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AS Level Chemistry > AS INORGANIC CHEMISTRY > Flashcards

AS INORGANIC CHEMISTRY Flashcards

1
Q

What is the atomic radius?

A

It is the distance between the

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2
Q

What is the atomic radius?

A

It is the distance between the nucleus and the outermost electron

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3
Q

What is the trend of atomic radius across a period?

A

It decreases

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4
Q

why are metal ions smaller than their atoms?

A
  • The Cations have lost their valence electrons
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5
Q

What is the trend in the ions going from Na+ to Si4+

A

They get smaller due to the increasing nuclear charge attracting the electrons in the second principle quantum shell.

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6
Q

Why are anions smaller than their original atoms?

A

because each atom has gained one or more electrons in its third quantum shell.
this increases the repulsion while the nuclear charge stays the same.

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7
Q

Why does Silicon have the highest melting point?

A

Each Si is covalently bonded to the neighbouring Si atoms.

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8
Q

What is the trend of melting points for period 3 metals?

A

They increase

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9
Q

Why does melting point increase for period 3 metals?

A

Because the electrostatic forces between the cations and the sea of free delocalized electrons gets stronger.

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10
Q

What is the bonds between the covalent molecules

A

instantaneous dipole- induced dipole forces

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11
Q

Why does electrical conductivity increase going from Na to Al?

A

Because there is an increase in the valence electrons going into the sea of delocalized electrons.
This means that there are more electrons to move around when they are conducting electricity.

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12
Q

Why is Si not a good electrical conductor?

A

Since it forms a giant molecular structure, there are no free electrons to move around within the structure.
It is therefore classified as a semimetal.

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13
Q

What is the first ionization energy?

A

It is the energy required to remove one mole of electrons from one mole of the element in the gaseous state to form one mole of gaseous electrons.

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14
Q

What is the general trend in the first ionization energy across Period 3?

A

It increases

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15
Q

Why is there a general increase in the first ionization energy across period 3?

A
  1. Nuclear charge increases
  2. The atomic radius decreases
  3. There are stronger attractions between the nucleus and the outer electrons.
  4. It, therefore, gets harder to remove the outer electrons.
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16
Q

Where are dips found in the trend of first ionization energy?

A

Mg - Al

P - S

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17
Q

What is ceramic?

A

It is a rigid material that is made up of an infinite 3D network of sintered metals bonded to carbon, nitrogen and oxygen.

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18
Q

What is sintering?

A

It is when a powdered material is heated below its melting point, which results in the formation of new bonds between the powder grains to form one large mass.

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19
Q

What are some examples of ceramics?

A
  1. Magnesium oxide
  2. Aluminium oxide
  3. Silicon dioxide
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20
Q

Why are ceramics hard and brittle?

A

Hard: They have strong bonds and forces that hold the atoms and ions together in the 3D structure.
Brittle: If the 3D structure is distorted, the ceramic will easily break.

21
Q

Why do ceramics have very high melting points

A

They have strong covalent or ionic bonds in the structure also means that ceramics have high melting points.
A lot of energy is required to break these bonds.

22
Q

Why are Ceramics good insulators?

A

Covalently bonded ceramics have no free electrons

Ionic bonded ceramics have no ions that can freely move around.

23
Q

What are the applications of Magnesium oxide as a Ceramic?

A
  1. Furnace linings due to their high melting points

2. Heating elements - for example, electrical cookers as ceramics are good electrical insulators.

24
Q

What are the applications of Aluminium Oxide as a ceramic?

A
  1. High temperature and voltage electrical insulators due to their high melting and electrical insulating properties.
  2. Replacement Hip joints as they are highly durable
25
Q

What are the uses of silicon dioxide?

A

Furnace linings due to the high melting point of the giant covalent structure.

26
Q

What is Sodium’s Reaction with Oxygen?

A
  • Forms Na2O
  • Heated
  • Vigorous reaction
  • Bright Yellow flame
  • White solid
27
Q

What is Magnesium’s reaction with Oxygen?

A
  • Forms MgO
  • Heated
  • Vigorous reaction
  • Bright white flame
  • White Solid formed
28
Q

What is Aluminium’s reaction with Oxygen?

