Structure And Bonding Of Carbon
Muhtasari
Sharpen a pencil and you are holding one of the softest solids in the laboratory. Look at a ring set with a diamond and you are looking at the hardest natural material on Earth. Yet nothing separates them at the level of the atom. Both are pure carbon: the same element, six protons in every nucleus, no impurity that matters. What differs is how the atoms are joined up, and that turns out to be everything.
This lesson takes that difference apart. You will count the bonds each carbon atom makes in a diamond and in a flake of pencil lead, work out why sheets held to each other by almost nothing are exactly what a lubricant needs, hunt down the one spare electron that lets a pencil line carry a current, and meet the hollow cage molecules chemists have built out of the same element since 1985. It is also the topic where this course draws its sharpest tier line, so you will find out exactly which half of the story every candidate has to know and which half belongs to the Extension Tier alone.
Malengo
- The element carbon can form four covalent bonds.
- In diamond, each carbon atom forms four covalent bonds with other carbon atoms in a giant covalent structure, so diamond is very hard.
- In graphite, each carbon atom bonds to three others, forming layers. The layers are free to slide over each other because there are no covalent bonds between the layers and so graphite is soft and slippery. Extension Tier students should be able to explain the properties of graphite in terms of weak forces between the layers.
- In graphite, one electron from each carbon atom is delocalised. These delocalised electrons allow graphite to conduct heat and electricity. Students should realise that graphite is similar to metals in that it has delocalised electrons.
- Carbon can also form fullerenes with different numbers of carbon atoms. Fullerenes can be used for drug delivery into the body, in lubricants, as catalysts, and in nanotubes for reinforcing materials, eg in tennis racquets. Students are only required to know that the structure of fullerenes is based on hexagonal rings of carbon atoms.
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Hongera kwa kukamilisha somo la Structure And Bonding Of Carbon. Sasa kwa kuwa umechunguza dhana na mawazo muhimu, ni wakati wa kuweka ujuzi wako kwa mtihani. Sehemu hii inatoa mazoezi mbalimbali maswali yaliyoundwa ili kuimarisha uelewaji wako na kukusaidia kupima ufahamu wako wa nyenzo.
Utakutana na mchanganyiko wa aina mbalimbali za maswali, ikiwemo maswali ya kuchagua jibu sahihi, maswali ya majibu mafupi, na maswali ya insha. Kila swali limebuniwa kwa umakini ili kupima vipengele tofauti vya maarifa yako na ujuzi wa kufikiri kwa makini.
Tumia sehemu hii ya tathmini kama fursa ya kuimarisha uelewa wako wa mada na kubaini maeneo yoyote ambapo unaweza kuhitaji kusoma zaidi. Usikatishwe tamaa na changamoto zozote utakazokutana nazo; badala yake, zitazame kama fursa za kukua na kuboresha.
- In graphite, how many other carbon atoms is each carbon atom covalently bonded to? A. One B. Two C. Three D. Four Answer: C
- Why is graphite soft and slippery? A. The covalent bonds within each layer are weak B. There are no covalent bonds between one layer and the next, so the layers slide C. The carbon atoms are held together by ionic bonds D. Graphite contains no covalent bonds at all Answer: B
- Why does diamond not conduct electricity? A. Its atoms are held together by weak forces B. All four outer electrons of each carbon atom are used in covalent bonds C. It is transparent and colourless D. Its carbon atoms carry no charge Answer: B
- Which statement about fullerenes is correct? A. Their structure is based on hexagonal rings of carbon atoms B. They are giant covalent structures with no fixed formula C. Every fullerene contains exactly 12 carbon atoms D. Each carbon atom in a fullerene forms four covalent bonds Answer: A
- Graphite is similar to a metal because it: A. is shiny and can be bent into shape B. conducts heat and electricity using delocalised electrons C. reacts with dilute acids to give hydrogen D. forms positive ions in solution Answer: B
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