A-Level Chemistry (Edexcel) > Topic 4: Inorganic Chemistry and the Periodic Table > Flashcards

Topic 4: Inorganic Chemistry and the Periodic Table Flashcards

Predict chemical properties and reactions using group trends and periodicity. (90 cards)

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1
Q

What collective name is given to the elements in Group 2 of the Periodic Table?

A

Alkaline earth metals

Examples include Mg, Ca, Sr and Ba.

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2
Q

What happens to atomic radius as you move down Group 2 from Mg to Ba?

A

Increases

Additional electron shells increase the size of the atoms.

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3
Q

Fill in the blank:

The first ionisation energy of Group 2 elements generally _______ down the group.

A

decreases

Increased distance and shielding reduce attraction to the outer electron.

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4
Q

True or False:

The reactivity of Group 2 metals increases down the group.

A

True

Lower ionisation energies make electron loss easier.

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5
Q

What type of bonding holds atoms together in Group 2 metals?

A

Metallic bonding

Positive ions are surrounded by delocalised electrons in a lattice.

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6
Q

True or False:

Magnesium reacts rapidly with cold water.

A

False

Magnesium reacts very slowly with cold water but reacts faster with steam.

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7
Q

Fill in the blank:

Magnesium reacts with steam to produce magnesium _______ and hydrogen.

A

oxide

Mg + H2O (steam) → MgO + H2.

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8
Q

What trend occurs in the solubility of Group 2 hydroxides down the group?

A

Increases

For example, Mg(OH)2 is sparingly soluble while Ba(OH)2 is much more soluble.

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9
Q

True or False:

Magnesium hydroxide is used in medicine as an antacid.

A

True

It neutralises excess stomach acid.

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10
Q

What agricultural substance is used to neutralise acidic soils?

A

Calcium hydroxide

It increases soil pH to improve crop growth.

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11
Q

Fill in the blank:

The solubility of Group 2 _______ decreases down the group.

A

sulfates

BaSO4 is insoluble in water.

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12
Q

What reagent is used to test for sulfate ions in solution?

A

Acidified barium chloride

A white precipitate of BaSO4 confirms sulfate ions.

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13
Q

What property of magnesium hydroxide allows it to be used as an antacid?

A

It is sparingly soluble in water.

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14
Q

How does melting point change down Group 2?

A

It generally decreases down the group.

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15
Q

How is titanium extracted from TiCl₄ using magnesium?

A

TiCl₄ + 2Mg → Ti + 2MgCl₂

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16
Q

Why does the melting point of Group 2 elements decrease down the group?

A

The ions get larger, so charge density decreases and metallic bonding becomes weaker.

Weaker electrostatic attraction between positive ions and delocalised electrons.

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17
Q

What is the role of magnesium in extracting titanium from TiCl₄?

A

It acts as a reducing agent.

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18
Q

Why are CaO or CaCO₃ used in flue gas treatment?

A

To remove SO₂ (a pollutant)

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19
Q

What are the equations for removing SO₂ using CaO/CaCO₃?

A

CaO + SO₂ → CaSO₃
CaCO₃ + SO₂ → CaSO₃ + CO₂

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20
Q

Why is SO₂ removed from flue gases?

A

To reduce acid rain and environmental damage.

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21
Q

What is BaSO₄ used for in medicine?

A

Barium meal- lines the gut in X rays

It is insoluble so it does not release toxic Ba²⁺ ions, and it absorbs X-rays due to its high density, outlining the gut.

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22
Q

What is the equation for the sulfate test using BaCl₂?

A

Ba²⁺(aq) + SO₄²⁻(aq) → BaSO₄(s)

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23
Q

Why is the solution acidified when testing for sulfate ions?

A

To remove carbonate impurities that could also form a precipitate

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24
Q

What would happen if the solution was not acidified?

A

Carbonate ions could form BaCO₃(s), giving a false positive.

