Chemistry Chapter 4: Carbon Compounds

0.02%

Carbon dioxide

Carbonates, hydrogen-carbonates

<p>Coal and petroleum</p> Signup and view all the answers

<p>Compounds of carbon</p> Signup and view all the answers

<p>Covalent bond</p> Signup and view all the answers

<p>Carbon</p> Signup and view all the answers

<p>Burning the compound</p> Signup and view all the answers

<p>Medicines</p> Signup and view all the answers

<p>Elemental form and combined form</p> Signup and view all the answers

<p>Carbon dioxide</p> Signup and view all the answers

<p>It is the basis of many materials and living structures.</p> Signup and view all the answers

<p>It forms the basis of many essential compounds and living matter.</p> Signup and view all the answers

<p>The covalent bond.</p> Signup and view all the answers

<p>Coal or petroleum</p> Signup and view all the answers

<p>0.03%</p> Signup and view all the answers

<p>Many items are made of multiple materials.</p> Signup and view all the answers

<p>Food and clothing</p> Signup and view all the answers

<p>Combined form.</p> Signup and view all the answers

<p>Carbon is of immense significance to us.</p> Signup and view all the answers

<p>The 'other' category highlights that most things in our daily lives are compounds of carbon, despite not being metallic or glass/clay.</p> Signup and view all the answers

<p>The small amount of carbon available makes its properties more significant because it must be recycled and used very efficiently.</p> Signup and view all the answers

<p>The reaction produces carbon dioxide, which is useful because it can be identified through specific tests, confirming presence of carbon.</p> Signup and view all the answers

<p>The text says that all living structures are carbon-based, thus the study of these compounds is critical for understanding living systems.</p> Signup and view all the answers

<p>Carbon's capability to form covalent bonds, especially with itself, allows it to create large and complex compounds.</p> Signup and view all the answers

<p>The limited amounts of carbon suggest a reliance on efficient recycling processes or sustainable alternatives so as not to quickly deplete limited resources.</p> Signup and view all the answers

<p>The text states that it forms the basis for food, clothes, medicines and living structures, indicating diverse and complex uses of carbon.</p> Signup and view all the answers

<p>The goal is to demonstrate that many diverse materials we use daily are carbon based compounds.</p> Signup and view all the answers

<p>It appears in both the geological processes within the Earth's crust and within the biological structures indicating its universal importance.</p> Signup and view all the answers

<p>It suggests that unlike ionic compounds, carbon compounds often involves sharing electrons and this leads to different properties.</p> Signup and view all the answers

<p>The compounds do not give rise to ions due to their bonding.</p> Signup and view all the answers

<p>Carbon compounds generally have lower melting and boiling points than ionic compounds.</p> Signup and view all the answers

<p>The forces of attraction are not very strong.</p> Signup and view all the answers

<p>6</p> Signup and view all the answers

<p>4</p> Signup and view all the answers

<p>It would be difficult for the nucleus with six protons to hold on to ten electrons.</p> Signup and view all the answers

<p>It would require a large amount of energy to remove four electrons.</p> Signup and view all the answers

<p>Ionic compounds gain or lose electrons to form ions, whilst carbon compounds share.</p> Signup and view all the answers

<p>2 in the first shell, and 4 in the second shell.</p> Signup and view all the answers

<p>Elements react to attain a completely filled outer shell.</p> Signup and view all the answers

<p>The forces of attraction between the molecules in carbon compounds are weak.</p> Signup and view all the answers

<p>Carbon has four valence electrons, implying it can form four covalent bonds with other atoms.</p> Signup and view all the answers

<p>It is difficult because the nucleus with six protons struggles to hold onto ten electrons, which includes four extra electrons.</p> Signup and view all the answers

<p>For carbon (atomic number 6), the distribution is 2 electrons in the first shell and 4 in the second shell.</p> Signup and view all the answers

<p>Carbon compounds lack free-moving ions or electrons, which are necessary for electrical conductivity.</p> Signup and view all the answers

<p>It requires a large amount of energy to remove four electrons from carbon to form a $C^{4+}$ cation.</p> Signup and view all the answers

