Electronegativity & Bonding (CIE A Level Chemistry)

This question is about electronegativity. 

The electronegativities of some elements are shown in Table 3.1 below. 

Table 3.1

Define the term electronegativity. 

Use Table 3.1 to explain the trend in electronegativity across the Periodic Table.

Explain how the carbon-hydrogen bond (such as in CH₄) differs from the nitrogen-hydrogen bond (such as in NH₃) in terms of the bond polarity.

Explain, in terms of electronegativity, why the bonding in ammonia (NH₃) is covalent but the bonding in lithium chloride (LiCl) is ionic.

Chlorine (Cl) reacts with boron (B) to form boron trichloride (BCl₃).

Molecules and separate atoms (such as noble gases) are attracted to one another by intermolecular forces. 

The boiling point of tetrachloromethane (CCl₄) is 77 C whereas the boiling point of water (H₂O) is 100 C. 

Define the term electronegativity.

The periodic table displays the chemical elements, arranged in order of increasing atomic number. It is made up of groups and periods of elements.

State and explain the general trend in electronegativity across a period.

Chlorine, Cl₂, reacts with boron, B, to form boron trichloride, BCl₃.

Fig. 3.1

A compound formed from magnesium and oxygen has a different structure to a compound formed from phosphorus and oxygen.

Predict the type of bonds that will occur in each compound. Explain your answer.

Explain why the melting point of phosphorus(III) oxide, P₄O₆, is lower than that of magnesium oxide in terms of their bonding and structure.

Phosphorus(III) oxide, P₄O₆, contains no P–P or O–O bonds.

In the P₄O₆ molecule, all oxygen atoms are bonded to two other atoms and all phosphorus atoms are bonded to three other atoms.

Sketch a structure for P₄O₆.

Explain the difference in electronegativity shown in Fig. 3.1 between magnesium and calcium.