WLHS / Chem / Monson
Name
Date
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CHAPTER 6 READING GUIDE: The Periodic Table and Periodic Trends
6.1 - Organizing the Elements (p. 160-166)
1) Study Figure 6.2 on page 161. What criteria did Mendeleev use in placing elements into rows on his
Table?
A= Mendeleev arranged the elements in his periodic table in order of increasing atomic mass
2) In this table, which 2 elements are in the same horizontal row as fluorine and chlorine?
A= Fluorine: oxygen and neon Chlorine: Sulfur and Argon
3) How are elements arranged in the modern periodic table?
A= in the modern periodic table, elements are arranged in order of increasing atomic number
4) What are horizontal rows called?
Period
How many are there? seven
5) How many elements are in:
period 1: 2 Hydrogen and helium
period 4: 18 [Potassium-Krypton
period 2: 8 [lithium-Neon]
period 3: 8 [Sodium-argon]
]
6) Summarize the periodic law:
When elements are arranged in order of increasing atomic number, there is a periodic repetition of their
physical and chemical properties
7) As a result of the arrangement of elements into periods, what can we say about elements that end up
in the same vertical column?
A= within a column or group elements have same physical and chemical properties
Category:
Properties?
They are good conductors of heat, it has high luster surface all
metals are solid at room temperature except for mercury, they
can reflect light, ductile, malleable, crystal or amorphous
structure.
Chemical:
Metals in G1 and G2 are very reactive. Transition metals are
the less reactive
Examples
Sodium, Iron
and magnesium
Metals
Where on table?
They are located
Between group 1
and group 12
includes alkali,
alkaline earth and
transition metals
Most nonmetals are gases at room except from bromine which
is liquid temperature they are poor conductors of electricity and
heat, they have odor
Carbon, Neon
and Fluorine
Nonmetals
They are located
from group 14 to 18
includes nonmetals
and noble gases
including Hydrogen
Metalloids
They are located
from G13 to G17 in
form of a stair case
between other
metals and
nonmetals.
Chemical G18 contains the less reactive and G17 contains the
most reactive elements forming compound in the environment.
They generally have the similar properties that metals and
nonmetals have under certain conditions they can have metal
properties and under other conditions they might have
nonmetal.
Boron, Silicon
and Arsenic
8) Complete the chart below summarizing the 3 broad classes of elements.
6.2 - Classifying the Elements (p. 167-173)
9) What chemical properties do the noble gases share and how does this relate to their electron
configuration?
A= Noble gases are unreactive (inert). They have 8 electrons in their valence shell or outermost energy
level (stable octet).
10) For each element tell which period and group the element is in, identify the element, and state
whether it is a metal, nonmetal, or metalloid.
Element
Period
Group
Identity
Metal, nonmetal,
metalloid?
#34
#40
#14
#56
4
5
3
6
16
4
14
2
symbol Se and atomic number 34.
Symbol Zr atomic number 40
Symbol Si atomic number 14
Symbol Ba atomic number 56
Nonmetal
Metal
Metalloid
Metal
#18
#4
#82
#37
3
2
6
5
18
2
14
1
Symbol Ar atomic number 18
Symbol Be atomic number 4
Symbol Pb atomic number 82
Symbol Rb atomic number 37
Nonmetal
Metal
Metal
Metal
11) Classify the following as metals, nonmetals, or metalloids:
A) Manganese:
metal
D) nitrogen:
nonmetal
B) Arsenic:
metalloid
E) niobium:
metal
C) carbon:
nonmetal
F) radium:
metal
12) Iodine is used in many commercial chemicals and dyes. To what family does it belong? What are the
other members of this family? How many electrons are in the outermost energy level (valence
electrons)?
A= Iodine belongs to group 17 and it belongs to the halogens family, the other member contain fluorine,
chlorine, bromine and astatine, and they have 7 valence electrons in the last level of energy or shell.
6.3 – Periodic Trends (p. 174-183)
13) Explain WHY as you go down the periodic table, within a group, atomic radius increases.
A=
14) Explain why Cl (#17) is smaller then S (#16) considering it has one more proton than sulfur.
15) Arrange these elements in order of DECREASING atomic size:
A) S, Cl, Al, Na, Si, Mg, Ar, P: Na, Mg, Al, Si, P, S, Cl, Ar
B) Sb, Sr, Te, I, In, Xe, Rb: Rb, Sr, In, Sb, Te, I, Xe
C) Se, Po, O, S, Te: Po, Te, Se, S, O
D) Cs, Na, Li, H, Fr, Rb, K: Fr, Cs, Rb, K, Na, Li, H
16) Which element in each pair has the greater atomic radius (size)?
A) SODIUM or LITHIUM
D) STRONTUIM or MAGNESIUM
B) CARBON or GERMANIUM
E) SELENIUM or OXYGEN
C) BROMINE or FLUORINE
F) BISMUTH or THALLIUM
17) What is a CATION? A cation is a positively charged ion, i.e one that would ne attracted to the
cathode in electrolysis.
How does a CATION form? A cation forms when an atom losses one or more e- from its electron cloud
18) What is an ANION? An anion is an atom that has more electrons than protons, in other words, an
anion is an atom with a negative charge
How does an ANION form? An anion forms when ana atom gains one or more e- in its electron cloud.
19) Define IONIZATION ENERGY and describe its trend on the periodic table. (what happens and
WHY?) ionization enery is the quantity of energy that an isolated, gaseous atom, in the ground electronic
state must absorb to discharge an electron, resulting a cation
20) Which element in each pair has the LARGER ionization energy? (circle)
A) BORON or NITROGEN
D) ALUMINUM or SODIUM
B) FLUORINE or CHLORINE
E) CARBON or SILICON
C) BARIUM or CALCIUM
F) CHROMIUM or COBALT
21) How does the radius / size of a typical ANION compare with the radius / size of its corresponding
neutral atom? EXPLAIN why this trend is observed.
22) Arrange the following elements in order of INCREASING ionization energy:
A) Ba, Be, Mg, Ca, Sr:
B) Bi, Pb, Cs, At, Ba:
C) Na, P, Al, Cl, Mg, S:
D) Rb, Na, K, Cs, Li:
E) Te, S, O, Po, Se:
23) Define ELECTRONEGATIVITY and describe its trend on the periodic table. (what happens and
WHY?)