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WorksheetsHChem - CCS - Periodicity
Total questions: 25
Worksheet time: 15mins
In the periodic table, elements are arranged in order of increasing _____________
atomic size
ionisation energy
electronegativity
viscosity
The rows in the periodic table are called (a)
The measure of how large atoms are is known as the (a) (two words)
Across a period, the covalent radius _______
decreases
increases
stays the same
Down a group, covalent radius __________
increases
decreases
stays the same
As you move from left to right across a period, atoms have
greater nuclear charge
smaller nuclear charge
greater numbers of electron shells
smaller numbers of electron shells
___________ is the energy involved in removing one mole of electrons from one mole of atoms in the gaseous state.
ionisation energy
electronegativity
covalent radius
nuclear charge
Across a period from left to right, the ionisation energy
increases
decreases
stays the same
Going down a group, the ionisation energy
increases
decreases
stays the same
___________ is a measure of an atom's attraction for the electrons in a bond
ionisation energy
electronegativity
nuclear charge
viscosity
Across a period from left to right, the electronegativity of atoms
increases
decreases
stays the same
Going down a group, electronegativity
increases
decreases
stays the same
Name the element with the highest electronegativity.
(a)
A potassium atom is larger than a sodium atom because potassium has
a larger nuclear charge
a larger nucleus
more occupied energy levels
a smaller ionisation energy
First ionisation of an element refers to the
removal of one electron from each atom
addition of one electron to each atom
removal of one energy level from each atom
completion of one energy level in each atom
When inner electrons shield an outer electron from the attractive effect of the nucleus and less energy is needed to remove the outer electron as a result, this is known as the (a) effect.
This equation refers to
first ionisation energy
second ionisation energy
third ionisation energy
Which of these is the first ionisation energy of sulfur?
A
B
C
D
The spike graph shows the variation in successive ionisation energies of an element, Z. In which group of the periodic table is element Z.
1
3
4
6
Which statement correctly describes the reason for iodine having a larger covalent radius than fluorine?
iodine has a higher nuclear charge
iodine has more shells of electrons
iodine has a higher first ionisation energy
iodine is more reactive than fluorine
Of all the elements in group 1, francium will have
highest first ionisation energy
lowest electronegativity
smallest covalent radius
lowest relative atomic mass
Which of the following elements would require the most energy to convert one mole of gaseous atoms into one mole of gaseous ions carrying a two positive charge?
iron
cobalt
nickel
copper
Which alkali metal would form ions with the same electron arrangement as neon?
(a)
An atom of lithium is ______ than an atom of fluorine, because the atom of fluorine has _____ ________.
smaller, less protons
smaller, more protons
larger, less protons
larger, more protons
As you go down the halogens (Group 7), the melting and boiling points
increase
decrease
