Which of the following best defines
the first ionisation energy?
The energy required to remove
one mole of electrons from
one mole of gaseous ions.
The energy required to remove one mole
of electrons from one mole of gaseous atoms.
The energy required to remove one
electron from one atom in the solid state.
The energy required to add one mole
of electrons to one mole of gaseous atoms.
The second ionisation energy refers to:
The energy required to remove the
first electron from a gaseous atom.
The energy required to remove the second
electron from a gaseous ion with a +1 charge.
The energy released when a second electron is added to a neutral atom.
The energy required to break a covalent
bond in a diatomic molecule.
Which statement is true about the
relationship between first and
second ionisation energies of
an element?
They are equal for all noble gases.
They are the same for all alkali metals.
The second ionisation energy is always
smaller than the first.
The second ionisation energy is always
larger than the first.
A large jump between the third and
fourth ionisation energies of an
element indicates that:
The element has three valence electrons.
The element has four valence electrons.
The element is an alkali metal.
The element is a halogen.
Which of the following correctly explain
why the second ionisation energy
of sodium (Na) is much larger
than its first?
The second electron is removed from
the same energy level as the first.
The second electron is removed from an
inner shell closer to the nucleus.
Sodium has a small atomic radius.
Sodium has high electronegativity.
Define electronegativity
The tendency of atom to attract electron.
The energy required to remove an
electron from an atom.
The ability of an atom to form hydrogen
bonds.
Down a group in the periodic table,
electronegativity decreases because:
Nuclear charge decreases.
The number of protons decreases.
Shielding effect increases and atomic
radius increases.
Non-metallic character increases.
Across a period in the periodic table,
electronegativity generally:
Increases because nuclear charge
increases and atomic radius decreases.
Decreases because shielding effect
increases.
Increases because the number
of neutrons increases.
Decreases because metallic character
increases.
Which Period 3 oxide is acidic?
Na₂O
MgO
SO₃
Al₂O₃
Which of the following oxides is
amphoteric?
Na₂O
MgO
Al₂O₃
SO₂
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