Effect of Nuclear Charge

Q. Why size of noble gas is greater than that of halogen

Q.

In which of the following sets, elements have nearly same atomic radii?

1. 

2. 

3. 

4. 

Q.

Explain the trends in physical properties(point wise)

A.atomic radius (point wise)

B.Ionic radius (point wise)

C.Ionization Enthalpy (point wise)

D.Electron Gain Enthalpy (point wise)

E.Electronegative (point wise)

Q. Explain, the statement 'In each period, the atomic radii gradually decrease with increase in atomic number'. Give one example to justify your answer.

Q.

Why do metals have large atomic radii as compared to non metals?

Q.

Identify the correct order of the size of the following.

1. $C{a}^{2+}<K^{+}<Ar<S^{2-}<C{l}^{-}$

2. $Ar<C{a}^{2+}<K^{+}<C{l}^{-}<S^{2-}$

3. $C{a}^{2+}<K^{+}<Ar<C{l}^{-}<S^{2-}$

4. $C{a}^{2+}<Ar<K^{+}<C{l}^{-}<S^{2-}$

Q.

Which one of the following ions will be smallest in size?

1. $N{a}^{+}$

2. $M{g}^{2+}$

3. $O_2^{-}$

4. $F^{-}$

Q.

The correct order of the decreasing ionic radii among the following isoelectronic species is

1. $C{a}^{2+}>K^{+}>S^{2-}>C{l}^{-}$

2. $S^{2-}>C{l}^{-}>K^{+}>C{a}^{2+}$

3. $C{l}^{-}>S^{2-}>C{a}^2+>K^{+}$

4. $K^{+}>C{a}^{2+}>C{l}^{-}>S^{2-}$

Q. Identify the wrong statement in the following. [CBSE AIPMT 2012]

1. Amongst isoelectronic species, smaller the positive charge on the cation, smaller is the ionic radius
2. Amongst isoelectronic species, greater the negative charge on the anion, larger is the ionic radius
3. Atomic radius of the elements increases as one moves down the first group of the periodic table
4. Atomic radius of the elements decreases as one moves across from left to right in the 2nd period of the periodic table

Q. Arrange the following isoelectronic species in order of increasing ionization enthalpy (IE).

1. $O^{2-}<F^{-}<{Na}^{+}<{Mg}^{2+}$
2. $F^{-}<O^{2-}<{Na}^{+}<{Mg}^{2+}$
3. $O^{2-}<F^{-}<{Mg}^{2+}<{Na}^{+}$
4. None of these

Q. Arrange the following elements in the order of their decreasing metallic character.

1. Cl > Si > Al > Mg > Na
2. Na > Mg > Al > Si > Cl
3. Al > Na > Si > Ca > Mg
4. Na > Al > Mg > Cl > Si

Q. The correct order of decreasing ionic radius among the following anions would be:

1. $S{e}^{2-},I^{-},B{r}^{-},F^{-},O^{2-}$
2. $F^{-}.B{r}^{-},O^{2-},S{e}^{2-},I^{-}$
3. $I^{-},S{e}^{2-},B{r}^{-},O^{2-},F^{-}$
4. $F^{-},O^{2-},B{r}^{-},S{e}^{2-},I^{-}$

Q. On going across a period in the periodic table, the elements tend to become less metallic in character. Which one of the following is not an indication of this trend?

1. There is an overall increase in molar mass
2. There is a change in bond type for ionic to covalent
3. There is an increase in electronegativity
4. There is an overall decrease in ionisation energy

Q.

The correct order of the decreasing ionic radii among the following isoelectronic species is

1. $S^{2-}>C{l}^{-}>K^{+}>C{a}^{2+}$
   

2. $K^{+}>C{a}^{2+}>C{l}^{-}>S^{2-}$

3. $C{a}^{2+}>K^{+}>S^{2-}>C{l}^{-}$
   

4. $C{l}^{-}>S^2->C{a}^{2+}>K^{+}$
   

Q.

three elements X, Y, Z have ionic radii 1.33A, 0.95A and 0.60A respectively . arrange them in order of increasing atomic number. also explain the trends

Q.

The incorrect hydrated radius order is:

1. $L{i}_{\left(aq\right)}^{+}<B{e}_{\left(aq\right)}^{2+}$

2. $N{a}_{\left(aq\right)}^{+}<A{l}_{\left(aq\right)}^{3+}$

3. $I_{\left(aq\right)}^{-}>C{l}_{\left(aq\right)}^{-}$

4. $B{a}_{\left(aq\right)}^{2+}<C{a}_{\left(aq\right)}^{2+}$

Q.

Which one of the following is the smallest in size?

1. $N{a}^{3+}$
   

2. $O^{2-}$
   

3. $F^{-}$
   

4. $N{a}^{+}$

Q. Arrange the following elements in the order of their increasing non-metallic character:

1. Li < Be < C < O < F
2. F < O < C < Be < Li
3. F < O < C < Be < Li
4. F < O < Be < C < Li

Q. Which of the following set of elements is written in order of their increasing metallic character?

1. Mg, Al, Si
2. Be, Mg, Ca
3. C, O, N
4. Na, Li, K

Q.

Ionic radii are

1. Directly proportional to effective nuclear charge

2. Directly proportional to square of effective nuclear charge

3. Inversely proportional to effective nuclear charge

4. Inversely proportional to square of effective nuclear charge.

Q.

Ionic radii are

1. directly proportional to square of effective nuclear charge

2. inversely proportional to effective nuclear charge

3. inversely proportional to square of effective nuclear charge

4. directly proportional to effective nuclear charge

Q. 8.The bromine atom processor 35 electrons it contains 6 electrons in 2P orbital 6 electrons in 3p orbital electrons in 40 orbital which of these electrons experiences the lowest effective nuclear charge