<p>Carbon's ability to achieve a filled outer shell by gaining or losing four electrons impacts its reactivity.</p> Signup and view all the answers

<p>Carbon compounds primarily exhibit covalent bonding, leading to their molecular nature and differing physical properties.</p> Signup and view all the answers

<p>Carbon's four valence electrons allow it to form multiple stable bonds and its capacity for catenation leads to complex structures.</p> Signup and view all the answers

<p>Carbon compounds cannot conduct electricity due to the absence of mobile charge carriers.</p> Signup and view all the answers

<p>Carbon forms covalent bonds by sharing electrons. Covalent bonds do not form ions, explaining the low conductivity.</p> Signup and view all the answers

<p>It would have to gain or lose four electrons, a very difficult process, making it more likely to share electrons.</p> Signup and view all the answers

<p>Ionic compounds have strong electrostatic forces, unlike the weaker intermolecular forces in carbon compounds with covalent bonds.</p> Signup and view all the answers

<p>This is a driving force behind reactivity. For carbon, it leads to sharing electrons and forming covalent bonds.</p> Signup and view all the answers

<p>There are 2 electrons in the first shell, and 4 electrons in the second shell.</p> Signup and view all the answers

<p>It indicates carbon will share electrons through covalent bonding, which leads to compounds with low melting/boiling points and poor conductivity.</p> Signup and view all the answers

<p>The tendency to form covalent bonds and the four valence electrons making it able to bond with many other elements.</p> Signup and view all the answers

<p>The weak intermolecular forces lead to relatively low melting and boiling points.</p> Signup and view all the answers

<p>The configuration (2,4) explains why carbon neither gains nor loses electrons, but instead shares them, leading to covalent bonds and specific properties.</p> Signup and view all the answers

<p>With 4 valence electrons, it's difficult to gain or lose 4, so it shares electrons to complete its outer shell.</p> Signup and view all the answers

<p>triple covalent bond</p> Signup and view all the answers

<p>$CH_4$</p> Signup and view all the answers

<p>four</p> Signup and view all the answers

<p>covalent bond</p> Signup and view all the answers

<p>weak</p> Signup and view all the answers

<p>low melting and boiling points</p> Signup and view all the answers

<p>four</p> Signup and view all the answers

<p>1</p> Signup and view all the answers

<p>tetravalent</p> Signup and view all the answers

<p>single covalent bond</p> Signup and view all the answers

<p>Helium has two electrons in its K shell.</p> Signup and view all the answers

<p>A single covalent bond is represented by a line between the two atoms.</p> Signup and view all the answers

<p>The atomic number of chlorine is 17, and its valency is 1.</p> Signup and view all the answers

<p>An oxygen atom has six electrons in its L shell.</p> Signup and view all the answers

<p>A double bond.</p> Signup and view all the answers

<p>Single bonds.</p> Signup and view all the answers

<p>The atomic number of nitrogen is 7.</p> Signup and view all the answers

<p>Nitrogen has 2 electrons in its K shell and 5 in its L shell.</p> Signup and view all the answers

<p>There are three shared pairs of electrons in a triple bond.</p> Signup and view all the answers

<p>A triple bond.</p> Signup and view all the answers

<p>A triple covalent bond</p> Signup and view all the answers

<p>Three single covalent bonds</p> Signup and view all the answers

<p>Hydrogen has a valence of 1, and four hydrogen atoms bond with a single carbon atom.</p> Signup and view all the answers

<p>A covalent bond is formed by the sharing of an electron pair between two atoms.</p> Signup and view all the answers

<p>Intra-molecular bonds are strong, while inter-molecular forces are weak.</p> Signup and view all the answers

<p>Low melting and boiling points</p> Signup and view all the answers

<p>Each hydrogen atom shares one electron with the carbon.</p> Signup and view all the answers

<p>Carbon is tetravalent because it has four valence electrons.</p> Signup and view all the answers

<p>Atoms share electrons and neither gains nor loses electrons.</p> Signup and view all the answers

<p>Three pairs of electrons between two nitrogen atoms.</p> Signup and view all the answers

<p>A single bond involves one shared pair of electrons, a double bond involves two shared pairs, and a triple bond involves three shared pairs of electrons.</p> Signup and view all the answers

