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Inorganic Chemistry and the Periodic Table Flashcards

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1
Q

Describe in basic terms, the appearance of Group 2 metals

A
  • bright silvery solids
  • when exposed to air, they combine with oxygen to form oxides as surface layers, which makes them appear dull
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2
Q

Trend in ionisation energies in group two

A

Ionisation energy decreases down group two

Although nuclear charge increases, one new quantum shell is added each time, which is at a higher energy level and also increases repulsion (shielding)

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3
Q

What type of ions are made in reactions with group 2 elements and whats the general trend in reactivity

A

M2+ ions

a general increase

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4
Q

What happens to group two elements when they are burned in air And the general equations for these reactants

A

For a bright flame usually

These reactions become more vigorous down a group

They usually form solids, which are oxides

2M + O2 -> 2MO

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5
Q

What two ions are formed in oxides of group 2

A

M+2

O-2

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6
Q

What has to happen to the group 2 elements to combine with chlorine gas?

What happens to reactiviy as we go down the group in this reaction

And what is the general equation for this reaction

A

Heated in the gas

More vigorous down the group

M+Cl2 -> MCl2

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7
Q

How do group two metal react with water

What is the trend with reactivity down the group

What is the general equation for these reactions

A

As we move down the group, they react with increasing vigour, which can be seen by increase in effervescence and hydrogen bubbles

M + 2H2O -> M(OH)2 (aq) + H2 (g)

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8
Q

What are the products of group 2 metals reacting with water

A

M2+

OH-

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9
Q

What is the difference between these two group 2 reactions with water and why

Ca(s) + 2H2O(l) -> Ca(OH)2 (s) + H2 (g)

<span>Ba</span>(s) + 2H2O(l) -> Ba(OH)2 (aq) + H2 (g)

A

difference in state symbols for the hydroxides

Barium hydroxides is soluable in water

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10
Q

What happens to a group 2 (magnesium) when heated with steam

Write an equation for this reaction

And describe an experiment for it

A

Rapidly forms M (magnesium) oxides and hydrogen gas, in a vigorus reaction

Mg(s) + H2O(g) -> MgO(s) + H2(g)

Hydrogen is formed is burned as it leaves the tube, as it is highly flammable

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11
Q

What is the general trend of reactivity moving down the group

A

increasing reactivity

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12
Q

Group 2 oxides are classed as what and why

In which reaction does this occur and write a general equation

A

Basic oxides

Because they can react with water to form alkalis

These reaction occur when oxides are added to water

MO(s) +H2O(l) -> M(OH)2(aq)

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13
Q

What amkes oxides with water alkaline

A

The formation of hydroxide ions

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14
Q

The pH value of the alkaline solution formed with oxides in water depneds on what

A

Relative amounts of oxides and water

different solubilities of the hydroxides

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15
Q

How does the test for Carbon dioxide link to reactions with group 2 oxides and water

And what ias the equation for this reaction

A

limewater is use to test for CO2

As a white precipiate forms in the presence

Limewater is a saturated aq solution of calcium hydroxide

Carbon dioxide reacts forming calcium carbonate, whcih is insoluable in water

CO2 + Ca(OH)2 -> CaCO3 +H2O

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16
Q

As carbon dioxide is bubbled through limewater, the amount of precipate

A

increases

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17
Q

What is milk of magnesia

A

indigestion remedy, acts as an antacid

saturated soluation of magnesium hydroxide mixed with extra solids of magnesium hydroxide

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18
Q

How does Milk of magnesia work

and the name the equation for the reaction

A

neutralises some of the hydrochloric acid

Mg(OH)2 + 2HCl -> MgCl2 + 2H2O

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19
Q

All of group 2 oxides and hydroxides (alkalis) react with acids to form

This type of reaction is

What would you observe in these reactions

A

salts and water

Neutralisation reaction

a white solid reacts to form a colourless solution

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20
Q

Reactions of oxides and hydroixdes with acids are endothermic or exothermic?

