Quizlet Chemistry Comp, Electrolysis (IGCSE), Electrolysis - IGCSE, Chemistry - Electrolysis, Electrolysis, Oxidation, Oxidation Numbers, Balancing oxidation-reduction equations, Redox Reactions, Redox Reaction, Balancing Chemical Equations, Balancin...

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Adrenal genital syndrome

* virilism= congenital adrenal. Is secondary male characteristics

Carbon oxi#

+2,+4,-4

Apparatus used in a titration

- Pipette (to measure alkali) - Burette (to measure acid) - conical flask - retort stand - funnel - indicator

Acid reactions with ammonia

- acid + ammonia --> ammonium salt sulfuric acid + ammonia --> ammonium sulphate

How to test for carbonate ions

- add an acid (hydrochloric acid) - you can see if a gas is carbon dioxide by bubbling it through limewater - if the gas is carbon dioxide, it turns cloudy - if the limewater turns cloudy, then carbonate ions are present

CaS + H2O + CO2 -> Ca(HCO3)2 + H2S

...

CaS + H2O -> Ca(HS)2 + Ca(OH)2

...

size of needle for female

1-3

pH + pOH =

PH₃ + O₂ → P₄O₁₀ + H₂O

4PH₃ + 8O₂ → P₄O₁₀ + 6H₂O

In drinks, citrus, pop, etc.

Acid

What colour precipitate does Cu2+ produce when tested?

Blue precipitate

31. H2C2O4 + 2 H2O ⇄ 2 H3O+ + C2O42− Oxalic acid, H2C2O4, is a diprotic acid with K1 = 5 x 10−2 and K2 = 5 x 10−5. Which of the following is equal to the equilibrium constant for the reaction represented above? (A) 5 x 10−2 (B) 5 x 10−5 (C) 2.5 x 10−6 (D) 5 x 10−7 (E) 2.5 x 10−8

56. A 0.20-molar solution of a weak monoprotic acid, HA, has a pH of 3.00. The ionization constant of this acid is... (A) 5.0 x 10−7 (B) 2.0 x 10−7 (C) 5.0 x 10−6 (D) 5.0 x 10−3 (E) 2.0 x 10−3

Questions 9-12 refer to aqueous solutions containing 1:1 mole ratios of the following pairs of substances. Assume all concentrations are 1 M. (A) NH3 and NH4Cl (B) H3PO4 and NaH2PO4 (C) HCl and NaCl (D) NaOH and NH3 (E) NH3 and HC2H3O2 (acetic acid) 9. The solution with the lowest Ph

Cr (+2 charge)

Chromium (II)

All of the following species can function as Brönsted-Lowry bases in solution EXCEPT... (A) H2O (B) NH3 (C) S2− (D) NH4+ (E) HCO3−

what is the most heat resistant VIRUS in the worl

HBV; can be transmitted through sex or feces, food, water

Conjugate acid of Cl-

HCl

At the cathode...

Ions gain electrons.

What is an electrolyte?

Liquids that are good conductors of electricity

non-electrolytes are ......

Liquids that do not conduct electricity

MnO₂ + HCl → MnCl₂ + Cl₂ + H₂O

MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

Ni (+2 charge)

Nickel

N₂ + F₂ → NF₃

N₂ + 3F₂ → 2NF₃

Concentrated sulfuric acid change

Pungent gas is produced

Sb₂S₃ + HCl → H₃SbCl₆ + H₂S

Sb₂S₃ + 12HCl → 2H₃SbCl₆ + 3H₂S

Scandium

Groin: the gonads

Secrete sex steroids. Male: androgens, female: estrogen + progrsterone

If a substance gives up the electrons readily it is known as a...?

Strong reducing agent

Electrolysis

The breaking down of an ionic compound when molten or in an aqueous solution by the passage of electricity.

SCN (-1 charge)

Thiocyanate

True or False The number of electrons lost must equal the number of electrons gained.

True

NAD+ and NADH

When it got reduced to NADH, the postive + went away NADH gained hydrogen ions and electrons

Oxidation of any free element is...?

Zero

Zn (+2 charge)

Zinc

__Mg + __Cl₂ --> __MgCl₂

balanced

__MgO + __SO₃ --> __MgSO₄

balanced

__PCl₃ + __Cl₂ --> __PCl₅

balanced

Kb is what constant? ____ _________

base dissociation

A pH of 14 is strongly

basic

In any aqueous solution, when [H+] increases, [OH-] _____

decreases

When [H+] ______, [OH-] increases

decreases

In NADH, NAD+'s reduced form.. it is carrying

hydrogen ions and electrons.. potential energy

miss follicle

incorrect angle, increased pain and bruising, red scabs, % of infection increases

How to make insoluble salts

ion

erythema

redness

concordant

results that agree (very close together)

(NH₄)₂Cr₂O₇ → Cr₂O₃ + H₂O + N₂

(NH₄)₂Cr₂O₇ → Cr₂O₃ + 4H₂O + N₂

(NH4)2BeF4 -> BeF2 + NH3 + HF

...

K3[Fe(SCN)6] + Na2Cr2O7 + H2SO4 -> Fe(NO3)3 + Cr2(SO4)3 + CO2 + H2O + Na2SO4 + KNO3

...

K4Fe(CN)6 + KMnO4 + H2SO4 -> KHSO4 + Fe2(SO4)3 + MnSO4 + HNO3 + CO2 + H2O

...

K4[Fe(SCN)6] + K2Cr2O7 + H2SO4 -> Fe2(SO4)3 + Cr2(SO4)3 + CO2 + H2O + K2SO4 + KNO3

...

S + N₂O → SO₂ + N₂

1 S + 2 N₂O → 1 SO₂ + 2 N₂

SO₂ + H₂O → H₂SO₃

1 SO₂ + 1 H₂O → 1 H₂SO₃

SO₃ + H₂O → H₂SO₄

1 SO₃ + 1 H₂O → 1 H₂SO₄

SiC + Cl₂ → SiCl₄ + C

1 SiC + 2 Cl₂ → 1 SiCl₄ + 1 C

Method to make copper sulfate (crystals) with copper oxide and sulphuric acid

1) Add copper oxide and hot sulfuric acid to a beaker 2) Add copper oxide (i.e 3 spatulas) until it stops reacting with the acid/stops releasing carbon dioxide (fizzing) - this will tell us when all the acid has been used (saturated solution) CuO + H2SO4 --> CuSO4 + H2O 3) Filter the reaction mixture using a funnel with filter paper inside to remove excess copper carbonate. Once the process is over, pure copper sulfate solution is left in the flask 4) Leave to evaporate by putting the pure copper sulfate solution in an evaporating basin which is heated strongly by a Bunsen burner until half of the water has evaporated. Remaining water left to evaporate over a number of hours to form copper sulfate crystals

How to test for sulfate ions

1) Add dilute hydrochloric acid to the substance - this will remove any cabronates/sulfites which may react with the barium ions to form white precipitate. This can result to confusion in our results 2) Add barium chloride solution (containing barium ions) 3) If any sulfate ions are present, white precipitate will form which will be a positive result

__N₂ + __O₂ --> __NO

1, 1, 2

size of needle for male

4-5

Bitter taste

Base

sulfur dioxide

SO2

Sulphuric acid forms

Sulfate salts

SO3 (-2 charge)

Sulfite

Punngent gas produced

Sulfur dioxide

Hydrochloric acid forms

chlorine salts

What does respiration mean?

exchange of gases.. Respiration is when oxygen from the air move into the cells and the C02 in the cells moves out.

Are humans efficient at harvesting energy?

no. we must strip electron's energy off very slowly, making us inefficient at it.

K2Cr207

potassium dichromate

Base

- any substance that has a pH greater than 7 - if a base dissolves in water, it is called an alkali

titre

- the concentration of a solution determined by the titration - the minimum volume of a solution needed to reach the end point in a titration.

(NH4)2Cr2O7 -> NH3 + H2O + Cr2O3 + O2

...

(NH4)3AsS4 + HCl -> As2S5 + H2S + NH4Cl

...

Ag2S + KCN -> KAg(CN)2 + K2S

...

AgNO3 + FeCl3 -> Fe(NO3)3 + AgCl

...

Al + FeO -> Al2O3 + Fe

...

Al + HCl -> AlCl3 + H2

...

Al + KOH + H2O -> KAlO2 + H2

...

