Ionisation Energy

Q.

Out of N, O, Ne, Na, Na⁺select the species which have maximum and minimum ionization energy?

Q.

Ionisation energy increases as we move down the group of a periodic table whereas it decreases as we move from left to right of the periodic table.

1. True

2. False

Q.

In the modern periodic table, elements are arranged in the order of their

1. Decreasing atomic masses

2. Increasing atomic masses

3. Increasing atomic numbers

4. Decreasing atomic numbers

Q.

Was there any defect in Mendeleev's periodic table?

Is there any defect in the modern periodic table? What are those?

Q.

In which of the following elements, is the energy required to remove an electron from a neutral atom in its gaseous states the least?

1. K

2. Si

3. P

4. Na

Q.

Describe the trend of ionization potential along a period and a group in the periodic table.

Q. Nuclear charge refers to the effective positive charge of a nucleus. The nuclear charge of carbon is .

1. 8
2. 4
3. 6
4. 2

Q. List two observations which posed a challenge to Mendeleev’s Periodic Law.

Q. An element has successive ionization enthalpies as $1^{st}$ (940), 2080, 3090, 4140, 7030, 7870, 16000 and 19500 kJ $mo{l}^{-1}$^. To which group of the periodic table does this element belong?

1. 14
2. 15
3. 16
4. 17

Q.

For a given value of n (principal quantum number), ionization enthalpy is highest for

1. d - electrons

2. f - electron

3. s - electron

4. p - electron

Q.

Why do different elements exist in different states at the same temperature?

Q.

Select the factors that affect the ionisation energy of an element.

1. Effective nuclear charge

2. The number of neutrons in the nucleus

3. The energy provided to the atom of an element

4. Size of the atom

Q.

Which one of the following is/are correct statement(s) with respect to Mendeleev's periodic table?

1. The increasing order of atomic mass was not strictly followed.

2. All the columns were filled with elements.

3. Elements with similar properties were placed in the same group.

4. Elements are arranged according to their atomic mass.

Q.

Ionization potential increases over a period from left to right because the:

1. Atomic radius increases and nuclear charge increases

2. Atomic radius decreases and nuclear charge decreases

3. Atomic radius increases and nuclear charge decreases

4. Atomic radius decreases and nuclear charge increases

Q. The first four ionization enthalpy values of an element are 191, 578, 872 and 5962 kcal $mo{l}^{-1}$ Q.1) The number of valence electrons in the element is

1. 3
2. 1
3. 2
4. 4

Q.

State whether the ionisation potential increases going down a group.

Q. how many moles of electrons weigh 1kg?

Q. Which of the following will have the most negative electron gain enthalpy and which
the least negative? P, S, Cl, F, N, Br, I. Explain.

Q.

Assertion: The ionisation energy decreases as we go from left to right in a period.

Reason: The nuclear charge increases as we go from left to right in a period but the number of shells remain the same in a period.

1. Both assertion and reason are true and the reason is the correct explanation for the assertion.

2. The assertion is true but the reason is false.

3. The assertion is false but the reason is true.

4. Both assertion and reason are true but the reason is not the correct explanation for the assertion.

Q.

If one electron has been removed from an atom, it becomes increasingly difficult to remove the second and subsequent electrons from the resulting positively charged ions on account of electrostatic attraction between the nucleus and the remaining electrons. If the ionization values of elements are plotted against the atomic number, then peaks are occupied by:

1. Alkali metals

2. Alkaline earth metals

3. Noble gas elements

4. Halogens

Q.

Read the following questions and answer as per the directions given below:

Statement – I: The first ionization energy of Be is greater than that of B.

Statement – II: 2p-orbital is lower in energy than 2s.

1. Statement – I is true; Statement – II is true; Statement-II is the correct explanation for Statement – I.

2. Statement – I is true; Statement – II is true; Statement-II is not the correct explanation for Statement – I.
   

3. Statement – I is true; Statement – II is false.
   

4. Statement – I is false; Statement – II is true.

Q.

Electron gain enthalpy depends on?

1. Atomic size

2. Effective Nuclear charge

3. Screening or shielding effect

4. Stability of half filled and completely filled orbitals.

Q.

In my Pearson book it is written that Atmoic radius decreases due to increase in atomic number

Also

Ionization energy increases from top to bottom of a group since the atomic size decreases due to increase in atomic number

Please explain sir

Q.

$\text{Electron gain enthalpy}\alpha \frac{1}{Atomicsize}$

1. True

2. False

Q. Generally, the first ionization enthalpy increases along a period with few exceptions. Choose the correct option which is not an exception.

1. Mg and Al
2. Be and B
3. N and O
4. Na and Mg

Q.

Which of the following explanation is best for not placing hydrogen in either the group of alkali metals or halogens?

1. Hydrogen is much lighter element than the alkali metals or the halogens

2. None of the above

3. The ionization energy of hydrogen is to high for group of alkali metals, but too low of halogen group

4. Hydrogen can form compounds with all other elements

Q.

Which of the following configurations represents an atom of the group having the highest second ionization energy?

1. 1 2 2

2. 1 2 2

3. 1 2 2 3

4. 1 2 2 3

Q. Atomicity of FeCO₃ is ______.​

Q.

Amongst the following elements (whose electronic configurations are given below), the one having the highest ionisation energy is

1. $\left[Ne\right]3s^{2}3p^2$
   

2. $\left[Ne\right]3s^{2}3p^1$
   

3. $\left[Ne\right]3s^{2}3p^3$
   

4. $\left[Ar\right]3d^{10}4s^{2}4p^3$

Q.

Ionisation energy ___ down a group.