Question

1. Explain the following properties of ionic structures using structure and bonding.
(a) the particles in a solid usually form a regular lattice. Explain what that means in your own words.
(b) Which type of particles make up the lattice in an ionic compound?
(c) Solid sodium chloride will not conduct electricity, but a solution of sodium chloride will conduct. Explain this?
(d) A compound melts at 2500*C.
(i) What kind of structure do you think it has?
(ii) why do you think so?
(iii) Will it conduct electricity at 30000 C?
Give a reason?
2. Explain why calcium ion has a charge of +2?
Why is the charge on aluminium ion + 3?
Aluminium and nitrogen react to form an ionic compound called aluminium nitride.
(a) Answer these questions for an aluminium atom.
i) Does it gain or lose electrons, to form an ion? ---------------------------------------------------------------------------------------------
ii) How many electrons are transferred? -----------------------------------------
iii) Is the ion formed positive or negative? --------------------------------------------------
iv) What charge does the ion have? --------------------------------------------
b) Now repeat (a) but for the nitrogen atom
i)-----------------------------------
ii)-------------------------------------
iii)---------------------------------------
iv)-------------------------------------------
(c)
i) Give the electron distribution for the ions formed by the two atoms. aluminium ion ----------------------------------- nitrogen ion
ii) What do you notice about these electronic configurations or distributions.? Explain
d) Name another non-metal that will form an ionic compound with aluminium, in the same way as nitrogen does.

4. Draw a dot and cross diagram of sodium nitride. ( Na = 11, N = 7 )
b) The sodium nitride is an ionic bond with a giant ionic structure. List four of its properties
c) Name four other compounds of nitrogen that will have a similar structure.

Answer 1

Answer:

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