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Chemistry ✦ (Form 4) > Chapter 4 > Flashcards

Chapter 4 Flashcards

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1
Q

Explain group 1,2,3

A

All are metals
Can conduct electricity

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2
Q

Group 14 - 17

A

Non-metals

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3
Q

What are Group 18 elements also known as?

A

A: Inert gases or noble gases.

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4
Q

Name all the Group 18 elements.

A

Helium (He)
Neon (Ne)
Argon (Ar)
Krypton (Kr)
Xenon (Xe)
Radon (Rn)
Oganesson (Og).

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5
Q

What are the physical properties of Group 18 elements?
1. Water
2. Conduction
3. BP. MP
4. Attraction forces

A

Insoluble in water.
Do not conduct electricity or heat.
Boiling and melting points increase down the group.
Van der Waals forces increase as atom size increases.

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6
Q

Why are noble gases chemically non-reactive?

A

A stable duplet electron arrangement with two valence electrons.

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7
Q

Why are noble gases chemically non-reactive?

A

A stable octet/ duplet electron arrangement with eight/two valence electrons.

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8
Q

Give two uses of helium.

A

Filling weather balloons.
Oxygen tanks for divers.

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9
Q

Name one use of radon

A

Treating cancer.

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10
Q

What is neon used for?

A

Neon is used in advertising board lights.

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11
Q

List two uses of argon.

A

Filling electric bulbs.
Providing an inert atmosphere for high-temperature welding.

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12
Q

Give two uses of krypton.

A

Flashlights for cameras.
Lasers for eye retina treatment.

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13
Q

What are two uses of xenon?

A

Lighthouse lamps.
Anesthesia.

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14
Q

How do boiling points of Group 18 elements change down the group?

A

Boiling points increase down the group due to stronger van der Waals forces.

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15
Q

What causes the increase in van der Waals forces in noble gases?

A

The increase in atom size down the group.

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16
Q

What is the group name for Group 1 elements?

A

Alkali metals, except for hydrogen

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17
Q

List the elements in Group 1.

A

Hydrogen (H)
Lithium (Li)
Sodium (Na)
Potassium (K)
Rubidium (Rb)
Caesium (Cs)
and Francium (Fr).

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18
Q

What is the general physical state of Group 1 elements?

A

They are soft metals.

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19
Q

Are alkali metals good conductors?

A

Yes, they are good conductors of heat and electricity.

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20
Q

What happens to the atomic radius of Group 1 elements as you go down the group?

A

The atomic radius increases.

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21
Q

What trend is observed in the melting point of Group 1 elements down the group?

A

The melting point decreases.

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22
Q

How does density change down Group 1?

A

Density increases as you move down the group.

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23
Q

How does density change down Group 1?

A

Density increases as you move down the group.

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24
Q

What happens when Group 1 elements react with water?

A

They produce hydrogen gas and an alkaline solution.

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25
Q

Write the reaction of lithium with water.

A

2Li(s) + 2H₂O(l) → 2LiOH(aq) + H₂(g).

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26
Q

What happens when Group 1 elements react with oxygen?

A

They form metal oxides.

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27
Q

Write the reaction of lithium with oxygen.

A

4Li(s) + O₂(g) → 2Li₂O(s)

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28
Q

What is produced when Group 1 elements react with halogens?

A

Metal halides.

29
Q

Write the reaction of lithium with chlorine.

A

2Li(s) + Cl₂(g) → 2LiCl(s)

30
Q

How does reactivity (electropositivity) change as you go down Group 1?

A

Reactivity increases down the group.

31
Q

Why does electropositivity increase down Group 1?

A

The atomic radius increases, weakening the attractive force between the nucleus and the valence electron, making it easier to donate the electron.

32
Q

Describe physical properties of Group 1

A

Soft, shiny metals with low melting points that are highly reactive and burn easily.

33
Q

How do rubidium, caesium, and francium react with water and oxygen?

A

They react vigorously, producing heat and hydrogen gas with water, and forming oxides with oxygen.

34
Q

List the elements in Period 3.

A

Sodium (Na)
Magnesium (Mg)
Aluminium (Al)
Silicon (Si)
Phosphorus (P)
Sulphur (S)
Chlorine (Cl)
Argon (Ar).

35
Q

What happens to the atomic radius as you go across Period 3?

A

The atomic radius decreases across the period.

36
Q

Why does the atomic radius decrease across Period 3?

A

A: The number of protons increases, which increases the electrostatic force and pulls valence electrons closer to the nucleus.

37
Q

How does the number of valence electrons change across Period 3?

A

A: The number of valence electrons increases from left to right.

38
Q

What happens to electronegativity as you move across Period 3?

A

Electronegativity increases across the period.

39
Q

Why does electronegativity increase across Period 3?

A

The increasing number of protons strengthens the electrostatic force, attracting electrons more strongly.

40
Q

Describe the trend of melting and boiling points in Period 3.

A

They increase from the left to the middle of the period and then decrease again.

41
Q

How does the metallic nature of elements change across Period 3?

A

The elements change from metals to metalloids and then to non-metals as electronegativity increases.

42
Q

How does the nature of oxides change across Period 3?

A

The oxides change from basic to amphoteric and then to acidic.