Al + NH4ClO4 -> Al2O3 + AlCl3 + NO + H2O

...

Al + NaOH + H2O -> NaAl(OH)4 + H2

...

Al + O2 -> Al2O3

...

Al(NO3)3 + Na2CO3 -> Al2(CO3)3 + NaNO3

...

Al(OH)3 + H2SO4 -> Al2(SO4)3 + H2O

...

Be(OH)2 + NH4HF2 -> (NH4)2BeF4 + H2O

...

Bi(NO3)3 + H2S -> Bi2S3 + HNO3

...

C + SiO2 + Cl2 -> SiCl4 + CO

...

C10H16 + Cl2 -> C + HCl

...

C2H2 + O2 -> CO2 + H2O

...

C2H3Cl + O2 -> CO2 + H2O + HCl

...

C2H5OH + O2 -> CO + H2O

...

C2H5OH + O2 -> CO2 + H2O

...

C3H8 + O2 -> CO2 + H2O

...

C4H10 + O2 -> CO2 + H2O

...

C6H6 + O2 -> CO2 + H2O

...

Ca3(PO4)2 + SiO2 + C -> CaSiO3 + P4 + CO

...

Ca3(PO4)2 + SiO2 -> CaSiO3 + P2O5

...

Ca3(PO4)2 + SiO2 -> P4O10 + CaSiO3

...

Ca3P2 + H2O -> Ca(OH)2 + PH3

...

Ca5F(PO4)3 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF

...

CaCN2 + H2O -> CaCO3 + NH3

...

CaHPO4⋅2H2O + NaOH + H2O -> Na2HPO4⋅12H2O + Ca(OH)2

...

CaS2 + O2 -> CaS2O3

...

Cr(OH)3 + H2SO4 -> Cr2(SO4)3 + H2O

...

Cu + CO2 + O2 + H2O -> CuCO3⋅Cu(OH)2

...

Fe + O2 -> Fe2O3

...

FeCl3 + Ca(OH)2 -> CaCl2 + Fe(OH)3

...

FeCl3 + NH4OH -> Fe(OH)3 + NH4Cl

...

FeO + H3PO4 -> Fe3(PO4)2 + H2O

...

FeS + O2 -> Fe2O3 + SO2

...

FeS2 + O2 -> Fe2O3 + SO2

...

FeSO4 + K3[Fe(CN)6] -> Fe3[Fe(CN)6]2 + K2SO4

...

H2S + Cl2 -> S8 + HCl

...

H2SO4 + Al(OH)3 -> Al2(SO4)3 + H2O

...

H2SO4 + HI -> H2S + I2 + H2O

...

H2SO4 + NaHCO3 -> Na2SO4 + CO2 + H2O

...

I2 + HNO3 -> HIO3 + NO2 + H2

...

K2CO3 + C + N2 -> KCN + CO

...

K2MnO4 + H2SO4 -> KMnO4 + MnO2 + K2SO4 + H2O

...

K3AsO4 + H2S -> As2S5 + KOH + H2O

...

KO2 + CO2 -> K2CO3 + O2

...

KOH + AlCl3 -> KCl + Al(OH)3

...

Mg3N2 + H2O -> Mg(OH)2 + NH3

...

MgNH4AsO4 + 6H2O -> Mg2As2O7 + NH3 + H2O

...

MgNH4PO4 -> Mg2P2O7 + NH3 + H2O

...

MnO2 + HCl -> MnCl2 + H2O + Cl2

...

Na3AsO3 + H2S -> As2S3 + NaOH

...

NaCl + H2SO4 -> Na2SO4 + HCl

...

NaOH + Cl2 -> NaCl + NaClO + H2O

...

NaOH + Zn(NO3)2 -> NaNO3 + Zn(OH)2

...

NiS + O2 -> NiO + SO2

...

P4 + H2O -> H3PO4 + H2

...

P4 + O2 -> P2O5

...

P4O10 + H2O -> H3PO4

...

P4O10 + HCl -> POCl3 + HPO3

...

P4O6 + H2O -> H3PO3

...

P4O6 -> P4 + P2O4

...

PCl3 + H2O -> H3PO3 + HCl

...

Si + S8 -> Si2S4

...

Si2H3 + O2 -> SiO2 + H2O

...

SiCl4 + H2O -> H4SiO4 + HCl

...

SiH4 + O2 -> SiO2 + H2O

...

SiO2 + HF -> SiF4 + H2O

...

Sn(OH)2 + NaOH -> Na2SnO2 + H2O

...

Sn(OH)4 + NaOH -> Na2SnO3 + H2O

...

TiCl4 + Mg -> MgCl2 + Ti

...

U3O8 + HNO3 -> UO2(NO3)2 + NO2 + H2O

...

(CuOH)₂CO₃ → CuO + CO₂ + H₂O

1 (CuOH)₂CO₃ → 2 CuO + 1 CO₂ + 1 H₂O

Al(OH)₃ + NaOH → NaAlO₂ + H₂O

1 Al(OH)₃ + 1 NaOH → 1 NaAlO₂ + 2 H₂O

CaCO₃ → CaO + CO₂

1 CaCO₃ → 1 CaO + 1 CO₂

CaC₂ + N₂ → CaCN₂ + C

1 CaC₂ + 1 N₂ → 1 CaCN₂ + 1 C

NaH₂PO₄ → NaPO₃ + H₂O

1 NaH₂PO₄ → 1 NaPO₃ + 1 H₂O

NaPO₃ + CuO → NaCuPO₄

1 NaPO₃ + 1 CuO → 1 NaCuPO₄

[Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + KMnO₄ + H₂SO₄ → K₂Cr₂O₇ + MnSO₄ + CO₂ + KNO₃ + K₂SO₄ + H₂O ***This is the mother of all chemical equations***

10 [Cr(N₂H₄CO)₆]₄[Cr(CN)₆]₃ + 1176 KMnO₄ + 1399 H₂SO₄ → 35K₂Cr₂O₇ + 1176 MnSO₄ + 420 CO₂ + 660 KNO₃ + 223 K₂SO₄ + 1879 H₂O

# of buffer systems crucial in maintaining human blood pH within a narrow range (pH 7.35-7.45)

CO + O₂ → CO₂

2 CO + 1 O₂ → 2 CO₂

ClO₂ + H₂O → HClO₂ + HClO₃

2 ClO₂ + 1 H₂O → 1 HClO₂ + 1 HClO₃

Cu(CN)₂ → CuCN + C₂N₂

2 Cu(CN)₂ → 2 CuCN + 1 C₂N₂

Al + HCl → AlCl₃ + H₂

2Al + 6HCl → 2AlCl₃ + 3H₂

Na₃PO₄ + CaCl₂ → NaCl + Ca₃(PO₄)₂

2Na₃PO₄ + 3CaCl₂ → 6NaCl + Ca₃(PO₄)₂

What are electrodes?

A graphite (inert) or metal strip that conducts electricity.

Any change in oxidation number of an atom indicates what?

A redox reaction has taken place

Slippery feel

Acid

Said that acids are hydrogen-containing compounds that ionize to yield hydrogen ions (H+) in aqueous solutions.

Arrhenius

Said that bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution

Arrhenius

Three types of acids and bases: (hint: in alphabetical order)

Arrhenius, Bronsted-Lowry, Lewis

Why is alkali not measured using the burette

As alkali can damage glass wear

A 1-molar solution of which of the following salts has the highest pH? (A) NaNO3 (B) Na2CO3 (C) NH4Cl (D) NaHSO4 (E) Na2SO4

Nitric acid change

Brown gas produced

Iron(III) salts

Brown or orange

What colour precipitate does Fe3+ produce when tested?

Brown precipitate

Conjugate base of CH₃COOH

CH3COO-

Cn (-1 charge)

Cyanide

Acids that contain two ionizable hydrogens

Diprotic

Iron(III) salts

Fe3+

Negative ions

Form at the anode.

Alpha £

Glucagon

Glucagon=

Hormone

At the anode...

Ions lose electrons.

C2O4 (-2 charge)

Oxalate

The anode is the ........

Positive electrode

Anode

Positive electrode.

