What is the general trend observed for the first ionization energies of the elements in groups 13to 17?

1.  Ionization energies tend to increase from left to right in a period and are approximately constant in a group

2.  Ionization energies tend to increase from left to right in a period and decrease from top to bottom in a group

3.  Ionization energies tend to decrease from left to right in a period and increase from top to bottom in a group

4.  Ionization energies tend to decrease from left to right a period and decrease from top to bottom in a group

Which of the following pairs of substances are allotropes?

1.  ${\mathrm{CH}}_3{\mathrm{CH}}_2\mathrm{OH} \mathrm{and} {\mathrm{CH}}_3{\mathrm{OCH}}_3$

2.  $\mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_2 \mathrm{and} \mathrm{Fe}{\left({\mathrm{NO}}_3\right)}_3$

3.  NaCl and KCl

4.  ${\mathrm{O}}_2 \mathrm{and} {\mathrm{O}}_3$

 Element 114 is most likely to be a

1.  Reddish-brown volatile liquid

2.  A pale yellow-green gas

3.  A colourless crystal

4.  A grey-silvery metal

Which gas-phase atom has the largest radius?

1.  Na

2.  K

3.  Mg

4.  Ca

In which list are atoms of the elements Be, B, Mg and Al arranged from smallest to largest atomic radius?

1.  Be < B < Mg < Al

2.  Mg < Be < Al < B

3.  B < Be < Al < Mg

4.  Al < Mg < B < Be

What property of the oxygen atom is represented by the equation : $O\left(g\right)+e^{-}\to O^{-}\left(g\right)$?

1.  Electronegativity

2.  First electron affinity

3.  First ionization energy

4.  Lattice energy

Which of the following isoelectronic species has the largest radius?

1.  $K^{+}$

2.  $C{a^2}^{+}$

3.  $P^{3-}$

4.  $S^{2-}$

Which group best illustrates the transition from non-metallic to metallic behavior with increasing atomic number?

1.  Be, Mg, Ca, Sr

2.  N, P, As, Sb

3.  F, Cl, Br, l

4.  Fe, Ru, Os, Hs

The ionisation energy will be maximum for the process:

1. $Ba\to B{a}^{2+}$

2. $Be\to B{e}^{2+}$

3. $Cs\to C{s}^{+}$

4. $Li\to L{i}^{+}$

Which of the following statements is not correct?

1.  The first ionization energy generally decreases from top to bottom within a group

2.  The atomic radius generally increases from top to bottom within a group

3.  The first ionization energy generally decreases from left to right across a period

4.  The second ionization energy of an atom is always greater than the first ionization energy