REVIEW UNIT

We will be reviewing the following chemical concepts:

A) Qualitative Observations vs. Quantitative Observations B) Physical Properties and Physical Change C) Chemical Properties and Chemical Change D) Classification of Matter E) Symbols on the Periodic Table – Atomic Notation F) Isotopes and Ions G) Bohr‐Rutherford Diagrams H) Forming Ions I) Forming Ionic Compounds J) Naming Binary Ionic Compounds K) Polyatomic Ions L) Naming and Writing Formulas of Polyatomic Compounds

A) QUALITATIVE vs. QUANTITATIVE OBSERVATIONS

qualitative observations →

quantitative observations → B) PHYSICAL PROPERTIES and PHYSICAL CHANGE physical property →

There are 3 common states of matter:

SOLID LIQUID GAS

Volume

Mass

Shape

PPHYSICAL PROPERTIES OF MATTERR

Colour → example: red, green, orange, etc.

Odour → how the substance smells (burnt, flowery, odourless)

Taste → how the substance tastes (sweet, sour, salty)

Clarity → the ability of the substance to transmit light

Cannot see through Can almost see through Can see through clearly (transmits no light) (transmits some light) (transmits all light)

Lustre → the ability of a substance to reflect light high lustre _____________________ low lustre _______________________ Form → the shape of a substance (crystalline = ordered and amorphous = disordered)

crystalline _____________________ amorphous _______________________ Texture → the “feel” of a substance (smooth, rough) Hardness → ability of a substance to be scratched (soft or hard)

Soft _____________________ hard _______________________ Brittleness → ability of a substance to break apart or shatter brittle _____________________ flexible _______________________ Ductility → ability of a substance to be stretched into a wire

Melting point → the temperature a substance melts at

Boiling point → the temperature a substance boils at

Malleability → how easily a metal can be hammered, pressed or rolled into thin sheets Viscosity → how easily a liquid flows __________________ __________________ HIGH viscosity LOW viscosity

Instructions: Use the words and definitions on the previous page to fill in the following: 1. _____________________ describes an object’s ability to reflect light. 2. Substances with an ordered structure such as sugar are said to be ______________________. 3. Burnt, flowery, and putrid are terms used to describe a substance’s ______________________. 4. Fine, course, gritty, and silky are terms used to describe an object’s ______________________. 5. _____________________ describes an object’s ability to transmit light. Objects that transmit no

light through them are said to be ________________; objects that transmit some light through

them are said to be _________________; objects that transmit all of the light through them are

said to be _________________.

6. The ability of a substance to be stretched into a thin wire is called ______________________. 7. Substances that can bend without breaking are called ___________________, whereas substances

that break or shatter easily are called ___________________.

8. The ability of a substance to be hammered into thin sheets is called _____________________. 9. Name a substance that fits the description below: a) brittle ____________________ e) hard ____________________ b) malleable ____________________ f) ductile ____________________ c) opaque ____________________ g) amorphous ____________________ d) high luster ____________________ h) course ____________________ 10. Indicate a physical property that would allow you to distinguish between the following pairs of

objects.

a) salt and sugar ____________________ b) salt and flour ____________________

PHYSICAL PROPERTIES OF MATTER WORKSHEET

Instructions: At each station you will find two materials. Follow the instructions in the table

below at each station. At each station use the definition provided to help you identify the property that the materials have in common and the physical property that might be used to differentiate the two materials.

Station #

What to do at the station Physical property that

these two objects at this station have in common

Physical Property that could differentiate the two pieces of matter at this

station

1 Observe the two objects.

2 Using the nail try to scratch the surface of each piece of matter.

3 Observe the two flasks. Waft the contents towards your nose.

4 Pour Liquid A into Beaker A. Pour Liquid B into Beaker B. Pour both liquids back into each flask.

5 Rub each object with your finger.

6 Observe the objects.

7 Observe the objects.

8 Shake a small amount of Solid A onto your hand and lick your hand. Do the same for Solid B.

9 Observe the two substances under each microscope.

10 Observe the two objects.

PHYSICAL PROPERTIES OF MATTER ACTIVITY

PPHYSICAL CHANGEE physical change →

There are 3 types of physical change:

Change of State

Note: new properties may appear BUT the particle of the starting substance is the same.

Example: ice melting

ICE (SOLID WATER) LIQUID WATER

Physical Property

* both ice and liquid water are made of ________________________________.

Dissolving Experiment: FIRST, taste sugar →

SECOND, put sugar into the water and mix (DISSOLVING)

THIRD, taste water → Observations: When sugar was put into water, the sugar particles spread out (cannot

see anymore)

BUT, sugar particles are still there because _________________________.

