Chemistry Module Form 4 (4) 104e5b
This document was ed by and they confirmed that they have the permission to share it. If you are author or own the copyright of this book, please report to us by using this report form. Report 3i3n4
Overview 26281t
& View Chemistry Module Form 4 (4) as PDF for free.
More details 6y5l6z
- Words: 2,208
- Pages: 25
mohd faisol mansor/chemistry form 4/chapter 4
CHAPTER 4 PERIODIC TABLE OF ELEMENTS
54
mohd faisol mansor/chemistry form 4/chapter 4
PERIODIC TABLE
55
mohd faisol mansor/chemistry form 4/chapter 4
Historical Development of Periodic Table
Antoine Lavoiser (1743 – 1794)
Johann Dobereiner (1780 – 1849)
John Newlands (1837 – 1898)
divided element according their similar chemical properties
arranged element in order of increasing atomic mass
first scientist classify substances.
Lothar Meyer (1830 – 1895)
Dmitri Mendeleev (1834 – 1907)
showing that the properties of the elements formed a periodic pattern against their atomic masses.
arranged the elements in order of increasing atomic mass and grouped them according to similar chemical properties.
Henry J.G. Moseley (1887 – 1915) Studied the X-ray spectrum of elements. He rearranged the elements in order of increasing proton number.
Concluded that the proton number should be the basis for the periodic change of chemical properties instead of the atomic mass. Leading to the modern Periodic Table.
56
mohd faisol mansor/chemistry form 4/chapter 4
Arrangement of Element in the Periodic Table Element in the Periodic Table are arranged in an increasing order of proton number ranging 1 to 118.
GROUP The number of valence electron in an atom decides the position of the group of an element.
Element with similar chemical properties are placed in the same vertical column
GROUP
Valence electron 1 and 2
18 vertical column called a group 7 horizontal rows called a period
GROUP
Valence electron 3 until 8
Example: PERIOD Equal to the number of shell occupied with electrons in its atom
An atom of element X has a proton number of 15. In which group and period we can find element X in Periodic Table.
57
mohd faisol mansor/chemistry form 4/chapter 4
Exercise
Atom, Molecule & Ion
1. Element D has a proton number 19. Where is element D located in Periodic Table?
2. An atom of element E has 10 neutrons. The nucleon number of element E is 19. In which group and period of element E located in the Periodic Table?
3. An atom of element G has 3 shell occupied with electrons. It is placed in Group 17 of the Periodic Table. What is the electron arrangement of atom G?
4. An atom Y is located in Group 18 and period 2 of the periodic Table. What is the electron arrangement and proton number of atom Y?
5. Element R has a proton number of 11. Its atom has 6 neutrons. In which group and period can you find element R in the Periodic Table?
58
mohd faisol mansor/chemistry form 4/chapter 4
The advantage of grouping elements in the Periodic Table 1. Helps us to study the element systematically especially their physical and chemical properties. 2. Element with a same number valence electron is place in the same group because they have the same chemical properties. 3. It could be used to predict undiscovered properties. 4. To relate the characteristic of an element with atomic structure
59
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 18
GROUP 18
consist of helium, neon, argon, krypton, xenon and radon
Known as NOBLE GAS Exist as monoatomic gas.
Physical Properties of Group 18
COLOUR
SOLUBILITY
GROUP 18 NOBLE GAS ELECTRIC CONDUCTIVITY
DENSITY
MELTING & BOILING POINT
60
mohd faisol mansor/chemistry form 4/chapter 4
The inert properties of G18
All noble gas are inert which means unreactive. Noble gas are inert because the outermost occupied shell are full. This electron arrangements are very stable. Helium have 2 valence electron, this electron arrangement is called duplet electron arrangement whereas other noble gas have eight valence electron which called octet electron arrangement.
p/s:
All other element try to achieve noble gas electron arrangement to become stable.
