Download PreAP Chemistry

Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
6.1 Development of the Modern Periodic Table
Objectives
• Trace the development of the periodic table.
• Identify key features of the periodic table.
Main Idea: The periodic table _______________ over time as scientists discovered more
useful ways to _______________ and _______________ the elements.
Development of the Periodic Table
• In the 1700s, _______________ compiled a list of all the known elements of the
time.
•
•
•
•
•
•
The 1800s brought large amounts of information and scientists needed a way to
_______________ knowledge about elements.
_______________ proposed an arrangement where elements were ordered by
increasing atomic _______________.
Newlands noticed when the elements were arranged by increasing atomic mass, their
properties _______________ every _______________ element.
_______________ and _______________ both demonstrated a connection
between atomic _______________ and elemental properties.
_______________ rearranged the table by increasing atomic _______________,
and resulted in a _______________ periodic pattern.
Periodic repetition of chemical and physical properties of the elements when they
are arranged by increasing atomic number is called _______________.
1
Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
The Modern Periodic Table
 The _______________ periodic table contains boxes which contain the element's
name, symbol, atomic number, and atomic mass.
•
•
•
•
•
•
•
•
•
•
•
•
•
•
Columns of elements are called _______________.
Rows of elements are called _______________.
Elements in groups 1,2, and 13-18 possess a wide variety of chemical and physical
properties and are called the _______________ elements.
Elements in groups 3-12 are known as the _______________ _______________.
Elements are _______________ as metals, non-metals, and metalloids.
_______________ are elements that are generally shiny when smooth and clean,
solid at room temperature, and good conductors of heat and electricity.
_______________ _______________ are all the elements in group 1 except
hydrogen, and are very reactive.
_______________ _______________ metals are in group 2, and are also highly
reactive.
The transition elements are divided into _______________ metals and
_______________ transition metals.
The two sets of inner transition metals are called the _______________
_______________ and _______________ _______________ and are located at
the bottom of the periodic table.
_______________ are elements that are generally gases or brittle, dull-looking
solids, and poor conductors of heat and electricity.
Group 17 is composed of highly reactive elements called _______________.
Group 18 gases are extremely unreactive and commonly called _______________.
_______________ have physical and chemical properties of both metals and nonmetals, such as silicon and germanium.
2
Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
6.2 Classification of the Elements
Objectives
• Explain why elements in the same group have similar properties.
• Identify the four blocks of the periodic table based on their electron configuration.
Main Idea: Elements are organized into different _______________ in the periodic table
according to their _______________ _______________.
Organizing Elements by Electron Configuration
• Recall electrons in the highest principal energy level are called _______________
electrons.
• All _______________ elements have _____ valence electron.
• The _______________ _______________ of an element’s valence electrons
indicates the _______________ on the periodic table in which it is found.
• The number of valence electrons for elements in groups 13-18 is
_______________ _______________ than their group number.
The s-, p-, d-, and f-Block Elements
• The _______________ of the periodic table becomes clear if it is divided into
_______________ representing the atom’s energy sublevel being filled with
valence electrons.
• ___-block elements consist of group 1 and 2, and the element helium.
• Group 1 elements have a _______________ filled s orbital with one electron.
• Group 2 elements have a _______________ filled s orbital with two electrons.
• After the s-orbital is filled, valence electrons occupy the ___-orbital.
• Groups 13-18 contain elements with _______________ or _______________
filled p orbitals.
• The ___-block contains the transition metals and is the _______________ block.
• There are _______________, but d-block elements usually have filled outermost s
orbital, and filled or partially filled d orbital.
• The _______________ d orbitals can hold ___ electrons, so the d-block spans ten
groups on the periodic table.
• The __-block contains the _______________ _______________ metals.
• f-block elements have filled or partially filled outermost ___ orbitals and filled or
partially filled ____ and ____ orbitals.
• The 7 f orbitals hold ___ electrons, and the inner transition metals span 14 groups.
3
Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
Example Problem 1 ELECTRON CONFIGURATION AND THE PERIODIC TABLE Strontium,
which is used to produce red fireworks, has an electron configuration of [Kr]5s2. Without
using the periodic table, determine the group, period, and block of strontium.
