Grade 10
  1. Matter and its properties  1.1. States of matter  1.2. Physical and chemical properties of matter  1.3. Classification of substances (elements, compounds, mixtures)  1.4. Changes in Matter (Physical and Chemical Changes)  1.5. Law of conservation of mass and law of definite proportions
  2. Atomic Structure  2.1. Historical development of the atomic model  2.2. Subatomic particles (protons, neutrons, electrons)  2.3. Atomic number, mass number and isotopes  2.4. Electronic Configuration and Energy Levels  2.5. Valency, ion formation and oxidation state
  3. Periodic table  3.1. History and Development of the Periodic Table  3.2. Modern Periodic Law and Periodic Trends  3.3. Groups and Periods in the Periodic Table  3.4. Trends in the Periodic Table  3.5. Metals, non-metals, metalloids and their properties  3.6. Noble gases and their chemical inertness
  4. Chemical bond  4.1. Formation of Chemical Bonds (Octet Rule)  4.2. Ionic Bonding and Properties of Ionic Compounds  4.3. Covalent Bond and Properties of Covalent Compounds  4.4. Metallic bond and its properties  4.5. Molecular geometry and VSEPR theory  4.6. Polarity and dipole moment of molecules  4.7. Intermolecular forces
  5. Chemical Reactions and Equations  5.1. Types of Chemical Reactions  5.2. Writing and balancing chemical equations  5.3. Law of conservation of mass in chemical reactions  5.4. Factors Affecting Chemical Reactions  5.5. Catalysts and their role in chemical reactions  5.6. Exothermic and Endothermic Reactions
  6. Stoichiometry and Chemical Calculations  6.1. Mole concept and Avogadro number  6.2. Molar Mass and Gram-Mole Conversions  6.3. Empirical and molecular formula  6.4. Stoichiometric calculations and chemical yield  6.5. Limiting and Excess Reactants
  7. Acids, Bases and Salts  7.1. Properties and Definitions of Acids and Bases (Arrhenius, Bronsted-Lowry, Lewis)  7.2. pH Scale, pOH, and Indicators  7.3. Neutralization reactions and salt formation  7.4. Strength of Acids and Bases (Strong vs. Weak Acids and Bases)  7.5. Common Acids and Bases in Daily Life  7.6. Salts, their solubility and applications
  8. Metals and Nonmetals  8.1. Physical and chemical properties of metals  8.2. Physical and Chemical Properties of Non-Metals  8.3. Reactivity Series of Metals and Displacement Reactions  8.4. Extraction of metals from ores  8.5. Corrosion, its causes and prevention  8.6. Alloys, their composition and uses
  9. Carbon and its compounds  9.1. Allotropes of Carbon  9.2. Hydrocarbons and their classification (alkanes, alkenes, alkynes)  9.3. Functional groups in organic compounds  9.4. Nomenclature of organic compounds (IUPAC system)  9.5. Isomerism in organic chemistry (structural and geometrical)  9.6. Important organic reactions (combustion, addition, substitution, polymerization)  9.7. Applications of organic compounds in industry and daily life
  10. Environmental Chemistry  10.1. Air Pollution (Sources, Effects and Control)  10.2. Water Pollution (Causes, Effects and Remedies)  10.3. Greenhouse effect and global warming  10.4. Ozone layer depletion and its effects  10.5. Green Chemistry and Its Applications  10.6. sustainable chemistry practice
  11. Thermochemistry  11.1. Heat and Energy Changes in Chemical Reactions  11.2. Exothermic and Endothermic Reactions  11.3. Enthalpy, enthalpy change, and heat of reaction  11.4. Specific heat capacity and calorimetry  11.5. Energy Changes in Combustion Reactions
  12. Electrochemistry  12.1. Electrolytes and non-electrolytes  12.2. Electrolysis and its applications (electroplating, extraction of metals)  12.3. Redox reactions (oxidation and reduction)  12.4. Galvanic cell and electrochemical series  12.5. Corrosion and electrochemical prevention methods
  13. Chemical kinetics and equilibrium  13.1. Rate of chemical reactions and its measurement  13.2. Factors affecting the reaction rate (catalyst, temperature, concentration)  13.3. Reversible and irreversible reactions  13.4. Dynamic equilibrium and equilibrium constant  13.5. Le Chatelier's principle and its applications
  14. Gases and Gas Laws  14.1. Properties of gases and kinetic molecular theory  14.2. Boyle's Law (Pressure-Volume Relation)  14.3. Charles's Law  14.4. Gay-Lussac's Law  14.5. Combined Gas Law and Ideal Gas Law  14.6. Real Gases vs Ideal Gases
  15. Nuclear Chemistry  15.1. Introduction to Radioactivity and Nuclear Reactions  15.2. Types of radioactive decay (alpha, beta, gamma)  15.3. Half-life and applications of radioactive isotopes  15.4. Nuclear fission and fusion reactions  15.5. Nuclear power generation and its environmental impact

