PEH Periodic Table (Principles) - Get The Table Organized in Time! Lab Manual (English)

Virtual Lab Manual
Periodic Table (Principles): Get

the table organized in time!
Synopsis
Light up the elements! In this simulation, you will learn all the fundamental ins and outs of
the periodic table. Find out which elements have metallic characteristics, perform a flame
test, and explore trends in atomic properties among the main groups and periods.
Broken table
The periodic table is an amazing tool for getting an overview of all the elements in existence,
even the elements that only exist when we create them ourselves. But the table in this
virtual lab lab is broken; some of the elements have fallen out, and it’s your mission to figure
out where they belong by investigating their characteristics and properties.
Flame color test and atomic properties

To sort the first few elements in the table you can observe their flame colors. You may need
to use your knowledge about element classes as well to get the full overview.
There are surprisingly many atomic properties for which trends can be observed via the
periodic table. Moving on to the virtual holo-table, you will investigate these trends and
deduct how they behave when you move within and between periods and groups of the
table. You will need this knowledge to assign the most tricky fallen-out elements.
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Become the teacher
At the end of the simulation, a special visitor will be coming by the lab, and she needs you to
help her understand the basics of the periodic table.
Will you be able to grasp the periodic table well enough to explain it to the visitor?
Learning Objectives
At the
end of this simulation, you will be able to…
●Describe the structure and organization of the periodic table
●Classify elements of a family based on their location in the periodic table
●Distinguish metals from other element classes based on typical characteristics
●Use the flame color test to identify metals based on their position in the periodic
table
● Relate valence electrons and oxidation state of a main group element to its position in
the periodic table
● Describe the main trends among groups and periods for atomic properties
● Explain the causes on the atomic level for the main trends among groups and periods
concerning atomic radii, ionization energy and electronegativity
Techniques in Lab
● Flame color test
Theory
Periodic Table
In a periodic table, chemical elements are arranged in groups and periods according to their
atomic number, electron configuration, and their chemical properties.
Elements in the same period have the same number of electron shells and tend to have
similar properties. Thus, it is relatively easy to predict the chemical properties of an element
if one knows the properties of the elements around it. A new row (period) is started when a
new electron shell has its first electron.
Elements in the same group have the same electron configuration in their valence shell.

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Figure 1: Periodic Table
Atomic Number
The atomic number (Z) of a specific chemical element indicates the number of protons in the
nucleus of an atom of the chemical element. In the neutral state of an atom, the atomic
number also equals the number of electrons.
The atomic number is fixed for every element. In contrast, the number of neutrons may vary.
Together, protons and neutrons make up the atomic mass.
Figure 2: Explanation of the superscripts and subscripts in the atom of Lithium.

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Metals
Metals are chemical elements that are solid (with the exception of mercury, a liquid) shiny,
ductile, malleable, and good conductors of heat and electricity.
In the periodic table, metals are grouped together in the middle to the left-hand side (see
Figure 1).
Non-metals
Non-metals are chemical elements that lack the characteristic metallic properties and thus
appear dull and are poor conductors of heat and electricity. They tend to have a relatively
low melting point, boiling point, and density; and exist as solids, liquids, and gases at room
temperature and normal pressure.
In the periodic table, non-metals are grouped together on the right-hand side (see Figure 1).
Metalloids
Metalloids are “like a metal”, which means that they conduct heat and electricity moderately
well, and possess some properties of metals and some properties of non-metals. One known
example is silicon which acts as a semiconductor.
In the periodic table, metalloids are grouped together in the center to the right-hand side
(see Figure 1).
Flame Test
A flame test is a common analytic procedure that can be used to distinguish different metal
ions depending on the emission spectrum that is produced when the element is introduced
into a hot flame. When a metal ion solution is held into a flame, heat will excite the valence
electrons that emit a certain wavelength (λ) in the visible light spectrum when falling back to
their original state (Figure 3). Most metal ions, therefore, have a characteristic and known
flame color when applied to a flame test.
Figure 3: Electrons being excited and falling back while emitting light of a certain wavelength
(λ) in the flame test.

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Valence Electron
The valence shell is the outermost layer of an atom. Electrons in this shell are called valence
electrons.
The number of valence electrons of non-transition metals can easily be found by their
location in the periodic table (Figure 4).
Figure 4: Valence electrons of elements in group I to VIII
Octet Rule
The tendency of main group elements atoms to form chemical bonds in a way that each
atom obtains eight valence electrons is described by the "octet rule". Having eight electrons
in the valence shell is a particularly stable state with the same electron configuration as a
noble gas.
Two exceptions to the rule are hydrogen, lithium and helium. Hydrogen only needs one
additional electron and lithium needs to lose one electron to attain a stable configuration
with two electrons. Helium has a total of two valence electrons and, with this, in its most
stable form.

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Oxidation states in the periodic table
Among others, the periodic table can provide practical information about the oxidation state
of an element (Figure 5). This number is defined as the formal charge on the atom if all
bonds were assumed to be fully ionic. Knowing the oxidation number or state is very useful
for example when balancing reduction-oxidation (redox) reactions.
Figure 5: Oxidation states in the Periodic Table.
Trends in the periodic table

In the periodic table different general trends within one group or period can be observed as
summarized in Figure 6. While the atomic radius is increasing within one group, it is
decreasing when going from left to right within one period. Electronegativity and ionization
energy follow the same trends. An increase can be seen within one period, whereas both
values decrease moving down within a group.
Figure 6: Trends in the Periodic Table

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Virtual Lab Manual

Periodic Table (Principles): Get

Flame color test and atomic properties

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● Flame color test

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Figure 2: Explanation of the superscripts and subscripts in the atom of Lithium.

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Figure 4: Valence electrons of elements in group I to VIII

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Figure 5: Oxidation states in the Periodic Table.

Trends in the periodic table

Figure 6: Trends in the Periodic Table

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