Recent Lessons

Show all results for ""

Feature Overview

Ace your exams with our all-in-one platform for creating and sharing quizzes and tests.

Quizzes

Create quizzes and tests automatically from your content using AI.

Flashcards

Automatically turn your notes into digital flashcards.

Share, Export & Embed

Share with classmates or export to Excel and your learning management system.

Stats & Reporting

Auto-grading quizzes and tests with detailed stats and reports.

Mobile Apps

The smarter way to study – wherever you are.

Pricing

Search...

5 Questions

4 Views

Periodic Table Gradation Quiz

Choose a study mode

Play Quiz

Study Flashcards

Spaced Repetition

Chat to lesson

Podcast

Play an AI-generated podcast conversation about this lesson

Questions and Answers

Which of the following best describes the effect of increasing the number of electrons on a negative ion?

It decreases the repulsion force between the electrons, leading to a decrease in the energy level radius.

It increases the attraction force between the electrons and the nucleus.

It has no effect on the repulsion force between the electrons.

It increases the repulsion force between the electrons, leading to an increase in the energy level radius. (correct)

What effect does the nucleus charge have on the attraction of electrons as described in the text?

The nucleus charge decreases the attraction of electrons.

The nucleus charge has no effect on the attraction of electrons.

The nucleus charge has a variable effect on the attraction of electrons.

The nucleus charge increases the attraction of electrons. (correct)

How does ionization energy change as we move down a group in the periodic table?

Ionization energy increases as we move down a group.

Ionization energy decreases as we move down a group. (correct)

Ionization energy fluctuates as we move down a group.

Ionization energy remains constant as we move down a group.

What is the relationship between the effective nuclear charge and the radius of an atom?

<p>Increasing effective nuclear charge leads to a decreased radius of an atom.</p> Signup and view all the answers

What is ionization energy?

<p>Ionization energy is the amount of energy needed to remove an electron from an atom or ion.</p> Signup and view all the answers

Study Notes

Structure of the Modern Periodic Table

Consists of 18 vertical groups and 7 horizontal rows.
Divided into four blocks:
- Block S
- Block P
- Block D
- Block F

Gradation of Properties

Atomic Radius:
- Defined as the distance between the centers of two identical atoms in a molecule.
- In rows:
  - Atomic size decreases with an increase in atomic number.
  - This occurs due to the increased positive charge in the nucleus while electrons are added at the same energy level, leading to minimal shielding effect.
- In columns:
  - Atomic size increases with an increase in atomic number.
  - New energy levels are added, distancing electrons from nuclear charge.
  - Full energy levels shield outer electrons from the nucleus's attractive force.
Ionic Size:
- For positive ions:
  - Removal of outer electrons results in the nucleus holding a greater positive charge than the total negative charge from the remaining electrons.

Studying That Suits You

Use AI to generate personalized quizzes and flashcards to suit your learning preferences.

Description

Test your knowledge of the modern periodic table and its properties. Learn about the structure of the periodic table, including the 18 groups and 7 rows, and understand the division into 4 blocks. Explore the gradation of properties such as atomic radius and the factors affecting it.