A

exothermic

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21
Q

What is the use of calcium hydroxide and agricuture

And write an equation for this reaction where HNO3 (nitric acid) is soil

A

farmers have used lime to control acidity so that a great yeild of crop can be obtained

Lime is mostly Calcium Hydroxide, and neutralises excess acidity in the soil

Ca(OH)2 + 2HNO3 -> Ca(NO3)2 + 2H2O

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22
Q

True or False, all group 2 nitrates and Chlordies are soluble

A

True

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23
Q

Does the solubility of Group 2 nitrates increase or decrease down a group

A

Increase

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24
Q

How would you test for sulfate ions in aq solution

A

adding a solution containing barium ions

(usually barium chloride/nitrate)

Any sulfate ion in the solution will react with the barium ions to form a white precipitate of barium sulfate

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25
Q

When testing for sulfate ions in a aq solution you use, barium nitrate/chloride and it forms barium sulfate

Write an equation for this

A

Ba+2 (aq) + SO42- (aq) -> BaSO4 (S)

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26
Q

What has to be present to stop other anions, (like carbonate ions) from forming a white precipiate with the barium ions, when you’re wanting to test for sulfates

Therefore what can be done to stop this

A

H+ ions

Dilute nitric acid or dilute hydrochloric acid

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27
Q

What is the purpose of barium sulfates in hospitals

A

Barium meals

Not posionous because it’s insolubale

It helps soft tissue to show up better on an X-rays, because of the dense white soilds

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28
Q

What is thermal stability

A

is a measure of the extent to which a compound decomposes when heated

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29
Q

If something doesn’t decompose at all, it is

A

Very thermally stable

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30
Q

If something completely decomposes as much as possible, it is

A

Not thermally stable

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31
Q

What is responsible for the melting temperture of a compound

A

ionic bonding

And the strength of these bonds will determine how easily the substance melts

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32
Q

How thermally stable are ionic compounds and why

A

Very

Ions change from being regularly arranged in a gaint lattice to moving freely in a liquid, however no decomposition occurs

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33
Q

What are the 3 differences between group 2 nitrates/carbonates and group 1 chlorides

A

1) Charge on group 2 ions (M2+)
2) Size (ionic radius) is smaller in group 2 cation (proton number)
3) Nitrates (NO3-) + Carbonates (CO32-) anions more complex than halogen ions (Cl-)

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34
Q

What do the 3 difference between group 2 Nitrates/Carbonates and Group 1 halogens (chlorides), to the thermal stability

A

When group 2 nitrates/carbonates are heated, they do not melt, they decompose, meaning a decreased thermal stability

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35
Q

Why does a group 2 metal, which is bonded to a larger , more complex nitrate ion, mean they can decompose

A

Nitrate ions can change into smaller, more stable nitrite ions (NO2-)or oxide ino (O2-) by decomposing and releasing oxygen gas and/or nitrogen dioxide gas

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36
Q

Why does a group 2 metal, which is bonded to a larger , more complex Carbonate ion, means they can decompose

A

they can change into smaller, more stable oxide ions (O2-) by decomposing and releasing CO2

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37
Q

Why does a group 2 metal, when bonded to a nitrate/carbonate ion, meaning it more likely to decompose, in terms of size and charge

A

Stabilities of the nitrate/carbonate anions are influenced by the charge and size of the cation present

The smaller, more highly charged cations (+) affect anions (-) more, due to greater charge density

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38
Q

What happens to the white soilds or group 1 and 2 nitrates when heated

A

When they are heated, they all decompose to nitrates/oxides, and give off nitrogen dioixde (brown fumes) and/or oxygen

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39
Q

When nitrates of group 1 and 2 are decomposed and they contain water of crystallisation, what will observed

A

Steam

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40
Q

Describe the lesser decompostion of a group 1/2 nitrate

A

No brown fumes

Metal Nitrate -> Metal nitrite + Oxygen

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41
Q

Describe the greater decompostion of a group 1/2 nitrate

A

Brown fumes are observed

Metal nitrate -> metal oxide + nitrogen dioixe + oxygen

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42
Q

What is the general trend in group 1 for lesser and greater decompostion

A

Lithium : brown fumes

Sodium - Caesium : now brown fumes

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43
Q

What is the general trend for lesser or greater decompostion of group 2 nitrates

A

Beryllium - Barium = brown fumes

Therefore greater decomposition

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44
Q

How does charge and size link to greater and lesser decompositon of group 1/2 nitrates

A

Cation has a 2+ charge, has greater decompostion

Cation has 1+ charge and a smallest ionic radius (Lithium) decomposes

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45
Q

Write an equation for the greater decompostion of Lithium

(group 1)

