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Chemistry > TOPIC 3 > Flashcards

TOPIC 3 Flashcards

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1
Q

Which elements conduct electricity

A

Sodium
Magnesium
Aluminium

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2
Q

Describe silicon’s ability to conduct electricity

A

Semi-conductor

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3
Q

Which element oxide is amphoteric

A

Aluminium oxide

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4
Q

What does amphoteric mean

A

Both acidic or basic

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5
Q

Sodium oxide and magnesium oxide produce acidic or basic solution?

A

Basic

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6
Q

Which element oxides produce an acidic solution

A

All elements after aluminium

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7
Q

Equation for sulfur trioxide with water

A

SO3 (g) + H2O (l) - H2SO4 (aq)

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8
Q

Equation for NO2 and water

A

3NO2 (g) + H20 (l) - 2HNO3 (aq) + NO (g)

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9
Q

Na2O, MgO, Al2O3

A

IONIC

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10
Q

SiO2, P4O10, SO3, Cl2O7

A

COVALENT

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11
Q

Describe pH trend of period 3 oxides

A

Basic to acidic

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12
Q

Describe electron affinity of metals and non-metals

A

Metals have a low EA because they lose electrons and non-metals have a high EA

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13
Q

Explain the pattern of electron affinity down group 7

A

Electron affinity decreases down group 7. Less energy is released if further away from nucleus because there is a lot of shielding, weaker force of attraction. Chlorine has the highest electron affinity as fluorine is the smallest atom and so has a high electron density - repels electron that is trying to get into the atom.

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14
Q

Why does oxygen have 2 EA’s

A

1st EA - exothermic like everything else

2nd - endo - due to electron getting into negative ion and energy needs to be put in to overcome the repulsion

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15
Q

Why are cations smaller than parent?

A

Because electrons are lost, # of shells decreases. Also, shielding decreases, stronger force of attraction. Nuclear charge increases.

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16
Q

Why are anions larger than parent

A

Extra electrons increase repulsion, increase shielding, weaker electrostatic force of attraction

17
Q

Why do transition metals have variable oxidation states

A

4s and 3d are of similar energy

Their sequential ionisation energies are close together

18
Q

What are the 3 ferromagnetic metals

A

IRON
COBALT
NICKEl

19
Q

What makes a metal paramagnetic

A

Anything with lone electrons in domains

20
Q

Diamagnetic?

A

FULL ELECTRONS in domains

21
Q

Why is FeCo ligand diamagnetic and not paramagnetic?

A

use SPECTROCHEMICAL series

CO has the greatest energy difference, d-orbitals split largely

electron comes down

22
Q

Explain how the colour of solutions containing transition metals can be used to determine their concentration.

A

Prepare samples of the transition metal ion over a range of known concentrations.
Add a small quantity of a suitable ligand to each in order to identify the colour.
Choose the filter which gives the largest absorbance, and measure the absorbance of each sample using this filter.
Plot a graph of absorbance against concentration.
Take the sample of unknown concentration, add the ligand to intensify the colour, and measure its absorbance using the same filter.
Use the graph to deduce the concentration of the solution.

23
Q

State three different features of transition metal complexes that cause a change in the
value of ΔE, the energy change between the ground state and the excited state of the
d electrons

A 
Identity of the metal
Charge (on the metal) / oxidation state / charge on complex
(Identity of the) ligands
Co-ordination number / number of ligands
Shape
24
Q

Why are complexes of d-orbitals coloured?

A

D-orbitals are partially filled

The d-orbitals split into 2 levels due to repulsion of electrons in ligand with electrons in d-orbitals

Energy difference between the 3 low energy d-orbitals and the 2 high energy d-orbitals corresponds to a certain frequency in the visible part of the spectrum

Electron transitions occur from the lower to higher energy level

Complementary colour is seen

25
Q

What is the coordination number?

A

The number of lone pairs bonded to the metal ion

26
Q

Why are complexes of d-orbitals coloured?

A

D-orbitals are partially filled

The d-orbitals split into 2 levels due to repulsion of electrons in ligand with electrons in d-orbitals as ligand approaches

Energy difference between the 3 low energy d-orbitals and the 2 high energy d-orbitals corresponds to a certain frequency in the visible part of the spectrum

When white light falls on solution, that energy is absorbed

Electron transitions occur from the lower to higher energy level

Complementary colour is seen

27
Q

Define ligands

A

Ligands are molecules or ions use lone pair of electrons to form coordinate covalent bonds with a central metal ion

28
Q

Define polydentate ligands

A

Polydentate ligands are species that have more than one lone pair of electrons to form coordinate covalent bonds to a central metal ion

29
Q

Physical properties of metals

A 
High electrical conductivity
High melting point
High tensile strength
Malleable
Ductile
30
Q

Chemical properties of metals

A

Variable oxidation states
Formation of complex ions
Coloured compounds
Catalytic behaviour

31
Q

Describe the changes in melting point across period 3

A

Na to Al = metallic bonding, number of delocalised electrons increases, greater attraction to cations, more energy required to overcome. Also, charge density increases as atoms get smaller

Si = giant covalent, strong covalent bonds require a lot of energy to overcome

S - Ar = simple molecular, weak intermolecular forces, not a lot of energy to overcome

32
Q

Which elements have the highest electron affinity?

A

Group 17 elements have incomplete outer energy levels and a high effective nuclear charge of +7 so attracts electrons the most

Chemistry (7 decks)

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