Practice Problems page 186
8. Without using the periodic table, determine the group, period, and block of an atom
with the following electron configurations.
a. [Ne]3s2
b. [He]2s2
c. [kr]5s24d105p6
9. What are the symbols of the elements with the following valence electron
configurations?
a. s2d1
b. s2p3
c. s2p6
10. Challenge Wrote the electron configuration of the following elements.
a. the group 2 element in the fourth period
b. the group 12 element in the fourth period
c. the noble gas in the fifth period
d. the group 16 element in the second period
6.3 Periodic Trends
Objectives
• Compare period and group trends of several properties.
• Relate period and group trends in atomic radii to electron configuration.
Main Idea: Trends among elements in the periodic table include their size and their ability
to lose or attract electrons.
Atomic Radius
• _______________ _______________ is a periodic trend influenced by electron
configuration.
• For metals, atomic radius is _______________ the distance between adjacent
_______________ in a crystal of the element.
• For elements that occur as _______________, the atomic radius is half the
distance between nuclei of _______________ atoms.
4
Honors Chemistry
•
•
•
•
Chapter 6 The Periodic Table
Notes Outline
There is a general _______________ in atomic radius from left to right, caused by
increasing _______________ _______________ in the nucleus.
Valence electrons are not _______________ from the increasing nuclear charge
because no additional electrons come between the nucleus and the valence electrons.
Atomic radius generally _______________ as you move down a ______________.
The outermost orbital size ______________ down a group, making the atom larger.
Ionic Radius
• An _________ is an atom or bonded group of atoms with a positive or negative
_______________.
5
Honors Chemistry
•

•
•
•
•
Chapter 6 The Periodic Table
Notes Outline
When atoms _______________ electrons and form _______________ charged
ions, they always become _______________ for two reasons:
1. The loss of a valence electron can leave an _______________ outer
orbital resulting in a small radius.
2. Electrostatic _______________ _______________ allowing the
electrons to be pulled closer to the radius.
When atoms _______________ electrons, they can become _______________,
because the addition of an electron increases electrostatic _______________.
The ionic radii of _____________ ions generally _____________ from left to
right.
The ionic radii of _______________ ions generally decrease from left to right,
_______________ with group 15 or 16.
Both positive and negative ions _______________ in size moving down a group.
6
Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
Ionization Energy
• _______________ _______________ is defined as the energy required to
remove an electron from a gaseous atom.
• The energy required to remove the first electron is called the _______________
ionization energy.
• Removing the second electron requires _______________ energy, and is called the
_______________ ionization energy.
• Each successive ionization requires _______________ energy, but it is _____ a
steady increase.
• The ionization at which the large increase in energy occurs is related to the number
of _______________ electrons.
• First ionization energy _______________ from left to right across a
_______________.
• First ionization energy _______________ down a group because atomic size
_______________ and less energy is required to remove an electron
_______________ from the nucleus.
7
Honors Chemistry
•
•
Chapter 6 The Periodic Table
Notes Outline
The _______________ _______________ states that atoms tend to gain, lose or
share electrons in order to acquire a full set of eight valence electrons.
The octet rule is useful for _______________ what types of ions an element is
likely to form.
Electronegativity
• The _______________ of an element indicates its relative ability to attract
electrons in a chemical bond.
• Electronegativity _______________ down a group and _______________ left to
right across a period.
8
Honors Chemistry
Chapter 6 The Periodic Table
Notes Outline
Example Problem 2 INTERPRET TRENDS IN ATOMIC RADII Which has the largest
atomic radius: carbon (C), fluorine (F), beryllium (Be), or lithium (Li)?
Practice Problems page 189
16. Which has the largest atomic radius: magnesium (Mg), silicon (Si), sulfur (S), or
sodium (Na)? the smallest?
17. The figure shows helium, krypton, and radon. Which one is krypton? How can you
tell?
18. Can you determine which of the two unknown elements has the larger radius if the
only information given is that the atomic number of one of the elements is 20
greater than the other? Explain.
19. Challenge Determine which element in each pair has the largest atomic radius:
a. the element in period 2, group 1; or the element in period 3, group 18
b. the element in period 5, group 2; or the element in period 3, group 16
c. the element in period 3, group 14; the element in period 6, group 15
d. the element in period 4, group 18; or the element in period 2, group 16
9