C2 Bonding, structure, and the properties of matter

Last updated 6 days ago

178 Nsɛmmisa

4.2.1.1 Chemical Bonds

4.2.1.1

4.2.1.2 Ionic Bonding

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

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4.2.1.2

4.2.1.3 Ionic Compounds

4.2.1.3

4.2.1.4 Covalent Bonding

4.2.1.3

4.2.1.4

4.2.1.2

4.2.1.4

4.2.1.2

4.2.1.4

4.2.1.2

4.2.1.4

4.2.1.2

4.2.1.4

4.2.1.5 Metallic Bonding

4.2.1.5

4.2.2.1 The Three states of Matter

4.1.1.1

4.2.2.1

4.2.2.2 State Symbols

4.2.2.2

4.1.2.6

4.2.2.2

4.1.2.5

4.2.2.2

4.2.2.3 Properties of Ionic Compounds

4.2.2.3

4.2.2.4 Properties of small molecules

4.2.2.4

4.2.2.1

4.2.2.4

4.2.2.1

4.2.2.4

4.2.2.1

4.2.2.4

4.2.2.3

4.2.2.4

4.2.2.3

4.2.2.4

4.2.2.3

4.2.2.4

4.2.2.3

4.2.2.4

4.2.2.5 Polymers

4.2.2.5

4.2.2.2

4.2.2.5

4.2.2.6 Giant Covalent Structures

4.2.2.4

4.2.2.6

4.2.2.4

4.2.2.6

4.2.2.7 Properties of Metals and Alloys and 4.2.2.8 Metals as Condudctors

4.2.2.7

4.2.3 Structure and bonding of carbon

4.2.2.4

4.2.2.6

4.2.3.1

4.2.1.4

4.2.2.6

4.2.3.1

4.2.2.4

4.2.3.1

4.2.3.2

4.2.2.6

4.2.3.1

…

4.2.2.4

4.2.2.6

4.2.3.1

4.2.3.2

4.2.3.1

4.2.4 Bulk and surface properties of matter including nanoparticles

WS4.5

4.2.4.1

WS4.5

MS1c

MS5c

4.2.4.1

4.2.4.2

WS1.4

4.2.4.1

4.2.4.2

C2 Bonding, structure, and the properties of matter

Last updated 6 days ago

178 Nsɛmmisa

4.2.1.1 Chemical Bonds

Sort the type of bonding with its description

Draggable item		Corresponding Item
Covalent bonding		Transferring electrons
Metallic bonding		Sharing electrons
Alloy		Delocalised electrons through structure
Ionic bonding		Mixture of a metal and another element

4.2.1.1

4.2.1.2 Ionic Bonding

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Draw the ion formed from the Li atom

4.2.1.2

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Draw the ion formed from the Na atom

4.2.1.2

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Draw the ion formed from the K atom

4.2.1.2

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Draw the ion formed from the F atom

4.2.1.2

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Draw the ion formed from the Cl atom

4.2.1.2

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

4.2.1.2

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

Mg-

Mg+

Mg2-

Mg2+

4.2.1.2

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Draw dot and cross diagram - Calcium sulfide

4.2.1.2

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

4.2.1.2

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

4.2.1.2

What kind of bonding is this?

4.2.1.2

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What is the ion formed by Sodium (Na)?

Na⁺

Na^-

Na²⁺

Na^2-

4.2.1.2

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What is the ion formed by Oxygen (O)?

O^2-

O²⁺

O⁺

O^-

4.2.1.2

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What ion does Calcium (Ca) form?

Ca²⁺

Ca^-

Ca⁺

Ca^2-

4.2.1.2

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What ion does Fluorine (F) form?

F^-

F^2-

F²⁺

F⁺

4.2.1.2

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Which ion has a 2+ charge?

An ion that has lost two protons

An ion that has 2 protons

An ion that has lost two electrons

An ion that has gained two electrons

4.2.1.2

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

Mg-

Mg+

Mg2-

Mg2+

4.2.1.2

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Draw the ion formed from the Li atom

4.2.1.2

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Draw the ion formed from the Na atom

4.2.1.2

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Draw the ion formed from the K atom

4.2.1.2

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Draw the ion formed from the F atom

4.2.1.2

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Draw the ion formed from the Cl atom

4.2.1.2

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

-1

4.2.1.2

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

-1

4.2.1.2

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

4.2.1.2

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Fluorine GAINS an electron - what charge does it have?

