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Chemistry- study of physical properties of matter
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matter - anything that has mass or takes up space
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Areas of chemistry - organic, inorganic, biochemistry, analytical, and physical
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organic chemistry - study of chemicals containing carbon
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inorganic chemistry - study of chemicals not containing carbon
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biochemistry - study of processes taking place in organisms
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analytical chemistry - study of composition of matter
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physical chemistry - study of the mechanism, rate, and energy transfer that occurs when matter changes
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pure - pursuit of knowledge for itself
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applied - research directed to a specific goal
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macroscopic - visible to human eye
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microscopic - only visible with microscope
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Antoine Lavoisier - made chemistry become a measurable, observable science
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scientific method - observe, test hypothesis, and develop theories
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hypothesis - proposed explanation
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experiment - test a hypothesis
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pure - pursuit of knowledge for itself
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applied - research directed to a specific goal
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macroscopic - visible to human eye
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microscopic - only visible with microscope
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Antoine Lavoisier - made chemistry become a measurable, observable science
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scientific method - observe, test hypothesis, and develop theories
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hypothesis - proposed explanation
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experiment - test a hypothesis
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manipulated variable - variable changed intentionally during experiment
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responding variable - variable observed
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theory - well tested explanation for a broad set of observations
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scientific law - concise statement that summarises results of of observations and experiments
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extensive property - property depending on amount of matter in sample
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intensive property - property depending on type of matter in sample
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mass - a measure of amount matter (SI unit = kg)
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volume - a measure of space occupied by matter
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physical property - a substance that a person can measure without changing the material
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physical change - properties of a material change, but not composition
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vapour - a gas state of substance that is liquid or solid at room temp
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Solids - fixed volume, fixed shape, close particles
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Liquids - free shape, fixed volume, medium particle space
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Gas - free shape, easy to compress, far particles
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Addition and Subtraction of Sig Figs - round to the same number of decimal places as the measurement with the least number of decimal places
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Multiplication and Division - round answer to the same number of sig figs as the measurement with the least amount of sig figs
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measurement - a quantity that has both a number and a unit
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scientific notation - a number written as product of 2 numbers: a coefficient and 10/E to raised to a power, coefficient must be b/w 1 and 10 --- 6.789 x 1025
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accuracy a measurement of how close a measurement comes to the actual/true
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precision - a measure of how close a series of measurement are to each other
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sig figs - in measurement includes all digits that are known plus an estimated digit
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density -intensive property b/c it has to do with type of substance, not amount and density decreases with increasing temperatures
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density = mas/ volume in g/cm3
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reactant - substance present at start of chemical reaction
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product - substance present at end of chemical reaction
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participate - a solid that forms and settles out of liquid mixture
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Conservation of Mass - in any physical/chemical reaction, the mass of reactants must = the mass of the products ---- (10g H2 + 8g O2 = 18 H2O)
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temperature - kelvin (0C = 273 K)
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units of energy - is measured in calories or joules (joules is SI)
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conversion factor - ratio of equivalent measurement
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dimensional analysis - way to solve problems using units, dimensions, or measurements
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Atom - smallest particle of element that retains it identity in a chemical reaction
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Subatomic particles - protons, neutrons, electrons
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Electrons - negatively charged, located outside the nucleus, tiny (9.11 x10-24g), discovered by J.J. Thompson
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Protons - positively charged, located in the nucleus, large in comparison to electrons (1.67x10-24), discovered by Eugen Goldstein
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Neutrons - no charge, in nucleus, same mass as protons, discovered by James Chadwick
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Cathode Rays -the high-speed electrons emitted in a stream from the heated cathode of a vacuum tube
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J.J. Thompson's Plum Pudding Model - atoms were positively charged masses with negatively charged electrons distributed throughout the mass.
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Rutherford's Atomic Model/Theory - The atom is mostly empty space, there is small negatively charged nucleus, electrons are located outside of and around nucleus
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Democritus believed atoms were indivisible and indestructible.
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substance - uniform and definite composition of matter
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mixture - a physical blend of 2+ components (can be homogeneous or heterogeneous)
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heterogeneous - mixture not uniform throughout
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homogeneous - mixture uniform throughout
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phase - any part of a solution that is uniform throughout
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filtration - process separates a solid from liquid in hetero mix
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distillation - separates dissolved solids from liquid, which is boiled to produce vapour that has condensed into liquid
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1. every non zero digit is significant
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4. zeros at end of number and right of a decimal are significant
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2. zeros b/w non zero digits are significant
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5. zeros on right end of measurement that lie left of a decimal are not significant
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3. zeros appearing in front of non zeros (place holders) are not significant
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6. there are unlimited sig figs if: you are counting or situations involving exactly defined quantities
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Daltons' Atomic Theory
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1. all elements are composed of tiny indivisible particles called atoms
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2. atoms of same element are identical, atoms of any one element are different from those of another element
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3.atoms of different elements can mix together or chemically combine in simple whole number ratios
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4. chemical reactions occur when atoms are separated, joined, or arranged. atoms of one element are never changed into atoms of another element.
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Principle Energy Level
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Number of Sublevels
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Type of Sublevels
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n = 1
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1
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1s (1 orbital)
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n = 2
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2
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2s (1 orbital), 2p (3 orbital)
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n = 3
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3
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3s (1 orbital), 3p (3 orbital), 3d (5 orbital)
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n = 4
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4
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4s (1 orbital), 4p (3 orbital), 4d (5 orbital), 4f (7 orbital)
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Atomic Number - number of protons in nucleus in atom
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Mass Number - protons + neutrons = total mass #
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# neutrons = atomic # - mass#
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Energy Level N
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Maximum Number of Electrons
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1
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2
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2
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8
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3
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18
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4
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32
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element - simplest form of matter that has unique properties
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compound - substance containing 2+ elements in fixed proportion
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Quantum of Energy - is amount of energy required to move an electron from one energy level to another
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Orbit - each is associated with an energy level. The orbit an electron is in, determines energy of electron. Electrons can change orbits by gaining or losing energy
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Aufbau Principle - electrons occupy orbitals of lowest energy first
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*Electron Configuration - ways electron are arranged in various orbitals
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Pauli Exclusion Principle - atomic orbital can hold at most 2 electrons with opposite spin direction ↑↓
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Hunds Rule - electrons occupy orbitals of same energy in way that makes # of electrons w/ same spin direction as large as possible
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Atomic Number - number of protons in nucleus in atom
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Mass Number - protons + neutrons = total mass # (total # of of protons in nucleus of an element)
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# neutrons = atomic # - mass#
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isotopes - atoms same element that have same atomic number, but different atomic masses due to difference of neutrons
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atomic mass - a unit of mass to = 1/12 the mass of a carbon 12 atom
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period - horizontal row of elements in periodic table
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group - vertical column of elements in periodic table
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Cheatography n. The art of mapping complex subjects into clear, instantly navigable reference guides.