The Physical Properties of G18
The physical properties vary down the group. physical properties vary down the group are related to atomic size. Melting and boiling point of an element increase when going down the group because the atomic sizes increase, the forces attraction (Van der Waals forces) becomes stronger. Thus more heat energy is required to overcome the forces. The strength of Van der Waals forces propotional to the size of particle
61
mohd faisol mansor/chemistry form 4/chapter 4
Uses of Noble Gas Elements [ State the element of group 18 ]
Fill light bulb
laser for repair retina, photographic flash lamps
treatment cancer
fill airships and weather balloons
Car bulb, use in bubble chamber
advertising light and television tubes
62
mohd faisol mansor/chemistry form 4/chapter 4
Exercise 1. Table below shows the electron arrangements of atoms of elements P, Q, and R.
Element
Electron Arrangement
P
2.8
Q
2.8.18.8
R
2.8.18.32.18.8
a) Arrange the element in ascending order of boiling points. Give reasons for your answer.
b) Elements P, Q, and R are chemically unreactive. Why?
2) What is the meaning of a) Duplet electron arrangement
b) Octet electron arrangement
63
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 1 Known as Alkali Metals. Have valence electron of 1.
Consist of elements such as lithium, sodium, potassium, rubidium, caesium and francium.
Physical Properties of Group 1
HARDNESS
ELECTRIC CONDUCTIVITY
APPEARANCE
GROUP 1 ALKALI METALS
DENSITY
MELTING POINT
64
mohd faisol mansor/chemistry form 4/chapter 4
Element
Atomic Size
Melting / Boiling point
Density
Hardness
Lithium Sodium Potassium Rubidium Caesium Francium
A melting point of a metal indicates the strength of its metallic bonding in its structure. Generally, the strength of metallic bonding is directly proportional to the number of valence electron per atom divided by the radius of a metal. A metallic bond can be defined as the electrostatic force between the positively charged metallic ions and the ‘sea’ of electrons. Electropositivity is the measurement of an atom to release an electron and form positive ion When going down the group, what happen to the electropositivity of the element? Why?
65
mohd faisol mansor/chemistry form 4/chapter 4
Chemical Properties of Group 1 Elements React vigorously with water to produce alkaline metal hydroxide solution and hydrogen gas, H2. 2Li (s) + 2H2O
2LiOH (aq) + H2 (g)
Burn in oxygen gas rapidly to produce solid metal oxide 4Li (s) + O2 (g)
2 Li2O (s)
Solid metal oxide dissolve in water to form alkaline metal hydroxide Li2O (s) + H2O
2LiOH (aq)
Alkaline metal burn in chlorine gas, Cl2 to form white solid metal chloride 2Na (s) + Cl2
2NaCl (aq)
Exercise : 1. Why does Group 1 element have similar chemical properties?
2. Why is paraffin oil used to store metals such as sodium and potassium?
3. Element in Group 1 has similar chemical properties but differ in reactivity. Why?
66
mohd faisol mansor/chemistry form 4/chapter 4
To investigate the chemical properties of Lithium, Sodium & Potassium 1) The reaction of alkali metals with water
2) The reaction of alkali metals with O2 gas
[ Draw the diagram ]
[ Draw the diagram ]
[ Discussion ] 1. Why are the experiments involving sodium and potassium demonstrated by your teacher and not carried out by the students?
2. Write the chemical equations for the reactions of lithium, sodium and potassium with a) Water, H2O Lithium
:
Sodium
:
Potassium
:
b) Oxygen gas, O2 Lithium
:
Sodium
:
Potassium
: 67
mohd faisol mansor/chemistry form 4/chapter 4
3. Write the chemical equations for the reactions between the products from the combustion of each alkali metal with water. Lithium : Sodium : Potassium :
Exercise 1. A student performs two experiments to study the reaction of alkali metal with water. Experiment
Metal used
Observation
1
Sodium
Sodium moves rapidly and randomly on the water surface and emits ‘hiss’ sounds.
