1. Define
the following terms:
| (a) Atomic
Number |
(c) Ion
|
| (b) Mass
Number |
(d) Polyatomic
Ion |
2. Complete
the following table of particles found in the atom.
|
particle
|
proton
|
neutron
|
electron
|
|
charge
|
|
|
|
|
where
found in the atom?
|
|
|
|
|
appreciable
mass in atom?
|
|
|
|
|
can
be lost to form + ions?
|
|
|
|
| can
be gained to form - ions? |
|
|
|
|
becomes
involved in chemical reactions?
|
|
|
|
3. The
atom is mostly made up of _________________________.
4. Complete
the following table.(You may need to use your Periodic
Table.)
Element |
Symbol |
Atomic
No. |
Mass
No. |
No.
of Protons |
No.
of Neutrons |
No.
of Electrons |
Electron
Configuration |
Charge
on common Ion |
| Helium |
He |
2 |
|
|
2 |
|
2 |
|
| Lithium |
|
3 |
7 |
|
|
|
2, 1 |
|
| |
C |
|
13 |
6 |
|
|
|
|
| |
|
|
16 |
8 |
|
|
|
|
| Nitrogen |
|
|
|
7 |
7 |
|
|
|
| |
Mg |
|
|
12 |
|
|
2, 8, 2 |
|
| Sulphur |
|
16 |
32 |
|
|
|
|
|
| Neon |
|
|
20 |
10 |
|
|
|
|
| Sodium |
|
11 |
23 |
|
|
|
|
|
5.
| (a) |
Draw a
diagram of an atom of Oxygen (O) [atomic number = 8, mass number
= 16] and draw a diagram of an atom of Sodium (Na)
[atomic number = 11, mass number = 23]. |
| (b) |
Draw diagrams
of the ions formed by both atoms and mark in the symbol and
charge on the ion. |
| (c) |
Predict
the formula of sodium oxide. ____________________. |
6. Complete
the following table.
|
Shell
Number
|
1
|
2
|
3
|
|
Max.
Number of electrons
|
|
|
|
7. State some properties of ionic compounds.
8. For
each of the following indicate if it represents an atom, ion or
polyatomic ion.
(a) H ___________________
(b) Pb2+ ___________________ (c) HSO4-
_________________
(d) Na+
_________________ (e) Mg ___________________ (f) OH-
___________________
Use
the table of ions at the back of your workbook to answer the following questions
9 and 10.
9. Name
the substances represented by the following formulae. (5 Marks)
|
Formula
|
Name
|
|
AgBr
|
|
|
ZnSO4
|
|
|
CuCO3
|
|
|
Na2S
|
|
|
Fe(OH)3
|
|
10.
Compare ionic and molecular compounds.
11. How does an ionic bond differ from a covalent bond?
12.
State some properties of molecular compounds.
13.Write
the formulae for the following ionic substances.
|
Name
|
Working
Column
|
Answer
|
|
Sodium
bromide
|
|
|
|
Magnesium
oxide
|
|
|
|
Iron
(III) carbonate
|
|
|
|
Silver
nitrate
|
|
|
|
Potassium
sulfate
|
|
|
|
Copper
nitrate
|
|
|
|
Magnesium
phosphate
|
|
|
|
Ammonium
sulfate
|
|
|
14.Define
the following terms (Use examples where possible).
| (a) |
Element |
(d) |
Chemical
change |
| (b) |
Compound |
(e) |
Law
of constant mass |
| (c) |
Physical
change |
(f) |
Catalyst |
15.
How can you perform a flame test? Explain why some
atoms emit coloured light when they are placed in a flame.
16.Complete
the following table
Formula |
Element
or Compound
|
Number
of atoms of each element
|
Total
number of atoms
|
|
CuCl2
|
|
|
|
|
Br2
|
|
|
|
|
Co
|
|
|
|
|
CO
|
|
|
|
|
(NH4)2SO4
|
|
|
|
17.Complete
the following table showing the ratio of ions in the ionic compounds
| Substance |
Formula |
Ions present |
Ratio of
Ions |
| Sodium
chloride |
NaCl |
|
|
| Calcium
nitrate |
Ca(NO3)2 |
|
|
| Copper
phosphate |
Cu3(PO4)2 |
|
|
| Aluminium
oxide |
Al2O3 |
|
|
18.For each of the following changes state whether they are physical
or chemical changes.