Conclusion:

Change of Form

C) CHEMICAL PROPERTIES and CHEMICAL CHANGE chemical property →

Types of chemical properties: chemical change →

EVIDENCE a CHEMICAL CHANGE has occurred:

Answer the following questions in your notebook. Use full sentences, unless asked to do otherwise. 1. What is the major difference between a physical change and a chemical change?

2. Below is the definition of a chemistry term that has been discussed over the last two days. Write

out the word or words for each. The first one has been completed for you.

a) A change in which a new substance is produced. _______________________

b) A change in which no new substance is produced. _______________________

c) Salt is stirred into a pot of boiling water until it disappears. _______________________

d) Iron rusts if it gets wet. _______________________

e) The property that allows copper to be used as wiring. _______________________

f) Chalk breaks apart if you try to bend it. _______________________

g) Making toast is this kind of change. _______________________

h) Salt has an ordered molecular structure, its form is said to be… _______________________ 3. The following contain errors or are incomplete. Write complete, correct versions. Use full sentences.

a) Making ice cubes is a chemical change.

b) A chemical change may produce a new substance called a predominate.

chemical change

PHYSICAL AND CHEMICAL PROPERTIES/CHANGES WORKSHEET

c) A new colour when two chemicals are mixed indicates a physical change.

d) The ability to react with acid is an example of a physical change.

e) Ductility is a chemical property.

f) A change of state is a chemical change.

g) Corrosion is the reaction of a metal such as iron with nitrogen in the air.

4. Indicate whether each of the following is a physical change (PC) or a chemical change (CC).

a) Water freezing on a pond. ______ d) Bending a paper clip. ______ b) A cake baking. ______ e) carbon dioxide is produced by

mixing vinegar with baking soda ______

c) Dynamite exploding. ______

5. Circle the chemical properties and underline the physical properties in the sentences below.

a) Salt is a white, crystalline solid. It does not react with air but it dissolves easily in water. b) Gasoline is a colourless liquid that is very combustible. It has a low viscosity and does not

dissolve in water.

c) Water freezes at 0°C and boils at 100°C. It is colourless, odourless, and not combustible. However, if sodium metal is put into water an explosion can result.

D) CLASSIFICATION OF MATTER PURE SUBSTANCES

Pure substances contain only one kind of particle. They have the following criteria:

1) Uniform composition throughout 2) Components cannot be separated by physical means

3) Changes of state occur at fixed temperatures

MATTER

Types of Pure Substances:

i) Elements ⇒ Elements are pure substances that CANNOT be broken into simpler substances (by ordinary chemical means)

example:

ii) Compounds ⇒ Compounds are pure substances that contain two or more different elements in a fixed proportion

example: Water is a compound made of hydrogen and oxygen. In water there is always ___________ as many hydrogen atoms than oxygen atoms.

Some pictures of pure substances:

pure substance pure substance pure substance NOT a pure substance of matter of matter of matter because there are

__________________ __________________ __________________ _____________________ pure substance pure substance pure substance NOT a pure substance of matter of matter of matter because there are

__________________ __________________ __________________ _____________

H2 H2

H2 H2 H2

H2 H2 H2

H2

H2 H2

H2

H2

H2

O2

O2

O2 O2

O2

O2 O2

O2 O2 O2

O2

O2

O2

O2 H2O

H2OH2O

H2O

H2O

H2OH2OH2O

H2O

H2O

H2O

O2

O2 O2 H2

H2

H2

H2

O2

O2 O2 H2

H2

O2

O2

MIXTURES

When _______________________________ are mixed together, sometimes they mix evenly, and sometimes they mix unevenly. If the particles mix very well with one another, so well that you only see one phase (i.e one

one visible layer) then the mixture is called a ________________________________________.

Solutions can be made up of _____________, ______________, or ____________

Example: sugar or salt dissolved in water

If the particles do not mix well with one another, you will see more than one phase (i.e. more

than one visible layer). This is called a _________________________________________________.

example 1: oil mixed with water

Use the “map” above to help you classify the following as an element (E); compound (C); homogeneous mixture/solution (HOM); or heterogeneous mixture/mechanical mixture (HET).

