Periodic Table & Periodicity - Inorganic Chemistry PYQs

The element with outer electronic configuration \((n-1) d^2 n s^2\), where \(n=4\), would belong to

Among the given configurations, identify the element which does not belong to the same family as the others?

Choose the correct option regarding the following statements

Statement 1 Nitrogen has lesser electron gain enthalpy than oxygen.

Statement 2 Oxygen has lesser ionisation enthalpy than nitrogen.

Which statements among the following are correct about helium?

(i) Liquid helium is used to sustain powerful superconducting magnets.

(ii) Liquid helium is useful to carry low temperature experiments.

(iii) It is a heavy gas.

(iv) It is a flammable gas.

Which of the following represents the correct order of increasing electron gain enthalpy with negative sign for the elements?

1. Nitrogen (N) 2. Phosphorus (P) 3. Chlorine (Cl) 4. Fluorine (F)

The electronegativity of the given elements increases in the order.

Which of the following statements is/are correct?

1. Mercury is the only metal that exists as liquid at room temperature.

2. Among non-metals, carbon has the highest melting point.

3. Hydrogen is the most abundant element in the universe.

4. Oxygen is the most abundant element in the Earth's crust.

The first ionisation enthalpies of \(\mathrm{Mg}\) and \(\mathrm{Al}\) can be expected to be ............ .

In which of the following, elements are arranged in the correct order of their electron gain enthalpies?

In second period of the long form of the periodic table an element \(X\) has second lowest first ionisation enthalpy and element \(Y\) has second highest first ionisation enthalpy values. What are \(X\) and \(Y\) ?

Lithium shows diagonal relationship with element '\(X\)' and aluminium with \(Y . X\) and \(Y\) respectively are

The correct order of the metallic character of the elements \(\mathrm{Be}, \mathrm{Al}, \mathrm{Na}, \mathrm{K}\) is

Which of the following tetrahalides does not exist?

In which of the following oxides of three elements \(X, Y\) and \(Z\) are correctly arranged in the increasing order of acidic nature. The electronic configurations of \(X, Y\) and \(Z\) are \([\mathrm{Ne}] 3 s^2 3 p^1, [\mathrm{Ne}] 3 s^2 3 p^5\). [Ne] \(3 s^2\) respectively

Assertion (A) 16 th group elements have higher ionisation enthalpy values than 15 th group elements in the corresponding periods.

Reason (R) 15 th group elements have half-filled stable electronic configurations.

Assertion (A) Fluorine has smaller negative electron gain enthalpy than chlorine.

Reason (R) The electron-electron repulsion is higher in chlorine than in fluorine.