Atoms And Molecules Class 9 Science One Shot | NCERT Chapter 3 | CBSE Science | Chemistry
LearnoHub - Class 9,10・70 minutes read
Atoms are essential building blocks that can combine to form molecules. The Dalton Atomic Theory introduced symbols to represent elements and simplified identifying different units of matter.
Insights
- Atoms are the fundamental building blocks of matter, composed of a nucleus containing protons and neutrons orbited by electrons. The representation of atoms through symbols simplifies the identification of elements and ensures consistency in portraying the basic units of matter.
- The Laws of Chemical Combination, including the Law of Conservation of Mass and the Law of Constant Proportion, explain the behavior of atoms in chemical reactions. These laws dictate that atoms are indivisible, have unique properties, and combine in fixed ratios to form compounds, highlighting the foundational principles of chemistry.
Get key ideas from YouTube videos. It’s free
Recent questions
What are atoms made of?
Atoms consist of a dense nucleus with electrons.
Related videos
Physics Wallah Foundation
ATOMS AND MOLECLUES in 1 Shot || FULL Chapter Coverage (Concepts+PYQs) || Class 9th Chemisty
By: Rachel Taylor
Atoms, Elements, and Molecules
Free Animated Education
What Distinguishes Compounds from Molecules?
Pradeep Giri 11th and 12th Academy
11TH CHEMISTRY|1.SOME BASIC CONCEPTS OF CHEMISTY|LECTURE-8| DALTON ATOMIC THEORY|PRADEEP GIRI SIR
Revision Monkey
Atoms, Elements, Compounds and Mixtures
Summary
00:00
"Atoms: Building Blocks and Symbolic Representations"
- Atoms are small but essential building blocks that come together to form molecules, much like bricks forming walls and buildings.
- Maharishi Kanad, an Indian philosopher around 500 BC, proposed that matter is divisible into small particles called atoms.
- Greek philosophers like Democritus suggested that atoms are indivisible particles, but later research revealed their internal structure.
- Atoms consist of a dense, positively charged nucleus containing protons and neutrons, with electrons orbiting around it.
- John Dalton introduced the Dalton Atomic Theory, suggesting elements be represented by symbols indicating specific quantities of the element.
- Initially, symbols for elements were complex, but later simplified to one or two letters, derived from the element's name.
- Elements were named based on their properties or where they were first discovered, with symbols reflecting their names or Latin/Greek origins.
- Symbols for elements typically use the first letter capitalized and the second letter in lowercase, with exceptions for elements like zinc (Zn) and chlorine (Cl).
- The representation of atoms through symbols helped in simplifying the identification and understanding of different elements.
- The conventions for symbolizing elements were established to ensure consistency and clarity in representing the fundamental units of matter.
16:34
Dalton's Theory: Atoms and Chemical Laws
- In 1808, Dalton introduced the theory of atoms, listing all their properties.
- Matter is composed of indivisible particles called atoms.
- Atoms cannot be created or destroyed during chemical reactions.
- Atoms of the same element have identical properties.
- Atoms of different elements have different masses and properties.
- Different atoms combine in fixed ratios to form compounds.
- For example, hydrogen and oxygen combine in a 2:1 ratio to form water.
- Dalton's theory was successful due to explaining the Laws of Chemical Combination.
- The Law of Conservation of Mass states that mass is conserved in chemical reactions.
- The Law of Constant Proportion ensures that the relative number and kind of atoms in a compound remain constant.
32:09
"Standard Weights, Atoms, and Molecules Explained"
- Joe, a shopkeeper, uses standard weights like 500 grams and 1 kg to measure items.
- When Joe needs half a kilo of tomatoes, he adds tomatoes until the weight is close to the standard weight.
- The concept of standard weight is used to determine the weight of items relative to a standard reference.
- The atomic mass unit (u) is defined as 1/12th the mass of a carbon-12 atom.
- Isotopes are atoms with the same atomic number but different atomic masses.
- Noble gases are unreactive atoms that do not combine easily with other elements.
- Atoms are unable to exist independently and tend to combine with other atoms to form molecules.
- Molecules are formed when two or more atoms combine through strong attractive forces.
- Molecules of elements consist of atoms of the same type, while molecules of compounds contain atoms of different elements in a specific ratio.
- The atomicity of a molecule refers to the number of atoms it contains, with examples like H2 having an atomicity of two.
47:12
"Water, Ions, and Valency in Chemistry"
- Water is composed of two different types of atoms, hydrogen and oxygen, in a 2:1 ratio.
- The mass ratio of hydrogen to oxygen in water is 1:8.
- The atomic mass of hydrogen is 1u, while the atomic mass of oxygen is 16u.
- A water molecule (H2O) consists of two hydrogen atoms and one oxygen atom, resulting in a 2:1 ratio.
- Ions are charged species formed when metals and non-metals combine, with one being positively charged and the other negatively charged.
- Positive ions are called cations, while negative ions are called anions.
- Examples of ions include sodium ion (Na+) and chloride ion (Cl-).
- Some elements, like copper and iron, can have multiple valencies, denoted by Roman numerals in brackets.
- Valency is the combining capacity of an element, determining how many bonds it can form with other atoms.
- Valency dictates the composition of compounds, with elements combining based on their valencies.
01:02:45
"Writing Chemical Formulas: Rules and Examples"
- Learning to write chemical formulas involves understanding molecular mass and practicing with atoms and molecules.
- Chemical formulas are simplified representations of compounds using symbols for elements.
- Symbols of elements are written with metals on the left and non-metals on the right.
- Polyatomic ions are enclosed in brackets to indicate the number of ions present.
- Following specific rules, such as crossing over valences, helps in writing accurate chemical formulas.
- Examples like sodium chloride (NaCl) and magnesium chloride (MgCl2) illustrate the process of writing chemical formulas.
- Understanding valencies and crossing over valences is crucial in determining chemical formulas.
- Examples like calcium oxide (CaO) and sodium nitrate (NaNO3) demonstrate the application of rules in writing chemical formulas.
- Naming compounds based on their chemical formulas involves identifying the ions present and following the reverse steps of writing formulas.
- Molecular mass is calculated by summing the atomic masses of all atoms in a molecule, while unit mass formula is used for compounds with charged ions.
01:19:49
Calculating Formula and Molecular Masses in Chemistry
- To calculate the formula unit mass, add the atomic masses of the elements involved, such as sodium and chlorine, to get the total mass, like 58.5 u for NaCl.
- Molecular mass is determined by multiplying the atomic mass of each element by the number of atoms present, for example, O2 has a molecular mass of 32 u.
- For compounds like ZnO2 and K2CO3, the formula unit mass is found by adding the atomic masses of the elements in the formula, like 62 u for Na2O.
