Chemistry Atomic Radii & Ionization Energy

The atomic radius decreases from left to right, causing the outermost electron to be closer to the ______.

The ionisation energy value ______ as the atomic radius decreases.

There is a dip in ionisation energy between ______ and Boron.

Atoms with half full or completely full outermost sublevels have extra ______.

The second ionisation energy refers to the energy needed to remove an electron from an ion with a ______ charge.

A large increase in ionisation energy is observed when removing an electron from the filled n=1 energy ______.

Boron has a lower ionisation energy than Beryllium because its outermost shell is only ______ full.

The filled outer sublevel requires more energy to remove an electron from it in the ______ energy level.

The atomic radius is defined as half the distance between the nuclei of two atoms of the same element that are joined together by a single covalent ______.

As you move down the groups in the Periodic Table, the atomic radius ______ due to additional energy levels.

The screening effect of the inner electrons reduces the pull of the positive nuclear ______ on the outer electrons.

As we move across a period in the Periodic Table, the atomic radius ______ due to an increase in effective nuclear charge.

The first ionisation energy is the minimum energy required to completely remove the most loosely bound ______ from a neutral gaseous atom.

The values of the first ionisation energy decrease down a group in the Periodic Table due to increasing atomic ______.

Across a period in the Periodic Table, the ionisation energy values ______ due to increasing effective nuclear charge.

The element labeled B is ______.

The outermost electrons are somewhat shielded from the attractive force of the positively charged nucleus due to the ______ effect.

The reason for the large decrease in first ionisation energy between elements R and S is that R has a full outer ______.

The first ionisation energy of element H is lower than that of element G because H has a less stable ______.

Electronegativity is defined as the relative attraction that an atom has for a shared pair of ______ in a covalent bond.

H2O and NH3 contain intermolecular ______ bonds.

Alkali Metals are stored under ______ to prevent reactions with oxygen.

Moving down the group, Alkali Metals become more reactive with ______.

Fluorine is the most ______ element of the halogens.

Halogens do not exist free in nature and must be extracted from their ______.

The first ionisation energy is the minimum energy required to remove the most loosely-bound ______.

The sharp increase in ionisation energy for removal of the 5th electron indicates it is the first to be removed from the ______ shell.

Electronegativity values ______ down the groups in the Periodic Table.

A line emission spectrum provides evidence for the existence of ______ levels in atoms.

Ionisation energy values for elements increase with ______ atomic number.

As you go down a group, the atomic radius ______, leading to a weaker pull on electrons.

The chemical properties of elements are determined by the number of electrons in the ______ energy level.

Alkali metals have very low first ionisation energy values, making them ______ elements.

Alkali Metals react with water to form the ______ of the metal.

The first ionisation energy ______ down the group of alkali metals.

All alkali metals react with oxygen to form ______.

Hydrogen gas is released when alkali metals react with ______.