“C1.1 Fundamentals of Chemistry”

“C1.1 Fundamentals of Chemistry”

KS4 SCIENCEMr Powell 2013

Mr Powell 2012Index

Compound A pure substance

Mixture The smallest part of all substances

Atom Two or more of the same or different atoms chemically joined together.

MoleculeTwo or more atoms of the same element chemically joined

Element Two or more substances not chemically joined

Definitions Match Up PTASK: Logically compare these word to match the terms

O

O O

C

HHO

HHO

NN

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Think about the task you have just completed. Here are six groups of atoms to look at. Can you put a word(s) to describe the groups chemically from what you previously learned;

A)B)C)D)E)F)

Knowing your terms... PA

B

D

C

F

E

A. Elements or atoms

B. Mixture of elements or atoms

C. CompoundD. Mixture of

compoundsE. CompoundF. Mixture of

elements

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Periodic Table...

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What do you know?

In your book write down all you know about these items.....

• Gold

• Group 1 Metals

• Group 7 Non-metals

• Structure of an Atom

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Lesson Aims/ Levels1a) All substances are made of atoms which have symbols. (L)

1b) How do we classify atoms (M)

1c) What are groups and what do they mean (M/H)

Literacy: Verbal communicationsLow Demand (E-G)Standard Demand (B-D)High Demand (A*-B)

Keywords: atom, neutron, proton, electron, nucleus

Atoms, Elements and Compounds (page 24)C11.1

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The Periodic Table (Video First 15 mins)

1. What is she panning for? (Gold)2. Why is gold special? (It does not corrode)3. What is the periodic table (a roadmap of all the elements)4. Peter Atkins talks about the shiny ones on the left, what do we call these (metals)5. What do we call the other side of the table (non-metals)6. What is mercury used for? (thermometers / dental fillings)7. What state is mercury in at room temperature (liquid)8. Name a property of most metals (silvery grey/conduct electricity)9. What do the transition metals show in the table (a history of the use of metals bronze, age,

titanium)10. How does the periodic table show similar elements? (in vertical groups)11. Name a metal similar to lithium? (sodium, potassium etc..)12. What properties of gold are useful in making the jewellery? (melts at a low temperature, is

non-reactive.)13. Why is carbon very useful? (it can form long chains such as DNA)14. What are some metals are found as ores, how are they extracted (smelting – heating)15. What happens with group 1 metals when they meet water (they react violently)16. Why are the more reactive at the bottom of the group? (the outer electrons are shielded)17. What can group 7 elements be used for? (chemical weapons – Cl reacts with water to form

bleach)

Student – “Self Assessed”

Score /17 ?????

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Form into a small group of 3-4 people. One person is the “quizmaster” for a “round” Contestants have 30 seconds to talk about a topic without...

• Hesitation• Repetition• Stalling• Talking rubbish off topic• Telling lies!

Other contestants can challenge and take the floor, the winner is the person who finishes the 30s and gets 2 points but you also get a 1 point for each correct challenge.

Talk about these topics....

• Gold• Group 1 Metals• Group 7 Non-metals• Structure of an AtomExtension: others ideas from the worksheet!

I'm Sorry I Haven't got a Clue

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Atomic Model – RECAP!We used to think that atoms weren't made up of smaller pieces. The word "atom" actually comes from a Greek word which means "can't be split up". Now we know that all atoms are actually made of the same 3 tiny particles; protons, electrons and neutrons.

The protons are positive and the electrons are negative. Neutrons are neutral.

Protons and neutrons are much heavier than electrons and they are found in the middle of the atom called the nucleus. The electrons are in orbit around the outside.

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Quick Test....

1.Which particles are found in the nucleus of an atom?

2. Which particles orbit the nucleus?

3. Which atomic particle has a charge of +1?

4. Which atomic particle has no charge?

5. Which atomic particle has a charge of −1?

6. Two of the particles each have a mass of one atomic mass unit. The other has almost no mass. Which one has almost no mass?

1. protons and neutrons

2. electrons3. proton4. neutron5. electron6. electron


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C1.1 Book Answers...

