Preparation AMS and homework week 4 Term 2 Level L 2020



1.    Write the electronic configuration of chromium, atomic number 24.

2.    Write the electronic configuration of the fluoride ion. The Atomic number of F is 9.


3.    Write the electronic configuration of the calcium ion. The Atomic number of Ca is 20.

4.     What is special about the electronic configurations of the noble (inert) gases?


5.    Complete the following sentence: With the exception of helium, the electronic configurations of the noble gases end with ns? np?.

6.    Is this, the electronic configuration of a noble gas: 1s2 2s2 2p6 3s2 3p5?


7.    Fill in the blanks regarding s orbitals:
·       They are _________ in shape
·       They are present in _________ energy levels
·       The probability of finding an electron _________ as the distance from the nucleus increases.
·       In higher energy levels, the s orbital becomes _________ .
·       S orbital encompasses _________ % of the probability of finding the electron in the orbital.


8.    Fill in the blanks regarding d orbitals:
·       They exist in sets of _________
·       They are present in _________
·       Each shell having _________ , has only _________ set of _________ d-orbitals


9.    Fill in the blanks regarding p orbitals:
·       They exist in one set of _________ .
·       They are _________ shaped.
·       p orbitals in a specific energy level can accommodate a maximum of _________ electrons.
·       They are located along the _________
·       p orbitals are found in all energy level _________


10. Fill in the blanks regarding f orbitals:
·       They exist in sets of _________
·       They are present in _________
·       Each shell having _________ , has only _________ set of _________ f-orbitals


11.What is the maximum number of orbitals that may be found in the fifth shell?


12.What is the maximum number of electrons that may be found in the fifth shell?

13. What is the wavelength of an electromagnetic wave with a frequency of 6.00 × 1012 /s? c = 3.0 × 108 m/s

14. What is the energy of a photon of light whose wavelength is
6.0 × 10-7m?         h= 6.6 ×10 -34J.s?



15. What volume of 2.0 M H2SO4 contains 40 mmol of acid?


16. The oxidizing agent in the reaction:

Cu + H2SO4 → CuSO4 + H2O + SO2

17. Why is chemical equilibrium referred to as “dynamic”?

18. What is the effect on the equilibrium concentrations of the reactants and products when each of the
following systems is compressed?
a. H2(g) + Cl2(g) 2HCl(g)
b. 2H2(g) + O2 (g) →2H2O(g)
c. 2NH3(g) →3H2(g) + N2(g)
d. C(s) + ½ O2(g) →CO(g)



19. 0.20 moles of HI are injected into a rigid 200 cm3 container at 490oC and the following equilibrium was established:
2HI(g) H2(g) + I2(g) Keq = 0.020 at 490℃
Calculate the equilibrium concentration of each species when the system reaches equilibrium.

20. Give the name of the most suitable technique you can use in order to obtain crystals of potassium nitrate from its aqueous solution.

21. List the observation upon adding a few milliliters of silver nitrate solution to the following potassium
halide solutions. Identify the precipitate if any.
a) KF
b) KCl
c) KBr
d) KI


22. Which of the following equation is an oxidation reaction?
a. CuCO3 → CuO + CO2
b. ZnO + 2HCl → ZnCl2 + H2O
c. 2Cu + O2 → 2CuO
d. Na2CO3 + 2HCl → 2NaCl +H2O + CO2


23. A zinc rod is placed in a 1.0 M zinc nitrate solution. A copper strip is placed in a 1.0 M copper nitrate solution. The two half-cells are connected by a salt bridge and, externally, by a voltmeter. The voltmeter
reads 1.10V, and it shows that copper is the positive terminal of the cell.
a) In what direction does the current pass in the outside circuit (the voltmeter)?
b) In what direction do electrons pass in the outside circuit (the voltmeter)?
c) Which electrode is the cathode?
d) Write the equation of the net reaction that takes place at the cathode.
e) Which electrode is the anode?
f) Write the equation of the half-reaction that takes place at the anode
g) In what direction does the current pass in the solution?
h) Write the overall equation for the reaction taking place.
i) How much energy is released by the cell when 2.0 C pass by any point in the circuit?


24. What is the maximum number of orbitals and electrons that can be found in the second shell?

25. Write the electronic configuration of the following atoms: Na, P, K, Sc, Cr, Cu

26. Write the electronic configurations of the following ions: O–2, Na+, Mg+2, N–3, Fe+2, Cu+2

27. Use the Periodic Table to help write the formula of the following compounds or ions.
Barium Oxide                                           Aluminium nitride
Boron oxide                                              Aluminium ion
Aluminium fluoride                                 Sulphide ion
Sodium sulfide                                          Nitride ion
Calcium nitride                                         Phosphide ion
Potassium oxide                                       Chloride ion
Barium chloride                                        Calcium ion


28. Element X has a high tendency to form unipositive ions, while element Y has a high tendency to form doubly charged positive ions in their respective compounds. Which of the following electronic
configurations is for X and which is for Y:
1s2 2s2 2p6 3s2 1s2 2s2 2p6 3s1?

29. Element A forms a compound with potassium of formula K2A. Which of the following electronic
configurations is for A: 1s2 2s2 2p6 3s2 3p2 or 1s2 2s2 2p6 3s2 3p4?

30. What is the maximum number of orbitals and electrons that can be found in the fourth shell?


31. Starting from which shell may the following orbitals be present?
a. The s orbital
b. The p orbital
c. The d orbital
d. The f orbital

32. What is the maximum number of electrons that can be present in the following orbitals?
i. 3px
ii. all the 3d orbitals
iii. all the 5f orbitals
iv. 5s
v. all the 2f





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