A

4LiNO3 -> 2Li2O + 4NO2 + O2

46
Q

What is thermal stability of group 1/2 carbonates

A

Are white solids and when heated they do not decompose, or decompose to oxides + give off CO2

Therefore they are more thermally stable than metal nitrates

No visible obervations can be made

47
Q

What is the general trend of Thermal stability for group 1 carbonates

A

Lithium Carbonate : decompostion

Sodium - Caesium : no decompostion

48
Q

What is the general trend for thermal stability for Group 2 Carbonates

A

Beryllium - Barium : decompostion

49
Q

Write an equation for the decompostion of Lithium carbonate

A

Li2CO3 -> Li2O + CO2

50
Q

What has size and charge got to do with Decompostion of group 1/2 carbonates

A

Cation with a 2+ charge , decomposes

The smallest 1+ cation (Lithium Carbonate)

51
Q

How would you carry out a flame test

A
  • Light an bunsen burner
  • Using a dropper, add a few drops of Concentrated HCL to metal and mix so metal compound begins to dissolve.
  • We use HCl because it coverts metals into chlorides, which are more volitile than salts
  • Dip a clean metal wire (platinum/nichrome) or silica rod into mixture to obtain sample
  • Hold end of rod in flame and observe colour change
52
Q

What are the two main problems with the flame test

A
  • Many compounds contain small amount of sodium compouds as impurities, which causes a yellow/orange flame
  • Describe colours is subjects and value based judgement
53
Q

What colour does lithium show in the flame

A

Red

54
Q

What colour does Sodium show in the flame

A

Yellow/orange

55
Q

What colour does Potassium show in the flame

A

lilac

56
Q

What colour does Rubidium show in the flame

A

red/purple

57
Q

What colour does Caesium show in the flame

A

blue/violet

58
Q

What colour does Beryllium show in the flame

A

no colour

59
Q

What colour does Magnesium show in the flame

A

no colour

60
Q

What colour does Calcium show in the flame

A

(brick) red

61
Q

What colour does Strontium show in the flame

A

(crimson) red

62
Q

What colour does Barium show in the flame

A

(apple) red

63
Q

What causes the colour in the flame test

A

Electron transition

Electrons occupy orbitals at specific energy levels

Electrons can absorb energy and move to higher energy levels

This is the movement from ground state to excited state

This excited state occurs during the flame test

This movemment is immediately followed by an electron moving to ground state, which releases energy, which if corresponding to radiation is the visible light spectrum , a colour appears

64
Q

The test for the ammonium ion

And write the equation for this

A

An ammonium ion doesnt give a colour in the flame test

Therefore, we must add sodium hydroxide solution and warm the mixture, which releases amonium gas (alkaline) , which can be identified by using damp litmus paper, which turns blue to red

NH4+ + OH- -> NH3 + H2O

65
Q

What does the name for group 7 mean in Greek

A

Halogen

Hal = salt

Gen = producer

66
Q

What is the states of group 7 elements at room temperture

A

Fluorine - Yellow Gas

Chlorine - Green Gas

Bromine - Volatile brown liquid

Iodine - Volatile grey solid

67
Q

Halogens exits as what types of molecules

A

Diatomic molecules

68
Q

Halogens Melting and Boiling points depend on what

A

Strength of the molecular forces of attraction between molecules

London Forces

69
Q

How does an intaneous dipole occur in diatomic moleucles in the halogens

A
  • Pair of electrons forming covelent bonds, where electrons are equally shared between atoms
  • Therefore they are non-polar
  • However postive charge in the nuclei is fixed, however electron density flutuates
  • This can lead to the centres of postive and negative charges not coinciding
70
Q

An instaneous dipole can cause, what in another halogen atoms

A

induced dipoles

Halogens are non-polar, so would have no interacts with another

if an instaneous dipole occurs, it cause a induced dipole to happen

71
Q

Intermolecular forces in dipoles depend on what

A

Size - an increase in size, will increase the number of electrons and size of electron cloud

So force strengh increase down a group, which explains the increase in M.P. and B.P.

