![]() Law of Conservation of Mass = matter is neither created nor destroyed. In General Chemistry there are 3 Fundamental Chemical Laws to be aware of. Today we are going to discuss the Law of Conservation of Mass, the Law of Definite Proportions, the Law of Multiple Proportions, and Dalton's Atomic Theory. For example, it cannot explain the differences in the properties of the two carbon allotropes – diamond and graphite.3 - Chemical Quantities and StoichiometryĤ - Types of Chemical Reactions and Solution Stoichiometryħ - Quantum Mechanical View of the Atom, and Periodicityĩ - Covalent Bonding and Molecular Orbitalsġ0 - Liquids, Solids, and Intermolecular Forcesġ5 - Applications of Acid-Base Equilibriaġ6 - Spontaneity, Entropy, and Free Energyġ8 - Transition Metals and Coordination ChemistryĢ0 - An Introduction to Organic Chemistryġ - Structural, Bonding, Molecular PropertiesĢ - The Nature of Organic Compounds: Alkanes and Cycloalkanesģ - Stereochemistry of Alkanes and Cycloalkanes: 3-D Structures of MoleculesĤ - The Study of Organic Reactions: An Overviewġ0 - Substitution (SN2, SN1) and Elimination (E2, E1) Reactionsġ1 - Mass Spectrometry and IR Spectroscopyġ3 - Conjugated Systems and UV Spectroscopyġ5 - Electrophilic Aromatic Substitution (E.A.S.)ġ8 - Aldehydes and Ketones: Nucleophilic Addition ReactionsĢ0 - Carboxylic Acid Derivatives and Nucleophilic Acyl Substitution ReactionsĢ1 - Carbonyl Alpha-Substitution Reactions For example, argon and calcium have an atomic mass of approximately 40 amu.ĭalton’s theory could not explain the different allotropes of the same element. However, it was found that even atoms of different elements can have the same mass. For example, hydrogen, deuterium, and tritium are isotopes with different masses.ĭalton states that atoms of different elements can have different masses. However, it was later established that atoms of the same element can have different masses. However, we know an atom consists of electron, proton, and neutron.ĭalton states that atoms of a given element have precisely the same masses. ![]() Does not account for subatomic particlesĭalton stated that atoms are indivisible and cannot be further divided. While Dalton’s atomic theory laid the path toward the fundamental understanding of atoms and matter, it had a few demerits. However, both the sodium and chlorine atoms still exist. In the above example, sodium and chlorine combine to make salt. A chemical reaction is a rearrangement of atoms.ĭalton suggested that chemical reactions neither destroy nor create atoms. When they react, the Na and Cl atoms combine in a 1:1 ratio to form white crystals of sodium chloride (NaCl).Ĥ. The other is chlorine (Cl), which is a gas. One is sodium (Na), which is a highly reactive metal. For example, household common salt comprises two elements with varying physical and chemical properties. Compounds are formed from the combinations of two or more different types of atoms.ĭalton proposed that compounds comprise two or more atoms of different types. For example, an oxygen atom is different from a carbon atom.ģ. However, no two elements can have the same set of properties. Elements may share similar properties like boiling and melting points and electronegativity. All atoms of a given element are identical in mass and properties.ĭalton proposed that every single atom of a specific element is the same as that of every other element. ![]() Dalton proposed that all matter is made of tiny indivisible atoms, which he imagined as “solid and movable particles”.Ģ. The laws of conservation of mass and definite proportions can be explained using the concept of atoms. ![]()
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