Chemistry Unit 1 Review

Anything that has mass and takes up space

Chemical Properties (properties of matter as it exist) Chemical Properties (properties that we see as the molecules change) Chemical vs. Physical (chem-molecules change, phys-molecules dont change)

Something with the same thing throughout

Cannot be broken down, smallest atom

Combinations of one or more elements (no longer has characteristics of original element)

Combinations of one or more substances

The same throughout

Not the same throughout

Are Homogenous mixtures

Copper, Silver, gold malleable, best with electricity conduction

Exist in all three forms; solid, gas, liquid. Not malleable, heat poorly, no electricity

The process of knowing the natural universe

How we gain knowledge, systemic

Body of knowledge built off previous knowledge applied to experiment. Educated guess

Ways of testing hypothesis, controlled environments

General information

Specific statements, never to be violated

Birth out of Alchemy

Descriptive, no mathematical component ex.. A&P)

Implies a measurement or an amount of something. (ex.. Chemistry)

Fundamental Units Derived Units

1) Any nonzero is significant 2) Any zero between nonzeros is a sig fig 3) Zeros at the end of a number with a decimal are significant

1) Align the decimal points 2) Add or subtract 3) Round the final answer to the rightmost column in which all numbers have significant figures

Multiply or divide the number 2) Determine the number of sig figs in each of the original numbers 3) Round the final answer to the same number of sig figs as the original number with the fewest significant figures

1) Celcius 2) Fahrenheit 3) Kelvin

Intensive physical property Measures how tightly packed matter is Is a ratio of Mass & Volume

All these combined give matter

Smallest unit of an element (extremely small)

Smallest substance of an element (ex..H2O)

Building Blocks of matter (- First Concept: Democritus & Leucippus) ( - Modern: John Dalton) ( * All matter composed of atoms) (* Atoms of the same elements are the same, atoms of) (different elements are different) (* Atoms combine in whole number ratios to form compunds)

Some properties of both metals & non metals

Atoms or group of atoms that has acquired either a (+) or (-) charge

Electron- JJ Thomson (1806) Proton- Crooke Neutron- James Chadwick Nucleus- Rutherford (1911)

Positive charge located in core Electrons located in the large area of atom (Atom was basically empty)

Atomic Number- (Z) The number of protons Mass Number- (A) Number of protons plus neutrons (This number can change if neutrons change)

Atom from the same element with different number of neutrons

Light given off certain atoms

Groups of atoms that come together to form molecules (There are 7)

O2

Made of only two non-metals

Use a prefix to identify how many atoms are present; omit- mono

1) Always use a prefix 2) Stem name of atom 3) -ide ending

water (H2O) Ammonia (NH4) Methane (CH4)

1 atomic mass unit is 1/12 the mass of a carbon 12 atom

Takes into account the naturally occurring elements

1.00728 u

1.00866 u

0.000549 u

Sum of the masses of all the individual atoms (multiply the molar mass of each element by the subscript of that element in the molecular formula)

Positive charged ion (lose e-)

Negative charged ion (gain e-)

Name ion same as the atom and add the word ion to the end (ex.. Na+ - Sodium Ion)

Use stem name and change ending of name to -ide ending (ex.. o2- Oxide Ion)

Cation written first Anion written second Balanced so the charges equal zero (use subscripts to balance number of each type of ion)

Combine name of cation and anion Cation- Name of element Anion- stem name of element with -ide ending (no prefixes used with ionic compounds)

Variable Valence- more than one possible charge, always positive. (FeCl3 > Iron III Chloride)

Groups of atoms that have a charge associated with them, have unique names

Must have an H+ & one more element to be an acid & aqueous, dissolved in water (acids are sour, react with certain metals & emit gas)

Hydro- prefix -ic acid- suffix Stem name of element other than H

No prefix Suffix based on ending of polyatomic ion * -ate > -ic acid * -ite > -ous acid Stem name is based on name of polyatomic ion

Compounds withOH when dissolved in water' Named as ionic compounds - Hydroxide is the ion

Reactions of the Nucleus

Discovered radiation emitted from uranium (glows when exposed to sunlight)

Process of emitting energy and particles from nucleus of atom (reaction involves the nucleus; rearranges the protons and/or neutrons)

Energy and particles emitted from the nucleus

Alpha Particles Beta Particles Positrons Gamma Rays

Given off & a new element is formed by emission of either Alpha, Beta, Positron, etc.. (writing nuclear reaction of these reactions:) (-radioactive nucleus (parent isotope) > new nucleus + radiation) (daughter isotope)

Decay emitting alpha particles U-238 decays to Th-234 by emitting alpha particles

Radioactive decay by emitting beta particles Formation of Beta particle - Neutron is converted to a proton - Electron emitted from the nucleus Mass number- unchanged Atomic number increases by one

Same mass as an electron, emitted by nucleus Mass number stays the same Atomic number decreases by one (PET Scans)

Pure Energy Given off in conjunction with Alpha or Beta emitter Forms a more stable nucleus of the same element

Mass- must be equal on both sides of arrow Atomic number- must be equal on both sides of arrow

Time it takes for 1/2 of a radioactive sample to decay Half life gives an indication of stability

Equal to 1 decay per second

Equal to 3.7 x 10^10 decays per second

Equal to 0.01 J/g of tissue

Unit of radioactive exposure that includes a factor to account for the type of radioactivity (rem=rad*factor)

Geiger counter

1 - no detectable effect 20 - increased risk of some cancers 100 - damage to bone marrow 200- 300 - visible burns >300 - loss of white blood cells 600 - death

Not a good source of energy Einstein - mass and energy are alternate aspect of the same entity E=mc^2 (energy=mass(speed)^2)

Much more energy produced then by radioactive decay The missing mass is converted to energy (Reaction can be sustained; a chain reaction can occur when 3 N are produced thus building energy, converted to kg)

Energy source- Hydrogen; less radioactive waste Takes place continually in the sun Produces more energy than fission (impossible temp to maintain, 100 million c.)