Chemistry - Key Concepts - (1) Bonding and Structure
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Questions and Answers

Ionic compounds have a _____ structure, where many ______ and ______ ions are held together by _____ electrostatic forces of attraction.

lattice, positive, negative, strong

State and explain the structure of ionic compounds (2 marks).

Ionic compounds have a lattice structure, where many positive and negative ions are held together by strong electrostatic forces of attraction.

Ionic compounds have ___ melting/boiling points. This is because there are ____ electrostatic forces of ______ between oppositely charged ___. Therefore a ___ of energy is required to break these ____.

high, strong, attraction, ions, lot, bonds

State and explain why the melting and boiling points of ionic compounds are high or low.

<p>Ionic compounds have high melting/boiling points because there are strong electrostatic forces of attraction between oppositely charged ions, requiring a lot of energy to break these bonds.</p> Signup and view all the answers

Ionic compounds do not conduct electricity in a ____ state. This is because ions are ____ in place within a _____ structure and are not ____ to move. Ionic compounds can conduct electricity in a ____ state. This is because ions are ____ to move because most ionic compounds are _____ in water.

<p>solid, fixed, lattice, free, molten, free, soluble</p> Signup and view all the answers

State and explain whether ionic compounds conduct electricity in solid and molten states (3 marks).

<p>Ionic compounds do not conduct electricity in a solid state. This is because ions are fixed in place within a lattice structure and are not free to move. Ionic compounds can conduct electricity in a molten state. This is because ions are free to move because most ionic compounds are soluble in water.</p> Signup and view all the answers

Metallic bonds are ____ electrostatic forces of attraction between ______ metal ions and ________ electrons.

<p>strong, positive, delocalised</p> Signup and view all the answers

What are metallic bonds?

<p>Metallic bonds are strong electrostatic forces of attraction between positive metal ions and delocalised electrons.</p> Signup and view all the answers

Metals have a ____ _____ structure, where metal atoms ____ their outer shell electrons which are ____ to move in the structure.

<p>giant lattice, lose, free</p> Signup and view all the answers

State and explain the structure of metals (2 marks).

<p>Metals have a giant lattice structure, where metal atoms lose their outer shell electrons which are free to move in the structure.</p> Signup and view all the answers

Metals have ___ melting points. This is because there are many ____ attractive forces between ______ metal ions and a ___ of delocalised electrons. Therefore a ___ of energy is required to break these ____.

<p>high, strong, positive, sea, lot, bonds</p> Signup and view all the answers

State and explain why the melting points of metals are high (2 marks).

<p>Metals have high melting points. This is because there are many strong attractive forces between positive metal ions and a sea of delocalised electrons. Therefore a lot of energy is required to break these bonds.</p> Signup and view all the answers

Metals have ____ electrical and thermal _______. This is because _______ electrons move through the _____ structure. This is true in both ____ and molten state.

<p>good, conductivity, delocalised, metallic, solid</p> Signup and view all the answers

State and explain whether metals conduct electricity in solid and molten states (2 marks).

<p>Metals have good electrical and thermal conductivity. This is because delocalised electrons move through the metalic structure. This is true in both solid and molten state.</p> Signup and view all the answers

Metals are ______ because they can be hammered or pressed into different _____ and flat sheets without _______. Metals are _____ because they can be pulled to make wire without ______.

<p>malleable, shapes, shattering, ductile, breaking</p> Signup and view all the answers

Why are metals malleable and ductile? (2 marks).

<p>Metals are maleable because they can be hammered or pressed into different shapes and flat sheets without breaking. Metals are ductile because they can be pulled to make wire without breaking.</p> Signup and view all the answers

What is a covalent bond?

<p>A shared pair of electrons between atoms (A)</p> Signup and view all the answers

What is a covalent bond?

<p>A covalent bond is a shared pair of electrons between atoms.</p> Signup and view all the answers

What is valency?

<p>The number of electrons needed to attain a complete outer shell (B)</p> Signup and view all the answers

Match the element with its valency:

<p>Hydrogen (H) = 1 Oxygen (O) = 2 Nitrogen (N) = 3 Carbon (C) = 4</p> Signup and view all the answers

Covalent bonds have _ types of structure, the ____ _______ ______ such as diamond, ______, graphene and ____ balls. The other type are _____ _______ such as water, _______, chlorine and _____ ______.

<p>2, giant covalent lattice, graphite, bucky, simple covalents, hydrogen, carbon dioxide.</p> Signup and view all the answers

Select the correct structural properties of the covalent bond and allotrope of carbon: Diamond.

<p>Three dimensional network of many carbon atoms (A), Tetrahedral arrangement = each carbon atom is joined to 4 carbon atoms by covalent bonds (B), Giant molecular structure (C)</p> Signup and view all the answers

State and explain whether diamond has a high or low melting point (2 marks).

