Subjects

Subjects

More

Search

AI Knowunity

Subjects

/

Chemistry

/

Molecular and ionic compound structure and properties

/

Lewis diagrams

/

Lewis

Atomic Structure Basics for Exams: Fun Worksheets and Cool Notes!

View

Atomic Structure Basics for Exams: Fun Worksheets and Cool Notes!
user profile picture

Rebecca Lomelino

@rebeccalomelino_bcwe

·

0 Follower

Follow

The content appears to be about atomic structure and the periodic table, but the text is quite fragmented and contains some unclear symbols and notations. I'll create an SEO-optimized summary following your guidelines.

A comprehensive guide to atomic structure and fundamental chemistry concepts, focusing on subatomic particles, atomic theories, and electron configuration.

Key points:

  • Detailed exploration of protons, neutrons, and electrons
  • Historical atomic theories from Dalton to Bohr
  • Calculation methods for atomic mass and subatomic particles
  • Electron configuration rules and periodic table organization
  • Isotopes and their significance in atomic structure

3/5/2023

129

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Relative Atomic Mass (RAM)

This section introduces the concept of relative atomic mass and provides instructions on how to calculate it.

Definition: Relative atomic mass is the average mass of an atom, compared to 1/12 the mass of a Carbon-12 atom.

The document emphasizes the importance of memorizing this definition for exam purposes.

Calculating RAM: RAM = [(Mass of Isotope 1 × Abundance of Isotope 1) + (Mass of Isotope 2 × Abundance of Isotope 2)] ÷ 100

Example: For carbon with 90% Carbon-12 and 10% Carbon-14, the calculation would be: RAM = [(12 × 90) + (14 × 10)] ÷ 100 = 12.2

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Electron Configuration

This page outlines the rules for filling electron shells in atoms.

Electron shell capacities: • Shell 1 (closest to nucleus): 2 electrons (max) • Shell 2: 8 electrons (max) • Shell 3: 8 electrons (max) • Shell 4-7: 8 electrons each (max)

Highlight: Understanding electron configuration is crucial for predicting an element's chemical behavior and its position in the periodic table.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Atomic Theories

This page outlines the progression of atomic theories throughout history, highlighting key scientists and their contributions to our understanding of atomic structure.

  1. John Dalton (1803): Proposed that all matter is made of indivisible atoms, with atoms of the same element being identical.

  2. J.J. Thomson (1897): Discovered electrons, proving that atoms contain smaller particles.

  3. Ernest Rutherford (1911): Established the existence of a positively charged nucleus within the atom.

  4. Niels Bohr (1913): Introduced the concept of electrons occupying specific shells around the nucleus.

Highlight: Scientific theories are accepted or rejected based on experimental evidence and observations. Theories may become more convincing when predictions based on them are later confirmed.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Isotopes and Subatomic Particles

This page covers the similarities and differences between atoms of the same and different elements, as well as how to calculate the number of subatomic particles.

All atoms of the same element have the same atomic number, while atoms of different elements have different atomic numbers.

Vocabulary: Isotopes - atoms of the same element with the same number of protons and electrons but a different number of neutrons.

Calculating subatomic particles: • Number of protons = atomic number • Number of electrons = number of protons (in a neutral atom) • Number of neutrons = mass number - atomic number

Example: Carbon has three naturally occurring isotopes: Carbon-12, Carbon-13, and Carbon-14, all with 6 protons and electrons but different numbers of neutrons (6, 7, and 8 respectively).

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Mendeleev's Periodic Table

This page introduces Mendeleev's periodic table, which was a crucial step in the development of the modern periodic table.

The image shows the beginning of Mendeleev's table, highlighting the arrangement of elements into groups and series (periods).

Highlight: Mendeleev's table was revolutionary because it allowed for the prediction of undiscovered elements based on patterns in the table.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Periodic Table Structure

The periodic table organizes elements based on their atomic structure and properties.

Key points: • Elements are arranged in order of increasing atomic number • Rows are called periods, columns are called groups • The group number indicates the number of electrons in the outer shell • The period number indicates how many electron shells an atom has

Example: Lithium is in group 1, so it has 1 electron in its outer shell. It's also in period 2, meaning it has 2 electron shells.

Highlight: Elements in the same group have similar chemical and physical properties.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Structure of the Atom

The basic structure of an atom consists of a nucleus containing protons and neutrons, with electrons orbiting in shells around the nucleus. This fundamental arrangement is crucial for understanding atomic behavior and chemical properties.

Vocabulary: Subatomic particles - protons, electrons, and neutrons that make up an atom.

Highlight: Most of the atom's mass is concentrated in the nucleus, despite it being much smaller than the electron shells.

