Transcript Jeopardy Ch 4

Regions
Scientists
Families
Vocab
Trends
Grab Bag
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Name 4
characteristics
of metals.
Shiny, malleable,
ductile, and
conductive
What region of the
periodic table do
metals react with in
order to become
stable?
The nonmetals
Walk up to the periodic
table and point out ALL
the metals.
Potassium has
properties most
similar to calcium,
argon, or rubidium
Rubidium because
elements are most
similar to those in the
same group.
Write a noble gas
configuration for a
d-block element of
your choice
Use a noble gas in
brackets, then read the
next line on the periodic
table until you get to the
element.
Name the 3 scientists
who contributed to the
periodic table, in order.
Newlands,
Mendeleev,
and Moseley
Who arranged the
periodic table by
atomic number?
Henry Moseley
Who was the first
scientist to arrange the
periodic table by
properties and
the Law of Octaves?
John
Newlands
Whose contribution was
significant because he
had better technology
available to him?
Henry Moseley
Who left gaps
in the periodic
table and predicted
properties of
elements?
Dmitri
Mendeleev
Walk up & point to the
families on the periodic
table in order from
left to right & top
to bottom.
alkali metals, alkali-earth,
transitions, halogens,
noble gases,
lanthanides, actinides
Which family is
slightly harder,
denser and less
reactive than the
alkali metals?
Alkaline earth
metals
Which group has a small
peak on an ionization
energy graph due to a
half full orbital?
Group 15
Which 2 families
are the most
reactive?
Alkali metals
and halogens
Which family has 7
valence electrons? Give
a noble gas
configuration of any one
of them to demonstrate.
halogens
Define
Octet Rule.
The tendency of atoms to
gain or lose electrons in
order to become stable
(refers mainly to filling the
s and p orbitals.
Define
ionization energy.
The energy required
to remove an electron.
Define
electron affinity.
The amount of energy
released when an atom
gains an electron.
Define
nuclear charge.
The charge/strength
of the protons in
the nucleus.
Shielding
effect
The reduction in
attraction between the
valence e and the
nucleus due to the
interference of the core e
Where on the
periodic table is
ionization energy
the greatest?
Top right.
Which trend
increases down a
group but has no
change across a period?
The shielding effect.
(electron shielding)
Explain why atomic
radius decreases
across a period.
The nuclear charge
increases, and electrons
are added to the same
energy level, so the
attraction is greater.
Why does electron
shielding increase
down a group?
Core electrons are added
and the valence
electrons are further
from the nucleus.
Which atom has a
lower ionization energy:
silver (Ag), arsenic (As),
or strontium (Sr)? Explain
your answer.
Strontium, b/c it has more eshielding than arsenic, and a
greater desire to lose an ethan silver because it wants to
acquire a noble gas config.
Which family tends
to have a +2 charge?
Alkaline-Earth Metals
Why does group 16
have a -2 charge?
Group 16 wants to
gain 2 e to fill it’s
octet.
Draw arrows on the
board to represent the
increase in the trend of
atomic radii.
Should look like 9:30 on
a clock higher on the
right and higher at the
bottom
Which family has the
most negative electron
affinity values?
halogens
Although Xenon is a
noble gas, it has reacted
with other nonmetals.
He, Ne, and Ar have
not. How is this
possible?
Because it is so far down
the group, electron
shielding has permitted
highly electronegative
atoms to take a valence
electron.
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