regions
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Regions. Scientists. Families. Vocab. Trends. Grab Bag. Regions. Scientists. Families. Vocab. Trends. Grab Bag. $100. $100. $100. $100. $100. $100. $200. $200. $200. $200. $200. $200. $300. $300. $300. $300. $300. $300. $400. $400. $400. $400. $400. $400. $500. - PowerPoint PPT PresentationTRANSCRIPT
Regions
Scientists
Families
Vocab
Trends
Grab Bag
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Name 4 characteristics
of metals.
Shiny, malleable, ductile, and conductive
What region of theperiodic table do
metals react with inorder 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 scientistswho contributed to the periodic table, in order.
Newlands, Mendeleev,and Moseley
Who arranged the periodic table by atomic number?
Henry Moseley
Who was the firstscientist to arrange the
periodic table by properties and
the Law of Octaves?
JohnNewlands
Whose contribution was significant because he had better technology
available to him?
Henry Moseley
Who left gapsin 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 metalsand halogens
Which family has 7 valence electrons? Give
a noble gas configuration of any one of them to demonstrate.
halogens
DefineOctet Rule.
The tendency of atoms to gain or lose electrons in order to become stable
(refers mainly to filling the
s and p orbitals.
Defineionization energy.
The energy requiredto remove an electron.
Define electron affinity.
The amount of energyreleased when an atom
gains an electron.
Definenuclear 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 theperiodic table is ionization energy
the greatest?
Top right.
Which trendincreases down a group but has no
change across a period?
The shielding effect. (electron shielding)
Explain why atomicradius decreasesacross a period.
The nuclear chargeincreases, and electronsare added to the sameenergy level, so the attraction is greater.
Why does electronshielding increase
down a group?
Core electrons are addedand the valence
electrons are further from the nucleus.
Which atom has alower ionization energy:silver (Ag), arsenic (As),
or strontium (Sr)? Explain your answer.
Strontium, b/c it has more e- shielding than arsenic, and agreater desire to lose an e-
than silver because it wants to acquire a noble gas config.
Which family tendsto 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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