CHEMISTRY
I.
STUDY GUIDE
NAME: _________________________
DATE: __________________________
PERIOD: _________________________
Chapter 6
THE PERIODIC TABLE AND PERIODIC LAW
DEVELOPMENT OF THE MODERN PERIODIC TABLE - 6.1
A.
Development of the Periodic Table
1.
John Newlands (1837 - 1898)
a.
How did John Newlands organize the elements?
Arranged elements by increasing atomic mass. Created the law of Octaves. p.176.
2.
Meyer and Mendeleev
a.
How did Mendeleev (1834-1907) organize the elements?
Arranged the elements in order of increasing atomic mass. p.176.
3.
Mosley (1887 - 1915)
a.
Mosley arranged the elements in order of increasing
atomic number and not by increasing atomic mass
as Mendeleev proposed.
b.
B.
Please Define Periodic Law: States that when the elements are arranged by
increasing atomic number, there is a periodic repetition of their properties.
The Modern Periodic Table
1.
What are vertical columns called in the Periodic Table?
a.
Groups 1-18
b.
Family Names (Group 1-alkali metals, Group 2-alkaline earth metals, Group 13-Boron
Family, Group 14-Carbon Family, Group-15 Nitrogen Family, Group-16 Oxygen Family,
Group 17-Halogen Family, Group 18-Noble Gas or Inert Gas Family.
2.
What are the horizontal row called in the Periodic Table?
a.
Periods 1-7
b.
Series Names (Period-6 Lanthanide series, Period-7 Actinide series)
3.
Please Define Representative Elements: Elements from groups 1, 2, and 13-18 in the
modern periodic table, possessing a wide range of chemical and physical properties.
4.
Please Define Transitional Elements: Elements in groups 3-12 of the modern periodic
table and are further divided into transitional metals and inner transition metals.
5.
Metals
a.
Please Define Metal: An element that is solid at room temperature, a good
conductor of heat and electricity, and generally is shiny; most metals are ductile
(made into wire) and malleable (can be bent into shapes).
b.
Please Define Alkali Metals: Group 1 elements, except for hydrogen, they are
very reactive, most active metals, and usually exist as compounds with other
elements.
-2-
6.
7.
II.
c.
Please Define Alkaline Earth Metals: Group 2 elements in the modern
periodic table and are highly reactive.
d.
Please Define Transition Metals: The elements in groups 3-12 that are contained
in the d-block of the periodic table and with some exception is characterized by
a filled outermost s orbital of energy level (n), and filled or partially filled d orbitals
of energy level n-1. Atoms have multiple oxidation numbers.
e.
Please Define Inner Transition Metals: A type of B element that is contained in the
f-block of the periodic table and is characterized by a filled outermost orbital and
filled or partially filled 4f and 5f orbitals.
f.
Please Define Lanthanide Series: In the periodic table, the f-block elements from
period 6 that follow the element lanthanum.
g.
Please Define Actinide Series: In the Periodic Table, the f-block elements from
period 7 that follow the element actinium.
Nonmetals
a.
Please Define Nonmetals: Elements that are generally gases or dull, brittle solids,
that are poor conductors of heat and electricity.
b.
Please Define Halogens: Most highly reactive of all nonmetals found in Group 17.
c.
Please Define Noble Gases: An extremely unreactive Group 18.
Metalloids
a.
Please Define Metalloids: An element that has physical and chemical properties
of both metals and nonmetals.
CLASSIFICATION OF THE ELEMENTS - 6.2
A.
Organizing the Elements by Electron Configuration
1.
Please Define Valence electrons: An electron in the outer most orbital, or outer most
energy level; and determines the chemical properties of an element.
2.
Valence electrons and period
3.
Valence electrons of the representative elements
a.
What is another name for Representative Elements? The 8 Tall columns;
Groups 1,2 - to 13, 14, 15, 16, 17, and 18.
-3B.
III.
The s-, p-, d-, and f-Block Elements
1.
s-Block elements
2.
p-Block elements
3.
d-Block elements
4.
f-Block elements
PERIODIC TRENDS - 6.3
A.
Atomic Radius
1.
For metals such as sodium how is the atomic radius defined? Half the distance
between adjacent nuclei in a crystal of the element. Look at Figure 6-10, p. 187.
2.
For nonmetals as hydrogen how is the atomic radius defined? Diatomic molecules
that is half the distance between nuclei of identical atoms.
3.
Trends within periods
a.
What is the trend in the atomic radii size as one moves from left to right
across a period? A decrease in atomic radii.
Why? There is an increase in the number of protons and electrons across
each period, opposite charges attract, and therefore there is a shrinkage
in the atoms’ electron cloud or its atomic radius.
4.
Trends within groups
a.
What is the trend in the atomic radii size as one moves down a group or
family? A increase in atomic radii.
Why? Moving down each group or family the Energy Level increases and
therefore the atomic radii increases.
B.
Ionic Radius
1.
Please Define Ion: An atom or bonded group of atoms with a positive or negative
charge.
2.
What are the two reasons why positively charged ions become smaller?
a. The loss of a valence electron results in a smaller radius.
b. The fewer remaining electrons(like charges repel) are attracted more to the
positive nucleus.
-4-
C.
3.
Trends within periods
a.
Both positively and negatively charged ions gradually decrease
when moving across the Periodic Table. Why? The increase in the number of
protons across each period.
4.
Trends within groups
a.
Both positively and negatively charged ions gradually increase
when moving down the Periodic Table. Why? Energy levels increases and
and thereby the electron cloud.
Ionization Energy
1.
Please Define Ionization Energy: The energy required to remove an electron
from a gaseous atom; generally increases in moving from left-to-right across a period
and decreases in moving down a group.
2.
Removing more than one electron
a.
Why is it more difficult in removing successive electrons from a neutral
metal atom?
(1.) One is removing electrons that are closer to the positive nucleus.
(2.) Each successive electron removed makes the rest of the electrons
more negative and thus are attracted more to the positive nucleus.
3.
(3.) Electrons are remove from a stable octet which resembles the stability of
a Noble Gas.
Trends within periods
a.
What is the trend in Ionization Energy as one proceeds from left to right
across the Periodic Table? Increases
b.
4.
Why to the above? The number of protons increase , increasing the
positive charge of the nucleus as one moves from left to right across each period.
Trends within groups
a.
What is the trend in Ionization Energy as one proceeds down a group or
family? Decreases
b.
Why to the above? The Energy Levels increase, so the negative electrons
in the Electron Cloud are further away from the positive nucleus.
-55.
D.
IV.
Octet rule
a.
Please Define Octet rule: States that atoms lose, gain, or share electrons
in order to acquire the stable electron configuration of a noble gas.
Electro negativity
1.
Please Define Electronegativity: Indicates the relative ability of an element’s
atom to attract electrons in a chemical bond.
CHAPTER 6 ASSESSMENT- 6.4
A.
Please do the following problems on pages 199-200 in your Text.
1.
Problems 48, 49, 59, 60, 62, 63, 64, 69, and 78.