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25
What general **trend in electronegativity** occurs down **Group 7** from fluorine to iodine?
Decreases ## Footnote Increased atomic radius and shielding reduce the nucleus’ attraction for bonding electrons.
26
What happens to the **boiling point** of **halogens** as you move down Group 7?
Increases ## Footnote Larger molecules have stronger London dispersion forces.
27
# Fill in the blank: The increase in **boiling point** down the halogen group is due to stronger _\_\_\_\_\_\_ forces.
van der Waals ## Footnote These induced dipole–dipole forces increase with molecular size.
28
# True or False: **Chlorine** is a stronger **oxidising agent** than iodine.
True ## Footnote Oxidising ability decreases down the group.
29
What happens to the **oxidising ability** of **halogens** down Group 7?
Decreases ## Footnote Larger atoms gain electrons less easily.
30
# True or False: **Iodide ions** are stronger **reducing agents** than chloride ions.
True ## Footnote Reducing ability of halide ions increases down the group.
31
# Fill in the blank: In **displacement reactions**, a more reactive halogen will _\_\_\_\_\_\_ a less reactive halide from solution.
displace ## Footnote For example, Cl2 displaces Br- from solution.
32
What **reagent** is used to test for **halide ions** in aqueous solution?
Acidified silver nitrate ## Footnote It forms characteristic precipitates with halide ions.
33
# True or False: **Silver nitrate solution** is acidified to remove **interfering carbonate ions**.
True ## Footnote Nitric acid prevents false positives from other precipitates.
34
# Fill in the blank: A **white precipitate** formed with silver nitrate indicates the presence of _\_\_\_\_\_\_ ions.
chloride ## Footnote AgCl forms a white precipitate.
35
What happens when **dilute ammonia** is added to **silver chloride**?
Dissolves ## Footnote AgCl dissolves because it forms a soluble complex ion.
36
Which **silver halide** does not dissolve in **ammonia solution**?
Silver iodide ## Footnote AgI is the least soluble of the silver halides.
37
What **ions** are formed when **chlorine reacts with water** in the main equilibrium reaction?
Chloride and chlorate(I) ## Footnote Cl2 + H2O ⇌ Cl- + ClO- + H+.
38
What type of **ion** is **ClO⁻** formed when chlorine reacts with water?
Chlorate(I) ion ## Footnote Also known as the hypochlorite ion.
39
# Fill in the blank: When **chlorine dissolves in water**, it forms chloride ions and _\_\_\_\_\_\_ (I) ions.
chlorate ## Footnote These ions contribute to chlorine’s disinfectant properties.
40
# True or False: **Chlorine** can react with water to produce **oxygen and chloride ions**.
True ## Footnote An alternative reaction forms O2 and HCl.
41
What is the **main use of chlorine** in **public water supplies**?
To kill bacteria. ## Footnote Chlorine kills bacteria and other microorganisms.
42
# True or False: The **health benefits** of **chlorinating drinking water** generally outweigh the risks.
True ## Footnote Chlorination has greatly reduced waterborne diseases.
43
# Fill in the blank: Chlorine reacts with **cold dilute sodium hydroxide** to form sodium chloride and sodium _\_\_\_\_\_\_ (I).
chlorate ## Footnote The product is sodium chlorate(I) (sodium hypochlorite).
44
What common **household chemical** contains **sodium chlorate(I)**?
Bleach ## Footnote Sodium hypochlorite is widely used as a disinfectant and bleaching agent.
45
# True or False: **Chlorate(I) ions** act as **oxidising agents** in disinfectants.
True ## Footnote They kill microbes by oxidising biological molecules.
46
Why is **chlorine** effective in **killing bacteria** in water treatment?
Strong oxidising agent ## Footnote It disrupts essential cellular components in microorganisms.
47
# Fill in the blank: In **water treatment**, chlorine is added because it kills harmful _\_\_\_\_\_\_.
microorganisms ## Footnote This prevents diseases such as cholera and typhoid.
48
What **societal factor** must be considered when adding chemicals like **chlorine to water supplies**?
Risk–benefit balance ## Footnote Decisions weigh health benefits against potential chemical risks.
49
Explain **why the electronegativity** of the halogens **decreases** going down the group
The number of electron shells increases down the group. This increases atomic radius and electron shielding. As a result, the nucleus has a weaker attraction for bonding electrons.
50
What is the colour of the **silver bromide precipitate**?
Cream
51
What is the colour of the **silver iodide precipitate**?
Yellow
52
How does **NaCl react with concentrated H₂SO₄**?
Forms HCl gas. This is an acid-base reaction only, no redox occurs.
53
How does **NaBr** react with concentrated **H₂SO₄**?