2
Lithium
Lithium moves slowly on the water surface.
a) Write the chemical equation for the reaction between sodium and lithium with water. Lithium : Sodium : b) Between reactions of Experiment 1 and 2, which is more vigorous? Explain your answer from the point of electron arrangement.
c) Explain why sodium and lithium show similar chemical properties? d) Calculate the volume of hydrogen gas produced if 2.3 g of sodium is used. [RAM: Na, 23 ; molar volume: 24 dm3 mol-1]
68
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 17
GROUP 17
GROUP 17
consist of fluorine, chlorine, bromine, iodine and astatine.
Known as HALOGENS.
Elements are poisonous.
Have valence electron of 7.
Exist as diatomic molecules.
Element
Symbol of Atom
Symbol of Molecule
Physical state at room condition
Colour
Fluorine Chlorine Bromine Iodine Astatine
Melting & Boiling Point
Density
Electric Conductivity Physical State HALOGENS Smell
69
mohd faisol mansor/chemistry form 4/chapter 4
Element
Atomic Size
Melting / Boiling point
Density
Electronegativity
Fluorine Chlorine Bromine Iodine Astatine
Electronegativity is an ability of atom to receive an electron to become negative charged ions. All halogen have seven valence electron. Their atoms always gain one electron to form an ion with a charge of –1, in order to achieve stable octet electron arrangement.
Chemical Properties of Group 17 Elements
Halogen react with water to produce two acids Cl2 + H2O
HCl
+
HOCl
Halogen react with metal to produce metal halides 2Fe (s) + 3Cl2 (g)
FeCl3 (s)
Halogen react with sodium hydroxide solution to form sodium halide and sodium halate (I) and water I2(s) + 2NaOH (aq)
NaI (aq) + NaOI (aq) + H2O (l) 70
mohd faisol mansor/chemistry form 4/chapter 4
To Investigate the Chemical Properties of Halogens [Draw the Apparatus]
SECTION A : Reaction with Water 1) Chlorine
2) Bromine
3) Iodine
SECTION B : Reaction with Iron 1) Chlorine
2) Bromine
3) Iodine
SECTION C : Reaction with Sodium Hydroxide 1) Chlorine
2) Bromine
3) Iodine
71
mohd faisol mansor/chemistry form 4/chapter 4
[Discussion] 1.
Name the products formed when chlorine, bromine, and iodine react with water. Chlorine Bromine Iodine
2.
: : :
Write the chemical equations for the reaction of chlorine, bromine and iodine with water. Chlorine Bromine Iodine
: : :
3.
What is the function of soda lime in SECTION B?
4.
Name the products formed when chlorine, bromine, and iodine react with iron. Chlorine Bromine Iodine
5.
: : :
Write the chemical equation for the reaction of chlorine, bromine, and iodine with iron. Chlorine Bromine Iodine
: : :
72
mohd faisol mansor/chemistry form 4/chapter 4
4.
Name the products formed when chlorine, bromine, and iodine react with sodium hydroxide solution. Chlorine Bromine Iodine
5.
Write the chemical equation for the reaction of chlorine, bromine, and iodine with sodium hydroxide solution. Chlorine Bromine Iodine
6.
: : :
: : :
Describe the changes in reactivity of Group 17 elements when going down the group. Explain your answer.
73
mohd faisol mansor/chemistry form 4/chapter 4
Exercise 1. Table below shows several halogen elements with their proton numbers. Halogen
Proton Number
X
9
Y
17
Z
35
a) State the group that the halogen elements belong to in the Periodic Table.
b) i) Write the electron arrangement of elements X and Y.
ii) From your answers in (b)(i), deduce the period of elements X and Y.
c) Draw the electron arrangement of element Y.
d) State the changes of properties of halogens down the group from X to Z in of: i) Atomic radius
ii) Electronegativity
iii) Melting point and boiling point 74
mohd faisol mansor/chemistry form 4/chapter 4
e) i) Iron glow brightly when reacting with element Y. Write the chemical reaction to represent this reaction.
ii) Predict the observation for the reaction between iron and element Z.
iii) Between Y and Z, which is more reactive? Explain why.
f) i) Determine the elements X, Y and Z.
ii) State the colour for each elements X, Y, and Z.
iii) Why the physical state of halogen differ when down the group?
