Download Ch. 6 The Periodic Table and Periodic Law Vocabulary Review

Ch. 6 The Periodic Table and Periodic Law
Vocabulary Review
atomic number
New Vocabulary
periodic law
group
period
representative element
transition element
metal
valence electron
alkali metal
alkaline earth metal
New continued
transition metal
inner transition metal
lanthanide series
principal energy level
actinide series
nonmetal
halogen
noble gas
metalloid
ion
ionization energy
octet rule
electronegativity
Section 1: Development of the Modern Periodic Table
Main Idea:
The periodic table evolved over time as scientists discovered more useful ways to compare and organize the elements
Development of the Periodic Table
In the 1700s, Lavoisier compiled a ______________ of all the known elements of the time.
The 1800s brought large amounts of information and scientists needed a way to organize knowledge about elements.
______________________proposed an arrangement where elements were ordered by increasing atomic mass.
Newlands noticed when the elements were arranged by increasing atomic mass, their properties repeated every eighth element.
Meyer and Mendeleev both demonstrated a connection between ______________________and elemental properties. Moseley rearranged the table
by increasing atomic number, and resulted in a clear periodic pattern. Periodic repetition of chemical and physical properties of the elements when
they are arranged by increasing atomic number is called _________________________________
The ______________________contains boxes that contain the element's name, symbol, atomic number, and atomic mass
Columns of elements are called groups. Rows of elements are called periods.
Elements in groups 1,2, and 13–18 possess a wide variety of chemical and physical properties and are called the ______________________Elements
in groups 3–12 are known as the______________________.
Elements are classified as metals, nonmetals, and ______________________.
Metals 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.
______________________are in group 2, and are also highly reactive.
______________________elements are divided into transition metals and inner transition metals.
The two sets of inner transition metals are called the ______________________ and ______________________and are located at the bottom of the
periodic table.
Nonmetals 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 ______________________.
Metalloids, such as silicon and germanium, have physical and chemical properties of both ______________________.
Review Questions
How was the periodic table developed? ______________________________________________________________________________________________
What are the key features of the periodic table? _____________________________________________________________________________________
Section 2: Classification of the Elements
Organizing the Elements by Electron Configuration
Recall electrons in the highest principal energy level are called valence electrons. All group 1 elements have ___________________.
Alkali Metals: __________________________________________________________________________________________________________________________________________________________
Alkaline Earth: _______________________________________________________________________________________________________________________________________________________
Alkali Metals: __________________________________________________________________________________________________________________________________________________________
Transition metals: ___________________________________________________________________________________________________________________________________________________
Metalloids: ____________________________________________________________________________________________________________________________________________________________
Halogens: _____________________________________________________________________________________________________________________________________________________________
Noble Gases: __________________________________________________________________________________________________________________________________________________________
Group 2 elements have ______________________. The number of valence electrons for elements in groups 13–18 is ten less than their group
number. The energy level of an element’s valence electrons indicates the period on the periodic table in which it is found
The s-, p-, d-, and f-Block Elements
The shape of the periodic table becomes clear if it is divided into blocks representing the atom’s energy sublevel being filled with valence electrons.
s-block elements consist of group 1 and 2, and the element helium.
Group 1 elements have a partially filled s orbital with ______________________________
Group 2 elements have a completely filled s orbital with ________________________________________
Groups 13–18 fill the _________________. In group 18, both the s and p orbitals of the period’s principal energy level are __________________________________
The ______________________ contains the transition metals and is the largest block.
There are exceptions, but d-block elements usually have filled __________________________________, and filled or _______________________________________________.
The five d orbitals can hold 10 electrons, so the d-block spans ten groups on the periodic table. The f-block contains the inner transition metals.
f-block elements have filled or partially filled outermost s orbitals and filled or _____________________________________________________ The 7f orbitals hold 14
electrons, and the inner transition metals span 14 groups.
Review Questions
Why do elements in the same group have similar properties? ___________________________________________________________________________________________________
Based on their electron configurations, what are the four blocks of the periodic table? ________________________________________________________________________
Section 3: Periodic Trends
Atomic Radius
______________________is a periodic trend influenced by electron configuration. For metals, atomic radius is half the distance between adjacent
nuclei in a crystal of the element.
For elements that occur as molecules, the atomic radius is half the distance between nuclei of identical atoms that are chemically bonded together.
Atomic radius generally decreases from ______________________, caused by increasing positive charge in the nucleus. Valence electrons are not
shielded from the increasing nuclear charge because no additional electrons come between the nucleus and the valence electrons.
Atomic radius generally increases as you ______________________. The outermost orbital size increases down a group, making the atom larger.
Draw Trend here:
Ionic Radius
When atoms lose electrons and form ______________________ charged ions, they always become smaller for two reasons:
The loss of a valence electron can leave an empty outer orbital, resulting in a smaller radius.
Electrostatic repulsion decreases allowing the electrons to be pulled closer to the nucleus.
When atoms gain electrons, they can ______________________, because the addition of an electron increases electrostatic repulsion.
The ionic radii of positive ions generally decrease from left to right.
The ionic radii of negative ions generally decrease from left to right, beginning with group 15 or 16.
Both positive and negative ions increase in size moving down a group.
Draw Trend here:
Ionization Energy
Ionization energy is defined as the energy required ______________________an electron from a gaseous atom.
The energy required to remove the first electron is called the first ionization energy.
Removing the second electron requires more energy, and is called the second ionization energy.
First ionization energy increases from ______________________across a period.
First ionization energy decreases ______________________because atomic size increases and less energy is required to remove an electron farther
from the nucleus.
The ionization at which the large increase in energy occurs is related to the number of ______________________.
The octet rule 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.
Draw Trend here:
Electronegativity
The electronegativity of an element indicates its relative ability to ______________________in a chemical bond.
Electronegativity ______________________a group and increases left to right across a period.
Draw Trend here:
Review Questions:
What are the period and group trends of different properties?
How are period and group trends in atomic radii related to electron configuration?