(a) An iron nail rusts.
(b) A piece of iron becomes magnetised.
(c) an ice block melts.
(d) wine turns to vinegar
(e) milk goes sour
(f) naphthalene flakes left in the cupboard "disappear"
but a strong smell of naphthalene is observed.
19. For
each of the following reactions identify the reactant(s) and product(s).
hydrogen + oxygen —›
water
copper carbonate —› copper
oxide + carbon dioxide
20.State
the factors that affect the rate of a reaction.
21.
4g of hydrogen reacts with 32g of oxygen to make water.
If water is the only product, what is the mass of the water produced?
22.Match
the following terms with their correct definitions.
|
A.
Atom
|
(a) Pure
substance containing atoms of only one type. (All atoms have
the same number of protons.)
|
|
B. Atomic
Number
|
(b)
Building blocks of all materials; contains a central nucleus
surrounded by an electron cloud.
|
|
C. Mass
Number
|
(c)
Pure substance containing atoms of two or more elements.
|
|
D. Ion
|
(d)
The number of protons in the nucleus of an atom.
|
|
E. Polyatomic
Ions
|
(e)
The number of protons and neutrons in the nucleus of an atom.
|
|
F. Element
|
(f)
A charged particle formed when an atom gains or loses electrons
in a chemical reaction.
|
|
G. Compound
|
(g)
A charged particle containing two or more different atoms.
|
|
H. Molecule
|
(h)
Smallest unit of a pure substance. Atoms are bonded together
by covalent bonds.
|
23. Complete
the following table:
|
Element
|
Symbol
|
Element
|
Symbol
|
|
Silver
|
|
Iron
|
|
|
Gold
|
|
Sulfur
|
|
|
Mercury
|
|
Sodium
|
|
|
Potassium
|
|
Calcium
|
|
|
Copper
|
|
Chlorine
|
|
24. Mass
number = number of _____________ + number of ________________
25. State
the elements present in each of the following compounds. State whether the compound is ionic or covalent.
(a) SO2 ______________________________________
(e) HCl _____________________________________
(c) CH4 ______________________________________
(d) H2SO4 ____________________________________
(e) Na2CO3 ___________________________________
26. Where are metals located on the Periodic Table? Non-metals?
27. Name
the following compounds and state how many ions each contain.
(a) Mg(OH)3 ________________________________
__________
(b) Fe2(SO4)3 ___________________________________
__________
(c) (NH4)2SO4
_________________________________ _________
28.
Write formulae for the following covalent molecular compounds.
| (a) |
boron
trichloride |
(f) |
nitrogen
dioxide |
| (b) |
carbon
tetrachloride |
(g) |
diphosphorous
pentoxide |
| (c) |
phosphorous
trichloride |
(h) |
hydrogen
bromide |
| (d) |
sulfur
trioxide |
(i) |
sodium
fluoride |
| (e) |
dinitrogen
tetroxide |
|
|
29. Balance
the following equations.
(a) N2 + H2
—› NH3
(b) Zn + HCl —›
ZnCl2 + H2
(c) P4 + H2
—› PH3
(d) NO + O2
—› N2O4
(e) Fe2O3
+ C —› Fe +
CO
(f) CH4 + Br2
—› CBr4 +
HBr
30. Complete
the following by identifying the unknown
silver +
sulfur -›
magnesium
+ oxygen -›
potassium
+ chlorine -›
copper sulfate
+ silver nitrate -› copper nitrate + silver _____________
sodium ____________
+ lead nitrate -› sodium nitrate + ____________chloride
31. Rewrite
the following word equations as balanced formula equations.
hydrochloric
acid + zinc -› zinc chloride + hydrogen
copper chloride
+ lead nitrate -› lead chloride + copper nitrate
sodium hydroxide
+ sulfuric acid -› sodium sulfate + water
sodium carbonate
+ calcium fluoride -› calcium carbonate + sodium fluoride
hydrochloric
acid + sodium carbonate -› sodium chloride + carbon dioxide
+ water
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