Structures and Bonding

Structures and Bonding Review

Giant Covalent
Simple Molecules
Metallic and alloys
Giant Ionic

Giant Covalent Structures

Giant Covalent Structures

​What are the 3 examples which you need to know

Diamond
Graphite
Silicon Dioxide [Silica]

Diamond
Each Carbon atom is
bonded to 4 other carbon
atoms covalently. This
makes it strong

Silicon Dioxide
Covalent bonding

Giant covalent structures or macromolecules

Graphite
covalent bonding

Explain the properties of graphite

Property

Explanation

High melting and boiling
point

The covalent bonds between he carbon
atoms are very strong. This means it takes
a lot of energy to overcome these bonds.

Soft

Contains weak intermolecular forces
between the layers which means that the
layers can slide over each other easily
making graphite soft/slippery/lubricant.

Conducts electricity

It has delocalized electrons which can
carry the charge through the structure.

Multiple Select

Which are the correct for the structure of diamond? Tick all the correct answers.

• delocalised electrons

• rigid structure

• layers

• all electrons used in bonding

Explain the properties of Diamond

Property

Explanation

High melting and
boiling point

The covalent bonds between the carbon atoms are
very strong. This means that it takes a lot of energy to
overcome these bonds.

Hard

Each carbon atom is bonded to 4 other carbon atoms.
It is a macromolecule. The strong covalent bonds and
rigid structure means that diamond is very hard.

Does not conduct
electricity

Diamond does not contain any delocalized electrons
which can carry charges.

Multiple Choice

Melting points are very high – a large amount of energy is needed to break all the covalent bonds

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Multiple Choice

Why is diamond strong?

• It's made of carbon
• It doesn't conduct electricity
• It forms 4 strong covalent bonds, it is a macromolecule and a rigid structure

• So it can cut glass

Multiple Choice

Why is graphite so soft?

• A.  The atoms are arranged in hexagons in layers that are held together strongly
• B.  The atoms are arranged in hexagons in layers that are held together weakly by intermolecular forces

• C.  Carbon is strongly bonded to 3 other carbon atoms.
• D.  Carbon is weakly bonded to 3 other carbon atoms.

Multiple Choice

Why does graphite conduct electricity?

• Ions are free to move to carry the charge, through the structure

• Atoms can move through the structure

• Free electrons that can carry the charge through the structure

Multiple Choice

Why is graphite so soft and slippery?

• It is made of layers of atoms with weak forces between them

• It is made of small molecules

• It is an ionic compound

• The covalent bonds are weak

Multiple Choice

Each Carbon atom is bonded to 4 other carbon atoms

• Diamond

• Graphite

• Both

Multiple Choice

Each Carbon atom is bonded to 3 other carbon atoms

• Diamond

• Graphite

• Both

Multiple Choice

Is it the hardest natural substance known

• Diamond

• Graphite

• Both

Multiple Choice

Graphite or Diamond?

• Diamond

• Graphite

• Both

Multiple Choice

Graphite or Diamond?

• Diamond

• Graphite

• Both

Multiple Choice

What structure is shown in the diagram?

• Diamond
• Graphite
• fullerene

Multiple Choice

Elements such as  Silicon, diamond and graphite.  Compounds include  SiO₂

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Multiple Choice

Graphite and diamond are both forms of the element carbon.

Which option shows the number of other carbon atoms that each carbon atom is covalently bonded to in graphite and diamond?

• graphite: 3

  diamond: 3

• graphite: 3

  diamond: 4

• graphite: 4

  diamond: 3

• graphite: 4

  diamond: 4

Multiple Choice

Which substance is a macromolecule?

• ammonia

• carbon dioxide

• diamond

• water

Multiple Select

Diamond and silicon(IV) oxide both have giant structures.

Which statements are correct?

• Silicon(IV) oxide is bonded ionically.

• Both substances are compounds.

• There are strong covalent bonds in diamond.

• Both substances have very high melting points.

Simple Molecules

Multiple Choice

Identify structure shown as simple covalent or other.

• Simple covalent

• Other

Multiple Choice

Identify structure shown as simple covalent or other.

• Simple covalent

• Other

Multiple Choice

Identify the simple covalent structure.

• A

• B

• C

• D

Explanation Slide...

In the ball–and–stick model, each ball represents a particle and the stick the bond between the particles.

Explanation Slide...

The structure is formed due to the strong electrostatic force of attraction between oppositely charged particles.

Explanation Slide...

Magnesium oxide forms an ionic structure because it contains metal and non-metal ions. Metal ions attract all non–metal ions and vice–versa; they bond to all the oppositely charged ions that are closest.

Explanation Slide...

All models have advantages and disadvantages. This type of model does not show the forces of attraction between ions and how these ions are formed. It does show the pattern of ions in the structure between the ions.

Multiple Select

Which type of bonding forms giant structures? Tick all the correct answers.

• ionic

• giant covalent

• metallic

• simple/molecular covalent

Multiple Choice

Which type of bonding contains ions? Tick all the correct answers.

• ionic

• giant covalent

• metallic

• simple/molecular covalent

Multiple Select

Which type of bonding involves the losing and gaining of electrons. Tick all the correct answers.

• ionic

• giant covalent

• metallic

• simple/molecular covalent

• graphite

Multiple Select

Which of the following will conduct electricity as a solid? Tick all the correct answers.

• sodium chloride

• sulfur

• graphite

• copper

• diamond

Multiple Select

Which of the following liquids or solutions will conduct electricity? Tick all the correct answers.

• salty water

• mercury

• bromine

• sugary water

Multiple Select

Which of the following contain weak intermolecular forces?Tick all the correct answers.

• water

• molten sodium chloride

• bromine

• mercury

Multiple Choice

Which structures is a metal?

