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

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

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Draw the ion formed from the Li atom

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Draw the ion formed from the Na atom

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Draw the ion formed from the K atom

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Draw the ion formed from the F atom

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Draw the ion formed from the Cl atom

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

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

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Draw dot and cross diagram - Calcium sulfide

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

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

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What kind of bonding is this?

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What is the ion formed by Sodium (Na)?

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What is the ion formed by Oxygen (O)?

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What ion does Calcium (Ca) form?

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What ion does Fluorine (F) form?

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Which ion has a 2+ charge?

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

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Draw the ion formed from the Li atom

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Draw the ion formed from the Na atom

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Draw the ion formed from the K atom

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Draw the ion formed from the F atom

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Draw the ion formed from the Cl atom

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

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

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

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Fluorine GAINS an electron - what charge does it have?

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Draw dot and cross diagram - Lithium fluoride

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Draw dot and cross diagram - Magnesium chloride

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Draw dot and cross diagram - Lithium Oxide

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Draw dot and cross diagram - Calcium sulfide

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

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

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

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

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

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

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What is the formula for lithium sulfide?

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What is the formula for potassium bromide?

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What is the formula for beryllium nitride?

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What is the formula for aluminum sulfide?

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What is the formula for sodium phosphide?

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

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When Li loses an electron, it becomes Li+1

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

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

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

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

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

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Ionic Compounds
Simple Molecules

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How are these compounds classified?

Methane
Magnesium Oxide
Sodium Chloride
Carbon Dioxide

Small Covalent Compounds
Ionic Compounds

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Describe the difference between an ionic and covalent bond.

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

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

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What kind of chemical bonding is taking place with Bromine?

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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)

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How are these compounds classified?

Methane
Magnesium Oxide
Sodium Chloride
Carbon Dioxide

Small Covalent Compounds
Ionic Compounds

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Describe the difference between an ionic and covalent bond.

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

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

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Which one has the stronger bond?

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Which of the following is a covalent compound?

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How many valence electrons are shared in each covalent bond?

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What kind of bonding is this?

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In a metallic bond, where are the electrons located?

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Give the definition of metallic bonding ( 1 mark)

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

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Which of the following are states of matter?

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

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

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Ice is the solid state of water.

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

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

Solid
Liquid
Gas

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What is matter with a definite shape and definite volume?

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

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

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

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

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If a substance cools down, its molecules

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If a substance heats up, its molecules

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Why don’t covalent compounds conduct electricity?

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Why are ionic substances soluble in water?

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Why don’t covalent compounds conduct electricity?

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Why do ionic compounds have high melting and boiling points?

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Why are most ionic compounds soluble in water?

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

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Did the ionic compounds conduct electricity?

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Did the ionic compounds have high or low melting points?

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Match keyword to definition

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

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

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Why do ionic compounds have high melting and boiling points?

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Why are most ionic compounds soluble in water?

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

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Why don’t covalent compounds conduct electricity?

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Why are ionic substances soluble in water?

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What are the properties of ionic substances?

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

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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

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Giant structure or simple molecule?

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Giant structure or simple molecule?

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Giant structure or simple molecule?

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

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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

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

Complete the structure of poly(ethene)

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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 _______ .

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Which state of matter are most polymers at room temperature

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Giant structure or simple molecule?

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Giant structure or simple molecule?

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Giant structure or simple molecule?

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Giant structure or simple molecule?

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Properties

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

Giant Covalent Structures
Small Covalent Molecules

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

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

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

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Sort the covalent compounds

Water
Graphite
Oxygen
Silicon Dioxide
Diamond
Hydrogen

Giant Covalent Structure
Small Covalent Molecules

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Which of these are giant covalent structures?

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

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

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

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Which is NOT a common property of alloys?

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Match the vocabulary terms to their definitions

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

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

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

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What is an alloy?

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

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Match the property to the right type of covalent structure.

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

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

Methane
Graphite
Silicon dioxide
Diamond

Hard
Soft

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Match the property to the appropriate covalent form.

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

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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

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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

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What is a distinctive feature of the structure of diamond?

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Why can graphite conduct electricity?

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

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What is this?

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1a:

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1b:

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

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

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What is the surface area for the first cube?

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What is the volume for the first cube?

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What is the SA:V for the first cube?

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What is the surface area for the second cube?

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What is the volume for the second cube?

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What is the SA:V for the second cube?

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

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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 =_______ 

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

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Justify your above answer

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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.

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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.

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