1) Koolaid in water ______ 5) chocolate chip cookie ______ 9) pure sodium (Na) ______ 13) air (N2, O2, CO2) ______

2) Ceasar salad ______ 6) oxygen (O2) ______ 10) vegetable soup ______ 14) pure water (H2O) ______

3) Copper (Cu) ______ 7) salt (NaCl) ______ 11) gravel driveway ______ 15) pizza (with toppings) ______

4) Propane (C3H8) ______ 8) hydrogen peroxide (H2O2) ______ 12) a cup of coffee ______ 16) a twoonie ______

YES

Matter

How many substances are present? More than oneOnly one

What can see?Is it on the Periodic table?

NO

More than one thing

Only one thing

WORKSHEET

D) INSIDE THE ATOM Elements are pure substances that cannot be broken down into simpler substances. Elements are

made up of _____________. But what is an atom made of?

Atoms are made of particles called ____________________________.

Subatomic Particle Location Charge Relative Mass

The number of ________________ in an atom

determines what type of element it is.

Example:

Counting Subatomic Particles

Atom Number of Protons

Total Positive Charge

Number of Electrons

Total Negative Charge

Overall Charge

hydrogen

oxygen

magnesium

copper

E) A look at the Symbols on the PERIODIC TABLE – ATOMIC NOTATION

On the Periodic Table you see for oxygen:

Atomic number → Mass number →

SOME EXAMPLES

Oxygen Fluorine # of protons = _______ # of protons = _______

# of electrons = _______ # of electrons = _______

# of neutrons = _______ # of neutrons = _______

Example 3: An unknown element’s mass number = 31. It also has 16 neutrons

# of Protons = ________

# of Electrons = ________

# of Neutrons = ________

Therefore, the mystery element ___________________.

O16

8

O 16

8 F

19

9

? 31

+

Try These

Element

# protons

13 9

# neutrons

14 14 10

Mass number

27

# electrons

If an atom of boron has 5 protons and 6 neutrons. What is its atomic mass? Which atom has 6 protons and 6 neutrons? Which atom has 16 protons, 16 neutrons, and 16 electrons?

Ar40

18 Na 23

11

Element Name

Atomic Number

Mass Number

Atomic Notation

Number of Protons

Number of Electrons

Number of Neutrons

argon

hydrogen

4

5

carbon

19

2

12

neon

31

Ar18

40

ATOMIC NOTATION WORKSHEET

F) ISOTOPES and IONS 1) ISOTOPES ‐ not all atoms of the same element will have the same number of _____________. ‐ an element that has different numbers of ________________ is called an ______________. ‐ isotopes have the ____________________________________. THIS MEANS for an ISOTOPE:

1)

2)

Subatomic Particle

#of PROTONS

# of ELECTRONS

# of NEUTRONS

O 15

8 O

16

8 O 17

8

2) IONS Elements react with one another because elements can form ions. Ions → →

ION NAME How it Happens… What it means…

Cation

Anion

Neutral Atom → The reason atoms gain or lose electrons is because _____________________________ Atoms are considered stable when they have __________ in their outside orbit (called the ______________________________). This is called the ______________ rule. Exceptions to the octet rule:

G) Bohr‐Rutherford Diagrams A Bohr‐Rutherford diagram is a diagram or picture that summarizes where and how many protons, electrons, and neutrons there are in an atom. Rules for Electrons: 1st orbit (energy level) →

2nd orbit (energy level) →

3rd orbit (energy level) →

4th orbit (energy level) → The general formula is: Example: How many electrons are there in the 5th orbital/energy level? Answer:

EXAMPLES: a) carbon b) magnesium C) chlorine

C12

6 Mg

24

12

Cl 36

17

P = ___

E = ___

N = ___

P = ___

E = ___

N = ___

P = ___

E = ___

N = ___

H) FORMING IONS 1. 2. 3. How does Na become Na1+?

Is this stable?

Why? Now Na1+ has the same number of electrons in its valence orbit as the element ___________. This

element is still sodium because it has __________________.

How does Cl become Cl1‐?

Is this stable?

Why? Now Cl1‐ has the same number of electrons in its valence orbit as the element ___________. This

element is still chlorine because it has __________________.