72
Q

Describe the method for the sublimation of iodine

Write an equation for this change

A

Warm gently over a bunsen burner

It should vapourise, producing a purple vapour

It should then deposit forming crystals, on the cool finger in the tube containing ice

I2 (s) -> I2 (g)

73
Q

What is electronegativity and how does it relate to the haolgens

A

is the ability of an atom to attract the pair of electrons in a covelent bond

Electronegativity of group 7 is the highest in the periodic table

Fluorine has the highest electronegativity of all elements

74
Q

What does electronegativity depend on

A
  • Nuclear Charge
  • distance between nucleus and bonding pair of electrons
  • sheilding effect of electrons in inner energy levels
75
Q

How does electronegativity relate to group 7

A

Fluorine is an extremely reactive elements, the most

Reactivity decrease down the group with electronegativity

This is because of its great charge density

76
Q

How do you convert from degree celeius to kelvin

A

+/- 273

77
Q

In redox reactions, halogens act as what

A

Halogen act as oxidising agents (reduced) as so gain electrons

78
Q

In a displacement reaction, why would one halogen replace another halogen

A

Due to one halogen being more reactive than another

Electronegatitvity decreases down a group

79
Q

What would be an experiment for demonstrating the displacement in halogens

A
  • This occurs in an aqueous solution, however the interpreting colour change can be difficult so by adding a solvent like cyclohexane, which halogens are more soluble in water.
  • The halogen dissolves in the organic upper layer, and colour change can be see more easily
  • The colour chage will demonstrate the displacement
80
Q

What is the colour of chlorine, bromine and iodine in an aqueous solution

And what is the colour of them when cyclohexane is added

A

Pale green, yellow, and brown

pale green, red, brown

81
Q

What type of reaction happens when you mix chlorine and water

What are the products of the reaction

Cl₂ + H₂O

Is there any visible colour change

A

Disproportionation

HCl

Chloric (i) acid = HOCl

No colour change

82
Q

The product of mixing chlorine and water is chlorine water

What purpose in real life can be used with this product

A

Chlorine disinfects water, kills water-borne diseases like cholera

83
Q

What type of reaction happens when you mix chlorine with a cold alkali (NaOH)

What are the products for this reaction (Cl₂ + 2NaOH)

Which product in this reaction has a specific use in society

A

Disproportionation

NaCl

NaClO = Sodium chlorate (l)

H₂

Sodium chlorate (l) is a disinfectant, known for bleaching action (the active ingredient in household bleach)

84
Q

What type of reaction happens when you mix chlorine and a hot alkali

What are the products (3Cl₂ + 6NaHO)

Which product has a use in society

A

Disproportionation

5NaCl

NaClO₃

3H₂O

NaClO₃ (sodium chlorate (v)) used in bleaching and weed killing

85
Q

Balance the equation:

Cl₂ + NaHO → NaCl + NaClO₃ + H₂O

A

3Cl₂ + 6NaHO → 5NaCl + NaClO₃ + 3H₂O

86
Q

Does the oxidising power of diatomic halogens increase or decrease, why?

A

The oxidising power of diatomic halogens increase up the group because the electronegativity (moving to an ion from a diatomic molecule)

87
Q

Does the reducing power of halides increase or decrease down a group, why

A

The reducing power of halides decreases down the group (moving to diatomic molecule from an ion). Halide becomes oxidised. This is because it is easier to lose electrons, ionisation energy

2X⁻ → X₂ + 2e⁻

88
Q

Concentrate sulphuric acids ….

A

contains few ions (weak), position of equilibrium lies to the right

89
Q

Write equations for the partial ionisation of Sulphuric acid into SO₄²⁻

A

H₂SO₄ ⇌ H⁺ + HSO₄

HSO₄⁻ ⇌ H⁺ + SO₄²⁻

90
Q

Sulphuric acids, especially when concentrated is oxidised or reduced

A

is reduced (oxidising agent)

91
Q

When an ionic compound, with chloride, bromide, and iodide, reacts with sulphuric acid, which compound has the biggest reducing power

A

Metal Chloride only acids as an acids

Metal Bromide, the bromide ions have greater reducing power so 2H₂0 + SO₂ is formed

Metal Iodide, much greater reducing power, cause sulphuric acid to be reduced, so either

2H₂0 + SO₂,

4H₂0 + S

4H₂0 + H₂S is formed

92
Q

When metal chloride reacts with sulphuric acid, what are the observations and products

