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Chemistry -Unit 1 > Electronic structure and the periodic table > Flashcards

Electronic structure and the periodic table Flashcards

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1
Q

What does the dual nature of electromagnetic radiation mean?

A

It can be considered as a stream of particles called photons with wave properties

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2
Q

What does h stand for and what is the value?

A

Planck’s constant: 6.63 x 10^-34

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3
Q

What does L stand for and what is the value?

A

Avogadro’s constant: 6.02 x 10^23

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4
Q

Give two equations for the Energy of a wave.

A

E=Lhv/1000

E=Lhc/1000 (wavelength)

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5
Q

What is wavenumber?

A

1/(wavelength)

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6
Q

What can flame tests be used for?

A

Can be used to identify the metal ions present in compounds.

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7
Q

What are flames tests especially effective on?

A

Group one metals

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8
Q

Where does the colour originate from when in a flame test?

A

The movement of electrons in the metal ion

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9
Q

Wen is energy released in an atom?

A

Electrons which have been excited into higher and more unstable energy levels tend to fall back down to their original energy levels releasing energy as they do so

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10
Q

What is the energy released as?

A

Visible light

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11
Q

Why is the flame between different metals a different colour?

A

Due to varying electron transitions

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12
Q

Why might a flame test not work very well?

A

If the colours are quite faint and hard to distinguish.

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13
Q

What is the lowest series which is in the UV part of the electromagnetic spectrum?

A

The Lyman series

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14
Q

What is the middle series which is in the visible light part of the electromagnetic spectrum?

A

The Balmer series

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15
Q

What is the highest series which is in the IR part of the electromagnetic spectrum?

A

The Paschen series

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16
Q

What are the lines in the emission spectra due to?

A

Due to photons of energy that are emitted when electrons in higher energy levels move to lower energy levels

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17
Q 
What is the opposite colour for: 
red, 
orange, 
yellow, 
green?
A

Blue-green,
Blue,
violet,
Purple

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18
Q

Can you give the shapes of molecules in increasing size.

A 
Linear
bent or angular 
trigonal planar
trigonal pyramidal
tetrahedral
Trigonal bipyramidal
Octahedral
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19
Q

What does the letter n represent?

A

The principle quantum number

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20
Q

What is the relationship between the value of n and the distance from the nucleus?

A

The larger the value of n, the further the electrons are from the nucleus and the greater their energy.

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21
Q

What does the high resolution emission spectrum of sodium suggest?

A

That the shells are subdivided into subshells.

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22
Q

Which subshell has the lowest energy?

A

S

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23
Q

What is the principle quantum number?

A

It indicates the energy of the electron, it’s distance from the nucleus and any electron with the same principle quantum number occupies the same electron shell or energy level.

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24
Q

What is the angular momentum quantum number?

A

It specifies the shape of the orbital by using the letters s,p,d,f

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25
Q

What is the magnetic quantum number?

A

It provides information about the number of orbitals and their orientation or direction in space

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26
Q

How are the p orbitals aligned?

A

They are dumbbell shaped and are aligned along one of the three perpendicular axes.

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27
Q

Which of the d orbitals has a different shape

A

the dz^2

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28
Q

What is Heisenberg’s uncertainty principle?

A

‘It is impossible to define with absolute precision, simultaneously , both the position and momentum of an electron, so electrons can be described in terms of probability rather than by definite position.

29
Q

What is the spin quantum number?

A

Determines the direction of spin an electron has within an orbital. The electron can spin in one of two directions denoted as +1/2 or -1/2

30
Q

What is an atomic orbital?

A

Defined as the region in space in which the probability of finding an electron is high.

31
Q

What is the Pauli exclusion principle?

A

No two atoms in the same atom can have the same four quantum numbers

32
Q

What is the aufbau principle?

A

electrons fill orbitals in order of increasing energy meaning the lowest energy subshells are filled first

33
Q

What’s the benefit of orbital box notation over spectroscopic notation?

