Chemistry Form 3

WEEK: June 1 to June 5

Use the crossword below to learn more about atoms.

Chemistry Form 4

TOPIC: Mole Relationships                                 WEEK: June 1 to June 5

Determine the molar mass (in g/mol) for the following substances:

1. Na
2. C₈H₁₀N₄O₂ (caffeine)

Moles-Number of Particles Relationship:

1. How many moles of lithium are there in:

1. 1.2 x 10²⁴ lithium atoms?
2. 3.0 x 10²³ atoms of Na?

2. Calculate the number of atoms in each of the following amounts:
1. 1.004 mol Carbon (C)
2. 2.5 mol chlorine (Cl)

Mass – Atoms of Particles Relationship:

1. How many Boron atoms are there in 2.00 g of Boron?

2. Calculate the number of atoms in 54.0 g of Aluminum

Additional Practice:

1. How many moles of carbon dioxide are there in 66.0 g of dry ice, which is solid CO₂?

2. How many water molecules are there in 200.0 g of water?

3. The optimal daily intake dose of Vitamin C is 400 mg per day. How many moles of Vitamin C, also known as ascorbic acid, C₆H₈O₆, does that equal to?

Chemistry Form 4

WEEK: Mat 25 to May 29

Use your knowledge of the Periodic Table to figure out the answers to the statements in the following document. Have fun.

Chemistry Form 3

WEEK: May 25 to May 29

Please complete the following worksheet on Elements, compounds and Mixtures. Answers may be sent via email (leonabel8@gmail.com) or Edmodo (Code = i3f3cg)

Chemistry Form 3

Form 3 CHEMISTRY Trinity Term                                     WEEK: May 18 – May 22

Teacher: Leon Abel                                                                 My e-mail: leonabel8@gmail.com

Topic: Atomic Structure – Read carefully, then use your notes and/or other resource materials to answer the questions

1.     Which particle(s) in the atom is/are responsible for the

a.      mass of the atom

b.     volume of the atom

2.     Define the following terms:

a.      Atomic mass

b.     Mass number

c.      Isotope

3.     For each of the following nuclear notations, give the number of protons, electrons and neutrons:

a.      ¹¹₅B

b.     ²³₁₁Na

c.      ⁴⁰₂₀Ca

4.     Give the similarities and differences between the two isotopes of sodium, sodium-23 and sodium-24

5.     Explain what a radioactive isotope is.

You may use the following video to assist you:

Chemistry Form 4

Form 4 CHEMISTRY Trinity Term                      WEEK: May 18 to May 22

Teacher: Leon Abel                                                  Email: leonabel8@gmail.com

Chemical Equations and Reactions – Read carefully then Answer ALL of the following questions:

1.     Which law do we make use of when balancing chemical equations?

2.     Balance the following chemical equations:

a.      Aluminum + oxygen à aluminum oxide

b.     CH₄(g) + O₂(g) à CO₂(g) + H₂O(l)

c.      NaOH(aq) + HCl(aq) à NaCl(aq) + H₂O(l)

d.     Sodium + water à sodium hydroxide + hydrogen

3.     Balance the following equations then classify the reactions using the words in the square bracket.             [ synthesis, decomposition, single displacement, ionic precipitation, neutralization ]

a.      H₂CO₃(g) à H₂O(l) + CO₂(g)

b.     Fe(s) + Cl₂(g) à FeCl₃(s)

c.      Zn(s) + HCl(aq) à ZnCl₂(aq) + H₂(g)

d.     NaOH(aq) + H₂SO₄(aq) à Na₂SO₄(aq) + H₂O(l)

e.      AgNO₃(aq) + MgBr₂(aq) à AgBr(s) + Mg(NO₃)₂(aq)

Chemistry Form 3

Form 3 CHEMISTRY Trinity Term                                                    May 11-15

Teacher: Leon Abel                        My e-mail: leonabel8@gmail.com

Week 4 Topic: Mixtures and Separations – Read carefully, then use your notes and/or other resource materials to answer the questions

1.     Copper is described as an element. What does this tell us about copper?

2.     What is a compound?

3.     Give TWO differences between pure substances and mixtures.

4.     What makes a mixture different to a compound?

5.     What is the difference between a homogeneous mixture and a heterogeneous mixture?

6.     How does the particle size of:

a.      a solution compare with that of a suspension

b.     a suspension compare with that of a colloid?

7.     Which of the following mixture types, solutions, suspensions and colloids:

a.      does not transmit light?

b.     can be separated by filtration?

c.      will not settle out after standing?

