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82 Cards in this Set

  • Front
  • Back
mass
the amount of matter something takes up
volume
the amount of space something takes up
matter
anything that takes up space
metal
everything to the left side of the periodic table, conductors, lose an e-, malleable and ductile
nonmetal
everything to the right side of the periodic table, gain an e-, covalent bond
metalloid
properties similar to metals and non metals
alkali metals
1st column of the periodic table, + one charge
alkali earth metals
2nd column of the periodic table, + 2 charge
transition metals
metals in between the alkali earth metals (column 2) and column 13
halogens
refers to the elements in the column before the noble gases aka column 17; need one more electron to have a full valence shell thus a charge of -1
noble gases
have a full valence shell; column 18
groups
columns PT
families
columns in the PT
rows
rows in the PT
periods
rows in the PT
isotope
an atom of the same element with a different number of neutrons
isotopic notation
(mass number) (charge)
X
(atomic #)
ion
charged atom
ionic bond
formed between 2 ions of opposite charge; can form:
cation- lose an e-; + charge
anion- gain an e-; - charge
covalent bond
bond formed by sharing an e-; use prefixes to name
atomic number
the number of protons in an atom's nucleus
atomic mass
average mass of the nuclei of a particular element; this is a weighted average
mass number
mass of the nucleus of an atom; this is equal to the number of protons plus the number of neutrons in the nucleus of all atoms of an element
accuracy
how right an answer is; how close to it
precision
consistency; how often you are right
sig digs
digits known with certainty plus one estimated digit; when +/- use the least number of decimal places; when X/ / use the least number of sig digs
density
mass per unit volume for a substance;
mass/ vol
water displacement
measurement of volume by seeing how hight the water goes when object placed in water, measure how high the water went from original place
limiting reactant
the reactant that runs out first
reactant
substances used in a reaction
product
substance created in a reaction
mole ratio
get the numbers from the coefficients infront of the element; use it to go form mole to mole
coefficient
the number infront of the symbol
subscript
the writing in small print under something
mole
unit of measurement to measure very small things; used to compare substances
molarity
moles/ 1L; used to measure concentration
empirical formula
lowest whole number ratio of elements in a compound
molecular formula
actual ratio of elements in a compound
solute
substance being dissolved
solvent
substance that the solvent is being dissolved in
solution
homogenous, clear, will not filter out or settle out, negative tyndall effect and is composed of atomic size particles
dilute
adding more solvent to a known soln to make less concentrated soln; to weaken the soln
concentrated (concentration)
how much is dissolved
acid
substance with a H+ ion
base
substance with HOH
solubility rules
tell you whether a substance will dissolve or precipiate ( pg 114)
chemical properties
only be observed by changing the composition of the material/ rusting/ burning/ tarnishing
physical properties
can be observed and measured with out changing the composition
homogeneous
appears to be the same composition throughout; solutions and colloids
heterogeneous
the mixture is not uniform in composition; suspensions,
suspension
heterogeneous, will filter, will settle out and is composed of relatively large particles
colloid
homogeneous, cloudy, will not filter, does not settle out, positive tyndall effect, and is composed of small, microscopic particles
ex: milk
Pauli Exclusion Principle
no two e- in the same atom can have the same 4 quantum numbers
Heisenberg Uncertainty principle
exact location and speed of an e- cannot be determined without changing the its location and speed. most probable location of the e- within the e- cloud is described by the 4 quantum numbers
Aufbrau Principle
the method of e- configuration with teh 1s, 2s, 2d
ionization E
the E needed remove the most loosely held e- from an atom
electromagnetic spectrum
(in order from longest wave/ least E)
radio waves; microwaves; visible light (ROYGBIV); ultraviolet; x-rays; gamma radiation
amu
1/12th the mass of a carbon 12 atom; approximately the mass of a p/ n
protons
positively charged particles in the nucleus
electrons
negatively charged particles floating around the nucleus
neutrons
neutral particles in the nucleus
leptons
primary subatomic particles
hadrons
composite (made up several things) subatomic particles
wavelength
from trough to trough/ crest to crest' the longer the least E
amplitude
from the standing wave to to the crest/ amplitude
frequency
wavelength/ time= like the speed of the wave
democritus
believed that matter was made up of small shapes that can no longer be divided
mendeleev
1st to arrange a table of elements vertically using atomic mass and horizontally using chemical properties
rutherford
discovered the types of radiation
alpha-positive; beta-negative; gamma-neutral
heisenberg
heisenberg uncertainty principle
dalton
his hypothesis: an atom is the smallest unit of an element that can exist either alone or in combination with other atoms of the same or different elements
mosley
arranged the elements in order of their atomic number horizontally and formed columns of elements with similar properties (modern)
pauli
pauli exclusion principle
thompson
discovered the electron
principle quantum number
shows E level, distance from nucleus (1 the closest); size; 1,2,3,4
orbital quantum number
"shape" of the cloud of probability; S-sphere, 2 e-; P- figure 8, 6 e-; d- 4 leaf clover; 10e-, f-very complex; 14 e-
magnetic quantum number
orientation in space; mathematical function on x,y, z axis
spin quantum number
indicates the direction of spin, each e- in a pair mist spin in opp directions because of like charges attract
electron configuration (arrow and shorthand)
arrow-> arrows in order of s, pxyz, d
shorthand-> writing it out in numbers; when writing it, starting at 3, put 4s before 3d
periodicity
with increasing number of atomic number the e- config of atoms display a periodic pattern of change in phy and chem properties
atomic radius
alkali metals have the largest radius because only have 1 e- so they hold it loosely in order to get to full outer shell; halogens have smallest radisu b/c they hold e- tightly b/c only need 1 more to have full outer shell; moving form left to right size decreases; moving up to down size increases (b/c add another E level)
ionization E
E needed to remove the most loosely held e-; ionization E increases as at # increases in any horizontal row; in column there is a gradual decrease in ionization E as at # increases