Ionization Enthalpy
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The general electronic configuration of p-block elements is______.
- Boron and silicon.
- Boron and aluminium.
- Boron and gallium.
- Boron and carbon.
- Boron
- Beryllium
- Magnesium
- Silicon
The element sulphur has atomic number 16 and mass number 32. Calculate the number of electrons, protons, and neutrons in the ion formed. Represent the ion. What will be its vaÂlency?
Within each pair of elements, respectively, the elements that release more energy upon an electron gain are:
Name the noble gas with 3 shells.
IIIIE1400589IE225101120
Elements I and II respectively are likely to be?
- Non-metal, alkali metal
- Alkali metal, alkaline earth metal
- Alkaline earth metal, non metal
- Alkaline earth metal, alkali metal
- F < S < P < B
- P < S < B < F
- B < P < S < F
- B < S < P < F
- False
- True
Consider the following table:
Element | Atomic no. | No. of neutrons |
---|---|---|
A | 3 | 4 |
B | 9 | 10 |
C | 13 | 14 |
D | 17 | 18 |
E | 18 | 22 |
(i) How many protons are there in an atom of D?
(ii) What is the mass number of B?
(iii) Write electron distribution of C.
(iv) What is the valency of E?
(v) What is the number of electrons present in a monovalent positive cation of A and a monovalent anion of D?
- Fluorine
- Sulphur
- Iron
- Beryllium
S1:Na2O2<MgO<ZnO<P4O10: Acidic property.
S2:Na<Mg>Al<Si: First ionisation energy.
S3:F>Cl>Br: Electron affinity.
- TTT
- TFF
- TTF
- TFT
- Na
- K
- Mg
- Ca
Why is it not possible to form ion? Explain with respect to periodic properties.
The smallest ion among the following is:
- Cr2+
- Mn3+
- Mo2+
- Tc3+
Mg→Mg2++2e− is:
- +170 K cal mol−1
- +526 K cal mol−1
- −170 K cal mol−1
- −526 K cal mol−1
On moving across a period, the atomic size decreases and nuclear charge increases and therefore the force of attraction exerted by the nucleus on the electron in the outermost shell increases.
Potassium forms K+ ion but it does not form K2+ because of;
Very low value of (I.E.)1 and (I.E.)2
Very high value of (I.E.)1 and (I.E.)2
Low value of (I.E.)1 and low value of (I.E.)2
Low value of (I.E.)1 and high value of (I.E.)2
Ionization energy is directly proportional to the atomic radius and the effective nuclear charge. (True/False)
True
False
- I.E2(N)>I.E2(O)
- I.E2(O)>I.E2(N)
- I.E1(O)<I.E1(N)
- I.E2(Li)>I.E2(Be)
- The first ionisation potential of Al is less than the first ionisation potential of Mg.
- The second ionisation potential of Mg is greater than the second ionisation potential of Na.
- The first ionisation potential of Na is less than the first ionisation potential of Mg.
- The third ionisation potential of Mg is greater than third ionisation potential of Na.
What is the ionization energy of Magnesium?
- lanthanide contraction
- change in the electronic configuration
- poor screening of d-electrons
- all of the above
In which of the following options the order of arrangement does not agree with the variation of property indicated against it?
B<C<N<O (increasing first ionisation enthalpy)
I<Br<CI<F (increasing electron gain enthalpy)
Li<Na<K<Rb (increasing metallic radius)
Al3+<Mg2+<Na+<F− (increasing ionic size).
- I2<I′2
- I′1>I′′1
- I1<I′1<I′′2
- I1<I′′1<I′1
Amongst the following elements (whose electronic configurations are given below), the one having the highest ionisation energy is
[Ne]3s23p1
[Ne]3s23p3
[Ne]3s23p2
[Ar]3d104s24p3
Which of the following represents the correct order of increasing first ionization enthalpy for Ca, Ba, S, Se and Ar?
Ca < S < Ba < Se < Ar
S < Se < Ca < Ba < Ar
Ba < Ca < Se < S < Ar
Ca < Ba < S < Se < Ar
Which is the correct order for ionic radii?
Li+ < Al3+ < Mg2+ < K+
Al3+ < Mg2+ < K+ < Li+
Mg2+ < Al3+ < K+ < Li+
None of the above
The second ionization potential of an element M is the energy required to
Remove one mole of electrons from one mole of gaseous anions
Remove one mole of electrons from one mole of gaseous cations of the element
Remove one mole of electrons from one mole of monovalent gaseous cations of the element
Remove 2 moles of electrons from one mole of gaseous atoms
- 1
- 2
- 3
- 4