Chemistry Notes PDF

Health and Medicine Sanitation systems Surgery with anesthesia VACCINES Antibiotics Gene therapy Energy and the Environment Fossil fuels Solar energy Nuclear energy Materials and Technology Polymers, ceramics, liquid crystals Room-temperature superconductors Molecu...

Health and Medicine Sanitation systems Surgery with anesthesia VACCINES Antibiotics Gene therapy Energy and the Environment Fossil fuels Solar energy Nuclear energy Materials and Technology Polymers, ceramics, liquid crystals Room-temperature superconductors Molecular computing Food and Agriculture Genetically Modified crops (GMOs) Bio pesticides (eg. Bacillus thuringensis) Organic fertilizers Dalton's Atomic Theory Law of Multiple Proportions Law of Conservation of Mass **Cathode Ray Tube** - J.J. Thomson, measured mass/charge of electrons **Millikan's Experiment** - Measured mass of electrons **Thomson's Model** - Positive charge spread around the sphere **Rutherford's Experiment** - atoms positive charge is concentrated in the nucleus -proton (p) has opposite (+) charge of electron (-) -mass of p is 1840 x mass of e- (1.67 x 10-24 g) **Rutherford's Model of** **the Atom** - "If the atom is the Houston Astrodome, then the nucleus is a marble on the 50-yard line." **Chadwick's Experiment**- Neutron (n) is neutral (charge = 0) mass p ≈ mass n ≈ 1840 x mass electrons - - = atomic number (Z) + number of neutrons - numbers of neutrons in their nuclei **Isotopes of Hydrogen**: (1) Protium (2) Deuterium (3) Tritium A **molecule** is an aggregate of two or more atoms in a definite arrangement held together by chemical forces. A **diatomic molecule** contains only two atoms A **polyatomic molecule** contains more than two atoms An **ion** is an atom, or group of atoms, that has a net positive or negative charge. **cation** -- ion with a positive charge it becomes a cation. **anion** -- ion with a negative charge it becomes an anion. A **monatomic** **ion** contains only one atom A **polyatomic** **ion** contains more than one atom A **molecular formula** shows the exact number of atoms of each element in the smallest unit of a substance An **empirical formula** shows the simplest whole-number ratio of the atoms in a substance **ionic compounds** consist of a combination of cations and an anions The formula is usually the same as the empirical formula The sum of the charges on the cation(s) and anion(s) in each formula unit must equal zero An **acid** can be defined as a substance that yields hydrogen ions (H+) when dissolved in water. For example: HCl gas and HCl in water An **oxoacid** is an acid that contains hydrogen, oxygen, and another element. HNO3 nitric acid H2CO3 carbonic acid H3PO4 phosphoric acid A **base** can be defined as a substance that yields hydroxide ions (OH-) when dissolved in water. NaOH sodium hydroxide KOH potassium hydroxide Ba(OH)2 barium hydroxide **Organic chemistry** is the branch of chemistry that deals with carbon compounds