P₄ + O₂ → P₂O₃

P₄ + 3O₂ → 2P₂O₃

RIG

Reduction is gain of electrons

Ag (+1 charge)

Silver

Cortisol

Steroid hormone secreted by the adrenal glands in response to tissue damage

Sn (+2 charge)

Tin (II)

reversible reaction

a chemical reaction in which the products re-form the original reactants

name 2 metals less reactive than hydrogen

copper and silver

According to Lewis, a substance can accept or donate a pair of electrons to form a ____ bond

covalent

What forms at the cathode?

either a metal or hydrogen

Name the buffer system involving etha--

ethanoic acid-ethanoate ion

True or false: all salts are neutral

false

a method of balancing redox reactions by balancing the oxidation and reduction half-reactions

half-reaction method

Strong acids have ___ Ka values

large

If it is an oxidation, I will...

loose an electron

concentration formula

moles/volume

what is spread viral

mumps, rubella, chicken pox, polio

neutral

Acidified potassium manganate

purple to colourless

The solution of known concentration is called the

standard solution

___ acids are completely ionized in aqueous solutions

strong

Example of diprotic acid (name)

sulfuric acid

what are molten ionic compounds broken into

their elements (metal and non metal)

inert substance is ........

unreactive

Example of amphoteric substance (common name)

water

adrenal glands

(Suprarrenales) sit on top of kidneys

Neutralisation (1st acid equation)

- A reaction of an acid with a base, forming a salt and water - acid + alkali ---> salt + water - H+ + OH- ---> H2O - example: hydrochloric acid + sodium hydroxide --> sodium chloride + water

H in NaH

-1

Hydrogen's oxidation number?

1+ when combined with nonmetals 1- when combines with metals

1dm3 =

1000cm3

HAsO₂ → As₂O₃ + H₂O

2 HAsO₂ → 1 As₂O₃ + 1 H₂O

HAsO₃ → As₂O₅ + H₂O

2 HAsO₃ → 1 As₂O₅ + 1 H₂O

MgCl2 Oxidation Number

2+(2 x -1)=0

__NaOH + __CO₂ --> __Na₂CO₃ + __H₂O

2, 1, 1, 1

AgNO₃ + Cu → Cu(NO₃)₂ + Ag

2AgNO₃ + Cu → Cu(NO₃)₂ + 2Ag

HgO → Hg + O₂

2HgO → 2Hg + O₂

what is the half equation for the reaction at the positive electrode in the electrolysis of bauxite

2O²- ---> O² + 4e-

AgBr + GaPO₄ → Ag₃PO₄ + GaBr₃

3AgBr + GaPO₄ → Ag₃PO₄ + GaBr₃

How do we lose potential energy?

Because we do respiration in steps, every time we will lose energy. We lose the potential energy by losing heat in our bodies.

Be₂C + H₂O → Be(OH)₂ + CH₄

Be₂C + 2H₂O → 2Be(OH)₂ + CH₄

Conjugate acid of CH₃COO-

CH₃COOH

C₃H₈ + O₂ → CO₂ + H₂O

C₃H₈ + 5O₂ → 3CO₂ + 4H₂O

C₅H₁₂ + O₂ → CO₂ + H₂O

C₅H₁₂ + 8O₂ → 5CO₂ + 6H₂O

What two ions form when water dissociates?

H+ and OH-

oxidation number

Indicates the oxidation state of an element in its free state or in a compound

Beta B

Insulin

Hydrogen -1

NaH(+1,-1)

Formula for sodium hydroxide

NaOH

What colour precipitate does Fe2+ produce when tested?

Pale green precipitate

S + HNO₃ → H₂SO₄ + NO₂ + H₂O

S + 6HNO₃ → H₂SO₄ + 6NO₂ + 2H₂O

SO₂ + Li₂Se → SSe₂ + Li₂O

SO₂ + 2Li₂Se → SSe₂ + 2Li₂O

Pancreas

Sits behind the stomach, hormonal cells. Secretes hormones & glucagon

A pH of 0 is strongly

acidic

______ is a solution in which the pH remains relatively constant when small amounts of acid or base are added

buffer

calculating moles (2)

concentration x volume

H2PO4 (-1 charge)

dihydrogen phosphate

insertion= when over insertion can cause..

good in HF can cause petechiae

electron acceptor?

oxidizing agent

Cesium Oxidation Number

Group 1 metals oxidation number in their compounds

H in H20

H in NH3

K in K2SO4 oxi #

Na in NaCl oxi #

What is the unusual oxidation number of oxygen in a compound?

Thallium oxi#s

+1,+3

Hydrogen in its compounds

+1,-1 in ionic hydrides

Beryllium oxidation number

Ca in CaO

Group II metals oxi#in their compounds

Magnesium Oxidation Number!

Mg in MgCl2

Radium oxi #

Scrontium oxi #

Hg oxidation number

+2,+1

Actinium oxi#

Aluminium oxi#

Scandium oxidation number

Cr oxidation number

+3, +6

C in NaHCO3

SnCL4 (Sn)

Silicon oxi#

+4,-4

(S) SO4 -2

K2Cr2O7

KMnO4.Mn oxidation

Rule 4 for MnO4-

Neutralisation of dilute acids with bases - metal carbonate (2nd acid equation)

- Acid + metal carbonate --> salt + water + carbon dioxide - 2HCL + Na2CO3 --> 2NaCl + H2O + CO2 hydrochloric acid + sodium carbonate --> Sodium chloride + water + carbon dioxide - H2SO4 + Cu2CO3 --> Cu2SO4 + H2O + CO2 sulfuric acid + copper carbonate ---> Copper sulphate + water + carbon dioxide

formula for copper sulfate crystals

- Copper carbonate + sulfuric acid ---> copper sulphate + water + carbon dioxide CuCO3 + H2SO4(aq) ---> CuSO4(aq) + H2O + CO2

Alkali composition

- Dissolve in water and split up forming hydroxide ions (ionise) - Strong alkalis fully ionise in water - Weak alkalis only partially ionise in water - Ammonia is an alkali (NH3)

Naming salts

- First part of name comes form the metal in the alkali base - Second part comes from the acid - NaOH + HCl ---> NaCl + H2O - Sodium hydroxide + hydrochloric acid --> sodium chloride + water

Neutralisation of strong acids and bases

- HCl + KOH ---> KCl + H2O hydrochloric acid + potassium hydroxide --> potassium chloride + water - H2SO4 + NaOH --> Na2SO4 + H2O sulfuric acid + sodium hydroxide --> sodium sulfate + water

Acid reactions with metals (4rd acid equation)

- acid + metal --> salt + hydrogen hydrochloric acid + magnesium --> magnesium chloride + hydrogen - cannot see salt produced as it has been dissolved in the acid observations with magnesium: effervescence - hydrogen gas produced quickly, reacts immediately with acid observation with zinc: slight fizzing, hydrogen gas rises towards the surface as more acid is added, slow reaction observations with iron: slow reaction with acid: tiny bubbles of hydrogen gas rising towards the surface of the acid (very small fizz), very slow reaction, observation: no reaction

Acid composition

- contains hydrogen ions - acids splits up to form a hydrogen ion and another ion in water (ionise). HCl (aq) ---> H+ (aq) + Cl- - Hydrogen ions gives acids their characteristics - Strong acids fully ionise in water to release H+ ions (hydrochloric acid, sulphuric acid, nitric acid). pH is usually from 0-2 - Weak acids (ethnic, critic, carbonic) only partially ionise to release H+ ions

Transition metals

- elements that form a bridge between elements on the left and right sides of the periodic table - high melting/boilng points - malleable - high density - good electrical + thermal conductivity - form coloured compounds - good catalysts

SnCl4 (Cl)

-1

Group VII element

-1in halides sometimes positive for Cl,Br and I

O in CO2

-2

O in Na2O

-2

Oxygen in its compounds

-2,except in peroxides and superoxides

The [H+] of a basic solution is less than 1 x 10^?M

-7

The [H+] of an acidic solution is greater than 1 x 10^? M

-7

(NH4)2Cr2O7 -> Cr2O3 + N2 + H2O

...

Al2(SO4)3 + Ca(OH)2 -> CaSO4 + Al(OH)3

...

Al2O3 + C + N2 -> AlN + CO

...

Al4C3 + H2O -> CH4 + Al(OH)3

...

AlCl3 + AgNO3 -> AgCl + Al(NO3)3

...

As + NaOH -> Na3AsO3 + H2

...

As2O5 + H2O -> H3AsO4

...

Au + HCl + HNO3 -> AuCl3 + NO + H2O

...

