Everything in the universe is composed of basic elements, and at their smallest level, these elements are atoms.
There are a total of 118 elements in the modern periodic table out of which 98 are found in nature rest are chemically synthesized in laboratories. An atom of any element is composed of electrons, protons, and neutrons and possesses a different property from the other.
Table of Contents
118 Elements and their Symbols and Atomic Numbers
The Tabulated view of all 118 elements and their symbols along with their atomic number, element name, atomic mass, and number of protons and neutrons is described below:
Atomic Number
Symbol
Element Name
Atomic Mass
Number of Protons
Number of Neutrons
1
H
Hydrogen
1.008
1
0
2
He
Helium
4.0026
2
2
3
Li
Lithium
6.94
3
4
4
Be
Beryllium
9.0122
4
5
5
B
Boron
10.81
5
6
6
C
Carbon
12.011
6
6
7
N
Nitrogen
14.007
7
7
8
O
Oxygen
15.999
8
8
9
F
Fluorine
18.998
9
10
10
Ne
Neon
20.180
10
10
11
Na
Sodium
22.990
11
12
12
Mg
Magnesium
24.305
12
12
13
Al
Aluminum
26.982
13
14
14
Si
Silicon
28.095
14
14
15
P
Phosphorus
30.974
15
16
16
S
Sulphur
32.06
16
16
17
Cl
Chlorine
35.45
17
18
18
Ar
Argon
39.948
18
22
19
K
Potassium
39.098
19
20
20
Ca
Calcium
40.078
20
20
21
Sc
Scandium
44.956
21
24
22
Ti
Titanium
47.867
22
26
23
V
Vanadium
50.942
23
28
24
Cr
Chromium
51.996
24
28
25
Mn
Manganese
54.938
25
30
26
Fe
Iron
55.845
26
30
27
Co
Cobalt
58.933
27
32
28
Ni
Nickle
58.693
28
31
29
Cu
Copper
63.546
29
35
30
Zn
Zinc
65.38
30
35
31
Ga
Gallium
69.723
31
39
32
Ge
Germanium
72.630
32
41
33
As
Arsenic
74.922
33
42
34
Se
Selenium
78.971
34
45
35
Br
Bromine
79.904
35
45
36
Kr
Krypton
83.798
36
48
37
Rb
Rubidium
85.468
37
48
38
Sr
Strontium
87.62
38
50
39
Y
Yttrium
88.906
39
50
40
Zr
Zirconium
91.224
40
51
41
Nb
Niobium
92.906
41
52
42
Mo
Molybdenum
95.95
42
53
43
Tc
Technetium
98
43
55
44
Ru
Ruthenium
101.07
44
57
45
Rh
Rhodium
102.9055
45
58
46
Pd
Palladium
106.42
46
60
47
Ag
Silver
107.8682
47
61
48
Cd
Cadmium
112.411
48
64
49
In
Indium
114.818
49
66
50
Sn
Tin
118.71
50
69
51
Sb
Antimony
121.76
51
71
52
Te
Tellurium
127.6
52
76
53
I
Iodine
126.9045
53
74
54
Xe
Xenon
131.293
54
77
55
Cs
Cesium
132.9055
55
78
56
Ba
Barium
137.327
56
81
57
La
Lanthanum
138.9055
57
82
58
Ce
Cerium
140.116
58
82
59
Pr
Praseodymium
140.9077
59
82
60
Nd
Neodymium
144.24
60
84
61
Pm
Promethium
145
61
84
62
Sm
Samarium
150.36
62
88
63
Eu
Europium
151.964
63
89
64
Gd
Gadolinium
157.25
64
93
65
Tb
Terbium
158.9253
65
94
66
Dy
Dysprosium
162.5
66
97
67
Ho
Holmium
164.9303
67
98
68
Er
Erbium
167.259
68
99
69
Tm
Thulium
168.9342
69
100
70
Yb
Ytterbium
173.04
70
103
71
Lu
Lutetium
174.967
71
104
72
Hf
Hafnium
178.49
72
106
73
Ta
Tantalum
180.9479
73
108
74
W
Tungsten
183.84
74
110
75
Re
Rhenium
186.207
75
111
76
Os
Osmium
190.23
76
114
77
Ir
Iridium
196.9665
77
115
78
Pt
Platinum
192.217
78
117
79
Au
Gold
195.078
79
118
80
Hg
Mercury
200.59
80
121
81
Tl
Thallium
204.3833
81
123
82
Pb
Lead
207.2
82
125
83
Bi
Bismuth
208.9804
83
126
84
Po
Polonium
209
84
125
85
At
Astatine
210
85
125
86
Rn
Radon
222
86
136
87
Fr
Francium
223
87
136
88
Ra
Radium
226
88
138
89
Ac
Actinium
227
89
138
90
Th
Thorium
232.0381
90
142
91
P
Protactinium
231.0359
91
140
92
U
Uranium
238.0289
92
146
93
Np
Neptunium
237
93
144
94
Pu
Plutonium
244
94
150
95
Am
Americium
243
95
148
96
Cm
Curium
247
96
151
97
Bk
Berkelium
247
97
150
98
Cf
Californium
251
98
153
99
Es
Einsteinium
252
99
153
100
Fm
Fermium
257
100
157
101
Md
Mendelevium
258
101
157
102
No
Nobelium
259
102
157
103
Lr
Lawrencium
262
103
159
104
Rf
Rutherfordium
261
104
163
105
Db
Dubnium
262
105
163
106
Sg
Seaborgium
266
106
165
107
Bh
Bohrium
264
107
163
108
Hs
Hassium
277
108
169
109
Mt
Meitnerium
268
109
167
110
Ds
Darmstadtium
261.9
110
171
111
Rg
Roentgenium
271.8
111
169
112
Cn
Copernicium
285
112
173
113
Nh
Nihonium
286
113
171
114
Fl
Flerovium
289
114
175
115
Mc
Moscovium
290.196
115
173
116
Lv
Livermorium
293
116
177
117
Ts
Tennessee
294
117
177