<p>Diamond has a high melting point. This is because diamond has many strong covalent bonds. This means that lots of energy is required to break them.</p> Signup and view all the answers

State and explain whether diamond can conduct electricity (2 marks).

<p>Diamond can't conduct electricity. This is because diamond has no free electrons within its structure.</p> Signup and view all the answers

Why is diamond used for making cutting tools?

<p>Diamond has a network of many carbon atoms joined together by strong covalent bonds. (A)</p> Signup and view all the answers

Select the correct structural properties of the covalent bond and allotrope of carbon: Graphite.

<p>4th non-bonding electron is free to move (C), Giant molecular structure (A), Hexagonal layered arrangement (B), Three dimensional network of many carbon atoms, each carbon atom is held together to 3 carbon atoms by covalent bonds (D), Layers are held together by weak forces of attraction (@)</p> Signup and view all the answers

State and explain whether graphite can conduct electricity (2 marks).

<p>Graphite can conduct electricity. This is because each carbon atom is joined to 3 other carbon atoms. Therefore, there is one electron per carbon atom that is free to move and carry an electric current.</p> Signup and view all the answers

State and explain whether graphite has a high or low melting point (2 marks).

<p>Graphite has a high melting point. This is because graphite has many strong covalent bonds within its layers. This means that lots of energy is required to break them.</p> Signup and view all the answers

Why is graphite soft and used as a lubricant?

<p>Layers slide past each other due to the weak intermolecular forces of attraction between them (A)</p> Signup and view all the answers

Select the correct structural properties of the covalent bond and allotrope of carbon: Graphene.

<p>Single layer/sheet graphite structure (C), Two-dimensional network of carbon atoms (D), Giant molecular structure (A), 4th non-bonding electron of each carbon atom is free to move (B), Each carbon atom is joined to 3 carbon atoms by covalent bonds (@)</p> Signup and view all the answers

State and explain whether graphene has a high or low melting point (2 marks).

<p>Graphene has a high melting point. This is because graphene has many strong covalent bonds within its layers. This means that lots of energy is required to break them.</p> Signup and view all the answers

State and explain whether graphene can conduct electricity (2 marks).

<p>Graphene can conduct electricity. This is because each carbon atom is joined to 3 other carbon atoms. Therefore, there is one electron per carbon atom that is free to move and carry an electric current.</p> Signup and view all the answers

Graphene is light and strong; why? Provide 2 reasons (1 for each).

<p>Graphene is just 1 layer of graphite - so it is light (A), All covalent bonds in a single layer - hence strong (B)</p> Signup and view all the answers

Select the correct structural properties of the covalent bond and allotrope of carbon: Buckminster fullerenes or Bucky Balls.

<p>Hollow balls - called nanotubes (A), Made by rolling a sheet of graphene (B), 50 carbon atoms are arranged in a pentagon or a hexagon (C)</p> Signup and view all the answers

State and explain whether buckminster fullerenes/bucky balls have a high or low melting point (2 marks).

<p>Buckminster fullerences/bucky balls have low melting points. This is because of the weak intermolecular forces of attraction between there molecules. Therefore they require little energy to break.</p> Signup and view all the answers

State and explain whether buckminster fullerenes/bucky balls can conduct electricity (2 marks).

<p>Buckminster fullerenes/bucky balls can conduct electricity. This is because they have free electrons within their structure in order to carry an electric current.</p> Signup and view all the answers

Match the type of buckminster fullerene with the key property regarding the difference between them:

<h1>=</h1> <p>Bucky Balls = Soft in solid state because they don't have a giant covalent structure, and have weak intermolecular forces of attraction between them Nanotubes = Very strong because they have a giant covalent structure, made of many strong covalent bonds</p> Signup and view all the answers

What is an allotrope?

<p>Different structural forms of the same element (A)</p> Signup and view all the answers

Match the allotrope of carbon with their correct structure:

<p>Diamond = Three dimensional network of carbon atoms Graphite = Three dimensional network of carbon atoms Graphene = Two dimensional network of carbon atoms Buckminsterfullerenes = Hollow Balls</p> Signup and view all the answers

Match the allotrope of carbon with their correct structure:

<p>Diamond = Each carbon atom is joined to 4 carbon atoms by covalent bonding Graphite = 4th non-bonding electron is free to move Graphene = 4th non-bonding electron is free to move Buckminsterfullerene = Made by rolling a sheet of graphene</p> Signup and view all the answers

Match the allotrope of carbon with their correct structure:

<p>Diamond = Tetrahedral arrangement Graphite = Hexagonal layered arrangement Graphene = Single layer/sheet graphite structure Buckminster fullerenes = 50 carbon atoms are arranged in a pentagon or a hexagon</p> Signup and view all the answers

Which two allotropes of carbon have each carbon atom joined to 3 other carbon atoms?

