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Chem. chc flex exam

Chemistry

QuestionAnswer
matter anything that takes up space
physical properties describes matter and measured or observed
chemical Properties anything that undergoes a chemical reaction irreversible
Physical Change A change that changes physical property
Chemical change chemical reaction
Solid Atom packed tightly, don't move, definite volume, and definite shape.
Liquid Particles packed loosely, do move, definite volume, and indefinite shape.
Gas atoms packed extremely loosely, do move, indefinite volume and shape.
Law of conservation of mass matter is not created or destroyed
Mixtures Physically combined and can be physically separated
Homogenous Mixtures looks same throughout; can't see components
Heterogenous Mixtures not the same can see components of the mixture
Substance are element or compound and are pure
Democritus made of small indivisible particles
Rutherford Gold foil experiment discovered the nucleus
Dalton father of atom theory it had 6 postulates
Proton positive
Neuotron no charge
Electron negative
atomic number number of protons
Mass number Neutrons+Protons
Bohr electrons exist in perfect circular orbit
GMM does not define path for electrons
electron configuration what orbitals your electrons are in
Aufbau rule lowest energy filled first
hund rule you must completely filled lower levels before moving on
Pauli rule arrow in same orbitals can't have same direction
solution liquid mixture
solute component in a solution
solvent able to dissolve other substances.
filtration pass (a liquid, gas, light, or sound) through a device to remove unwanted material.
distillation the action of purifying a liquid by a process of heating and cooling.
isotope the same element that contain equal numbers of protons but different numbers of neutrons
atomic orbital shell of an atom where electrons are at
sublevel level that is lower than or subordinate to another level s,p,d,f
valance electrons outermost shell of electrons
electron dot structure Consist of the element’s symbol surrounded by dots that represent the atom’s valence electrons
orbital diagram a box or circle represents an orbital
periodic law states that there is a periodic repetition of physical & chemical properties of the elements when arranged according to increasing atomic number.
group vertical columns
period horizontal rows
representative elements 1, 2, and 13-18
transition metals 3-12
alkali metals group 1 (except H); very reactive & generally exist as compounds.
alkaline earth metals group 2; highly reactive metals, also found in compounds.
halogens highly reactive elements. Often part of compounds.
noble gas group 18; highly UNreactive due to having a full valence shell.
ion an atom or molecule with a net electric charge due to the loss or gain of one or more electrons
ionic bond The electrostatic force that holds these oppositely charged particles together
ionic compound If compounds contain ionic bonds
cation positive ions
anion negative ions
formula unit chemical formula for an ionic compound
crystal-lattice a three dimensional geometric arrangement of particles
lattice energy The energy required to separate the ions of an ionic compound
oxidation number The charge of a monatomic ion is equal to its oxidation state
monatomic ion ion is a one atom ion
polyatomic ion ions made up of more than one atoms
binary ionic compound compound with 2 elements
ternary ionic compound compound with 2 or more
covalent bond Atoms in non-ionic compounds share electrons
molecule connected by covalent bonds
Lewis structure Drawings that visually demonstrate how electrons are shared and arranged around atoms
binary covalent compound composed of two different elements (usually nonmetals)
VSEPR model Valence-shell Electron-Pair Repulsion
Created by: LudwigL25
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