Scps Chemistry Worksheet With Answers - Periodicity Page 7
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119. Which element on the periodic table has
a.
lowest ionization energy -
Cesium
b.
highest second ionization energy –
Lithium
c.
highest electronegativity -
Fluorine
d.
highest ionization energy
– Helium – followed by Fluorine
e.
largest atomic radius –
Cesium
10. Explain the relationship between the relative size of an ion to its atom and the charge on the
ion.
Cation: has lost an e-, therefore electrostatic repulsion b/w e- is decreased and the size of the ion
shrinks. The cation of an element is smaller than the neutral atom of the same element.
Anion: has gained an e-, therefore electrostatic repulsion b/w e- is increased and the size of the
ion increases. The anion of an element is larger than the neutral atom of the same element.
11. Explain why noble gases are inert and do not form ions.
Inert means un-reactive. The noble gases have a full octect of valence electrons, 2s and 6 p
electrons in its outer valence shell. The noble gases do not need to nor do they have to accept or
lose electrons. The number of valence electrons determines an element’s chemical properties,
therefore with 8 valence e-, the Noble gases do not form ions.
12. Will the shielding effect be more noticeable in metals or non metals? Explain your answer.
When comparing metals and nonmetals across the same period, the metals will have the more
noticeable shielding affect. As you move across the PT, the number of p+ in the nucleus
increases thus increasing the nuclear charge of the atom. The shielding effect of the inner core e-
becomes less noticeable with the nonmetals because the valence e- are pulled more tightly
towards the nucleus.
SCPS Chemistry Worksheet – Periodicity -
page 7
13. Why do elements in the same family generally have similar properties? Choose one as an
example to support your reasoning.
Halogens Family – The number of valence e- determine the element’s chemical properties such
as reactivity. Each member of the halogen family has 7 e- in its valence shell. Therefore, the
members of the halogen family all have similar chemical properties.
14. Arrange each of the following in order of increasing ionization energy and explain your
reasoning: Calcium, iron, copper, bromine and krypton.
Calcium, copper, iron, bromine, krypton.
15. Factors affecting ionization
energy include nuclear charge, the
shielding effect, the atomic radius
Ar
and the electron arrangements in a
IE
sublevel. Use the appropriate
factors to explain the overall trend
indicated by the dark line and the
exceptions to it in the graph (light
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