In text questions...

a) about 100b) Because you can combine them together in

millions of different ways.c) Because an element may have different names in

different languages.d) metals – barium (Ba), vanadium (V), mercury

(Hg) non-metals – phosphorus (P), krypton (Kr) (Harder)

Summary Questions

1 atoms, molecule, compounds, bonds 2 In a mixture, the different substances are not joined to each other by chemical bonds, but in a compound the atoms are held together tightly by chemical bonds – this makes them difficult to separate. (Harder)


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Atomic Model Recap S

a) Chargeb) Neutralc) Electronsd) Protonse) Protonsf) Nucleusg) Atomich) Protoni) Nucleonsj) Nucleusk) Massl) Atomic Mass

Word BANK

Nucleus, Mass, Protons, Charge, Proton ,Nucleons, Atomic, Atomic Mass, Protons, Nucleus, Neutral, Electrons

Write a-l in your book and write in the correct order for the words.

A*-B – don’t use the word bank (9/12)C-D - Use the word bank to help you (6/12)

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Atomic Structure (page 26)C11.2

Lesson Aims/ Levels2) Atoms have a small central nucleus, of protons and neutrons, surrounded by

electrons. (L)

3) The relative electrical charges are +1/-1/0 for proton, electron and neutron (S)

4) Atoms have no overall electrical charge. (S)

5) All atoms of a particular element have the same number of protons (Atomic Number). (L)

6) The total mass (atomic mass) of an atom is the sum of the number of protons and neutrons. (S/H)

Low Demand (E-G)Standard Demand (B-D)High Demand (A*-B)

Keywords: charge, relative, atomic number, atomic mass, neutron, proton, electron, nucleus

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Modelling....

TASK: Can you create your own particle model for atoms, mixtures & compounds. Work as a team of 2 or 3.

1. Draw some diagrams, then make some examples (S/H)

2. Explain/ Discuss its strengths and weaknesses? (H)

Extra Help... page 26

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Ions....

TASK: Using the model you have made for an Atom can you now use it to show the following.

1. Atoms have a small central nucleus, of protons and neutrons, surrounded by electrons. (L)

2. The relative electrical charges are +1/-1/0 for proton, electron and neutron (S)

3. Atoms have no overall electrical charge. (S)

4. All atoms of a particular element have the same number of protons (Atomic Number). (L)

5. The total mass (atomic mass) of an atom is the sum of the number of protons and neutrons. (S/H)

Discuss your ideas in a small group then write down your findings on your sheet and share with others in your group and “Peer Assess”...

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a) protons, neutrons, electrons

b) 8 electrons

c) silicon

d) They increase by 8 between each element.

Summary Questions

1 neutrons, electrons, negative, atomic 2 Because protons and electrons have the same amount of charge but with opposite signs, the charge on a proton is exactly cancelled out by the charge on an electron. 3 a 7 protons, 7 electrons and 7 neutrons. (Harder) b 17 protons, 17 electrons and 18 neutrons. (Harder)


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Homework – Revision!

http://www.sporcle.com/games/g/elements

http://www.sporcle.com/games/g/elements

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The Arrangement of Electrons in Atoms (page 28)C11.3

Lesson Aims/ Levels7) Electrons occupy particular energy levels. Each electron in an atom is at a

particular energy level (in a particular shell). The electrons in an atom occupy the lowest available energy levels (innermost available shells). (H)

8) Elements in the same group in the periodic table have the same number of electrons in their highest energy level (outer electrons) and this gives them similar chemical properties. (S)

9) The elements in Group 0 of the periodic table are called the noble gases. They are un-reactive because their atoms have stable arrangements of electrons. (H)

10) Chemical reactions can be represented by word equations (S)


Keywords: electron shell, outer electron, chemical properties, noble gas, stable

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Blind Date Do they Match – fill your sheet in?Sodium, Na 11, Group 1,

Alkali Metals, 1 electron in outer shell, reacts in water,

releases hydrogen.

Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form

MgO.

Aluminium, Al 13, makes pans, Group 3, metal, reacts

with bromine strongly.

Chlorine, Cl 17, Group 7, with 7 outer electrons, makes PVC, corrosive, used in swimming

pools, bleaches roses!

Oxygen, O 8, Gives life! Group 6, 6 electrons in the outer shell,

oxidises (burns) other elements.

