Unit 4 Question Packet
The Periodic Table
SKILLS
1. identifying PROPERTIES OF METALS,
METALLOIDS, & NONMETALS
2. identifying GROUP PROPERTIES
3. classifying elements
Name …………………KEY………………………
Period ………….
4. identifying PROPERTIES OF ELEMENTS
5. explaining PROPERTIES OF ELEMENTS
6. identifying TRENDS IN THE PERIDIOC TABLE
SKILL #1:
Identifying PROPERTIES OF
- refer to your notes & RB p. 19-25
METALS, METALLOIDS, & NONMETALS
1. Write in the space, “metals”, “metalloids”, or “nonmetals” to indicate which type of
element each statement is describing.
a. metals
Located on the left side of the P.T.
b. nonmetals
Located on the right side of the P.T.
c. nonmetals
Solids are brittle
d. metals
Majority of the elements
e. nonmetals
Gain electrons to form negative ions
f.
metalloids
Located along the “staircase”
g. metals
Have luster
h. metals
Malleable
i.
metals
Lose electrons to form positive ions
j.
metals
Ductile
k. metals
Excellent conductors of heat & electricity
l.
nonmetals
Poor electrical & heat conductors
m. metals
Low electronegativity values
n. metals
Low ionization energy
o. nonmetals
High ionization energy
p. nonmetals
High electronegativity values
q. nonmetals
Ions are larger than their atoms
r.
metals
Ions are smaller than their atoms
SKILL #2:
Identifying GROUP PROPERTIES
- refer to your notes & RB p. 19-25
2. Write in the space, “Group 1 metals”, “Group 2 metals”, “transition metals”, “halogens”,
or “noble gases” to indicate which group each statement is describing.
Colored solutions
a. Transition metals
Full valence shell
b. Noble gases
Most active metals
c. Group 1 metals
Most active nonmetals
d. Halogens
Monatomic gases
e. Noble gases
Halogens
Diatomic elements
f.
Stable and unreactive
g. Noble gases
7 valence electrons
h. Halogens
Group 2 metals
2 valence electrons
i.
Group 1 metals
Form ions with a +1 charge
j.
SKILL #3:
Classifying elements
- refer to your notes, RB p. 19-25, & the P.T.
3. Check all the boxes which describe the element.
Metal
Sb
Sr
Rn
P
Pt
Cs
S
Fe
Br
Ar
H
Si
B
F
He
Se
Zn
Ra
SKILL #4:
Metalloid
Nonmetal
Group
1
Group
2
Transition
metal
Halogen
Noble
gas
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Diatomic
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Monatomic
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identifying PROPERTIES OF ELEMENTS
– use your notes, RB p. 19-25, Table S & the P.T.
4. Use Table S to fill in the names and states of each element below. Then, check all the
boxes which describe the element.
Physical Properties
Name
C
carbon
Ag
silver
Mg magnesium
I
iodine
S
sulfur
Au
gold
Fe
iron
Br
bromine
Ar
argon
H
hydrogen
Hg
mercury
Se
selenium
F
fluorine
He
helium
State at STP
(s, l, or g)
s
s
s
s
s
s
s
l
g
g
l
s
g
g
Brittle
Malleable
/ductile
Conductor
Good
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Poor
Chemical Properties
Ionization
ElectroElectrons
energy
negativity
Low High Low High Lose Gain
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5. Describe one chemical property of Group 1 metals that results from the atoms of each
metal having only one valence electron. form 1+ ions; react vigorously with water;easily lose
one electron
SKILL #5:
explaining PROPERTIES OF ELEMENTS
6. Given:
– use your notes, RB p. 19-25 & the P.T.
Samples of Na, Ar, As, Rb
a. Which two of the given elements have the most similar chemical properties?
Na and Rb
b. Explain your answer in terms of atomic structure.
They have the same number of valence electrons
7. Given:
Samples of sulfur, oxygen, and phosphorus
a. Which two of the given elements have the most similar chemical properties?
sulfur and oxygen
b. Explain your answer in terms of atomic structure.
They have the same number of valence electrons
8. Based on the Periodic Table, explain why Na and K have similar chemical properties. [1]
They have the same number of valence electrons
form 1+ ions
are located in same group
9. Explain the following in terms of atomic structure:
a. Cesium has a larger atomic radius than rubidium.
(same group) Cesium has more shells of electrons
b. Cesium has a lower first ionization energy than rubidium.
(same group) Cesium has more electron shells, easier to remove electrons
c. Bromine has a lower first ionization energy than chlorine.
(same group) Br has more electron shells – easier to remove electrons
d. The atomic radius of copper is 128 picometers while Ag has an atomic radius of
144 picometers.
(same group) Ag has one more shell of electrons, so it is larger than Cu
e. The atomic radius of lithium is 155 pm while neon has an atomic radius of 51 pm.
(same period) Neon has more protons in its nucleus which pull the e-‘s in closer.
f.
Lithium has a lower first ionization energy than beryllium.
(same period) Lithium has one less proton in its nucleus, so it’s easier to pull an eaway
g. Chlorine has a greater electronegativity than sulfur.
(same period) Chlorine has one more proton in its nucleus, so it’s better at
attracting electrons
h. Potassium has a lower first ionization energy than calcium.
(same period) K has one less proton in its nucleus, so it’s easier to pull an e- away
SKILL #6:
identifying TRENDS IN THE PERIDIOC TABLE
– refer to your notes, RB p. 26-28, Table S,
and the P.T.
10. Base your answers to the following questions on the information below.
a. Complete the table above.
b. On the grid below, mark an
appropriate scale on the axis
labeled “First Ionization Energy
(kJ/mol).” An appropriate scale is
one that allows a trend to be seen.
c. On the grid, plot the data from the
table. Circle and connect the
points.
First Ionization Energy of Group 1 Elements
Element
Atomic First Ionization Energy
Number
(kJ/mol)
lithium
3
520
sodium
11
496
potassium
19
419
rubidium
37
403
cesium
55
376
d. State the trend in first ionization
energy for the elements in the table
as atomic number increases. [1]
Ionization energy decreases.
11. Complete the table below by checking the appropriate boxes.
Remember the snow-woman “AMIE”
Across a Period 
Increases
Decreases
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Atomic radius
Metallic character
Ionization energy
Electronegativity
Why?
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# of protons
increases
Down a Group 
Increases
Decreases
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# of electron shells
increases
12. Complete the statements below by checking the correct ending.
(hint: use Table J for e and f)
increases
a.
b.
c.
d.
e.
f.
As the elements in a Period are considered from left to right, the
number of valence electrons in each successive element…
As the elements in Group 17 are considered from top to bottom,
the number of valence electrons in each successive element…
Going left to right across a Period, the number of electron
shells…
As the elements in a Group are considered from top to bottom,
the number of electron shells…
As the elements in Group 1 are considered from top to bottom,
the reactivity of each successive element….
As the elements in Group 17 are considered from top to bottom,
the reactivity of each successive element…
decreases
remains
the same
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