1st Year Chemistry Chapter 1 “Periodic Table and Periodic Properties” Notes 2026 – Complete Guide

Class: FSc Part 1 (1st Year) | Subject: Chemistry | Chapter 1: Periodic Table and Periodic Properties | Punjab Board New Syllabus

Updated 2026: Complete notes for 1st Year Chemistry Chapter 1 “Periodic Table and Periodic Properties” are available below, covering every group, trend, and exam-style question needed for the Punjab Board FSc Part 1 exam and MDCAT/ECAT preparation.

Looking for 1st Year Chemistry Chapter 1 Notes?

If you’re searching for FSc Part 1 Chemistry Chapter 1 notes, you’ve landed on the right page. “Periodic Table and Periodic Properties” is the opening chapter of the 11th class chemistry book under the new syllabus for all Punjab boards — Lahore, Gujranwala, Multan, Sargodha, Rawalpindi, Faisalabad, DG Khan, Bahawalpur, and Sahiwal — as well as the Federal Board (FBISE). This page brings together the table’s structure, periodic trends, and key groups in one place, so you don’t have to piece together notes from five different websites.

The Map That Explains the Rest of Chemistry

The periodic table isn’t just a chart to memorize — it’s a predictive tool. Once you understand why properties change the way they do across a period or down a group, you can often predict how an unfamiliar element will behave without ever looking it up. This chapter builds that reasoning skill from the ground up as the new opening chapter of FSc Part 1, and it pays off directly in later chapters on atomic structure, chemical bonding, and group-specific chemistry.

Chapter 1 – Topics Covered

Section numbering may vary slightly by edition, but all Punjab boards cover the same core topics listed above.

Key Concepts Explained

Arrangement of the Periodic Table

The modern periodic table arranges elements in order of increasing atomic number (not atomic mass, which was Mendeleev’s original 1869 method). A horizontal row is called a period, and elements in the same period have the same number of electron shells. A vertical column is called a group, and elements in the same group have the same number of electrons in their outermost shell, which is why they share similar chemical properties.

Electronic Configuration and Position

An element’s position in the periodic table can be read directly from its electronic configuration: the period number equals the number of electron shells, and for main-group elements, the group number relates directly to the number of outermost (valence) electrons. This link between configuration and position is one of the most commonly tested ideas in this chapter.

Atomic Radius

Atomic radius decreases across a period from left to right, because the increasing number of protons (nuclear charge) pulls the electron shells in more tightly, while the number of shells stays the same. Atomic radius increases down a group, because each successive element has an additional electron shell, putting the outermost electrons further from the nucleus despite the increased nuclear charge.

Ionization Energy

Ionization energy is the energy needed to remove one mole of electrons from one mole of gaseous atoms. It increases across a period, since the increasing nuclear charge holds the outermost electrons more tightly. It decreases down a group, since the outermost electron is further from the nucleus and increasingly shielded by inner shells, making it easier to remove despite the larger nuclear charge.

Electronegativity and Melting/Boiling Points

Electronegativity (the tendency of an atom to attract a shared pair of electrons in a bond) follows the same general pattern as ionization energy: it increases across a period and decreases down a group. Melting and boiling points don’t follow one single trend across the whole table — they rise through the metallic elements on the left, peak around the middle (giant covalent structures like carbon and silicon), then fall sharply for the simple molecular non-metals on the right.

Group I, Group VII, and the Noble Gases

Group I (the alkali metals: lithium, sodium, potassium) are soft, reactive metals that become more reactive going down the group, since their single outer electron becomes easier to lose. Group VII (the halogens: fluorine, chlorine, bromine, iodine) are reactive non-metals that become less reactive going down the group, since it becomes harder to attract one additional electron. Group 0 (the noble gases: helium, neon, argon) have a complete outer shell already, making them exceptionally unreactive and existing as single, separate atoms rather than molecules.

Transition Elements

The transition elements, found in the central block of the periodic table, share several distinctive properties: they typically show variable oxidation states (unlike main-group metals), form coloured compounds, and act as effective catalysts in many industrial reactions, such as iron in the Haber process and vanadium(V) oxide in the Contact process.

Sample Solved Reasoning Questions

Q1. Explain why atomic radius decreases across Period 3 (from sodium to argon).

