C2 Bonding, structure, and the properties of matter - J Bryant | Library

4

Draggable item		Corresponding Item
Covalent bonding		Transferring electrons
Metallic bonding		Sharing electrons
Ionic bonding		Delocalised electrons through structure

4.2.1.1

Required

1

Draw the ion formed from the Li atom

4.2.1.2

Required

1

Draw the ion formed from the Na atom

4.2.1.2

Required

1

Draw the ion formed from the K atom

4.2.1.2

Required

1

Draw the ion formed from the F atom

4.2.1.2

Required

1

Draw the ion formed from the Cl atom

4.2.1.2

1

What type of bonding is shown in the video below? ALSO, explain how you know.

4.2.1.2

Required

1

What is the ion formed when Magnesium (Atomic Number: 12) loses two electrons?

4.2.1.2

Required

1

Draw dot and cross diagram - Calcium sulfide

4.2.1.2

1

Draw electron configuration diagrams to show how an atom of lithium becomes an ion

4.2.1.2

1

Potassium is in Group 1. How many electrons does it lose when it becomes an ion?

4.2.1.2

1

What kind of bonding is this?

4.2.1.2

Required

1

What is the ion formed by Sodium (Na)?

4.2.1.2

Required

1

What is the ion formed by Oxygen (O)?

4.2.1.2

Required

1

What ion does Calcium (Ca) form?

4.2.1.2

Required

1

What ion does Fluorine (F) form?

4.2.1.2

Required

1

Which ion has a 2+ charge?

4.2.1.2

Required

1

What is the ion formed when Magnesium (Atomic Number: 12) loses two electrons?

4.2.1.2

Required

1

Draw the ion formed from the Li atom

4.2.1.2

Required

1

Draw the ion formed from the Na atom

4.2.1.2

Required

1

Draw the ion formed from the K atom

4.2.1.2

Required

1

Draw the ion formed from the F atom

4.2.1.2

Required

1

Draw the ion formed from the Cl atom

4.2.1.2

Required

1

Lithium LOSES an electron (electrons are negative). What charge does it have?

4.2.1.2

Required

1

Beryllium LOSES two electrons (electrons are negative). What charge does it have?

4.2.1.2

Required

1

Magnesium LOSES two electron (electrons are negative). What charge does it have?

4.2.1.2

Required

1

Fluorine GAINS an electron - what charge does it have?

4.2.1.2

Required

1

Draw dot and cross diagram - Lithium fluoride

4.2.1.2

Required

1

Draw dot and cross diagram - Magnesium chloride

4.2.1.2

Required

1

Draw dot and cross diagram - Lithium Oxide

4.2.1.2

Required

1

Draw dot and cross diagram - Calcium sulfide

4.2.1.2

Required

1

Why do metals form positive ions, while non-metals form negative ions?

4.2.1.2

Required

1

Use dot and cross diagram to show the electronic changes that occur during the reaction between calcium and fluorine.

4.2.1.2

5

Match the formulas of the following ionic compounds to their names.

Draggable item		Corresponding Item
MgO		Sodium sulfide
		Potassium chloride

4.2.1.2

5

Match the names of the following ionic compounds to their formulas.

Draggable item		Corresponding Item
Aluminum chloride		Be3P2

4.2.1.2

1

What is the formula for lithium sulfide?

4.2.1.2

Required

1

What is the formula for potassium bromide?

4.2.1.2

Required

1

What is the formula for beryllium nitride?

4.2.1.2

1

What is the formula for aluminum sulfide?

4.2.1.2

Required

1

What is the formula for sodium phosphide?

4.2.1.2

Required

1

When atoms gain or lose electrons, they do not form ions

4.2.1.2

Required

1

When Li loses an electron, it becomes Li+1

4.2.1.2

1

Draw electron configuration diagrams to show how an atom of lithium becomes an ion

4.2.1.2

1

Draw electron configuration diagrams to show how an atom of fluorine becomes an ion

4.2.1.2

1

Potassium - Use your periodic table to find the number of electrons

4.2.1.2

1

Draw the atom Boron and how it becomes the ion B+3

4.2.1.2

1

In a giant ionic structure, there are strong electrostatic forces in all directions between _______  charged particles.