Forms **HBr** gas. **HBr** can be oxidized by **H₂SO₄** to produce **Br₂**. ## Footnote This occurs because **Br⁻** is a stronger reducing agent than **Cl⁻**.
54
How does **NaI** react with concentrated **H₂SO₄**?
Forms **HI** gas. **HI** is a strong reducing agent, leading to further reactions that can produce: * **I₂** (iodine) * **H₂S**, **SO₂**, or **S** (depending on conditions)
55
Why do **larger halide ions** have **stronger reducing ability**?
Larger ions (I⁻, Br⁻) have weaker hold on their electrons, making them more able to donate electrons → stronger reducing agents → more likely to reduce H₂SO₄
56
What type of **trend** occurs in the **oxides of Period 3 elements** from sodium to sulfur?
Basic to acidic ## Footnote Oxides change from basic → amphoteric → acidic across the period.
57
What type of **oxide** is **sodium oxide** when it reacts with water?
Basic oxide ## Footnote Na2O reacts with water to form sodium hydroxide solution.
58
# Fill in the blank: Sodium oxide reacts with **water** to produce sodium _\_\_\_\_\_\_.
hydroxide ## Footnote Na2O + H2O → 2NaOH, forming a strongly alkaline solution.
59
# True or False: **Magnesium oxide** forms an **alkaline solution** when reacting with water.
True ## Footnote MgO reacts slowly with water to form Mg(OH)2.
60
Which **Period 3 oxide** is **amphoteric** and reacts with both acids and bases?
Aluminium oxide ## Footnote Al2O3 shows both acidic and basic behaviour.
61
# True or False: **Silicon dioxide** reacts readily with **water** to form an acidic solution.
False ## Footnote SiO2 does not react with water due to its giant covalent structure.
62
# Fill in the blank: **Phosphorus(V) oxide** reacts with water to form _\_\_\_\_\_\_ acid.
phosphoric ## Footnote P4O10 + H2O forms H3PO4.
63
What type of **oxides** are **sulfur dioxide and sulfur trioxide**?
Acidic oxides ## Footnote They react with water to form sulfurous and sulfuric acids.
64
# True or False: **Sulfur trioxide** reacts with water to form **sulfuric acid**.
True ## Footnote SO3 + H2O → H2SO4.
65
Why does **silicon dioxide** have a very **high melting point**?
Giant covalent structure ## Footnote Strong covalent bonds extend throughout the lattice.
66
# Fill in the blank: **Sodium oxide and magnesium oxide** have high melting points due to strong _\_\_\_\_\_\_ bonding.
ionic ## Footnote Ionic lattices require large amounts of energy to break.
67
How does the **pH of solutions formed by Period 3 oxides** generally change from Na to S?
Decreases ## Footnote Solutions change from strongly alkaline to acidic across the period.
68
**Observations** when **sodium reacts with water**
Floats, melts into a ball, moves rapidly, fizzing (H₂), may ignite
69
How does **magnesium react with cold water**?
Very slow reaction forming magnesium hydroxide and hydrogen
70
How does **magnesium** react with **steam**?
Reacts faster to form magnesium oxide and hydrogen ## Footnote Equation: Mg + H₂O(g) → MgO + H₂
71
What **oxides do Na–S form** with oxygen?
Na₂O, MgO, Al₂O₃, SiO₂, P₄O₁₀, SO₂, SO₃
72
Which **oxides** are **simple molecular**?
P₄O₁₀, SO₂, SO₃
73
**Trend** in **melting point of oxides** Na → S
Increases (Na₂O → Al₂O₃), then decreases sharply (SiO₂ → SO₃) ## Footnote Increases from Na₂O → Al₂O₃ due to stonger ionic bonding. SiO₂ has the highest melting point due to giant covalent structure with many strong bonds. From P₄O₁₀ the melting point decreases because they are simple molecular with weak intermolecular forces.
74
Does **Al₂O₃ react with water**?
No (insoluble, amphoteric oxide)
75
What happens when **SO₂ reacts with water**?
Forms sulfurous acid (H₂SO₃, weak acid)
76
**Anion** formed from **phosphoric acid**
PO₄³⁻ (phosphate)
77
**Anion** from **sulfurous acid**
SO₃²⁻ (sulfite)
78
**Anion** from **sulfuric acid**
SO₄²⁻ (sulfate)
79
How do **basic oxides** react with acids?
Neutralisation → salt + water
80
How do **acidic oxides** react with bases?
Forms a salt and water in a neutralisation reaction
81
How does **Al₂O₃ react with acid**?
Al₂O₃ + 6HCl → 2AlCl₃ + 3H₂O
82
How does **Al₂O₃ react with base**?
Al₂O₃ + 2NaOH + 3H₂O → 2NaAl(OH)₄
83
Observation when **magnesium reacts with oxygen**?
Burns with bright white flame to form MgO
84
How does **sodium react with oxygen**?
Very vigorously to form sodium oxide (Na₂O)
85
How does **aluminium react with oxygen**?
Forms Al₂O₃ but reaction is limited bry protective oxide layer
86
How does **silicon react with oxygen**?
Reacts at high temperature to form SiO₂
87
How does **phosphorus react with oxygen**?
Burns readily to form P₄O₁₀ (white smoke)
88
Observation when **sulfur reacts with oxygen**?
Burns with blue flame to form SO₂ (can further oxidise to SO₃)
89
pH of NaOH
14
90
What is the **pH of Mg(OH)₂ in water**?
9–10 ## Footnote because it is only slightly soluble, so it produces a low concentration of OH⁻ ions
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