Across Period 3, each successive element has one more proton in its nucleus, increasing nuclear charge.

All Period 3 elements have the same number of electron shells (3), so shielding stays roughly constant.

The increased nuclear charge pulls the outer electron shell in more tightly, so atomic radius decreases.

Q2. Explain why reactivity increases down Group I but decreases down Group VII.

Group I atoms react by losing their single outer electron; going down the group, that electron is further from the nucleus and more shielded, so it’s lost more easily — reactivity increases.

Group VII atoms react by gaining one electron; going down the group, the incoming electron is added to a shell further from the nucleus, so it’s attracted less strongly — reactivity decreases.

Q3. An element X is in Period 3 and Group II. State its number of electron shells and outer-shell electrons.

Period number = number of electron shells, so X has 3 electron shells.

Group II means 2 outer-shell (valence) electrons.

This matches magnesium (Mg), electronic configuration 2,8,2.

These are representative reasoning-style answers. Full notes should also include specific reactions of Group I metals with water and Group VII halogen displacement reactions, which are common practical-based exam questions.

MCQs, Short Questions & Long Questions

FSc Part 1 Chemistry Chapter 1 is tested across all three question formats in the board exam, so preparation should cover each type separately:

• MCQs: Quick identification of group/period position, trends, and electronic configuration
• Short Questions: “Give reason” explanations (2–4 lines) on periodic trends, and stating properties of a group
• Long Questions: Predicting properties of an unfamiliar element from its position, or explaining a full periodic trend with reasoning

Common Mistakes Students Make in Chapter 1

• Confusing period (row, same number of shells) with group (column, same number of outer electrons)
• Explaining periodic trends by only mentioning nuclear charge and forgetting shielding, or vice versa
• Assuming melting/boiling point follows a single smooth trend across an entire period, when it actually peaks near the middle
• Mixing up Group I’s increasing reactivity down the group with Group VII’s decreasing reactivity down the group

Why This Chapter Matters for MDCAT and ECAT

Periodic trends and group properties are a reliable, frequently tested topic in MDCAT and ECAT, since questions can be answered quickly once the underlying reasoning (nuclear charge vs. shielding) is understood, without needing lengthy calculations. As the new opening chapter of FSc Part 1, a strong grasp here also builds the reasoning habits needed for atomic structure and chemical bonding questions later in the entry test.

Availability for All Boards

These notes are prepared according to the Punjab Board syllabus and are useful for all Punjab boards (Lahore, Gujranwala, Multan, Sargodha, Rawalpindi, Faisalabad, DG Khan, Bahawalpur, Sahiwal), as well as the Federal Board (FBISE) and KPK Board, since Chapter 1 content is broadly consistent across these syllabi.

Download Notes PDF

Click below to view or download the complete Chapter 1 notes in PDF format, including every exam-style question and worked example.

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Explore More 1st Year Chemistry Notes

• 1st Year Chemistry Chapter 2 – Atomic Structure
• 1st Year Chemistry Chapter 3 – Chemical Bonding
• 1st Year Chemistry Chapter 4 – Stoichiometry
• 1st Year Chemistry Chapter 5 – States and Phases of Matter
• 1st Year Physics Notes
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• 1st Year Mathematics Notes

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Frequently Asked Questions (FAQs)

Q1. Are these Chapter 1 notes free to download?

Yes, all notes on this page are completely free to view and download in PDF format.

Q2. Which board are these notes for?

These notes are prepared according to the Punjab Board syllabus and are useful for all Punjab boards, as well as the Federal Board (FBISE) and KPK Board.

Q3. Why does ionization energy decrease down a group even though nuclear charge increases?

Although nuclear charge does increase down a group, the outermost electron is also further from the nucleus and shielded by more inner electron shells. These two effects work in opposite directions, but the increased distance and shielding outweigh the increased nuclear charge, so ionization energy decreases overall.

Q4. Does this page include exam-style questions?

Yes, the notes include fully solved reasoning-style short questions and MCQs matching the board paper pattern, along with long questions.

Q5. How can I download the PDF?

Click the “Download PDF” button above and the notes will open or download directly to your device.

Q6. Are these notes updated for the current syllabus?

Yes, these notes are prepared strictly according to the latest Punjab Textbook Board syllabus for FSc Part 1 Chemistry.

Comments & Feedback

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