Trends on the Periodic Table

What happens the atomic radii across a period in the periodic table

• The atomic radius increases across a period

• The atomic radius is not changed across a period

• The atomic radius reduces in size across a period

• The atomic radius is affected by the group name

What happens the electronegativity across a period?

• The electronegativity increases across a period

• The electronegativity stays the same across a period

• The electronegativity is linked to radius size

• The electronegativity reduces across a period

Answer explanation

The power of attraction that an atoms has for a shared pair of electrons in a covalent bond?

Elements on the left of the table tend to lose electrons and forms ions.

Group 7 elements only need 1 more electron to satisfy the octet rule and will readily share of take an electron to achieve this.

What happens the ionisation energy down a group on the periodic table?

• Ionisation energy stays the same downa group

• The ionisation energy increases down a group

• The ionisatisation energy relies on electronegativity

• The ionisation energy decreases down a group

What is the effective nuclear charge?

• It is the increase in protons as you move across a period

• It is the increase in number of positive charged protons and the increase in negative charged electrons across a period

• It is the increase in size of the atom across a period

• It is the increas in size of atomic radius across a group

Answer explanation

As you travel across a period the number of protons (+ve) increases by 1 in each element and the number of electrons (-ve). As the +ve and -ve charge increases this causes a greater pull between the charged particles and this reduces the size of the radius.

This is the effect of increased nuclear charge.

The first ionisation energy is ........

• the energy that a compound has to help it form a bond

• the energy required to add electrons to another atom to make a compound

• the energy that an atom has to break its bond in a gaseous state

• the energy required to remove the most loosely bound electrons from a neutral gaseous atom in its ground state

What is the ground state of an element?

• When the electrons are excited and move to a higher energy level

• When the electrons are removed and no more electrons exist in the atom

• When the electrons are in the lowest possible energy level

• When the electrons move to another atom by sharing electrons.

What is the electronegativity of an element .....

• the power of attraction that an atom in a molecule has for a shared pair of electrons in a covalent bond

• the charge that the atoms have when they form ions

• it is the number of electrons that an atom has

• It is the power of attraction that a molecule has to form ionic bonds

How can we predict the polarity of covalent bonds?

• Using the ionisation energy table values

• Using the atomic radius values

• Using the electronegativity values

• Using the deionisation values