118
Og
Oganesson
294
118
176
What is a Periodic Table?
Initially, the number of elements was small, and the knowledge of the physical and chemical properties of these elements was also limited, but in the early 19th century the discovery of new elements and growth in the knowledge of physical and chemical properties of elements had become hard for the scholars to remember the behavior and properties of all the elements.
Thus a need for a systematic arrangement of elements was there, where the elements are stacked based on their properties, physical properties such as melting point, boiling point, and chemical properties such as electronegativity, valence electron, etc and thereafter the periodic table was introduced.
A periodic table is a tabular arrangement of chemical elements in the increasing order of the atomic number which is the number of protons in their nucleus. The arrangement of the elements thus formed shows a recurring pattern in their properties known as “periodic laws”.
118 Elements in Periodic Table
Following illustration represents all 118 elements in periodic table:
118 Elements and Their Symbols in Periodic Table
Atomic Number
The nucleus of each element consists of a different number of protons and neutrons, the number of protons in each nucleus of each element is found to be unique, so it became the base for arranging the elements in increasing order of their nucleus protons. Number of protons in the nucleus also determines the electronegativity and other factors of the elements.
The number of protons in the nucleus of each element is unique and it is referred as Atomic Number. It is the fundamental property of any element and is denoted by the symbol “Z”.
The elements in the periodic table are arranged in the increasing order of their atomic number, for example, H (Hydrogen) has atomic number 1, He (Helium) has atomic number 2, and so on.
Mass Number
The individual mass of an atom of an element is very minute and also difficult to measure. The mass of an electron is approximately 9.10938356 × 10-28 g, the mass of the proton is 1.6726219 × 10-24 g and the mass of neutron is 1.675 × 10-24 g. Since the mass of an atom is merely and remembering the exact mass was a tough job, so the mass number was introduced which is the total number of protons and neutrons in its nucleus.
The Mass Number of an atom is the total number of protons and neutrons in its nucleus. It is represented by the letter A. The mass number of an atom of an element gives an approximate measure of the total mass of the atom. It is expressed in atomic mass units (u) or unified atomic mass units (AMU).
Where 1 AMU = 1.67377 × 10 -24 g
Symbols Of Elements
Each element is assigned some unique symbol which is usually an English letter (or two). These symbols are used universally to represent and uniquely identify that particular element and are also used for scientific purposes to represents elements in a clean and concise manner. Thus we can say that,
Symbols of element are shorthand to uniquely identify and represent that element.
The symbols of the elements are widely used to represent the elements in chemical formulas, equations, and other representations of chemical reactions.
How Symbols are Derived?
The symbols of elements are derived from the name of the element in English or another language eg. the symbol of Hydrogen is H, that comes from its name in English. It is important to note that the symbol of an element is usually a capital letter and when it contains two letters, the second letter is smaller letter. However, in cases where the first two letters are already taken, or for historical reasons, the symbol may not directly correspond to the element’s name (e.g., Fe for iron comes from its Latin word “ferrum”).
118 Elements and Their Symbols: FAQs
1: Who is the Father of the Periodic Table?
Mendeleev is often credited as the father of periodic table.
2: What is an Element?
