Study of Periodicity in Chemistry

What is the definition of first ionisation energy?

• The energy required to add one electron to a mole of gaseous atoms to form a mole of gaseous 1- ions.

• The energy required to remove one electron from a mole of gaseous atoms to produce one mole of gaseous 1+ ions.

• The energy required to remove all electrons from a mole of gaseous atoms.

• The energy required to break the molecular bonds in one mole of gaseous molecules.

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Which equation correctly represents the first ionisation energy of sodium (Na)?

• Na(g) -> Na+(g) + e-

• Na+(g) + e- -> Na(g)

• Na(g) + e- -> Na-(g)

• 2Na(g) -> 2Na+(g) + 2e-

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Which element has the highest third ionization energy among the first 20 elements?

• Oxygen (O)

• Lithium (Li)

• Neon (Ne)

• Boron (B)

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Which of the following elements has the lowest second ionization energy?

• Potassium (K)

• Calcium (Ca)

• Sodium (Na)

• Magnesium (Mg)

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What does the graph generally illustrate about the first ionisation energy as the atomic number increases?

• It decreases steadily.

• It increases steadily.

• It shows a series of peaks and troughs

• It remains constant.

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Based on the graph, which atomic number range shows a significant drop in first ionisation energy?

• 0 to 2

• 4 to 5

• 10 to 12

• 16 to 18

What is the approximate first ionisation energy at atomic number 10?

• 500 kJ/mol

• 1000 kJ/mol

• 1500 kJ/mol

• 2000 kJ/mol

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Which element has the highest first ionization energy according to the graph?

• Helium (He)

• Neon (Ne)

• Lithium (Li)

• Beryllium (Be)

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Which of the following factors can explain the trend in ionization energies and reactivity of elements?

• Nuclear attraction, Atomic radius, Nuclear charge, Shielding

• Electron affinity, Molecular geometry, Covalent bonding, Ionic bonding

• Phase changes, Heat capacity, Vapor pressure, Boiling point

• Chemical kinetics, Reaction mechanisms, Catalysts, Enzyme activity

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Why do melting points vary across a period on the periodic table?

• Because of the change in bonding and structure type.

• Because of the decreasing atomic radius

• Because of the uniform electron distribution

• Because of the decreasing number of neutrons

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