118 Elements and Their Symbols and Atomic Numbers

118 Elements and Their Symbols and Atomic Numbers

Edited By Team Careers360 | Updated on Jul 02, 2025 04:23 PM IST

In the periodic table, there are 118 elements are each of which has a unique name, symbol, and atomic number. Arrangements of elements in the periodic table depend on their atomic number and properties. These elements represent the wide range of Metals, Non-metals, and Noble Gases. The first element, or the element whose atomic number is 1, is Hydrogen, represented by ‘H’, and the last element, whose atomic number is 118, is Oganesson, represented by the symbol ‘Og’. Most of the symbols are similar to the names of the elements, but there are certain symbols of objects with Latin roots. Its example is the lead described by Pb , which is derived from its Latin name "Plumbum". One such example would be the 'Fe' symbol used to represent the metal and could be associated with the Latin word iron, "Ferrum".

This Story also Contains
  1. Atomic number
  2. What does the symbol of an element Mean?
  3. Chemistry periodic table/Chemical Chart:
  4. Some Solved Examples
118 Elements and Their Symbols and Atomic Numbers
118 Elements and Their Symbols and Atomic Numbers

Atomic number

118 elements and their symbols and atomic numbers are arranged from left to right and top to bottom in order of increasing atomic number. In the modern periodic table, the elements' names and symbols are listed in order of increasing atomic number. Order generally coincides with increasing atomic mass. The rows are called periods. In a periodic table arranged in order of increasing atomic number, elements and symbols having similar chemical properties naturally line up in the same group.

The current table, today, contains a total of as element 118 elements and their symbols and atomic numbers. Since the names of the elements can be long and complex to use, they are indicated by using a symbol. Each item has a unique symbol.

What does the symbol of an element Mean?

A sign or symbol is a note usually consisting of one or two letters that are used to represent a chemical object. There are also 3-character symbols. These are things that have just been merged and so-called for a while. There are some rules for marking. The first letter of the mark is usually capitalized, while the second (or third) letter is usually written in small letters. Eg. - Ca for Calcium, He for Helium, etc. If an item mark contains only one letter, it is always capitalized.

Eg. -Nitrogen (N), Oxygen (O), etc.

Symbols are often used to represent objects in a timeline. The chemical formula and proportions must also be used for those properties.

The following table provides a list of 118 elements and their symbols, atomic numbers, and the number of atoms.

Periodic table of elements with names and their symbols(List of elements)

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Chemistry periodic table/Chemical Chart:

Name of the chemical element symbols

Name of the Element

Symbol of the Element

Atomic Number

Hydrogen

H

1

Helium

He

2

Lithium

Li

3

Beryllium

Be

4

Boron

B

5

Carbon

C

6

Nitrogen

N

7

Oxygen

O

8

Fluorine

F

9

Neon

Ne

10

Sodium

Na

11

Magnesium

Mg

12

Aluminium

Al

13

Silicon

Si

14

Phosphorus

P

15

Sulfur

S

16

Chlorine

Cl

17

Argon

Ar

18

Potassium

K

19

Calcium

Ca

20

Scandium

Sc

21

Titanium

Ti

22

Vanadium

V

23

Chromium

Cr

24

Manganese

Mn

25

Iron

Fe

26

Cobalt

Co

27

Nickel

Ni

28

Copper

Cu

29

Zinc

Zn

30

Gallium

Ga

31

Germanium

Ge

32

Arsenic

As

33

Selenium

Se

34

Bromine

Br

35

Krypton

Kr

36

Rubidium

Rb

37

Strontium

Sr

38

Yttrium

Y

39

Zirconium

Zr

40

Niobium

Nb

41

Molybdenum

Mo

42

Technetium

Tc

43

Ruthenium

Ru

44

Rhodium

Rh

45

Palladium

Pd

46

Silver

Ag

47

Cadmium

Cd

48

Indium

In

49

Tin

Sn

50

Antimony

Sb

51

Tellurium

Te

52

Iodine

I

53

Xenon

Xe

54

Cesium

Cs

55

Barium

Ba

56

Lanthanum

La

57

Cerium

Ce

58

Praseodymium

Pr

59

Neodymium

Nd

60

Promethium

Pm

61

Samarium

Sm

62

Europium

Eu

63

Gadolinium

Gd

64

Terbium

Tb

65

Dysprosium

Dy

66

Holmium

Ho

67

Erbium

Er

68

Thulium

Tm

69

Ytterbium

Yb

70

Lutetium

Lu

71

Hafnium

Hf

72

Tantalum

Ta

73

Tungsten

W

74

Rhenium

Re

75

Osmium

Os

76

Iridium

Ir

77

Platinum

Pt

78

Gold

Au

79

Mercury

Hg

80

Thallium

Tl

81

Lead

Pb

82

Bismuth

Bi

83

Polonium

Po

84

Astatine

At

85

Radon

Rn

86

Francium

Fr

87

Radium

Ra

88

Actinium

Ac

89

Thorium

Th

90

Protactinium

Pa

91

Uranium

U

92

Neptunium

Np

93

Plutonium

Pu

94

Americium

Am

95

Curium

Cm

96

Berkelium

Bk

97

Californium

Cf

98

Einsteinium

Es

99

Fermium

Fm

100

Mendelevium

Md

101

Nobelium

No

102

Lawrencium

Lr

103

Rutherfordium

Rf

104

Dubnium

Db

105

Seaborgium

Sg

106

Bohrium

Bh

107

Hassium

Hs

108

Meitnerium

Mt

109

Darmstadtium

Ds

110

Roentgenium

Rg

111

Copernicium

Cn

112

Nihonium

Nh

113

Flerovium

Fl

114

Moscovium

Mc

115

Livermorium

Lv

116

Tennessine

Ts

117

Oganesson

Og

118

Some Solved Examples

Example.1 What is the symbol of silver?

1) Si

2) Ar

3) (correct)Ag

4) Sb

Solution

The symbol of silver is Ag derived from the Latin word Argentum.

Hence, the answer is the option (4).

Example.2 Which of the following represents elements in increasing order of their atomic size?

1) I, Br, Cl

2) N, O, F

3) (correct)Be, Mg, Ca

4) Se, S, O

Solution

As we have learned

Vander Waals Radius - It represents the overall size of the atom which includes its valence shell in a non-bonded situation. It is half the distance between two similar atoms in separate molecules in a solid.Vanderwaals radius > metallic radius > covalent radius. Atomic size increases as we move down in a group

Hence, the answer is the option (3).

Example.3 Which of the following has the largest size

1) (correct)Al

2) Al+

3) Al+2

4) Al+3

Solution

With successive ionisations, the size of the species decreases. This is due to an increase in the effective nuclear charge which tends to hold the valence electrons more tightly thus leading to a reduction in the size.

Thus, the correct order of size is Al>Al+>Al2+>Al3+.

Hence, the answer is the option (1).

Example.4 Mendeleev’s periodic table is based on:

1) Atomic number

2) (correct)Atomic weight

3) Ionization enthalpy

4) None of the above

Solution

Mendeleev arranged the elements in horizontal rows and vertical columns in his table in order of their increasing atomic weights. In this way, elements with similar properties occupied the same vertical column.

Hence, the answer is the option (2).

Example 5: The element that does not belong to the same period of the remaining elements (modern periodic table) is:

(1) Palladium

(2) Iridium

(3) Osmium

(4) Platinum

Solution:

Palladium $\Rightarrow 5^{\text {th }}$ period
Iridium, Osmium, Platinum $\Rightarrow 6^{\text {th }}$ Period

Hence, the correct answer is option (1).

Also, check-

Frequently Asked Questions (FAQs)

1. How many elements are there in the periodic table?

There are 118 elements in the periodic table. The first element of the periodic table is Hydrogen, and the last element is Oganesson.  

2. Explain, what is the atomic number?

The atomic number is the number of protons present in the nucleus of the atom. The number of protons is unique for every element means no two different elements have the same number of protons in their nucleus.  

3. Why symbols of some elements not match their names?

Symbols of some elements are derived from their Greek names. For example, the Latin name of gold is ‘aurum’, that why the symbol of gold is ‘Au’. In the same way, the symbol of sodium is ‘Na’ because it is derived from its Latin name ‘natrium’.  

4. Are all these elements found in nature, or are some man-made?

There are 118 elements in the periodic table, out of which many elements occur naturally, like Oxygen, carbon, iron, etc, while elements with high atomic numbers, like those whose atomic number is greater than 92, are synthesized in laboratories and nuclear reactors.

5. Why are noble gases unique?

Noble gases like Helium, Neon, Argon, Krypton, Xenon, and Radon are generally inert, which means they do not react easily with other elements. This is due to their fully valence electron shells, which make them stable.    

6. What determines an element's atomic number, and why is it important?
An element's atomic number is determined by the number of protons in its nucleus. It's crucial because it defines the element's identity and determines its position in the periodic table. Elements with different atomic numbers are different elements, regardless of their isotopes or ionic forms.
7. How do atomic numbers relate to an element's electron configuration?
The atomic number determines the number of electrons in a neutral atom of that element. This, in turn, dictates the element's electron configuration, which is crucial in determining its chemical properties and behavior.
8. What's the relationship between an element's atomic number and its mass number?
The atomic number is the number of protons, while the mass number is the total number of protons and neutrons. The difference between these numbers gives the number of neutrons. This relationship is crucial for understanding isotopes.
9. How do atomic numbers relate to the concept of isotopes?
Isotopes of an element have the same atomic number (same number of protons) but different mass numbers (different numbers of neutrons). This means isotopes have identical chemical properties but can have different physical properties, like radioactivity.
10. What's the significance of noble gases in terms of their atomic numbers and electron configurations?
Noble gases (atomic numbers 2, 10, 18, 36, 54, 86) have full outer electron shells, making them extremely stable and unreactive. Their atomic numbers correspond to complete electron shell fillings, which is key to understanding electron configuration patterns.
11. How does the arrangement of elements in the periodic table relate to their atomic numbers?
Elements in the periodic table are arranged in order of increasing atomic number. This arrangement reveals periodic trends in element properties, as elements in the same column (group) have similar electron configurations and chemical behaviors.
12. What's the significance of element 118, and why is it special?
Element 118, Oganesson, is currently the heaviest known element and the last one in the 7th period of the periodic table. It's significant because it completes the p-block of the periodic table and is the last element that can be placed using the current table structure.
13. How does knowing an element's symbol and atomic number help in understanding its properties?
The symbol quickly identifies the element, while the atomic number provides information about its structure (number of protons and electrons). Together, they allow chemists to predict the element's behavior, its position in the periodic table, and its relationships with other elements.
14. Why are the lanthanides and actinides separated from the main periodic table?
Lanthanides (atomic numbers 57-71) and actinides (89-103) are placed separately for convenience, as including them in the main table would make it too wide. They have similar properties within each series due to their f-orbital electron configurations.
15. How do transition metals differ from main group elements in terms of their symbols and atomic numbers?
Transition metals and main group elements don't differ in how their symbols and atomic numbers are assigned. However, transition metals, located in the d-block, have atomic numbers 21-30, 39-48, 57-80, and 89-112, and often use electrons from multiple shells in bonding.
16. Why do elements have symbols, and how are they determined?
Elements have symbols as shorthand representations for easier communication in chemistry. They are typically derived from the element's name in English or other languages, often using the first one or two letters. For example, 'H' for Hydrogen, 'He' for Helium, and 'Na' (from Latin 'Natrium') for Sodium.
17. Why do some elements have symbols that don't seem to match their names?
Some elements have symbols derived from their Latin or Greek names, or historical names. For instance, 'Au' for Gold (from Latin 'Aurum'), 'K' for Potassium (from Latin 'Kalium'), and 'W' for Tungsten (from German 'Wolfram').
18. Why are some elements represented by single-letter symbols while others have two letters?
Single-letter symbols are used for the first 26 elements discovered or commonly known. Two-letter symbols are used for subsequent elements to avoid duplication. The first letter is always capitalized, while the second is lowercase.
19. How are new elements named and given symbols?
New elements are typically named by their discoverers, subject to approval by the International Union of Pure and Applied Chemistry (IUPAC). Temporary systematic element names and symbols based on their atomic numbers are used until an official name is approved.
20. How do atomic numbers relate to the concept of valence electrons?
Atomic numbers determine the total number of electrons, which dictates the electron configuration. Valence electrons, the outermost electrons involved in bonding, can often be predicted from an element's group number in the periodic table.
21. How do atomic numbers help in predicting an element's reactivity?
Atomic numbers determine electron configurations, which in turn influence reactivity. Elements with similar outer electron configurations (same group) tend to have similar reactivities. For example, alkali metals (Group 1) are highly reactive due to their single outer electron.
22. Why are hydrogen and helium placed separately from other elements with similar outer electron configurations?
Hydrogen (atomic number 1) is placed alone because it behaves differently from other elements. Helium (atomic number 2) is placed with noble gases due to its full outer shell, despite having a different electron configuration from other noble gases.