-1

-2

-3

4.2.1.2

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Draw dot and cross diagram - Lithium fluoride

4.2.1.2

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Draw dot and cross diagram - Magnesium chloride

4.2.1.2

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Draw dot and cross diagram - Lithium Oxide

4.2.1.2

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Draw dot and cross diagram - Calcium sulfide

4.2.1.2

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

4.2.1.2

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

4.2.1.2

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

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

4.2.1.2

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

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

4.2.1.2

What is the formula for lithium sulfide?

LiS₂

LiS

Li₂S

Li₂S₂

4.2.1.2

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What is the formula for potassium bromide?

K₂Br₂

KBr₂

K₂Br

KBr

4.2.1.2

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What is the formula for beryllium nitride?

Be₂N

Be₃N₂

Be₂N₃

BeN

4.2.1.2

What is the formula for aluminum sulfide?

Al₃S

Al₂S₃

AlS

Al₃S₂

4.2.1.2

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What is the formula for sodium phosphide?

NaP₃

Na₃P

Na₃P₃

NaP

4.2.1.2

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

Nokorɛ

Ɛnyɛ ampa

4.2.1.2

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When Li loses an electron, it becomes Li⁺¹

Nokorɛ

Ɛnyɛ ampa

4.2.1.2

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

4.2.1.2

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

4.2.1.2

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

4.2.1.2

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

4.2.1.2

4.2.1.3 Ionic Compounds

4.2.1.3

4.2.1.4 Covalent Bonding

Ionic Compounds
Simple Molecules

4.2.1.3

4.2.1.4

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

Describe the difference between an ionic and covalent bond.

4.2.1.2

4.2.1.4

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

4.2.1.4

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

4.2.1.4

What kind of chemical bonding is taking place with Bromine?

Triple bond

Double bond

Quadruple bond

Single bond

4.2.1.4

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

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

Describe the difference between an ionic and covalent bond.

4.2.1.2

4.2.1.4

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

4.2.1.4

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

Ionic bond

Common bond

Covalent bond

Isotope bond

4.2.1.4

Which one has the stronger bond?

Oxygen

Nitrogen

4.2.1.4

Which of the following is a covalent compound?

SiO₂

NaCl

CaCl₂

Fe₂O₃

4.2.1.4

How many valence electrons are shared in each covalent bond?

4.2.1.4

What kind of bonding is this?

4.2.1.4

4.2.1.5 Metallic Bonding

In a metallic bond, where are the electrons located?

In the nucleus

In a 'sea' of delocalised electrons

They are evenly distributed among the protons

In the outer shell of the atoms

4.2.1.5

Give the definition of metallic bonding ( 1 mark)

4.2.1.5

4.2.2.1 The Three states of Matter

Which friend is most correct?

4.1.1.1

4.2.2.1

These particles are most likely in what state?

Solid

Liquid

Gas

All of the above

4.2.2.1

Gas particles have the least amount of kinetic energy, particles are slow, and particles virbrate.

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

Solid has defintie shape and does not change volume

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

Liquid does....

change shape and change volume

change shape but not volume

not change shape but change volume

not change shape and not change volume

4.2.2.1

The element chlorine is a

solid

liquid

gas

4.2.2.1

Draw the particles in a solid

4.2.2.1

Draw the particles in a liquid

4.2.2.1

Draw the particles in a gas

4.2.2.1

Name the process for changing a solid into a liquid.

4.2.2.1

Name the process for changing a gas into a liquid.

4.2.2.1

This graph shows a cooling curve?

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

Which section of the graph represents melting?

4.2.2.1

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

Solid

Liquid

Gas

4.2.2.1

Which of the following are states of matter?

Solid

Sunny

Gas

Happy

4.2.2.1

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

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

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

4.2.2.1

Ice is the solid state of water.

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

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

has a definite volume but no defined shape
particles collide and move everywhere
has a volume that can change
particles vibrate in a fixed position
has a defined shape and volume
are somewhat close together but can move freely

Solid
Liquid
Gas

4.2.2.1

What is matter with a definite shape and definite volume?

