Test Review – Periodic Table
Unit 2 Section A
Use your periodic table to enter the symbol of the element for each of the
following questions.
The name given to all the
elements on the left side of the
periodic table which have from 1
to 3 valence electrons, conduct
electricity and heat, are malleable
and ductile.
Metals
The name given to all the
elements on the right side of the
periodic table which have from 5
to 7 valence electrons, do not
conduct electricity or heat, and
are brittle in texture.
Nonmetals
The name given to all the
elements on the border of metals
and nonmetals which are not
malleable or ductile, and
sometimes can conduct
electricity (semiconductors)
Metalloids
The vertical columns of the
periodic table. These groups
share common characteristics
and are placed in these columns
by their number of valence
electrons.
Families (groups)
The horizontal rows of the
periodic table. These tell the
number of electron shells or
energy levels for each element.
Periods
The name given to the electrons
found in the outside shell of each
atom.
Valence electrons
These are the group IA elements
with 1 valence electron in their
outside shell.
Alkali metals
These are the group IIA elements
with 2 valence electrons in their
outside shell.
Alkali Earth Metals
These are the group VII A
elements with 7 valence
electrons in their outside shell.
Halogens
These are the group VIII A or
group 0 elements with 8 valence
electrons in their outside shell.
They have filled outside shells
and are inert.
Noble Gases
These are the Group B metals.
They are not very reactive and
their valence
electrons can change from 1 to 3.
They resist corrosion and are
used for coins and jewelry.
Transition metals
These groups include large
elements which are sometimes
radioactive and some are
synthetically made.
Rare earth metals
The family of most reactive
metals.
Alkali metals
The family of most reactive
nonmetals
Halogens
The family of least reactive
elements all of which are gases.
Noble gases
Examples of this family
include Be, Mg, and Ca.
Alkali earth metals
Examples of this family
include Cl, Br, F, and I
Halogens
Examples of this family include
Cu, Ag, Au, Fe, and Zn.
Transition metals
Examples of this family
include He, Ne, Ar, and Kr.
Noble gases
Examples of this family
include Li, Na, and K
Alkali metals
Examples of this family include
Uranium, Plutonium, and Curium.
Rare earth metals
Examples of this family
include B, Si, As, and Ge,
Metalloids
Name the halogen in period 4.
Name the halogen in period 4.
Name the halogen in period 4.
Br
Name the alkali metal in
period 2.
Name the alkali metal in period 2.
Name the alkali metal in period 2.
Li
Name an element with
properties similar to Neon.
Name an element with properties
similar to Neon.
He, Ar, Kr, Xe, or Rn
Which element has 8 protons?
Which element has 8 protons?
O
Which element has 20
electrons?
Which element has 20 electrons?
Ca
Which element has 24
neutrons?
Which element has 24 neutrons?
44.956 = 45
45 – 21 = 24
Sc - Scandium
44.956 = 45
45 – 21 = 24
Which element has an atomic
mass (weight) closest to 56?
Which element has an atomic mass
(weight) closest to 56?
Fe
Name the alkaline earth metal
in period 3.
Name the alkaline earth metal in
period 3.
Mg
Which period 3 element is the
most reactive metal?
Which period 3 element is the most
reactive metal?
Na
Which period 2 element is the
most reactive nonmetal?
Which period 2 element is the most
reactive nonmetal?
F
Which element has 2 more
protons than Iron?
Which element has 2 more protons
than Iron?
Iron = Fe = 26
26 + 2 = 28
Ni
Iron = Fe = 26
26 + 2 = 28
What is the least reactive
period 4 element?
What is the least reactive period 4
element?
Kr
Which two elements are in the
same family and have properties
most similar to Zinc?
Which two elements are in the
same family and have properties
most similar to Zinc?
Cd and Hg
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Alkali Metals:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Alkali Metals:
1) 1
2) IA
3) Most reactive metals; combine
with Halogens
4) Na, K
5) Outer e- config: *s1
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Alkali Earth Metals:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Alkali Earth Metals:
1) 2
2) IIA
3) +2 charge
4) Ca, Mg
5) Outer e- config: *s2
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Transition Metals:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Transition Metals:
1) 1-3
2) Group B
3) Valence varies, resist corrosion
4) Cu, Ag, Au, Zn, Fe
5) Sublevel orbital block = d
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Rare Earth Metals:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Rare Earth Metals:
1) 1-3
2) Group B
3) Large, synthetic, radioactive
4) U, La, Ac
5) Sublevel orbital block = f
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Metalloids:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Metalloids:
1) 3-7
2) IIIA-VIIA
3) Semi-metals, Semiconductors
4) Si, B, As
5) Outer e- config: *s2 *p1 - *s2 *p5
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Halogens:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Halogens:
1) 7
2) VIIA
3) Most reactive nonmetals
4) Cl, Br
5) Outer e- config: *s2 *p5
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Noble Gases:
1)
2)
3)
4)
For each of the following Groups (Families) state;
1) The # of valence e-,
2) The Group #,
3) Defining characteristics,
4) Example
Noble Gases :
1) 8
2)
VIIIA or 0
3) Inert, least reactive
4) Ne, Kr
5) Outer e- config: *s2 *p6
• Explain how the sizes of atomic radii
change as you travel down and across
the periodic table:
• Explain how the sizes of atomic radii
change as you travel down and across
the periodic table:
• Sizes increase going down table
• Sizes decrease going left to right
Size increases going down table
Size decreases going left to right
Smallest
Largest
Place these elements in order of increasing atomic radii size:
P, Cl, Fr, Mg, K =
Place these elements in order of increasing atomic radii size:
P, Cl, Fr, Mg, K = Cl,
P, Mg, K, Fr
• Explain how the electronegativity of
atom change as you travel down and
across the periodic table:
• Explain how the electronegativity of
atom change as you travel down and
across the periodic table:
• Electronegativity decreases going
down table
• Electronegativity increases going left to
right
Electronegativity decreases going down table
Electronegativity increases going left to right
Highest
Lowest
Place these elements in order of decreasing electronegativity:
Ca, Br, As, Cl, Rb =
Place these elements in order of decreasing electronegativity:
Ca, Br, As, Cl, Rb = Cl,
Br, As, Ca, Rb
• Which two Groups (families) are most
reactive and why?
• Which two Groups (families) are most
reactive and why?
• 1) Alkali metals – Group 1A – only 1
valence electron
• 2) Halogens – Group VII A – 7 valence
electrons
• What is the main property of noble
gases and why?
• What is the main property of noble
gases and why?
• Inert – Don’t react
• 8 valence electrons (octet) in outside shell,
filled outer shells.
• Why do all elements in a group (or
family) have similar properties?
• Why do all elements in a group (or
family) have similar properties?
• Same number of outside or valence
electrons, so same reactivity.