Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry > Inorganic Chemistry and the Periodic Table > Flashcards

Inorganic Chemistry and the Periodic Table Flashcards

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
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What two ions are formed in oxides of group 2

A

M+2

O-2

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What are the products of group 2 metals reacting with water

A

M2+

OH-

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What is the general trend of reactivity moving down the group

A

increasing reactivity

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What amkes oxides with water alkaline

A

The formation of hydroxide ions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

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

A

increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

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

A

exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

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

A

True

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

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

A

Increase

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
When testing for sulfate ions in a aq solution you use, barium nitrate/chloride and it forms barium sulfate Write an equation for this
Ba+2 (aq) + SO42- (aq) -\> BaSO4 (S)
26
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
H+ ions Dilute nitric acid or dilute hydrochloric acid
27
What is the purpose of barium sulfates in hospitals
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
28
What is thermal stability
is a measure of the extent to which a compound decomposes when heated
29
If something doesn't decompose at all, it is
Very thermally stable
30
If something completely decomposes as much as possible, it is
Not thermally stable
31
What is responsible for the melting temperture of a compound
ionic bonding And the strength of these bonds will determine how easily the substance melts
32
How thermally stable are ionic compounds and why
Very Ions change from being regularly arranged in a gaint lattice to moving freely in a liquid, however no decomposition occurs
33
What are the 3 differences between group 2 nitrates/carbonates and group 1 chlorides
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-)
34
What do the 3 difference between group 2 Nitrates/Carbonates and Group 1 halogens (chlorides), to the thermal stability
When group 2 nitrates/carbonates are heated, they do not melt, they decompose, meaning a decreased thermal stability
35
Why does a group 2 metal, which is bonded to a larger , more complex nitrate ion, mean they can decompose
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
36
Why does a group 2 metal, which is bonded to a larger , more complex Carbonate ion, means they can decompose
they can change into smaller, more stable oxide ions (O2-) by decomposing and releasing CO2
37
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
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
38
What happens to the white soilds or group 1 and 2 nitrates when heated
When they are heated, they all decompose to nitrates/oxides, and give off nitrogen dioixde (brown fumes) and/or oxygen
39
When nitrates of group 1 and 2 are decomposed and they contain water of crystallisation, what will observed
Steam
40
Describe the lesser decompostion of a group 1/2 nitrate
No brown fumes Metal Nitrate -\> Metal nitrite + Oxygen
41
Describe the greater decompostion of a group 1/2 nitrate
Brown fumes are observed Metal nitrate -\> metal oxide + nitrogen dioixe + oxygen
42
What is the general trend in group 1 for lesser and greater decompostion
Lithium : brown fumes Sodium - Caesium : now brown fumes
43
What is the general trend for lesser or greater decompostion of group 2 nitrates
Beryllium - Barium = brown fumes Therefore greater decomposition
44
How does charge and size link to greater and lesser decompositon of group 1/2 nitrates
Cation has a 2+ charge, has greater decompostion Cation has 1+ charge and a smallest ionic radius (Lithium) decomposes
45
Write an equation for the greater decompostion of Lithium (group 1)
4LiNO3 -\> 2Li2O + 4NO2 + O2
46
What is thermal stability of group 1/2 carbonates
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
What is the general trend of Thermal stability for group 1 carbonates
Lithium Carbonate : decompostion Sodium - Caesium : no decompostion
48
What is the general trend for thermal stability for Group 2 Carbonates
Beryllium - Barium : decompostion
49
Write an equation for the decompostion of Lithium carbonate
Li2CO3 -\> Li2O + CO2
50
What has size and charge got to do with Decompostion of group 1/2 carbonates
Cation with a 2+ charge , decomposes The smallest 1+ cation (Lithium Carbonate)
51
How would you carry out a flame test
- 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
What are the two main problems with the flame test
- 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
What colour does lithium show in the flame
Red
54
What colour does Sodium show in the flame
Yellow/orange
55
What colour does Potassium show in the flame
lilac
56
What colour does Rubidium show in the flame
red/purple
57
What colour does Caesium show in the flame
blue/violet
58
What colour does Beryllium show in the flame
no colour
59
What colour does Magnesium show in the flame
no colour
60
What colour does Calcium show in the flame
(brick) red
61
What colour does Strontium show in the flame
(crimson) red
62
What colour does Barium show in the flame
(apple) red
63
What causes the colour in the flame test
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
The test for the ammonium ion And write the equation for this
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
What does the name for group 7 mean in Greek
Halogen Hal = salt Gen = producer
66
What is the states of group 7 elements at room temperture
Fluorine - Yellow Gas Chlorine - Green Gas Bromine - Volatile brown liquid Iodine - Volatile grey solid
67
Halogens exits as what types of molecules
Diatomic molecules
68
Halogens Melting and Boiling points depend on what
Strength of the molecular forces of attraction between molecules London Forces
69
How does an intaneous dipole occur in diatomic moleucles in the halogens
