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WorksheetsPeriodic Table
Total questions: 30
Worksheet time: 2hrs 59mins
Elements in the same ..................have similar chemical properties.
period
group
block
As you move down the periodic table atoms get bigger. This is because ____________.
The atoms have more mass.
The atoms have more protons.
The atoms have more shells.
The atoms have more neutrons
As you move across the periodic table atoms tend to get smaller because, ______________.
the atoms have more mass.
the atoms have less shell.
the atoms have higher Zeff.
the atoms have less electrons.
Which group has the smallest atomic radius?
Alkali metals
Halogens
Noble Gases
Transition metals
Atomic radius generally increases as we move __________.
down a group and from right to left a period
up a group and from left to right a period
down a group and from left to right a period
up a group and from right to left a period
Why is iodine larger than bromine?
iodine has a greater Zeff than bromine
iodine has a greater number of protons than bromine
iodine has more energy levels and greater shielding effect than bromine
iodine has more valence electrons than bromine
Which group and period does the element with the electron configuration 1s2 2s2 belong to?
Group 1 Period 2
Group 2 Period 2
Group 14 Period 2
Group 12 Period 4
How many valence electrons does an element with the electron configuration 1s22s22p4 have?
6
4
8
2
Of the elements Al, Mg, Si, Na, which has the smallest atomic radius?
Al
Mg
Si
Na
Effective nuclear charge ________ across a period.
increases
decreases
stays the same
What is effective nuclear charge?
The charge that effects the mass of the atom.
The charge that the protons feel from the rest of the atom.
The charge felt by the valence electrons.
The charge felt by the core electrons.
As you move down a group, the effective nuclear charge
increase
decreases
stays the same
Determine the Group, Period and Block for the element with electronic configuration 1s2 2s2 2p6 3s2 3p4
Block p Period 3 Group 16
Block p Period 3 Group 14
Block s Period 3 Group 6
Block p Period 4 Group 14
Going down a group , attraction between nucleus with the valence electrons become __________ as shielding effect ___________.
stronger , decreases
weaker, increases
stays the same, remain unchanged
weaker, decreases
Ionization energy _______ across the period .
increases
decreases
stays the same
As you move across a period, the attraction between nucleus and valence electrons _______ as the effective nuclear charge ___________.
remain unchanged, stays the same
stronger, decreases
weaker, increases
stronger, increases
First Ionisation energy is ___________.
maximum energy required to remove 1 mol electron from 1 mol of gaseous atom
minimum energy required to remove 1 mol electron from 1 mol of gaseous atom
minimum energy required to add 1 mol electron from 1 mol of gaseous atom
minimum energy required to remove 1 mol electron from 1 mol of gaseous unipositive ion
When going across a period, the atomic size ______ so the first IE ___________.
increases, increases
decreases, decreases
decreases, increases
increases, decreases
Factors affecting the ionisation energy: (select all correct answers)
Atomic radius
Effective nuclear charge
Shielding effect
Number of valence electrons.
The equation for the first ionisation energy of a sodium atom is:
Na (g) -> Na+ (g) + e-
Na+ (g) -> Na2+ (g) + e-
Na (s) -> Na+ (g) + e-
Na+ (g) + e- -> Na (g)
When there is drastic increase in successive ionisation energy , the electron is removed from __________.
valence shell
inner shell
Electronegativity trends will ....
Increase across a period and increase down a group
Increase across a period and decrease down a group
Decrease across a period and increase down a group
Decrease across a period and decrease down a group
Electronegativity is...
the energy required to remove an electron from a specific atom.
how easy of an atom to lose electrons.
the tendency of an atom to attract electrons to itself when bonded to another atom.
the energy released when an electron is added.
What is meant by isoelectronic?
Group of atoms or ions have the same proton numbers.
Group of atoms or ions have the same electronic configuration
Group of atoms or ions have the same electrical properties
Group of atoms or ions have the same electronic charge
Which of the pair is the isoelectronic species?
Na+ and Si4+
Na+ and Cl-
Mg2+ and Al +
S2- and O2-
Given the highest ratio of ionisation energy is IE4/IE3. Provide the valence electronic configuration.
ns2 np2
ns2 np1
ns2 np3
ns2
Which of the following is an amphoteric oxide?
Na2O
MgO
Al2O3
Cl2O
Second Ionisation energy is ___________.
maximum energy required to remove 1 mol electron from 1 mol of gaseous atom
minimum energy required to remove 1 mol electron from 1 mol of gaseous atom
minimum energy required to add 1 mol electron from 1 mol of gaseous atom
minimum energy required to remove 1 mol electron from 1 mol of gaseous unipositive ion
A metal ‘M’ is in the group 2 of the Periodic Table. What will be the formula of its oxide?
MO
M2O
M2O3
MO2
Alkaline earth metals P and Q have 4 shells and 5 shells respectively. Choose correct statement about P and Q.
P has a larger atomic radius than Q
P has a higher ionisation energy than Q
P has greater shielding effect than Q
P is less electronegative than Q