Grade 10 → Periodic table ↓


Groups and Periods in the Periodic Table


The periodic table is an organized, scientific way of arranging known elements in order based on similar properties. One of the key organizational aspects of the periodic table is the arrangement of elements into groups and periods. Understanding the structure of groups and periods is important as it helps predict the behavior and evolution of chemical properties in elements. Let us understand these concepts in detail, exploring their significance and characteristics.

Understanding the arrangement of the periodic table

The periodic table is made up of rows and columns that form a grid layout. Each element is placed in a specific place based on its atomic number (the number of protons in the nucleus) and its chemical properties.

,
| h | | | | | | | |that |
,
|Li |BE | | | | B |C |
,

The snippet above provides a simple representation of the beginning of the periodic table, showing hydrogen (H), helium (He), lithium (Li), beryllium (Be), boron (B), and carbon (C). The vertical columns are known as groups, while the horizontal rows are known as periods.

What are groups in the periodic table?

A group in the periodic table is a vertical column of elements that share certain chemical properties. There are 18 groups in the modern periodic table. Each group is given a number from 1 to 18, increasing from left to right in the table.

,
|Group |1 |That |
,
| |Li |
,

The diagram above shows the elements of group 1 (also called the alkali metals), which includes elements such as lithium (Li). Elements in the same group usually have the same valence electron configuration, which means they react similarly.

Properties and examples of group elements

Let us consider group 1, which consists of the following alkali metals:

  • Lithium (Li): 1s 2 2s 1
  • Sodium (Na): 1s 2 2s 2 2p 6 3s 1
  • Potassium (K): 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1

Alkali metals are highly reactive because they have one electron in their outermost shell, which is easily lost during chemical reactions. This characteristic provides similar chemical behaviour and properties in this group.

What are periods in the periodic table?

Periods in the periodic table refer to the horizontal rows of elements. There are seven periods in the modern periodic table. Each period represents an increase in the principal quantum number (n) of the outermost energy level of the atoms.

,
|h | |he |
,
|li |
,

In the diagram, the first half of Period 1 is shown, starting with hydrogen (H). Each subsequent period moves to the next row of the table.

Properties and examples of periodic elements

As you move from left to right in a period, the atomic number of the elements increases. This means an increase in the number of protons and electrons, which changes the atomic size and potential reactivity. Consider the second period which has the following elements:

  • Lithium (Li): [He] 2s 1
  • Beryllium (Be): [He] 2s 2
  • Boron (B): [He] 2s 2 2p 1

The trend across a period is generally for ionization energy and electronegativities to increase as the size of the atom decreases, because the valence electrons move closer to the more positively charged nucleus.

Relationships between groups and periods

Groups and periods of the periodic table are interconnected through the electronic configuration of the elements. Elements in the same group show similar chemical behaviour due to having the same number of electrons in their outermost shell, while electrons in elements of the same period fill the same principal energy level.

,
|B |C |
,

The shared characteristics of groups and periods allow chemists to predict how elements will react and bond with each other, as well as trends related to other chemical and physical properties. For example, metallic characteristics decrease across a period but increase as one moves down a group.

Viewing trends by group and period

Below is a simplified representation to show the group and period trends in atomic radius, electronegativities, and reactivity.

,
|Reactivity(large)|---->
,

,
|Electronegativity|
,
,
| small | big

As you can see, trends are plotted on the periodic table, showing how properties change across different periods and groups, and providing insight into the behavior and possible chemical bonding of the elements.

Conclusion

Understanding groups and periods is important for understanding the periodic table and predicting the chemical reactions and bonds formed by the elements. Elements are arranged in groups with similar chemical properties, and periods indicate the filling of electron energy levels. Through these structures, much can be understood about atomic structure, chemical reactivity, and potential applications in scientific studies and practical applications.

Overall, a solid understanding of groups and periods provides a strong foundation for further chemistry studies and enhances the ability to link atomic properties to observable chemical phenomena.


Grade 10 → 3.3


U
username
0%
completed in Grade 10

← Prev (3.2)
Modern Periodic Law and Periodic Trends
Next (3.4) →
Trends in the Periodic Table

Comments 



Groups and Periods in the Periodic Table

https://www.chemistryelite.com/g10/3.3?ceal=en