F4-C4-Periodic Table of Elements

8/6/2019 F4-C4-Periodic Table of Elements

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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of Elements

A Historical Development Of The Periodic Table

1 Antoine Lavoiser (1743-1794)The first Scientist classifies substances including . and .,

into ..and.

Substances were classified into four groups with similar chemical

properties.

His classification was unsuccessful because , and a few

other compounds were also considered as elements.

2 Johann Dobereiner (1780-1849) Divided the elements into groups ofthree elements with similar

chemical properties, known as .

The atomic mass of the middle element was approximately the averageatomic mass of the other two elements in each triad.

This classification led chemist to realise that there was a relationship between

the . and the atomic mass of each element.

Example :

Element in triad LiNa

KAverage relativeatomic mass of Li

and K

Relative atomicmass,Ar

7 39 2

397 +

= 23

3 John Newlands (1837-1898) He arranged the known elements in order ofincreasing atomic mass.

Elements with similar chemical properties were repeated at every eighth

element. This was known as the Law of.

This system was inaccurate because the Law of Octaves was obeyed by thefirst 17 elements only and there were some elements with wrong atomicmass/mass number.

1

CHAPTER 4: PERIODIC TABLE OFELEMENTS

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However, Newlands was the first chemist to show the existence of. for the properties of elements.

4 Lothar Meyer (1830-1895) He plotted a graph of.. against for allthe known elements.

Atomic volume =

He realised that elements with .. occupiedequivalent positions along the curve.

He was successful in showing that the properties of the elements formed a

periodic pattern against their..

5 Dimitri Mendeleev (1834-1907) Arranged the elements in order of ...

He grouped the elements according to ... [Elements with similar chemical properties were in the same group].

He left gaps in the table to be filled by .. elements.

He was able to predict the properties of undiscovered elements.

[e.g : Ekasilicon, Es is predicted by Mendeleev in 1869 was discovered asGermanium, Ge in 1886 ].

6 Hendry J. G. Moseley (1887-1915) Studied the .. of elements.

[Introduced the concepts ofproton numberof each elements]

2

Mass of 1 mol (g)

Density (g cm-3)

Li

Atomic

volume

Atomic mass

Na

K

Be

Mg

Ca

B

Al

What colourshould be here?


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He concluded that should be used as the basis forthe periodic changes of chemical properties of elements instead of the atomicmass.

He rearranged the elements in order ofincreasing proton number in thePeriodic Table.

B Arrangement of Elements in the Periodic Table

Elements in the Periodic Table are arranged in an .. order of

.., ranging from 1 to 103.

Elements with .. are placed in the same vertical column

called ..

LanthanidesActinides

There are vertical columns of elements in the Periodic Table.

Each vertical column of elements is called a ..

The vertical columns are known as to .

There are horizontal rows of elements in the Periodic Table.

Each of these horizontal rows of elements is called a

The horizontal rows are known as . to.

Activity1:-

In the table below, write :

(a) Group 1 to 18(b) Period number 1 to 7

(c) the symbol of each element from Hydrogen to Calcium

1 181 H 2 H

e2

3 4

C

3

Horizontal row

Verticalcolumn


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a

LanthanidesActinides

The number ofvalence electrons in an atom decides the ..of an element in the Periodic Table.

Example :

The proton number of sodium, Na is 11.

The electron arrangement of sodium atom is 2.8.1The valence electron of sodium is 1Sodium is placed in Group 1 in a Periodic Table.

For elements with 1 and 2valence electrons, the group number of the

element is the number of valence electrons in its atom.

For elements with 3to8 valence electrons, the group number of the elementis the number of valence electrons in its atom plus ten (+10) [ valence

electron + 10 ]

Example :

The proton number of chlorine is 17The electron arrangement of chlorine is 2.8.7The valence electrons of chlorine is 7

Chlorine is placed in Group 17 [ 7 +10 ]

Elements from period 3

The position of theperiodof an

element in the

Periodic Table isdetermined by the

number of

..

occupied/filled with

electrons in the

atom of that element.