Solid

Liquid

Gas

4.2.2.1

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

Solid

Liquid

Gas

4.2.2.1

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

4.2.2.1

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

Nokorɛ

Ɛnyɛ ampa

4.2.2.1

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

the particles move faster

the substance becomes less dense

the temperature decreases

the particles get farther apart

4.2.2.1

If a substance cools down, its molecules

move slower

move faster

disappear

stop moving

4.2.2.1

If a substance heats up, its molecules

move faster

disappear

move slower

stop moving

4.2.2.1

4.2.2.2 State Symbols

In the reaction, we made Hydrogen gas. How should we represent that in a chemical equation?

H_2(g)

H_2(l)

H_2(s)

H_2(aq)

4.2.2.2

In the reaction 2H₂_(g) + O₂_(g) → 2 H₂O_(l), which substance is a liquid?

H₂

O₂

H₂O

4.2.2.2

In the displacement reaction of Halogens,
Cl_2(g) + 2NaBr_(aq)→ 2NaCl_(aq) + Br_(l)
which is a liquid?

4.1.2.6

4.2.2.2

This question is about how Group 1 metals react in water
In the equation
2Na_(s) + 2H₂O_(l)→ 2NaOH_(aq)+ H_2(g)
what is NaOH?

4.1.2.5

4.2.2.2

4.2.2.3 Properties of Ionic Compounds

Why don’t covalent compounds conduct electricity?

4.2.2.3

Why are ionic substances soluble in water?

4.2.2.3

Why don’t covalent compounds conduct electricity?

4.2.2.3

Why do ionic compounds have high melting and boiling points?

A large amount of energy is needed to overcome the strong ionic bonds.

Energy is needed to overcome the electrostatic attraction between the ions.

Energy is needed to melt the ions to form a liquid.

Large amounts of energy are needed to transfer the electrons between the atoms.

4.2.2.3

Why are most ionic compounds soluble in water?

A large amount of energy is needed to break the ionic bonds.

Water molecules are attracted to the ions in the lattice.

The ionic forces of attraction are overcome.

The ionic compound melts when in contact with water.

4.2.2.3

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

Yes

4.2.2.3

Did the ionic compounds conduct electricity?

Yes

Sometimes

4.2.2.3

Did the ionic compounds have high or low melting points?

Low

High

4.2.2.3

Match keyword to definition

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

4.2.2.3

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

NaCl_(s)

NaCl_(aq)

NaCl_(l)

4.2.2.3

Why do ionic compounds have high melting and boiling points?

Energy is needed to melt the ions to form a liquid.

A large amount of energy is needed to overcome the strong ionic bonds.

Energy is needed to overcome the electrostatic attraction between the ions.

Large amounts of energy are needed to transfer the electrons between the atoms.

4.2.2.3

Why are most ionic compounds soluble in water?

The ionic forces of attraction are overcome.

A large amount of energy is needed to break the ionic bonds.

Water molecules are attracted to the ions in the lattice.

The ionic compound melts when in contact with water.

4.2.2.3

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

Sodium forms ions with a higher charge than magnesium.

More energy is needed to overcome the bond between sodium and chlorine ions.

The electrostatic attraction between magnesium ions and oxygen ions is stronger.

Oxygen forms ions with a higher charge than chlorine.

4.2.2.3

Why don’t covalent compounds conduct electricity?

4.2.2.3

Why are ionic substances soluble in water?

4.2.2.3

What are the properties of ionic substances?

They do not dissolve in water

They do dissolve in water

They are solids at room temperature

They are liquids and gases at room temperature

They never conduct electricity

They conduct electricity when molten or dissolved

4.2.2.3

What is the name of this compound?

Sodium fluorate

Sodium fluoride

Sodium fluorine

4.1.1.1

4.2.1.2

4.2.2.3

4.2.2.4 Properties of small molecules

This interactive let's you change the intermolecular attractions between particles at the same temperature. While you can't actually do this in real life, this simulation will help you explore how the strength of intermolecular attractions determine if a substance is a solid, liquid, or gas at a given temperature.

Use this interactive to answer questions 1-4

Which statement best describes a substance that has weak intermolecular attractive forces between particles?

The particles move freely and are close together.

The particles don't move much and are spread out.

The particles move freely and are spread out.

The particles don't move much and are close together.

4.2.2.4

Which statement best describes a substance that has strong intermolecular attractive forces between particles?

The particles don't move much and are spread out.

