Chapter 1
Chemistry- study of physical properties of matter |
matter - anything that has mass or takes up space |
Areas of chemistry - organic, inorganic, biochemistry, analytical, and physical |
organic chemistry - study of chemicals containing carbon |
inorganic chemistry - study of chemicals not containing carbon |
biochemistry - study of processes taking place in organisms |
analytical chemistry - study of composition of matter |
physical chemistry - study of the mechanism, rate, and energy transfer that occurs when matter changes |
Chapter 1
pure - pursuit of knowledge for itself |
applied - research directed to a specific goal |
macroscopic - visible to human eye |
microscopic - only visible with microscope |
Antoine Lavoisier - made chemistry become a measurable, observable science |
scientific method - observe, test hypothesis, and develop theories |
hypothesis - proposed explanation |
experiment - test a hypothesis |
Chapter 1
pure - pursuit of knowledge for itself |
applied - research directed to a specific goal |
macroscopic - visible to human eye |
microscopic - only visible with microscope |
Antoine Lavoisier - made chemistry become a measurable, observable science |
scientific method - observe, test hypothesis, and develop theories |
hypothesis - proposed explanation |
experiment - test a hypothesis |
manipulated variable - variable changed intentionally during experiment |
responding variable - variable observed |
theory - well tested explanation for a broad set of observations |
scientific law - concise statement that summarises results of of observations and experiments |
Chapter 2
extensive property - property depending on amount of matter in sample |
intensive property - property depending on type of matter in sample |
mass - a measure of amount matter (SI unit = kg) |
volume - a measure of space occupied by matter |
physical property - a substance that a person can measure without changing the material |
physical change - properties of a material change, but not composition |
vapour - a gas state of substance that is liquid or solid at room temp |
Solids - fixed volume, fixed shape, close particles |
Liquids - free shape, fixed volume, medium particle space |
Gas - free shape, easy to compress, far particles |
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Chapter 3
Addition and Subtraction of Sig Figs - round to the same number of decimal places as the measurement with the least number of decimal places |
Multiplication and Division - round answer to the same number of sig figs as the measurement with the least amount of sig figs |
12.345 + 6.1 = 18.4
(1.502)(3.8) = 5.7076 = 5.7
Chapter 3
measurement - a quantity that has both a number and a unit |
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 |
accuracy a measurement of how close a measurement comes to the actual/true |
precision - a measure of how close a series of measurement are to each other |
sig figs - in measurement includes all digits that are known plus an estimated digit |
Error = Experimental Value - Accepted Value
% = | error | / accepted value x 100%
Chapter 3
density -intensive property b/c it has to do with type of substance, not amount and density decreases with increasing temperatures |
density = mas/ volume in g/cm3 |
Chapter 2
reactant - substance present at start of chemical reaction |
product - substance present at end of chemical reaction |
participate - a solid that forms and settles out of liquid mixture |
Conservation of Mass - in any physical/chemical reaction, the mass of reactants must = the mass of the products ---- (10g H2 + 8g O2 = 18 H2O) |
Clues that a chemical change has ocurred:
- transfer energy
- color change
- production of gas
- participate forms
Chapter 3
temperature - kelvin (0C = 273 K) |
units of energy - is measured in calories or joules (joules is SI) |
conversion factor - ratio of equivalent measurement |
dimensional analysis - way to solve problems using units, dimensions, or measurements |
5 Base of SI
meter = length
kilograms = mass
kelvin = temperature
second = time
mole = number of molecules
litre = volume
1 J = 0.2390 cal
1 cal = 4.184 Joules
mole = number of molecules
litre = volume
Converting - 8.351 g to mg
smaller = multiply
bigger = divide
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Chapter 4
Atom - smallest particle of element that retains it identity in a chemical reaction |
Subatomic particles - protons, neutrons, electrons |
Electrons - negatively charged, located outside the nucleus, tiny (9.11 x10-24g), discovered by J.J. Thompson |
Protons - positively charged, located in the nucleus, large in comparison to electrons (1.67x10-24), discovered by Eugen Goldstein |
Neutrons - no charge, in nucleus, same mass as protons, discovered by James Chadwick |
Cathode Rays -the high-speed electrons emitted in a stream from the heated cathode of a vacuum tube |
J.J. Thompson's Plum Pudding Model - atoms were positively charged masses with negatively charged electrons distributed throughout the mass. |
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 |
Democritus believed atoms were indivisible and indestructible. |
Chapter 2
substance - uniform and definite composition of matter |
mixture - a physical blend of 2+ components (can be homogeneous or heterogeneous) |
heterogeneous - mixture not uniform throughout |
homogeneous - mixture uniform throughout |
phase - any part of a solution that is uniform throughout |
filtration - process separates a solid from liquid in hetero mix |
distillation - separates dissolved solids from liquid, which is boiled to produce vapour that has condensed into liquid |
Sig Fig Rules
1. every non zero digit is significant |
4. zeros at end of number and right of a decimal are significant |
2. zeros b/w non zero digits are significant |
5. zeros on right end of measurement that lie left of a decimal are not significant |
3. zeros appearing in front of non zeros (place holders) are not significant |
6. there are unlimited sig figs if: you are counting or situations involving exactly defined quantities |
Chapter 4
Daltons' Atomic Theory |
1. all elements are composed of tiny indivisible particles called atoms |
2. atoms of same element are identical, atoms of any one element are different from those of another element |
3.atoms of different elements can mix together or chemically combine in simple whole number ratios |
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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Summary of Principle Energy Levels, and, Orbitals
Principle Energy Level |
Number of Sublevels |
Type of Sublevels |
n = 1 |
1 |
1s (1 orbital) |
n = 2 |
2 |
2s (1 orbital), 2p (3 orbital) |
n = 3 |
3 |
3s (1 orbital), 3p (3 orbital), 3d (5 orbital) |
n = 4 |
4 |
4s (1 orbital), 4p (3 orbital), 4d (5 orbital), 4f (7 orbital) |
Chapter 4
Atomic Number - number of protons in nucleus in atom |
Mass Number - protons + neutrons = total mass # |
# neutrons = atomic # - mass# |
Maximum Numbers of Electrons
Energy Level N |
Maximum Number of Electrons |
1 |
2 |
2 |
8 |
3 |
18 |
4 |
32 |
Chapter 2
element - simplest form of matter that has unique properties |
compound - substance containing 2+ elements in fixed proportion |
Compounds can be broken down, but elements cannot.
Scientists use chemical symbols to represent elements.
Chemical symbols are always 1 or 2 letters with first letter capitalized
Chapter 5
Quantum of Energy - is amount of energy required to move an electron from one energy level to another |
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 |
Aufbau Principle - electrons occupy orbitals of lowest energy first |
*Electron Configuration - ways electron are arranged in various orbitals |
Pauli Exclusion Principle - atomic orbital can hold at most 2 electrons with opposite spin direction ↑↓ |
Hunds Rule - electrons occupy orbitals of same energy in way that makes # of electrons w/ same spin direction as large as possible |
Chapter 4
Atomic Number - number of protons in nucleus in atom |
Mass Number - protons + neutrons = total mass # (total # of of protons in nucleus of an element) |
# neutrons = atomic # - mass# |
isotopes - atoms same element that have same atomic number, but different atomic masses due to difference of neutrons |
atomic mass - a unit of mass to = 1/12 the mass of a carbon 12 atom |
period - horizontal row of elements in periodic table |
group - vertical column of elements in periodic table |
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