<p>Graphite (B), Graphene (C)</p> Signup and view all the answers

Which allotrope of carbon has layers that are held together by weak intermolecular forces of attraction?

<p>Graphite (B)</p> Signup and view all the answers

Which allotrope of carbon does not have a giant molecular structure?

<p>Buckminster fullerences (D)</p> Signup and view all the answers

Which allotrope of carbon has a low melting point?

<p>Buckminster fullerences (D)</p> Signup and view all the answers

Which allotrope of carbon doesn't conduct electricity?

<p>Diamond (A)</p> Signup and view all the answers

What is the main difference between graphite and graphene?

<p>Graphite has a structure containing layers held together by weak intermolecular forces of attraction while graphene doesn't have any layers and can be described as a single layer/sheet graphite structure.</p> Signup and view all the answers

Which allotrope of carbon is hard-used for making cutting tools?

<p>Diamond (A)</p> Signup and view all the answers

Which allotrope of carbon is soft-used as a lubricant?

<p>Graphite (B)</p> Signup and view all the answers

Which allotrope of carbon is light and strong?

<p>Graphene (C)</p> Signup and view all the answers

Simple covalent bonds/molecular compounds have ___ melting/boiling points. This is because of the ____ intermolecular forces of attraction. This means that ___ energy is required to ____ these intermolecular forces.

<p>low, weak, less, break</p> Signup and view all the answers

State and explain why the melting points of simple covalents/molecular compounds are high or low (2 marks).

<p>Simple covalent bonds/molecular colpounds have low melting/boiling points. This is because of the weak intermolecular forces of attraction. This means that less energy is required to break these intermolecular forces.</p> Signup and view all the answers

Simple covalents/molecular compounds ___ conduct electricity. This is because they don't have any ____ electrons/ions. This means that they cannot carry and ______ current.

<p>can't, free, electric</p> Signup and view all the answers

State and explain whether simple covalents/molecular compounds conduct electricity (2 marks).

<p>Simple covalents/molecular compounds can't conduct electricity. This is because they don't have any free electrons/ions. This means that they cannot carry and electric current.</p> Signup and view all the answers

Simple covalents/molecular compounds have a _____ molecular structure. Atoms within a molecule are joined together by ______ bonds. There are ____ intermolecular forces of attraction between the molecules.

<p>simple, covalent, weak</p> Signup and view all the answers

State and explain the structure of simple covalents/molecular compounds (2 marks).

<p>Simple covalents/molecular compounds have a simple molecular structure. Atoms within a molecule are joined together by covalent bonds. There are weak intermolecular forces of attraction between the molecules.</p> Signup and view all the answers

The bigger the molecule, the _____ the melting/boiling point. This is because the bigger the molecule is, the _____ the intermolecular forces of attraction. This means that more _____ is required to ____ them.

<p>higher, greater, energy, break</p> Signup and view all the answers

Why is it that the bigger the molecule, the higher the melting/boiling point?

<p>This is because the bigger the molecule is, the greater the intermolecular forces of attraction. This means that more energy is required to break them.</p> Signup and view all the answers

Why do longer polymers have higher boiling/melting points than shorter ones?

<p>Longer polymers have stronger intermolecular forces between them. In longer polymers, chains get tangled up with one another. Therefore longer polymers require more energy than shorter polymers to break them.</p> Signup and view all the answers

Longer polymers have _____ boiling/melting points than shorter ones because longer polymers have _____ intermolecular forces between them. In longer polymers, _____ get tangled up with one another. Therefore _____ polymers require more energy than shorter polymers to break them.

<p>higher, stronger, chains, longer</p> Signup and view all the answers

Match the substance with its definition:

<h1>Compound = A substance that can be split into simpler substances because it contains the atoms of two or more elements joined together Molecule = A substance in which two or more atoms are joined together by covalent bonding only Polymer = A long chain molecule made by joining many smaller simpler molecules (monomers) together</h1> Signup and view all the answers

Match the following types of compounds with their corresponding bonding types:

<h1>Ionic compounds = Ionic bonding Metals = Metallic bonding Molecular compounds = Covalent bonding</h1> Signup and view all the answers

Match the type of bonding with the types of atoms involved:

<h1>Covalent bonding = Non-metal + Non-metal</h1> <p>Ionic bonding = Metal + Non-metal Metallic bonding = Metal + Metal</p> Signup and view all the answers

Match the following types of elements with how their bond forms:

<p>Metal = Becomes a positive ion Non-metal = Becomes a negative ion Metal = Loses electrons Non-metal = Gains electrons</p> Signup and view all the answers