<p>H x o H</p> Signup and view all the answers

<p>An oxygen atom has 6 valence electrons and needs 2 more to complete its octet.</p> Signup and view all the answers

<p>A diatomic molecule of oxygen has a double bond because each oxygen atom shares two electrons with another oxygen atom.</p> Signup and view all the answers

<p>Chlorine has an electronic configuration of 2, 8, 7; this means it has a valency of 1.</p> Signup and view all the answers

<p>Cl x o Cl with 6 dots around each Cl in addition to x's and o's.</p> Signup and view all the answers

<p>Nitrogen has 5 valence electrons and needs 3, so it forms a triple bond by contributing 3 electrons to be shared with another nitrogen.</p> Signup and view all the answers

<p>In a water molecule, oxygen forms single bonds with two hydrogen atoms with each sharing one electron.</p> Signup and view all the answers

<p>Hydrogen atoms can only form single covalent bonds, because they only need one more electron.</p> Signup and view all the answers

<p>The number of bonds an atom is likely to form often equals the number of electrons it needs to complete its octet.</p> Signup and view all the answers

<p>Each nitrogen atom in N$_2$ shares three electrons with the other, resulting in a triple bond.</p> Signup and view all the answers

<p>The water molecule (H$_2$O) contains two single covalent bonds between oxygen and hydrogen.</p> Signup and view all the answers

<p>The electron dot structure for Cl$_2$ shows that each chlorine atom shares one valence electron, forming a single covalent bond.</p> Signup and view all the answers

<p>O$_2$ forms a double bond as each oxygen atom shares two electrons, resulting in two shared pairs of electrons.</p> Signup and view all the answers

<p>In H$_2$, each hydrogen atom contributes one electron, forming a single covalent bond through sharing.</p> Signup and view all the answers

<p>The atomic number determines the number of electrons and therefore the valency, which influences bonding capacity.</p> Signup and view all the answers

<p>Covalent bonds form when atoms share pairs of electrons to achieve stable electron configurations.</p> Signup and view all the answers

<p>Electron sharing enables diatomic molecules to complete their valence shells, leading to stability.</p> Signup and view all the answers

<p>Electronegativity affects the distribution of shared electrons, influencing bond polarity in covalent compounds.</p> Signup and view all the answers

<p>In NH3, nitrogen shares three of its electrons with three hydrogen atoms, achieving a full outer shell, while each hydrogen achieves a duet.</p> Signup and view all the answers

<p>Methane (CH4) contains four single covalent bonds, and carbon achieves a noble gas configuration by sharing its four valence electrons with four hydrogen atoms.</p> Signup and view all the answers

<p>N2 has a triple covalent bond, allowing each nitrogen atom to share three pairs of electrons, thus each achieving a stable octet.</p> Signup and view all the answers

<p>Covalent bonds are strong due to the sharing of electron pairs between atoms, but intermolecular forces are weak as they do not involve electron sharing.</p> Signup and view all the answers

<p>Intermolecular forces in covalently bonded substances such as NH3 are generally weaker than the ionic bonds in ionic compounds.</p> Signup and view all the answers

<p>Carbon is tetravalent because it has four valence electrons that it can share to form four covalent bonds, achieving a stable octet.</p> Signup and view all the answers

<p>Achieving noble gas configuration provides stability to the atoms involved, as they have filled outer electron shells which minimizes energy.</p> Signup and view all the answers

<p>Shared electron pairs between atoms create covalent bonds, allowing each atom to fulfill their respective electron configuration needs.</p> Signup and view all the answers

<p>The structure of methane reflects covalent bonding by showing carbon forming four single bonds with hydrogen atoms, utilizing its four valence electrons.</p> Signup and view all the answers

<p>The low melting and boiling points of covalently bonded compounds like methane are due to weaker intermolecular forces compared to the strong ionic bonds.</p> Signup and view all the answers

<p>Diamond has a three-dimensional structure where each carbon is bonded to four others, while graphite has a layered structure where each carbon is bonded to three others in a plane.</p> Signup and view all the answers