Theperiod number

of an element isthe number of shell occupied withelectrons in its atom.

Example :

Element

Protonnumber

Electronarrangem

ent

Valence

electron

Group

Na 11 2.8.1 1 1

Mg 12

Al 13 2.8.3 3 13

Si 14

P 15

S 16

Cl 17 2.8.7 7 17

Ar 18

4

Group :

Valence electrons + 10


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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of ElementsThe proton number of magnesium is 12The electron arrangement of magnesium is 2.8.2

There are 3 shells occupied with electrons in magnesium atom.

The period number of magnesium in the Period Table is 3

Activity2:-

Complete the following table :

Element Li C O Ne Mg Al P Cl K Ca

Protonnumber

3 6 8 10 12 13 15 17 19 20

Electronarrangement

2.1 2.4 2.8 2.8.2 2.8.3

Number of

valenceelectron

1 4 8 3

Group 1 14 18 13

Number ofshellsoccupiedwithelectrons

2 2 2 3

Period 2 2 2 3

Specific name of certain groups :

Group Specific name

1 Alkali metal #

2 Alkali-earth metal

3 to 12Transition

element #17 Halogen #

18 Noble gas #

#The important groups that will be studied from the aspect ofphysicalandchemicalproperties.

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Activity3:-

1 Write the electron arrangement for each element in the following Periodic Table.

Symbol of element : [ Standard form ]

GROUP

1 181

H1..

2 13 14 15 16 17

4 He2..

7 Li3

..

9Be4

..

11 B5

..

12 C6

..

14 N7

..

16 O8

..

19F

9

..

20 Ne

10..

23 Na11..

24 Mg12..

3 4 5 6 7 8 910

11

12

27 Al13..

28 Si14..

31 P15..

32 S16..

35 Cl17..

40 Ar18..

39 K19..

40 Ca20..

TRANSITION ELEMENTS

2 Complete the statement and answer the following questions based on the tablebelow.

Element

Nucleonnumber

Number ofneutrons

A 9 4

B 31 16

C 35 18

(i)The proton number of A is and the number of electrons in an atom

A is ...

The electron arrangement of atom A is..

6

A

XZ

Nucleon number

Proton number1

2

3

4

PERIOD


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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of ElementsThe valence electron of atom A is ..

Atom A is in Group ..and Period ..

(ii) Atom B is in Group ..and Period ..

(iii) A student states that atom C is in Group 17 and Period 3 in Periodic

Table of Element. Is the statement true or false? Explain your answer.

...............

...............

...............

Advantages of Grouping Elements in the Periodic TableThe systematic arrangement of elements in the Periodic Table helps us to study the

elements systematically, especially in their and ..

properties.

Elements with the .. number of . are placed in the

sameGroup because they have the same chemical properties.

Elements are arranged systematically in the Periodic Table in the order of

increasing ofproton number which enable chemists to study, understand andremember :

(a) the chemical and physical properties of all the elements and compounds in anorderly manner.

(b) the properties of elements and their compounds are predicted based on the

position of elements in the Periodic Table.(c) the relationship between the elements from different groups can be known.

C GROUP 18 ELEMENTS

1. Group 18 elements consists of ., .., .., ,

. and ..

2. These elements are known as gases.

3. Group 18 elements exist as monoatomic at room condition because Noble

gases achived stable electron arrangement which is for helium

and for other elements.

4. Noble gases do not have to lose, gainorshare electrons.

Physical Properties of Group 18 Elements

Noble gases have very .. atomic sizes.

They are . gases at room temperature and pressure.

Noble gases have .. melting and boiling points and also ..

densities.

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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of ElementsNoble gases are in water, conduct electricity and

. conductors of heat.

Going down Group 18 [Refer to Text Book, page 64]

Element

Relative

atomicmass

Proto

nnumber

Atomic

radius(nm)

Meltin

g point(oC)

Boiling

point(oC)

Densit

y(g dm-3)

Helium,

He4 2

Neon,

Ne20 10

Argon,

Ar40 18

Krypton,

Kr84 36

Xenon,Xe 131 54

Radon,

Rn222 86

When going down Group 18 :

The atomic size as the number of shells in the atom .. from

Helium to Radon.

