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Unit 1: A/B Review

Terms for Chemistry.

Question/TermAnswer/Definition
Atom The smallest unit of matter that retains its unique properties
Element Different types of atoms, can be either a pure substance or a compound
Pure Substance Every atom is the EXACT same type
Compound 2+ atoms bonded together (either same type of different)
Chemical Symbol Initials of element (ie. He)
Democritus & Dalton >500 B.C/1800; found that if matter is repeatedly cut, eventually you reach an uncut-able sphere, called the "Atmos"
Thompson 1904; Positive sphere with negative regions attached called "electrons"; "Plum Pudding Model"
Rutherford 1911; Found that an atom had a nucleus with orbiting electrons; volume is mostly empty space
Neils Bohr 1913; Electrons orbit within specific energy levels; 7 different energy levels
Modern 40s-50s; Quantum Mechanics/Electron cloud model; Different energy levels with orbitals rather than orbits
Orbit A fixed path of movement
Orbitals Sub-region within and energy level
Proton 1 AMU; Positive Charge; Found in nucleus
Neutron 1 AMU; Neutral charge; Found in nucleus
Electron 0 AMU; Negative charge; Found in cloud
Isotope Atoms of the same element with different numbers of neutrons
Valence Electrons Electrons in the highest level in an atom
Ion A particle that has more or fewer electrons than protons
Cation A positively charged Ion
Anion A negatively charged Ion
"s" orbital 1st orbital; spherical shape; 1 orbital; 2 electrons max
"p" orbital 2nd orbital; pear shaped; on the x-axis, y-axis, and z-axis; 3 orbitals; 6 electrons max
"d" orbital 3rd orbital; dumbbell shape; on the x-axis, y-axis, z-axis, x-y prime-axis, and x-z axis; 5 orbitals; 10 electrons max
"f" orbital 4th orbital; funky shape; 7 orbitals; 14 electrons max
Aufbau Principle Electrons enter orbitals of lowest energy first; "s" is ALWAYS the lowest energy level within a principle energy level
Pauli Exclusion Principle An orbital may have at most 2 electrons; for an orbital to be filled with electrons, they must be opposite spins
Hund's Rule When electrons occupy orbitals of equal energy, one Electron enters each orbital until all orbitals contain one Electron with parallel spins.
Core electrons All electrons not within the valence cloud
Electronegativity An atom's ability to take away electrons; gets stronger as you move right & up on the periodic table
Ionization energy An atom's ability to hold onto its electrons; Gets stronger as you go up and right
Atomic Radius The distance between the nucleus and the valence cloud; Gets larger as you go down and left
Reactivity How well an atom bonds to another atom; gets stronger as you get closer to either end of the periodic table.
Metallic character Shows traits of metals; Gets stronger as you move down and left on the periodic table.
Non-Metallic character Shows traits of non-metals; Gets stronger as you go up and right on the periodic table.
Metals Left side of metalloid line; Malleable, ductile, conductive and has potential to be magnetic
Non-Metals H and right side of metalloid line; Brittle solids, ractive, low melting and boiling points
Metalloids On metalloid line; both metallic and nonmetallic properties
Alkali Metals Group 1; highly reactive; never found alone in nature; silvery; low density; soft metals; vigorous reaction to water
Alkaline Earth Metals Group 2; silvery; soft metals; distinguishable flame colors; reactive with water
Transition Metals Groups 3-12; Magnetic under specific conditions
Halogens Group 17; All forms of matter at room temperature; produces a type of salt when mixed with metals; only found as compounds due to reactivity
Noble Gasses Group 18; Inert/Unreactive; glow with electricity.
Metalloid Line Stairstep line found on periodic table
Created by: cbrock7086
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