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Chemistry Chapter 3: Atome- Building Blocks of Matter


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The earliest particle theory was deveolped by?
democritus in 400
Demcritus called natures basic particle the what?
The fact the chemical compound contains the same elements in exactly the same proportiond by mass regardless of the size of the sample or source of the coumpound
law of definite proportions
if 2 or more drifferent compounds are composed of the same 2 elemnts, then thre ratio of masses of the 2nd elemnt combined with a certain mass of the 1st elemnt in always a ratio of small whole #s
law of multiple proportions
mass is neither destryoed nor created during ordinary chemical reactions or physical change
law of conservation of mass
all matter is composed of extremely samll partcles called atoms?
atoms of a given elemnt are identicale in size, mass, and other properties?
atoms cannot be subdivied, created, destroyed?
atoms of different elements combined in simple whole# ratios to form chemical compoundas?
in chemical reactions, atoms are combined, seperated, or rearanged?
What are the 2 parts of Dalton's theory that is not correct?
1. atoms are divisble into smaller particles
2. a given element can ahve atoms wiht different masses
the smallest particle of an elemnt that retains the chemical properties of the element
What are the parts of the atom?
nucleous, proton, nuetron, electron, and subtomic particles
Whose experiment revelaed that the electron has a neg. charge?
JJ Thomson
1897 (Plum Pudding)
Who confirmed that the electron has a neg. chatge?
What was the gold foil experiment?
Rutherfors, Geiger,& Marsden bobarded a thin, gold foil with fast moving alpha particle.
short-range, proton-nuetron, proton-proton, and nutron-nitron forces hold the nuclear particles together
nuclear forces
the region occupied by the electrons
electron cloud
the distance from the center of the nucleous to the outer portion of the electron cloud is
radious of an atom
atoms of the same elemnt that have different masses
the total # of protons and nuetrons in the nucleous of an isotoep
mass #
the weighted ave. of the atomic masses of the naturally occurring isotopes of an element
average atomic mass
the mass if ine mole of a pure substance
molar mass

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