Fluorine F 9, Group 7 missing 1 electron, reacts well with everyone, lights a cig on

contact!

Neon, Ne 10, Group 8, 8 electrons in outer shell, non-

reactive, hangs about in ones!

Lithium Li 3, Soft metal, shiny, very reactive, Group 1, kept

in oil.

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Electronic Config…

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Electronic Config…

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a Arranged around the nucleus in shells. b The energy level closest to the nucleus. c 2 d 2,8,6 (Harder)

Summary Questions

1 nucleus, shells, energy, group, electrons

3 They both have full outer shells or energy levels of electrons/very stable arrangements of electrons.


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Quick Check....

A) For the following elements can you write down the electronic configuration....

For example.. Calcium is...... 2,8,8,2

1) Mg2) Al3) S4) Si5) K

B) Can you draw the electronic configuration for Si and K (Harder)

Answers

1) Mg 2,8,22) Al 2,8,33) S 2,8,64) Si – 2,8,45) K – 2,8,8,1


Sodium, Na 11, Group 1, Alkali

Metals, 1 electron in outer shell,

reacts in water, releases hydrogen.

Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form MgO.

Aluminium, Al 13, makes pans, Group

3, metal, reacts with bromine

strongly.

Chlorine, Cl 17, Group 7, with 7 outer electrons,

makes PVC, corrosive, used in swimming pools, bleaches roses!

Oxygen, O 8, Gives life! Group 8, 6 electrons in the

outer shell, oxidises (burns) other

elements.

Fluorine F 9, Group 7 missing 1 electron,

reacts well with everyone, lights a cig

on contact!

Neon, Ne 10, Group 8, 8 electrons in outer shell, non-reactive, hangs about in ones!

Lithium Li 3, Soft metal, shiny, very reactive, Group 1,

kept in oil.

Sodium, Na 11, Group 1, Alkali

Metals, 1 electron in outer shell,

reacts in water, releases hydrogen.

Magnesium, Mg 12, Likes Group 7, bonds with two at a time, Reacts with O2 to form MgO.

Aluminium, Al 13, makes pans, Group

3, metal, reacts with bromine

strongly.

Chlorine, Cl 17, Group 7, with 7 outer electrons,

makes PVC, corrosive, used in swimming pools, bleaches roses!

Oxygen, O 8, Gives life! Group 8, 6 electrons in the

outer shell, oxidises (burns) other

elements.

Fluorine F 9, Group 7 missing 1 electron,

reacts well with everyone, lights a cig

on contact!

Neon, Ne 10, Group 8, 8 electrons in outer shell, non-reactive, hangs about in ones!

Lithium Li 3, Soft metal, shiny, very reactive, Group 1,

kept in oil.

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1. Atoms of which three elements are drawn above?

2. Write out the electronic configuration for all three?

3. What do they all have in common?

Reactions Review...

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Forming Bonds (page 30) – “Stealing” or “Sharing”C11.4

Lesson Aims/ Levels• Chemical reactions can be represented by word

equations or by symbol equations. (H) (Balancing is HT only skill)

• When elements react, their atoms join with other atoms to form compounds. This involves giving, taking or sharing electrons to form ions or molecules. (H)

• Compounds formed from metals and non-metals consist of ions. (H)

• Compounds formed from non-metals consist of molecules. In molecules the atoms are held together by covalent bonds. (S)


Keywords: symbol, ionic bonding, molecule, compound, covalent bond.

OR?

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Covalent Bonding – “Sharing”

http://www.animatedscience.co.uk/ks4-covalent-bonding

1. Look through the examples of covalent or “shared” bonded molecules from non-metals

2. In your book draw out several examples to show how the electrons are configured before bonding and after bonding when electrons are shared....

MoreExamples...

Chlorine Cl2

Ammonia NH3

Hydrogen H2

Hydrogen Chloride HClWater H2OOxygen O2

http://www.animatedscience.co.uk/ks4-covalent-bonding

Mr Powell 2012Index

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Ionic Bonding “Stealing”

Mr Powell 2012Index

1. Each shell has a maximum number of electrons that it can hold.

2. In noble gases the shells are completely full rather than partially full…this is why they are so unreactive.

3. During bonding other atoms try to attain the “full electron shell” structure of the noble gases.

1st Shell: 2 electrons

2nd Shell: 8 electrons

3rd Shell: 8 electrons

Ionic Bonding “Stealing” - Metals and non metals

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Sodium atom Chlorine atom

Sketch the atoms above and then consider…

Both atoms would be more stable if they had full outer shells, what would be the simplest way for each atom to gain a full outer shell?


