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
No comments:
Post a Comment