4.2.1.3

1

4.2.1.3

4.2.1.4

1

How are these compounds classified?

Methane
Magnesium Oxide
Sodium Chloride
Carbon Dioxide

Small Covalent Compounds
Ionic Compounds

4.2.1.2

4.2.1.4

2

Describe the difference between an ionic and covalent bond.

4.2.1.2

4.2.1.4

1

Complete the figure below to show the outer shell electrons in a molecule of Si2H6

4.2.1.4

1

Give one limitation of using a dot and cross diagram to represent a molecule.

4.2.1.4

1

What kind of chemical bonding is taking place with Bromine?

4.2.1.4

3

This is Hydrogen Cyanide and it follows all the rules of covalent bonding. Use your knowledge of covalent bonding to complete the diagram. (Grade 7/8 Bonding Question)

4.2.1.4

1

How are these compounds classified?

Methane
Magnesium Oxide
Sodium Chloride
Carbon Dioxide

Small Covalent Compounds
Ionic Compounds

4.2.1.2

4.2.1.4

2

Describe the difference between an ionic and covalent bond.

4.2.1.2

4.2.1.4

2

The chlorine molecule forms a single bond. Please complete the diagram

4.2.1.4

1

A chemical bond formed when two atoms share one or more pairs of valence electrons.

4.2.1.4

1

Which one has the stronger bond?

4.2.1.4

1

Which of the following is a covalent compound?

4.2.1.4

1

How many valence electrons are shared in each covalent bond?

4.2.1.4

1

What kind of bonding is this?

4.2.1.4

1

In a metallic bond, where are the electrons located?

4.2.1.5

1

Give the definition of metallic bonding ( 1 mark)

4.2.1.5

2

4.2.2.1

2

4.2.2.1

2

4.2.2.1

1

4.2.2.1

1

4.2.2.1

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4.2.2.1

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4.2.2.1

1

4.2.2.1

1

4.2.2.1

1

4.2.2.1

1

4.2.2.1

1

What is the state of matter that has a definite shape and volume?

4.2.2.1

1

Which of the following are states of matter?

4.2.2.1

1

Water can exist in all three states of matter (solid, liquid, gas).

4.2.2.1

1

Can you give an example of a gas that you breathe in?

4.2.2.1

1

Ice is the solid state of water.

4.2.2.1

9

Drag the characteristics or details to the correct state of matter.

4.2.2.1

20

What is matter with a definite shape and definite volume?

4.2.2.1

20

What is matter that has a definite volume, but NOT a definite shape.

4.2.2.1

10

Type the name for each change of state next to the letter that represents this change on the diagram below

4.2.2.1

10

Substances are usually the most dense when they are in the solid state.

4.2.2.1

10

Which of the following is NOT true? As thermal energy is added to a substance...

4.2.2.1

1

If a substance cools down, its molecules

4.2.2.1

1

If a substance heats up, its molecules

4.2.2.1

1

4.2.2.2

1

4.1.2.6

4.2.2.2

1

4.1.2.5

4.2.2.2

1

Why don’t covalent compounds conduct electricity?

4.2.2.3

1

Why are ionic substances soluble in water?

4.2.2.3

1

Why don’t covalent compounds conduct electricity?

4.2.2.3

2

Why do ionic compounds have high melting and boiling points?

4.2.2.3

2

Why are most ionic compounds soluble in water?

4.2.2.3

1

In our practical, did ionic compounds dissolve in water and become soluble?

4.2.2.3

1

Did the ionic compounds conduct electricity?

4.2.2.3

1

Did the ionic compounds have high or low melting points?