23. What's the significance of the atomic number 82 (lead) in terms of nuclear stability?
Lead-82 is the heaviest stable element. Elements with higher atomic numbers are all radioactive. This relates to the concept of nuclear stability and the neutron-to-proton ratio needed for stable nuclei.
24. How do atomic numbers help in understanding the periodic law?
The periodic law states that element properties are periodic functions of their atomic numbers. This means elements with similar properties appear at regular intervals when arranged by atomic number, forming the basis of the periodic table's structure.
25. Why do some elements have multiple oxidation states, and how does this relate to their atomic numbers?
Multiple oxidation states often occur in elements with partially filled d or f orbitals. The atomic number determines the electron configuration, which in turn influences the possible oxidation states. Transition metals, with their variable d-orbital occupancy, often exhibit multiple oxidation states.
26. How do atomic numbers relate to the concept of effective nuclear charge?
Atomic number determines the nuclear charge. Effective nuclear charge is the net positive charge experienced by an electron, considering the shielding effect of inner electrons. It generally increases across a period and decreases down a group.
27. What's the relationship between an element's atomic number and its electronegativity?
Electronegativity generally increases with atomic number across a period (due to increasing effective nuclear charge) and decreases down a group (due to increasing atomic radius). This trend is directly related to the electron configuration determined by the atomic number.
28. How do atomic numbers help in understanding the concept of isoelectronic species?
Isoelectronic species have the same number of electrons but different atomic numbers. Understanding atomic numbers helps identify such species, as the number of electrons in an ion can be calculated by subtracting (for cations) or adding (for anions) to the atomic number.
29. Why are there gaps in the sequence of atomic numbers for naturally occurring elements?
Gaps in the sequence of atomic numbers for naturally occurring elements exist because some elements are synthetic and do not occur in nature. These elements, typically with high atomic numbers, are created in laboratories through nuclear reactions.
30. How do atomic numbers relate to the concept of electron affinity?
Electron affinity generally increases across a period and decreases down a group, following trends similar to electronegativity. This is because atomic number determines electron configuration, which influences how easily an atom can accept an additional electron.
31. What's the significance of the atomic number 92 (uranium) in terms of naturally occurring elements?
Uranium (atomic number 92) is the highest atomic numbered element found in significant quantities in nature. All elements with higher atomic numbers are either synthetic or found only in trace amounts in nature, marking a transition in the periodic table.
32. How do atomic numbers help in understanding the concept of ionization energy?
Ionization energy generally increases across a period and decreases down a group. This trend is directly related to the electron configuration and effective nuclear charge, both determined by the atomic number.
33. Why do elements in the same group have similar chemical properties despite having different atomic numbers?
Elements in the same group have similar outer electron configurations, despite different atomic numbers. This similarity in valence electrons leads to similar chemical properties, illustrating the periodic nature of element properties.
34. How do atomic numbers relate to the concept of atomic radius?
Atomic radius generally decreases across a period and increases down a group. This trend is due to the increasing nuclear charge (determined by atomic number) across a period and the addition of new electron shells down a group.
35. What's the significance of the atomic number 26 (iron) in terms of nuclear binding energy?
Iron-56 (with 26 protons and 30 neutrons) has the highest binding energy per nucleon of any nucleus. This makes it the most stable nucleus, which is significant in understanding nuclear reactions and the formation of elements in stars.
36. How do atomic numbers help in predicting the magnetic properties of elements?
Atomic numbers determine electron configurations, which influence magnetic properties. Elements with unpaired electrons (often transition metals) are paramagnetic or ferromagnetic, while those with paired electrons are diamagnetic.
37. Why do some elements have fractional atomic weights despite having whole number atomic numbers?
Fractional atomic weights result from the natural occurrence of multiple isotopes of an element. While the atomic number (number of protons) is always a whole number, the average mass of an element's isotopes can be fractional.
38. How do atomic numbers relate to the concept of metallic character?
Metallic character generally decreases across a period and increases down a group. This trend is related to the ease of losing electrons, which is influenced by the electron configuration and effective nuclear charge, both determined by the atomic number.
39. What's the significance of the atomic number 50 (tin) in terms of the dividing line between metals and metalloids?
Tin, with atomic number 50, sits at the border between metals and metalloids on the periodic table. It exhibits properties of both, illustrating how atomic number influences an element's position and properties in the periodic table.
40. How do atomic numbers help in understanding the concept of atomic emission spectra?
Each element has a unique atomic emission spectrum due to its specific electron configuration, which is determined by its atomic number. When excited electrons return to lower energy levels, they emit light at characteristic wavelengths, creating a "fingerprint" for each element.
41. Why are elements with even atomic numbers generally more abundant than those with odd atomic numbers?
Elements with even atomic numbers are often more abundant due to the greater stability of nuclei with even numbers of protons and neutrons. This phenomenon, known as the Oddo-Harkins rule, is related to nuclear binding energies and the processes of nucleosynthesis.
42. How do atomic numbers relate to the concept of electron shielding?
Electron shielding increases with atomic number as more inner electrons shield outer electrons from the nuclear charge. This concept is crucial in understanding trends in atomic size, ionization energy, and other periodic properties.
43. What's the significance of the atomic number 118 in terms of the current limits of the periodic table?
Element 118 (Oganesson) is currently the highest atomic numbered element synthesized and the last element that fits in the traditional periodic table structure. Beyond this, new elements would require a new period and potentially new groups, challenging our current understanding of element organization.
44. How do atomic numbers help in understanding the concept of diagonal relationships in the periodic table?
Diagonal relationships exist between certain elements with similar properties but different atomic numbers, like lithium and magnesium. These relationships arise from a balance between atomic size and electronegativity, both influenced by atomic number.
45. Why do transition metals often have similar properties despite having different atomic numbers?
Transition metals have similar properties due to their partially filled d-orbitals, which allow for multiple oxidation states and similar reactivity. While their atomic numbers differ, their outer electron configurations are often similar, leading to comparable chemical behaviors.
46. How do atomic numbers relate to the concept of electron promotion in transition metals?
Atomic numbers determine the ground state electron configuration. In transition metals, electrons can be promoted from s to d orbitals during bonding. This promotion, possible due to the energy levels determined by atomic number, explains some of their unique properties.
47. What's the significance of the atomic number 83 (bismuth) in terms of radioactive decay?
Bismuth-209, with 83 protons, was long considered the heaviest stable isotope. However, it was discovered to be slightly radioactive with an extremely long half-life. This discovery challenged our understanding of nuclear stability at high atomic numbers.
48. How do atomic numbers help in predicting the melting and boiling points of elements?
Atomic numbers influence melting and boiling points through their effect on atomic size and bonding strength. Generally, these points increase across a period and decrease down a group, with exceptions due to factors like metallic bonding strength in transition metals.
49. Why do some elements with consecutive atomic numbers have very different properties?
Elements with consecutive atomic numbers can have very different properties if they're in different groups. For example, chlorine (17) and argon (18) have drastically different properties due to their different outer electron configurations, despite having consecutive atomic numbers.
50. How do atomic numbers relate to the concept of lanthanide contraction?
Lanthanide contraction refers to the decrease in atomic and ionic radii across the lanthanide series (atomic numbers 57-71). This is due to poor shielding by f-electrons, leading to increased effective nuclear charge as atomic number increases.
51. What's the significance of the atomic number 43 (technetium) in terms of naturally occurring elements?
Technetium, atomic number 43, is the lowest numbered element that does not occur naturally on Earth. All isotopes of technetium are radioactive with relatively short half-lives, illustrating how atomic structure influences nuclear stability.
52. How do atomic numbers help in understanding the concept of relativistic effects in heavy elements?
In elements with high atomic numbers, electrons in inner orbitals move at speeds approaching the speed of light. These relativistic effects can influence properties like color (e.g., gold's yellow color) and chemical behavior, especially for elements with very high atomic numbers.
53. Why do elements in the same period have different properties despite having consecutive atomic numbers?
Elements in the same period have different properties due to their increasing number of valence electrons as atomic number increases. This leads to changes in reactivity, bonding behavior, and other chemical properties across a period.
54. How do atomic numbers relate to the concept of atomic clocks?
Atomic clocks use the precise frequency of electron transitions in specific atoms, often cesium-133 (atomic number 55). The atomic number determines the electron configuration and thus the specific transition used, making it crucial for the clock's accuracy.
55. What's the significance of the atomic number 94 (plutonium) in terms of synthetic elements?
Plutonium, atomic number 94, is the first synthetic element to be produced in macroscopic quantities and used practically (in nuclear weapons and reactors). It represents a milestone in our ability to create and utilize synthetic elements, showcasing how understanding atomic numbers and structure can lead to technological applications.

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