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There are currently 118 total elements (though we may discover more!) Because of this, we use the Periodic Table to sort them all into different rows and columns. Each column, called a "group" contains elements with similar characteristics/properties.
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Jetzt kostenlos anmeldenThere are currently 118 total elements (though we may discover more!) Because of this, we use the Periodic Table to sort them all into different rows and columns. Each column, called a "group" contains elements with similar characteristics/properties.
In this article, we will be looking at group 4A and learning all about the different and wonderful elements contained within it!
Let's begin by looking what what group 4A elements are.
Group 4A elements are the elements in the 14th column of the periodic table.
The group 4A elements are the 4th column across when you ignore the transition metals. They are also called the "Carbon family" since carbon is the first of these elements.
Below is where these elements can be found on the periodic table:
Fig.1- Periodic table with group 4A marked
The elements in Group 4A are:
There is another element called flerovium (Fl). It is a man-made element that is highly radioactive. While its properties and reactivity have been studied, the findings are not fully conclusive, which is why we won't be discussing it much.
Group 4A contains elements of all three types: non-metal, metalloid/semimetal, and metal. Because of this, we will be dividing our discussion into sections. However, we are first going to talk about some general properties of group 4A elements.
1. Electron Configuration and oxidation state
All the group 4A elements have the same general Electron Configuration for their 4 Valence Electrons: ns2np2.
Because of this, they all have the common oxidation state of +4 (lose 4 electrons). However, both tin and lead can have +2 oxidation states, where they lose their p-electrons.
Electron configuration shows how electrons are arranged
Valence Electrons are the outermost electrons. They are responsible for bonding
An element's Oxidation state is the number of electrons lost (+n) or gained (-n) during bonding
2. Boiling points
The boiling points of each element decrease as you down group 4A.
3. Atomic radius
The atomic radius is the distance between the center of the nucleus and the outermost electron(s).
As you move down group 4A, the atomic radius increases.
4. Ionization energy (energy it takes to remove one electron)
As you move down group 4A, ionization energy decreases. However, lead's ionization energy is slightly larger than tin's
5. Electron affinity
Electron affinity decreases as you move down the 4A group.
Electron affinity is the change in energy when an electron is absorbed; the stronger the attraction, the more energy is released
5. Reactions with hydrogen
All group 4A elements react with hydrogen. They generally have the form EH4, where "E" is a group 4A element.
6. Reactions with Oxygen
All group 4A elements react with oxygen. They all have the general for EO2. Both lead and carbon can also form EO compounds.
7. Reactions with Group 17 elements (Halogens)
All group 4A elements will react with the group 17 elements (F, Cl, Br, etc.). The elements form EX4 compounds, where "X" is one of the Halogens.
Carbon is the first of the group 4A elements and is the only nonmetal of the group.
Carbon is an incredibly important element. So much so that there is an entire branch of chemistry dedicated to it called Organic Chemistry. Carbon is the 4th most abundant element and is an essential element for life.
Since it is a non-metal, it mostly forms covalent bonds. Which are bonds where electrons are shared between elements instead of transferred from one to the other (i.e. ionic bonds). Carbon can come in many forms, such as Graphite and Diamond, as shown below.
Fig.2-Carbon as Graphite (left) and Diamond (right)
It also commonly forms compounds containing hydrogen (H₂), nitrogen (N2), and oxygen (O2).
Due to its many forms and compounds, carbon has a plethora of uses, such as:
There are two metalloids/semimetals in group 4A. These are silicon and germanium.
Silicon is a grayish element with a metallic shine (seen below)
Fig.3-A piece of purified silicon (Public Domain).
Germanium looks very similar, as it is also a grayish solid with a metallic sheen.
Fig.4-A sample of crystalline germanium
Since they are metalloids, they tend to form Covalent Bond like carbon.
Both elements are commonly used as semiconductors, which act as intermediates between conductors and insulators. Because of this, they are often used in computers.
They both also react with hydrogen (H₂) and nitrogen (N2). Both elements can form several different hydrides (hydrogen compounds), with two of the most common being GH2 and G2H4 where "G" is silicon or germanium. As for the nitrogen compounds, they both can form nitrides with the formula G3N4.
Lastly, we have our metals: tin and lead Tin and lead are both soft, malleable, metals.
Tin is silvery-white:
Fig.5-Sample of tin (Public Domain)
However, tin is gray with a bluish tint:
Fig.6-Lead cube (Public domain)
Because of their metallic nature, they form ionic bonds.
They both commonly react with hydrogen and halogens (group 17). Since they have oxidation states of +2 and +4, they can form either MH2 and MH4 for hydrogen compounds (where M is tin or lead) and either MX2 or MX4 for halide compounds (where X is a halogen).
In addition, they also react with oxygen to form either MO or MO2, depending on the oxidation state.
Tin is mainly used in alloys, which are mixtures of metals. Such alloys include bronze (95% copper and 5% tin) and dental plating (60% silver, 27% tin, and 13% copper).
Lead's applications have been largely phased out. Lead is poisonous, and it can accumulate in the body over time, causing many health problems such as anemia (lack of red blood cells) and infertility. Previously, it had been used in items such as paints, pencils, and batteries.
Group 4A is also called group 14 or the carbon family.
Group 4A has the common oxidation state of +4
Group 4A is the 4th column in the periodic table if you skip the transition metals.
Group 4A elements contain a non-metal, metalloids, and metals. They are all crystalline solids that are grayish (except for carbon, which can be a power or solid that is black or clear).
They have the common oxidation state of +4 and their valence electrons have the general configuration of ns2np2.
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SIGNUP SIGNUPFlashcards in Group 4A16
Start learningWhere is group 4A located on the periodic table?
14th column
What are the group 4A elements?
How many valence electrons do each group 4A element have?
4
What is the general electron configuration for group 4A's valence electrons?
ns2np2
What is the common oxidation state for all group 4A elements?
+4
True or False: Group 4A elements tend to gain electrons
False
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