The document provides an information table detailing the location, relative mass, and charge of each subatomic particle. It's important to note that protons and neutrons have a much higher mass than electrons.

Example: If an atom were the size of a football field, the nucleus would be comparable to a single blueberry.

The overall charge of an atom is neutral because the number of protons (positive) equals the number of electrons (negative), canceling each other out.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Atomic Number and Mass Number

This section explains two fundamental concepts in atomic structure: atomic number and mass number.

Definition: Atomic number is the total number of protons within the nucleus of an atom, which is also equal to the number of electrons in a neutral atom.

The atomic number is represented by the smaller number on the periodic table.

Definition: Mass number is the total number of protons and neutrons within the nucleus of an atom.

The mass number is represented by the larger number on the periodic table.

Example: For fluorine (F), the atomic number is 9, and the mass number is 19.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

View

Similar Content

Know Types of IMFs thumbnail

0

45

Types of IMFs

Notes on the types of inter-molecular forces including London dispersion forces, dipole-dipole forces, hydrogen bonds, and ion-dipole forces. Includes lots of example problems.

Know Binary Ionic Compound thumbnail

7

61

10th/11th

Binary Ionic Compound

This is about recognizing and naming Binary Ionic Compound

Know Covalent Bonds Worksheet thumbnail

0

5

Covalent Bonds Worksheet

2 questions each with 2 sub-questions. The questions are solved with the correct solutions

Can't find what you're looking for? Explore other subjects.

Knowunity is the # 1 ranked education app in five European countries

Knowunity was a featured story by Apple and has consistently topped the app store charts within the education category in Germany, Italy, Poland, Switzerland and United Kingdom. Join Knowunity today and help millions of students around the world.

Ranked #1 Education App

Download in

Google Play

Download in

App Store

Knowunity is the # 1 ranked education app in five European countries

4.9+

Average App Rating

13 M

Students use Knowunity

#1

In Education App Charts in 12 Countries

950 K+

Students uploaded study notes

Still not sure? Look at what your fellow peers are saying...

iOS User

I love this app so much [...] I recommend Knowunity to everyone!!! I went from a C to an A with it :D

Stefan S, iOS User

The application is very simple and well designed. So far I have found what I was looking for :D

SuSSan, iOS User

Love this App ❤️, I use it basically all the time whenever I'm studying

Subjects

/

Chemistry

/

Molecular and ionic compound structure and properties

/

Lewis diagrams

/

Lewis

Atomic Structure Basics for Exams: Fun Worksheets and Cool Notes!

user profile picture

Rebecca Lomelino

@rebeccalomelino_bcwe

·

0 Follower

Follow

The content appears to be about atomic structure and the periodic table, but the text is quite fragmented and contains some unclear symbols and notations. I'll create an SEO-optimized summary following your guidelines.

A comprehensive guide to atomic structure and fundamental chemistry concepts, focusing on subatomic particles, atomic theories, and electron configuration.

Key points:

  • Detailed exploration of protons, neutrons, and electrons
  • Historical atomic theories from Dalton to Bohr
  • Calculation methods for atomic mass and subatomic particles
  • Electron configuration rules and periodic table organization
  • Isotopes and their significance in atomic structure

3/5/2023

129

 

7/8

 

Chemistry

6

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Relative Atomic Mass (RAM)

This section introduces the concept of relative atomic mass and provides instructions on how to calculate it.

Definition: Relative atomic mass is the average mass of an atom, compared to 1/12 the mass of a Carbon-12 atom.

The document emphasizes the importance of memorizing this definition for exam purposes.

Calculating RAM: RAM = [(Mass of Isotope 1 × Abundance of Isotope 1) + (Mass of Isotope 2 × Abundance of Isotope 2)] ÷ 100

Example: For carbon with 90% Carbon-12 and 10% Carbon-14, the calculation would be: RAM = [(12 × 90) + (14 × 10)] ÷ 100 = 12.2

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Electron Configuration

This page outlines the rules for filling electron shells in atoms.

Electron shell capacities: • Shell 1 (closest to nucleus): 2 electrons (max) • Shell 2: 8 electrons (max) • Shell 3: 8 electrons (max) • Shell 4-7: 8 electrons each (max)

Highlight: Understanding electron configuration is crucial for predicting an element's chemical behavior and its position in the periodic table.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Atomic Theories

This page outlines the progression of atomic theories throughout history, highlighting key scientists and their contributions to our understanding of atomic structure.

  1. John Dalton (1803): Proposed that all matter is made of indivisible atoms, with atoms of the same element being identical.

