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Chemistry
the study of chemicals and the study of matter and its changes
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5 steps of scientific method
- 1. Observations
- 2. Hypothesis
- 3. Experimentation ◦ (repeat of steps 1-3 many times)
- 4. Law
- 5. Theory
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Qualitative vs quantitative
Qualitative-observed (color,
Quantitative-recorded (numerical data obtained through measurements)
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Mixtures
A combination of 2 or more substances in which the substances retain their distinct identities
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Hetero mixture
composition of mixtureis not the same throughout (it is not uniform
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Homo mixture
composition of mixture is the same throughout
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Elements
cannot be separated into simpler substances by chemical means
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Compounds
composed of units of elements chemically bound to each other in a fixed proportion
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Physical vs chemical properties
- Physical properties = measured or observed without changing the composition or identity of the substance
- ie. Color, Melting point, Boiling point
- Chemical properties = require a chemical change of the substance to observe these properties
- ie. Acid/base, Combustion, precipitation
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Extensive and intensive properties
- Extensive property = dependent on howmuch matter is being studied. Property depends on the extent of the matter andcan be added together
- ie. Mass, Volume
Intensive property = does NOT depend on the quantity of matter being studied. Values cannot be added together ie. Temperature, Density
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Solid, Liquid, Gas
- Solid-molecules not moving; in a fixed position
- Liquid-molecules "roll over each other""
- Gas-no attraction to other molecules
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Endothermic Phase Change
All require energy input:
- Solid to liquid◦ Called melting ◦ Temperature of change is called melting point
- Liquid to gas ◦ Called boiling, evaporation or vaporization ◦ Temperature of change is called boiling point ◦
- Solid to gas ◦ Called sublimation
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Exothermic Phase change
All require energy release
- Gas to liquid◦ Called condensation ◦ Temperature of change is called boiling point
- Liquid to solid ◦ Called freezing ◦ Temperature of change is called freezing point (which isthe same temperature as the melting point)
- Gas to solid ◦ Called deposition
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Temperature comparisons
oR Rankine
oF Farhenheit
oC Celsius
K Kelvin
oR and oF have same degree size, but different zero points
oC and K have same degree size, but different zero points
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Dalton's Atomic Theory
- 1. each element is composed of atoms
- 2. atoms of a given element are identical, atomsof different elements are different in somefundamental way
- 3. chemical compounds are formed when atomscombine with each other; a compound always hasthe same relative number and types of atoms
- 4. chemical reactions involve reorganization ofatoms, not a change in the identity of the atomsthemselves
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Democritus and Leucippus
- Atomic scissors
- Indivisible particles that retained properties of thatelement called atoms
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Antoine Lavoisier
Law of Conservation of Mass
mass is neither created nor destroyed by a chemical reaction
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Joseph Louis Proust
Law of Definite Proportions (or Law of Constant Composition)
Given compound contains exactly the same proportion of elements by mass
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Modern atomic theory
- J.J. Thomson – electron as first discoveredsubatomic particle
- Robert Millikan – electron charge magnitudeand mass
- Earnest Rutherford – proton existence verifiedas second subatomic particle
- James Chadwick – neutron as third subatomicparticle
- Rutherford – protons and neutrons located innucleus and electrons in electron cloud
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Atomic mass
weighted average atomic mass of all isotopes for that element
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Special groups on PT
- Group 1A- Alkali metals
- Group 2A- Alkaline earth metals
- Group 7A-halogens
- Group 8A-noble gases
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Metals
- Tend to lose electrons to form cations
- Shiny, lusterous
- Conduct heat and electricity
- Malleable and ductile
- Most are solids at room temperature
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Non-metals
- Tend to gain electrons to form anions
- Not shiny, not lusterous
- Not conduct heat or electricity
- Not malleable and not ductile
- Most are liquids or gases at room temperature
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Cations
= ions with a net positive charge, resultfrom electron loss
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Anions
= ions with a net negative charge, resultfrom electron gain
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Type I ion
- Type I indicates that the metal only forms ONE type of cation
- All group 1A and 2A metals
- Aluminum (Al3+) Zinc (Zn2+) Silver (Ag+)
- Ends with "ide"
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Type II ions
Type II indicates that the metal forms more than one type of cation
- Two different systems for doing this:
- Older system is to modify the Latin name of the element to indicate:
- Lesser with the suffix –ous Greater with the suffix – ic
- Newer system is to use Roman numeral to specify the ion used
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Binary Acid
- Those composed of just hydrogen cation and single anion
- EX: HCl is hydrochloric acid
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Oxyacids
Those composed of hydrogen cation/s plusoxyanions (polyatomic anions that containoxygen)
- -ite suffix is the lesser and becomes –ous acid
- -ate suffix is the greater and becomes –ic acid
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Numeric prefixes
- Mono
- Di
- Tri
- Tetra
- Penta
- Hexta
- Hepta
- Octa
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