WorksheetsPeriodicity Starter
Total questions: 10
Worksheet time: 5mins
Which of the following statements is NOT correct?
The atomic radii of the elements decrease across period 3
The first ionisation energies of the elements generally increase across period 3
The melting points of the elements increase across period 3
Which of the folowing correctly lists the atomic radii (in nm) of the elements Na, Mg, Al and Si
0.190, 0.145, 0.118, 0.111
0.111, 0.118, 0.145, 0.190
0.111, 0.145, 0.118, 0.190
0.190, 0.118, 0.145, 0.111
Which of these statements BEST explains the decrease in atomic radii across period 3 fro sodium to argon?
Shielding increases, pulling electrons closer to the nucleus
Shielding decreases, pulling electrons closer to the nucleus
The effective nuclear charge increases, pulling electrons closer to the nucleus
How doe shielding vary across period 3 from sodium to argon?
It increases significantly
It decreases significantly
There is no significant variation
Which of these statements explains why the first ionisation energy of sodium is less than that of magnesium?
The effective nuclear charge is less in sodium, so more energy is required to remove an electron
The effective nuclear charge is less in sodium, so less energy is required to remove an electron
The effective nuclear charge is less in magnesium, so more energy is required to remove an electron
Which of the following elements has a first ionisation energy that is lower than expected?
magnesium
aluminium
phosphorous
Which of these statements is the BEST explanation for why the first ionisation energy of aluminium is lower than that of magnesium?
The highest energy electron in aluminium is removed from a 3p orbital as opposed to a 3s orbital
There is mutual repulsion between 3p electrons in aluminium
The aluminium ions have a higher charge density than magnesium
Which of these statements is the BEST explanation for why the first ionisation energy of sulfur is lower than that of phosphorous?
The highest energy electron in sulfur is removed from a 3p orbital as opposed to a 3s orbital
There is mutual repulsion between the two paired electrons in the 3p orbital in sulfur
There is mutual repulsion between the two paired electrons in the 3s orbital in phosphorous
There is no pair of electrons in the 3p orbital in phosphorous
Which of the following elements has a covalently-bonded macromolecular structure similar to diamond?
silicon
sulfur
phosphorus
Which of these statements best explains why chlorine has a lower melting point than sulfur?
Chlorine atoms have a greater relative atomic mass than sulfur
Chlorine atoms have weaker covalent bonds than sulfur atoms
Chlorine molecules are held together by weaker van der Waals forces than sulfur molecules