75
mohd faisol mansor/chemistry form 4/chapter 4
Comparison & Similarities between Group 1 and Group 17
Properties Atomic Size Melting & Boiling Point Density
Reactivity
Group
Down the Group
1 17 1 17 1 17 1 17
76
mohd faisol mansor/chemistry form 4/chapter 4
Elements in a Period 3 Element
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Symbol Proton Number Electron Arrangement Metal Properties Physical State [RC] Atomic Radius Electronegativity Property of the oxide
The proton number ____________ by one unit. All atom of the element have __________ shells occupied by electron. The number of valence electron ____________ from 1 to 8. All element exist as __________ except chlorine and argon. The atomic radius of element ________________. The electronegativity of element ______________. The oxides of element in Period 3 change from basic to acidic properties, therefore the metallic properties decrease across the period. On the other hand non-metallic properties of the elements increase.
Note: the atomic radius ______________ and electro negativity ______________ due to the increasing nuclei attraction on the valence electrons. (nuclei attraction force increase with the increase of proton number)
77
mohd faisol mansor/chemistry form 4/chapter 4
Transition Elements Transition elements are elements from Group 3 to Group 12
All the elements are metals, usually solids with shiny surfaces, ductile, malleable and have tensile strength. Have high melting and boiling point as well as high density. Good conductors of heat and electricity. Three special characteristics of transition element Show different oxidation number in their compound. Form coloured ions or compound.
Act as catalysts.
78
CHAPTER 4 PERIODIC TABLE OF ELEMENTS
54
mohd faisol mansor/chemistry form 4/chapter 4
PERIODIC TABLE
55
mohd faisol mansor/chemistry form 4/chapter 4
Historical Development of Periodic Table
Antoine Lavoiser (1743 – 1794)
Johann Dobereiner (1780 – 1849)
John Newlands (1837 – 1898)
divided element according their similar chemical properties
arranged element in order of increasing atomic mass
first scientist classify substances.
Lothar Meyer (1830 – 1895)
Dmitri Mendeleev (1834 – 1907)
showing that the properties of the elements formed a periodic pattern against their atomic masses.
arranged the elements in order of increasing atomic mass and grouped them according to similar chemical properties.
Henry J.G. Moseley (1887 – 1915) Studied the X-ray spectrum of elements. He rearranged the elements in order of increasing proton number.
Concluded that the proton number should be the basis for the periodic change of chemical properties instead of the atomic mass. Leading to the modern Periodic Table.
56
mohd faisol mansor/chemistry form 4/chapter 4
Arrangement of Element in the Periodic Table Element in the Periodic Table are arranged in an increasing order of proton number ranging 1 to 118.
GROUP The number of valence electron in an atom decides the position of the group of an element.
Element with similar chemical properties are placed in the same vertical column
GROUP
Valence electron 1 and 2
18 vertical column called a group 7 horizontal rows called a period
GROUP
Valence electron 3 until 8
Example: PERIOD Equal to the number of shell occupied with electrons in its atom
An atom of element X has a proton number of 15. In which group and period we can find element X in Periodic Table.
57
mohd faisol mansor/chemistry form 4/chapter 4
Exercise
Atom, Molecule & Ion
1. Element D has a proton number 19. Where is element D located in Periodic Table?
2. An atom of element E has 10 neutrons. The nucleon number of element E is 19. In which group and period of element E located in the Periodic Table?
3. An atom of element G has 3 shell occupied with electrons. It is placed in Group 17 of the Periodic Table. What is the electron arrangement of atom G?
4. An atom Y is located in Group 18 and period 2 of the periodic Table. What is the electron arrangement and proton number of atom Y?
5. Element R has a proton number of 11. Its atom has 6 neutrons. In which group and period can you find element R in the Periodic Table?
