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A-LEVEL CHEM: Exam Questions > AS-Level Chemistry: June 2016 Paper 1 PP > Flashcards

AS-Level Chemistry: June 2016 Paper 1 PP Flashcards

1
Q

Give the full Electron Configuration of an Al Atom and of a Cr3+ Ion.

(2 marks)

A

-Al Atom: 1s2 2s2 2p6 3s2 3p1

-Cr3+ Ion: 1s2 2s2 2p6 3s2 3p6 3d3

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2
Q

Deduce the Formula of the Ion that has a Charge of 2+ with the Same Electron Configuration as Krypton.

(1 mark)

A

Sr2+

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3
Q

Deduce the Formula of the Compound that contains 2+ Ions and 3- Ions that both have the Same Electron Configuration as Argon.

(1 mark)

A

Ca3P2

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4
Q

Deduce which of Na+ and Mg2+ is the Smaller Ion.
Explain your answer.

(2 marks)

A

-Smaller ion: Mg2+

-Explanation: Because Mg2+ has more protons, so Higher Nuclear Attraction AND with the SAME shielding effect.

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5
Q

Write an Equation to represent the process that occurs when the First Ionisation Energy for Sodium is measured.

(1 mark)

A

Na(g) —–> Na+(g) + e-

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6
Q

Explain why the First Ionisation Energy of Sulphur is Different from that of Phosphorus.

(2 marks)

A
  • e- Paired in P-Orbital in Sulphur.

-Paired e- Repel, so Less Energy needed to remove.

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7
Q

The student identified use of the Burette as the Largest source of Uncertainty in the
experiment.
Using the Same Apparatus, suggest how the procedure could be improved to
Reduce the Percentage Uncertainty in using the Burette.
Justify your suggested improvement.

(2 marks)

A

-Suggestion: Use a More Concentrated Solution.

-Justification: So a Larger Titre/reading will be needed.

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8
Q

In terms of Structure and Bonding explain why the Boiling Point of Bromine is Different from that of Magnesium.
Suggest why Magnesium is a Liquid over a much greater Temperature range compared to Bromine.

(5 marks)

A

-Bromine is Simple Molecular Structure.

-Magnesium is Metallic Structure. Positive Ions in a Cloud of Delocalised Electrons.

-Br2 has Weak Van der Waals Forces between the Molecules.

-Mg has much Stronger Metallic Bonds. So More Energy is required to overcome & break these Bonds.

-Mg has a much greater Liquid range because Forces of Attraction in Liquid/Molten Metal are Stronger.

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9
Q

Explain how Ions are Accelerated, Detected and have their Abundance Determined in a Time of Flight (TOF) Mass spectrometer.

(3 marks)

A

-Ions Accelerated by Attraction to Negatively Charged Plate.

-Ions Detected by Gaining Electrons.

-Abundance Determined by size of Current Flowing in the Detector upon impact.

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10
Q

Name the type of Bond formed between N and Al in H3NAlCl3 and explain how this bond is formed.

(2 marks)

A

-Type of Bond: Dative Covalent / Coordinate Bond.

-Explanation: Shared Pair of Electrons from the NH3.

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11
Q

Explain how the value of the Cl-Al-Cl Bond Angle in AlCl3 Changes, if at all, on formation of the Compound H3NAlCl3.

(2 marks)

A

-Aluminium is now surrounded by 4 Electron Pairs. Tetrahedral.

-Therefore Bond Angle Decreases from 120’ in AlCl3 to 107’-111’ in H3NAlCl3.

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12
Q

Write a Half-Equation for the Oxidation of Chloride Ions.

(1 mark)

A

2Cl- —–> Cl2 + 2e-

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13
Q

Write a Half-Equation for the Reduction of Chlorate(I) Ions to Chlorine in Acidic conditions.

(1 mark)

A

2ClO- + 4H+ + 2e- —–> Cl2 +2H2O

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14
Q

Write an overall Equation for the Redox Reaction of Chlorate(I) Ions with Hydrochloric Acid.

