BONDING & STOICHIOMETRY QUIZ
1. An element D has atomic number 17, one type of atom of element D has a nucleon
number of 35 and the other, 37.
(a) Draw the electronic structure of an atom of D
[1]
(b) State with reason, the Group and Period number of element D in the periodic
table.
[2]
(c) State how element D forms an ion and why the ion is stable.
[2]
(d) (i) if element D reacted with magnesium, what type of bonding would be
formed?
[1]
(ii) Draw the structure of the compound formed between element D and
magnesium (show outer shell electrons only)
[2]
(e) What term is used to describe the different kinds of atoms of an element? [1]
(f) Would you expect this compound to dissolve in water? Give a reason for your
answer.
[2]
(g) Under what conditions would you expect this compound to conduct electricity?
[2]
2. An element has the electronic structure 2.8.4
a. Suggest the chemical formula of the compound which this element forms with
Chlorine. Draw a ‘cross and dot’ diagram of the structure of this compound.
b. Compare and contrast the boiling point and electrical conductivity of this
compound with those of sodium chloride.
3. The bar chart shows the period of elements from lithium to neon. Which property of
these elements is shown on the chart?
A.
B.
C.
D.
The number of electrons used in bonding
The number of orbits holding electrons
The nucleon (mass) number
The proton (atomic) number
4. The elements X and Y form the compound X2Y. What is the correct electronic
configuration of the atoms X and Y?
A
B
C
D
Electronic Configuration of
Atom of X
Atom of Y
2.1
2.7
2.2
2.7
2.1
2.6
2.2
2.6
5. What is the formula of the compound formed when element X of atomic number 12
combines with element Y of atomic number 17?
A. XY2
B. X2Y
C. XY
D. XY3
E. X3Y
6. Calculate the mass of calcium in 10g of calcium carbonate.
7. Copper metal is displaced from its solution when an iron nail is placed into a solution
of blue copper (II) sulphate. The clear solution which remains after the reaction is
complete is iron (II) sulphate.
Derive the ionic equation for this reaction.
8. 10.7g of a sample of rust, Fe2O3.XH2O, where X is a whole number was heated
strongly to remove the water and 8.0g of iron (III) oxide, Fe2O3 was obtained.
Determine the value of X in the formula of rust.
[3]
9. Copper (II) oxide is reduced by hydrogen gas to copper metal and water.
(a) Write a balanced equation with state symbols for this reaction.
[2]
3
(b) 160g of copper (II) oxide is reacted with 60dm of hydrogen measured at rtp.
(i) Show by means of calculation which reagent is in excess.
[4]
(ii) Calculate the mass of excess reagent.
[3]
(iii) Calculate the mass of copper produced
[2]
10. A spillage of 9.8 tons of sulphuric acid results from an accident by a road tanker.
Slaked lime is used to neutralize the acid.
(a) State the effect of the acid on the vegetation.
[1]
(b) The chemical equation for the neutralization is given below.
H2SO4(aq) + Ca(OH)2(s) CaSO4(s) + H2O(l)
(i) Balance the equation.
[1]
(ii) calculate the mass of slaked lime needed to neutralize 9.8 tons of spilt
sulphuric acid.
[2]
(iii) State one use of lime in agriculture
[1]
(c) Explain why sulphuric acid is said to be a strong acid.
11.
[1]