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Sodium atom Chlorine atom

Sodium ion Chloride ionCopy these

ions


+1 -1

Sodium ion Chlorine ion

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Ionic Bonding...

Atoms have an equal number of protons and neutrons, so the charges cancel out. However after sodium has given an electron to chlorine, the electrons and protons in both atoms no longer balance:

Sodium Chlorine 10 electrons 10- 18 electrons 18- 11 protons 11+ 17 protons 17+

1+ 1-

The atoms are now ions and are charged Na+ and Cl-

Na+

[2,8]+

+ -

Cl-

[2,8,8]-

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1. Draw diagrams to show the ions that would be formed when the following atoms are involved in ionic bonding.

2. For each one state whether electrons have been lost or gained and show the charge on the ion.

• Aluminium (Al), Fluorine (F), Potassium (K), Oxygen (O)

Learning Check....

Apply this skill to draw out these molecules using the square brackets

1. KF

2. AlF3 (Harder)

3. Al2O3 (Harder)

Na+

[2,8]+

+

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a K+

b covalent bonds

Summary Questions

1 positive, lose, gain, negative, attract, ionic, covalent, share 2 a Sodium fluoride b Na+ and F-

c NaF


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Progress Check...

OR?

Write down the two key things we have learned about today, giving an example of each by...

1. Diagram (Low Demand)

2. Written Explanation (Standard Demand)

3. Both linked in detail (High Demand)

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Chemical Equations (page 32)C11.5

Lesson Aims/ Levels

No atoms are lost or made during a chemical reaction so the mass of the products equals the mass of the reactants. (H)


Keywords: reactants, products

2Na + Cl2 → 2NaCl

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Balancing Equations....

Can you check the products and reactants and balance these equations...

H2 + Br2 → HBr

Na + Cl2 → NaCl

CH4 + O2 → CO2 + H2O

P + Cl2 → PCI3

CaCO3 → CO2 + CaO

Fe + H2O → H2 + Fe3O4 (High Demand)

1. H2 + Br2 → 2HBr

2. 2Na + Cl2 → 2NaCl

3. CH4 + 2O2 → CO2 + 2H2O

4. 2P + 3Cl2 → 2PCl3

5. CaCO3 → CO2 + CaO (already balanced)

6. 3Fe + 4H2O → 4H2 + Fe3O4

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In text questions... a A lighted splint burns with a squeaky ‘pop’. b Reactant: calcium carbonate. Products: calcium oxide and carbon dioxide. c H2 + Cl2 → 2HCl

Summary Questions

1 As no new atoms can be created or destroyed in a chemical reaction, the number and type of atoms in the reactants must equal the number and type of atoms in the products. 2 a 4.4 g b magnesium carbonate → magnesium oxide + carbon dioxide 3 a 2Ca + O2 → 2CaO b 4Al + 3O2 → 2Al2 O3

c 2Na + 2H2 O → 2NaOH + H2


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Progress Check...

1. H2 + Br2 → 2HBr

2. 2Na + Cl2 → 2NaCl

3. CH4 + 2O2 → CO2 + 2H2O

4. 2P + 3Cl2 → 2PCl3

5. CaCO3 → CO2 + CaO (already balanced)

6. 3Fe + 4H2O → 4H2 + Fe3O4

A. Using an example of a reaction you have looked at today and page 33 in the book.

B. “making an equation balance”

C. Write a method of steps that you would employ to balance any other reaction you might be given

D. Then swap with another person and test it out to see if it worked on all of these six.

E. Check each reaction in turn, each one correct to the method gets 1 mark.

?6

Balancing Equations Extra Help....


H2 + Br2 → HBr

Na + Cl2 → NaCl

CH4 + O2 →

Balancing Equations Extra Help....


H2 + Br2 → HBr

Na + Cl2 → NaCl

CH4 + O2 →

Documents

“C1.1 Fundamentals of Chemistry”