Au + KCN + O2 + H2O -> K[Au(CN)2] + KOH

...

Au2O3 -> Au + O2

...

Au2S3 + H2 -> Au + H2S

...

B2O3 + H2O -> H3BO3

...

BaCl2 + Al2(SO4)3 -> BaSO4 + AlCl3

...

C7H10N + O2 -> CO2 + H2O + NO2

...

C7H16 + O2 -> CO2 + H2O

...

C7H6O2 + O2 -> CO2 + H2O

...

CH4 + O2 -> CO2 +H2O

...

CO2 + H2O -> C6H12O6 + O2

...

Ca + AlCl3 -> CaCl2 + Al

...

Ca(NO3)2 -> CaO + NO2 + O2

...

Ca(OH)2 + P4O10 + H2O -> Ca(H2PO4)2

...

Ca10F2(PO4)6 + H2SO4 -> Ca(H2PO4)2 + CaSO4 + HF

...

Ca3(PO4)2 + C -> Ca3P2 + CO

...

Ca3(PO4)2 + H2SO4 -> CaSO4 + H3PO4

...

Ca3(PO4)2 + H3PO4 -> Ca(H2PO4)2

...

CuSO4 + KCN -> CuCN + K2SO4 + C2N2

...

Fe + H2O + O2 -> Fe2O3.H2O

...

Fe + H2O -> Fe3O4 + H2

...

Fe(OH)3 -> Fe2O3 + H2O

...

Fe2(SO4)3 + Ba(NO3)2 -> BaSO4 + Fe(NO3)3

...

Fe2(SO4)3 + KOH -> K2SO4 + Fe(OH)3

...

Fe2O3 + C -> CO + Fe

...

Fe2O3 + CO -> Fe + CO2

...

Fe2O3 + H2 -> Fe + H2O

...

Fe3O4 + H2 -> Fe + H2O

...

FeC2O4⋅2H2O + H2C2O4 + H2O2 + K2C2O4 -> K3[Fe(C2O4)3]⋅3H2O

...

H3AsO3 -> As2O3 + H2O

...

H3BO3 + Na2CO3 -> Na2B4O7 + CO2 + H2O

...

H3BO3 -> H4B6O11 + H2O

...

H3PO3 -> H3PO4 + PH3

...

H3PO4 + (NH4)2MoO4 + HNO3 -> (NH4)3PO4⋅2MoO3 + NH4NO3 + H2O

...

H3PO4 + Ca(OH)2 -> Ca(H2PO4)2 + H2O

...

H3PO4 + HCl -> PCl5 + H2O

...

HCl + HNO3 -> NOCl + Cl2 + H2O

...

HCl + K2CO3 -> KCl + H2O + CO2

...

HClO4 + P4O10 -> H3PO4 + Cl2O7

...

Hg(OH)2 + H3PO4 -> Hg3(PO4)2 + H2O

...

Hg2CrO4 -> Cr2O3 + Hg + O2

...

KBr + Al(ClO4)3 -> AlBr3 + KClO4

...

KClO3 -> KCl + O2

...

KClO3 -> KClO4 + KCl

...

KNO3 + C12H22O11 -> N2 + CO2 + H2O + K2CO3

...

MnO2 + KOH + O2 -> K2MnO4 + H2O

...

NH3 + NO -> N2 + H2O

...

NH3 + O2 -> HNO2 + H2O

...

NH3 + O2 -> NO + H2O

...

NH4Cl + Ca(OH)2 -> CaCl2 + NH3 + H2O

...

NH4VO3 -> V2O5 + NH3 + H2O

...

NO + NaOH -> NaNO2 + H2O + N2O

...

Na + H2O -> NaOH + H2

...

Na2B4O7 + HCl + H2O -> NaCl + H3BO3

...

Na2CO3 + HCl -> NaCl + H2O + CO2

...

Na2O2 + H2O -> NaOH + O2

...

Na2S2 + O2 -> Na2S2O3

...

Na2SnO3 + H2S -> SnS2 + NaOH + H2O

...

PCl5 + H2O -> H3PO4 + HCl

...

PCl5 + P2O5 -> POCl3

...

POCl3 + H2O -> H3PO4 + HCl

...

Pb + Na + C2H5Cl -> Pb(C2H5)4 + NaCl

...

Pb(NO3)2 -> PbO + NO2 + O2

...

Pb(OH)2 + NaOH -> Na2PbO2 + H2O

...

Pb3(VO4)2⋅PbCl2 + HCl -> VO2Cl + PbCl2 + H2O

...

Pb3O4 + HNO3 -> Pb(NO3)2 + PbO2 + H2O

...

S8 + O2 -> SO3

...

Sb + O2 -> Sb4O6

...

Se + NaOH -> Na2Se + Na2SeO3 + H2O

...

Si + NaOH + H2O -> Na2SiO3 + H2

...

UO2 + HF -> UF4 + H2O

...

UO2(NO3)2⋅6H2O -> UO3 + NO2 + O2 + H2O

...

V2O5 + Al -> Al2O3 + V

...

V2O5 + Ca -> CaO + V

...

V2O5 + HCl -> VOCl3 + H2O

...

VO2Cl + NH4OH -> NH4VO3 + NH4Cl + H2O

...

Zn + NaOH + H2O -> Na2Zn(OH)4 + H2

...

[Ag(NH3)2]Cl + HNO3 -> NH4NO3 + AgCl

...

