak field ligands

A

Ligands that cause a smaller difference in energy between subsets of d orbitals

42
Q

Spectrochemical series

A

The series in which ligands are placed in order by their ability to split d orbitals

43
Q

Colours of transition metal complexes

A

When light is absorbed as electrons in a lower energy d orbital are promoted to a d orbital of higher energy. If one colour of lights is absorbed the complementary colour will be present in the complex.

44
Q

What light causes electrons to transition to higher energy levels

A

When Energy corresponding to ultraviolet(200-400nm) and visible(400-700nm) is absorbed

45
Q

Heterogeneous catalysts

A

Catalysts that are in a different state of matter to reactants
Heterogenous catalyst can be explained as the formation of an activated complex on the surface of the reactant molecule And the adsorption of relative molecules onto active site. This is sue to the presence of unpaired d electrons. This provides alternative pathways of lower activation energy.

46
Q

Homogeneous catalysts

A

Catalysts that are in the same state as reactants
Homogeneous catalysis can be explained in terms of changing oxidation states with the formation of intermediate complexes.

Advanced Higher Chemistry (4 decks)

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