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Matter
The substance of which all physical objects are made.
Physical property
A characteristic that can be observed or measured without changing the substance's identity.
Extensive properties
Depend on the amount of matter (e.g., mass, volume).
Intensive properties
Do not depend on the amount of matter (e.g., density, temperature).
Chemical property
A property that can only be observed by changing the chemical identity of the substance.
Law of Conservation of Mass
Mass is neither created nor destroyed in a chemical reaction.
Mixture
A combination of two or more substances that can be physically separated.
Parts of an atom
Protons (positive charge), Neutrons (neutral), Electrons (negative charge).
Atomic number
The number of protons in an atom.
Atomic mass
The weighted average mass of the atoms in a naturally occurring sample of the element.
Isotope
Atoms of the same element with different numbers of neutrons.
Calculate atomic mass
Multiply the mass of each isotope by its percent abundance, then add the values % divide by 100.
Quantum theory
Energy is quantized, meaning it exists in discrete units.
Quantum Mechanical Model
A model of the atom where electrons are found in orbitals, not fixed paths.
Electron configuration
The arrangement of electrons in an atom's electron shells.
Hund's Rule
Electrons occupy orbitals in a way that maximizes unpaired electrons before pairing.
Major groups of elements
Metals, Nonmetals, and Metalloids.
Similar properties in groups
They have the same number of valence electrons.
Electronegativity
A measure of an atom's ability to attract electrons in a chemical bond.
Ionic bond
A bond formed by the transfer of electrons from one atom to another.
Cation
A positively charged ion, formed when an atom loses electrons.
Anion
A negatively charged ion, formed when an atom gains electrons.
Properties of ionic compounds
High melting points, good conductors of electricity in molten or dissolved form.
Metallic bonding
A type of bonding where electrons are free to move, explaining properties of metals like electrical conductivity.
Octet Rule
Atoms tend to gain, lose, or share electrons to achieve a full set of eight valence electrons.
Covalent bonding
A bond formed when two atoms share electrons.
Sigma and pi bonds
Sigma bonds are formed by head-on overlapping of orbitals; pi bonds form by side-to-side overlapping.
Polar covalent bond
A bond where electrons are shared unevenly, causing a dipole.
Nonpolar covalent bond
A bond where electrons are shared equally between atoms.
Lewis Dot Structures
Represent atoms with their valence electrons, and use lines to represent bonds.
Solid
Matter with a definite shape and volume, not compressible
Liquid
A state of matter that has no definite shape but has a definite volume, not compressible.
Gas
Matter with no definite shape or volume, compressible.
Linear
Shape with 2 atoms connected to the central atom, and 0 unshared electron pairs.
V Shaped
Shape with 2 atoms connected to the central atom, and 2 unshared electron pairs.
Trigonal Planar
Shape with 3 atoms connected to central atom, and 0 unshared pairs.
Trigonal Pyramidal
Shape with 3 atoms connected to central atom, and 1 unshared electron pair.
Tetrahedral
Shape with 4 atoms connected to central atom, and no unshared electron pair.
s sublevel
1 orbital, 2 electrons
p sublevel
3 orbitals, 6 electrons
d
5 orbitals, 10 electrons
f
7 orbitals, 14 electrons
Dalton's Theory
All substances are made of atoms. Atoms are small particles that cannot be created, divided, or destroyed.
Atoms of the same element are exactly alike, and atoms of different elements are different.
Atoms join with other atoms to make new substances.
Thomson
Discovered electrons; Plum Pudding Model
Rutherford
Gold foil experiment, discovered nucleus
Bohr
discovered electrons around the nucleus; Planetary Model
atomic radius trend
Increases at the bottom left of the periodic table.
Metallic Character Trend
Increases at the bottom left of the p table.
Ionic Radius Trend
Increases at bottom left of periodic table.
Electronegativity Value Trend
Increases at the top right of the periodic table.
Antoine Lavoisier
Complied list of 33 known elements into 4 categories: gases, metals, nonmetals, and earths. "Lavoisier's Table of Simple Substances.
John Newlands
Arranged elements by increasing atomic mass; "Law of Octaves"
Dimitri Mendeleev
Demonstrated connection between atomic mass & properties. Predicted undiscovered elements & their properties.
Henry Moseley
discovered atomic number; modern p table influenced by his research
Properties of Metals
Shiny, solid at room temp, and good heat/electricity conductors.
properties of mettaloids
Exhibits properties between metals & nonmetals, semi-conductors.
Properties of nonmetals
Gases or brittle, dull looking solids, poor conductors.
Alpha Particle
4/2 He
Beta Particle
0/-1 e
Gamma Particle
0/0 Y
Nuclear Reaction
A reaction that involves a change in the nucleus of an atom
Alpha Radiation
radiation deflected toward the negatively charged plate
Beta Radiation
Radiation deflected toward the positively charged plate
Gamma Ray
High energy radiation with no mass.
Equation relating wavelength and frequency to the speed of light.
c=λv
An equation relating energy to frequency
E=hv
An equation relating energy to wavelength to the speed of light.
E=hc/λ
Speed of Light (C)
3.00 x 10^8 m/s
Plank Constant (h)
6.626 x 10^-34
Malleability
ability to be shaped into a different form.
Ductility
Ability to draw metal into a wire.
Heat Capacity
Can absorb certain amount of heat before changing temperature.
Luster
How shiny the metal is.
Conductivity
Ability to transmit heat or light.
Evaporation
Process by which an element or compound transitions from a liquid to a gas.
Filitration
Process of removing solid particles from a fluid by using filter medium.
Crystallization
Chemical process where a liquid solidifies into highly structured solid with well defined crystal lattice.
Sublimation
Conversion of a solid to a gas without becoming a liquid
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