MYP 10 Chemistry 2012-13
Bonding Worksheet
Name: _________________________________ ( )
Class: _________ Date: _____________
_________________________________________________________________________________
1. Describe the variation in melting points and electrical conductivities of the elements sodium to argon,
and expain these variations in terms of their structures and bonding.
2(a) Draw electron dot structures for N2 and F2 and explain why F2 is much more reactive than N2.
(b) Compare the polarity of the bonds N-F and C-F. Are the molecules NF3 and CF4 polar or non-polar?
In all your answers give your reasons.
[SL paper 2, May 99]
3. Explain at the molecular level why ethanol (C2H5OH) is soluble in water, but cholesterol (C27H45OH)
and ethane (C2H6) are not.
[SL paper 2, May 01]
4. The elements potassium and fluorine and the compound potassium fluoride can be used to show the
connection between bonding structure and physical properties.
(a) Describe the type of bonding in potassium metal and explain why potassium is a good conductor of
electricity.
(b) Draw a Lewis structure for fluorine. Name and describe the bonding within and between the
molecules in liquid fluorine.
(c) Write the electronic structures of both potassum and fluorine and describe how the atoms combine to
form potassium fluoride.
(d) Explain why potassium fluoride does not conduct electricity until it is heated above its melting point.
5(a) The letters A, B, C and D represent four consecutive elements in the periodic table. The number of
electrons in the highest occupied energy levels are
A: 3
B: 4
C: 5
D: 6
Write the formula for
(i)
An ionic compound that form between A and C, showing the charges.
(ii)
A covalent compound containing B and D.
(b) State the number of protons, neutrons and electrons in the ion 126𝐶 606-.
(c) State the type of bonding in the compound SiF4. Draw the Lewis structure for this compound.
(d) Outline the principles of the valence shell electron pair repulsion (VSEPR) theory.
(e)(i) Use the VSEPR theory to predict and explain the shape and bond angle of each of the molecules
SBR2 and C2Br2.
(ii) Deduce whether or not each molecule is polar, giving a reason for your answer.
6(a)(i) Use the VSEPR theory to deduce the shape of H3O+ and C2H4. For each species, draw the Lewis
structure, name the shape and state the value of the bond angle(s).
(ii) Predict and explain whether each species is polar.
(iii) Using Table 7 of the Data Booklet, predict and explain which of the bonds O-H, O-N or N-H would
be most polar.
(b) Predict and and explain which of the following compounds consist of molecules:
NaCl, BF3, CaCl2, N2O, P4O6, FeS and CBr4
(c) Diamond, graphite and C60 fullerene are three allotropes of carbon.
(i) Describe the structure of each allotrope.
(ii) Compare the bonding in diamond and graphite.