The particles move freely and are spread out.

The particles don't move much and are close together.

The particles move freely and are close together.

4.2.2.4

Identify the state of matter for the substance with weak intermolecular attractions.

gas

liquid

solid

4.2.2.1

4.2.2.4

Identify the state of matter for the substance with strong intermolecular attractions.

gas

solid

liquid

4.2.2.1

4.2.2.4

The boiling point of a substance is the temperature at which the substance changes states from liquid to gas. Boiling point is a physical property that is determined by intermolecular attractions. In the interactive below, there are two tiny drops of liquid, one polar and the other non-polar. Use the interactive to answer questions 5-8

How do intermolecular attractions affect the boiling point of a substance?

The stronger the intermolecular attractions, the higher the boiling point.

The weaker the intermolecular attractions, the higher the boiling point.

Intermolecular attractions don't affect boiling points.

4.2.2.1

4.2.2.4

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

4.2.2.3

4.2.2.4

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
Usually Gas or Liquid

Small Covalent Molecule Properties
Ionic Properties

4.2.2.3

4.2.2.4

Giant structure or simple molecule?

Giant Structure

Simple Molecule

4.2.2.4

Giant structure or simple molecule?

Giant structure

Simple molecule

4.2.2.4

Giant structure or simple molecule?

Giant structure

Simple molecule

4.2.2.4

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

4.2.2.3

4.2.2.4

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
Usually Gas or Liquid

Small Covalent Molecule Properties
Ionic Properties

4.2.2.3

4.2.2.4

4.2.2.5 Polymers

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

4.2.2.5

Which state of matter are most polymers at room temperature

(s)

(l)

(g)

(aq)

4.2.2.2

4.2.2.5

4.2.2.6 Giant Covalent Structures

Giant structure or simple molecule?

Giant structure

Simple Molescule

4.2.2.6

Giant structure or simple molecule?

Giant structure

Simple molecule

4.2.2.6

Giant structure or simple molecule?

Giant structure

Simple molecule

4.2.2.6

Giant structure or simple molecule?

Giant structure

Simple molecule

4.2.2.6

Properties

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

Giant Covalent Structures
Small Covalent Molecules

4.2.2.4

4.2.2.6

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

4.2.2.6

(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

(a)State why sodium chloride conducts electricity when molten. (1 mark)

4.2.2.3

Sort the covalent compounds

Oxygen
Hydrogen
Diamond
Water
Silicon Dioxide
Graphite

Giant Covalent Structure
Small Covalent Molecules

4.2.2.4

4.2.2.6

Which of these are giant covalent structures?

4.2.2.6

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

Nokorɛ

Ɛnyɛ ampa

4.2.2.6

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

Nokorɛ

Ɛnyɛ ampa

4.2.2.6

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

Nokorɛ

Ɛnyɛ ampa

4.2.2.6

4.2.2.7 Properties of Metals and Alloys and 4.2.2.8 Metals as Condudctors

Which is NOT a common property of alloys?

Lower melting point than pure metals

High reactivity with other elements

Great toughness

High resistance to corrosion

4.2.2.7

Match the vocabulary terms to their definitions

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
Conductivity		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
Luster		Refers to if an object is a solid, liquid or gas

4.2.2.7

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

4.2.2.7

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

Only silver and copper conduct electricity

Electrons can move freely in metallic bonds

All metals are magnetic

Metals are in liquid state

4.2.2.7

What is an alloy?

A pure metal

A type of gas

Made of non-metal elements

A mixture of two or more metals

4.2.2.7

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

Different elements in the mix improve certain properties

Alloys contain only precious metals

Alloys are rarer and therefore stronger

Pure metals are always weak and brittle

4.2.2.7

4.2.3 Structure and bonding of carbon

Match the property to the right type of covalent structure.

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

4.2.2.4

4.2.2.6

4.2.3.1

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

Silicon dioxide
Diamond
Graphite
Methane

Hard
Soft

4.2.1.4

4.2.2.6

4.2.3.1

Match the property to the appropriate covalent form.

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

4.2.2.4

4.2.3.1

4.2.3.2

Match the covalent structure with the correct description about structure.

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

4.2.2.6

4.2.3.1

…

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

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

4.2.2.4

4.2.2.6

4.2.3.1

What is a distinctive feature of the structure of diamond?

