Ionic and Metallic Structures Quiz

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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.

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. 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.

solid, fixed, lattice, free, molten, free, soluble Signup and view all the answers

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

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. Signup and view all the answers

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

strong, positive, delocalised Signup and view all the answers

What are metallic bonds?

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

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

giant lattice, lose, free Signup and view all the answers

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

Metals have a giant lattice structure, where metal atoms lose their outer shell electrons which are free to move in the structure. 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 __.

high, strong, positive, sea, lot, bonds Signup and view all the answers

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

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. 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.

good, conductivity, delocalised, metallic, solid Signup and view all the answers

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

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. 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 ____.

malleable, shapes, shattering, ductile, breaking Signup and view all the answers

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

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. Signup and view all the answers

What is a covalent bond?

A shared pair of electrons between atoms Signup and view all the answers

What is a covalent bond?

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

What is valency?

The number of electrons needed to attain a complete outer shell Signup and view all the answers

Match the element with its valency:

Hydrogen (H) = 1 Oxygen (O) = 2 Nitrogen (N) = 3 Carbon (C) = 4 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 _ ____.

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

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

Three dimensional network of many carbon atoms Signup and view all the answers

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

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. Signup and view all the answers

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

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

Why is diamond used for making cutting tools?

Diamond has a network of many carbon atoms joined together by strong covalent bonds. Signup and view all the answers

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

4th non-bonding electron is free to move Signup and view all the answers

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

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. Signup and view all the answers

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

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. Signup and view all the answers

Why is graphite soft and used as a lubricant?

Layers slide past each other due to the weak intermolecular forces of attraction between them Signup and view all the answers

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

Single layer/sheet graphite structure Signup and view all the answers

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

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. Signup and view all the answers

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

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. Signup and view all the answers

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

Graphene is just 1 layer of graphite - so it is light Signup and view all the answers

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

Hollow balls - called nanotubes Signup and view all the answers

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

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. Signup and view all the answers

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

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

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

<h1>=</h1> 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 Signup and view all the answers

What is an allotrope?

Different structural forms of the same element Signup and view all the answers

Match the allotrope of carbon with their correct structure:

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

Match the allotrope of carbon with their correct structure:

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 Signup and view all the answers

Match the allotrope of carbon with their correct structure:

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 Signup and view all the answers

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

Graphite Signup and view all the answers

Ionic and Metallic Structures Quiz

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Questions and Answers

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

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

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 ____.

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

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.

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

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

What are metallic bonds?

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

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

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 ____.

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

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

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

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 ______.

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

What is a covalent bond?

What is a covalent bond?

What is valency?

Match the element with its valency:

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

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

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

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

Why is diamond used for making cutting tools?

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

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

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

Why is graphite soft and used as a lubricant?

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

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

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

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

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

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

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

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

What is an allotrope?

Match the allotrope of carbon with their correct structure:

Match the allotrope of carbon with their correct structure:

Match the allotrope of carbon with their correct structure:

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

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

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

Which allotrope of carbon has a low melting point?

Which allotrope of carbon doesn't conduct electricity?

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Ionic compounds have a _ structure, where many and ions are held together by _ 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 __.

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.

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

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

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 __.

Metals have electrical and thermal _. This is because ___ electrons move through the _ structure. This is true in both __ and molten state.

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 ____.

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