The most preferred structure among the following with the lowest energy for SO3 is:
1. | 2. | ||
3. | 4. |
The Lewis dot symbols for atoms of the elements Mg, Na, O, and N, respectively, would be:
1. | ||||
2. | ||||
3. | ||||
4. |
Lewis symbols for the atoms and ions: S and S2–; Al and Al3+; H and H– respectively, would be:
1. | ||||||
2. | ||||||
3. | ||||||
4. |
The favourable factors for the formation of an ionic bond would be:
1. | Low ionization enthalpy, High negative electron gain enthalpy, High lattice energy. |
2. | High ionization enthalpy, High electron gain enthalpy, High lattice energy. |
3. | Low ionization enthalpy, Low electron gain enthalpy, Low lattice energy. |
4. | High ionization enthalpy, Low electron gain enthalpy, High lattice energy. |
The bond length can be defined as -
1. | The equilibrium distance between the nuclei of two bonded atoms in a molecule. |
2. | The farthest distance between the nuclei of two bonded atoms in a molecule. |
3. | The shortest distance between the nuclei of two bonded atoms in a molecule. |
4. | None of the above. |
can be represented by structures 1 and 2 shown below.
These two structures cannot be taken as the canonical forms of the resonance hybrid, because :
1. | The positions of the atoms have changed.
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2. | The positions of the atoms are constant.
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3. | H3PO3 does not show resonance.
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4. | Two hydrogen atoms are missing. |
The application of dipole moment is/are :
1. | It is used to differentiate polar and non-polar bonds. |
2. | It is helpful in calculating the percentage ionic character of a molecule. |
3. | Both '1' and '2' |
4. | None of the above. |
CH4 does not exhibit square planar geometry because:
1. | For square planar geometry, 5 bonds are required. |
2. | Carbon does not have d-orbitals to undergo dsp2 hybridization. |
3. | Due to steric hindrance CH4 does not exhibit square planar geometry. |
4. | Carbon does not have d-orbitals to undergo d2sp3 hybridization. |
The lone pairs of electrons can be defined as:
1. | Electron pairs that participate in bonding.
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2. | Electron pairs that do not participate in bonding.
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3. | Electron pairs that are present in inner most shell.
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4. | Electron pairs that are present in valence shell of ions. |
The set of oxides of nitrogen that are paramagnetic in nature is:
1. NO, N2O
2. N2O3, NO
3. NO, NO2
4. N2O, NO2