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Chemistry > Transition metals, Isomerism, Period 3 chlorides and oxides > Flashcards

Transition metals, Isomerism, Period 3 chlorides and oxides Flashcards

1
Q

Whats the difference between D-block elements and transition metals

A

All elements between period 3 to 12 are in the D-block however only elements that have partially filled d-subshells are transition metals

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2
Q

general electronic configuration of transition metals and outliers

A
  • [Ar]3dn4s2
  • Chromium = [Ar]3d5 4s1 - more energetically favourable
  • Copper = [Ar]3d10 4s1
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3
Q

Trend of ions formed by transition metals

A
  • +3 common up to manganese
  • manganese up to +7 and chromium up to +6
  • +2 common after manganese
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4
Q

Whats a ligand

A
  • either neutral or anion
  • lewis base
  • donate a pair of electrons through a dative covalent bond to metal ion
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5
Q

Whats a coordination number

A

The number of ligands surrounding a molecule in a complex

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6
Q

Shapes of complexes with different coordination numbers

A

2 - linear
4 - tetrahedral (common)
4 - square planar if the molecule has 8 electrons in the d subshell (rare)
6 - octahedral

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7
Q

Whats an enantiomer

A
  • A molecule that has two non-superimposable mirror images
  • Polarised light bounces off them in opposite directions
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8
Q

What is Kstab

A
  • Stability constant
  • ∑[products]/∑[reactants]
  • H2O isnt included as its in excess
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9
Q

Whats a chiral centre

A

A carbon joined by 4 unique atoms/groups

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10
Q

Reactions of period 3 elements

A
  • They react with oxygen in a combustion reaction where oxygen is the reducing agent
  • They react with chlorine which also acts as an oxidising agent
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11
Q

Trend of oxidation number and apparence of period 3 chlorides

A
  • General increase as you go across the period from +1 to +4
  • P can be +3 or +5
  • S can be +1,+2 or +4
  • White solid up to Al
  • All after are liquid except PCl5 which is white solid
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12
Q

Trend of melting point of period 3 chlorides

A
  • General decrease, P goes up
  • Na and Mg show ionic bonding (giant ionic lattices) whereas the rest is covalent (simple molecular)
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13
Q

Properties of giant ionic lattices

A
  • High melting point
  • Highly soluble in water
  • Electrical insulators when solid
  • Electrical conductors when molten or dissolved
  • Breaking the lattice is exothermic
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14
Q

Hydrolysis of period 3 chlorides

A
  • Ionic lattices dissolve in water
  • Silicon IV - Water attacks the Si and releases 2HCl and SiO2
  • Phosphorus - Hydrolysed to release HCl
  • Al - Al3+ formed and a hydrogen can be released to form 2+
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15
Q

Trends of oxidation numbers and apperance of period 3 oxides

A
  • +1 to +4 for the first 4
  • P - +3 and +5
  • S - +4 and +6
  • Cl - +1 and +7
  • White solid up to P
  • S is a colourless gas
  • ClO+1 is a yellow gas, Cl2O7 is a colourless liquid
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16
Q

Trend of melting points of period 3 oxides

A
  • Increase from Na to Mg then steady decrease
  • Na2O, MgO and Al2O3 are ionic so they have high MP
  • Mg2+ has a much higher charge density so has stronger ionic bonding
  • SiO is giant covalent
  • The rest are simple covalent
16
Q

Trend of melting points of period 3 oxides

A
  • Increase from Na to Mg then steady decrease
  • Na2O, MgO and Al2O3 are ionic so they have high MP
  • Mg2+ has a much higher charge density so has stronger ionic bonding
  • SiO is giant covalent
  • The rest are simple covalent
17
Q

Characteristics of ionic oxides

A
  • They can accept protons making their solutions alkaline
  • Al2O3 can act as a base or acid - its amphoteric
18
Q

Properties of SiO2

A
  • Each Si bonded to 4 oxygens
  • High melting point
  • Doesn’t dissolve in water or conduct electric
19
Q

Properties of simple covalent oxides

A
  • P4O10 has a higher MP than P4O6 as it is larger and has more room for van der waals forces
  • SO3 has a higher MP than SO2 as its planar and can stack, both polar
  • Cl2O and Cl2O7 are both polar but the latter has a higher MP as its bigger
  • They all dissolve in water to produce an acid
20
Q

What makes transition metals have colour

A
  • Their incomplete d-subshell as electrons get excited between d-orbitals with higher energy that can absorb light
  • Zinc is colouless as it has a full subshell
  • They absorb certain wavelengths of light and whats reflected is seen
  • The colour seen is the opposite of whats seen
21
Q

What can change the colour of the solution

A
  • Changing the ligand changes the size of the gap between d-orbitals
  • Different oxidation states
22
Q

Whats a catalyst

A

A substance that regenerates after use and provides an alternative pathway that has a lower activation energy

23
Q

Difference between hetero and homogeneous

A

Hetero - The catalyst is not in the same state as the reactants

Homo - The catalyst is in the same state as the reactants

Chemistry (4 decks)

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