43
Q

What is aluminium (Al) commonly used for?

A

A: As a material in cans.

44
Q

What is magnesium (Mg) commonly used for?

A

As a substance in lighters.

45
Q

What is phosphorus (P) commonly used for?

A

A: In fireworks.

46
Q

What is sulphur (S) used for?

A

A: As a fungicide.

47
Q

What are metalloids like silicon (Si) used for?

A

A: As semiconductors in electronic microchips for computers and mobile phones.

48
Q

Summarize the key trends in Period 3 elements.

Atomic radius:
Valence electrons:
Electronegativity:
Melting/Boiling Points:
Metallic Nature:
Oxide Nature:

A

Atomic radius: Decreases.

Valence electrons: Increase.

Electronegativity: Increases.

Melting/Boiling Points: Increase to the middle, then decrease.

Metallic Nature: Changes from metals to metalloids to non-metals.

Oxide Nature: Changes from basic to amphoteric to acidic.

49
Q

Where are transition elements located on the periodic table?

A

A: From Group 3 to Group 12.

50
Q

What are the general characteristics of transition metals?

A

High density.
High hardness.
Silvery surface.
High tensile strength.
High conductivity (thermal and electrical).
Ductile and malleable.
High melting and boiling points.

51
Q

What is a unique chemical property of transition elements?

A

A: They have multiple oxidation states.

52
Q

Provide examples of oxidation states for transition elements.
A:

Chromium:
Manganese:
Iron:
Copper:

A

Chromium:
+3 (Chromium(III) chloride, CrCl₃)
+6 (Potassium dichromate, K₂Cr₂O₇)

Manganese:
+2 (Manganese(II) chloride, MnCl₂),
+4 (Manganese(IV) oxide, MnO₂),
+7 (Potassium manganate(VII), KMnO₄).

Iron:
+2 (Iron(II) sulphate, FeSO₄)
+3 (Iron(III) chloride, FeCl₃).

Copper:
+1 (Copper(I) oxide, Cu₂O) and
+2 (Copper(II) oxide, CuO).

53
Q

Why do transition elements form colored compounds?

A

The presence of unpaired d-electrons allows light absorption, leading to characteristic colors.

54
Q

Give examples of colored ions and their colors.

Chromium(III)
Dichromate(VI)
Manganese(II)
Manganate(VII)
Iron(II)
Iron(III)
Copper(II)
Nickel(II)

A

(Cr³⁺): Green.
(Cr₂O₇²⁻): Orange.
(Mn²⁺): Pink.
(MnO₄⁻): Purple.
(Fe²⁺): Green.
(Fe³⁺): Brown.
(Cu²⁺): Blue.
(Ni²⁺): Green.

55
Q

What role do transition elements play in catalysis?

A

They act as catalysts to increase the rate of reactions.

56
Q

Name examples of transition elements and their catalytic functions.

Iron (Fe):
Platinum (Pt):
Vanadium(V) oxide (V₂O₅):
Nickel (Ni) or Platinum (Pt):

A

Iron (Fe): Haber process
for ammonia production.

Platinum (Pt): Ostwald process
for nitric acid production.

Vanadium(V) oxide (V₂O₅):
Contact process
for sulphuric acid production.

Nickel (Ni) or Platinum (Pt): hydrogenation of vegetable oils
to make margarine.

57
Q

What are some industrial uses of
Iron (Fe):

A

Building bridges and as a catalyst in the Haber process.

58
Q

What are some industrial uses of
Platinum (Pt):

A

Catalyst in nitric acid production.

59
Q

What is vanadium(V) oxide used for in industry?

A

A: It is used as a catalyst in the Contact process to produce sulfuric acid (H₂SO₄).

60
Q

What is titanium commonly used for in industry?

A

A: Titanium is used to make paints and as a material for high-strength alloys.

61
Q

How is manganese used in industry?

A

A: Manganese is used to make stained glass and is also a component in steel production.

62
Q

What is the role of nickel in industry?

A

A: Nickel is used in the hydrogenation process to turn vegetable oils into margarine and in the production of stainless steel.

63
Q

What is copper widely used for?

A

A: Copper is used in electrical wiring due to its excellent conductivity.

64
Q

How do the oxides of transition elements change across the period?

A

A: The oxides change from basic to amphoteric and then to acidic as you move across the period.

65
Q

What is the effect of increasing the number of protons in transition metals? (Size)

A

A: As the number of protons increases, the atomic radius decreases due to the stronger electrostatic pull between protons and electrons.

66
Q

How does electronegativity change across Period 3?

A

A: Electronegativity increases across the period as the number of protons increases attraction force .

67
Q

How does the melting point of transition elements change across the period?

A

A: Melting points increase towards the middle of the period and then decrease again towards the right.

68
Q

Going down group 1

A

The atomic radius increases.
Density increases.
The melting point decreases.
Electropositivity also increase
The attractive force between the nucleus and the single electron decreases as the radius increases.

69
Q

Going down group 17

A

The atomic radius increases.
Reactivity decreases.
Boiling and melting point increases.
The van der Waals force
Size of the atom increases.
The electronegativity decreases
Radius increases
Force between the valence electron and nucleus decreases.

Chemistry ✦ (Form 4) (11 decks)

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