An element is a substance that consists of only one type of atom, and each element is characterized by the number of protons found in the nucleus of its atoms.
3: What is an Atom?
An atom is the basic building block of matter and it is made up of protons, neutrons, and electrons. An atom is the smallest unit of an element that is responsible for the chemical properties of that element.
4: What are Chemical Symbols and their Significance?
Chemical symbols are shorthand representations of an element. These symbols consist of one or two letters often derived from the name of the element. They have a significant role in communicating information about elements in a concise and standardized manner.
5. What has only 1 atom?
Some elements consist of only 1 atom and they are known as monoatomic. For example, Helium, and Potassium
6: What are Isotopes of Hydrogen?
Hydrogen has three isotopes namely Protium (H11 ), Deuterium(H12), and, Tritium(H11).
7: What is the Connection between the Atomic Number and the Number of Protons?
The atomic number of an element is equal to the number of protons in the atom of the element.
8: Which is the most Reactive Metal?
Francium(Fr) is considered the most reactive metal of all.
9: Which Metal Remains Liquid at Room Temperature?
Mercury is the only metal which remains in a liquid state at room temperature.
Neeraj Anand, Param Anand
Er. Neeraj K.Anand is a freelance mentor and writer who specializes in Engineering & Science subjects. Neeraj Anand received a B.Tech degree in Electronics and Communication Engineering from N.I.T Warangal & M.Tech Post Graduation from IETE, New Delhi. He has over 30 years of teaching experience and serves as the Head of Department of ANAND CLASSES. He concentrated all his energy and experiences in academics and subsequently grew up as one of the best mentors in the country for students aspiring for success in competitive examinations.
In parallel, he started a Technical Publication "ANAND TECHNICAL PUBLISHERS" in 2002 and Educational Newspaper "NATIONAL EDUCATION NEWS" in 2014 at Jalandhar. Now he is a Director of leading publication "ANAND TECHNICAL PUBLISHERS", "ANAND CLASSES" and "NATIONAL EDUCATION NEWS".
He has published more than hundred books in the field of Physics, Mathematics, Computers and Information Technology. Besides this he has written many books to help students prepare for IIT-JEE and AIPMT entrance exams. He is an executive member of the IEEE (Institute of Electrical & Electronics Engineers. USA) and honorary member of many Indian scientific societies such as Institution of Electronics & Telecommunication Engineers, Aeronautical Society of India, Bioinformatics Institute of India, Institution of Engineers. He has got award from American Biographical Institute Board of International Research in the year 2005.
CBSE Class 11 Chemistry Syllabus is a vast which needs a clear understanding of the concepts and topics. Knowing CBSE Class 11 Chemistry syllabus helps students to understand the course structure of Chemistry.
Unit-wise CBSE Class 11 Syllabus for Chemistry
Below is a list of detailed information on each unit for Class 11 Students.
UNIT I – Some Basic Concepts of Chemistry
General Introduction: Importance and scope of Chemistry.
Nature of matter, laws of chemical combination, Dalton’s atomic theory: concept of elements, atoms and molecules.
Atomic and molecular masses, mole concept and molar mass, percentage composition, empirical and molecular formula, chemical reactions, stoichiometry and calculations based on stoichiometry.
UNIT II – Structure of Atom
Discovery of Electron, Proton and Neutron, atomic number, isotopes and isobars. Thomson’s model and its limitations. Rutherford’s model and its limitations, Bohr’s model and its limitations, concept of shells and subshells, dual nature of matter and light, de Broglie’s relationship, Heisenberg uncertainty principle, concept of orbitals, quantum numbers, shapes of s, p and d orbitals, rules for filling electrons in orbitals – Aufbau principle, Pauli’s exclusion principle and Hund’s rule, electronic configuration of atoms, stability of half-filled and completely filled orbitals.
UNIT III – Classification of Elements and Periodicity in Properties
Significance of classification, brief history of the development of periodic table, modern periodic law and the present form of periodic table, periodic trends in properties of elements -atomic radii, ionic radii, inert gas radii, Ionization enthalpy, electron gain enthalpy, electronegativity, valency. Nomenclature of elements with atomic number greater than 100.
UNIT IV – Chemical Bonding and Molecular Structure
Valence electrons, ionic bond, covalent bond, bond parameters, Lewis structure, polar character of covalent bond, covalent character of ionic bond, valence bond theory, resonance, geometry of covalent molecules, VSEPR theory, concept of hybridization, involving s, p and d orbitals and shapes of some simple molecules, molecular orbital theory of homonuclear diatomic molecules(qualitative idea only), Hydrogen bond.
UNIT V – Chemical Thermodynamics
Concepts of System and types of systems, surroundings, work, heat, energy, extensive and intensive properties, state functions. First law of thermodynamics – internal energy and enthalpy, measurement of U and H, Hess’s law of constant heat summation, enthalpy of bond dissociation, combustion, formation, atomization, sublimation, phase transition, ionization, solution and dilution. Second law of Thermodynamics (brief introduction) Introduction of entropy as a state function, Gibb’s energy change for spontaneous and nonspontaneous processes. Third law of thermodynamics (brief introduction).
UNIT VI – Equilibrium
Equilibrium in physical and chemical processes, dynamic nature of equilibrium, law of mass action, equilibrium constant, factors affecting equilibrium – Le Chatelier’s principle, ionic equilibrium- ionization of acids and bases, strong and weak electrolytes, degree of ionization, ionization of poly basic acids, acid strength, concept of pH, hydrolysis of salts (elementary idea), buffer solution, Henderson Equation, solubility product, common ion effect (with illustrative examples).
UNIT VII – Redox Reactions
Concept of oxidation and reduction, redox reactions, oxidation number, balancing redox reactions, in terms of loss and gain of electrons and change in oxidation number, applications of redox reactions.
UNIT VIII – Organic Chemistry: Some basic Principles and Techniques
General introduction, classification and IUPAC nomenclature of organic compounds. Electronic displacements in a covalent bond: inductive effect, electromeric effect, resonance and hyper conjugation. Homolytic and heterolytic fission of a covalent bond: free radicals, carbocations, carbanions, electrophiles and nucleophiles, types of organic reactions.
UNIT IX – Hydrocarbons
Classification of Hydrocarbons Aliphatic Hydrocarbons: Alkanes – Nomenclature, isomerism, conformation (ethane only), physical properties, chemical reactions. Alkenes – Nomenclature, structure of double bond (ethene), geometrical isomerism, physical properties, methods of preparation, chemical reactions: addition of hydrogen, halogen, water, hydrogen halides (Markovnikov’s addition and peroxide effect), ozonolysis, oxidation, mechanism of electrophilic addition. Alkynes – Nomenclature, structure of triple bond (ethyne), physical properties, methods of preparation, chemical reactions: acidic character of alkynes, addition reaction of – hydrogen, halogens, hydrogen halides and water.
Aromatic Hydrocarbons:
Introduction, IUPAC nomenclature, benzene: resonance, aromaticity, chemical properties: mechanism of electrophilic substitution. Nitration, sulphonation, halogenation, Friedel Craft’s alkylation and acylation, directive influence of functional group in monosubstituted benzene. Carcinogenicity and toxicity.
To know the CBSE Syllabus for all the classes from 1 to 12, visit the Syllabus page of CBSE. Meanwhile, to get the Practical Syllabus of Class 11 Chemistry, read on to find out more about the syllabus and related information in this page.
CBSE Class 11 Chemistry Practical Syllabus with Marking Scheme
In Chemistry subject, practical also plays a vital role in improving their academic scores in the subject. The overall weightage of Chemistry practical mentioned in the CBSE Class 11 Chemistry syllabus is 30 marks. So, students must try their best to score well in practicals along with theory. It will help in increasing their overall academic score.
CBSE Class 11 Chemistry Practical Syllabus
The experiments will be conducted under the supervision of subject teacher. CBSE Chemistry Practicals is for 30 marks. This contribute to the overall practical marks for the subject.
The table below consists of evaluation scheme of practical exams.
Evaluation Scheme
Marks
Volumetric Analysis
08
Salt Analysis
08
Content Based Experiment
06
Project Work
04
Class record and viva
04
Total
30
CBSE Syllabus for Class 11 Chemistry Practical
Micro-chemical methods are available for several of the practical experiments. Wherever possible such techniques should be used.
A. Basic Laboratory Techniques 1. Cutting glass tube and glass rod 2. Bending a glass tube 3. Drawing out a glass jet 4. Boring a cork
B. Characterization and Purification of Chemical Substances 1. Determination of melting point of an organic compound. 2. Determination of boiling point of an organic compound. 3. Crystallization of impure sample of any one of the following: Alum, Copper Sulphate, Benzoic Acid.
C. Experiments based on pH
1. Any one of the following experiments:
Determination of pH of some solutions obtained from fruit juices, solution of known and varied concentrations of acids, bases and salts using pH paper or universal indicator.
Comparing the pH of solutions of strong and weak acids of same concentration.
Study the pH change in the titration of a strong base using universal indicator.
2. Study the pH change by common-ion in case of weak acids and weak bases.
D. Chemical Equilibrium One of the following experiments:
1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of either of the ions. 2. Study the shift in equilibrium between [Co(H2O)6] 2+ and chloride ions by changing the concentration of either of the ions.
