Chapter 2: Atomic Structure And Interatomic Bonding

Front 1

Atomic Number (Z)

Back 1

Number of protons in the nucleus

Front 2

Atomic Mass (A)

Back 2

Sum of masses of protons and neutrons

Front 3

Isotopes

Back 3

Same elements with different atomic masses (different number of neutrons)

Front 4

Atomic Weight

Back 4

Weighted average of the atomic masses of the atom's naturally occurring isotopes

Front 5

Atomic Mass Unit (AMU)

Back 5

Used to compute atomic weight, where one of these is 1/12 of the atomic mass of the most common isotope of carbon (Carbon12)

Front 6

Quantum Mechanics

Back 6

Principles of laws that govern systems of atomic and subatomic entities

Front 7

Bohr Atomic Model

Back 7

Electrons are assumed to revolve around the atomic nucleus in discrete orbitals

Front 8

Mole

Back 8

6.022E23 of anything

Front 9

1 g/mol

Back 9

1 amu/atom(or molecule)

Front 10

Wave-Mechanical Model

Back 10

Electron is considered to exhibit both wavelike and particle-like characteristics; electron is no longer treated as a particle moving in discrete orbital - position is considered to be probability of an electron's position

Front 11

Quantum Numbers

Back 11

Four parameters characterizing electrons: size, shape, orientation electron subshells

Front 12

Shells

Back 12

Specified by principal quantum number n
Designated by K, L, M, N, O
Corresponds to n = 1, 2, 3, 4, 5

Front 13

Subshell

Back 13

Signified by second quantum number: s, p, d, f

Front 14

Spin movement

Back 14

Up or down, possible values of +1/2 or -1/2

Front 15

Electron States

Back 15

Values of energy permitted for electrons

Front 16

Pauli Exclusion Principle

Back 16

Each electron state can hold no more than two electrons, which must have opposite spins

Front 17

Ground State

Back 17

All electrons occupy the lowest possible energies in accord with the foregoing restrictions

Front 18

Electron configuration

Back 18

Structure of an atom represents the manner in which states are occupied

Front 19

Valence Electrons

Back 19

Electrons that occupy the outermost shell

Front 20

Stable Electron Configurations

Back 20

Outermost shell is filled

Front 21

Periodic table

Back 21

Elements classified according to electron configuration

Front 22

Electropositive

Back 22

Elements capable of giving up valence electrons to be positively charged ions (typically metals)

Front 23

Electronegative

Back 23

Right-hand side of periodic table; readily accept electrons to form negatively charged ions

Front 24

F(N)

Back 24

Net force between two atoms: F(A)+F(R) => attractive and repulsive components

Front 25

Equilibrium in force

Back 25

F(A)+F(R)=0

Front 26

Bonding Energy

Back 26

E(0) corresponds to the energy at the minimum point of the net energy curve

Front 27

Primary/chemical bonds

Back 27

How atoms interact

Front 28

Ionic Bonding

Back 28

Transfer of electrons

Front 29

Coulombic

Back 29

Attractive bonding forces (word for)

Front 30

Attractive Energy

Back 30

E(A) in E(A)=-A/r

Front 31

Covalent Bonding

Back 31

Atoms each contribute at least one electron to the bond

Front 32

Metallic Bonding

Back 32

Valence electrons are not bound and freely drift throughout the entire metal

Front 33

Secondary Bond
Van der Waals
Physical Bonds

Back 33

Bonding that arises from dipoles (when there is some separation of positive and negative portions of an atom or molecule)