<p>The difference arises from the arrangement and bonding of carbon atoms. In diamond, the carbons are in a rigid, three-dimensional lattice while in graphite they form layered hexagonal sheets.</p> Signup and view all the answers

<p>In graphite, each carbon atom is bonded to three others in a plane, forming hexagonal layers. One of these bonds is a double bond, with the extra electron being free to move in the layer making it a good conductor.</p> Signup and view all the answers

<p>Natural diamonds are still considered valuable due to their rarity, size, unique origins and sometimes higher quality.</p> Signup and view all the answers

<p>Allotropes are different structural forms of the same element. Carbon allotropes, like diamond and graphite, are formed by variation in the way the carbon atoms are bonded together.</p> Signup and view all the answers

<p>Fullerenes, like C-60, have a spherical or cage-like structure, whereas diamond has a rigid three-dimensional network, and graphite adopts a layered hexagonal array structure.</p> Signup and view all the answers

<p>Diamond, unlike graphite, is a poor conductor of electricity, hence cannot conduct current, despite its hardness.</p> Signup and view all the answers

<p>Shared electrons in covalent bonds do not produce charged particles, these compounds are typically poor conductors of electricity.</p> Signup and view all the answers

<p>In diamond each carbon atom forms four single covalent bonds in a tetrahedral arrangement. In graphite one of bonds is a double bond and the other 3 bond in the same plane.</p> Signup and view all the answers

<p>Graphite's layered structure allows the layers to slide easily over each other making it a good lubricant, whereas diamond's ridged network structure does not have the same property.</p> Signup and view all the answers

<p>Diamond has a rigid 3D structure, while graphite has a layered hexagonal structure.</p> Signup and view all the answers

<p>Four.</p> Signup and view all the answers

<p>Three.</p> Signup and view all the answers

<p>Graphite is a good conductor of electricity.</p> Signup and view all the answers

<p>By subjecting pure carbon to very high pressure and temperature.</p> Signup and view all the answers

<p>Fullerene (specifically C-60 or Buckminsterfullerene).</p> Signup and view all the answers

<p>Hexagonal.</p> Signup and view all the answers

<p>Its rigid three-dimensional structure.</p> Signup and view all the answers

<p>Diamond is hard, while graphite is soft and slippery.</p> Signup and view all the answers

<p>One of the bonds is a double-bond.</p> Signup and view all the answers

<p>In a diamond, each carbon atom is bonded to four other carbon atoms in a rigid three-dimensional structure. This strong, interconnected network of covalent bonds makes it very difficult to break or deform the structure, resulting in extreme hardness.</p> Signup and view all the answers

<p>Within a sheet of graphite, each carbon atom is bonded to three others in a hexagonal array. This structure includes one double bond and allows for delocalized electrons to move freely, making it a good conductor of electricity.</p> Signup and view all the answers

<p>In carbon compounds, electrons are shared through covalent bonds, forming neutral molecules without free charged particles. Graphite, however, has delocalized electrons within is structure that can move freely, which is why is it able to conduct electricity.</p> Signup and view all the answers

<p>In diamond, each carbon is bonded to four others with strong 3D bonds, resulting in a rigid structure and extreme hardness. In graphite, each carbon is bonded to three in a layered hexagonal arrangement, leading to softness, slipperiness and electrical conductivity via mobile electrons.</p> Signup and view all the answers

<p>Allotropes of carbon have differing atomic arrangements leading to dramatically different physical properties. For example, diamond's 3D network results in hardness, whereas graphite's layered structure results in softness and conductivity.</p> Signup and view all the answers

<p>Fullerenes like C-60, have carbon atoms arranged in spherical or cage-like structures, with C-60 having a football shape. Their discovery expanded the known forms of carbon allotropes beyond just diamond and graphite, highlighting carbon's versatility.</p> Signup and view all the answers

<p>Synthetic diamonds are composed of the same pure carbon structure, and are formed under high pressure and temperature, making them indistinguishable from natural diamonds chemically and structurally.</p> Signup and view all the answers

<p>Diamond has a strong 3D network making it hard; graphite has layered sheets, making it slippery and conductive; fullerenes, like C-60, have closed cage-like structures with properties different than the others. They all have differing structure and properties due to different bonding arrangements.</p> Signup and view all the answers

<p>Though each carbon in graphite is singly bonded to three others, one bond is a double bond, meaning that it shares 4 electrons and its valency is satisfied even though there are 3 atoms attached.</p> Signup and view all the answers

<p>Graphite’s conductivity is due to the delocalized electrons within its layered structure, unlike most compounds where electrons are tightly held in covalent bonds, meaning they can't freely move to conduct electricity.</p> Signup and view all the answers

<p>catenation</p> Signup and view all the answers

<p>saturated compounds</p> Signup and view all the answers

<p>Unsaturated compounds have double or triple bonds between carbon atoms, while saturated compounds only have single bonds.</p> Signup and view all the answers

<p>long chains and branched chains</p> Signup and view all the answers

<p>rings</p> Signup and view all the answers

<p>four</p> Signup and view all the answers

<p>oxygen, hydrogen, and nitrogen</p> Signup and view all the answers

<p>They are very strong.</p> Signup and view all the answers

<p>small size</p> Signup and view all the answers

<p>due to its catenation ability and tetravalency</p> Signup and view all the answers

<p>catenation</p> Signup and view all the answers

<p>double and triple bonds</p> Signup and view all the answers

<p>The carbon-carbon bond is very strong.</p> Signup and view all the answers

<p>Carbon has a valency of four, meaning it can form four bonds with other atoms.</p> Signup and view all the answers

<p>oxygen, hydrogen, nitrogen, sulfur, and chlorine</p> Signup and view all the answers

<p>Carbon's small size is why it forms such strong bonds.</p> Signup and view all the answers

<p>The bonds that carbon forms are very strong.</p> Signup and view all the answers

<p>Carbon exhibits catenation to a much greater extent than other elements like silicon.</p> Signup and view all the answers

<p>Catenation and tetravalency.</p> Signup and view all the answers

<p>Catenation is the property that allows carbon to form long chains or rings of other carbon atoms.</p> Signup and view all the answers

<p>Carbon has a valency of four, allowing it to bond with four atoms from other elements or carbon, creating varied structures.</p> Signup and view all the answers

<p>Carbon compounds are more stable due to the strong carbon-carbon bonds, while silicon compounds are typically more reactive.</p> Signup and view all the answers

<p>Saturated compounds contain only single bonds between carbon atoms, while unsaturated compounds have double or triple bonds.</p> Signup and view all the answers

<p>Carbon's small atomic size allows it to form strong covalent bonds with other elements, enhancing stability.</p> Signup and view all the answers

<p>The ability of carbon to catenate and its tetravalent nature allow for an immense variety of structures.</p> Signup and view all the answers

<p>Carbon forms strong bonds with elements like oxygen and nitrogen, resulting in compounds with specific and varied properties.</p> Signup and view all the answers

<p>Double and triple bonds in carbon compounds create unsaturated structures, affecting reactivity and stability.</p> Signup and view all the answers

<p>Catenation allows carbon atoms to link together in lengthy chains or rings, facilitating complex molecular structures.</p> Signup and view all the answers

<p>Carbon-carbon bonds are exceptionally strong and stable compared to bonds formed by other elements like silicon.</p> Signup and view all the answers

<p>Tetravalency and catenation.</p> Signup and view all the answers

<p>That organic compounds could only be formed within a living system.</p> Signup and view all the answers

<p>Friedrich Wöhler, by preparing urea from ammonium cyanate.</p> Signup and view all the answers

<p>Carbon and hydrogen.</p> Signup and view all the answers

<p>Linking carbon atoms together with a single bond.</p> Signup and view all the answers

<p>By bonding with hydrogen atoms.</p> Signup and view all the answers

<p>Single bonds.</p> Signup and view all the answers

<p>That all atoms are connected via single bonds.</p> Signup and view all the answers

<p>Carbonate and hydrogencarbonate salts.</p> Signup and view all the answers

<p>Tetravalency and catenation.</p> Signup and view all the answers

<p>That they could only be formed within a living system and required a 'vital force'.</p> Signup and view all the answers

<p>Urea.</p> Signup and view all the answers

<p>Carbides, oxides of carbon, carbonate and hydrogencarbonate salts.</p> Signup and view all the answers

<p>Link the carbon atoms together with a single bond.</p> Signup and view all the answers

<p>C2H6</p> Signup and view all the answers

<p>By bonding with hydrogen atoms.</p> Signup and view all the answers

<p>Single bonds.</p> Signup and view all the answers

<p>A carbon compound where all valencies of the atoms are satisfied by single bonds between them.</p> Signup and view all the answers

<p>Tetravalency and catenation.</p> Signup and view all the answers

<p>The 'vital force' theory was the idea that organic compounds could only be formed within living systems. Friedrich Wöhler disproved it.</p> Signup and view all the answers

<p>Organic chemistry.</p> Signup and view all the answers

<p>Link the carbon atoms together with a single bond</p> Signup and view all the answers

<p>All the valencies of the atoms are satisfied by single bonds between them.</p> Signup and view all the answers

<p>That organic compounds could be synthesized outside of living systems.</p> Signup and view all the answers

<p>Linking the carbon atoms together.</p> Signup and view all the answers

<p>Saturated compounds have only single bonds, while unsaturated compounds have at least one double or triple bond.</p> Signup and view all the answers

<p>Carbides, oxides of carbon, and carbonate and hydrogencarbonate salts.</p> Signup and view all the answers

<p>Each carbon-carbon bonds is a single bond.</p> Signup and view all the answers

Chemicals that contain carbon, essential for life.

Carbon is crucial for living organisms and many materials.

Earth's crust has 0.02% carbon; atmosphere contains 0.03% carbon dioxide.

Carbon can form many types of compounds and bonds.

A type of chemical bond where carbon atoms share electrons.

All living organisms are made up of carbon compounds.

Burning carbon compounds produces carbon dioxide and energy.

Carbon exists in nature mainly as carbonates and hydrocarbons.

Everyday items like clothes, food, and books are carbon-based.

Methods to identify carbon in compounds often involve combustion.

Only 0.02% of Earth's crust is carbon, mainly in minerals.

The atmosphere has 0.03% carbon dioxide, a vital gas.

Items like food, clothes, and medicines contain carbon.

A bond where carbon shares electrons with other atoms.

Burning carbon compounds releases carbon dioxide.

All living beings are fundamentally carbon-based.

Despite low abundance, carbon is vital for life and materials.

Burning compounds containing carbon typically produces CO2.

Found in carbonates, hydrocarbons, coal, and petroleum.

Carbon forms a wide variety of compounds and bonds.

Burning carbon compounds produces carbon dioxide and energy.

Only 0.02% of Earth’s crust is carbon, mainly as minerals.

The atmosphere has 0.03% carbon dioxide, essential for life.

All living structures are fundamentally made of carbon compounds.

Carbon primarily exists in nature as carbonates and hydrocarbons.

Methods to identify carbon involve combustion for CO2 confirmation.

Carbon forms strong covalent bonds by sharing electrons.

Carbon's properties allow it to create diverse compounds.

Carbon compounds are poor conductors of electricity and have low melting and boiling points.

Carbon compounds generally have lower melting points compared to ionic compounds.

The boiling points of carbon compounds are also lower than those of ionic compounds.

Ionic compounds have high melting and boiling points due to strong ionic bonds.

Carbon has four valence electrons that determine its reactivity.

Elements tend to react to attain a full outer shell like noble gases.

Carbon cannot easily gain four electrons to become a C4– anion.

Carbon has high energy requirement to lose four electrons, forming C4+ cation.

Carbon compounds do not conduct electricity well, indicating lack of freed ions.

Most carbon compounds do not conduct electricity due to lack of ions.

Carbon has four valence electrons which determine its bonding behavior.

Carbon finds it difficult to gain four electrons to become a C4– anion.

Carbon requires a lot of energy to lose four electrons, forming a C4+ cation.

The bonding in carbon compounds does not produce free ions due to sharing electrons.

Carbon's reactivity stems from its need to gain or lose four electrons for stability.