BEFORE AFTER

BEFORE AFTER

Complete Bohr‐Rutherford diagrams for the following:

1a) C 1b) C

2a) O 2b) O 3a) sodium atom 3b) sodium ion

Na 4a) chlorine atom 4b) chlorine ion

Cl

12

6

14

6

23

11

35

17

16

8

18

8

Bohr‐Rutherford Diagrams of IONS and ISOTOPES WORKSHEET

5a) potassium atom 5b) potassium ion

K 6a) sulphur atom 6b) sulphur ion

S 7a) aluminum atom 7b) aluminum ion

Al

8a) nitrogen atom 8b) nitrogen ion

N

39

19

32

16

27 13

15

7

I) FORMING IONIC COMPOUNDS

Group 1 Group 2 Group 3 Group 4 Group 5 Group 6 Group 7

H → Li → Na → K →

Be → Mg → Ca →

B → Al →

N → P →

O → S →

F → Cl → Br →

Ionic Compounds

Write out the formula’s for the following:

a) calcium chloride ____________________ b) aluminum oxide ____________________

Ionic Compound Ions Involved Correct Formula

aluminum bromide potassium oxide aluminum sulphide calcium sulphide calcium chloride sodium nitride sodium phosphide hydrogen sulphide aluminum fluoride beryllium oxide

Writing formulas for Ionic Compounds WORKSHEET

J) Naming Binary Ionic Compounds ionic bond →

→ Example of an ionic bond: Rules for Naming Ionic Compounds

Metal element (cation) is first

Remove the ending from the name of the second element, the non-metal and add “-ide” Examples:

Formula Elements Name

MgO

NaCl

Al2S3

1. Write the formulas for the following binary ionic compounds. a) magnesium oxide _______________ h) magnesium nitride _______________

b) sodium fluoride _______________ i) aluminum sulphide _______________

c) aluminium nitride _______________ j) calcium nitride _______________

d) potassium sulphide _______________ k) beryllium oxide _______________

e) lithium iodide _______________ l) calcium bromide _______________ 2. Write the names for the following binary ionic compounds. a) Li2O ___________________________ b) AlCl3 ___________________________

c) MgS ___________________________ d) CaO ___________________________

e) Na2S ___________________________ f) KBr ___________________________

g) K3P ___________________________ h) CaF2 ___________________________

i) Ca3N2 ___________________________ j) BeF2 ___________________________ 3. The following questions following the same rules as the above questions. You will notice though that the

names have a Roman numeral number in it. This number is telling you what the positive charge is on the metal.

Example: iron (II) chloride: Therefore the formula is FeCl2 a) iron (III) chloride ________________ b) lead (II) oxide ___________________ c) iron (II) sulphide ________________ d) lead (IV) iodide ___________________ e) copper (I) oxide ________________ f) copper (II) oxide ___________________

comes from the (II) in the name Fe2+

BINARY IONIC COMPOUNDS WORKSHEET

K) Polyatomic Ions Monatomic ions → ions composed of only one atom Example: Na+, Cl‐, Mg2+, O2‐ Polyatomic ions → an ion that is composed of two or more atoms Example: NO3

‐

Name of Polyatomic Ion Ion Formula Ionic Charge

Ammonium NH4+ 1+

Hydroxide OH‐ 1‐

Nitrate NO3‐ 1‐

Chlorate ClO3‐ 1‐

Sulphate SO42‐ 2‐

Carbonate

Bicarbonate

CO32‐

HCO3

1‐

2‐ 1‐

Phosphate PO43‐ 3‐

L) Naming Polyatomic Compounds

* similar to naming monatomic ionic compounds EXCEPT ending is “‐ate” Example: Monatomic ionic compound:

Polyatomic ionic compound: Writing Formulas for Polyatomic Compounds * have to recognize that there is a positive half and a negative half to the compound * positive half MUST EQUAL negative half Example: sodium sulphate calcium nitrate More examples: a) sodium hydroxide __________ b) potassium carbonate __________ c) aluminum sulphate __________ d) ammonium phosphate __________

a) KClO3 _______________________ g) CaCO3 _______________________ b) KNO3 _______________________ h) Ca3(PO4)2 _______________________ c) NaClO3 _______________________ i) Na2CO3 _______________________ d) AlPO4 _______________________ j) Be(NO3)2 _______________________ e) Mg(NO3)2 _______________________ k) NH4OH _______________________ f) KOH _______________________ l) (NH4)2SO4 _______________________

a) sodium sulphate _____________ i) ammonium nitrate _____________ b) potassium hydroxide _____________ j) magnesium hydroxide _____________ c) calcium carbonate _____________ k) lithium sulphate _____________ d) calcium nitrate _____________ l) copper (I) chlorate _____________ e) iron (II) nitrate _____________ m) sodium phosphate _____________ f) iron (III) nitrate _____________ n) sodium carbonate _____________ g) calcium phosphate _____________ o) aluminum hydroxide _____________ h) lithium sulphate _____________ p) aluminum sulphate _____________

Polyatomic Compounds WORKSHEET

1. Which of the following statements about a mixture is FALSE?

a) components can be separated by physical means b) is composed of two or more pure substances

c) is either homogeneous or heterogeneous d) can be found on the period table 2. Carbon is best classified as; a) mixture; solution b) pure substance; element c) pure substance; compound d) mixture; element e) none of the above 3. Which of the following statements about solutions is/are TRUE ?

