Group Properties And Trends

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Group I Properties

Group I metals are called alkali metals because they form alkaline solutions with water.
They have one electron in their outer shell.
Physical properties: soft, shiny when cut, good conductors of heat/electricity, low melting points (decrease down group), low densities.
Stored under oil to prevent reaction with oxygen and water vapour in air.
React with water to form metal hydroxide and hydrogen gas: 2M + 2H₂O → 2MOH + H₂.
Reactivity increases down the group: Li fizzes slowly, Na more vigorous, K burns with lilac flame.
Melting point decreases down group; density generally increases (exception early group).
Predict properties of unknown alkali metals using trends: e.g., Rb reacts very violently, Cs may explode.

Electron configuration of sodium (Group I) showing one outer electron.

Group VII Properties

Group VII elements are halogens: non-metals, poisonous, diatomic (F₂, Cl₂, Br₂, I₂, At₂).
They have seven electrons in outer shell and gain one electron to form halide ions.
Physical state changes down group: Cl₂ pale green gas, Br₂ red-brown liquid, I₂ grey-black solid.
Density increases down group; melting/boiling points increase down group.
Reactivity decreases down group (opposite to Group I).
Reason: atomic radius increases and electron shielding increases, so attraction for an incoming electron weakens.
Colour darkens down group: F₂ yellow, Cl₂ green, Br₂ red-brown, I₂ violet vapour, At₂ black.

Physical states of the halogens at room temperature

Group VII Displacement Reactions

A more reactive halogen displaces a less reactive halogen from an aqueous halide solution.
Reactivity order: Cl₂ > Br₂ > I₂.
Chlorine displaces bromide: 2KBr + Cl₂ → 2KCl + Br₂ (solution turns orange/yellow).
Chlorine displaces iodide: 2KI + Cl₂ → 2KCl + I₂ (solution turns brown).
Bromine displaces iodide: MgI₂ + Br₂ → MgBr₂ + I₂ (solution turns brown).
No reaction occurs if the halogen is less reactive than the halide (e.g., Br₂ with KCl).
Aqueous colours: Cl₂ very pale green (dilute appears colourless), Br₂ orange, I₂ brown.

Summary table of displacement reactions

Transition Elements

Transition elements are metals found in the centre of the Periodic Table between Group 2 and 3.
Typical metallic properties: lustrous, hard, strong, good conductors, high melting points (except Hg).
Unique properties: form ions with different charges (e.g., Fe²⁺ and Fe³⁺).
They are useful as catalysts (e.g., iron in Haber process).
They form coloured compounds (e.g., copper sulfate blue, copper oxide black, copper carbonate green).
Scandium and zinc are not considered transition elements because they do not form coloured compounds and have only one oxidation state.

Coloured compounds formed by transition metal ions

Noble Gases

Noble gases are in Group VIII (Group 18): non-metals, monatomic, colourless, gaseous.
They have full outer electron shells (e.g., He: 2, Ne: 2,8, Ar: 2,8,8).
Full outer shells make them unreactive (inert) – they do not easily form bonds.
They have very low melting and boiling points.

The noble gases are located at the right of the Periodic Table

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1.Complete the sentence.
Easy
Group I metals are called the ____ metals because they form alkaline solutions when they react with water.
2.Which of the following is a physical property of Group I metals?
Easy
- AThey are hard and brittle
- BThey have high melting points compared to other metals
- CThey are soft and can be cut easily
- DThey are gases at room temperature
3.The reactivity of Group I metals decreases as you move down the group.
Easy
True or false?
4.State the colour of iodine in aqueous solution.
Easy
5.Which halogen is a red-brown liquid at room temperature?
Easy
- AChlorine
- BBromine
- CIodine
- DAstatine
6.How many electrons are in the outer shell of a halogen atom?
Easy
- A7
- B6
- C9
- D8
7.Arrange the following halogens in order of increasing reactivity (least reactive first).
Medium
- Iodine
- Bromine
- Chlorine
8.Predict the colour of astatine based on the trend in Group VII.
Medium

