Periodic Table Trends of Carbon Group Elements Explained
A carbon group element consists of six chemical elements that make up group 14 elements of the periodic table, Carbon family elements contain carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). The properties of the carbon group periodic table
and other compounds in that family are intermediate between the properties related to the elements of the adjacent boron and nitrogen group elements.
The electronic configurations (ground state) of carbon group elements show that each of them has four electrons in its outermost shells. If n represents the outermost shell (where n is 2 for carbon, 3 for silicon, and so on), then these four electrons are represented by the symbols ns2np2. Elements belonging to Group 14 have oxidation states of +4 and +2 for the heavier elements due to the inert pair effect.
This page deals with details of the periodic properties of carbon family elements, Let’s discuss carbon group numbers and briefly discuss the individual properties of carbon, silicon, germanium, tin, lead, and flerovium.
Carbon Group Periodic Table
All the carbon family elements are familiar in daily life either in the pure elemental form or in the form of compounds, except germanium and the artificially produced flerovium, they are not present naturally, also except for silicon, none is abundant in the Earth’s crust.
Carbon can form a different variety of compounds both in the plant and animal kingdoms. Silicon and its minerals form a fundamental component of the Earth’s crust; silica (silicon dioxide) is also called sand.
Germanium can form some minerals and is mostly found in small concentrations with the mineral zinc blende and in coals. Even though germanium is considered one of the rarer elements, its importance is in its properties like semiconductors.
Some carbon-containing molecules are carbon dioxide (CO2) and methane (CH4).
Carbon
Carbon is the 4th most abundant common element present on earth’s crust and occurs naturally as anthracite (a type of coal), graphite, and diamond.
Symbol: C
Atomic Number: 6
Atomic Mass: 12.0107 u
It is mostly used in organic chemistry, as it is the distinguishing feature of an organic compound.
And is also unique among the elements because of its ability to form strongly bonded chains, with hydrogen atoms. It is considered to be the "backbone" of biology, as all life forms on earth are carbon-based. This is due to its qualities of small size and its unique electron configuration. Since carbon atoms are small in size, their p-orbital electrons overlap considerably and enable π bonds to form. Common molecules that are carbon-based are carbon dioxide (CO2) and methane (CH4).
Impure carbon which is in the form of charcoal obtained from wood and coke obtained from coal is used in metal smelting. It is commonly used in the iron and steel industries.
Graphite is used in pencils and used to make brushes in electric motors and in furnace linings. Activated charcoal is used for purification and filtration and can be found in respirators also.
Carbon fibre also finds its application as a very strong, lightweight, material. It is currently used in tennis rackets, skis, fishing rods, rockets, and airplanes.
Silicon
Symbol: Si
Atomic Number: 14
Atomic Mass: 28.0855 u
Silicon is the 2nd most common element which is found in the earth's crust (after oxygen) and is considered the backbone of the mineral world. It is classified as neither metal nor nonmetal but is a metalloid. Silicon is inert, primarily reacting with halogens. Silicon plays a much smaller role in biology, It may have functioned as a catalyst in the formation of the earliest organic molecules Plants highly depend on silicates in order to hold nutrients in the soil, where their roots can absorb them. Silicon (primarily found in silica, SiO2, molecule) has been used for millennia in the creation of ceramics and glass. if carbon can be considered as the backbone of human intelligence, silicon can be considered as the backbone of artificial intelligence. Silicon can be found in sandy beaches and is also a major component of concrete and brick.
Being a semiconductor, it is used to make transistors.
It is most commonly used in computer chips and solar cells.
It can be used while production of fire bricks.
Most waterproofing systems use silicones as a component.
Silicon can be used in many moulds and moulding compounds.
It is also one of the components of ferrosilicon which is an alloy commonly used in the steel industry.
Germanium
Symbol: Ge
Atomic Number: 32
Atomic Mass: 72.64 u
It is a rare element that is used in the manufacturing of semiconductor devices. The physical and chemical properties of germanium are somewhat similar to those of silicon. It is gray-white in colour and it forms a crystal structure.
Germanium acts as a semiconductor that is doped with arsenic and other elements and can be used as a transistor in electronic applications.
The oxides of Germanium have a high index of dispersion and refraction that makes it good to use in wide-angle camera lenses & objective lenses for microscopes.
It can be used as an alloying agent in contact with fluorescent lamps and as a catalyst.
They are used in infrared spectroscopes because both germanium and germanium oxides are transparent to infrared radiation.
Stannum
Symbol: Sn
Atomic Number: 50
Atomic Mass: 118.71 u
Tin is a soft, malleable metal that has a low melting point. It has two solid-state allotropes at regular temperatures and pressures and is denoted by α and β. At higher temperatures (above 13°C), tin exists as white tin and is often used in the formation of alloys. At lower temperatures, it can be transformed into gray tin, it loses its metallic properties and turns powdery.
Tin shows a chemical similarity with both of its neighbours in group 14 i.e germanium and lead and has two main oxidation states, +2 and the slightly more stable in +4 state.
Gray tin can be used to plate iron food cans in order to prevent them from rusting. Tin is malleable, ductile, and crystalline. It has 27 isotopes of which 9 are stable and 18 are unstable. It is a superconductor at low temperatures.
It can be used in the process of tin plating, coating and polishing as it has a high resistance to corrosion
It is used in the soldering of steel as it possesses high magnetic strengths and lower melting points
It can be used in the manufacture of other alloys like bronze and copper
It is used as a reducing agent and as a dyeing agent for glass, ceramics, and sensors.
