Atomic Structure Progress Quiz

Created by

Hosni chembio

teacher

Created by

Hosni chembio

teacher

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What is the smallest component of an element?

Atom

What are the three subatomic particles that make up an atom?

Proton, Neutron, Electron

What is the relationship between protons and electrons in a neutral atom?

The number of protons equals the number of electrons.

How is the atomic number of an element defined?

The atomic number is the number of protons in the atom.

What defines an element?

An element is a substance made of atoms with the same atomic number.

What is the formula for calculating the mass number of an atom?

Mass number = Number of protons + Number of neutrons

What are isotopes?

Isotopes are atoms of the same element with the same proton number but different nucleon numbers.

What are cations and anions?

Cations are positive ions with fewer electrons than protons; anions are negative ions with more electrons than protons.

What is the maximum number of electrons that can occupy the first electron shell?

2 electrons

How do you determine the number of valence electrons in an element?

The number of valence electrons equals the group number.

What distinguishes radioactive isotopes from non-radioactive isotopes?

Radioactive isotopes have unstable nuclei that release radiation; non-radioactive isotopes have stable nuclei.

What are two major applications of isotopes?

Medical uses (e.g., killing cancer cells) and industrial uses (e.g., uranium-235 for electricity generation).

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Boost your knowledge before diving into past papers. Use these questions to reinforce your understanding of the lessons and supercharge your revision. They'll help you recall key concepts and stay on top of your studies

Questions

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1. What are the three subatomic particles that make up an atom?

A Protons, neutrons, and ions B Protons, molecules, and electrons C Protons, neutrons, and electrons D Electrons, ions, and molecules

2. What determines the identity of an element?

A The mass number B The number of neutrons C The number of electrons D The number of protons

3. What is the term for atoms with the same number of protons but different numbers of neutrons?

A Isotopes B Ions C Cations D Anions

4. What is the maximum number of electrons that can occupy the outer shell of an atom?

A 10 electrons B 2 electrons C 8 electrons D 6 electrons

5. What is the maximum number of electrons that the first electron shell can hold?

A 4 electrons B 6 electrons C 2 electrons D 8 electrons

6. What is the relationship between the number of valence electrons and the group number in the periodic table?

A The number of valence electrons is double the group number B They are equal C There is no relationship D The number of valence electrons is half the group number

7. Where are protons and neutrons located in an atom?

A In the valence shell B In the outer shell C In the electron shells D In the nucleus

8. How do you determine the mass number of an atom?

A Neutrons + Electrons B Protons + Neutrons C Protons + Electrons D Protons only

9. What is the charge of a neutron?

A 1- (negative) B 1+ (positive) C 0 (neutral) D 2+ (positive)

10. What is the maximum number of electrons that can occupy the second electron shell of an atom?

A 8 electrons B 6 electrons C 2 electrons D 4 electrons

11. What is the main difference between radioactive and non-radioactive isotopes?

A Non-radioactive isotopes have unstable nuclei B Non-radioactive isotopes release radiation C Radioactive isotopes have the same mass D Radioactive isotopes have unstable nuclei that release radiation

12. Why do isotopes have similar chemical properties?

A They have the same number of valence electrons B They have different numbers of neutrons C They have different atomic numbers D They have the same mass number

13. What is one medical use of isotopes?

A Determining atomic mass B Killing cancer cells C Generating electricity D Creating new elements

14. How are isotopes of an element written?

A Using their symbol, mass number (upper left), and atomic number (lower left) B Using their symbol and proton number C Using their symbol and atomic mass D Using their symbol and neutron number

15. What is the charge of an atom with more electrons than protons?

A Neutral atom B Positive ion (cation) C Negative ion (anion) D Isotope

Study Notes

Understanding Atomic Structure and Subatomic Particles

This document provides a comprehensive overview of atomic structure, focusing on the fundamental components of atoms, the arrangement of subatomic particles, and the significance of isotopes and ions in chemistry.

The Atom and Subatomic Particles

Definition: The atom is the smallest unit of an element, consisting of a nucleus surrounded by electron shells.
Composition: Atoms are made up of three main subatomic particles: protons (positive charge, located in the nucleus), neutrons (no charge, also in the nucleus), and electrons (negative charge, orbiting the nucleus).

Atomic Structure and Electron Configuration

Atomic Number and Mass Number: The atomic number is defined as the number of protons in an atom, while the mass number is the total count of protons and neutrons. These numbers are essential for identifying elements and their isotopes.
Electron Shells: Electrons fill shells starting from the innermost layer, with the first shell holding up to 2 electrons and subsequent shells holding up to 8 electrons each. The outermost electrons are known as valence electrons, which determine an element's chemical properties.

Isotopes and Ions

Isotopes: Isotopes are variants of the same element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers. They exhibit similar chemical properties due to having the same number of valence electrons.
Ions: Ions are formed when an atom has an unequal number of protons and electrons. Anions have more electrons than protons (negative charge), while cations have fewer electrons (positive charge).

Key Takeaways

Atoms consist of a nucleus and electron shells, with subatomic particles playing distinct roles in their structure.
The atomic number identifies an element, while isotopes differ in neutron count but share chemical properties.
Understanding electron configuration is crucial for predicting an element's reactivity and behavior in chemical reactions.