Concepts 2

Front 1

Dalton

Back 1

Hypothesized that every element has atoms.

Front 2

Molecule

Back 2

Cluster of atoms that can be isolated

Front 3

Electrolysis

Back 3

"Splitting by electricity". Allowed rapid discovery of many elements.

Front 4

Earth's Composition

Back 4

Oxygen, Silicon, Magnesium, Iron, Aluminum, Calcium

Front 5

Composition of Living Organisms

Back 5

Hydrogen, Carbon, Nitrogen, Oxygen, Phosphorus, Sulfur

Front 6

Star Composition

Back 6

Hydrogen and Helium

Front 7

Thompson

Back 7

Identified the electron.

Front 8

Rutherford

Back 8

Experimented with gold foil. Proved the existence of the nucleus.

Front 9

Rutherford's model of the atom

Back 9

Positvely charged nucleus surrounded by orbiting cloud of negatively charged electrons.

Front 10

Bohr

Back 10

Said electrons exist in various levels located around the nucleus. "energy levels"

Front 11

Ground state

Back 11

When all electrons are in lower energy levels

Front 12

Photon

Back 12

a packet of electromagnetic radiation emitted when electrons drop to lower energy levels. Both a particle and a wave.

Front 13

Spectrum

Back 13

total collection of photons emitted by a given atom. Each atom has a unique spectrum.

Front 14

Spectroscopy

Back 14

Study of elemental composition using absorption lines.

Front 15

Uses of spectroscopy

Back 15

1. Study of stellar gasses and interstellar dust composition.
2. Chemical tests on unknown substances.
3. Study of soil and rock.

Front 16

Atomic Number

Back 16

Number of electrons in the shell.

Front 17

Alkali Metals

Back 17

First Column.

Front 18

Alkali Earths

Back 18

Second Column.

Front 19

Noble Gasses

Back 19

Eighth column.

Front 20

Atomic interactions

Back 20

When two atoms interact, their outermost shell electrons dictate their interactions and govern bonding properties.

Front 21

Pauli Exclusion Principle

Back 21

No two electrons can occupy the same energy state at the same time.

Front 22

Valence Electrons

Back 22

Electrons in the outer shell

Front 23

Chemical bonding

Back 23

Commonly involves exchange or sharing of valence electrons.

Front 24

Valence

Back 24

Number of electrons in outer shell. "Combining power" of atoms.

Front 25

Quest of the atom

Back 25

To achieve the lowest energy state it can

Front 26

Chemical bonds

Back 26

The result of redistribution of electrons that leads to a more stable configuration between two or more atoms

Front 27

Ionic Bonds

Back 27

Chemical bond which electrical force between two oppositely charged ions holds the atoms together. One atom gives up an electron and the other receives the electron.

Front 28

Alloy

Back 28

two or more metallic elements combined in a metallic bond.

Front 29

Malleability

Back 29

A property of metals that allows atoms to rearrange themselves. Can be bent shaped molded.

Front 30

Metallic Bond

Back 30

electrons are continually redistributed so they are shared by many atoms at one time.

Front 31

Covalent Bonds

Back 31

Molecules that share electrons. (diatomic gasses)

Front 32

Organic Chemistry

Back 32

Study of Carbon bonding and related bonding.

Front 33

Polar molecules

Back 33

Molecules with either a positive or negative side to them.

Front 34

Hydrogen bonds

Back 34

Weak electrical attraction developed by the H atom itself after it is bonded to another element like O or N.