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WorksheetsPeriodicity
Total questions: 14
Worksheet time: 9mins
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
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 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.
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
Why does ionization energy decrease going down a group?
Adding more energy levels makes the ve- further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Why does electronegativity increase across a period?
Adding more energy levels makes the ve- further from the nucleus
There are more valence electrons in the outer shell
There are more protons in the nucleus
There are less protons in the nucleus
Which is smaller... Mg or Mg2+ ?
Mg because it gains an energy level
Mg due to extra electron repulsion
Mg2+ because of extra electron repulsion
Mg2+ because it loses an energy level
Which is the correct order of melting points of these Period 3 elements?
phosphorus > sulfur > chlorine > argon
argon > chlorine > phosphorus > sulfur
sulfur > phosphorus > chlorine > argon
chlorine > phosphorus > sulfur > argon
Which of the following is a correct statement about the trend in atomic radius across Period 3 of the Periodic Table?
radius increases because the atoms have more electrons
radius decreases because nuclear charge increases
radius increases because shielding (screening) increases
radius decreases because shielding (screening) decreases
The diagram shows how a property of Period 3 elements varies across the period. What is the property?
Atomic radius
Electronegativity
First ionisation energy
Melting point
Which of these Period 3 elements has the highest melting point?
Aluminium
Phosphorus
Sodium
Sulfur
Which element has the highest first ionisation energy?
Aluminium
Phosphorus
Silicon
Sulfur
Which properties are typical of most non-metals in period 3?
I. They form ions by gaining one or more electrons.
II. They are poor conductors of heat and electricity.
III. They have high melting points.
I and II only
I and III only
II and III only
I, II and III
