Transcript Jeopardy - Chemistry Unit 4- back-up copy

Let’s Play
Sit in teams of 4.
Periodic TableHistory and
Organization
Periodic
Families
What is my
size?
Giving up
electrons
I love electrons!
Potpourri
Periodic
Table- History
and
Organization
Periodic
Families
What is my
size?
Giving up
electrons
I love
electrons!
Potpourri
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$100
He is sometimes
called the “father
of the Periodic
Table”
Mendeleev
$200
On the original
periodic table,
elements were
organized by similar
properties and this
Atomic mass
(or weight)
$300
These are the two ways
elements on the modern
periodic table are
organized
Similar properties
and atomic
number
$400
The names given to rows
and columns on the
periodic table
Periods (rows)
and groups
(columns)
$500
These elements tend to
lose electrons and are
found on the left side of
the periodic table
Metals
$100
Lithium is a member of this
family of highly reactive metals
Alkali metals
$200
Chlorine is a member of
this family
Halogens
$300
Xenon is a member of
this family
Noble Gases
$400
Atoms of elements in
this family tend to lose
two electrons
Alkaline Earth
Metals
$500
Thorium is a member of
this family
Actinide Family
$100
Which has a smaller
ionic radius, cesium or
potassium?
Potassium
$200
How does a neutral
atom compare in size
to its cation?
The neutral atom
is larger; the
cation is smaller
$300
Why is an anion larger
than its neutral atom?
The anion has more
electrons that repel
each other and
cause the electron
cloud to expand
$400
What is the general trend
for atomic radii as you
move from left to right
across a row on the
periodic table and why?
Atomic radius
decreases; increasing
nuclear charge pulls
electrons is closer
$500
What is the reason for
the difference in size
between a neutral
atom and its cation?
The cation has
lost (electrons) an
entire energy level
$100
What is the general
trend in ionization
energy as you move
down a group on the
periodic table?
Ionization energy
decreases
$200
What is the general
trend in ionization
energy as you move
across a period from left
to right?
IE increases
$300
What is the difference
between first, second,
and third ionization
energies?
st
1
nd
IE<2
rd
IE<3
IE
st
Or 1 IE= energy to remove
nd
the first electron, 2 is to
remove the second, etc.
$400
Why is the first
ionization energy for
sodium so much lower
than the first ionization
energy for magnesium?
Sodium has 1 valence electron in the 3s sublevel,
and it wants to lose this electron. Magnesium has
two electrons in the 3s sublevel so this sublevel is
completely filled. It requires a lot more energy to
remove an electron from a full sublevel.
Daily
Double!
Daily
Double!
Why is the third ionization energy
for beryllium significantly higher
than its second ionization
energy?
Beryllium has 2 valence electrons in a
2s subshell. Once it has lost two
electrons (2nd IE), it has lost an entire
energy level and has a noble gas
electron configuration. The 3rd IE
involves removing one of the core
electrons from a stable noble gas
configuration which requires
significantly more energy. Also the
protons have a much stronger pull on
the remaining electrons.
$100
The measure of the ability of an atom
in a chemical compound to attract
electrons from another atom in the
compound is called this.
Electronegativity
$200
Why does electronegativity
increase as you move from
left to right on the periodic
table?
Effective nuclear charge
increases and radius
decreases, increasing the
force/pull of the nucleus on
electrons
$300
What is the name for the energy
released when an electron is added
to an atom?
Electron affinity
$400
What is the most
electronegative
element?
Fluorine
$500
Why are valence
electrons of larger
atoms less
atttracted to the
nucleus?
Shielding effect (more core
electrons blocking their “view”)
or greater distance = lower
Coulombic force
$100
These are the
most reactive
metals
Alkali metals
$200
The outer shell
electrons involved
in bonding are
called this.
Valence electrons
$300
Metals tend to
___________ electrons to
become ___________
Lose, cations
$400
Put the following atoms in
order from lowest to highest
ionization energy (first IE)
Ba, Cu, Ne
Ba<Cu<Ne
$500
Put the following atoms in
order from smallest to the
largest ionic radii.
K, Mg, P
P<Mg<K
Final
Jeopardy
Periodicity
The shielding effect is
one of the three primary
factors that affect the
periodic trends. Name or
describe the other two.
1. Nuclear charge
(number of protons in the
nucleus)
2. Highest energy level (or
number of energy levels)
Daily
Double!