Chemistry Form 3

Form 3 CHEMISTRY Trinity Term

My e-mail: leonabel8@gmail.com

Week 3 Topic: States of Matter – Read carefully, then use your notes answer the questions

1.     Diffusion and Osmosis are TWO processes used as proof for the particulate theory of matter.

a.      Define diffusion 

b.     Define osmosis 

c.      Identify TWO (2) real world examples of diffusion taking place. 

d.     Describe ONE (1) situation in which osmosis is taking place 

e.      What is the relation between diffusion and osmosis? (How are they similar; how are they different?) 

2.     Solids, liquids and gases are three states of matter which exist depending on the amount of movement energy the particles of matter have.

a.      What is movement energy called? Hint: it begins with k. 

b.     Aside from the energy of the particles, what is responsible for the existence of the three states of matter Hint: forces of… 

c.      How does the shape of a solid differ to that of a liquid? 

d.     Explain why gases are easy to compress but solids are harder to compress. Hint word: space 

e.      Explain why both liquids and gases have variable shape however the liquid has a definite volume while the gas has a variable volume. Hint: energy, space and forces of… 

Chemistry Form 3

Form 3 CHEMISTRY Trinity Term

Week 2

1.     State the FOUR (4) main ideas of the particulate theory of matter.

2.     What is the relationship between the temperature of a particle and the movement of the particle?

3.     What are the THREE (3) states of matter?

4.     Research, then write the answer to the following IN YOUR OWN WORDS: why do scientists find the particle theory of matter useful?

Chemistry Form 4

Form 4 CHEMISTRY Trinity Term

Teacher: Leon Abel                                                  Email: leonabel8@gmail.com

Week 4: The Periodic Table – Read carefully then Answer ALL of the following questions:

1.     Explain the relationship between the electronic structure and the chemical properties of an element.

2.     What is a strong indication of an element’s metallic or non-metallic nature?

3.     How does the metallic and non-metallic nature of elements in Period 3 change from left to right?

4.     Which element in Period 3 has the greatest metallic nature?

5.     What is the collective name for all the elements in Group II?

6.     Does the reactivity of the elements in Group II increase or decrease down the group?

7.     Compare the reactivity of beryllium and calcium.

8.     What is similar in the electronic configuration of the elements in Group VII?

9.     How does the reactivity of the elements in Group VII change as one move up the group?

10.  Write the electronic configuration of the following:

a.      Sodium

b.     Chlorine

c.      Carbon

d.     Sulphur

Chemistry Form 4

Form 4 CHEMISTRY Trinity Term

Week 3: Chemical Bonding – Read carefully then Answer ALL of the following questions:

1.     Excerpt from Chemistry for CSEC by Nelson Thornes: “When atoms bond with each other, usually only the outermost electron shells are involved in the process. Atoms combine with each other to attain a more stable electronic configuration. The noble gases are stable atoms because of their electronic configuration…in their electronic configuration, their outermost shell is full.” Explain why atoms bond with one another.  2 marks

2.     Compare ionic bonding to covalent bonding. 2 marks

3.     Calcium forms an ionic bond with fluorine to form a compound: 2 marks

a.      Give the name of the compound

b.     Give the formula of the compound

4.     Research the term “delocalized electron” then explain how it applies to metallic bonding. 2 marks

5.     Explain why metals are electrical conductors. 2 marks

Chemistry Form 4

Form 4 CHEMISTRY Trinity Term

Week 2: Chemical Bonding

Answer ALL of the following questions:

1.     Write the formula of EACH of the following compounds:

a.      Potassium chloride

b.     Ammonium phosphate

c.      Calcium hydroxide

d.     Lithium manganate (VII)

e.      Iron (III) oxide

f.      Lead (II) sulphate

g.     Iron (II) bromide

h.     Zinc nitrate

i.       Silver carbonate

2.     Write the name for EACH of the following compounds:

a.      Mg₃(PO₄)₂                

b.     AgCl

c.      ZnI₂

d.     Al(HCO₃)₃

e.      FeBr₃

f.      FeSO₄                      

g.     Cu₂O                        

h.     CuO                           

i.       CuO₂                            

j.       Pb(NO₃)₂

3.     State whether the following are ionic or molecular crystals:

a.      KBr

b.     I₂

c.      H₂O

d.     Graphite

e.      CaCO₃

4.     Name the type of bonding in:

a.      Sodium chloride

b.     Diamond

c.      Graphite