A-Level Physical Chemistry Electronegativity

1. Atoms with more inner shells or subshells have a lower electronegativity.

2. The electronegativity of an atom is not significantly affected by the presence of inner shells or subshells.

3. Atoms with more inner shells or subshells have a higher electronegativity.

1. Nuclear charge

2. Relative abundance of an isotope

3. Atomic radius

4. Shielding

1. The electronegativity of an atom increases as its radius increases.

2. The electronegativity of an atom decreases as its radius increases.

3. The electronegativity of an atom is not significantly affected by its radius.

1. Electronegativity decreases across a period.

2. There is no significant change in electronegativity within a period.

3. Electronegativity increases across a period.

1. The reactivity series of metals

2. The periodic table

3. Pauling scale

4. Data from IR spectroscopy

1. Shielding effect remains reasonably constant across a period.

2. Shielding effect decreases when moving across a period.

3. Shielding effect increases when moving across a period.

1. Lithium

2. Hydrogen

3. Silicon

4. Fluorine

1. The electronegativity of an atom is not significantly affected by its nuclear charge.

2. The electronegativity of an atom decreases as its nuclear charge increases.

3. The electronegativity of an atom increases as its nuclear charge increases.

1. It is the ability of an atom to attract a pair of electrons towards itself in a covalent bond.

2. It is a property of isotopes that have different number of neutrons and protons in their nucleus.

3. It results from the positive nucleus' ability to attract negative electrons in the outer shell.

4. In a covalent bond, an electronegative atom attracts electron density toward itself.

1. Electronegativity decreases as you move down the group.

2. There is no significant change in electronegativity within a group.

3. Electronegativity increases as you move down the group.