12 Questions
What is the general trend of atomic radius across a period?
Atomic radii decrease from left to right across a period.
Why does the 1st ionisation energy increase across a period?
It is due to the increasing number of protons as the electrons are being added to the same shell.
What is the reason for the small drop in 1st ionisation energy between Mg and Al?
Mg has its outer electrons in the 3s subshell, whereas Al is starting to fill the 3p subshell, making Al's electron slightly easier to remove.
What is the reason for the small drop in 1st ionisation energy between P and S?
Sulfur's outer electron is being paired up with another electron in the same 3p orbital, resulting in a slight repulsion between the two negatively charged electrons.
What is the classification of elements based on?
The classification of elements is based on which orbitals the highest energy electrons are in.
What is the definition of periodicity?
Periodicity is the repeating pattern of physical or chemical properties going across the periods.
What type of bonding is responsible for the high melting and boiling points of Na, Mg, and Al, and why does it get stronger as the number of electrons in the outer shell increases?
Metallic bonding, which gets stronger as the number of electrons in the outer shell increases because more electrons are released to the sea of electrons, resulting in stronger bonds.
Why does Si have a very high melting and boiling point, and what type of bonding is responsible for this?
Si has a very high melting and boiling point due to macromolecular bonding, which involves many strong covalent bonds between atoms that require high energy to break.
What type of bonding is responsible for the low melting and boiling points of Cl2, S8, and P4, and why does S8 have a higher melting point than P4?
Simple molecular bonding, which involves weak van der Waals forces between molecules, is responsible for the low melting and boiling points. S8 has a higher melting point than P4 because it has more electrons, resulting in stronger van der Waals forces between molecules.
Why does Ar have a very low melting and boiling point, and what type of bonding is responsible for this?
Ar has a very low melting and boiling point due to monoatomic bonding, which involves weak van der Waals forces between individual atoms.
What is the trend in melting and boiling points observed in period 2, and what types of bonding are responsible for this trend?
The trend in period 2 is similar to that in period 3, with a significant drop in melting and boiling points between Be and B, and N and O, due to the change from metallic to macromolecular bonding, and then to simple molecular bonding.
What is the reason for the increase in melting and boiling points from Na to Al, and how does this relate to the type of bonding present in these elements?
The increase in melting and boiling points from Na to Al is due to the increase in the number of electrons in the outer shell, which results in stronger metallic bonds, requiring higher energy to break.
Test your understanding of periodicity, a fundamental concept in chemistry, and learn how to classify elements into s, p, and d blocks. Explore the trends of atomic radius across periods and understand the role of protons and electrons in shaping these properties.
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