Cl2 oxidation number

Na oxidation number

The pH scale ranges from __ to __

0, 14

(CN)₂ + NaOH → NaCN + NaOCN + H₂O

1 (CN)₂ + 2 NaOH → 1 NaCN + 1 NaOCN + 1 H₂O

(NH₄)₂SO₄ + CaCO₃ → (NH₄)₂CO₃ + CaSO₄

1 (NH₄)₂SO₄ + 1 CaCO₃ → 1 (NH₄)₂CO₃ + 1 CaSO₄

AgBr + Na₂S₂O₃ → Na₃[Ag(S₂O₃)₂] + NaBr

1 AgBr + 2 Na₂S₂O₃ → 1 Na₃[Ag(S₂O₃)₂] + 1 NaBr

AlN + H₂O → NH₃ + Al(OH)₃

1 AlN + 3 H₂O → 1 NH₃ + 1 Al(OH)₃

Al₂O₃ + Na₂CO₃ → NaAlO₂ + CO₂

1 Al₂O₃ + 1 Na₂CO₃ → 2 NaAlO₂ + 1 CO₂

As₂O₃ + H₂O → H₃AsO₃

1 As₂O₃ + 3 H₂O → 2 H₃AsO₃

BaCO₃ + HNO₃ → Ba(NO₃)₂ + CO₂ + H₂O

1 BaCO₃ + 2 HNO₃ → 1 Ba(NO₃)₂ + 1 CO₂ + 1 H₂O

BaO + H₂O → Ba(OH)₂

1 BaO + 1 H₂O → 1 Ba(OH)₂

BaO₂ + H₂SO₄ → BaSO₄ + H₂O₂

1 BaO₂ + 1 H₂SO₄ → 1 BaSO₄ + 1 H₂O₂

BaSO₂ + H₂SO₄ → Ba(HSO₄)₂

1 BaSO₂ + 1 H₂SO₄ → 1 Ba(HSO₄)₂

Be(OH)₂ → BeO + H₂O

1 Be(OH)₂ → 1 BeO + 1 H₂O

BeF₂ + Mg → MgF₂ + Be

1 BeF₂ + 1 Mg → 1 MgF₂ + 1 Be

BeO + C + Cl₂ → BeCl₂ + CO

1 BeO + 1 C + 1 Cl₂ → 1 BeCl₂ + 1 CO

BeSO₄ + NH₄OH → Be(OH)₂ + (NH₄)₂SO₄

1 BeSO₄ + 2 NH₄OH → 1 Be(OH)₂ + 1 (NH₄)₂SO₄

C + H₂O → CO + H₂

1 C + 1 H₂O → 1 CO + 1 H₂

CO₂ + NH₃ + H₂O → NH₄HCO₃

1 CO₂ + 1 NH₃ + H₂O → 1 NH₄HCO₃

CO₂ + NH₃ → OC(NH₂)₂ + H₂O

1 CO₂ + 2 NH₃ → 1 OC(NH₂)₂ + 1 H₂O

Ca(ClO₃)₂ → CaCl₂ + O₂

1 Ca(ClO₃)₂ → 1 CaCl₂ + 3 O₂

Ca(HCO₃)₂ → CaCO₃ + CO₂ + H₂O

1 Ca(HCO₃)₂ → 1 CaCO₃ + 1 CO₂ + 1 H₂O

Ca(OH)₂ + CO₂ → CaCO₃ + H₂O

1 Ca(OH)₂ + 1 CO₂ → 1 CaCO₃ + 1 H₂O

Ca(OH)₂ + H₃PO₄ → CaHPO₄ + H₂O

1 Ca(OH)₂ + 1 H₃PO₄ → 1 CaHPO₄ + 2 H₂O

Ca(OH)₂ + CO₂ → Ca(HCO₃)₂

1 Ca(OH)₂ + 2 CO₂ → 1 Ca(HCO₃)₂

CaCO₃ + HCl → CaCl₂ + H₂O + CO₂

1 CaCO₃ + 2 HCl → 1 CaCl₂ + 1 H₂O + 1 CO₂

CaC₂ + H₂O → C₂H₂ + Ca(OH)₂

1 CaC₂ + 2 H₂O → 1 C₂H₂ + 1 Ca(OH)₂

CaO + H₂O → Ca(OH)₂

1 CaO + 1 H₂O → 1 Ca(OH)₂

CaO + C → CaC₂ + CO

1 CaO + 3 C → 1 CaC₂ + 1 CO

CaS + H₂O → Ca(OH)₂ + H₂S

1 CaS + 2 H₂O → 1 Ca(OH)₂ + 1 H₂S

CaSO₄ → CaS + O₂

1 CaSO₄ → 1 CaS + 2 O₂

Ca₃(PO₄)₂ + H₂SO₄ → CaSO₄ + Ca(H₂PO₄)₂

1 Ca₃(PO₄)₂ + 2 H₂SO₄ → 2 CaSO₄ + 1 Ca(H₂PO₄)₂

CdSO₄ + H₂S → CdS + H₂SO₄

1 CdSO₄ + 1 H₂S → 1 CdS + 1 H₂SO₄

CuSO₄ + KCN → Cu(CN)₂ + K₂SO₄

1 CuSO₄ + 2 KCN → 1 Cu(CN)₂ + 1 K₂SO₄

FeS + H₂SO₄ → H₂S + FeSO₄

1 FeS + 1 H₂SO₄ → 1 H₂S + 1 FeSO₄

Fe₂O₃ + SiO₂ → Fe₂Si₂O₇

1 Fe₂O₃ + 2 SiO₂ → 1 Fe₂Si₂O₇

Hg₂CO₃ → Hg + HgO + CO₂

1 Hg₂CO₃ → 1 Hg + 1 HgO + 1 CO₂

H₂CO₃ → H₂O + CO₂

1 H₂CO₃ → 1 H₂O + 1 CO₂

H₂SO₃ → H₂O + SO₂

1 H₂SO₃ → 1 H₂O + 1 SO₂

H₃PO₄ + Ca(OH)₂ → CaHPO₄⋅2H₂O

1 H₃PO₄ + 1 Ca(OH)₂ → 1 CaHPO₄⋅2H₂O

H₄As₂O₇ → As₂O₅ + H₂O

1 H₄As₂O₇ → 1 As₂O₅ + 2 H₂O

K₂O + H₂O → KOH

1 K₂O + 1 H₂O → 2 KOH

Li₂O + H₂O → LiOH

1 Li₂O + 1 H₂O → 2 LiOH

MnO₂ + K₂CO₃ + KNO₃ → K₂MnO₄ + KNO₂ + CO₂

1 MnO₂ + 1 K₂CO₃ + 1 KNO₃ → 1 K₂MnO₄ + 1 KNO₂ + 1 CO₂

MnS + HCl → H₂S + MnCl₂

1 MnS + 2 HCl → 1 H₂S + 1 MnCl₂

Mn₂O₃ + Al → Al₂O₃ + Mn

1 Mn₂O₃ + 2 Al → 1 Al₂O₃ + 2 Mn

NH₃ + O₂ → HNO₃ + H₂O

1 NH₃ + 2 O₂ → 1 HNO₃ + 1 H₂O

NH₄NO₃ → N₂O + H₂O

1 NH₄NO₃ → 1 N₂O + 2 H₂O

NaCl + NH₄HCO₃ → NaHCO₃ + NH₄Cl

1 NaCl + 1 NH₄HCO₃ → 1 NaHCO₃ + 1 NH₄Cl

Na₂Cr₂O₇ + S → Cr₂O₃ + Na₂SO₄

1 Na₂Cr₂O₇ + 1 S → 1 Cr₂O₃ + 1 Na₂SO₄

Na₂O + H₂O → NaOH

1 Na₂O + 1 H₂O → 2 NaOH

Na₂SO₃ + S → Na₂S₂O₃

1 Na₂SO₃ + 1 S → 1 Na₂S₂O₃

N₂ + H₂ → NH₃

1 N₂ + 3 H₂ → 2 NH₃

N₂O₃ + H₂O → HNO₂

1 N₂O₃ + 1 H₂O → 2 HNO₂

N₂O₅ + H₂O → HNO₃

1 N₂O₅ + 1 H₂O → 2 HNO₃

PCl₅ + H₂O → POCl₃ + HCl

1 PCl₅ + 1 H₂O → 1 POCl₃ + 2 HCl

PCl₅ + KNO₂ → NOCl + POCl₃ + KCl

1 PCl₅ + 1 KNO₂ → 1 NOCl + 1 POCl₃ + 1 KCl

PbCrO₄ + HNO₃ → Pb(NO₃)₂ + H₂CrO₄

1 PbCrO₄ + 2 HNO₃ → 1 Pb(NO₃)₂ + 1 H₂CrO₄

SiO₂ + Ca(OH)₂ → CaSiO₃ + H₂O

1 SiO₂ + 1 Ca(OH)₂ → 1 CaSiO₃ + 1 H₂O

SiO₂ + Na₂CO₃ → Na₂SiO₃ + CO₂

1 SiO₂ + 1 Na₂CO₃ → 1 Na₂SiO₃ + 1 CO₂

SrBr₂ + (NH₄)₂CO₃ → SrCO₃ + NH₄Br

1 SrBr₂ + 1 (NH₄)₂CO₃ → 1 SrCO₃ + 2 NH₄Br

UF₄ + Mg → MgF₂ + U

1 UF₄ + 2 Mg → 2 MgF₂ + 1 U

UO₃ + H₂ → UO₂ + H₂O

1 UO₃ + 1 H₂ → 1 UO₂ + 1 H₂O

Xe + F₂ → XeF₆

1 Xe + 3 F₂ → 1 XeF₆

Zn + HCl → ZnCl₂ + H₂

1 Zn + 2 HCl → 1 ZnCl₂ + 1 H₂

Zn + KOH → K₂ZnO₂ + H₂

1 Zn + 2 KOH → 1 K₂ZnO₂ + 1 H₂

Zn(OH)₂ + NaOH → Na₂ZnO₂ + H₂O

1 Zn(OH)₂ + 2 NaOH → 1 Na₂ZnO₂ + 2 H₂O

Method to make copper sulfate (crystals) with copper carbonate and sulfuric acid

1) Add copper carbonate and sulfuric acid to a beaker 2) Add copper carbonate (i.e 3 spatulas) until it stops reacting with the acid/stops releasing carbon dioxide (fizzing) - this will tell us when all the acid has been used CuCO3 + H2SO4 (aq)---> CuSO4 (aq) + H2O + CO2 3) Filter the reaction mixture using a funnel with filter paper inside to remove excess copper carbonate. Once the process is over, pure copper sulfate solution is left in the flask 4) Leave to evaporate by putting the copper chloride in an evaporating basin which is heated strongly by a Bunsen burner until half of the water has evaporated. Remaining water left to evaporate over a number of hours to form copper sulfate crystals

