Year 10 - Chemistry Revision
1) Name the following compounds:
(a) PBr3
(b) CBr4
(c) Na2SO4
(d) Cu(NO2)2
(e) CaCl2
(f) Fe2O3
(g) P2O5
(h) N2O3
(i) P3O6
(j) Mg3(PO4)2
(k) IF5
(l) Li2O
(m) CuS
(n) CrPO4
(o) K3N
(p) Fe2(CO3)3
(q) (NH4)3PO4
(r) SnS
(s) NaHSO3
(t) NaC2H3O2 (u) SnS2
(x) PbCl2
(y) Ag3PO4
(z) Ca(CN)2
(v) N2S3
(w) B4H10
2) Write the formula for the following compounds.
(a) Potassium chloride
(b) Calcium nitrate
(c) Silicon tetrachloride
(d) Diphosphorus pentoxide (e) Lead (IV) sulfide (f) Dihydrogen sulfide
(g) Carbon Tetrabromide
(k) Barium oxide
(h) copper (I) sulfide (i) Tin (II) chloride (j) Dinitrogen Trihydride
(l) Aluminium sulfide (m) Zinc (II) phosphide
(n) Iron (II) oxide
(o) Potassium permanganate (p) Hydrogen Peroxide
(q) Potassium dichromate
(r) Tin (II) perchlorate
(t) Titanium (IV) chloride
(s) Diboron hexahydride
3) Write word equations and then balanced formula for the following reactions:
(a)
(b)
(c)
(d)
(e)
(f)
(g)
(h)
(i)
(j)
(k)
(l)
Magnesium burns in the presence of oxygen to produce magnesium oxide.
Aluminium metal reacts with chlorine gas to produce Aluminium chloride.
Electrolysis can be used to split water into hydrogen and oxygen.
Nitrogen dioxide gas dissolves in water to produce nitric acid (HNO3) and nitrogen monoxide.
A solution of lead (II) nitrate is mixed with sodium phosphate to produce sodium nitrate and a
precipitate of lead (II) phosphate.
Sodium metal ignites in the presence of chlorine gas to produce sodium chloride.
Mercury (II) oxide decomposes into mercury and oxygen.
Aluminium metal is displaced by copper (II) sulfate solution producing copper metal and aluminium
sulfate.
Gallium is heated in the presence of oxygen gas to produce gallium (III) oxide.
Aluminium sulfate reacts with sodium hydroxide to produce an aluminium hydroxide precipitate and
sodium sulfate.
Nitrogen triiodine explodes to produce nitrogen gas and iodine gas.
Potassium permanganate reacts violently with hydrogen peroxide to produce potassium peroxide,
manganese (IV) oxide, water and oxygen gas.
4) Determine what type of reaction each reaction is in question 3 (exclude d and l).
5) Determine the number of electrons, proton and neutrons in each of the following.
(a) C
(b) S
(c) Fe
(d) Na
(e) Be2+
(h) O
(i) I-
(j) Mg2+
(k) Na+
(l) S2-
(g) Ca2+
(f) Ca
6) What is an isotope?
7)
(a) Distinguish between ionic, covalent and metallic bonding.
(b) The following table shows the properties of ionic, covalent and metallic substances.
Property
Ionic
Covalent
Metallic
Melting and Boiling Point
High
Low
High
Malleability
Brittle
Soft
Soft
Conductivity
None as solid
None
High
High in solution
(i)
(ii)
(iii)
(iv)
Why metals are able to conduct electricity?
Explain why metals are malleable and ductile.
Explain why ionic compounds can only conduct electricity when dissolved in
solution.
*Challenge* Explain why ionic compounds are brittle.
8) Why noble gases are said to be inert (stable)?
9)
(a) What is the difference between an endothermic and an exothermic reaction?
(b) *Challenge* Is the breaking of chemical bonds an endothermic or an exothermic process? What
about the formation of new bonds?
10) Distinguish between elements, compounds and mixtures.
11) On the periodic table:
a) Label the group numbers.
b) Shade the transition metals
blue.
c) Shade the metalloids green.
d) Shade
yellow.
the
non-metals
e) Identify the valency of each
group.
Answers
1) (a) Phosphorous tribromide (b) carbon tetrabromide
(c) sodium sulfate
(d) copper (I) nitrite (e) calcium chloride (f) iron (III) oxide
(g) diphosphorous pentaoxide
(h) dinitrogen trioxide
(i) triphosphorous hexaoxide (j) magnesium phosphate
(k) iodine pentafluoride
(l) lithium oxide
(m) copper (II) sulfide
(n) chromium phosphate
(o) potassium nitride (p) iron (III) carbonate
(q) ammonium phosphate
(r) tin (II) sulfide
(s) sodium hydrogen sulfite
(t) sodium acetate
(u) tin (IV) sulfide
(v) dinitrogen trisulfide
(w) tetraboron decahydride
(x) lead (II) chloride (y) silver (I) phosphate
(z) calcium cyanide
2) (a) KCl
(b) Ca(NO3)2
(c) SiCl4
(d) P2O5
(e) PbS2
(f) H2S
(g) CB4
(h) Cu2S
(i) SnCl2
(j) N2H3
(k) BaO
(l) Al2S3
(p) H2O2
(q) K2Cr2O7
(r) Sn(ClO4)2 (s) B2H6
(m) Zn3(PO3)2
(o) KMnO4
(t) TiCl4
3)
a) Magnesium + oxygen magnesium oxide
2Mg
+ O2 2MgO
b) Aluminium + chlorine Aluminium chloride
2Al
+
3Cl2
2AlCl3
c) water hydrogen + oxygen
2 H2 O 2H2
+
O2
d) nitrogen dioxide + water nitric acid + nitrogen monoxide
3NO2 +
H2 O
2HNO3
+
NO
e) lead (II) nitrate + sodium phosphate sodium nitrate + lead (II) phosphate
3Pb(NO3)2
+
2Na3PO4
f) sodium + chlorine sodium chloride
2Na + Cl2
2NaCl
g) Mercury (II) oxide mercury + oxygen
2HgO
2Hg + O2
6NaNO3
+
Pb3(PO4)2
h) Aluminium + copper (II) sulfate copper + aluminium sulfate
2Al
+
3Cu +
3CuSO4
Al2(SO4)3
i) Gallium + oxygen gallium (II) oxide
2Ga + O2
2GaO
j) Aluminium sulfate + sodium hydroxide Aluminium hydroxide + sodium sulfate
Al2(SO4)3
+
6NaOH
2Al(OH)3
+
3Na2SO4
k) nitrogen triiodide nitrogen + iodine
2NI3
N2
+
3I2
l) Potassium permanganate + hydrogen peroxide potassium peroxide + manganese (IV) oxide + water + oxygen
2KMnO4
+
2H2O2
K2 O2
+
2MnO2
4) a) combination
b) combination
c) decomposition
f) combination
g) decomposition
h) single replacement i) combination
j) double replacement (k) decomposition
+ 2H2O + 2O2
e) double replacement