A
  • Forms Al2O3
  • Powdered Al
  • Fast reaction
  • Bright white flame
  • White Powder
29
Q

What is Silicon’s reaction with Oxygen?

A
  • Forms SiO2
  • Powdered Si is heated Strongly
  • Slow Reaction
  • Bright white Sparkles
  • White Powder
30
Q

What is Phosphorus reaction with Oxygen?

A
  • Forms P4O10
  • Heated
  • Vigorous Reaction
  • Yellow or white flame
  • White clouds
31
Q

What is Sulfur’s reaction with Oxygen?

A
  • Forms SO2
  • Powdered S is heated
  • Gentle reaction
  • Blue flame
  • Toxic fumes are produced
32
Q

What is the reaction of Sodium with Chlorine?

A
  • NaCl
  • Heated
  • Vigorous reaction
33
Q

What is the reaction of Magnesium with Chlorine?

A
  • Forms MgCl2
  • Heated
  • Vigorous reaction
34
Q

What is the reaction of Aluminium with Chlorine?

A
  • Al2Cl6
  • Heated
  • Vigorous reaction
35
Q

What is the reaction of Silicon with Chlorine?

A
  • SiCl4
  • Heated
  • Slow reaction
36
Q

What is the reaction of Phosphorus with Chlorine?

A
  • PCl5 formed

- heated in excess Chlorine

37
Q

How does sodium react with cold water?

A
  • 2Na(s) + H2O -> 2NaOH(aq) + H2(aq)
  • The sodium melts into a ball and moves across the water surface until it disappears.
  • Hydrogen gas is given off
  • The solution formed is strongly alkaline due to the sodium hydroxide.
38
Q

How does Magnesium react with cold water?

A
  • Reacts extremely slowly with cold water
  • Mg(s) + 2H2O -> Mg(OH)2 (aq) + H2(g)
  • The solution formed is only weakly alkaline as Magnesium hydroxide formed is only weakly alkaline
39
Q

How does Magnesium react with steam?

A
  • When Magnesium is heated, it reacts vigorously with steam to make Magnesium oxide and Hydrogen gas
  • Mg(s) + H2O(g) -> MgO(s) + H2(s)
40
Q

Why doesn’t Al2O3 and SiO2 not react with water?

A

They are both insoluble in water

41
Q

What is the reaction of P4O10 with

A
  • P4O10(s) + 6H2O -> 4H3PO4
  • Strongly acidic
  • vigorous reaction
42
Q

What is the reaction of SO2 and SO3 with water

A

SO2(g) + H2O(l) ->H2SO3 (aq)

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

43
Q

What is the reaction of Al2O3 with H2SO4?

A

Al2O3(s) + H2SO4(aq) -> Al2(SO4)3(aq) + 3H2(l)

Reacts with acids to form a salt an water.

44
Q

What is the reaction of Al2O3 with hot concentrated alkali?

A

Al2O3(s) + 2NaOH(aq) -> 3H2O(l) + 2NaAl(OH)4(aq)

45
Q

what is the reaction of SiO2 with hot concentrated alkali

A

SiO2 + 2NaOH -> Na2SiO3(aq) + H2O(l)

Reacts with an alkali to form a salt and water.

46
Q

What is the reaction of SO2 and SO3 with NaOH

A

SO2 + 2Na(OH)(aq) -> Na2SO3(aq) + H2O (l)

SO3 + 2NaOH(aq) -> Na2SO4 (aq) +H2O (l)

47
Q

How does the chlorides of Sodium and Magnesium react with water?

A
  • They are white solids that dissolve to produce colorless solutions.
48
Q

How does the chlorides of Aluminum react with water?

A
  • The Dimers are broken down to Al3+ and Cl- ions, which enter the solution
  • The highly charged Al3+ ion become hydrated and causes a water molecule that is bonded to the Al3+ to lose an H+ which turns the solution acidic.
  • The H+ and the Cl- react to produce HCl which leaves as white fumes.
  • [Al(H2O)6]3+(aq) -> Al(H2O)5OH + H+(aq)

AS Level Chemistry (11 decks)

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