WorksheetsAS periodicity
Total questions: 24
Worksheet time: 16mins
Which of the following elements has the smallest atomic radius?
Sulfur
Chlorine
Aluminum
Sodium
Which Block is letter C
s - block
p - block
d - block
f - block
When Zeff increases, the nucleus attraction
towards electrons become
Weaker
Stronger
Remain the same
Across a period from left to right , atomic radius
decreases
increases
increases, then decreases
decreases, then increases
Cations are _________________ in size than anions.
bigger
smaller
same
What is meant by isoelectronic species?
Groups of atoms and ions which have the same valence electrons.
Groups of atoms and ions which have the same electronic configuration.
Groups of atoms and ions which have the same n.
What is the tendency of an atom to attract electrons towards itself?
atomic radius
ionization energy
shielding
Electronegativity
What happens to atomic radius across a period?
the atoms get bigger because the nucleus is bigger as more protons are added
the atoms get bigger because there are more ve-
the atoms get smaller because with more attraction to the extra protons, the e- cloud moves closer to the nucleus
Which atom has the LOWER ionization energy?
Al
Cl
Across a period from left to right , atomic radius
decreases
increases
increases, then decreases
decreases, then increases
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 element has the highest first ionisation energy?
Aluminium
Phosphorus
Silicon
Sulfur
Which of these Period 3 elements has the highest melting point?
Aluminium
Phosphorus
Sodium
Sulfur
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
Which elements are shown in increasing order of the stated property?
Atomic radius: phosphorus, sulfur, chlorine.
First ionisation energy: sodium, magnesium, aluminium.
Electronegativity: sulfur, phosphorus, silicon.
Melting point: argon, chlorine, sulfur.
Which of these elements has the highest second ionisation energy?
Na
Mg
Ne
Ar
Which one of the following statements is correct?
The first ionisation energies of the elements in Period 3 show a general decrease from sodium to chlorine.
The electronegativities of Group 2 elements decrease from magnesium to barium.
The strength of the intermolecular forces increases from hydrogen fluoride to hydrogen chloride.
The ability of a halide ion to act as a reducing agent decreases from fluoride to iodide.
What is the general trend with ionization energy as one moves across a period from left to right?
Ionization energy generally decreases
Ionization energy generally increases
Ionization energy does not change
Ionization energy is the same value for all elements
Ionization energy is directly proportional to the atomic radius
What is the trend for reactivity of the alkali metals as one moves down a group?
Reactivity increases
Reactivity decreases
Reactivity is relatively the same for the whole group
Alkali metals are generally unreactive
The reactivity decreases then increases
Which element has the highest electronegativity?
F
K
I
Cs
H