4.2.2.3

5

Match keyword to definition

Draggable item		Corresponding Item
charge carrier		A measure of how well a material conducts electricity.
		A measure of how well a material transfers energy when heated.

4.2.2.3

1

Which of the following ionic substances is not a good electrical conductor?

4.2.2.3

2

Why do ionic compounds have high melting and boiling points?

4.2.2.3

2

Why are most ionic compounds soluble in water?

4.2.2.3

2

Why is the melting point of magnesium oxide, MgO, higher than sodium chloride, NaCl?

4.2.2.3

1

Why don’t covalent compounds conduct electricity?

4.2.2.3

1

Why are ionic substances soluble in water?

4.2.2.3

1

4.2.2.3

1

4.1.1.1

4.2.1.2

1

4.2.2.3

2

4.2.2.3

1

Why do ionic compounds have higher melting points than simple covalent compounds?

4.2.2.3

4.2.2.4

1

Which of these is the property of ionic and small covalent molecules?

Does Not Conduct Electricity
Conducts Electricity when Dissolved
Forms Giant Ionic Lattice
High Melting Point
Low Melting Point

4.2.2.3

4.2.2.4

1

Giant structure or simple molecule?

4.2.2.4

1

Giant structure or simple molecule?

4.2.2.4

1

Giant structure or simple molecule?

4.2.2.4

1

Why do ionic compounds have higher melting points than simple covalent compounds?

4.2.2.3

4.2.2.4

1

Which of these is the property of ionic and small covalent molecules?

Does Not Conduct Electricity
Conducts Electricity when Dissolved
Forms Giant Ionic Lattice
High Melting Point
Low Melting Point

4.2.2.3

4.2.2.4

2

Poly(ethene) is produced from ethene.
The structure of ethene is:

Complete the structure of poly(ethene)

4.2.2.5

1

Complete the missing parts of the sentence

Polymers are  _______ molecules made up of smaller, repeating units. Each smaller individual molecule is called a  _______ and they join together in a process called _______ .

4.2.2.5

1

Which state of matter are most polymers at room temperature

4.2.2.2

4.2.2.5

1

Giant structure or simple molecule?

4.2.2.6

1

Giant structure or simple molecule?

4.2.2.6

1

Giant structure or simple molecule?

4.2.2.6

1

Giant structure or simple molecule?

4.2.2.6

6

Properties

Low melting and boiling points
Very high melting points
Almost never conduct electricity
Gases or liquids
Never conduct electricity

4.2.2.4

4.2.2.6

1

(a)Explain why silicon dioxide has a high melting point. (2 marks)

4.2.2.6

1

(a)Suggest why the melting point of silicon dioxide is higher than the melting point of sodium chloride. (1 mark)

4.2.2.3

4.2.2.6

1

4.2.2.3

6

Sort the covalent compounds

Silicon Dioxide
Diamond
Oxygen
Graphite
Hydrogen

4.2.2.4

4.2.2.6

3

4.2.2.6

1

Giant covalent structures are not as strong as small covalent molecules due to their smaller size.

4.2.2.6

1

Giant covalent structures like diamond, graphite, and silicon dioxide generally have high melting and boiling points.

4.2.2.6

1

All giant covalent structures are insulators, as they cannot conduct electricity.

4.2.2.6

1

Which is NOT a common property of alloys?

4.2.2.7

1

Match the vocabulary terms to their definitions

Draggable item		Corresponding Item

4.2.2.7

1

Explain why metals can conduct electricity and are malleable? (2 marks)

4.2.2.7

1

What is the primary reason metals are good conductors of electricity?

4.2.2.7

1

What is an alloy?

4.2.2.7

1

Why do alloys typically have more advantageous properties than pure metals?

4.2.2.7

1

Match the property to the right type of covalent structure.

Draggable item		Corresponding Item
Low melting and boiling points		Giant covalent structures
High melting and boiling points		Diamond
Does not conduct electricity		Small covalent molecules

4.2.2.4

4.2.2.6

4.2.3.1

1

Which of the following properties do these structures hold in terms of their hardness?