• A

• B

• C

• D

Multiple Choice

This is a picture of ammonia. What does the symbol X represent in the diagram?

• Neutron

• Proton

• Electron

Multiple Choice

Identify physical properties of the substance shown.

i. low melting point

ii. conducts electricity when solid

iii. high melting point

• i only

• i, ii and iii

• iii only

• i and iii only

Multiple Choice

Use the property described to classify the structure as simple covalent or other.

Conducts electricity only when molten or in solution.

• Simple covalent

• other

Multiple Choice

Use the property described to classify the structure as simple covalent or other.

Exist as a liquid at room temperature.

• Simple covalent

• other

Multiple Choice

Use the property described to classify the structure as simple covalent or other.

Does not conduct electricity under any condition.

• Simple covalent

• other

Metallic Structures and Alloys

Multiple Choice

What type bonding is described here?

Melting points are generally high - lots of energy is needed to overcome the attractions between positive ions and delocalised electrons.

• Simple Covalent

• Metallic

• Ionic

• Giant Covalent

Multiple Choice

Electrons that are free to move in metals

• delocalized electrons
• oxidation number
• chemical bond
• salts

Multiple Choice

What does malleable mean?

• able to be shaped
• will break easily
• can be used for wire
• is shiny

Multiple Choice

At room temperature, most metals are

• liquid
• solid
• gas
• an alloy

Multiple Choice

What is the basis of a metallic bond?

• the attraction of neutral metal atoms.
• the attraction between protons and neutrons.
• the attraction between positive metal ions and interlocking electrons.
• the attraction between positive metal ions and free floating electrons.

Multiple Choice

Many alloys are softer than the elements that are in them.

• True

• False

Multiple Choice

Metals are hard because metals have a

• sea of electrons that tightly hold the nuclei together

• they form triple bonds

• low melting point

• high luster

Multiple Choice

Why does copper wire conduct electricity when a potential difference is applied?

• The crystal lattice breaks down

• Copper (II) ions move to the cathode

• The atoms of copper become ionised

• Bonding electrons in the crystal lattice move

Multiple Choice

What does malleable mean?

• Breaks easily

• Always stays in the same shape

• Can be drawn into wires

• Can be forced into a certain shape without breaking

Multiple Choice

Why are metals malleable?

• The metal ions can easily slide past one another

• The metal ions cannot easily slide past one another

• The metal ions repel one another

• The metal ions attract one another

Giant Ionic Structures

Explain the properties of Giant Ionic Compounds

Multiple Choice

What is the name given to the type of model shown in the diagram?

• ball–and–stick

• particle

• dot–and–cross

• 2D diagram

Multiple Choice

Which of the following types of structure do ionic compounds form?

• giant covalent structures

• 3D lattices of positively and negatively charged ions

• small, simple molecules

• lattice of positively charged ions in a sea of delocalised electrons

Multiple Select

Magnesium oxide, MgO, contains ionic bonds. Which of the following statements about magnesium oxide are correct?

• It contains Mg²⁺ and O²⁻ ions.

• One Mg²⁺ ion is attracted to only one O²⁻ ion.

• Mg²⁺ ions attract all nearby O²⁻ ions.

• It contains MgO simple molecules.

Multiple Choice

The diagram shows a 3D model of the giant ionic structure of magnesium oxide. What is an advantage of this type of model?

• It shows the alternating pattern of positive and negative ions.

• It shows the forces of attraction between the ions.

• It shows how the electrons are transferred.

• It is to scale.

Multiple Choice

Giant lattice structure held together by attraction between  positive and negatively charged ions 

• simple covalent molecules
• metallic
• ionic
• giant covalent 

Multiple Choice

Magnesium bromide is an ionic compound with the chemical formula MgBr₂.  What does the "2" tell you?

• There are 2 bromide ions for every magnesium ion
• Bromide has a 2- charge
• Bromide has a 2+ charge
• There are 2 magnesium ions to every bromide ion

Multiple Choice

Why do ionic compounds conduct electricity when they are molten or dissolved?

• Their ions are free to move.

• Their ions are held in fixed positions.

Multiple Choice

Which two compounds are ionic?

• compound A

• compound B

• compound C

• compound D

• compound E

Multiple Choice

When an atom loses an electron, it becomes a:

• positive ion
• negative ion
• neutral ion
• neutral atom

Multiple Select

Magnesium oxide is insoluble in water. Can magnesium oxide conduct electricity?

Select yes or no and a reason.

• Yes

• No

• Magnesium oxide can be heated so that it melts and conducts electricity.

• Magnesium oxide doesn't dissolve, so it stays in its solid state and doesn't conduct electricity.

Multiple Choice

A 'giant lattice structure held together by attraction between positive and negatively charged ions' describes what?

• simple covalent molecules

• metallic

• ionic

• giant covalent

Multiple Select

Tick all the properties of ionic compounds

• Dissolve in water

• low melting and boiling points

• High melting and boiling points

• Conduct electricity when solid

• Conduct electricity when molten or aqueous

Multiple Select

Can ionic substances conduct electricity? Select all that apply.

• Never

• As a liquid/molten

• As a solid

• Dissolved in water/as a solution

Multiple Choice

What happens when magnesium loses 2 electrons?

• It stabilizes to a net charge of 0

• It turns into an atom

• It becomes negatively charged

• It becomes positively charged

Multiple Choice

Which elements tend to lose electrons?

• Metals

• Non-metals

Multiple Select

Which of the following will have high/very high melting points? Tick all the correct answers.

• sodium chloride

• water

• graphite

• copper

• bromine

Multiple Choice

The metal ion has a ________________ charge.

• negative

• positive

• neutral/no

Multiple Choice

How is a metal ion formed?

• gaining an electron

• losing an electron

• sharing electrons