SECTION A (30 POINTS)
Fill in the gaps with the relevant terms. Each answer is 1 point.
1. Faraday discovered__________________, a type of radiation emitted by the negative
terminal cathode that crossed the evacuated tube to the positive terminal or
____________
2. In 1895, Wilhelm Roentgen discovered _____________ , a type of electromagnetic
radiation in the invisible region and which he called so because of its unknown nature.
3. ____________________ is the spontaneous emission of energy from unstable atoms.
4. ________________________are negatively charged particles produced by changes
occuring within the nuclei of radioactive atoms and have the same properties as
electrons.
5. Most of the mass and all of the positive charge of an atom are centered in a very small
region called the __________________
6. Two or more atoms having the same atomic number (Z) but different mass numbers
(A) are called ____________________
7. _______________________________ quantum number determines the geometrical
shape of the electron probability distribution.
8. The element or ions which have the same number of electrons are called
____________________
9. __________________________, is a measure of the energy change that occurs when a
gaseous atom gains an electron .
10. The oxides of metals have _____________ character, but the oxides of nonmetals
have ____________ character.
11. _______________________________ are d block and f block elements of the
periodic table.
12. The group IA elements are called ______________________. Each of them has
_________ electron in their outermost s orbital. They are the group having the
smallest _________________________________ among the other groups of
elements in the periodic table.
13. _____________________________ are composed of two or more different elements
14. As a result of the electron transfer, the metal atom becomes a positive ion and is
a_______________. And the nonmetal atom becomes a negative ion and is called an
______________.
15. Liquid pressure depends only on the ______________ of the liquid column and the
________________ of the liquid.
16. The density of a gas is directly proportional to its ___________________.
17. The migration of molecules of different substances as a result of random molecular
motion is called __________________
18. At very high pressures and low temperatures gases tend to behave as
________________, which can be explained with the concept
_________________________________(PV/nRT > 1)
19. If there is no possible transfer of energy and matter between the system and its
surroundings, the system is called ________________
20. Heat transfer between the system and its surroundings occurs as a result of
_________________ difference.
21. The quantity of heat required to change the temperature of a system by one degree is
called ________________________(mass x specific heat)
22. In thermodynamics _____________ means the transfer of energy between the system
and its surroundings due to an external macroscopic force.
23. The device used to measure the pressure of a gas in a closed vessel is called
___________________
SECTION B ( 18 POINTS)
In this section you are responsible for answering 9 multiple choice questions. For each
question there is only one right answer. Each question is 2 points.
The ion X3+ has the electron configuration: 1 s2 2 s2 2 p6 3 s2 3 p6 4 s2 3 d10 4 p6
1. The element is in the gruop
a) IA
b) IIB
c) III B
d) IVA
e) VIIIA
2. It forms with Oxygen(O) the following compound
a) XO
b) X2O3
c) X3O2
d) XO3
e) X2O
3.Its neutron number is
a) 48
b) 41
c) 50
d) 89
e) 84
The ion X2- has the electron configuration: 1 s2 2 s2 2 p6 3 s2 3 p6 4 s2 3 d10 4 p6 5s2 4d10 5 p6
4. The element is in the gruop
a)II A
b)IV B
c)VI A
d)VI B
e) VIIIA
5. It has the oxidation state(O.S) in the compound XF6
a) +6
b) -2
c) +4
d) -4
e) +1
6.Which of the statements is correct?
a)
b)
c)
d)
e)
The element makes ionic bonds with halogenes
It is a transition element
Its ionization energy is greater than Iodine
The atomic radius of the element is greater than that of its ion X2The element X is paramagnetic
Given the spdf notation of the element Z as follows:
1 s2 2 s2 2 p6 3 s2 3 p6 4 s1 3 d10
7. The total number of electrons having magnetic quantum number ml > +1
a) 4
b)2
c) 6
d)1
e)10
8.The total number of electrons having angular momentum quantum number l = 1
a) 0
b) 9
c) 1
d)10
e)12
9. The total number of electrons having principal quantum number n<=2
a) 29
b)10
c)8
d) 19
e)16
SECTION C (52 POINTS)
1. Given the ions:
O2-, Ne, Na+, F-, Mg2+, Al3+
a)Arrange the ions in the increasing order of atomic radius (4 points)
b)Which of them has the highest negative electron affinity? (1 point)
c)Which of them has the lowest first ionization energy? (1 point)
d)Which of the elements (O, Ne, Na, F, Mg, Al) is/are diamagnetic (2 points).
2. Complete the table with the correct numbers ( 4 points)
Z
A
Proton
Neutron
Electron
W
74
184
74
+
Cs
133
55
Cu2+
63
34
3. Calculate the O.S of the elements underlined in the given compound (6 points)
a) B2Cl4
b)UO2+
c) W2Cl93d) N2H4
e) H3PO4
f) FeO42-
4. Write the chemical formula of the following compounds (4 points)
a) Sulphurhexafluoride(1 point)
b) Copper(II)chromate(1 point)
c) Hypochlorousacid (1 point)
d) Dinitrogentetroxide (1 point)
5. Name the compounds given below (6 points)
a) Au2S
b) Fe2(SO4)3
c) P2O5
6. Calculate the mole content and the total number of atoms of CCl4 which has a mass
of 50 g. (C=12 ; Cl=35,5) (4 points)
7. If a hydrocarbon mixture is burnt with oxygen, 5,28 g of CO2 and 2,7 g of H2O are
produced (C=12 ; O=16 ; H=1)
Write the chemical reaction
a) Determine the empirical formula of the mixture ( 2 points)
b) What is the mass of the sample burnt? (2 points)
c) How much O2 in grams is consumed? (2 points)
8. A gas mixture is composed of N2 and C2H6. The partial pressure of N2 is 0,3 atm and
the partial pressure of C2H6 is 0,45 atm.
What is the weight of C2H6 in grams, if the mixture occupies a volume of 20,4 L at
100˚C (C=12 ; H=1) (6 points)
9. The following reaction is given:
3 Fe (s) + 4 H2O (g)
Fe3O4(s) + 4 H2 (g)
a)How many grams of iron(Fe) are required to form 100 L of H2 at 0˚C and 1
atm(STP)? (Fe= 55,8 g/mol) (4 points)
b) Determine the density of H2 (g) at 25˚C and 0,2 atm (H=1)(R=0,082 atmL/molK)
(4 points)