Match the type of bond with their corresponding structure:

<p>Metallic = Giant lattice structure Simple covalent/molecular compound = Simple molecular structure Ionic = Lattice structure Giant covalent = Giant molecular structure (mostly)</p> Signup and view all the answers

Match the type of bond with their corresponding melting/boiling point:

<p>Ionic = High melting point Metallic = High melting point Giant covalent = High melting point (mostly) Simple covalent/molecular compound = Low melting point</p> Signup and view all the answers

Match the type of bond with how they conduct electricity:

<p>Metallic = Conduct electricity Simple covalent/molecular compound = Doesn't conduct electricity Ionic = Conduct electricity in a molten state Giant covalent = Conduct electricity (except for Diamond)</p> Signup and view all the answers

Which type of bond creates substances that are malleable and ductile?

<p>Metallic (B)</p> Signup and view all the answers

Which types of bonds share pairs of electrons between atoms?

<p>Giant covalent (C), Simple covalent/molecular compounds (D)</p> Signup and view all the answers

Which type of bond have strong electrostatic forces of attraction between positive metal ions and delocalised electrons?

<p>Metallic (B)</p> Signup and view all the answers

Which type of bond has the allotropes of carbon?

<p>Giant covalent (C)</p> Signup and view all the answers

Match the bonding model with one of their advantages:

<p>Structural formula = Shows number of atoms of each element in a molecule 3D Space filling model = Shows what the molecules look like Ball and stick model = Shows how each atom is bonded to other atoms Metallic model = Shows how positive metal ions are held in a lattice</p> Signup and view all the answers

Match the bonding model with one of their limitations:

<p>Dot and cross diagram = Does not show the relative sizes of the atoms 3D Space filling model = Doesn't explain how the bonds have formed Ball and stick model = Atoms are shown too far apart and there aren't really 'sticks' holding the atoms Metallic model = Doesn't show the positive metal ions vibrating</p> Signup and view all the answers

Match the advantages and limitations of the following bonding models:

<p>Advantage of dot and cross diagram = Shows what happens to electrons when bonds form Advantage of ball and stick model = Shows the molecules 3D shape of the structure Limitation of dot and cross diagram = Does not show the accurate shape of the molecules Limitation of ball and stick model = Doesn't show chemical symbol of each element or bonding/non-bonding electrons</p> Signup and view all the answers

Match the advantages and limitations of the following bonding models:

<p>Advantage of structural formula = Shows the formula of elements or compounds Limitation of structural formula = Doesn't show the relative sizes of the atoms Advantage of 3D space filling model = Shows relative sizes of the atoms Limitation of 3D space filling model = Does not show how many bonds are formed</p> Signup and view all the answers

Match the advantages and limitations of the following bonding models:

<p>Advantage of dot and cross diagram = Explains how the formula of compounds is obtained Limitation of structural formula = Does not show the 3D shape of the molecule Advantage of metallic model = Explains why metals conduct electricity Limitation of 3D space filling model = May not be able to see all the atoms in a complex model version</p> Signup and view all the answers

What type of bonding model is this?

<p>Dot and cross diagram for covalent bonding</p> Signup and view all the answers

What type of bonding model is this?

<p>Structural formula</p> Signup and view all the answers

What type of bonding model is this?

<p>3D Space filling model</p> Signup and view all the answers

What type of bonding model is this?

<p>Ball and stick model</p> Signup and view all the answers

What type of bonding model is this?

<p>Metallic model</p> Signup and view all the answers

Flashcards

Electrostatic forces in ionic compounds

A strong force of attraction between oppositely charged ions within a crystal lattice.

Delocalized electrons in metals

Metals have electrons that are free to move throughout the structure. These electrons can carry heat and electricity.

Valency

The number of electrons an atom needs to gain or lose to achieve a full outer shell.

Covalent bond

A strong bond formed by sharing a pair of electrons between two non-metal atoms.

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Malleability of metals

Metals can be shaped into different forms without breaking due to the ability of layers of metal ions to slide over each other.

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Metallic Lattice

A giant structure where positive metal ions are surrounded by a sea of delocalized electrons.

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Forces in Metallic Lattice

Forces of attraction between positive metal ions and delocalized electrons in metallic lattices.

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Delocalized Electrons

Electrons that are free to move throughout the structure of a metal.

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Ductility of Metals

The ability of a metal to be drawn out into wires without breaking.

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Ionic Lattice Structure

Ionic compounds have a tightly packed structure where positive and negative ions are held together by strong attractions. This structure is called a lattice.

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Metallic Lattice Structure

Metals have a structure where positive metal ions are surrounded by a 'sea' of freely moving electrons. This is called the metallic lattice structure.

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