Each carbon atom is bonded to four other carbon atoms

Each carbon atom is not bonded to any atom

Each carbon atom is bonded to five other carbon atoms

Each carbon atom is bonded to three other carbon atoms

4.2.3.1

Why can graphite conduct electricity?

It has lose atoms that carry current

One electron from each carbon atom is delocalised

It contains metal ions

It is a liquid at room temperature

4.2.3.2

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

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4.2.3.2

What is this?

4.2.3.1

4.2.4 Bulk and surface properties of matter including nanoparticles

1a:

4.2.2.7

1b:

4.2.4.2

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

1 kilometre (km) = 100 metres (m)

1 millimetre (mm) = 0.001 metres (m)

1 micrometre (μm) = 0.01 metres (m)

1 picometre (pm) = 0.1 metres (m)

WS4.5

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

1 × 10⁹ m

2500 μm

0.001 mm

20 000 pm

WS4.5

What is the surface area for the first cube?

MS5c

MS1c

MS5c

MS1c

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

It remains the same, as the total volume of the material does not change.

It decreases, because the surface area decreases more rapidly than the

volume.

It increases, because the surface area increases relative to the volume.

It varies depending on the material, and not on the size of the particles.

4.2.4.1

WS4.5

MS1c

MS5c

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

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4.2.4.1

Justify your above answer

Nanoparticles have a much higher surface area to volume ratio than bulk materials

The chemical composition of nanoparticles is the same as that of bulk

materials.

4.2.4.1

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

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

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

C2 Bonding, structure, and the properties of matter

C2 Bonding, structure, and the properties of matter

Sort the type of bonding with its description

Draw the ion formed from the Li atom

Draw the ion formed from the Na atom

Draw the ion formed from the K atom

Draw the ion formed from the F atom

Draw the ion formed from the Cl atom

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

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

Draw dot and cross diagram - Calcium sulfide

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

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

What kind of bonding is this?

What is the ion formed by Sodium (Na)?

What is the ion formed by Oxygen (O)?

What ion does Calcium (Ca) form?

What ion does Fluorine (F) form?

Which ion has a 2+ charge?

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

Draw the ion formed from the Li atom

Draw the ion formed from the Na atom

Draw the ion formed from the K atom

Draw the ion formed from the F atom

Draw the ion formed from the Cl atom

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

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

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

Fluorine GAINS an electron - what charge does it have?

Draw dot and cross diagram - Lithium fluoride

Draw dot and cross diagram - Magnesium chloride

Draw dot and cross diagram - Lithium Oxide

Draw dot and cross diagram - Calcium sulfide

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

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

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

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

What is the formula for lithium sulfide?

What is the formula for potassium bromide?

What is the formula for beryllium nitride?

What is the formula for aluminum sulfide?

What is the formula for sodium phosphide?

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

When Li loses an electron, it becomes Li+1

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

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

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

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

How are these compounds classified?

Describe the difference between an ionic and covalent bond.

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

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

What kind of chemical bonding is taking place with Bromine?

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)

How are these compounds classified?

Describe the difference between an ionic and covalent bond.

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

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

Which one has the stronger bond?

Which of the following is a covalent compound?

How many valence electrons are shared in each covalent bond?

What kind of bonding is this?

In a metallic bond, where are the electrons located?

Give the definition of metallic bonding ( 1 mark)

Which friend is most correct?

These particles are most likely in what state?

Gas particles have the least amount of kinetic energy, particles are slow, and particles virbrate.

Solid has defintie shape and does not change volume

Liquid does....

The element chlorine is a

Draw the particles in a solid

Draw the particles in a liquid

Draw the particles in a gas

Name the process for changing a solid into a liquid.

Name the process for changing a gas into a liquid.

This graph shows a cooling curve?

Which section of the graph represents melting?

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

Which of the following are states of matter?

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

When Li loses an electron, it becomes Li⁺¹

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

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

In the reaction 2H₂_(g) + O₂_(g) → 2 H₂O_(l), which substance is a liquid?

In the displacement reaction of Halogens,
Cl_2(g) + 2NaBr_(aq)→ 2NaCl_(aq) + Br_(l)
which is a liquid?

This question is about how Group 1 metals react in water
In the equation
2Na_(s) + 2H₂O_(l)→ 2NaOH_(aq)+ H_2(g)
what is NaOH?

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