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WorksheetsSTPM PERIODICITY
Total questions: 10
Worksheet time: 5mins
Among which of the following pairs of the Period 3 elements is the difference in boiling point the greatest?
Silicon and argon
Sodium and argon
Sodium and silicon
Aluminium and chlorine
Which of the following statements is true regarding the oxides of the elements in Period 3 (sodium to chlorine) of the Periodic Table?
Sodium oxide is the strongest base because sodium is the most electropositive element in Period 3
Going across Period 3 the properties of the oxides changes from base to acid because the bond between the element and oxygen gets stronger.
Aluminium oxide is amphoteric because it is in Group 13.
Oxide of phosphorus forms the strongest acid because it is the most soluble in water.
Going across Period 3 (sodium to chlorine) in the Periodic Table
The electronegativity of the elements decreases.
The ionisation energy of the element decreases
The standard electrode potential of the elements increases.
The strength of the elements as reducing agents increases.
The proton numbers of elements X, Y and Z are 14, 19 and 26 respectively. Which of the following statements is true with regard to X, Y and Z?
X is a d-block element.
Y is a strong oxidizing agent
Z exhibits only one oxidation state in its compounds.
The oxide of X with the formula of XO3- exists as a polymer.
Which of the following is true for the elements in the Periodic Table?
There are fewer metals compared to non-metals.
The size of the atoms increases with increasing nucleon number.
The metallic property increases on going down a group.
The reactivity increases on going down a group.
An oxide of G has a boiling point 2230°C. It dissolves in aqueous sodium hydroxide solution but not in water and acid. Oxide G is
PbO2
P2O5
SiO2
Al2O3
The first ionisation energy generally increases across a period in the Periodic Table. Which statement explains why the first ionisation energy of sulphur is lower than that of phosphorus?
The electrons in the p orbitals of sulphur experience greater electrostatic repulsion than that of phosphorus
The sulphur atom has more electrons than phosphorus atom.
The S-S bond is weaker than the P-P bond.
The size of S8 molecule is bigger than P4 molecule.
The properties of elements can be deduced from electronic configurations. Which statement is true about Na+ ion, Cl- ion, Ar atom and K+ ion?
Na+ ion is bigger than Cl- ion.
The charge density of Na+ ion is lower than that of Cl- ion.
The ionisation energy of K+ ion is higher than that of Na+ ion.
Cl- ion, K+ ion and Ar atom have the same electronic configuration.
The acid-base properties of oxides are related to their structure and chemical bonding. Which oxide dissolved in water to form an acidic solution?
MgO
Al2O3
. SiO2
SO3
Which statement explains the difference in the first
ionisation energies between beryllium and boron?
Boron atom has more valence electrons.
Boron atom has a greater shielding effect.
Beryllium atom has a more stable electronic
configuration.
The 2p electron in boron atom is at a higher
energy level than the 2s electron in beryllium atom
