Chemistry 1A: Chapter 2 Page | 1 Chapter 2: Atoms and Elements Homework: Read Chapter 2: Work out sample and practice problems in textbook. Check for the MasteringChemistry.com assignment and complete before due date Early Ideas on Matter: Philosophers (Chinese, Greeks, etc) has speculated about the nature of “stuff” Leucippus (fifth century BC) and his student Democritus (460-370 BC) first suggested the material world when broken down to the extreme would consist of indivisible particles called atomos, meaning indivisible. Alchemists through the middle ages physically experimented with matter aiming to create gold from base metals and an elixir for everlasting life. Englishman Robert Boyle (1627-1691) is generally credited as the first to study the separate science we call chemistry and the first to perform rigorous experiments. Antoine Lavoisier (1743-1794) discovered the mass of combustion products exactly equals the mass of the starting reactants. Law of Mass Conservation (Law of Conservation of Matter); Mass is neither created nor destroyed in chemical reactions Joseph Proust (1754-1826) studied copper carbonate, the two tin oxides, and the two iron sulfides. He made artificial copper carbonate and compared it to natural copper carbonate, showing that each had the same proportion of weights between the three elements involved (Cu, C, O). He showed that no intermediate indeterminate compounds exist between the two tin oxides or the two iron sulfides. Law of Definite Proportions (Law of Constant Composition); Elements combine together in specific proportions. All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. These early ideas led to the foundation steps in atomic theory. Atomic theories explain the behavior of atoms. We will cover Dalton’s Indivisible atom, JJ Thomson’s Plum Pudding model, Rutherford’s Nuclear model of the atom, the Bohr’s Quantum (orbit) model that mathematically only works for one electron systems and the Orbital Wave Mechanical model. The first three models are found in Chapter 2 while the last two are found in Chapters 7
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C h e m i s t r y 1 A : C h a p t e r 2 P a g e | 1
Chapter 2: Atoms and Elements
Homework:
Read Chapter 2: Work out sample and practice problems in textbook.
Check for the MasteringChemistry.com assignment and complete before due date
Early Ideas on Matter:
Philosophers (Chinese, Greeks, etc) has speculated about the nature of “stuff”
Leucippus (fifth century BC) and his student Democritus (460-370 BC) first
suggested the material world when broken down to the extreme would consist of
indivisible particles called atomos, meaning indivisible.
Alchemists through the middle ages physically experimented with matter aiming to
create gold from base metals and an elixir for everlasting life.
Englishman Robert Boyle (1627-1691) is generally credited as the first to study the
separate science we call chemistry and the first to perform rigorous experiments.
Antoine Lavoisier (1743-1794) discovered the mass of combustion products exactly
equals the mass of the starting reactants.
Law of Mass Conservation (Law of Conservation of Matter); Mass is neither
created nor destroyed in chemical reactions
Joseph Proust (1754-1826) studied copper carbonate, the two tin oxides, and the two
iron sulfides. He made artificial copper carbonate and compared it to natural copper
carbonate, showing that each had the same proportion of weights between the three
elements involved (Cu, C, O). He showed that no intermediate indeterminate
compounds exist between the two tin oxides or the two iron sulfides.
Law of Definite Proportions (Law of Constant Composition); Elements
combine together in specific proportions. All samples of a given compound,
regardless of their source or how they were prepared, have the same
proportions of their constituent elements.
These early ideas led to the foundation steps in atomic theory. Atomic theories explain
the behavior of atoms. We will cover Dalton’s Indivisible atom, JJ Thomson’s Plum
Pudding model, Rutherford’s Nuclear model of the atom, the Bohr’s Quantum (orbit)
model that mathematically only works for one electron systems and the Orbital Wave
Mechanical model. The first three models are found in Chapter 2 while the last two are found in Chapters 7