Download Periodic Table of Elements

Periodic Table of Elements
A periodic table is a tabular display of elements organized by their atomic
numbers, electron configurations, and chemical properties.
LEARNING OBJECTIVES
● Explain how properties of elements vary within groups
● Describe arrangement of elements in the periodic table
● Explain how properties of elements vary across periods
KEY POINTS
● A periodic table is a useful framework for analyzing chemical behavior. Such
tables are widely used in chemistry and other sciences.
● The periodic table lists all the elements, with information about their atomic
weights, chemical symbols, and atomic numbers.
● A group, or family, is a vertical column in the periodic table. Groups usually have
more significant periodic trends than do periods and blocks. The vertical
columns (groups) of the periodic table are arranged such that all its elements
have the same number of valence electrons. All elements within a certain group
thus share similar properties
● A period is a horizontal row in the periodic table. Elements in the same period
show trends in atomic radius, ionization energy, electron affinity, and atomic
numbers.
KEY TERMS ● atomic number
○ The number, equal to the number of protons in an atom, that determines
its chemical properties. Symbol: Z
● group
○ A vertical column in the periodic table, which signifies the number of
valence shell electrons in an element's atom.
● period
○ A horizontal row in the periodic table, which signifies the total number of
electron shells in an element's atom.
● atomic orbital
○ The quantum mechanical behavior of an electron in an atom describing
the probability of the electron's particular position and energy.
● ionization energy
○ the amount of energy required to remove an electron from an atom or
molecule in the gas phase
● electron affinity
○ the amount of energy released when an electron is added to a neutral atom
or molecule to form a negative ion
Element Symbols
The periodic table is structured as an 18 X 7 grid, positioned above a
smaller double row of elements. The periodic table only lists chemical
elements, and includes each isotope of each element within one cell. In the
typical periodic table, each element is listed by its element symbol and
atomic number. For example, "H" denotes hydrogen, "Li" denotes lithium,
and so on. Most elements are represented by the first letter or first two
letters of their English name, but there are some exceptions. Two notable
exceptions include silver and mercury. The symbol for silver is "Ag" from
Latin ​
argentum, ​
which means "gray" or "shining." The symbol for
mercury is "Hg" from the Latinized Greek ​
hydrargyrum, ​
which means
"water-silver." Many periodic tables include the full name of element as
well and color-code the elements based on their phase at room
temperature (solid, liquid, or gas).
The periodic table The periodic table is a tabular display of all the chemical elements. The atoms are grouped in
order of increasing atomic number.
The periodic table is a tabular display of the chemical elements. The
elements are organized based on their atomic numbers, electron
configurations, and recurring chemical properties.
In the periodic table, elements are presented in order of increasing atomic
number (the number of protons). The rows of the table are called periods;
the columns of the s- (columns 1-2 and He), d- (columns 3-12), and
p-blocks (columns 13-18, except He) are called groups . (The terminology
of s-, p-, and d- blocks originate from the valence atomic orbitals the
element's electrons occupy. ) Some groups have specific names, such as
the halogens or the noble gases. Since, by definition, a periodic table
incorporates recurring trends, any such table can be used to derive
relationships between the properties of the elements and predict the
properties of new, yet-to-be-discovered, or synthesized elements. As a
result, the periodic table provides a useful framework for analyzing
chemical behavior, and such tables are widely used in chemistry and other
sciences.
Blocks in the Periodic Table A diagram of the periodic table, highlighting the different blocks
History of the Periodic Table
Although precursors exist, Dmitri Mendeleev is generally credited with the
publication, in 1869, of the first widely recognized periodic table.
Mendeleev designed the table in such a way that recurring ("periodic")
trends in the properties of the elements could be shown. Using the trends
he observed, he even left gaps for those elements that he thought were
"missing. " He even predicted the properties that he thought the missing
elements would have when they were discovered. Many of these elements
were indeed later discovered, and Mendeleev's predictions were proved to
be correct.
Rows and Periods
The element symbol is always almost accompanied by other information
such as atomic number and atomic weight. Atomic number describes the
number of protons in one atom of that element. For example, an atom of
oxygen contains 8 protons. Elements are listed in order of increasing
atomic number from left to right. Each row of the periodic table is called a
period and each column of the periodic table is called a group (or family).
Some groups have specific names like the halogens or noble gases.
Elements within the same period or group have similar properties. Groups
A group, or family, is a vertical column in the periodic table. Groups
usually have more significant periodic trends than do periods and blocks,
which are explained below. Modern quantum mechanical theories of
atomic structure explain group trends by proposing that elements in the
same group generally have the same electron configurations in their
valence (or outermost, partially filled) shell. Consequently, elements in the
same group tend to have shared chemistry and exhibit a clear trend in
properties with increasing atomic number. However, in some parts of the
periodic table, such as the d-block and the f-block, horizontal similarities
can be as important as, or more pronounced than, vertical similarities.
Periods
A period is a horizontal row in the periodic table. Although groups
generally have more significant periodic trends, there are regions where
horizontal trends are more significant than vertical group trends, such as
in the f-block, where the lanthanides and actinides form two substantial
horizontal series of elements. Elements in the same period show trends in
atomic radius, ionization energy, and electron affinity. Atomic radius
usually decreases from left to right across a period. This occurs because
each successive element has an added proton and electron, which causes
the electron to be drawn closer to the nucleus, decreasing the radius.
The periodic table Here is the complete periodic table with atomic numbers, groups, and periods. Each entry on
the periodic table represents one element, and compounds are made up of several of these
elements.
Determining Chemical Properties using the Periodic Table
Chemical properties of each element are determined by the element's
electronic configuration, and particularly by its outermost valence
electrons. An element's location in the periodic table is largely dependent
on its electrons; the number of valence shell electrons determines its
group, and the type of orbital in which the valence electrons lie in
determines the element's block. In addition, the total number of electron
shells an atom determines which period it belongs to. Because of its
structure, the periodic table has become an extremely useful tool for
assessing and predicting elemental and chemical trends.