更多題目

9.Which observation would be expected when rubidium reacts with water?
Medium
- ASlow fizzing and the metal moves slowly
- BVigorous reaction with a lilac flame
- CVery violent reaction, possibly exploding
- DNo reaction because rubidium is stored under oil
10.Write the word equation for the reaction of sodium with water.
Medium
sodium + water → ____ + ____
11.Match each transition element property to its example.
Medium
- Forms ions with different charges
- Useful as catalysts
- Forms coloured compounds
- Iron forms Fe²⁺ and Fe³⁺
- Iron in the Haber process
- Copper forms blue copper sulfate
12.Noble gases are monoatomic and have full outer electron shells.
Easy
True or false?
13.Group I metals are called alkali metals because they form alkaline solutions when they react with water.
Easy
True or false?
14.How many electrons are in the outer shell of a Group I metal atom?
Easy
- A1
- B2
- C7
- D8
15.Which of the following is a correct observation when potassium reacts with water?
Medium
- ASlow fizzing and the metal floats
- BBurns with a lilac flame
- CA red-brown colour appears
- DThe metal sinks to the bottom
16.Arrange the following Group I metals in order of increasing reactivity (least reactive first).
Medium
- Potassium
- Lithium
- Sodium
17.The melting point of Group I metals increases as you go down the group.
Easy
True or false?
18.What is the colour of bromine at room temperature?
Easy
- APale yellow-green gas
- BRed-brown liquid
- CGrey-black solid
- DColourless gas
19.The reactivity of halogens increases as you go down Group VII.
Easy
True or false?
20.Match each halogen to its physical state at room temperature.
Easy
- Chlorine
- Bromine
- Iodine
- Solid
- Liquid
- Gas
21.Chlorine water is added to potassium bromide solution. What colour change is observed?
Medium
- AColourless to brown
- BColourless to orange
- COrange to colourless
- DBrown to colourless
22.Which of the following are properties of transition elements? (Select all that apply)
Medium
- AForm ions with different charges
- BAre good catalysts
- CForm colourless compounds
- DHave low melting points
23.Match each Group I metal to the correct observation when it reacts with water.
Medium
- Lithium
- Sodium
- Potassium
- Burns with a lilac flame
- Relatively slow reaction, fizzing
- More vigorous fizzing, moves rapidly
24.Arrange the following halogens in order of increasing melting point (lowest first).
Medium
- Chlorine
- Bromine
- Iodine
25.Which statement explains why the reactivity of halogens decreases down Group VII?
Medium
- AAtomic radius decreases, making it easier to gain an electron
- BThe number of electron shells increases, reducing attraction for an incoming electron
- CThe outer shell has fewer electrons, so the atom is less reactive
- DThe melting point increases, so the elements are less reactive
26.Which of the following displacement reactions will occur? (Select all that apply)
Medium
- AChlorine + potassium bromide solution
- BBromine + potassium chloride solution
- CIodine + potassium bromide solution
- DBromine + potassium iodide solution
- EChlorine + potassium iodide solution
27.Match each halogen to its colour in aqueous solution.
Easy
- Chlorine
- Bromine
- Iodine
- Orange
- Brown
- Very pale green (usually colourless)
28.Rubidium is below potassium in Group I. Which observation would you NOT expect when rubidium reacts with water?
Medium
- AA violent reaction
- BA lilac flame
- CThe metal moves slowly on the surface
- DDissolves very quickly
29.Which of the following are true about noble gases? (Select all that apply)
Medium
- AThey are diatomic
- BThey are colourless gases
- CThey have very low melting points
- DThey are reactive because they need to gain electrons
- EThey have full outer electron shells
30.The table shows the melting points of some Group I metals. | Metal | Melting point (°C) | |-------|-------------------| | Lithium | 180 | | Sodium | 98 | | Potassium | 63 | | Rubidium | ? | What is the most likely melting point of rubidium?
Medium
- A39 °C
- B63 °C
- C98 °C
- D180 °C
31.Which of the following displacement reactions will occur?
Medium
- AChlorine + potassium bromide
- BBromine + potassium chloride
- CIodine + potassium bromide
- DIodine + potassium chloride
32.A student adds a piece of potassium to water. Which observation indicates that potassium is more reactive than sodium?
Medium
- APotassium fizzes less vigorously than sodium
- BPotassium burns with a lilac flame
- CPotassium moves slowly on the water surface
- DPotassium dissolves more slowly than sodium
33.The noble gases are monoatomic and have full outer electron shells.
Easy
True or false?
34.Group I metals are stored under oil because they react readily with oxygen and water vapour in the air.
Easy
True or false?
35.Which statement explains why the reactivity of Group I metals increases down the group?
Medium
- AThe outer electron is further from the nucleus and more easily lost
- BThe outer electron is closer to the nucleus and more easily lost
- CThe atoms have more protons, making them more reactive
- DThe melting point decreases, making them more reactive
36.Which of the following are properties of the halogens? (Select all that apply)
Medium
- AThey are diatomic
- BThey have seven electrons in their outer shell
- CThey are metals
- DThey are poisonous
- EThey conduct electricity
37.Match each halogen to its colour at room temperature.
Easy
- Chlorine
- Bromine
- Iodine
- Pale yellow-green gas
- Red-brown liquid
- Grey-black solid
38.Chlorine water is added to potassium iodide solution. What colour change is observed?
Medium
- AColourless to brown
- BColourless to orange
- CBrown to colourless
- DOrange to colourless
39.Which statement explains why noble gases are unreactive?
Easy
- AThey have full outer electron shells
- BThey have low melting points
- CThey are colourless
- DThey are monoatomic
40.Which of the following are properties of Group VII elements? (Select all that apply)
Medium
- AThey are diatomic.
- BThey have seven electrons in their outer shell.
- CThey are all gases at room temperature.
- DTheir reactivity increases down the group.
- EThey form halide ions by gaining one electron.
41.The reactivity of Group I metals increases as you move down the group.
Easy
True or false?
42.The table shows the melting points of some Group I metals. | Metal | Melting point (°C) | |-------|-------------------| | Lithium | 180 | | Sodium | 98 | | Potassium | 63 | | Rubidium | ? | Which metal is likely to be rubidium?
Easy
- ALithium, 180 °C
- BSodium, 98 °C
- CPotassium, 63 °C
- DRubidium, 39 °C
43.A student adds a piece of lithium to water. Which of the following observations is correct?
Medium
- AThe lithium floats and moves rapidly on the surface, producing a lilac flame.
- BThe lithium fizzes slowly and moves on the surface without a flame.
- CThe lithium sinks and reacts vigorously with a yellow flame.
- DThe lithium dissolves quickly and the solution turns red litmus blue.
44.Complete the sentence about Group I metals.
Easy
Group I metals are stored under oil to prevent them from reacting with ____ and ____.
45.State one reason why noble gases are unreactive.
Easy
46.State the colour of iodine vapour.
Easy
47.Complete the sentence about the reactivity of Group I metals.
Easy
The reactivity of Group I metals ____ as you go down the group.
48.A student adds a piece of sodium to water and collects the hydrogen gas produced. If 0.46 g of sodium reacts completely, what volume of hydrogen gas is produced at room temperature and pressure? (Molar mass Na = 23 g/mol; molar volume at RTP = 24 dm³/mol)
Hard
49.Chlorine water is added to potassium bromide solution. State the colour change observed.
Easy
50.Complete the sentence about noble gases.
Easy
Noble gases are ____ because they have full outer electron shells.
51.Explain why the reactivity of Group I metals increases down the group.
Medium
52.Explain why the reactivity of Group I metals increases as you move down the group.
Medium
53.A student adds a piece of sodium to water and collects the hydrogen gas produced. If 0.46 g of sodium reacts completely, what volume of hydrogen gas is produced at room temperature and pressure? (Molar mass Na = 23 g/mol; molar volume at RTP = 24 dm³/mol)
Hard
- A2.24 dm³
- B0.24 dm³
- C1.24 dm³
- D-0.76 dm³