58
mohd faisol mansor/chemistry form 4/chapter 4
The advantage of grouping elements in the Periodic Table 1. Helps us to study the element systematically especially their physical and chemical properties. 2. Element with a same number valence electron is place in the same group because they have the same chemical properties. 3. It could be used to predict undiscovered properties. 4. To relate the characteristic of an element with atomic structure
59
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 18
GROUP 18
consist of helium, neon, argon, krypton, xenon and radon
Known as NOBLE GAS Exist as monoatomic gas.
Physical Properties of Group 18
COLOUR
SOLUBILITY
GROUP 18 NOBLE GAS ELECTRIC CONDUCTIVITY
DENSITY
MELTING & BOILING POINT
60
mohd faisol mansor/chemistry form 4/chapter 4
The inert properties of G18
All noble gas are inert which means unreactive. Noble gas are inert because the outermost occupied shell are full. This electron arrangements are very stable. Helium have 2 valence electron, this electron arrangement is called duplet electron arrangement whereas other noble gas have eight valence electron which called octet electron arrangement.
p/s:
All other element try to achieve noble gas electron arrangement to become stable.
The Physical Properties of G18
The physical properties vary down the group. physical properties vary down the group are related to atomic size. Melting and boiling point of an element increase when going down the group because the atomic sizes increase, the forces attraction (Van der Waals forces) becomes stronger. Thus more heat energy is required to overcome the forces. The strength of Van der Waals forces propotional to the size of particle
61
mohd faisol mansor/chemistry form 4/chapter 4
Uses of Noble Gas Elements [ State the element of group 18 ]
Fill light bulb
laser for repair retina, photographic flash lamps
treatment cancer
fill airships and weather balloons
Car bulb, use in bubble chamber
advertising light and television tubes
62
mohd faisol mansor/chemistry form 4/chapter 4
Exercise 1. Table below shows the electron arrangements of atoms of elements P, Q, and R.
Element
Electron Arrangement
P
2.8
Q
2.8.18.8
R
2.8.18.32.18.8
a) Arrange the element in ascending order of boiling points. Give reasons for your answer.
b) Elements P, Q, and R are chemically unreactive. Why?
2) What is the meaning of a) Duplet electron arrangement
b) Octet electron arrangement
63
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 1 Known as Alkali Metals. Have valence electron of 1.
Consist of elements such as lithium, sodium, potassium, rubidium, caesium and francium.
Physical Properties of Group 1
HARDNESS
ELECTRIC CONDUCTIVITY
APPEARANCE
GROUP 1 ALKALI METALS
DENSITY
MELTING POINT
64
mohd faisol mansor/chemistry form 4/chapter 4
Element
Atomic Size
Melting / Boiling point
Density
Hardness
Lithium Sodium Potassium Rubidium Caesium Francium
A melting point of a metal indicates the strength of its metallic bonding in its structure. Generally, the strength of metallic bonding is directly proportional to the number of valence electron per atom divided by the radius of a metal. A metallic bond can be defined as the electrostatic force between the positively charged metallic ions and the ‘sea’ of electrons. Electropositivity is the measurement of an atom to release an electron and form positive ion When going down the group, what happen to the electropositivity of the element? Why?
65
mohd faisol mansor/chemistry form 4/chapter 4
Chemical Properties of Group 1 Elements React vigorously with water to produce alkaline metal hydroxide solution and hydrogen gas, H2. 2Li (s) + 2H2O
2LiOH (aq) + H2 (g)
Burn in oxygen gas rapidly to produce solid metal oxide 4Li (s) + O2 (g)
2 Li2O (s)
Solid metal oxide dissolve in water to form alkaline metal hydroxide Li2O (s) + H2O
2LiOH (aq)
Alkaline metal burn in chlorine gas, Cl2 to form white solid metal chloride 2Na (s) + Cl2
2NaCl (aq)
Exercise : 1. Why does Group 1 element have similar chemical properties?
