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PS: Ch 6-7

Ch. 6-7

Question or TermAnswer or Definition
substance composed of one type of atom element
idea that you cannot measure velocity and position simultaneously of an electron Heisenberg uncertainty principle
bonding where ALL electrons are shared among ALL atoms metallic
idea where the outermost shell wants to obtain eight electrons octet rule
electrons shared by more than 2 atoms delocalized
the name of the rows on the periodic table period
theoretical pieces that may make up protons and neutrons quarks
process of combining 2 nuclei fusion
part of a solution that is dissolved solute
the time required for one half of radioactive substance to decay into the daughter substance half-life
Where in an atom are the protons and neutrons found nucleus
protons have a __?__ charge positive
neutrons have a __?__ charge No
electrons have a __?__ charge negative
substance that comes out of a solution precipitate
mixture containing tiny clumps/particles colloid
what will increase the rate a substance is dissolved grinding, temperature increase, and stirring
molecules with the same types and number of atoms but in different arrangements isomers
type of radioactive decay where an electron is lost beta
atoms that have same element but different mass numbers or neutrons isotopes
idea where no 2 electrons can have the same 4 quantum numbers Pauli exclusion principle
type of chemical formula where the general arrangement of atoms in a molecule is shown structural
3 physical properties elements are divided into metals, semimetals, and nonmetals
atom that has a positive charge because of losing an electron cation
atom that has a negative charge because of gaining an electron anion
only metal that is a liquid at room temperature mercury
bonding that transfers electrons ionic
idea that electrons do not absorb or release in a smooth flow but rather in sudden packets quantum theory
when three pairs of electrons are shared between two atoms triple covalent bond
when an atom is covalently bonded to an atom with different electronegativity polar bond
simplest ratio of atoms in a nonmolecular compound formula unit
most of the mass of the human body is made up of what element oxygen
describes how the strength of atoms of an element pull on electrons in a chemical bond electronegativity
when that atomic nucleus breaks up or changes by emitting radiation radioactive decay
outermost shell contains what type of electrons valence electrons
idea that elements show regular repeating properties when arranged by increasing atomic numbers periodic law
if a substance has a strong intermolecular force has a __?__ boiling point than a substance with weak intermolecular force higher
Ag Silver
Au Gold
K Potassium
Na Sodium
O Oxygen
C Carbon
B Boron
N Nitrogen
Pb Lead
S Sulfur
H Hydrogen
Mn Manganese
U Uranium
F Fluorine
minimum amount of fissionable material needed to cause a chain reaction critical mass
diagram that shows the location of valence electrons in all atoms lewis structure
sum of atomic masses of all atoms in a molecule molecular mass
when molecules of a mixture are completely mixed together homogeneous mixture
when molecules of a mixture are NOT completely mixed together heterogeneous mixture
intermolecular force present in all polar molecules dipole-dipole
intermolecular force is the attraction between oppositely charged ends of polar molecules dipole-dipole
intermolecular force that occurs between all molecules London forces
intermolecular force that has a temporary concentration of electrons resulting in a temporary dipole London forces
strongest intermolecular force present hydrogen bonding
Intermolecular force where hydrogen is present and bonded to a more electronegative atom hydrogen bonding
Created by: Mrs. Sechrist