Diamond
Silicon dioxide
Methane
Graphite

Hard
Soft

4.2.1.4

4.2.2.6

4.2.3.1

1

Match the property to the appropriate covalent form.

Draggable item		Corresponding Item
Conducts electricity		Graphite
Low hardness		Small covalent molecules
Extremely hard and strong		Diamond

4.2.2.4

4.2.3.1

4.2.3.2

1

Match the covalent structure with the correct description about structure.

Draggable item		Corresponding Item
Layers can slide over each other		Carbon nanotube
Form three-dimensional network		Graphite
Regular network of carbon atoms in a hexagonal pattern		Diamond and silicon dioxide

4.2.2.6

4.2.3.1

…

1

Match each statement with the right covalent structure(s).

Draggable item		Corresponding Item
Usually gases or liquids at room temperature		Small covalent molecules
Not soluble in water		Giant covalent structures
Hard, lustrous and have high thermal conductivity		Diamond

4.2.2.4

4.2.2.6

4.2.3.1

1

What is a distinctive feature of the structure of diamond?

4.2.3.1

1

Why can graphite conduct electricity?

4.2.3.2

1

Graphite and other giant covalent structures are easily dissolved in water.

4.2.3.2

1

What is this?

4.2.3.1

1

1a:

4.2.2.7

1

1b:

4.2.4.2

1

Which of the following is a correct conversion in the metric
system?

WS4.5

1

Which of the following values could describe the size of a
nanoparticle?

WS4.5

1

MS5c

1

MS5c

1

MS1c

1

MS5c

1

MS5c

1

MS1c

1

How does the surface area to volume ratio change when a bulk
material is split into smaller nanoparticles?

4.2.4.1

1

WS4.5

6

Calculate the surface area to volume ratio for a nanoparticle that is a
cube with a side length of 15 nm, and one of 60 nm. No units are required

Surface area 1 = _______ 
Volume 1 = _______ 
SA:V 1 = _______ 

Surface area 2 = _______ 
Volume 2 = _______ 
SA:V 2 =_______ 

MS1c

MS5c

1

The properties of nanoparticles are identical to those of the same materials in
bulk form.

4.2.4.1

1

Justify your above answer

4.2.4.1

6

Titanium dioxide nanoparticles are used in sunscreen,
and silver nanoparticles are used in socks. Explain how the properties of these
nanoparticles makes them suitable for each application.

4.2.4.1

4.2.4.2

6

Consider the potential risks associated with the inhalation of nanoparticles.

Describe and explain what those risks could be.

Describe how society might address the use of nanoparticles in industry.

4.2.4.2

WS1.4

3

Explain how a high surface area to volume ratio of a substance used
as a catalyst affects the reactivity of particles.

4.2.4.1

4.2.4.2

Draggable item		Corresponding Item
MgO		Sodium sulfide
Mg3N2		Potassium chloride
KCl		Magnesium oxide
Na2S		Lithium sulfide
Li2S		Magnesium nitride

Draggable item		Corresponding Item
Aluminum chloride		Be3P2
Sodium oxide		RbBr
Potassium nitride		Na2O
Rubidium bromide		AlCl3
Beryllium phosphide		K3N

Draggable item		Corresponding Item
Ductility/Ductile		Means a substance can be pounded or hammered into thin sheets. (can bend)
Malleabitilty		means if an object can transfer heat or electricity
Luster		How an object reflects light
Physical State		How the surface of an object looks or feels
Texture		if a substance can be made in to thin wire
Conductivity		Refers to if an object is a solid, liquid or gas

Draggable item		Corresponding Item
charge carrier		A measure of how well a material conducts electricity.
electrical conductivity		A measure of how well a material transfers energy when heated.
melting point		Temperature at which a substance changes from solid to a liquid state.
thermal conductivity		A particle that enables electrical conductivity.
Solubility		How well a solute dissolves in a solvent