The melting and boiling points is very low.

because the atoms of Noble gases are attracted by weakVan der Waal

force.

Less energy is required to overcome it.

However, the melting and boiling points increases when going down Group

18.

because the atomic size of each element down the group,

the forces of attaraction between the atoms of each element become

.

thus more is required to the stronger forces of

... during melting or boiling.

The density of an element .. down the group because the atomic

mass of each element is

The Inert Property of Group 18 Elements

All Noble gases are inertwhich means .. .

Noble gases and the electron arrangement of their atoms [Refer to Text Book, page65]

Noble gas Electron

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arrangementHelium 2Neon 2.8Argon 2.8.8Krypton 2.8.18.8Xenon 2.8.18.18.8Radon 2.8.18.32.18.8

Helium has two valence electrons. This is called a . electron

arrangement.

Other Noble gases have eight valence electron called the .. electron

arrangement.

These electron arrangements are very stable.

That is why Noble gases exist as monoatomic gases and are chemically

unreactive; because they achived the stable octet/duplet electron

arrangement.

Uses of Group 18 Elements

Noble gas Uses

Helium, He

Neon, Ne

Argon, Ar

Krypton, Kr

Xenon, Xe

Radon, Rn

D GROUP 1 ELEMENTS

1. Write the name and symbols of elements in Group 1 (exceptHydrogen)

2. Group 1 are also known as which react with water to formalkaline solutions.

3. Shade in the boxes for all the elements in Group 1 in the Periodic Table ofElements :

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4. Write the proton number and electron arrangement for all elements in Group1.

Elements

Proton

number

Electronarrangeme

nt

Density / gcm-3

Boilingpoint /

0C

Li 3 2.1 0.534 1360

Na 0.971 900

K 0.862 777

Rb 2.8.18.8.1 1.530 505

Cs 2.8.18.18.8.1 1.973

Fr2.8.18.32.18.8.1

All Group 1 elements have valence electron in their outermostoccupied shells.

5. Physical Properties of Group 1 elements :

Soft / hard* metals

Low / high* densities.

Low / high* melting points.

silvery solid with shiny surface.

good of heat and electricity.

Change in the physical properties going down the group :

The atomic size because the number of shells

increases.

The density because the increasing in atomic mass isfaster than the increasing in atomic volume/size.

The melting and boiling points because when the atomic sizeincreases, the metal bondbetween the metal atoms becomes weaker.

The hardness of the metal .

6. Chemical Properties of Group 1 elements :

(a) React with water to produce alkaline metal hydroxide solutions

[colourless solutions] and released gas.

10

compared to other metals

such as iron and copper.

water

metal*

Redlitmus paper

turnsRedlitmus paper


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Metal* Observation

Li

Lithium moves slowlyon water surface with hiss

sound.

The colourless solution formed; turns red litmus paperto blue.

Na

Sodium moves quicklyon water surface with hisssound.


K

Potassium moves vigorouslyon water surface withhiss sound.


Chemical equation :

2Li + 2H2O 2LiOH + H2 Lithium Water Lithium Hydrogen

hydroxide gas

+ 2H2O 2NaOH +

2K + 2H2O +

(b) React with oxygen gas to produce metal oxides [white solids].

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Gas jar

Metal*

Oxygen gas

White fume

Gas jar spoon


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Metal* Observations

Li

Lithium burns slowlywith a red flame.

A white / fume solid is produced.

Na

Sodium burns brightlywith a yellow flame.

A white solid is produced.

K

Potassium burns very brightwith apurple/lilac flame.

A white solid is produced.

Example :

4Li + O2 2Li2OLithium Oxygen gas Lithium oxide

+ O2 2Na2O

. Oxygen gas ..

4K + O2

. Oxygen gas ..

(c) React with chlorine gas to produce metal . [white solids].

