Atomic Structure

X and Y are elements from the same group of the Periodic Table.

The 5th to 9th ionisation energies for X and Y are shown.

Which row identifies elements X and Y?

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An ion with a charge of $2-$ contains 10 electrons and 14 neutrons.

What is its nucleon number?

Options

A   14
B   22
C   24
D   26

Q, R and S are consecutive elements in Period 3 of the Periodic Table. Element R has the highest first ionisation energy and the lowest melting point of these three elements.

What are the identities of Q, R and S?

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The first seven ionisation energies of an element between lithium and neon in the Periodic Table are shown.

$$1310 \quad 3390 \quad 5320 \quad 7450 \quad 11\,000 \quad 13\,300 \quad 71\,000 \quad \text{kJ mol}^{-1}$$

What is the outer electronic configuration of the element?

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A   $2\text{s}^2$
B   $2\text{s}^2 2\text{p}^1$
C   $2\text{s}^2 2\text{p}^4$
D   $2\text{s}^2 2\text{p}^6$

Which statement about a 3p orbital is correct?

Options

A   It can hold a maximum of six electrons.
B   It has the highest energy of the orbitals with principal quantum number 3.
C   It is at a higher energy level than a 3s orbital but has the same shape.
D   It is occupied by one electron in an isolated phosphorus atom.

Which diagram shows the electronegativity of the elements Na, Mg, Al and Si plotted against their first ionisation energies?

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A   Diagram A
B   Diagram B
C   Diagram C
D   Diagram D

How many neutrons are contained in an atom of iron with a mass number of 60?

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A   26
B   30
C   34
D   60

A helium ion contains two protons, two neutrons and one electron.

This helium ion and a proton are passed separately through a uniform electric field.

The particles are travelling at the same velocity.

Which arrow describes the path of each particle?

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Which isolated gaseous atom has a total of five electrons occupying spherically shaped orbitals?

Options

A   sodium
B   fluorine
C   boron
D   potassium

Why is the second ionisation energy of sodium larger than the second ionisation energy of magnesium?

Options

A   The attraction between the nucleus and the outer electron is greater in $\text{Na}^+$ than in $\text{Mg}^+$.
B   The nuclear charge of $\text{Na}^+$ is greater than that of $\text{Mg}^+$.
C   The outer electron of $\text{Na}^+$ is more shielded than the outer electron of $\text{Mg}^+$.
D   The outer electron of Na is in the same orbital as the outer electron of Mg.