Give two examples of redox reactions

1) The burning of wood in a fireplace 2) The metabolization of food by your body

How to set up a titration

1) Use a pipette to transfer the sodium hydroxide (alkali + analyse) into a conical flask and record volume added 2) Add a few drops of indicator - this is to see the end point (point when the analyse has been neutralised) 3) Place the conical flask on a white file and the funnel in the burette - this ensures we can see a colour change clearly 4) Pour acid into the funnel through the burette and read off initial volume 5) Add acid in a trial run order to get a rough idea what volume is required 6) In the first run, add acid until a colour change is observed. then add the acid drip by drip. This important as to not overshoot the end-point 7) The end volume is then read off 8) Swirl the mixture during the titration as this allows both solutions to properly dissolve 9) Repeat the process until similar (concordant) volumes are obtained. Any anomalies are excluded from calculating the mean value 10) This is a type of neutralisation reaction DISCLAIMER: when forming crystals with titration, only use indicator to calculate titre of a solution. then use the titre to neutralise the acid and alkali WITHOUT the indicator

__BaCl₂ + __Na₂SO₄ --> __NaCl + __BaSO₄

1, 1, 2, 1

__Cu + __HCl --> __CuCl₂ + __H₂

1, 2, 1, 1

__Mg + __HCl --> __MgCl₂ + __H₂

1, 2, 1, 1

__Mg + __HF --> __MgF₂ + __H₂

1, 2, 1, 1

__Sn + __HF --> __SnF₂ + __H₂

1, 2, 1, 1

__CS₂ + __O₂ --> __CO₂ + __SO₂

1, 3, 1, 2

__Al₂(SO₄)₃ + __Ca(OH)₂ --> __Al(OH)₃ + __CaSO₄

1, 3, 2, 3

Fluorine's oxidation number?

how is aluminium extracted from the ore bauxite (whole process)

1. electrolysis 2. aluminium oxide has a very high melting point so it's mixed with cryolite to lower the melting point. 3. the molten mixture contains free ions so it'll conduct electricity 4. the positive Al3+ ions are attracted to the negative electrode where they each pick up three electrons and turn into neutral aluminium atoms. These then sink down to the bottom of the electrolysis tank 5. the negative O2- ions are attracted to the positive electrode where they each lose two electrons. The neutral oxygen atoms will then combine to form O² molecules

For aqueous solutions, the product of the hydrogen-ion concentration and the hydroxide-ion concentration equals =

1.0 x 10⁻¹⁴

How does the ecosystem use photosynthesis to make energy?

1.Plants take C02 in atmosphere and water through roots, uses light energy to convert it into organic molecule such as glucose. Then it releases O2 (waste product) 2. The next process is cellular respiration .. it takes the organic molecules such as carbon, hydrogen, oxygen bonded together, r groups and proteins--it takes the energy stored in these carbon hydrogen bonds/ the molecules and combines it with 02 and then breaks it all back down.

HIO₃ → I₂O₅ + H₂O

2 HIO₃ → 1 I₂O₅ + 1 H₂O

HNO₂ + O₂ → HNO₃

2 HNO₂ + 1 O₂ → 2 HNO₃

HNO₃ + P₂O₅ → N₂O₅ + HPO₃

2 HNO₃ + 1 P₂O₅ → 1 N₂O₅ + 2 HPO₃

HgO → Hg + O₂

2 HgO → 2 Hg + 1 O₂

H₂ + O₂ → H₂O

2 H₂ + 1 O₂ → 2 H₂O

H₂O₂ → H₂O + O₂

2 H₂O₂ → 2 H₂O + 1 O₂

H₃AsO₄ → As₂O₅ + H₂O

2 H₃AsO₄ → 1 As₂O₅ + 3 H₂O

H₃PO₄ → H₄P₂O₇ + H₂O

2 H₃PO₄ → 1 H₄P₂O₇ + 1 H₂O

K + Br₂ → KBr

2 K + 1 Br₂ → 2 KBr

KHSO₄ → K₂S₂O₇ + H₂O

2 KHSO₄ → 1 K₂S₂O₇ + 1 H₂O

Mg(OH)₂ → (MgOH)₂O + H₂O

2 Mg(OH)₂ → 1 (MgOH)₂O + 1 H₂O

NaHCO₃ → Na₂CO₃ + CO₂ + H₂O

2 NaHCO₃ → 1 Na₂CO₃ + 1 CO₂ + 1 H₂O

NaOH + FeSO₄ → Na₂SO₄ + Fe(OH)₂

2 NaOH + 1 FeSO₄ → 1 Na₂SO₄ + 1 Fe(OH)₂

Na₂HPO₄ → Na₄P₂O₇ + H₂O

2 Na₂HPO₄ → 1 Na₄P₂O₇ + 1 H₂O

N₂ + O₂ → N₂O

2 N₂ + 1 O₂ → 2 N₂O

__CO + __O₂ --> __CO₂

2, 1, 2

__H₂ + __O₂ -->__H₂O

2, 1, 2

__K + __I₂ --> __KI

2, 1, 2

__Mg + __O₂ --> __MgO

2, 1, 2

__Na + __F₂ --> __NaF

2, 1, 2

__SO₂ + __O₂ --> __SO₃

2, 1, 2

__LiCl + __Mg(NO₃)₂ --> __LiNO₃ + __MgCl₂

2, 1, 2, 1

__Na + __MgF₂ --> __NaF + __Mg

2, 1, 2, 1

__K + __H₂O --> __KOH + __H₂

2, 2, 2, 1

__Al + __Cl₂ --> __AlCl₃

2, 3, 2

__MgS + __O₂ --> __MgO + __SO₂

2, 3, 2, 2

__Al + __Cu(NO₃)₂ --> __Cu + __Al(NO₃)₃

2, 3, 3, 2

Oxygen's oxidation number?

