Atomic Structure

Give the full electronic configuration of a fluorine atom.

Deduce the number of pairs of electrons in the second energy shell, $n = 2$, of an oxygen atom.

Draw the shape of the highest energy orbital that contains electrons in an atom of calcium.

Write an equation to represent the first ionisation energy of sulfur.

Explain why the first ionisation energy of sulfur is less than the first ionisation energy of phosphorus.

Arrange the three species $\text{F}^-$, $\text{Ne}$ and $\text{Na}^+$ in order of increasing radius.

Explain your answer.

.................................. < .................................. < ..................................
smallest radius largest radius

Construct an equation to represent the first ionisation energy of oxygen.
Include state symbols.

State and explain the general trend in first ionisation energies across Period 2.

Explain why ionisation energy A in Fig. 1.1 does not follow the general trend in first ionisation energies across Period 2.

Element E is in Period 3 of the Periodic Table.
The first eight ionisation energy values of E are shown in Table 1.1.

Table 1.1

Deduce the full electronic configuration of E.
Explain your answer.

full electronic configuration of E =

explanation

Write an equation for the first ionisation energy of Mg.

Include state symbols.

Explain the observed trend in first ionisation energies down Group 2.

The second ionisation energy of Be is $1757 \text{ kJ mol}^{-1}$.

Explain why the second ionisation energy of Be is higher than the first ionisation energy of Be.

Complete the diagram with the relative charge of each of the electrically charged plates.

On the diagram, draw a line to show how a separate beam of neutrons from the same source behaves in the same electric field.

State the number of occupied orbitals in an isolated atom of $_{36}\text{Kr}$.

Complete the diagram to show the number and relative energies of the electrons in an isolated atom of $_{14}\text{Si}$.

The diagram shows a type of orbital.

State the total number of electrons that exist in all orbitals of this type in an atom of $_9\text{F}$.

The first ionisation energies of elements in the first row of the d block ($_{21}\text{Sc}$ to $_{29}\text{Cu}$) are very similar. For all these elements, it is a 4s electron that is lost during the first ionisation.

Suggest why the first ionisation energies of these elements are very similar.

Hydron is a general term used to represent the ions $^1\text{H}^+$, $^2\text{H}^+$ and $^3\text{H}^+$.

State, in terms of subatomic particles in the nucleus, what is the same about each of these ions and what is different.

same ..........................................................................................................................................

different ......................................................................................................................................

Write an equation for the first ionisation energy of Mg.

Include state symbols.

Explain the observed trend in first ionisation energies down Group 2.

The second ionisation energy of Be is $1757 \text{ kJ mol}^{-1}$.

Explain why the second ionisation energy of Be is higher than the first ionisation energy of Be.

Explain what is meant by the term first ionisation energy.

Suggest why the first ionisation energy of B is much less than that of A.

P–T are successive elements in Period 3 of the Periodic Table.

The letters are not the symbols of the elements.

On the axes, sketch a graph to show the trend in the atomic radius of the elements P–T.

Explain your answer.

explanation

Complete the table to show the composition and identity of some atoms and ions.

State and explain the group number of element Y.

group number ...............................

explanation .........................................................................................................................

State and explain the general trend in first ionisation energies across the third period.

Complete the electronic configuration of element X.

$1s^2$ .................................................................................................................................

Calculate the abundance of the third isotope.

The relative atomic mass of this sample of oxygen is 16.0044.

Calculate the mass number of the third isotope. You must show your working.

Label the energy levels to indicate the principal quantum number and the type of orbital at each energy level.

On the axes below, draw a sketch diagram of one of each different type (shape) of orbital that is occupied by the electrons in a second-period element.

Label each type.

Complete the electronic configurations of nitrogen atoms and oxygen atoms on the energy level diagrams below.
Use arrows to represent electrons.

Use the Data Booklet to state the value of the first ionisation energy of nitrogen and of oxygen.

N ............................... $\text{kJ mol}^{-1}$

O ............................... $\text{kJ mol}^{-1}$

Explain, with reference to your answer to (a)(iii), the relative values of these two ionisation energies.

Give the equation, including state symbols, for the first ionisation energy of sulfur.

Explain why there is a general increase in first ionisation energies across the Period from sodium to argon.

Explain why the first ionisation energy of magnesium is greater than that of aluminium.

Explain why the first ionisation energy of phosphorus is greater than that of sulfur.

Define isotopes.

Complete Table 2.1 to show the number of protons and nucleons in one atom of $^{56}\text{Fe}$.

Table 2.1

Deduce the number of pairs of electrons in the shell with principal quantum number $n = 3$ in an Fe atom.

Write an equation to represent the first ionisation energy of iron.

Suggest how the value for the first ionisation energy of $^{54}\text{Fe}$ compares to the first ionisation energy of $^{56}\text{Fe}$. Explain your answer in terms of the factors that affect ionisation energy.