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Semester 1 Final

Chemistry Unit 1-4 Final Review; NO UNIT 5

Proton positively charged atom
Atom a small molecule or particle of a chemical element
Mass Number the total number of protons and neutrons in a nucleus
Atomic Mass Units a unit of mass used to measure atoms
Electron negatively charged atom
Isotopes two of the same atoms with a different number of neutrons in the nucleus
Atomic Number this is how the elements are numbered on the pt; it tells you how many protons an atom has
Atomic Mass this is present of the pt; it tells you how much that element weighs; measured in amu
Nucleus small, dense region consisting of protons and neutrons at the center of an atom
Neutron neutral, no charge atoms; they "orbit" the nucleus in the electron cloud
Cation a positively charged ion
Anion a negatively charged ion
Transitional Metals located in the center of the pt (section d)
Non-Metals dull, brittle elements that are not good conductors of energy or heat
Inner Transitional Metals the last two secluded rows of the pt (f section)
Group 1 alkali metals
Group 2 alkaline earth metals
Group 17 halogens
Group 18 noble gases
Valence Electrons electrons in the outer-most shell that are available for bonding
Polar Covalent a bond in which electrons are not shared evenly
Non-Polar Covalent a bond in which electrons are shared evenly
Octet Rule this states that atoms will give, take, or share electrons in order to get eight electrons in their outer shell
Scientific Method 1. identify the problem 2. observe the problem 3. hypothesis 4. explore 5. conclusion
Atomic Radius the distance from the nucleus to the outer-most electron; gets larger as you go up, gets smaller as you go left to right
Ionization Energy the amount of energy needed to remove an electron from the atom; gets smaller as you go down, gets larger as you go left to right
Electron Affinity this is an atom's "want" or "like" for electrons; gets smaller as you go down, gets larger as you go left to right
Electronegativity an atom's ability to attract electrons, how sexy it is; gets smaller as you go down, gets larger as you go left to right
Ion positively or negatively charged atoms in which electrons have been gained or lost, protons never change
Metallic Bond bonds made between metals; there are always always free electrons floating around
Matter anything that has mass and volume
Pure Substance can not be physically broken down; definite composition
Mixture can be physically broken down; no definite composition
Homogeneous looks like one thing; ex. milk
Heterogeneous looks like two things; ex. gravel
Compounds two or more chemically bonded elements
Metalloids have properties of both metals and non-metals; located on the stair-step
Metals hard, dense elements with a high luster (shiny); they can be bent (malleable), pulled (ductile), and they are good conductors of electricity of heat
Polyatomic Ions a covalent bonded set of two or more atoms that behave as a single unit
Chemical Formula representation of compounds and/or elements in a reaction
Law of Definite Proportions a given chemical compound always contains the same elements in the exact same proportions by mass
Element the purest form; cannot be broken down into something with properties
Solution both substances are in one state of matter; uses distillation to separate
Colloid when the substances are in two different states, but one is too small to see or is filtered well; ex. dust in air
Suspension when the substances are in two different states of matter; will generally settle over time; ex. muddy water; use filtration to separate
Distillation a physical process that uses a substances' boiling point to separate the mixture
Tyndall Effect a strong light that shows the particles
Electrolysis the use of electricity to break bonds
Super Saturated Solution a solution that contains more than the maximum amount of solute that is capable of being dissolved at a given temperature
Representative Elements elements that have a roman numeral followed by an A; all elements in the S & P sections
Quanta an amount of energy needed to jump to the next orbit / energy level
Energy Levels seven levels in which the electron orbits; lowest level called the ground state... - electrons must get excited to jump!
photons light
periodic law when the periodic table was organized by the increasing atomic number, periodic pattern appear
alloy when two or more metals have bonded
hydrogen bonding when hydrogen bonds to another non-metal that has a higher electronegativity; found in most living things
ionic bonding when a cation and anion bond; when a metal bonds with a non-metal or polyatomic
covalent bonds bonds made between non-metals; electrons are always shared so they are very strong
dipoles when a small charge occurs from the uneven sharing of electrons
dipole moment the area in which a small charge occurs from the uneven sharing of electrons
definite composition the statement that in a pure compound the elements are always combined in fixed proportions by weight
filtration the mechanical or physical process used for the separation of one substance from another
Democritus - First to try and explain matter - the Greeks were the first to contemplate the atom
John Dalton - First to try and describe the atom - Tiny marbles - Atoms indivisible (false)
JJ Thompson - Second to purpose an atomic theory - tested the particles (atoms) found with magnets - plum pudding theory; + overall, - particles float around
Rutherford - correctly explain the structure of the atom - gold foil experiment - small, dense, + center —> nucleus; atoms must be neutral
Bohr - studied Rutherford’s atom - quanta/energy; and energy levels - atomic spectra: fingerprints of that element, light given off
Mendeleev - first to create a PT - based on atomic masses - made predictions of future elements
Moseley - created modern PT sorted by atomic number - periodic law - used X-rays to determine # of protons
Created by: 584jth02
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