It is used as an anti-fouling agent for boats and ships In the shipping industry.
It is employed in some products in the form of stannous chloride (SnCl2)in dental applications.
It finds its applications in the electrodes of batteries like Li-ion batteries.
It can be widely used in the manufacture of food containers that are made of steel.
This element in organic form is most dangerous to human health. It can cause severe effects in humans such as Eye and skin irritations, Headaches, Sickness, dizziness, Breathlessness, Severe sweating along with many other problems.
Plumbum
Symbol: Pb
Atomic Number: 82
Atomic Mass: 207 u
Lead a very soft, silvery-white, or grayish metal is very similar to tin in that it is a soft, malleable metal with a low melting point. It was widely used in water and sewage pipes, Lead is toxic to human health, especially to children. Even very low-level exposure can cause nervous system damage and can prevent proper production of haemoglobin (the molecule in red blood cells responsible for carrying oxygen through the body), Lead is stable in an oxidation state of +2 or +4. Its oxides can have multiple industrial uses like oxidizing agents, such as cathodes in lead-acid storage cells. It is used in heavy and industrial machinery, sheets, and other parts made from lead compounds which can be used to dampen noise and vibration.
Flerovium
Symbol: Fl
Atomic Number: 114
Atomic Mass: 289 u
Flerovium (Fl) was discovered in 1998 by scientists in Dubna. It is radioactive and very short-lived, The long-lasting isotope of flerovium has an atomic weight of 289 and a half-life of 0.97 seconds. Three other isotopes of flerovium have half-lives of 0.52, 0.51, and 0.16 seconds respectively.
Conclusion
Here, we have studied carbon family elements and some of their uses and properties, Different elements of this group are carbon (C), silicon (Si), germanium (Ge), tin (Sn), lead (Pb), and flerovium (Fl). Carbon is commonly used almost everywhere whereas Flerovium is radioactive in nature.
FAQs on Carbon Group Elements: Comprehensive Guide for Students
1. Which elements belong to the Carbon family, also known as Group 14?
The Carbon family, or Group 14 of the periodic table, consists of five elements. In order of increasing atomic number, they are: Carbon (C), Silicon (Si), Germanium (Ge), Tin (Sn), and Lead (Pb). Carbon is a non-metal, silicon and germanium are metalloids, and tin and lead are metals, showing a clear trend in metallic character down the group.
2. What is catenation, and why is this property most prominent in carbon?
Catenation is the unique ability of an atom to form strong covalent bonds with other atoms of the same element, resulting in long chains, branched chains, or ring structures. This property is most prominent in carbon due to two main reasons:
- The C-C bond is exceptionally strong and stable, with a high bond enthalpy.
- Carbon's small size and tetravalency (ability to form four bonds) allow it to form a vast number of stable, complex molecules without steric hindrance.
3. How do the structures and properties of diamond and graphite differ?
Diamond and graphite are two well-known allotropes of carbon with vastly different structures and properties.
- Diamond: Each carbon atom is sp³ hybridised and bonded to four other carbon atoms in a rigid, three-dimensional tetrahedral network. This makes diamond the hardest known natural substance and an electrical insulator.
- Graphite: Each carbon atom is sp² hybridised and bonded to three other carbons in the same plane, forming hexagonal layers. The layers are held by weak van der Waals forces, allowing them to slide over one another, which makes graphite soft, slippery, and a good lubricant. The free electron in the unhybridised p-orbital makes it a good conductor of electricity.
4. Why does the stability of the +2 oxidation state increase for elements down Group 14?
The increasing stability of the +2 oxidation state down Group 14 is explained by the 'inert pair effect'. As we move down the group from Carbon to Lead, the intervening d- and f-orbitals offer poor shielding for the outermost s-electrons. This results in a stronger attraction of the ns² electrons by the nucleus, making them less likely to participate in bonding. Consequently, only the p-electrons are lost, leading to a stable +2 oxidation state, which is the most stable state for lead (Pb).
5. Carbon dioxide (CO₂) is a gas, but silicon dioxide (SiO₂) is a high-melting solid. What explains this major difference?
This difference is due to the nature of their chemical bonding. Carbon is small enough to form strong pπ-pπ double bonds with oxygen, resulting in discrete, linear CO₂ molecules. The forces between these individual molecules are weak (van der Waals forces), so CO₂ is a gas at room temperature. In contrast, silicon is larger and cannot form stable π-bonds. Instead, each silicon atom forms four strong single covalent bonds with four oxygen atoms, creating a giant three-dimensional covalent network structure. Breaking these strong covalent bonds requires a large amount of energy, making SiO₂ a hard, high-melting point solid.
6. What are the general trends in atomic radii and ionisation enthalpy for the Carbon family?
For Group 14 elements, the general trends in physical properties are as follows:
- Atomic Radii: The atomic radius increases steadily as we move down the group from Carbon to Lead. This is because a new electron shell is added for each successive element.
- Ionisation Enthalpy: The first ionisation enthalpy generally decreases down the group due to the increase in atomic size and shielding effect. However, there is a slight increase from Tin (Sn) to Lead (Pb) because of the poor shielding provided by the inner d- and f-electrons, which leads to a stronger effective nuclear charge.
7. What are silicones and what makes them useful in real-world applications?
Silicones are synthetic polymers with a repeating `(-R₂Si-O-)` backbone, where R is an organic group. They are important because of their unique properties:
- High thermal stability: They can withstand high and low temperatures without breaking down.
- Water repellency: They are hydrophobic and used for waterproofing.
- Chemical inertness: They do not react with many chemicals, making them safe for various applications.
