Chapter 2: Atoms and Elements Flashcards
atomos
indivisible
atomic theory
all matter is composed of atoms
law of conservation of mass
in a chemical reaction, matter is neither created nor destroyed
- consistent with the idea that matter is composed of small, indestructible particles
when a chemical reaction occurs, the total mass of the substances involved in the reaction does not change
law of definite proportions (law of constant composition)
all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements
law of multiple proportions
when two elements (call them A and B) form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a ratio of small whole numbers
- an atom of A combines with either one, two, three, or more atoms of B
- the ratio of these two masses is itself a small whole number
Dalton’s atomic theory
- each element is composed of tiny, indestructible particles called atoms
- all atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements
- atoms combine in simple, whole-number ratios to form compounds
- atoms of one element cannot change into atoms of another element. in a chemical reaction, atoms only change the way they they are bound together with other atoms
J.J. Thomson
proposed that the negatively charged electrons were small particles held within a positively charged sphere
- incorrect plum-pudding model
nuclear theory
- most of the atom’s mass and all of its positive charge are contained in a small core called a nucleus
- most of the volume of the atom is empty space, throughout which tiny, negatively charge electrons are dispersed
- there are as many negatively charged electrons outside the nucleus as there are positively charged particles (named protons) within the nucleus, so that the atom is electrically neutral
neutrons
neutral particles within the nucleus
subatomic particles
protons, neutrons, electrons
proton
charge = +1
neutron
charge = 0
electron
charge = -1
atomic number
the number of protons in an atom’s nucleus
chemical symbol
either a one- or two-letter abbreviation listed directly below its atomic number on the periodic table