E. Quantitative Estimation i. Using a mechanical balance/electronic balance. ii. Preparation of standard solution of Oxalic acid. iii. Determination of strength of a given solution of Sodium hydroxide by titrating it against standard solution of Oxalic acid. iv. Preparation of standard solution of Sodium carbonate. v. Determination of strength of a given solution of hydrochloric acid by titrating it against standard Sodium Carbonatesolution.
F. Qualitative Analysis 1) Determination of one anion and one cation in a given salt Cations‐ Pb2+, Cu2+, As3+, Al3+, Fe3+, Mn2+, Ni2+, Zn2+, Co2+, Ca2+, Sr2+, Ba2+, Mg2+, NH4+ Anions – (CO3)2‐ , S2‐, NO2‐ , SO32‐, SO2‐ , NO ‐ , Cl‐ , Br‐, I‐, PO43‐ , C2O2‐ ,CH3COO‐ (Note: Insoluble salts excluded)
2) Detection of ‐ Nitrogen, Sulphur, Chlorine in organic compounds.
G) PROJECTS Scientific investigations involving laboratory testing and collecting information from other sources.
A few suggested projects are as follows:
Checking the bacterial contamination in drinking water by testing sulphide ion
Study of the methods of purification of water.
Testing the hardness, presence of Iron, Fluoride, Chloride, etc., depending upon the regional variation in drinking water and study of causes of presence of these ions above permissible limit (if any).
Investigation of the foaming capacity of different washing soaps and the effect of addition of Sodium carbonate on it.
Study the acidity of different samples of tea leaves.
Determination of the rate of evaporation of different liquids Study the effect of acids and bases on the tensile strength of fibres.
Study of acidity of fruit and vegetable juices.
Note: Any other investigatory project, which involves about 10 periods of work, can be chosen with theapproval of the teacher.
Practical Examination for Visually Impaired Students of Class 11
Below is a list of practicals for the visually impaired students.
A. List of apparatus for identification for assessment in practicals (All experiments) Beaker, tripod stand, wire gauze, glass rod, funnel, filter paper, Bunsen burner, test tube, test tube stand, dropper, test tube holder, ignition tube, china dish, tongs, standard flask, pipette, burette, conical flask, clamp stand, dropper, wash bottle • Odour detection in qualitative analysis • Procedure/Setup of the apparatus
B. List of Experiments A. Characterization and Purification of Chemical Substances 1. Crystallization of an impure sample of any one of the following: copper sulphate, benzoic acid B. Experiments based on pH 1. Determination of pH of some solutions obtained from fruit juices, solutions of known and varied concentrations of acids, bases and salts using pH paper 2. Comparing the pH of solutions of strong and weak acids of same concentration.
C. Chemical Equilibrium 1. Study the shift in equilibrium between ferric ions and thiocyanate ions by increasing/decreasing the concentration of eitherions. 2. Study the shift in equilibrium between [Co(H2O)6]2+ and chloride ions by changing the concentration of either of the ions.
D. Quantitative estimation 1. Preparation of standard solution of oxalic acid. 2. Determination of molarity of a given solution of sodium hydroxide by titrating it against standard solution of oxalic acid.
E. Qualitative Analysis 1. Determination of one anion and one cation in a given salt 2. Cations – NH+4 Anions – (CO3)2-, S2-, (SO3)2-, Cl-, CH3COO- (Note: insoluble salts excluded) 3. Detection of Nitrogen in the given organic compound. 4. Detection of Halogen in the given organic compound.
Note: The above practicals may be carried out in an experiential manner rather than recording observations.
We hope students must have found this information on CBSE Syllabus useful for their studying Chemistry. Learn Maths & Science in interactive and fun loving ways with ANAND CLASSES (A School Of Competitions) App/Tablet.
Frequently Asked Questions on CBSE Class 11 Chemistry Syllabus
Q1
How many units are in the CBSE Class 11 Chemistry Syllabus?
There are 9 units in the CBSE Class 11 Chemistry Syllabus. Students can access various study materials for the chapters mentioned in this article for free at ANAND CLASSES (A School Of Competitions).
Q2
What is the total marks for practicals examination as per the CBSE Class 11 Chemistry Syllabus?
The total marks for the practicals as per the CBSE Class 11 Chemistry Syllabus is 30. It includes volumetric analysis, content-based experiment, salt analysis, class record, project work and viva.
Q3
Which chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry?
The organic chemistry chapter carries more weightage as per the CBSE Syllabus for Class 11 Chemistry.
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