(1 mark)

A

ClO- + Cl- +2H+ —–> Cl2 + H2O

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15
Q

A Solution of Sodium Chlorate(I) was added to a Colourless Solution of Potassium Iodide.
Suggest what is Observed.
Explain the Reaction that leads to this Observation.

(3 marks)

A

-Goes Brown

-Due to Iodine

-Because I- is Oxidised.

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16
Q

Which Element is in the d-block of the Periodic Table? (1)

A) Selenium

B) Antimony

C) Tantalum

D) Lead

A

C) Tantalum

17
Q

Which Species contains an Element with an Oxidation State of +4? (1)

A) NO2 +

B) ClO3 -

C) H2SO3

D) PCl5

A

C) H2SO3

18
Q

There are 392mol of pure Gold in a bar measuring 10cm by 10cm by 40cm.
What is the Density of Gold in kg dm^-3? (1)

A) 193

B) 19.3

C) 1.93

D) 0.193

A

B) 19.3

19
Q

Ions of two Isotopes of Iron are:
53Fe2+ 56Fe2+
Which statement is correct? (1)

A) The Ions of both the Isotopes have the Electronic Configuration 1s2 2s2 2p6 3s2 3p6 4s2 3d6

B) The Ions of both the Isotopes contains 26 Neutrons.

C) 53Fe2+ has fewer Protons than 56Fe2+

D) After Acceleration to the same Kinetic Energy 56Fe2+ will move more Slowly than 53Fe2+

A

D

20
Q

Which of these Decreases down Group 2? (1)

A) First Ionisation Energy

B) Atomic Radius

C) Number of Protons

D) Reactivity with Water

A

A) First Ionisation Energy

21
Q

Which Substance exists as a Macromolecule? (1)

A) Cu

B) SiO2

C) P4O10

D) MgO

A

B) SiO2

22
Q

A pale brown Mixture of NO2 and N2O4 is allowed to reach Equilibrium in a sealed
Gas Syringe according to the following Equation.
2NO2(g) ⇌ N2O4(g)
When the plunger is pushed further into the Syringe the Pressure Increases and the
Mixture becomes paler in Colour.
When the Syringe is placed in a hot oven the Mixture becomes darker in Colour.
Which of the following statements is correct? (1)

A) NO2 is brown and the Forward Reaction is Exothermic.

B) NO2 is brown and the Forward Reaction is Endothermic.

C) NO2 is colourless and the Forward Reaction is Exothermic.

D) NO2 is colourless and the Forward Reaction is Endothermic.

A

A

23
Q

Which Molecule has the Largest Dipole? (1)

A) ClF3

B) BF3

C) SF6

D) CF4

A

A) ClF3

24
Q

In a Molecule of a Hydrocarbon, the fraction by Mass of Carbon is 9/11.
What is the Empirical Formula of the Hydrocarbon? (1)

A) CH

B) CH3

C) C3H8

D) C5H12

A

C) C3H8

25
Q

30cm^3 of Xenon are Mixed with 20cm^3 of Fluorine. the Gases React according to the following Equation. Assume the the Temperature and Pressure remain Constant.
Xe(g) + F2(g) —–> XeF2(g)
What is the final Volume of Gas after the Reaction is complete? (1)

A) 50cm^3

B) 40cm^3

C) 30cm^3

D) 20cm^3

A

C) 30cm^3

26
Q

Which of the following Solutions would React exactly with a Solution containing 0.0500mol Sulfuric Acid? (1)

A) 50.0cm^3 of 1.00mol dm−3 KOH

B) 100.0cm^3 of 2.00mol dm^-3 KOH

C) 100.0cm^3 of 2.00mol dm^-3 Ba(OH)2

D) 50.0cm^3 of 1.00mol dm^-3 Ba(OH)2

A

D

A-LEVEL CHEM: Exam Questions (5 decks)

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