字卡

What are the Group I metals called?

They are called the alkali metals because they form alkaline solutions when reacted with water.

List the first three Group I metals.

Lithium (Li), sodium (Na), and potassium (K).

How many electrons are in the outer shell of Group I metals?

One electron.

Describe the trend in melting point down Group I.

Melting point generally decreases as you move down the group.

Why are Group I metals stored under oil?

To prevent them from reacting with oxygen and water vapour in the air.

Write the general equation for the reaction of a Group I metal with water.

2M (s) + 2H₂O (l) → 2MOH (aq) + H₂ (g)

What is observed when lithium reacts with water?

Relatively slow reaction, fizzing, and lithium moves on the surface of the water.

What is observed when potassium reacts with water?

More vigorous than sodium, burns with a lilac flame, moves very rapidly on the surface, and dissolves very quickly.

How does reactivity change down Group I?

Reactivity increases as you move down the group.

What are the halogens?

Group VII non-metals that are poisonous and diatomic, including fluorine, chlorine, bromine, iodine, and astatine.

How many electrons are in the outer shell of halogens?

Seven electrons.

State the physical states of chlorine, bromine, and iodine at room temperature.

Chlorine is a pale yellow-green gas, bromine is a red-brown liquid, and iodine is a grey-black solid.

How does reactivity change down Group VII?

Reactivity decreases as you go down the group.

Why does halogen reactivity decrease down the group?

Atomic radius increases and electron shielding increases, reducing the attraction for an incoming electron.

What happens when chlorine solution is added to potassium bromide solution?

Chlorine displaces bromine, forming potassium chloride and bromine; the solution turns orange.

Write the ionic equation for the displacement of bromide by chlorine.

2Br⁻ (aq) + Cl₂ (aq) → 2Cl⁻ (aq) + Br₂ (aq)

What colour is aqueous iodine?

Brown.

List three typical properties of transition elements.

They form ions with different charges, are useful as catalysts, and form coloured compounds.

Give an example of a transition element used as a catalyst.

Iron is used as the catalyst in the Haber process.

Why are scandium and zinc not considered transition elements?

They do not form coloured compounds and have only one oxidation state.

What are the noble gases?

Group VIII non-metals that are monoatomic, colourless, gaseous, and unreactive.

Why are noble gases unreactive?

They have full outer electron shells, making them stable with no need to gain or lose electrons.

Give the electronic configuration of neon.

2,8

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