Chem Final Ch. 4

Front 1

Atom

Back 1

smallest particle of an element that retains its identity in a chemical reaction.

Front 2

dalton's atomic theory

Back 2

All elements are composed of tiny indivisible particles called atoms.
Atoms of the same element are identical. The atoms of any one element are different from those of any other element.
Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds.
Chemical reactions occur when atoms are separated, joined, or rearranged. Atoms of one element, however, are never changed into atoms of another element as a result of a chemical reaction.

Front 3

yeah

Back 3

Three kinds of subatomic particles are electrons, protons, and neutrons.

Front 4

electrons

Back 4

negatively charged subatompic particles

Front 5

cathode ray

Back 5

glowing beam? positivley charged plates attract them?

Front 6

proton

Back 6

positively charged subatomic particles

Front 7

neutrons

Back 7

subatomic particles with no charge but with a mass nearly equal to that of a proton.

Front 8

nucleus

Back 8

tiny central core of an atom and is composed of protons and neutrons.

Front 9

nuclear atom

Back 9

In the nuclear atom, the protons and neutrons are located in the nucleus. The electrons are distributed around the nucleus and occupy almost all the volume of the atom.

Front 10

yeah 2

Back 10

Elements are different because they contain different numbers of protons.

Front 11

atomic number

Back 11

the number of protons in the nucleus of an atom of that element. Because all hydrogen atoms have one proton, the atomic number of hydrogen is 1.

Front 12

mass number

Back 12

total number of protons and neutrons in an atom

Front 13

yeah

Back 13

The number of neutrons in an atom is the difference between the mass number and atomic number.

Front 14

isotopes

Back 14

atoms that have the same number of protons but different numbers of neutrons.Because isotopes of an element have different numbers of neutrons, they also have different mass numbers

Front 15

atomic mass

Back 15

a weighted average mass of the atoms in a naturally occurring sample of the element. To calculate the atomic mass of an element, multiply the mass of each isotope by its natural abundance, expressed as a decimal, and then add the products.

Front 16

period

Back 16

each of the horizontal rows on the periodic tables.

Front 17

group

Back 17

Each vertical column of the periodic table