A

Orbital box notation shows the spin of electrons in degenerate orbitals

34
Q

What is a covalent bond?

A

A covalent bond is formed when atomic orbitals overlap to form a molecular orbital

35
Q

What is the effect on the potential energy when two s orbitals overlap?

A

There is a drop in potential energy

36
Q

What is a dative covalent bond?

A

When one atom provides both the electrons that form the bond, the bond is identical to normal covalent bonds

37
Q

Draw the lewis dot diagram for ozone.

A

(complete in jotter)

38
Q

What molecular shape would you get if the prediction calculation gave you the number 2,3,4,5,6?

A
  1. Linear
  2. Trigonal planar
  3. Tetrahedral
  4. Trigonal bipyramidal
  5. Octahedral
39
Q

What is the condition for the prediction calculation to work?

A

All the electron pairs hace to be bonding pairs

40
Q

What is the drawing for the molecular shapes?

A

(complete in jotter)

41
Q

Which elements don’t fill up the 4s orbital before the 3d?

A

Chromium and Copper

42
Q

Why don’t they fill up the 4s orbital before the 3d?

A

There is a special stability associated with all the d orbitals being either half filled or completely filled

43
Q

Why can transition metals have variable valencies?

A

Because transition metals can lose the 4s electron and some of or all of the three d electrons to form positive ions

44
Q

Why are 4s electrons lost before 3d electrons?

A

The presence of electrons in the 3d subshell raises the energy of the 4s electrons above that of the 3d

45
Q

What is a d block transition metal?

A

Those elements that contain an incomplete d subshell in at least one of their ions

46
Q

What is the oxidation state of Fe 2+

A

+2

47
Q

What is the oxidation state in an uncombined element or Cl2?

A

0

48
Q

What must the algebraic sum of all the oxidation numbers in a molecule be equal to?

A

0

49
Q

What must the algebraic sum of all the oxidation numbers in a polyatomic ion be equal to?

A

The charge on the ion

50
Q

What type of ligands exist?

A

Monodentate
Bidentate
Hexadentate

51
Q

What is a complex?

A

A central metal ion surrounded by ligands?

52
Q

What are ligands?

A

Negative ions or uncharged molecules (electron donors) with one or more lone pair electrons

53
Q

What is a bidentate ligand?

A

A ligand which donates two pairs of electrons

54
Q

Give an example of a hexadentate ligand

A

EDTA

55
Q

What is the coordination number?

A

The number of bonds from the ligands to the central metal ion

56
Q

What are the negative ion names for iron copper lead and tin?

A

Iron: ferrate
Copper: cuprate
Lead: plumbate
Tin: stannate

57
Q

What is the name given to the colour of the solution after white light has been transmitted through it?

A

The complementary colour

58
Q

Which two orbitals are split upwards in the splitting of the d orbitals?

A

The dx^2-dy^2 and dz^2

59
Q

Which of the d orbitals are split downwards?

A

dxy dzy dxz

60
Q

What is the crystal field strength?

A

The difference in energy between the two sets of orbitals

61
Q

Why do complexes of the same metal ion have different colours when different ligands are added?

A

Different ligands cause different crystal field splittings

62
Q

What is the spectrochemical series?

A

A measure of their ability to split the d orbitals

63
Q

How do catalysts speed up chemical reactions?

A

They provide an alternative reaction pathway with a lower activation energy

64
Q

Why can transition metals form a variable number of bonds?

A

Because of the availability of unoccupied or partially occupied d orbitals

65
Q

What does the presence of unpaired electrons or unfilled d orbitals allow?

A

Allows intermediate complexes to form, providing reaction pathways of lower energy

66
Q

When can a reactant species attach themselves to the transition metal in a compound?

A

When the transition metal has a coordination number of four

67
Q

Why can transition metals act as catalysts?

A

because of their ability to exist in a variety of different oxidation states

68
Q

What happens once the reaction has reached completion?

A

The transition metal returns to its original oxidation state

Chemistry -Unit 1 (7 decks)

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