2- in most compounds and ions 1- in peroxides 2+ when combined with F

Ag₂O → Ag + O₂

2Ag₂O → 4Ag + O₂

Al + H₂SO₄ → Al₂(SO₄)₃ + H₂

2Al + 3H₂SO₄ → Al₂(SO₄)₃ + 3H₂

AlBr₃ + K₂SO₄ → KBr + Al₂(SO₄)₃

2AlBr₃ + 3K₂SO₄ → 6KBr + Al₂(SO₄)₃

CuFeS₂ + O₂ → Cu + FeO + SO₂

2CuFeS₂ + 5O₂ → 2Cu + 2FeO + 4SO₂

C₂H₂N₂O₄ + O₂ → CO₂ + H₂O + N₂

2C₂H₂N₂O₄ + O₂ → 4CO₂ + 2H₂O + 2N₂

C₂₁H₃₀O₂ + O₂ → CO₂ + H₂O

2C₂₁H₃₀O₂ + 55O₂ → 42CO₂ + 30H₂O

C₃H₈O + F₂ → CF₄ + HF + O₂

2C₃H₈O + 20F₂ → 6CF₄ + 16HF + O₂

C₄H₁₀ + O₂ → CO₂ + H₂O

2C₄H₁₀ + 13O₂ → 8CO₂ + 10H₂O

C₆H₆ + O₂ → CO₂ + H₂O

2C₆H₆ + 9O₂ → 12CO₂ + 6H₂O

C₇H₅N₃O₆ → N₂ + H₂O + CO + C

2C₇H₅N₃O₆ → 3N₂ + 5H₂O + 7CO + 7C

C₈H₁₈ + O₂ → CO₂ + H₂O

2C₈H₁₈ + 25O₂ → 16CO₂ + 18H₂O

Fe₂O₃ + C → Fe + CO₂

2Fe₂O₃ + 3C → 4Fe + 3CO₂

what is the half equation for the reduction of hydrogen

2H+ + 2e‐ ----> H²

HCN + CuSO₄ → H₂SO₄ + Cu(CN)₂

2HCN + CuSO₄ → H₂SO₄ + Cu(CN)₂

HCl + CaCO₃ → CaCl₂ + H₂O + CO₂

2HCl + CaCO₃ → CaCl₂ + H₂O + CO₂

H₂ + O₂ → H₂O

2H₂ + O₂ → 2H₂O

H₂O + O₂ → H₂O₂

2H₂O + O₂ → 2H₂O₂

H₂S + SO₂ → S + H₂O

2H₂S + SO₂ → 3S + 2H₂O

K + Cl₂ →KCl

2K + Cl₂ →2KCl

KClO → KCl + O₂

2KClO → 2KCl + O₂

KClO₃ → KCl + O₂

2KClO₃ → 2KCl + 3O₂

LiHCO₃ + H₂SO₄ → Li₂SO₄ + H₂O + CO₂

2LiHCO₃ + H₂SO₄ → Li₂SO₄ + 2H₂O + 2CO₂

NH₃ + CuO → Cu + N₂ + H₂O

2NH₃ + 3CuO → 3Cu + N₂ + 3H₂O

NH₃ + H₂SO₄ → (NH₄)₂SO₄

2NH₃ + H₂SO₄ → (NH₄)₂SO₄

Na + H₂O → NaOH + H₂

2Na + 2H₂O → 2NaOH + H₂

NaBr + CaF₂ → NaF + CaBr₂

2NaBr + CaF₂ → 2NaF + CaBr₂

NaBr + Cl₂ → Br₂ + NaCl

2NaBr + Cl₂ → Br₂ + 2NaCl

NaCl + F₂ → NaF + Cl₂

2NaCl + F₂ → 2NaF + Cl₂

NaF + Br₂ → NaBr + F₂

2NaF + Br₂ → 2NaBr + F₂

NaHCO₃ + H₂SO₄ → CO₂ + Na₂SO₄ + H₂O

2NaHCO₃ + H₂SO₄ → 2CO₂ + Na₂SO₄ + 2H₂O

NaHCO₃ → Na₂CO₃ + CO₂ + H₂O

2NaHCO₃ → Na₂CO₃ + CO₂ + H₂O

NaNO₃ + PbO → Pb(NO₃)₂ + Na₂O

2NaNO₃ + PbO → Pb(NO₃)₂ + Na₂O

RbNO₃ + BeF₂ → Be(NO₃)₂ + RbF

2RbNO₃ + BeF₂ → Be(NO₃)₂ + 2RbF

The information below describes a redox reaction. Ag+(aq)+Al(s)--->Ag(s)+Al3+(aq) Ag+(aq)+e---->Ag(s) Al(s)-->Al3+(aq)+3e- What is the coefficient of silver in the final, balanced equation for this reaction?

Mg + N₂ → Mg₃N₂

3 Mg + 1 N₂ → 1 Mg₃N₂

O₂ → O₃

3 O₂ → 2 O₃

Aluminum's oxidation number

__Mg + __AlCl₃ --> __MgCl₂ +__Al

3, 2, 3, 2

AgNO₃ + FeCl₃ → Fe(NO₃)₃ + AgCl

3AgNO₃ + FeCl₃ → Fe(NO₃)₃ + 3AgCl

Cu + HNO₃ → Cu(NO₃)₂ + NO + H₂O

3Cu + 8HNO₃ → 3Cu(NO₃)₂ + 2NO + 4H₂O

Fe₂O₃ + CO → Fe₃O₄ + CO₂

3Fe₂O₃ + CO → 2Fe₃O₄ + CO₂

Hg(OH)₂ + H₃PO₄ → Hg₃(PO₄)₂ + H₂O

3Hg(OH)₂ + 2H₃PO₄ → Hg₃(PO₄)₂ + 6H₂O

H₂SO₄ + B(OH)₃ → B₂(SO₄)₃ + H₂O

3H₂SO₄ + 2B(OH)₃ → B₂(SO₄)₃ + 6H₂O

MgO + H₃PO₄ → Mg₃(PO₄)₂ + H₂O

3MgO + 2H₃PO₄ → Mg₃(PO₄)₂ + 3H₂O

NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + H₂O

3NH₄OH + H₃PO₄ → (NH₄)₃PO₄ + 3H₂O

__Al + __O₂ --> __Al₂O₃

4, 3, 2

__Fe +__O₂ --> __Fe₂O₃

4, 3, 2

Al + O₂ → Al₂O₃

4Al + 3O₂ → 2Al₂O₃

Al₂O₃ + Fe → Fe₃O₄ + Al

4Al₂O₃ + 9Fe → 3Fe₃O₄ + 8Al

Fe + O₂ →Fe₂O₃

4Fe + 3O₂ →2Fe₂O₃

what is the oxidation half equation for oxygen forming from hydroxide ions

4OH‐ ---> O² + 2H²O + 4e‐

P + O₂ → P₂O₅

4P + 5O₂ → 2P₂O₅

how long does it take tweezed hair to regrow

5-6 weeks

CO + I₂O₅ → CO₂ + I₂

5CO + I₂O₅ → 5CO₂ + I₂

virgin growth is hair that has not been touched in

6-8 months

AgI + Fe₂(CO₃)₃ → FeI₃ + Ag₂CO₃

6AgI + Fe₂(CO₃)₃ → 2FeI₃ + 3Ag₂CO₃

K + B₂O₃ → K₂O + B

6K + B₂O₃ → 3K₂O + 2B

A neutral solution has a pOH of

Acidic solutions have a pH lower than

Neutral solutions have a pH of

Actinium (Ac)

angle of inclination, hair doesnt exist at

90 or 0 degrees

55. The equilibrium constant for the reaction represented by the equation below is greater than 1.0. Which of the following gives the correct relative strengths of the acids and bases in the reaction? H2PO4− + HBO32− ⇄ HPO42− + H2BO3− Acids Bases A.H2PO4− > H2BO3− and HBO32− > HPO42− B.H2BO3− > H2PO4− and HBO32¯ > HPO42− C.H2PO4− > H2BO3− and HPO42− > HBO32− D.H2BO3− > H2PO4− and HPO42− > HBO32− E.H2PO4− = H2BO3− and HPO42− = HBO32−

A solution of calcium hypochlorite, a common additive to swimming-pool water, is... (A) basic because of the hydrolysis of the OCl− ion (B) basic because Ca(OH)2 is a weak and insoluble base (C) neutral if the concentration is kept below 0.1 molar (D) acidic because of the hydrolysis of the Ca2+ ions (E) acidic because the acid HOCl is formed

HC2H3O2(aq) + CN− (aq) ⇄ HCN(aq) + C2H3O2− (aq) The reaction represented above has an equilibrium constant equal to 3.7 x 104. Which of the following can be concluded from this information? (A) CN− (aq) is a stronger base than C2H3O2− (aq) (B) HCN(aq) is a stronger acid than HC2H3O2(aq) (C) The conjugate base of CN− (aq) is C2H3O2− (aq) (D) The equilibrium constant will increase with an increase in temperature. (E) The pH of a solution containing equimolar amounts of CN− (aq) and HC2H3O2 (aq) is 7.0

The net ionic equation for the reaction between silver carbonate and hydrochloric acid is... (A) Ag2CO3(s) + 2 H+ + 2 Cl− 2 AgCl(s) + H2O + CO2 (g) (B) 2 Ag+ + CO32− + 2 H+ + 2 Cl− 2 AgCl(s) + H2O + CO2(g) (C) CO32− + 2 H+ H2O + CO2(g) (D) Ag+ + Cl¯ AgCl(s) (E) Ag2CO3(s) + 2 H+ 2Ag+ + H2CO3

Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 8. A solution prepared to be initially 1 M in NaCl and 1 M in HCl.

What part of the curve corresponds to the optimum buffer action for the acetic acid/acetate pair? (A) Point V (B) Point X (C) Point Z (D) Along all of section WY (E) along all of section YZ

Alkali

A base that dissolves in water to form a solution with a pH greater than 7

Brine is electrolysed in...

A diaphragm cell.

Define a conductor?

A material that allows heat and electricity to pass through it.

Define an insulator?

A material that does not allow heat or electrons to move through it easily.

what is an electrolyte

A molten or dissolved ionic compound that conducts electricity

An anion is ..........

A negatively charged ion

A cation is ........

A positively charged ion

In an ecosystem that uses photosynthesis, O2 release is considered what?

A waste product

Why does the breakdown of glucose not turn into ATP

ADP and phosphate is in the cell. When we break apart the glucose, the energy that is released is used to fuel the reaction of taking ADP and attaching the phosphate back to it. This is why we say it regenerates Breaking down of glucose down not turn into ATP. IT is the energy of breaking down glucose that fuels the reaction that turns ADP back into ATP.

What is ADP? what is the Pi in the ADP+Pi

ADP is adenosine diphosphate. Pi is inorganic phosphate

C2H3O2 (-1 charge)

Acetate

Can be strong or weak electrolytes in aqueous solution

Acid

React with metals to produce hydrogen gas

Acid

Tastes sour

Acid

Used as preservative (foods)

Acid

Used in fragrances and flavors

Acid

Ka is what constant? _____ ___________

Acid dissociation

What is ATP?