A

misty fumes

HCl

93
Q

When metal bromide reacts with sulphuric acid, what are the observations and products

A

misty fumes = HBr

Brown fumes = Br₂

Colourless gas with chocking smell= SO₂

94
Q

When metal iodide reacts with sulphuric acid, what are the possible observations and products

A

Misty fume = HI

Purple fumes/Black solid = I₂

Colourless gas with chocking smell = SO₂

Yellow solid = S

Colourless gas with rotten egg smell= H₂S

95
Q

What are the possible products when sulphuric acid is reduced

A

sulphur dioxide

sulphur

hydrogen sulphide

96
Q

Write a half equation for sulphuric acid being reduced to sulfur dioxide

which halide can do this

A

H₂SO₄ + 2H⁺ + 2e⁻ → 2H₂0 + SO₂

bromide and chloride

colourless gas with chocking smell

97
Q

Write a half equation for the reduction of sulphuric acid to sulfur

which halides can do this

A

H₂SO₄ + 6H⁺ + 6e⁻ → 4H₂0 + S

Chlorine

Yellow solid

98
Q

Write a half equation for the reduction of sulphuric acid to hydrogen sulfide

What halide can do this

A

H₂SO₄ + 8H⁺ + 8e⁻ → 4H₂0 + H₂S

Chloride

Colourless gas with rotten egg smell

99
Q

When testing for Halide ions in a solution, what does this test depend on

A

on very low solubility of silver halides in water and their different solubilities in ammonia

100
Q

Describe the test for Halides ions in a solution

A
  1. Dilute Nitric/Hydrochloric acid must be added.
  2. To avoid other white precipitates (anions) forming, there must be H+ ions present
  3. Reagent is silver nitrate solution (AgNO₃)
  4. The precipitate obtained is then added to ammonia solution (diluted and concentrate) due to precipitates having a similar colour
101
Q

When Silver Nitrate is added to a halide in water, a precipitate is formed

Write an ionic equation for this

A

Ag⁺ + X⁻ → AgX

102
Q

What colour precipitate is formed when silver nitrate is added to chloride ions

Is the precipitated soluble in dilute or concentrated aqueous ammonia

A

White precipitate is formed

Soluble in dilute aqueous ammonia

Soluble in concentrated aqueous ammonia

103
Q

What colour precipitate formed when Bromide ions are added to silver nitrate

Is the precipitated soluble in either dilute or concentrated aqueous ammonia

A

Cream precipitate

Insoluble in dilute aqueous ammonia

Soluble in concentrated aqueous ammonia

104
Q

What colour precipitate forms when iodide ions are added to silver nitrate

Is this precipitate soluble in dilute or concentrated ammonia

A

Yellow precipitate

Insoluble in dilute aqueous ammonia

Insoluble in concentrated aqueous ammonia

105
Q

Hydrogen halides exits as

A

Colourless gases

Polar

Diatomic molecules

106
Q

Do hydrogen halides react with water

A

Readily react forming acidic solutions, all of which are colourless

107
Q

When hydrogen fluoride reacts with water

what products are formed

write an equation for this

A

Hydrofluoric acid

HF + H₂O ⇌ H₃O⁺ + F⁻

108
Q

When hydrogen chloride reacts with water

What are the products formed

Write an half equation for this

A

Hydrochloric acid

HCl + H₂O ⇌ H₃O⁺ + Cl⁻

109
Q

When hydrogen bromide reacts with water

What is the product formed

Write a half equation for this

A

Hydrobromic acid

HBr + H₂O ⇌ H₃O⁺ + Br⁻

110
Q

When hydrogen iodide reacts with water

What are the products formed

Write a half equation for this

A

Hydriodic acid

HI + H₂O ⇌ H₃O⁺ + I⁻

111
Q

Hydrogen Halides react with ammonia gas to form

A

salts, which are all white ionic solids

112
Q

Describe an experiment reacting hydrogen halides with ammonia gas

A
  1. Ammonia and hydrogen chloride are given out by separate pieces of cotton wool, on end two ends of an enclosed tube
  2. The cotton will is socked in concentrated aqueous NH₃ and HCl
  3. Colourless gases move through the tube, till they meet forming ammonium chloride
  4. The ammonia gas will move more quickly than the hydrogen chloride as it is lighter, and therefore more further through the tube

Chemistry (12 decks)

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