Question 1

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Question 3

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Question 4

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Question 5

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Question 6

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Question 7

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Electron configurations for atoms of different elements are shown below.

Which electron configuration represents the element with the largest first ionisation energy?

1s²2s²2p⁶3s²
1s²2s²2p⁶3s²3p⁴
1s²2s²2p⁶3s²3p⁶
1s²2s²2p⁶3s²3p⁶4s²

Question 8

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Which of the following statements about 2-methylpropan-2-ol, CH₃C(CH₃)(OH)CH₃, are correct ?

The structure contains 16 bonding pair of electrons
The O-C-C bond angle is 109.5 ^o
The total number of electrons is 32

I and II only
I and III only
II and III only
I, II and III

Question 9

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The following equation shows the dissociation equilibrium of PCl₅.

PCl₅(g) → PCl₃(g) ＋ Cl₂(g)

The percentage yield of PCl₃ varies with temperature.

At 160°C PCl₃ yield is 13% and at 300°C yield is100%.

Which of the following rows is correct?

	The reaction is	Shape of PCl₃ molecule
A	exothermic	trigonal pyramidal
B	exothermic	trigonal planar
C	endothermic	trigonal pyramidal
D	endothermic	trigonal planar

Question 10

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Which of the following metals would have the highest melting point?

Na
Mg
Al
K

Question 11

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The correct order of increasing boiling points for the following compounds is

1-chlorobutane < butane < butan-1-ol
Butan-1-ol < 1-chlorobutane < butane,
Butane < 1-chlorobutane < butan-1-ol
Butan-1-ol < butane < 1-chlorobutane

Question 12

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Which equation below can represent both an enthalpy change of formation and combustion?

CH₄(g) + 2O₂(g) → CO₂(g) + 2H₂O(l)
2Na(s) + ½O₂(g) → Na₂O(s)
HCl(aq) + NaOH(aq) → NaCl(aq) + H₂O(l)
CO(g) + C(s) → CO₂(g)

Question 13

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Titanium occurs naturally as the mineral rutile, TiO₂. One possible method of extraction of titanium is to reduce the rutile by heating with carbon.

TiO₂(s) + 2C(s) → Ti(s) + 2CO(g)

The standard enthalpy changes of formation of TiO₂(s) and CO(g) are –890 kJ mol^-1 and –110.5 kJ mol^-1 respectively.

What is the standard enthalpy change of the extraction of titanium?

+ 669 kJ mol^–1
+ 779.5 kJ mol^–1
– 779.5 kJ mol^–1
– 669 kJ mol^–1

Question 14

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In the gas phase, phosphorus pentachloride can be thermally decomposed into gaseous phosphorus trichloride and chlorine.

PCl₅→ PCl₃+ Cl₂

The table below gives the relevant bond energies found in these compounds.

bond

bond energy / kJ mol^–1

P–Cl (in both chlorides)

Cl–Cl

$x$

$y$

What is the enthalpy change in the decomposition of the reaction?

$y - 2 x$
$2 x - y$
$8 x + y$
$x + y$

Question 15

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The standard enthalpy change, ΔH^Ө, for the following reaction is -246 kJ.

N₂(g) + 3F₂(g) → 2NF₃(g)

The bond energy of N≡N is 945 kJ mol^-1 and F–F is 159 kJ mol^-1

What is the bond energy of the N–F bond?

$\frac{246 - (945 + (3 \times 159))}{6}$
$\frac{- 246 + (945 + (3 \times 159))}{6}$
$\frac{246 + (945 + (3 \times 159))}{6}$
$246 + (945 + (3 \times 159))$

Question 16

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Question 17

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Question 18

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Question 19

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Some species may be classified as amphiprotic, some as amphoteric and some as both. Which of the following applies to HPO₄²⁻?

Amphiprotic but not amphoteric
Amphoteric but not amphiprotic
Amphiprotic and amphoteric
Neither amphiprotic nor amphoteric

Question 20

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Determine which of the following solutions would be basic at 25 °C?

K_w = 1.0 × 10⁻¹⁴mol² dm^-6

[H⁺] = 1.0 × 10⁻² mol dm⁻³
[OH⁻] = 1.0 × 10⁻¹² mol dm⁻³
solution of pH = 5.00
[H₃O⁺] = 1.0 × 10⁻¹² mol dm⁻³

Question 21

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Question 22

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Question 23

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Question 26

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Question 27

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Question 28

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Question 29

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Question 30

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DP IB Chemistry: SL

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