Adenosine triphosphate It has 3 phosphate molecule

How to insert needle

Always insert needle on the underside of the hair, parallel to the hair, under the hair, size of the hair=size of needle. Never parallel or perpendicular

what is the half equation for the reaction at the negative electrode during the electrolysis of bauxite

Al³+ + 3e- ---> Al

Al₂(SO₃)₃ + NaOH → Na₂SO₃ + Al(OH)₃

Al₂(SO₃)₃ + 6NaOH → 3Na₂SO₃ + 2Al(OH)₃

Al₄C₃ + H₂O → CH₄ + Al(OH)₃

Al₄C₃ + 12H₂O → 3CH₄ + 4Al(OH)₃

NH4 (+1 charge)

Ammonium

what is an aqueous solution

An aqueous solution is a solution in which the solvent is water.

what happens during electrolysis

An electric current is passed through an electrolyte which causes the ions to move towards the electrodes where they react and the ions get discharged

What is electroplating?

An electrolytic process in which metal ions are reduced and the metal atoms are deposited on a surface

NAD+ wants to accept electrons, right now it's acting as

An electron acceptor. This means its in a state of oxidize.. When NAD picks up hydrogens and electrons, it becomes reduced..

Salt

An ionic compound made from the neutralization of an acid with a base.

acid

Any substance that forms an aqueous solution with a pH less than 7

Rule 6 for oxidation number

Atoms in a polyatomic ion is the sum of the oxidisation numbers

54. Which of the following is the correct equilibrium expression for the hydrolysis of CO32− ? (A) K = [HCO3− ] / ( [CO32− ] [H3O+] ) (B) K = ( [HCO3−] [OH−] ) / [CO32−] (C) K = ( [CO32− ] [OH−] ) / [HCO3−] (D) K = [CO32− ] / ( [CO2] [OH−]2 ) (E) K = ( [CO32− ] [H3O+] ) / [HCO3−]

8. Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 10. A solution prepared to be initially 0.5 M in CH3COOH and 1 M in CH3COONa

A molecule or an ion is classified as a Lewis acid if it... (A) accepts a proton from water (B) accepts a pair of electrons to form a bond (C) donates a pair of electrons to form a bond (D) donates a proton to water (E) has resonance Lewis electron-dot structures

A pure white crystalline solid dissolves in water to yield a basic solution that liberates a gas when excess acid is added to it. On the basis of this information, the solid could be... (A) KNO3 (B) K2CO3 (C) KOH (D) KHSO4 (E) KCl

At 25°C, aqueous solutions with a pH of 8 have a hydroxide ion concentration, [OH−], of... (A) 1 × 10−14 M (B) 1 × 10−8 M (C) 1 × 10−6 M (D) 1M (E) 8M

Commercial vinegar was titrated with NaOH solution to determine the content of acetic acid, HC2H3O2. For 20.0 milliliters of the vinegar, 32.0 milliliters of 0.500-molar NaOH solution was required. What was the concentration of acetic acid in the vinegar if no other acid was present? (A) 1.60 M (B) 0.800 M (C) 0.640 M (D) 0.600 M (E) 0.400 M

Equal volumes of 0.10-molar H3PO4 and 0.20-molar KOH are mixed. After equilibrium is established, the type of ion a solution in largest concentration, other than the K+ ion, is... (A) H2PO4− (B) HPO42− (C) PO43− (D) OH− (E) H3O+

Mixtures that would be considered buffers include which of the following? I. 0.10 M HCl + 0.10 M NaCl II. 0.10 M HF + 0.10 M NaF III. 0.10 M HBr + 0.10 M NaBr (A) I only (B) II only (C) III only (D) I and II (E) II and III

When dilute nitric acid was added to a solution of one of the following chemicals, a gas was evolved, This gas turned a drop of limewater, Ca(OH)2, cloudy, due to the formation of a white precipitate. The chemical was... (A) household ammonia, NH3 (B) baking soda, NaHCO3 (C) table salt, NaCl (D) epsom salts, MgSO4 . 7H2O (E) bleach, 5% NaOCl

When phenolphthalein is used as the indicator in a titration of an HCl solution with a solution of NaOH, the indicator undergoes a color change from clear to red at the end point of the titration. This color change occurs abruptly because... (A) phenolphthalein is a very strong acid that is capable of rapid dissociation (B) the solution being titrated undergoes a large pH change near the end point of the titration (C) phenolphthalein undergoes an irreversible reaction in basic solution (D) OH− acts as a catalyst for the decomposition of phenolphthalein (E) phenolphthalein is involved in the rate-determining step of the reaction between H3O+ and OH−

Which of these is not crucial to human blood? (A) Ammonium ion-ammonia, (B) ethanoic acid-ethanoate ion, (C) Dihydrogen phosphate-monohydrogen phosphate

Which, if any, of the following species is in the greatest concentration in a 0.100-molar solution of H2SO4 in water? (A) H2SO4 molecules (B) H3O+ ions (C) HSO4− ions (D) SO42− ions (E) All species are in equilibrium and therefore have the same concentrations.

Why does cellular respiration not oxidize glucose in a single step?

B/c there is a Stepwise Energy Harvest via NAD+ and the Electron Transport Chain -- it requires a metabolic pathway. it must be harvested slowly and in steps, not all at once

BaS + PtF₂ → BaF₂ + PtS

According to Bronsted-Lowry, is ammonia a base or acid?

Base

Cleaning agents, antacids

Base

Example: milk of magnesia

Base

React with acids

Base

Used as antacids (neutralization reaction)

Base

Used in chemical reactions (making polymers, drugs, etc)

Base

Used in making soaps, detergents, etc

Base

Why would the electrons be attracted to the oxygen?

Because Oxygen is highly electronegative .. it's pulling the electrons down the electron chain

What is respiration?

Biological organisms burn fuel sources inside their cells in order to release energy to do the work of running the biochemical reactions that keep them alive The basic oxidation reaction is : C6H12O6 + 6O2-> 6CO2 + 6H2O

Changes the color of an acid-base indicator (acid, base, or both)

Both

Who defines a base as a hydrogen-ion acceptor

Bronsted-Lowry

Who defines an acid as a hydrogen-ion donor

Bronsted-Lowry

2 NH3 ⇄ NH4+ + NH2− In liquid ammonia, the reaction represented above occurs. In the reaction NH4+ acts as... (A) a catalyst (B) both an acid and a base (C) the conjugate acid of NH3 (D) the reducing agent (E) the oxidizing agent

Correct procedures for a titration include which of the following? I. Draining a pipet by touching the tip to the side of the container used for the titration II. Rinsing the buret with distilled water just before filling it with the liquid to be titrated III. Swirling the solution frequently during the titration (A) I only (B) II only (C) I and III only (D) II and III only (E) I, II, and III

How can 100. mL of sodium hydroxide solution with a pH of 13.00 be converted to a sodium hydroxide solution with a pH of 12.00? (A) By diluting the solution with distilled water to a total volume of 108 mL (B) By diluting the solution with distilled water to a total volume of 200 mL (C) By diluting the solution with distilled water to a total volume of 1.00 L (D) By adding 100. mL of 0.10 M HCl (E) By adding 100. mL of 0.10 M NaOH

In the titration of a weak acid of unknown concentration with a standard solution of a strong base, a pH meter was used to follow the progress of the titration. Which of the following is true for this experiment? (A) The pH is 7 at the equivalence point. (B) The pH at the equivalence point depends on the indicator used. (C) The graph of pH versus volume of base added rises gradually at first and then much more rapidly. (D) The graph of pH versus volume of base added shows no sharp rise. (E) The [H+] at the equivalence point equals the ionization constant of the acid.

To determine the molar mass of a solid monoprotic acid, a student titrated a weighed sample of the acid with standardized aqueous NaOH. Which of the following could explain why the student obtained a molar mass that was too large? I. Failure to rinse all acid from the weighing paper into the titration vessel II. Addition of more water than was needed to dissolve the acid III. Addition of some base beyond the equivalence point (A) I only (B) III only (C) I and II only (D) II and III only (E) I, II, and III

What volume of 0.150-molar HCl is required to neutralize 25.0 milliliters of 0.120-molar Ba(OH)2? (A) 20.0 mL (B) 30 0 mL (C) 40.0 mL (D) 60.0 mL (E) 80.0 mL

cellular respiration with the oxidation of sugar glucose:

C6H12O6 + 6O2 --> 6CO2 + 6H2O + