Periodic Table and Elemental Configurations: A Comprehensive Guide
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Periodic Table and Elemental Configurations
This lesson provides a comprehensive overview of the periodic table and the elemental configurations of various elements.
You’ll learn about the classification of elements, the unique properties of noble gases, the reactivity of alkali metals, and the importance of transition metals.
Dive into the world of chemistry and explore the atomic structures that underlie the behavior of different elements
Electronic configuration for group 1:
The elements in Group 1 of the periodic table are known as the alkali metals. Here is the electronic configuration for each alkali metal :
Element Atomic NO. E. Configuration
Hydrogen (H) 1 1s¹
Lithium (Li) 3 [He] 2s¹
Sodium (Na) 11 [Ne] 3s¹
Potassium (K) 19 [Ar] 4s¹
Rubidium (Rb) 37 [Kr] 5s¹
Cesium (Cs) 55 [Xe] 6s¹
Francium (Fr) 87 [Rn] 7s¹
In this table, the electronic configurations are written according to the nearest noble gas with a lower atomic number in square brackets. The alkali metals have one electron in their outermost s orbital, making them highly reactive and prone to losing that electron in chemical reactions to form cations with a +1 charge.
Electronic configuration for group 2:
The elements in Group 2 of the periodic table are known as the alkaline earth metals. Here is the electronic configuration for each alkaline earth metal :
Element Atomic NO. E.Configuration
Beryllium (Be) 4 [He] 2s²
Magnesium (Mg) 12 [Ne] 3s²
Calcium (Ca) 20 [Ar] 4s²
Strontium (Sr) 38 [Kr] 5s²
Barium (Ba) 56 [Xe] 6s²
Radium (Ra) 88 [Rn] 7s²
In this table, the electronic configurations are written according to the nearest noble gas with a lower atomic number in square brackets.
The alkaline earth metals have two electrons in their outermost s orbital, making them chemically reactive, although less so than the alkali metals in Group 1.
They tend to lose those two outermost electrons in chemical reactions to form cations with a +2 charge.
Electronic configuration for group 3:
The elements in Group 3 of the periodic table belong to the transition metals and have variable electron configurations. Here is the electronic configuration for each element in Group 3 :
Element Atomic NO. E. Configuration
Scandium (Sc) 21 [Ar] 4s² 3d¹
Yttrium (Y) 39 [Kr] 5s² 4d¹
Lanthanum (La) 57 [Xe] 6s² 5d¹
Actinium (Ac) 89 [Rn] 7s² 6d¹
Scandium and yttrium are considered the first two elements of Group 3. The electron configurations shown are for their neutral, ground-state atoms.
Transition metals have partially filled d orbitals and their configurations may vary as they progress through the transition series.
The lanthanide and actinide series, which start with lanthanum and actinium, respectively, have more complex electron configurations due to the presence of f orbitals.
Electronic configuration for group 4:
The elements in Group 4 of the periodic table belong to the carbon group and have variable electron configurations. Here is the electronic configuration for each element in Group 4 :
Element Atomic NO. E. Configuration
Carbon (C) 6 1s² 2s² 2p²
Silicon (Si) 14 1s² 2s² 2p⁶ 3s² 3p²
Germanium (Ge) 32 [Ar] 4s² 3d¹⁰ 4p²
Tin (Sn) 50 [Kr] 5s² 4d¹⁰ 5p²
Lead (Pb) 82 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p²
Carbon and silicon are nonmetals, while germanium, tin, and lead are metals.
The electron configurations are for their neutral, ground-state atoms.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels and the transition from nonmetals to metals.
Electronic configuration for group 5:
The elements in Group 5 of the periodic table, also known as the nitrogen group, have variable electron configurations. Here is the electronic configuration for each element in Group 5 :
Element Atomic no. E. Configuration
Nitrogen (N) 7 1s² 2s² 2p³
Phosphorus (P) 15 1s² 2s² 2p⁶ 3s² 3p³
Arsenic (As) 33 [Ar] 4s² 3d¹⁰ 4p³
Antimony (Sb) 51 [Kr] 5s² 4d¹⁰ 5p³
Bismuth (Bi) 83 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p³
The electron configurations shown are for their neutral, ground-state atoms.
Group 5 elements typically have five valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 6
The elements in Group 6 of the periodic table, also known as the chalcogens, have variable electron configurations. Here is the electronic configuration for each element in Group 6 :
Element Atomic NO. E. Configuration
Oxygen (O) 8 1s² 2s² 2p⁴
Sulfur (S) 16 1s² 2s² 2p⁶ 3s² 3p⁴
Selenium (Se) 34 [Ar] 4s² 3d¹⁰ 4p⁴
Tellurium (Te) 52 [Kr] 5s² 4d¹⁰ 5p⁴
Polonium (Po) 84 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁴
The electron configurations shown are for their neutral, ground-state atoms.
Group 6 elements typically have six valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 7
The elements in Group 7 of the periodic table, also known as the halogens, have variable electron configurations. Here is the electronic configuration for each element in Group 7 :
Element Atomic NO. E. Configuration
Fluorine (F) 9 1s² 2s² 2p⁵
Chlorine (Cl) 17 1s² 2s² 2p⁶ 3s² 3p⁵
Bromine (Br) 35 [Ar] 4s² 3d¹⁰ 4p⁵
Iodine (I) 53 [Kr] 5s² 4d¹⁰ 5p⁵
Astatine (At) 85 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁵
The electron configurations shown are for their neutral, ground-state atoms.
