Ionic Bonding
1. Define and ionic bond. (1)
Name:_______________________
2. Define an ion. (1)
3. What types of atoms form ionic bonds. (1)
4. Draw an electron orbital diagram and write electron arrangement for a sodium atom (2).
5. Why does a sodium atom want to lose one electron. (1)
6. Draw an electron orbital diagram and electron arrangement of a sodium ion. (1)
7. Draw an electron orbital diagram and write electron arrangement for a chlorine atom (2).
8. Why does a chlorine atom want to gain one electron. (1)
9. Draw an electron orbital diagram and electron arrangement of a chloride ion. (1)
10. Using diagrams show what happens when a sodium atoms and chlorine atom combine. Name
the product formed and give its formula. (5)
11. Magnesium can react with nitrogen to form a new compound.
a) Write the electron arrangement of both magnesium and nitrogen. (2)
b) Draw an electron shell diagram to represent how magnesium and nitrogen atoms react to
form ions. Name the ions (3)
c) Explain how the ions form an ionic bond. (2)
d) State the formula of magnesium nitride. (1)
12. The compound formed between magnesium and oxygen is primarily (1)
A. ionic with a formula of MgO
B. ionic with a formula of MgO2
C. covalent with a formula of MgO
D. covalent with a formula of MgO
13. Identify which of the following elements will form ionic bonds (1)
A. Silver
B. hydrogen and oxygen
C. copper and sulphur
D. tin and copper
14. Element A is in group 1, and element B in group 7, of the periodic table. Which ions will
be present in the compound formed when A and B react together? (1)
A. A+ and B–
B. A 2+ and B–
C. A+ and B 2–
D. A 2– and B+
Ionic Formula
Name:_______________________
1. Distinguish between a monatomic and polyatomic ion. (2)
2. Using calcium chloride as an example, explain why its formula is CaCl2. (2)
3. Use aluminium sulphate as example explain the “cross over” rule for writing the formula for an
ionic compound. (2)
4. Using an ion chart write formula for each of the following compounds. (6)
a) potassium nitrate
b) calcium chloride
c) sodium hydroxide
d) copper (II) sulphate
e) ammonium sulphide
f) aluminium nitrate
g) Lithium fluoride
h) Lithium phosphate
i) Potassium sulphate
5. Using an ion chart state the names of the following compounds. (5)
a) KCl
b) BaSO4
c) Al2O3
d) FeI2
e) Cu3(PO4)2
6. Write the symbol formula for the positive ion for each of the following compounds. (6)
a) Mn(SO4)2
b) Co(OH)3
c) NiCO3
d) Pt(NO3)2
e) Na2CO3
f) Ca(HCO3)2
7. Using the ion chart make up your own compound. Give its name and formula. (2)
Covalent Bonding
Name:_______________________
1. Define a covalent bond. (2)
2. All chemical bonds involve electrostatic attraction. State the names of the particles between
which the electrostatic attraction occurs in a covalent bond. (1)
3. Using Lewis dot diagrams explain what happens when one oxygen atoms and two hydrogen
atoms combine to form water. (2)
4. Using Lewis dot diagrams explain what happens when two oxygen atoms combine. (2)
5. What happens when oxygen and chlorine combine together? (1)
A.
Each chlorine atom gains two electron.
B.
Each chlorine atom loses two electrons.
C.
Each oxygen atom shares two electrons.
D.
Each oxygen atom loses two electrons.
6. Identify the substances in the following list which can accurately be described as being
composed of covalent molecules. (1)
a) Carbon dioxide
b) Ice
c) Bronze
d) Potassium bromide
e) Hydrogen chloride
7. Draw Lewis structure (electron dot diagrams) for the following substances. (7)
a) N2
b) HBr
c) CH4
d) CO2
e) NH3
f) OHg) NH4+
8. State the number of bonding pairs of electrons and the number of non-bonding (lone) pairs of
electrons around the central atom in the molecules listed in question 7. (7)
Explaining the shapes of covalent molecules
1. State the valence shell repulsion theory (2)
Name:_______________________
2. What is the valence shell electron pair repulsion theory (VSEPR) used to predict? (1)
A. The energy levels in an atom
B. The shapes of molecules and ions
C. The electronegativities of elements
D. The type of bonding in compounds
3. According to VSEPR theory, repulsion between electron pairs in a valence shell decreases in
the order: (1)
A. lone pair-lone pair > lone pair-bond pair > bond pair-bond pair.
B. bond pair-bond pair > lone pair-bond pair > lone pair-lone pair.
C. lone pair-lone pair > bond pair-bond pair > bond pair-lone pair.
D. bond pair-bond pair > lone pair-lone pair > lone pair-bond pair.
4. Identify the four basic shapes of molecules. (4)
5. State the bond angles of each of the substances below. (4)
a) H2O
b) CO2
c) NH3
d) CH4
6. Using VSEPR theory explain why:
a) Water has a bent shape. (3)
b) Ammonia has a trigonal pyramid shape (3)
c) Methane has a tetrahedral shape (3)
7. Identify a molecule from the list below to match each description. You may use each molecule
from the list more than once. (6)
I. Carbon dioxide (CO2)
II.
chloromethane (CCl4)
III.
water (H2O)
IV. chlorine gas (Cl2)
V. ammonia (NH3)
a) Trigonal Pyramid
b) Four non-bonding pairs of electrons
c) Similar to a hydrogen sulphide, H2S molecule in shape
d) Contains double bonds
e) Tetrahedral
f) Linear
Electronegativity and Polarity
1. Define electronegativity (2)
Name:_______________________
2. Explain the trend in electronegativity down a group and across a period (2)
3. Using a table of electronegativity values, identify
I.
which element in the pair below is the most electronegative. Identify with a slight
– or +. (3)
II.
the compound made by each pair as either covalent or ionic (3)
a) sodium and sulphur
b) sulfur and oxygen
c) lead and oxygen
4. Identify, with a reason which metal fluoride is the most ionic? (2)
A. NaF
B. CsF
C. MgF2
D. BaF2
5. Which of the following pairs of atoms would have the greatest difference in electronegativities
and hence would be the most polar? (1)
a) Fluorine and hydrogen
b) Chlorine and hydrogen
c) Nitrogen and hydrogen
d) Oxygen and hydrogen
6. Copy and complete the table below (12)
Name of covalent
molecule
Carbon dioxide
(CO2)
methane (CH4)
Water (H2O)
Structural
Formula
Are bonds polar?
Overall net force
Yes/No
Is the molecule
polar or non-polar
Intra and Intermolecular Forces
Name:_______________________
1. Define a covalent bond (2)
2. Distinguish between a inter and intramolecular force (bond) (2)
3. Name the three types of intermolecular forces. (2)
4. Define the term electronegativity (2)
5. Draw a diagram to show the intramolecular covalent and intermolecular hydrogen bonds
between two water molecules. (3)
6. Using labelled diagrams distinguish between polar and non-polar molecules using HCl and Cl2 as
examples. (4)
7. For each of the following molecules, identify the type of intermolecular bonding (van der
Waals’ forces, permanent dipole–dipole attractions, hydrogen bonding) present. (5)
a) HCl
b) NH3
c) H2O
d) SiH4
e) N2
8. When the following bond types are listed in decreasing order of strength (strongest first), what
is the correct order? (1)
A. covalent > hydrogen > van der Waals’
B. covalent > van der Waals’ hydrogen
C. hydrogen . covalent > van der Waals’
D. van der Waals’ > hydrogen > covalent
9. Which type of intermolecular forces exist in dry ice, CO2 (s) (0=C=0)? (1)
A. Covalent bonds
B. Dipole-dipole attractions
C. Van der Waals’ forces
D. Hydrogen bonds
10. List the following bonds in order from weakest to strongest. (1)
a) Permanent dipole–dipole bonds between SO2 molecules
b) Covalent bonds between carbon and hydrogen in CH4
c) Van der Waals’ forces between atoms of helium
d) Permanent dipole–dipole bonds between HF molecules
e) Covalent bonds between nitrogen atoms in N2 molecules
f) Van der Waals’ forces between molecules of carbon dioxide, CO2
Lattice Structures
Name:_______________________
1. Describe with the help of a labelled diagram model the unit cell lattice structure of sodium
chloride. (2)
2. State two physical properties of calcium chloride. (2)
3. State the particles that are responsible for the conduction of electricity in a metal and ionic
compound. (2)
4. Explain why calcium chloride conducts electricity when it is in its liquid or molten form but not
when it is a solid. (2)
5. Draw a labelled diagram to show the model of a metal like potassium. (2)
6. The bonding in a metal is often referred to as the ‘electron sea’ model. Describe what is meant
by the terms: (2)
a) delocalised electrons
b) lattice of positive ions
7. Which is a correct description of metallic bonding? (1)
A. positively charged metal ions are attracted to negatively charged ions
B. negatively charged metal ions are attracted to positively charged metal ions
C. positively charged metal ions are attracted to delocalized electrons
D. negatively charged metal ions are attracted to delocalized electrons
8. What are responsible for the high electrical conductivity of metals? (1)
A. delocalized positive ions
B. delocalized valence electrons
C. delocalized atoms
D. delocalized negative ions
9. Describe what each of the following properties suggests about the nature of the bonding in
metals? (2)
a) Metals conduct electricity.
b) Most metals have high melting points.
Organic Chemistry
Name:_______________________
1. State two characteristics of a homologous series.
2. Give the molecular formula and draw structural formulas of each of the following molecules.
a) Butane
b) Ethanol
c) The carboxylic acid with 6 carbon atoms
d) The alkene with 8 hydrogen atoms
e) The ketone with 3 carbon atoms
3. Classify each of the following as alkanes or alkenes.
a) C12H24
b) C16H32
c) C15H32
d) C72H146
4. Draw structural formulas for the structural isomers of
a) pentane
b) pentene
c) pentanol
d) pentanoic acid
5. Name the hydrocarbon molecules whose formulas are given below.
a) CH3CHCHCH3
b) CH3(CH2)2CH2OH
c) CH3(CH2)3CH3