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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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