ionisation energy

Ionisation energy is ___________.

• maximum energy required to remove 1 electron from 1 mol of gaseous atom

• minimum energy required to remove 1 electron from 1 mol of gaseous atom

• first ionisation energy

• second ionisation energy

When across a period, the atomic size decreases so the first IE ___________.

• increases

• decreases

• constant

• i am not sure

When going down a group, the atomic size increases so the first IE __________.

• increases

• decreases

• constant

• I am not sure

Factors affecting the ionisation energy:

• Atomic radius

• Effective nuclear charge

• Shielding effect

• All of the above

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)

Which equation correctly describes the first ionization energy of X?

• X --> X^- + e^-

• X --> X⁺ + e^-

• X --> X^- + e⁺

• X + e^- --> X^-

• X + e^- --> X⁺

In general ionization energy ____ as you go down a group,

and ____ as you go across the periodic table.

• decreases, decreases

• decreases, increases

• increases, decreases

• increases, increases

Which periodic group has the smallest atomic radius?

• Alkali metals
• Halogens
• Noble Gases
• Transition metals

Which statement correctly and completely identifies a trend?

• Atomic radius decreases across a period and increases down a group.
• Electronegativity decreases across a period and decreases down a group.
• Ionization energy increases across a period and increases down a group.
• Ionic radius increases across a period and increases down a group.

Ionization energy is...

• the energy required to add an electron to a specific atom
• how much energy it takes to remove an electron from an atom
• the energy required to shield the outer electrons from the nucleus
• a measure of the ability of an atom to attract electrons