12

Gas jar

Metal*

Chlorine gas

White fume

Gas jar spoon


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7. Reactivity of elements in Group 1 :

When going down Group 1,

the proton number are ..

the number of shells occupied with electrons are

the atomic size of atoms are

the single valence electron becomes away from thenucleus.

the force of attraction between the nucleus and valence electron (nuclei

attraction) becomes

it is for the atom to donate the single valence

electron to achieve the stable octet/duplet electron arrangement of

the atom of Noble gases.

Reactivity increases when going down the group!

Activity4 :-

1. Table below shows the electron arrangements of element W, X and Y.Arrange the elements in ascending order of reactivity.

Eleme

nt Proton Number

Electron

Arrangement

W 11 2.8.1

X 3 2.1

Y 19 2.8.8.1

Answer: .

Safety precautions in handling Group 1 elements

Alkali metals are very reactive. Safety precautions must be taken when handlingalkali metals.

The elements must be stored in paraffin oil in bottles Do not hold alkali metals with your bare hands Use forceps to take them Wear safety goggles Wear safety gloves Use a small piece of alkali metal when conducting experiments

E GROUP 17 ELEMENTS

Activity 5

1) State the uses of Chlorine and iodine

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a) Chlorine .

b) Iodine ..

2 (a) Give the physical state of halogens below at room temperature :

i) Fluorine:

ii) Chlorine:

iii) Bromine: .

iv) Iodine : .

(b) Fill in the blanks below.

2Cl melting and colour of Density

2Br boiling points halogens .

2I .. becomes

.

3) When going down the Group 17, the melting and boiling points increase. Explain

..

.

4) Chemical Properties of Group 17 Elementsa) Group 17 elements react with water to form two acids

Example: 2Cl + OH2 HCl + HOCl

hydrochloric hypochlorusacid acid

Write a balanced equation when bromine reacts with water.

..

b). In gaseous state they react with hot iron to form a brown solid, iron(III) halides.

Example: Fe2 + 23Br 32FeBr

Write a balanced equation when iodine vapour reacts with iron

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c). Group 17 elements react t with sodium hydroxide solution, NaOH , toform

sodium halide, sodium halate (I) and water

Example: 2I + NaOH2 NaI + NaOI + OH2

Write a balanced equation when chlorine reacts with sodium hydroxidesolution

.5) The reactivity of Group 17 elements decreases when going down the group.

Explain why.

a) When going down the Group 17 atomic size ..b) The outermost occupied shell becomes . from the

nucleus.c) Therefore the strength to attract one electron into the outermost

occupied shell by the nucleus becomes

6) Chlorine gas reacts more vigorously with hot iron as compared to brominegas. Explain (Proton number: Cl, 17 ; Br, 35)

.

..

Activity 6

To investigate the Chemical properties of Group 17 elements. The Reaction ofhalogens with iron

1) Data and Observation (Complete the following table)

HalogenReactant

Observation

Chlorine Bromine Iodine

Water

Iron wool

Sodium hydroxide , NaOHsolution

2) Based on your results, arrange the halogens, 2Cl , 2Br , 2I in ascending orderof reactivity.

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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of Elements.

3) Element E is placed below element D in Group 17 of the Periodic Table.

(a). Compare the melting and boiling points of element D with element E.Explain your answer

.

..

..

(b). Write a chemical equation for the reaction between element D and hotiron.

.

F ELEMENTS IN A PERIOD

Activity 7Period 3 in the Periodic Table Properties of Elements

1) Complete the table and answer the question given below

Element Na Mg Al Si P S Cl Ar

Proton number 11 12 13 14 15 16 17 18

ElectronarrangementNumber ofvalence electronsAtomic radius

(pm)

186 160 143 118 110 104 100 94

Physical state atroom temperature

Solid

Solid Solid Solid Solid Solid Gas Gas

Electronegativity 0.9 1.2 1.5 1.8 2.1 2.5 3.0 -

2) Fill in the blanks with the correct answer.

a). The proton number .. by one unit from one element

to the next element

b) All the atoms of elements have .. shells occupied with

electrons.

