Unit 1a - Inorganic Chemistry Flashcards

(41 cards)

1
Q

How can electromagnetic radiation be described

A

wavelength and frequency

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2
Q

Electromagnetic radiation is said to have …..

A

dual nature

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3
Q

what is a photon

A

quantised energy proportional to the frequency of radiation

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4
Q

photons in high frequency have …. energy compared to low frequency

A

greater

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5
Q

What happens when a photon of light is emitted

A

after excited electrons are promoted to a higher energy level they fall back to lower energy levels emitting a photon of light

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6
Q

describe the appearance of emission and absorption spectrum

A

emission - black background with coloured lines

absorption - coloured background with black lines

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7
Q

what does absorption spectrum measure

A

the intensity of absorbed light at different wavelengths

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8
Q

what does the emission spectrum measure

A

the intensity of emitted light at different wavelengths

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9
Q

what is the principle quantum number (n)

A

indicates the main energy level for an electrons and is related to the size of the orbital

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10
Q

what is the angular momentum quantum number (l)

A

determines the shape of the subshell

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11
Q

what is the magnetic quantum number (m1)

A

determines the orientation of the orbital

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12
Q

what is the spin magnetic quantum number (ms)

A

determines the direction of spin

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13
Q

what is the aufbau principle

A

electrons fill orbitals in order of increasing energy

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14
Q

what is hund’s rule

A

when degenerate orbitals are available electrons fill signally before together

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15
Q

What does degenerate mean

A

of equal energies

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16
Q

what is pauli’s principle

A

no orbital hold more than two electrons and they must spin in opposite directions

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17
Q

what are the 4 blocks of the periodic table

18
Q

what does half-filled and full subshells suggest? and why?

A

higher ionisation energy because they have more stable electron configurations

19
Q

why do negatively charged electrons repel each other

A

they are arranged to minimise repulsion and maximise separation

20
Q

linear

A

2 bonding and no non-bonding

bond angle - 180

21
Q

trigonal planar

A

3 bonding pairs no non-bonding pairs

bond angle - 120

22
Q

tetrahedral

A

4 bonding pairs no non-bonding pairs

bond angle - 109.5

23
Q

trigonal pyramidal

A

3 bonding pairs and 1 non-bonding pair

bond angle - 107.5

24
Q

angular

A

2 bonding pairs and 2 non-bonding pairs

bond angle - 104.5

25
trigonal bipyramidal
5 bonding pairs and no non - bonding pairs | bond angle - 120
26
octahedral
6 bonding pairs and no non-bonding pairs | bond angle - 90 and 180
27
put order of repulsion in decreasing order
non-bonding/non-bonding pair non-bonding/bonding pair bonding/bonding pair
28
what is the definition of a transition metal
have incomplete d-subshell in a least one of their ions
29
Why are chromium and copper exception to aufbau principle
exempt due to special stability associated with d shell being half-filled or completely filled
30
what subshell do transition metals lose from first
4s rather than 3 d
31
all noble gases are characterised by the competition of outermost orbital. This orbital is
s or p orbitals
32
name Na3[Co(f)6]
sodium hexafluoridocolbalt (III)
33
how can oxidation be defined
increase in the oxidation number
34
how can reduction be defined
decrease in oxidation number
35
What is a ligand
A ligand is a molecule with at least one non-bonding pair of electrons available for bonding with a metal ion
36
ligand can be classed as
monodentate, bidentate up to hexadentate
37
what is the coordination number
the total number of bonds form the ligand to the central atom
38
what is a weak filed ligand
ligand which causes a small difference in energy between subsets of d orbital
39
what is a strong filed ligand
causes a large difference in energy between subsets of d orbitals
40
what colour is observed if magenta is being emitted
green light
41
what are heterogenous and homogeneous catalysts
homo - same state as reactant | hetro - different state form reactant