Group 7 elements typically have seven valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 18
The elements in Group 18 of the periodic table, also known as the noble gases, have stable and completely filled electron configurations.
Here is the electronic configuration for each noble gas element in Group 18 :
Element Atomic NO. E. Configuration
Helium (He) 2 1s²
Neon (Ne) 10 1s² 2s² 2p⁶
Argon (Ar) 18 1s² 2s² 2p⁶ 3s² 3p⁶
Krypton (Kr) 36 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶
Xenon (Xe) 54 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ 5s² 5p⁶
Radon (Rn) 86 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 4p⁶ 5s² 5p⁶ 6s² 6p⁶
The noble gases have full outermost electron shells, making them very stable and chemically unreactive under normal conditions.
They are known for their inert nature due to their electron configurations, which are fully filled with electrons.
Electronic configuration for group 3B
The elements in Group 3B of the periodic table are transition metals and have variable electron configurations.
Here is the electronic configuration for each element in Group 3B :
Element Atomic NO. E. Configuration
Scandium (Sc) 21 [Ar] 4s² 3d¹
Yttrium (Y) 9 [Kr] 5s² 4d¹
Lanthanum (La) 57 [Xe] 6s² 5d¹
Actinium (Ac) 89 [Rn] 7s² 6d¹
The electron configurations shown are for their neutral, ground-state atoms.
These transition metals have partially filled d orbitals, and their configurations may vary as they progress through the transition series. Lanthanum and actinium are sometimes considered the first elements of the lanthanide and actinide series, respectively.
The lanthanide and actinide series have more complex electron configurations due to the presence of f orbitals.
Electronic configuration for group 4B
The elements in Group 4B of the periodic table, also known as the transition metals, have variable electron configurations. Here is the electronic configuration for each element in Group 4B :
Element Atomic NO. E. Configuration
Titanium (Ti) 22 [Ar] 4s² 3d²
Zirconium (Zr) 40 [Kr] 5s² 4d²
Hafnium (Hf) 72 [Xe] 6s² 4f¹⁴ 5d²
Rutherfordium (Rf) 104 [Rn] 7s² 5f¹⁴ 6d²
The electron configurations shown are for their neutral, ground-state atoms.
Transition metals have partially filled d orbitals, and their configurations may vary as they progress through the transition series.
Hafnium and Rutherfordium have more complex configurations due to the presence of f orbitals for hafnium and the extended electron shells for superheavy elements like Rutherfordium.
Electronic configuration for group 5B
The elements in Group 5B of the periodic table, also known as Group 15 or the nitrogen group, have variable electron configurations. Here is the electronic configuration for each element in Group 5B :
Element Atomic NO. E. Configuration
Nitrogen (N) 7 1s² 2s² 2p³
Phosphorus (P) 15 1s² 2s² 2p⁶ 3s² 3p³
Arsenic (As) 33 [Ar] 4s² 3d¹⁰ 4p³
Antimony (Sb) 51 [Kr] 5s² 4d¹⁰ 5p³
Bismuth (Bi) 83 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p³
The electron configurations shown are for their neutral, ground-state atoms.
Group 5B elements typically have five valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 6B
The elements in Group 6B of the periodic table, also known as Group 16 or the chalcogens, have variable electron configurations. Here is the electronic configuration for each element in Group 6B :
Element Atomic NO. E.Configuration
Oxygen (O) 8 1s² 2s² 2p⁴
Sulfur (S) 16 1s² 2s² 2p⁶ 3s² 3p⁴
Selenium (Se) 34 [Ar] 4s² 3d¹⁰ 4p⁴
Tellurium (Te) 52 [Kr] 5s² 4d¹⁰ 5p⁴
Polonium (Po) 84 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁴
The electron configurations shown are for their neutral, ground-state atoms.
Group 6B elements typically have six valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 7A
The elements in Group 7A of the periodic table, also known as Group 17 or the halogens, have variable electron configurations.
Here is the electronic configuration for each element in Group 7A :
Element Atomic no. E.Configuration
Fluorine (F) 9 1s² 2s² 2p⁵
Chlorine (Cl) 17 1s² 2s² 2p⁶ 3s² 3p⁵
Bromine (Br) 35 [Ar] 4s² 3d¹⁰ 4p⁵
Iodine (I) 53 [Kr] 5s² 4d¹⁰ 5p⁵
Astatine (At) 85 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p⁵
The electron configurations shown are for their neutral, ground-state atoms.
Group 7A elements typically have seven valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.
Electronic configuration for group 5
The elements in Group 5 of the periodic table, also known as Group 15 or the nitrogen group, have variable electron configurations.
Here is the electronic configuration for each element in Group 5 :
Element Atomic No. E. Configuration
Nitrogen (N) 7 1s² 2s² 2p³
Phosphorus (P) 15 1s² 2s² 2p⁶ 3s² 3p³
Arsenic (As) 33 [Ar] 4s² 3d¹⁰ 4p³
Antimony (Sb) 51 [Kr] 5s² 4d¹⁰ 5p³
Bismuth (Bi) 83 [Xe] 6s² 4f¹⁴ 5d¹⁰ 6p³
The electron configurations shown are for their neutral, ground-state atoms.
Group 5 elements typically have five valence electrons, resulting in configurations with p-block electrons.
The configurations become progressively more complex as you move down the group due to the filling of higher energy levels.