Inorg Chem Unit 2

Front 1

Used to describe valence electron configuration

Back 1

Lewis symbol

Front 2

Drawing that describe the bonding in molecules

Back 2

Lewis structure

Front 3

Odd number of electron

Back 3

Free radicals

Front 4

Angle in any two bonds

Back 4

Bond angle

Front 5

Distance between the nuclei of two bonded atoms

Back 5

Bond distance

Front 6

VSEPR Theory

Back 6

Valence shell electron pair repulsion theory

Front 7

2 region, 180

Back 7

Linear

Front 8

3 region, 120

Back 8

Trigonal planar

Front 9

Four regions, 109.5

Back 9

Tetrahedral

Front 10

5 regions, 90, 120

Back 10

Trigonal biphyramidal

Front 11

Six regions, 90

Back 11

Octahedral

Front 12

Transfering

Back 12

Ionic bonds

Front 13

Sharing

Back 13

Covalent bonds

Front 14

Bonds in the product are stronger

Back 14

Exothermic

Front 15

Bonds in the product are weaker

Back 15

Endothermic

Front 16

Atoms that form a covalent bond are identical

Back 16

Pure covalent bond

Front 17

Bonding electrons are shared unequally

Back 17

Polar covalent bond

Front 18

Attraction between the molecules of sugar and water

Back 18

Intermolecular forces - Van der waals forces

Front 19

Molecules have both positive and negative end

Back 19

Dipole forces

Front 20

Hydrogen atom/ two polar molecules

Back 20

Hydrogen bonding

Front 21

Has both polar and non

Back 21

London dispersion forces

Front 22

Atoms share unequally

Back 22

Polar

Front 23

Atoms share equally

Back 23

Non polar

Front 24

Separation of charges which depends on moleculaf

Back 24

Polar/dipole

Front 25

Water loving

Back 25

Polar

Front 26

Lipid loving

Back 26

Non polar

Front 27

Number of chemical bonds it makes with other atoms

Back 27

Valence

Front 28

Involves in chem reaction

Back 28

Valence electron

Front 29

Electrons in the inner shells of an atom

Back 29

Core electrons

Front 30

Characterized by an oxidation number

Back 30

Oxidation state

Front 31

When reverse reaction state are equal

Back 31

Equilibrium

Front 32

When reverse reaction state are equal

Back 32

Equilibrium

Front 33

When reverse reaction state are equal

Back 33

Equilibrium

Front 34

At a given temp, the reaction quotient for a system at equi is constant

Back 34

Law of mass action

Front 35

Traits of acid sol'n

Back 35

Robert Boyle

Front 36

Modern acid base concept

Back 36

Humphry davy

Front 37

Acid can neutralize base

Back 37

Joseph Louis Gay Lussac

Front 38

Acid as a compound dissolves in water

Back 38

Svante Arrhenius

Front 39

Transfer of hydrogen ions

Back 39

Johannes Bronsted and Thomas Lowry

Front 40

Donates proton

Back 40

Bronsted lowry acid

Front 41

Accepts proton

Back 41

Bronsted lowry base

Front 42

Residue of acid donates

Back 42

Conjugate base

Front 43

When base accepts hydrogen

Back 43

Conjugate acid

Front 44

Reaction between bronsted lowry acid and water

Back 44

Acid ionization

Front 45

Accepts protons from water molecules

Back 45

Base ionization

Front 46

Ability to act as a base or acid

Back 46

Amphoteric

Front 47

Ability to accept and donate protons

Back 47

Amphoprotric

Front 48

Like molecules react to yield ions

Back 48

Autoionization

Front 49

Pertains to how much solute is in a solution

Back 49

Concentration

Front 50

Lar. Am. Of solute

Back 50

Concentrated soln

Front 51

Small ammount of solute

Back 51

Dilute soln

Front 52

Can dissolve more solute

Back 52

Unsat soln

Front 53

No more solute can be dissolved

Back 53

Sat soln

Front 54

Soln that holds more sol

Back 54

Supersaturated

Front 55

Dependent upon the no. Of particles of solute soln

Back 55

Colligative properties

Front 56

Water soln conduct electric current

Back 56

Electrytes

Front 57

Water soln are poor conductors

Back 57

Weak electrolytes

Front 58

Water soln will not carry elec current

Back 58

Non electrolytes

Front 59

Few salts /strong acid and base

Back 59

Strong electrolytes