2. Why is paraffin oil used to store metals such as sodium and potassium?
3. Element in Group 1 has similar chemical properties but differ in reactivity. Why?
66
mohd faisol mansor/chemistry form 4/chapter 4
To investigate the chemical properties of Lithium, Sodium & Potassium 1) The reaction of alkali metals with water
2) The reaction of alkali metals with O2 gas
[ Draw the diagram ]
[ Draw the diagram ]
[ Discussion ] 1. Why are the experiments involving sodium and potassium demonstrated by your teacher and not carried out by the students?
2. Write the chemical equations for the reactions of lithium, sodium and potassium with a) Water, H2O Lithium
:
Sodium
:
Potassium
:
b) Oxygen gas, O2 Lithium
:
Sodium
:
Potassium
: 67
mohd faisol mansor/chemistry form 4/chapter 4
3. Write the chemical equations for the reactions between the products from the combustion of each alkali metal with water. Lithium : Sodium : Potassium :
Exercise 1. A student performs two experiments to study the reaction of alkali metal with water. Experiment
Metal used
Observation
1
Sodium
Sodium moves rapidly and randomly on the water surface and emits ‘hiss’ sounds.
2
Lithium
Lithium moves slowly on the water surface.
a) Write the chemical equation for the reaction between sodium and lithium with water. Lithium : Sodium : b) Between reactions of Experiment 1 and 2, which is more vigorous? Explain your answer from the point of electron arrangement.
c) Explain why sodium and lithium show similar chemical properties? d) Calculate the volume of hydrogen gas produced if 2.3 g of sodium is used. [RAM: Na, 23 ; molar volume: 24 dm3 mol-1]
68
mohd faisol mansor/chemistry form 4/chapter 4
GROUP 17
GROUP 17
GROUP 17
consist of fluorine, chlorine, bromine, iodine and astatine.
Known as HALOGENS.
Elements are poisonous.
Have valence electron of 7.
Exist as diatomic molecules.
Element
Symbol of Atom
Symbol of Molecule
Physical state at room condition
Colour
Fluorine Chlorine Bromine Iodine Astatine
Melting & Boiling Point
Density
Electric Conductivity Physical State HALOGENS Smell
69
mohd faisol mansor/chemistry form 4/chapter 4
Element
Atomic Size
Melting / Boiling point
Density
Electronegativity
Fluorine Chlorine Bromine Iodine Astatine
Electronegativity is an ability of atom to receive an electron to become negative charged ions. All halogen have seven valence electron. Their atoms always gain one electron to form an ion with a charge of –1, in order to achieve stable octet electron arrangement.
Chemical Properties of Group 17 Elements
Halogen react with water to produce two acids Cl2 + H2O
HCl
+
HOCl
Halogen react with metal to produce metal halides 2Fe (s) + 3Cl2 (g)
FeCl3 (s)
Halogen react with sodium hydroxide solution to form sodium halide and sodium halate (I) and water I2(s) + 2NaOH (aq)
NaI (aq) + NaOI (aq) + H2O (l) 70
mohd faisol mansor/chemistry form 4/chapter 4
To Investigate the Chemical Properties of Halogens [Draw the Apparatus]
SECTION A : Reaction with Water 1) Chlorine
2) Bromine
3) Iodine
SECTION B : Reaction with Iron 1) Chlorine
2) Bromine
3) Iodine
SECTION C : Reaction with Sodium Hydroxide 1) Chlorine
2) Bromine
3) Iodine
71
mohd faisol mansor/chemistry form 4/chapter 4
[Discussion] 1.
Name the products formed when chlorine, bromine, and iodine react with water. Chlorine Bromine Iodine
2.
: : :
Write the chemical equations for the reaction of chlorine, bromine and iodine with water. Chlorine Bromine Iodine
: : :
3.
What is the function of soda lime in SECTION B?
4.
Name the products formed when chlorine, bromine, and iodine react with iron. Chlorine Bromine Iodine
5.
: : :
Write the chemical equation for the reaction of chlorine, bromine, and iodine with iron. Chlorine Bromine Iodine
: : :
72
mohd faisol mansor/chemistry form 4/chapter 4
4.
Name the products formed when chlorine, bromine, and iodine react with sodium hydroxide solution. Chlorine Bromine Iodine
5.
Write the chemical equation for the reaction of chlorine, bromine, and iodine with sodium hydroxide solution. Chlorine Bromine Iodine
6.
: : :
: : :
Describe the changes in reactivity of Group 17 elements when going down the group. Explain your answer.
73
mohd faisol mansor/chemistry form 4/chapter 4
Exercise 1. Table below shows several halogen elements with their proton numbers. Halogen
Proton Number
X
9
Y
17
Z
35
a) State the group that the halogen elements belong to in the Periodic Table.
b) i) Write the electron arrangement of elements X and Y.
ii) From your answers in (b)(i), deduce the period of elements X and Y.
c) Draw the electron arrangement of element Y.
d) State the changes of properties of halogens down the group from X to Z in of: i) Atomic radius
ii) Electronegativity
iii) Melting point and boiling point 74
mohd faisol mansor/chemistry form 4/chapter 4
e) i) Iron glow brightly when reacting with element Y. Write the chemical reaction to represent this reaction.
ii) Predict the observation for the reaction between iron and element Z.
iii) Between Y and Z, which is more reactive? Explain why.
f) i) Determine the elements X, Y and Z.
ii) State the colour for each elements X, Y, and Z.
iii) Why the physical state of halogen differ when down the group?
75
mohd faisol mansor/chemistry form 4/chapter 4
Comparison & Similarities between Group 1 and Group 17
Properties Atomic Size Melting & Boiling Point Density
Reactivity
Group
Down the Group
1 17 1 17 1 17 1 17
76
mohd faisol mansor/chemistry form 4/chapter 4
Elements in a Period 3 Element
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulphur
Chlorine
Argon
Symbol Proton Number Electron Arrangement Metal Properties Physical State [RC] Atomic Radius Electronegativity Property of the oxide
The proton number ____________ by one unit. All atom of the element have __________ shells occupied by electron. The number of valence electron ____________ from 1 to 8. All element exist as __________ except chlorine and argon. The atomic radius of element ________________. The electronegativity of element ______________. The oxides of element in Period 3 change from basic to acidic properties, therefore the metallic properties decrease across the period. On the other hand non-metallic properties of the elements increase.
Note: the atomic radius ______________ and electro negativity ______________ due to the increasing nuclei attraction on the valence electrons. (nuclei attraction force increase with the increase of proton number)
77
mohd faisol mansor/chemistry form 4/chapter 4
Transition Elements Transition elements are elements from Group 3 to Group 12
All the elements are metals, usually solids with shiny surfaces, ductile, malleable and have tensile strength. Have high melting and boiling point as well as high density. Good conductors of heat and electricity. Three special characteristics of transition element Show different oxidation number in their compound. Form coloured ions or compound.
Act as catalysts.
78
Related Documents 3h463d
Chemistry Module Form 4 (4) 104e5b
December 2019 92
Chemistry Form 4 Chapter 4 1d5t4t
October 2019 149
Chemistry Form 4 Chapter 4 1d5t4t
October 2019 97
Nilam Publication Module Chemistry Form 4 (answer) 5t4f49
December 2020 0
Spm Form 4 Chemistry Chap 4 Exercises 524b1h
November 2021 0
Notes Chemistry Form 4 Chapter 4 1 5qi5f
October 2019 142More Documents from "mohd faisol" 48b17
Chemistry Module Form 4 (4) 104e5b
December 2019 92
Proposal Hijab 2 335r1
December 2021 0
Laporan Kegiatan Promkes-phbs 6w126t
April 2020 25
Lirik Lagu Vierra Bersamamu Lyrics 6j6p5n
December 2019 101
Sap Discharge Planning m4932
April 2020 31