IB Chemistry Jeopardy SL

topic 1

100

This is the sum of all coefficients for the combustion of one mole of propane?

___ C₃H₈ + ___ O₂ → ___ CO₂ + ___ H₂O

What is 13

200

This is the sum of the coefficients when the equation is balanced with the smallest whole numbers?

__BaCl₂ (aq) + __Fe₂(SO4)₃ (aq) → __FeCl₃ (aq) + __BaSO₄ (s)

What is 9

300

4.00 mol of a hydrocarbon with an empirical formula of CH₂ has a mass of 280 g. This is the molecular formula of this compound.

What is C₅H₁₀

400

A compound with M_r = 102 contains 58.8 % carbon, 9.80 % hydrogen and 31 % oxygen by mass. This is its molecular formula.

A_r: C = 12.0; H = 1.0; O = 16.0 

C₅H₁₀O₂

500

This many moles of oxygen atoms are there in 0.500 mol of hydrated iron(II) ammonium sulfate, (NH₄)₂Fe(SO₄)₂•6H₂O

What is 7.00

topic 2

100

These subatomic particles are located in the nucleus of an atom

protons and neutrons

200

This is the composition of the nucleus of ²⁶Mg in terms of protons, neutrons and electrons.

12 protons, 14 neutrons, 0 electrons

300

The full electron configuration of an element is: 1s²2s²2p⁶3s²3p². It belongs to this group and period.

group 14, period 3

400

What is the condensed electron configuration of the Fe²⁺ ion?

[Ar]3d⁶

500

A sample of zinc has the following composition: 

⁶⁴Zn = 55% abundance, ⁶⁶Zn = 40% abundance, 

⁶⁸Zn = 5% abundance 

This is the relative atomic mass of the zinc in this sample.

What is 65.0

topic 3

100

This oxide, when added to water, produces the solution with the highest pH.

 SO₃  or  MgO  or Na₂O or  CO₂

What is Na₂O

200

This element is in the p-block:

Pb or Pm or Pt or Pu

What is Pb

300

This pair of elements shows the greatest difference in electronegativity:

Mg and O 

Li and F 

K and F

Li and I

What is K and F

400

This series represents atoms in order of decreasing atomic radius:

N > C > Be > Mg

Mg > N > C > Be

Mg > N > C > Be

Mg > N > C > Be

What is Mg > N > C > Be

500

This series is arranged in order of increasing radius:

F < Cl^- < Cl 

Rb < K < Na 

Al³⁺ < Mg²⁺ < Na⁺

 I^- < Br^- < Cl^-

What is Al³⁺ < Mg²⁺ < Na⁺ 

topic 4

100

These particles are responsible for electrical conductivity in metals.

What are electrons.

200

This compound contains both ionic and covalent bonds:

A.  SiH₄

B. NaNO₃

C. H₂CO

D. Na₂S

What is B. NaNO₃

300

Which bonds are arranged in order of increasing polarity? 

A. H–F < H–Cl < H–Br < H–I 

B. H–I < H–Br < H–F  < H–Cl 

C. H–I < H–Br < H–Cl < H–F

D. H–Br < H–I < H–Cl < H–F 

What is C. H–I < H–Br < H–Cl < H–F

400

This compound has the highest boiling point:

A.  CH₃CH₃

B.  CH₃OH

C.  CH₃CH₂OH

D.  CH₃CH₂CH₃

What is C.  CH₃CH₂OH

500

This molecule has a non-bonding (lone) pair of electrons on the central atom:

A.  BF₃

B.  SO₂

C.  CO₂

D.  SiF₄

B.  SO₂

topic 5

100

This is the energy released when one mole of a substance is burned in excess oxygen, under standard conditions.

What is the standard enthalpy of combustion.

200

This statement about bonding is correct:

A. Bond breaking is endothermic and requires energy

B. Bond breaking is endothermic and releases energy

C. Bond making is exothermic and requires energy

D. Bond making is endothermic and releases energy

What is A. Bond breaking is endothermic and requires energy

300

This is the energy change when one mole of a compound is formed from its elements in their standard states under standard conditions.

What is standard enthalpy of formation.

400

A student heated a calorimeter containing 100 cm3 of water with a spirit lamp and collected the following data:

Initial temperature of water: 20^oC

Final temperature of water: 55.0^oC

Mass of ethanol burned: 1.78 g

Density of water: 1.00 g cm^-3

This is the heat evolved when the ethanol was combusted, in kJ.

What is 14.6 kJ

500

Consider the following reactions:

Cu₂O (s) + 0.5O₂ (g) --> 2CuO (s)   delta H = -144 kJ

Cu₂O (s) --> Cu (s) + CuO (s) delta H = +11 kJ

This is the value of delta H for the reaction 

Cu(s) + 0.5O₂ (g) --> CuO (s)

What is -155 kJ