Rules
 Answers must be in the form of a question.
 Only one person per group may raise their hand per
question.
 Challenging Alex (me) will be a bad decision and make
you cry when you lose 1000 points.
 Keep the commotion to a minimum between
questions, I wont repeat.
 Incorrect answers will cost you points, correct answers
will earn you points.
Periodic
Trends
Lewis Dot
Groups
Periodic
Table
Mixed Bag
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Periodic Trends - 100
 This trend measures ½ the diameter between the
nuclei of two identical atoms.
Periodic Trends - 100
 Answer: What is atomic radius
Periodic Trends - 200
 This is the trend of atomic radius as you go across
period 3, starting with Na.
Periodic Trends - 200
 Answer: What is decreases
Periodic Trends - 300
 This phenomenon explains why first ionization energy
decreases down a group.
Periodic Trends - 300
 Answer: What is shielding
Periodic Trends - 400
 This element has the largest electronegativity
Periodic Trends – 400
 What is Fluorine
Periodic Trends - 500
 These types of ions have larger radii than their atomic
counterpart
Periodic Trends - 500
 What are anions
Lewis Dot - 100
 The dots in the Lewis Dot structure represent these.
Lewis Dot - 100
 What are valence electrons
Lewis Dot - 200
 A stable atom will have this many valence electrons.
Lewis Dot - 200
 What is 8
Lewis Dot - 300
 This is the Lewis Dot structure of an atom of Nitrogen.
Lewis Dot - 300
Lewis Dot - 400
 This is the Lewis Dot structure of an atom of Iodine.
Lewis Dot - 400
Lewis Dot - 500
 This would be the Lewis Dot structure of an ion of Na
with a charge of +1.
Lewis Dot - 500
 Answer:
 G or no dots.
Groups - 100
 This group is composed of elements that are all soft
silvery solids at room temperature and form ions with
a charge of +1.
Groups - 100
 What are the alkali metals.
Groups - 200
 The elements from this group are the most reactive
nonmetals.
Groups - 200
 What are the Halogens
Groups – 300
 This group of elements are non-reactive gases.
Groups - 300
 What are the Noble Gases
Groups – 400
 This metal often forms blue or green colored
compounds because it is an example of a transition
metal.
Groups - 400
 What is Copper
Groups - 500
 These elements are sometimes called inert.
Groups - 500
 What are the Noble Gases.
Periodic Table – 100
 These metals all have very high melting points and
form ions with a charge of +2.
Periodic Table - 100
 What are the alkaline earth metals.
Periodic Table - 200
 This nonmetal is a reddish liquid at room temperature.
Periodic Table - 200
 What is bromine
Periodic Table - 300
 This metal is a silvery liquid at room temperature.
Periodic Table - 300
 What is mercury.
Periodic Table – 400
 This element is a solid at room temperature but can
sublime.
Periodic Table – 400
 What is iodine
Periodic Table – 500
 These two elements are exceptions to the octet rule
Periodic Table - 500
 What are H and He.
Mixed Bag – 100
 Elements that share this in common all have valence
electrons in the same energy level.
Mixed Bag - 100
 What is period number
Mixed Bag - 200
 This property measures an atoms desire/draw for
electrons.
Mixed Bag - 200
 What is electronegativity
Mixed Bag - 300
 This element is considered an noble gas with only two
valence electrons.
Mixed Bag - 300
 What is He
Mixed Bag – 400
 This element was the unknown in the Emission
Spectra lab.
Mixed Bag – 400
 What is mercury
Mixed Bag - 500
 The elements of this group all have 5 valence electrons.
Mixed Bag – 500
 What is the nitrogen family.
Bonding
Ionic
Compounds
Oxidation
Practice
Questions
Practice
Questions 2
100
100
100
100
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200
200
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500
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Bonding - 100
 These electrons are involved in bonding
Bonding – 100
 What are valence
Bonding - 200
 These elements all have a desire to gain an electron so
they readily bond with metals.
Bonding - 200
 What are the Halogens
Bonding - 300
 These elements normally do not bond with other
elements to form compounds
Bonding - 300
 What are the Noble Gases
Bonding - 400
 These elements have varying numbers of valence
electrons and can form ions with a variety of charges.
Bonding – 400
 What are transition metals
Bonding – 500
 Valence electrons that are shared between two atoms
for this type of bond.
Bonding – 500
 What is covalent
Ionic Compounds - 100
 Ionic compounds are usually formed between one or
these and one of these types of elements.
Ionic Compounds – 100
 What is a metal and a nonmetal.
Ionic Compounds – 200
 This type of bond involves a transfer of electrons from
one atom to another.
Ionic Compounds – 200
 What is an ionic bond
Ionic Compounds – 300
 The product of ionic bonds are usually these. An
example is table salt.
Ionic Compounds – 300
 What is a crystal solid.
Ionic Compounds – 400
 The metal involved in the ionic compound forms this
type of ion (name of the ion).
Ionic Compounds – 400
 What is a cation
Ionic Compounds – 500
 This nonmetal is one of the few that can potentially
conduct electricity.
Ionic Compounds – 500
 What is carbon
Oxidation – 100
 The number of valence electrons lost, gained or shared
during bonding are called this.
Oxidation – 100
 What is oxidation number
Oxidation – 200
 This is true of the charge of all ionic compounds.
Oxidation – 200
 What is neutral.
Oxidation – 300
 If Na bonds with S, this would be a resulting neutral
compound.
Oxidation – 300
 What is Na2S
Oxidation – 400
 If Cu (VI) and O bond this would be the formula of the
resulting compound.
Oxidation – 400
 What is CuO3
Oxidation – 500
 This is the name of the compound (NH4)(No3)
Oxidation – 500
 What is ammonium nitrate.
Practice - 100
 What of the following elements has the greatest
metallic character:
 Na
 Cs
 Cu
 O
Practice – 100
 Na
Practice – 200
 This element has the largest electronegativity:
 Na
 Rb
 Se
 F
Practice – 200
 What is F
Practice – 300
 This element has the largest atomic radius:
 K
 Ca
 Rb
 Sr
Practice – 300
 What is Rb
Practice – 400
 This element has the largest first ionization energy:
 Be
N
 O
 Ne
Practice – 400
 What is Ne
Practice – 500
 This element would form ions with the largest ionic
radius:
 F
 Mg
 Be
 Li
Practice – 500
 What is F
Practice 2 – 100
 This element is the most stable:




H
He
Li
Be
Practice 2 – 100
 What is He
Practice 2 – 200
 This element may have properties of both metals and
nonmetals:
 Ge
 P
 Al
 Fe
Practice 2 – 200
 What is Ge
Practice 2 – 300
 This element has atoms with the largest atomic radius:
 Ni
 Cu
 Zn
 Ga
Practice 2 – 300
 What is Ni
Practice 2 – 400
 These phenomenon explains why Ni has a larger
atomic radius than Zn.
Practice 2 – 400
 What is nuclear charge and being in the same period
Practice 2 – 500
 This element has the strongest pull for electrons
 O
P
 Sr
 Fr
Practice 2 – 500
 What is O