C3

Question 1

Define allotropes of carbon.

Answer 1

Allotropes of carbon are different structural forms of carbon atoms that exist in the same physical state but have different arrangements.

Question 2

Structure of Diamond?

Answer 2

Diamond consists of carbon atoms arranged in a tetrahedral lattice structure, with each carbon atom bonded to four other carbon atoms.

Question 3

Properties of Diamond?

Answer 3

Diamond is the hardest known natural material, has high thermal conductivity, is transparent, and has a high refractive index

Question 4

Structure of Graphene?

Answer 4

Graphene is a single layer of carbon atoms arranged in a two-dimensional honeycomb lattice structure.

Question 5

Properties of Graphene

Answer 5

Graphene is the thinnest and strongest material known, conducts electricity and heat very well, and has potential applications in electronics and materials science

Question 6

Structure of Buckminsterfullerene

Answer 6

Buckminsterfullerene is a spherical molecule composed of 60 carbon atoms arranged in a hollow cage-like structure, consisting of 20 hexagons and 12 pentagons

Question 7

Properties of Buckminsterfullerene

Answer 7

Buckminsterfullerene is stable, conducts electricity, and has potential applications in nanotechnology, medicine, and materials science

Question 8

Structure of Carbon Nanotubes?

Answer 8

Carbon nanotubes are cylindrical molecules composed of carbon atoms arranged in a hexagonal lattice structure, forming tubes of nanometer-scale diameter

Question 9

Properties of Carbon Nanotubes?

Answer 9

Carbon nanotubes have high tensile strength, are excellent conductors of electricity, and have potential applications in electronics, materials science, and nanotechnology

Question 10

Structure of Graphite?

Answer 10

Graphite consists of carbon atoms arranged in layers of hexagonal rings, with weak van der Waals forces between the layers. Each carbon atom is bonded to three other carbon atoms in the same layer.

Question 11

Properties of Graphite

Answer 11

Graphite is soft, slippery, and a good conductor of electricity due to the presence of delocalized electrons between layers. It is used in pencils, lubricants, and as a moderator in nuclear reactors.

Question 12

Definition of Covalent Bonding

Answer 12

Covalent bonding is the sharing of electron pairs between atoms to form molecules

Question 13

How Covalent Bonds Form

Answer 13

Atoms share electrons to achieve a stable electron configuration, usually by filling their outermost energy level (valence shell).

Question 14

Types of Elements Involved in Covalent Bonding

Answer 14

Covalent bonds typically form between nonmetal atoms, as they have similar electronegativities and tend to share electrons rather than transfer them.

Question 15

Structure of Covalent Compounds?

Answer 15

Covalent compounds can have simple molecular structures (e.g., H2O, CO2) or giant covalent structures (e.g., diamond, graphite)

Question 16

Characteristics of Covalent Bonds?

Answer 16

Covalent bonds are strong within molecules but weak between molecules. They have low melting and boiling points compared to ionic compounds.

Question 17

Examples of Covalent Compounds?

Answer 17

Examples include water (H2O), methane (CH4), ammonia (NH3), carbon dioxide (CO2), and hydrogen chloride (HCl).

Question 18

Behavior of Covalent Compounds in Water?

Answer 18

Covalent compounds tend to be insoluble or only slightly soluble in water, as they do not dissociate into ions when dissolved.

Question 19

Definition of Ionic Bonding

Answer 19

Ionic bonding is the transfer of electrons from one atom to another, resulting in the formation of positively and negatively charged ions.

Question 20

Types of Elements Involved in Ionic Bonding

Answer 20

Ionic bonds typically form between metals and nonmetals, where the metal atom loses electrons to form a positively charged cation, and the nonmetal atom gains electrons to form a negatively charged anion.

Question 21

Formation of Ionic Compounds

Answer 21

Ionic compounds are formed by the electrostatic attraction between positively and negatively charged ions, resulting in a lattice structure.

Question 22

Characteristics of Ionic Compounds

Answer 22

Ionic compounds have high melting and boiling points, are brittle, and conduct electricity when dissolved in water or molten state (but not in solid form).

Question 23

Properties of Ionic Bonds

Answer 23

Ionic bonds are strong electrostatic forces of attraction between oppositely charged ions. They are non-directional and form a three-dimensional lattice structure.

Question 24

Examples of Ionic Compounds

Answer 24

Examples include sodium chloride (NaCl), potassium iodide (KI), calcium chloride (CaCl2), magnesium oxide (MgO), and aluminum oxide (Al2O3)

Question 25

Definition of Metallic Bonding

Answer 25

Metallic bonding is the electrostatic attraction between positively charged metal ions and delocalized electrons within a metal structure

Question 26

Role of Valence Electrons

Answer 26

Valence electrons in metal atoms become delocalized and are free to move throughout the metal lattice, forming a “sea of electrons.”

Question 27

Characteristics of Metallic Bonds

Answer 27

Metallic bonds are non-directional, strong, and result in malleable, ductile, and good conductors of heat and electricity.

Question 28

Formation of Metallic Crystals

Answer 28

Metallic crystals consist of closely packed positive metal ions surrounded by a “sea” of delocalized electrons.

Question 29

Conductivity of Metals

Answer 29

Metals conduct electricity due to the presence of delocalized electrons that are free to move and carry electric charge

Question 30

Malleability and Ductility

Answer 30

Metallic bonding allows metal atoms to slide past each other without breaking bonds, making metals malleable (able to be hammered into thin sheets) and ductile (able to be drawn into wires).

Question 31

Strength of Metallic Bonds

Answer 31

Metallic bonds are strong due to the attraction between positively charged metal ions and the sea of delocalized electrons.

Question 32

Definition of Nanoparticles

Answer 32

Nanoparticles are particles with dimensions in the nanometer range, typically between 1 and 100 nanometers.

Question 33

Properties of Nanoparticles

Answer 33

Nanoparticles often exhibit unique physical, chemical, and optical properties due to their small size and high surface area-to-volume ratio.

Question 34

Definition of Chemical Bonding:

Answer 34

Chemical bonding is the process by which atoms combine to form molecules or compounds through the sharing, gaining, or losing of electrons.