C3 Structure and Bonding – Papers 1 & 2 (Flashcards)

A comprehensive set of Q&A flashcards covering states of matter, ionic/covalent bonding, giant covalent and metallic structures, nanoparticles, and applications in nanoscience.

What are the three states of matter and their state symbols?

Solid (s), Liquid (l), Gas (g).

How can you determine the state of a substance at a given temperature using data?

Use data such as melting/boiling points to decide whether it is solid, liquid, or gas at that temperature.

In the particle model, how do energy, movement, and attraction between particles change when a substance is heated?

Energy increases, particles move faster, attractions weaken until a phase change occurs.

What are the four phase changes commonly discussed in C3.1?

Melting, Freezing, Boiling, Condensing.

What happens to energy and temperature at the melting point or boiling point?

Temperature remains constant while energy is used to break/form bonds and the substance changes state.

Why do different substances have different melting and boiling points?

Because they have different strengths of intermolecular/ionic/covalent bonds and structures.

How can you represent particle arrangement in the three states of matter?

Solids: tightly packed; Liquids: less ordered; Gases: far apart and moving freely.

What factors affect the rate of evaporation?

Temperature, surface area, air pressure, and presence of other substances.

What is a limitation of models describing states of matter?

They simplify reality and may not capture non-ideal behavior or all conditions.

What particles are involved in ionic bonding?

Metal atoms (forming positive ions) and non-metal atoms (forming negative ions) via electron transfer.

What does a dot-and-cross diagram show for compounds formed between Group 1 and Group 7 elements?

Transfer of electrons from Group 1 metal to Group 7 non-metal, forming ions and an ionic bond.

How do you draw dot-and-cross diagrams for unfamiliar ionic compounds?

Show metal losing electrons to form a cation and non-metal gaining electrons to form an anion, balancing charges.

How does a Group 1 metal atom become a positive ion?

It loses one electron to form a +1 ion (M+).

How does electron transfer enable ionic bonding when Group 1 metal reacts with Group 7 non-metal?

The metal donates electrons to the non-metal, creating oppositely charged ions that attract.

How can you deduce the charge of a monatomic ion from periodic-table position?

Group 1 +1, Group 2 +2, Group 6 -2, Group 7 -1 (noble gases are typically inert).

How does a Group 7 non-metal become a negative ion?

By gaining one electron to form a -1 ion.

What is the basic rule about ionic bonding in terms of charges?

Opposite charges attract.

How does the periodic table relate to the charge on its most stable monatomic ion?

Elements tend to form ions to achieve a noble-gas configuration; charges follow group trends (e.g., +1, +2, -2, -1).

What are the charges of ions for Group 1, Group 2, Group 6, and Group 7 elements?

+1, +2, -2, -1 respectively.

How can you determine the charges of unfamiliar ions using periodic-table positions?

Predict charges based on typical group trends and aim for a stable electron configuration.

How do you generate the formula of an ionic compound given the ion charges?

Balance the total positive and negative charges to zero; use the smallest whole-number ratio.

What is an ionic lattice?

A regular arrangement of ions held together by ionic bonds in a solid.

How do you interpret the formula of familiar ionic compounds to determine the ions present?

Identify the cation and anion and their charges, then balance to neutral.

How can you generate formulas for ionic compounds when the ion charges are given?

Use the cross-charge method to obtain subscripts, then simplify to the smallest whole numbers.

What are two key properties of ionic compounds?

High melting points and ability to dissolve in water.

Why do ionic compounds have high melting points?

Strong electrostatic forces in the lattice require a lot of energy to break.

Why don’t ionic compounds conduct electricity as solids but do when molten or dissolved?

In solids, ions are fixed in the lattice; in molten or dissolved form, ions are mobile and carry charge.

Do ionic compounds conduct electricity when molten or dissolved?

Yes, they do when molten or dissolved.

How do ions move to conduct electricity in solutions or when molten?

Ions become free to move and carry charge.

How can you apply the ionic model to predict properties of ionic compounds?

Consider lattice structure, ion charges, solubility, melting behavior, and conductivity.

What is a covalent bond?

A bond formed by sharing electron pairs between atoms.

How does a covalent bond form in terms of electronic structure?

Atoms share electrons to complete their outer shells, forming a molecule.

Which diagrams can you use for unfamiliar small molecules?

Dot-and-cross diagrams and ball-and-stick diagrams.

How can you recognise a covalent compound from its formula, name, or diagram?

Typically contains nonmetals and shows covalent bonds (shared electrons).

Which small molecules should you be able to draw dot-and-cross and ball-and-stick diagrams for?

H2, Cl2, O2, N2, HCl, H2O, NH3, CH4.

What is a double bond, and how is it formed?

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

What are some familiar examples of covalently bonded small molecules?

H2, Cl2, O2, N2, HCl, H2O, NH3, CH4.

How might the properties of a double bond differ from a single covalent bond?

Double bonds are shorter and stronger, affecting reactivity and physical properties.

Do small covalent molecules have low or high melting and boiling points?

Low melting and boiling points.

How does the size of a molecule affect its melting and boiling points?

Larger molecules generally have higher MP/BP due to greater intermolecular forces.

Do small molecules conduct electricity?

No.

Why do small molecules and polymers generally not conduct electricity?

They do not have free charged particles; electrons are localized in covalent bonds.

How can you compare substances with different bonding in terms of properties?

Ionic: high MP, soluble; covalent small molecules: low MP; metals: conductive and malleable; giant covalent: very high MP (e.g., diamond) and varying conductivities.

What are the main physical properties of diamond and graphite?

Diamond: very hard, high MP, poor electrical conductor; Graphite: layered, conducts electricity, relatively soft.

How can you recognise the structure of diamond and graphite from information?

Diamond has a 3D tetrahedral network; Graphite has layered hexagonal sheets with delocalized electrons within layers.

Why is graphite used as a lubricant and in electrodes?

Delocalized electrons enable conductivity; layers can slide over each other; holds together in sheets.

How can you justify a use for diamond based on its properties?

Its extreme hardness and high melting point make it ideal for cutting tools and industrial applications.

What is the relationship between graphite and graphene?

Graphene is a single layer of graphite; graphite is stacked graphene layers.

How can you recognise the structure of fullerenes and nanotubes?

Fullerenes: spherical cages (e.g., C60); nanotubes: cylindrical tubes composed of rolled graphene sheets.

What are common applications of fullerenes?

Drug delivery, catalysts, lubricants, and materials science applications.

What are the main physical properties of fullerenes?

Molecular carbon structures (spherical), often with unique electronic properties and stability.

What is the structure of fullerenes?

Carbon atoms arranged in a closed cage of pentagons and hexagons (e.g., C60 Buckminsterfullerene).

What uses or properties are associated with graphene, nanotubes, and fullerenes?

Graphene: excellent conductivity and strength; nanotubes: high strength, conductors; fullerenes: unique reactivity and applications in catalysis and medicine.

What is buckminsterfullerene, and what is its formula?

A C60 molecule, a spherical fullerene.

Why might graphene, nanotubes, and fullerenes be valuable in applications?

Because of high strength, large surface area, and unique electrical properties.

Why should nanotechnology research continue?

Potential to advance medicine, energy, electronics, and materials; must balance risks and benefits.

What is a key property of nanoparticles related to surface area to volume?

SA:V increases as particle size decreases, influencing reactivity, dissolution, and other properties.