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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of Elementsc) The number of valence electrons in each atom . from 1 to 8.

d) The physical state at room temperature changes from to

..

e) The atomic radius (atomic size) of elements from left to right

across the period 3

f) The electronegativity of elements. .. from left to right across the

period 3 .

Activity 8

1) Below are some oxides of elements of Period 3.

(a). Which of these oxides can react with(i) dilute nitric acid? .(ii) sodium hydroxide solution? .

(b). Based on your answers in (a), what inferences can you make about theproperties of each of the oxides?

Oxide of elements in Period 3 Acidic / Basic / AmphotericSodium oxide

Magnesium oxide

Aluminium oxide

Silicon (IV) oxide

Phosphorus (V) oxide

Sulfur dioxide

2)

The diagram above shows the symbols of lithium, carbon and fluorine.

(a). Which period in the Periodic Table can you find the three elements?Explain.

.

.(b). Arrange the three elements in order of increasing atomic size.

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*Sodium oxide, ONa2

*Silicon (IV) oxide,2

SiO

*Aluminium oxide, 32OAl *Sulphur dioxide, 2SO

Li

7

3 , C12

6 , F19

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(c). Compare the electronegativity of the three elements. Explain youranswer.

The electronegativity of the elements (i) from Li , C , F

This is due to the (ii).. nuclei attraction on the valence electronsand the

(iii) in atomic size.

G TRANSITION ELEMENTS

Activity 9

1 (a) Transtition elements are elements from Group . to Group.

(b) State 3 examples of transtition elements found in Period 4

..

2 Complete the diagram below.

3 Transition elements and their compounds are useful catalysts. Complete the

table below

Chemical Process Product CatalystsHaber

Special characteristics of Transition elements

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OstwaldContact

4 Transition elements form coloured ions or compound Complete the table below

Ion of transition element Formula of the ion Colour of aqueous solution

Cooper (II) ion

Iron (II) ionFe 2+

Iron (III) ion

Yellowish Brown

Chromium (III) ion

Chromate (VI) ion

Dichromate (VI) ion

Manganese (II) ion

Manganate (VI) ion

4 Transition elements form ions with different Oxidation Numbers.

Elements Compound Chemical Formula Oxidation NumberManganese Manganese (II) chloride

Manganese (IV) oxidePotassium manganate

(VI)Iron Iron (II) chloride

Iron (III) chlorideCopper Copper (I) chloride

Copper (II) oxide

**(Precious stones such as emerald, rubies, sapphire and jade are beautiful due to

the colours of the transition element compounds present in them )

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Activity 12

1 Diagram 1 shows part of the Periodic Table of the Elements. D, E, G, L, M, and J,

that do not represent the actual symbol of the element

Diagram 1

Using the letters in the Periodic Table of the Elements in Diagram 1, answer thefollowing questions.

(a) (i) State the position of element E in the Periodic Table.

..

(ii) Choose the element which exhibit different oxidation numbers in itscompounds.

.....

(b) Element D combines with element L to form a compound.Write the chemical formula of this compound.

..............................

(c) D and E have the same chemical properties

(i) Which element is more reactive?

...............................................................................................................

................

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LD

M

G

J

E


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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of Elements(ii) Explain your answer in (c) (i).

..

..

(d) Which element exists as diatomic molecules?

...

2 The information shows the chemical symbols which represent elements W, X,Y and Z.

W X Y Z

(a) State three subatomic particles in an atom..

.................................

(b) (i) What is the meaning of the period in the Periodic Table ofelement?

.......................................................................................................................

.....................................................................................................................

(ii) State the period of element W in the Periodic Table of element.Explain.

...........................

..............................................................................................................

(c) (i) Compare the atomic size of element W and X.

.......................................................................................................

......

(ii) Explain your answer in (c) (i).

22

27

13

35

17

12

6

23

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Pusat Tuisyen Ilmuan Jaya Chemistry Form 4 Chapter 4: Periodic Table of Elements.......................................................................................................

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End of Chapter 4

F4-C4-Periodic Table of Elements

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