* 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
An instaneous dipole can cause, what in another halogen atoms
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
Intermolecular forces in dipoles depend on what
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
Describe the method for the sublimation of iodine Write an equation for this change
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
What is electronegativity and how does it relate to the haolgens
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
What does electronegativity depend on
* Nuclear Charge * distance between nucleus and bonding pair of electrons * sheilding effect of electrons in inner energy levels
75
How does electronegativity relate to group 7
Fluorine is an extremely reactive elements, the most Reactivity decrease down the group with electronegativity This is because of its great charge density
76
How do you convert from degree celeius to kelvin
+/- 273
77
In redox reactions, halogens act as what
Halogen act as oxidising agents (reduced) as so gain electrons
78
In a displacement reaction, why would one halogen replace another halogen
Due to one halogen being more reactive than another Electronegatitvity decreases down a group
79
What would be an experiment for demonstrating the displacement in halogens
* 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
What is the colour of chlorine, bromine and iodine in an aqueous solution And what is the colour of them when cyclohexane is added
Pale green, yellow, and brown pale green, red, brown
81
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
Disproportionation HCl Chloric (i) acid = HOCl No colour change
82
The product of mixing chlorine and water is chlorine water What purpose in real life can be used with this product
Chlorine disinfects water, kills water-borne diseases like cholera
83
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
Disproportionation NaCl NaClO = Sodium chlorate (l) H₂ Sodium chlorate (l) is a disinfectant, known for bleaching action (the active ingredient in household bleach)
84
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
Disproportionation 5NaCl NaClO₃ 3H₂O NaClO₃ (sodium chlorate (v)) used in bleaching and weed killing
85
Balance the equation: Cl₂ + NaHO → NaCl + NaClO₃ + H₂O
**3**Cl₂ + **6**NaHO → **5**NaCl + NaClO₃ + **3**H₂O
86
Does the oxidising power of diatomic halogens increase or decrease, why?
The oxidising power of diatomic halogens increase up the group because the electronegativity (moving to an ion from a diatomic molecule)
87
Does the reducing power of halides increase or decrease down a group, why
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
Concentrate sulphuric acids ....
contains few ions (weak), position of equilibrium lies to the right
89
Write equations for the partial ionisation of Sulphuric acid into SO₄²⁻
H₂SO₄ ⇌ H⁺ + HSO₄ HSO₄⁻ ⇌ H⁺ + SO₄²⁻
90
Sulphuric acids, especially when concentrated is oxidised or reduced
is reduced (oxidising agent)
91
When an ionic compound, with chloride, bromide, and iodide, reacts with sulphuric acid, which compound has the biggest reducing power
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
When metal chloride reacts with sulphuric acid, what are the observations and products
misty fumes HCl
93
When metal bromide reacts with sulphuric acid, what are the observations and products
misty fumes = HBr Brown fumes = Br₂ Colourless gas with chocking smell= SO₂
94
When metal iodide reacts with sulphuric acid, what are the possible observations and products
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
What are the possible products when sulphuric acid is reduced
sulphur dioxide sulphur hydrogen sulphide
96
Write a half equation for sulphuric acid being reduced to sulfur dioxide which halide can do this
H₂SO₄ + 2H⁺ + 2e⁻ → 2H₂0 + SO₂ bromide and chloride colourless gas with chocking smell
97
Write a half equation for the reduction of sulphuric acid to sulfur which halides can do this
H₂SO₄ + 6H⁺ + 6e⁻ → 4H₂0 + S Chlorine Yellow solid
98
Write a half equation for the reduction of sulphuric acid to hydrogen sulfide What halide can do this
H₂SO₄ + 8H⁺ + 8e⁻ → 4H₂0 + H₂S Chloride Colourless gas with rotten egg smell
99
When testing for Halide ions in a solution, what does this test depend on
on very low solubility of silver halides in water and their different solubilities in ammonia
100
Describe the test for Halides ions in a solution
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
When Silver Nitrate is added to a halide in water, a precipitate is formed Write an ionic equation for this
Ag⁺ + X⁻ → AgX
102
What colour precipitate is formed when silver nitrate is added to chloride ions Is the precipitated soluble in dilute or concentrated aqueous ammonia
White precipitate is formed Soluble in dilute aqueous ammonia Soluble in concentrated aqueous ammonia
103
What colour precipitate formed when Bromide ions are added to silver nitrate Is the precipitated soluble in either dilute or concentrated aqueous ammonia
Cream precipitate Insoluble in dilute aqueous ammonia Soluble in concentrated aqueous ammonia
104
What colour precipitate forms when iodide ions are added to silver nitrate Is this precipitate soluble in dilute or concentrated ammonia
Yellow precipitate Insoluble in dilute aqueous ammonia Insoluble in concentrated aqueous ammonia
105
Hydrogen halides exits as
Colourless gases Polar Diatomic molecules
106
Do hydrogen halides react with water
Readily react forming acidic solutions, all of which are colourless
107
When hydrogen fluoride reacts with water what products are formed write an equation for this
Hydrofluoric acid HF + H₂O ⇌ H₃O⁺ + F⁻
108
When hydrogen chloride reacts with water What are the products formed Write an half equation for this
Hydrochloric acid HCl + H₂O ⇌ H₃O⁺ + Cl⁻
109
When hydrogen bromide reacts with water What is the product formed Write a half equation for this
Hydrobromic acid HBr + H₂O ⇌ H₃O⁺ + Br⁻
110
When hydrogen iodide reacts with water What are the products formed Write a half equation for this
Hydriodic acid HI + H₂O ⇌ H₃O⁺ + I⁻
111
Hydrogen Halides react with ammonia gas to form
salts, which are all white ionic solids
112
Describe an experiment reacting hydrogen halides with ammonia gas
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)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions