Scps Chemistry Worksheet With Answers - Periodicity Page 4
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115. Contrast ionization energy and electron affinity. In general, what can you say about these
values for metals and non-metals ?
Ionization energy is the energy required to remove an e- from a gaseous neutral atom. It is the
energy utilized in the formation of a cation. Ionization energies for metals will be lower than
ionization energies for non-metals because IE increases as you travel across the PT.
Electron Affinity is an atom’s attraction for electrons. Energy is either given off or force onto an
atom when an e- is added to a neutral atom. Electron affinity is a negative measurement of
increasing value as you move across the PT. It is the energy released or gained in forming an
anion. Nonmetals normally form anion therefore, the EA of non metals will be greater (more
negative).
6. What is the difference between electron affinity and electronegativity.
Electron affinity is the atoms attraction for e- the measurement of energy when an e- is added to
an atom. EN is a relative value reported on the Pauling scale that tells us how much an atom
pulls or attracts an e- while in a chemical bond with another atom.
7. Why is it difficult to determine electron affinities for metals?
Most metals, especially those in the alkali and alkaline groups, want to form cations by giving
away e- rather than forming anions by assuming an e- from another atom. For this reason, it is
difficult to measure the EA of metals.
SCPS Chemistry Worksheet – Periodicity -
page 4
D. Definitions - match
First ionization energy
Noble gases
Atomic radius
Increase
Nonmetals
Decrease
Ionization energy
Semimetal
Electron affinity
Metals
Shielding effect
electronegativity
Noble gas configuration
1.
Ionization energy
is the energy required to remove an electron from an atom.
2.
The attraction of an atom for an additional electron is called
electron
affinity.
3.
The energy needed to remove the most loosely held electron from a neutral atom is called
1
st
ionization energy.
4.
When they have a(n)
noble gas configuration,
ions have a stable, filled outer electron level.
5. Along with the increased distance of the outer electrons from the nucleus,
the shielding effect
of the inner electrons causes ionization energy to decrease going down a column of the periodic
table.
6. A low ionization energy is characteristic of a(n) metal.
7. Ionization energies tend to
increase
across periods of the periodic table.
8. An element with a high ionization energy is classified as a (n)
Non-metal (will also take Nobel
gas as an
answer).
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