a) are a pure substance b) are composed of two or more pure substances c) solutions are homogeneous d) A, B and C are all true e) only B and C are true 4. The chemical formula for sucrose (table sugar) is C12H22O11. This formula tells us that;

a) sucrose is a compound composed of three different elements b) a sucrose molecule contains 45 atoms in total c) in a single sucrose molecule, there are twice as

many hydrogen atoms as oxygen atoms d) all of the above

5. Based on the Bohr Model, which of the following statements about the atom is FALSE?

a) in a neutral atom, the number of protons equals the number of electrons

b) the protons and electrons are located in the nucleus c) neutrons have no charge ( ie. are neutral ) d) electrons orbit the nucleus in specific energy

levels e) the nucleus is dense, positively charged and is

located in the centre of the atom

For questions 6 to 15, use the following answer key to classify each substance. (E) element (HOM) homogeneous mixture (C) compound (HET) heterogeneous mixture

6. table salt (sodium chloride)

7. glass of Kool‐Aid

8. sand and water

9. sugar dissolved in water

10. gold

11. pure water ( H20 )

12. milk and cereal

13. neon

14. potassium iodide ( KI )

15. lead

For questions 16 to 25, write "PC" if it is a physical change and "CC" if it is a chemical change. 16. crushing an aspirin

17. rusting of iron

18. combustion of acetylene

19. evaporation of rubbing alcohol

20. tarnishing of silver

21. dissolving salt in water

22. the melting of snow

23. burning magnesium in oxygen

24. filtering clay from river water

25. mixing two colourless solutions together produces a yellow colour

UNIT 1 : Grade 9 & 10 REVIEW WORKSHEET

26. What is the major difference between a physical change and a chemical change? 27. What are the 5 indications that a chemical change has occurred (i.e. what do you see or feel)? 28. Use your notes to complete the following blanks. a) ______________ the number of protons in an atom

b) ______________ a change in which a new substance is formed

c) ______________ only contains one type of atom and is found on the Periodic Table

d) ______________ number of protons and neutrons in an atom

e) ______________ a mixture that only has only one layer or phase that you can see

f) ______________ contains two or more elements that are bonded together

g) ______________ the ability of a substance to be stretched into a wire

h) ______________ this is what you call a row on the Periodic Table

I) ______________ the ability of a substance to transmit light

j) ______________ a chemical compound composed of a metal and a non‐metal

k) ______________ is a type of ion that has a negative charge

29. Fill in the missing information in the table given below.

Element Element Symbol

Atomic Number

Atomic Mass

# of Protons

# of Electrons

# of Neutrons

Carbon 6 12

Potassium K 39 19

9 9 10

Silver Ag 48 114

Nitrogen N 7 7

30. Draw Bohr‐Rutherford diagrams for the following. a) calcium atom calcium ion

b) phosphorus phosphorus ion 31. What is the difference between a cation and an anion? Make sure that you include a discussion on the number of protons versus the number of electrons in each.

lose/gain _______ electrons

lose/gain _______ electrons

32. Complete the following table.

Element Number of

valence electrons Number of electrons

lost or gained Ion

Hydrogen 1 1 electron lost H1+

Calcium

Sulphur

Fluorine

Aluminum

Lithium

Nitrogen

33. Name the following binary ionic compounds.

a) KBr _____________________ b) CaO _______________________

c) Mg3N2 _____________________ d) K3N _______________________ 34. Write the formula for the following binary ionic compounds.

a) potassium sulphide ____________ f) aluminum nitride _____________

b) magnesium oxide ____________ g) calcium chloride _____________

c) aluminum sulphide ____________ h) hydrogen bromide _____________

d) beryllium phosphide ____________ i) iron (II) fluoride _____________

e) lead (IV) oxide ____________ j) copper (I) nitride _____________

35. Name the following polyatomic ionic compounds.

a) K2SO4 _____________________ d) NH4OH ______________________ b) NaNO3 _____________________ e) Al2(PO4)3 ______________________ c) MgSO4 _____________________ f) K2CO3 ______________________ 36. Write the formula for the following polyatomic ionic compounds. a) sodium carbonate _____________ e) calcium phosphate _____________

b) ammonium nitrate _____________ f) lithium sulphate _____________

c) iron (II) oxide _____________ g) iron (III) oxide _____________

d) magnesium sulphate _____________ h) aluminum phosphate _____________

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