Carbon struggles to form ions by gaining or losing four electrons due to its atomic structure.

Forming a C4– anion is difficult for carbon as it would require holding ten electrons with only six protons.

Creating a C4+ cation is energy-intensive for carbon as it would leave two electrons bound to six protons.

The lack of free ions in carbon compounds results in their poor conductivity.

Carbon has four valence electrons, crucial for determining its bonding behavior and reactivity.

A bond created by sharing one pair of electrons between two atoms.

A bond formed by sharing two pairs of electrons between two atoms.

A bond created by sharing three pairs of electrons between atoms.

Electrons in the outermost shell of an atom that determine bonding behavior.

A molecule composed of two atoms of the same element.

A representation showing valence electrons as dots around an atom's symbol.

A molecule formed by two hydrogen atoms sharing electrons (H2).

Oxygen atoms share electrons to form a double bond in O2 for stability.

The simplest carbon compound with the formula CH4.

Carbon has four valence electrons available for bonding.

Hydrogen has a valency of 1 because it can form one bond.

Weak forces that exist between molecules.

Covalently bonded molecules have lower melting and boiling points.

A strong bond involving three shared electron pairs.

Ammonia (NH3) has nitrogen bonded to three hydrogens.

Chlorine has atomic number 17 with 7 valence electrons, needing one more for stability.

Two oxygen atoms share two electrons each, forming a double bond (O2).

A diagram showing how nitrogen and hydrogen achieve noble gas configuration in ammonia (NH3).

Methane (CH4) has one carbon atom bonded to four hydrogen atoms.

NH3: a nitrogen atom bonded to three hydrogen atoms creating ammonia.

Chlorine has a valency of 1, needing one electron to complete its octet.

Oxygen forms a double bond by sharing two pairs of electrons between two atoms.

Illustrates the triple bond in a nitrogen molecule (N2).

NH3, a molecule with nitrogen bonded to three hydrogens.

The simplest carbon compound with the formula CH4.

Different forms of carbon with varying physical properties.

In diamond, each carbon atom bonds with four others in a 3D structure.

In graphite, carbon atoms bond in flat hexagonal layers.

A form of carbon arranged like a football, named after Buckminster Fuller.

Graphite conducts electricity due to free electrons between layers.

Diamonds can be created by high pressure and temperature applied to carbon.

Carbon has a valency of 4, allowing it to form four bonds.

Diamond is extremely hard, making it suitable for cutting tools.

Graphite is slippery, used as lubricant and in pencils.

Despite different physical forms, diamond and graphite have similar chemical properties.

Compounds formed by the sharing of electrons between atoms.

Different bonding structures in carbon result in varying physical properties like hardness and conductivity.

Ability of carbon to bond with itself forming long chains or rings.

Carbon compounds with only single bonds between carbon atoms.

Carbon compounds that contain at least one double or triple bond.

Carbon forms very strong bonds due to its small size and electronegativity.

Chemists know millions of carbon compounds, more than all others combined.

Carbon-carbon bonds are strong, allowing stable larger molecules.

Carbon bonds with elements like hydrogen, oxygen, and nitrogen.

Carbon's unique properties enable diverse and stable compounds.

Carbon compounds formed with strong bonds are exceptionally stable.

The strong bond between carbon atoms, vital for stable compounds.

Carbon-carbon bonds are strong and stable, vital for larger molecules.

Millions of known carbon compounds; more than all others combined.

Silicon can form compounds but is more reactive and less stable than carbon.

Carbon can form single, double, or triple bonds, affecting compound properties.

Carbon's small atomic size contributes to the strong bonds it forms.

Carbon's characteristic of having four valence electrons for bonding.

A carbon compound with three carbons and eight hydrogens; an example of a saturated compound.

The scientist who disproved the idea of 'vital force' by synthesizing urea from ammonium cyanate in 1828.

A simple form of carbon compound with two carbons and six hydrogens; follows saturated compound rules.

Carbon-containing compounds, many extracted from natural sources.

A hydrocarbon with the formula C3H8, three carbon atoms.

Disproved the notion that organic compounds require a 'vital force' for synthesis.

The study of carbon compounds, excluding carbides and carbonates.