Chem I Chap 4

Front 1

definition: solution

Back 1

homogeneous mixture of two or more substances

Front 2

definition: solvent

Back 2

substance present in larger amount

Front 3

definition: solute

Back 3

substance present in smaller amout

Front 4

definition: electrolyte

Back 4

substance that, when dissolved in water, conducts electricity

Front 5

definition:nonelectrolyte

Back 5

substance that, when dissolved in water, does not conduct electricity

Front 6

dissociation

Back 6

breaking up of a compound in to ion parts (cation and anion)

Front 7

are organic substances (containing C) electrolytes or non electrolytes?

Back 7

non electrolytes

Front 8

what is a weak electrolyte?

Back 8

an electrolyte that does not completely disassociate

Front 9

definition: polar

Back 9

molecule, such as water, with a positive and a negative region

Front 10

definition: reversible reaction

Back 10

can occur in both direction

Front 11

definition: precipitation reaction

Back 11

reaction which results in the formation of an insoluble product

Front 12

definition: precipitate

Back 12

an insoluble solid that separates from the solution

Front 13

definition: double displacement reaction

Back 13

reaction that involves the exchange of parts of the compounds

Front 14

definition: solubility

Back 14

the max amount of solute that will dissolve in a given quantity of solvent at a specific temperature

Front 15

Solubility: Halides

Back 15

All halides are soluble unless coupled with Ag Hg Pb

Front 16

Solubility: Nitrates NO3-, bicarbonates HCO3-, and chlorates ClO3-

Back 16

Always soluble

Front 17

Solubility: Alkali metal ions or NH4

Back 17

always soluble

Front 18

Solubility: Sulfates SO4 2-

Back 18

Soluble except for Ag+, Ca2+, Sr2+, Ba2+, Hg2 2+, Pb 2+

Front 19

Solubility: hydroxides

Back 19

not soluble unless combined with an alkali earth metal or Ba2+

Front 20

Solubility: carbonates (CO3 2-), phosphates (PO4 3-), chromates (CrO4 2-), sulfides S 2-)

Back 20

not soluble except when combined with an alkali metal ion or the NH4 ion

Front 21

Solubility: rule of thumb

Back 21

if both ion charges are more than one, probably not soluble

Front 22

definition: molecular equation

Back 22

formulas written as though all species existed as molecules or whole units

Front 23

definition: ionic equation

Back 23

shows dissolved species as free ions

Front 24

definition: spectator ions

Back 24

ions not involved in the over all reaction

Front 25

definition: net ionic equation

Back 25

shows only the species that take part in the reaction

Front 26

procedure for writing ionic and net ionic equations

Back 26

1) write balanced molecular equation
2)write ionic equation
3)identify and cancel spectator ions
4)check that the charges and number of atoms balance

Front 27

Definition: Bronsted acid

Back 27

proton donor

Front 28

Definition: Bronsted base

Back 28

proton acceptor

Front 29

definition: monoprotic acid

Back 29

each unit of the acid donates one proton upon ionization

Front 30

definition: diprotic acid

Back 30

each unit of the acid donates two protons upon ionization

Front 31

definition: triprotic acid

Back 31

each unit of the acid donates three protons upon ionization

Front 32

definition: weak acid

Back 32

does not completely dissociate, use solubility rules to determine

Front 33

definition: neutralization reaction

Back 33

reaction between an acid and a base

Front 34

What are the products of a neutralization reaction?

Back 34

Water and salt (salt is an ionic compound made of a cation other than H and a anion other that OH or O2)

Front 35

definition: redox reactions/ oxidation-reduction reactions

Back 35

electron transfer reactions

Front 36

definition: half reaction

Back 36

shows the intermediate steps of a redox reaction/ shows the electrons involved

Front 37

definition: oxidation reaction

Back 37

half reaction which shows the loss of electrons

Front 38

definition: reduction reaction

Back 38

half reaction which shows the gain of electrons

Front 39

definition: reducing agent

Back 39

the part which donates electrons

Front 40

definition: oxidizing agent

Back 40

the part which accepts electrons

Front 41

definition: oxidation number

Back 41

signifies the number of charges the atom would have in a molecule (or an ionic compound) if the electrons were transfered completely

Front 42

oxidation number rules: free elements

Back 42

0

Front 43

oxidation number rules: ions composed of only one atom

Back 43

Oxidation number is equal to the charge of the ion

Front 44

oxidation number rules: Oxygen

Back 44

normally -2, but there are exceptions

Front 45

oxidation number rules: Hydrogen

Back 45

+1, except when binded to metals of binary compounds, then it is -1

Front 46

oxidation number rules: Fluorine, Halogens

Back 46

Fluorine always -1, halogens are negative unless combined with oxygen

Front 47

oxidation number rules: neutral molecule or polyatomic ion

Back 47

sum of oxidation numbers must equal 0

Front 48

definition: combination reaction

Back 48

two or more substances combine to form a single product

Front 49

definition: decomposition reaction

Back 49

break down of a compound into 2+ components

Front 50

definition: combustion reaction

Back 50

a substance reacts with oxygen usually with the release of heat and light to produce a flame

Front 51

definition: displacement reaction

Back 51

an ion in a compound is replaced by an ion of another element

Front 52

definition: hydrogen displacement

Back 52

Separates water, making hydrogen a product of the reaction

Front 53

definition: metal displacement

Back 53

a metal is replaced by a metal of a different element

Front 54

definition: halogen displacement

Back 54

halogens higher in the group can replace halogens lower in the group

Front 55

definition: disproportionation reaction

Back 55

an element is simultaneously oxidized and reduced

Front 56

Molarity equals

Back 56

moles of solute/ Liters of Solution

Front 57

definition: dilution

Back 57

the procedure for preparing a less concentrated solution from a more concentrated solution

Front 58

Strategy for dilution problems

Back 58

M1V1=M2V2 where M= molarity and V= volume in liters

Front 59

definition: Titrations

Back 59

a solution of accurately known concentraion (standard solution)is added gradually to another solution of unknown concentration until the chemical reaction between the two is complete

Front 60

definition: indicator

Back 60

substance that changes color to indicate neutralization in an acid- bas titration or oxidation/ reduction in a redox reaction