  2. J.J. Thomson (1897): Discovered electrons, proving that atoms contain smaller particles.

  3. Ernest Rutherford (1911): Established the existence of a positively charged nucleus within the atom.

  4. Niels Bohr (1913): Introduced the concept of electrons occupying specific shells around the nucleus.

Highlight: Scientific theories are accepted or rejected based on experimental evidence and observations. Theories may become more convincing when predictions based on them are later confirmed.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Isotopes and Subatomic Particles

This page covers the similarities and differences between atoms of the same and different elements, as well as how to calculate the number of subatomic particles.

All atoms of the same element have the same atomic number, while atoms of different elements have different atomic numbers.

Vocabulary: Isotopes - atoms of the same element with the same number of protons and electrons but a different number of neutrons.

Calculating subatomic particles: • Number of protons = atomic number • Number of electrons = number of protons (in a neutral atom) • Number of neutrons = mass number - atomic number

Example: Carbon has three naturally occurring isotopes: Carbon-12, Carbon-13, and Carbon-14, all with 6 protons and electrons but different numbers of neutrons (6, 7, and 8 respectively).

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Mendeleev's Periodic Table

This page introduces Mendeleev's periodic table, which was a crucial step in the development of the modern periodic table.

The image shows the beginning of Mendeleev's table, highlighting the arrangement of elements into groups and series (periods).

Highlight: Mendeleev's table was revolutionary because it allowed for the prediction of undiscovered elements based on patterns in the table.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Periodic Table Structure

The periodic table organizes elements based on their atomic structure and properties.

Key points: • Elements are arranged in order of increasing atomic number • Rows are called periods, columns are called groups • The group number indicates the number of electrons in the outer shell • The period number indicates how many electron shells an atom has

Example: Lithium is in group 1, so it has 1 electron in its outer shell. It's also in period 2, meaning it has 2 electron shells.

Highlight: Elements in the same group have similar chemical and physical properties.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Structure of the Atom

The basic structure of an atom consists of a nucleus containing protons and neutrons, with electrons orbiting in shells around the nucleus. This fundamental arrangement is crucial for understanding atomic behavior and chemical properties.

Vocabulary: Subatomic particles - protons, electrons, and neutrons that make up an atom.

Highlight: Most of the atom's mass is concentrated in the nucleus, despite it being much smaller than the electron shells.

The document provides an information table detailing the location, relative mass, and charge of each subatomic particle. It's important to note that protons and neutrons have a much higher mass than electrons.

Example: If an atom were the size of a football field, the nucleus would be comparable to a single blueberry.

The overall charge of an atom is neutral because the number of protons (positive) equals the number of electrons (negative), canceling each other out.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Atomic Number and Mass Number

This section explains two fundamental concepts in atomic structure: atomic number and mass number.

Definition: Atomic number is the total number of protons within the nucleus of an atom, which is also equal to the number of electrons in a neutral atom.

The atomic number is represented by the smaller number on the periodic table.

Definition: Mass number is the total number of protons and neutrons within the nucleus of an atom.

The mass number is represented by the larger number on the periodic table.

Example: For fluorine (F), the atomic number is 9, and the mass number is 19.

(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par
(D Memo Structure of the atom = protons >= electrons. =neutrons proton Ineutron Lelectron -shell {these make Information table Subatomic par

Similar Content

AP Chemistry - Types of IMFs

Notes on the types of inter-molecular forces including London dispersion forces, dipole-dipole forces, hydrogen bonds, and ion-dipole forces. Includes lots of example problems.

0

45

0

Know Types of IMFs thumbnail

Chemistry - Binary Ionic Compound

This is about recognizing and naming Binary Ionic Compound

7

61

0

Know Binary Ionic Compound thumbnail

AP Chemistry - Covalent Bonds Worksheet

2 questions each with 2 sub-questions. The questions are solved with the correct solutions

0

5

0

Know Covalent Bonds Worksheet thumbnail

Can't find what you're looking for? Explore other subjects.

Knowunity is the # 1 ranked education app in five European countries

Knowunity was a featured story by Apple and has consistently topped the app store charts within the education category in Germany, Italy, Poland, Switzerland and United Kingdom. Join Knowunity today and help millions of students around the world.

Ranked #1 Education App

Download in

Google Play

Download in

App Store

Knowunity is the # 1 ranked education app in five European countries

4.9+

Average App Rating

13 M

Students use Knowunity

#1

In Education App Charts in 12 Countries

950 K+

Students uploaded study notes

Still not sure? Look at what your fellow peers are saying...

iOS User

I love this app so much [...] I recommend Knowunity to everyone!!! I went from a C to an A with it :D

Stefan S, iOS User

The application is very simple and well designed. So far I have found what I was looking for :D

SuSSan, iOS User

Love this App ❤️, I use it basically all the time whenever I'm studying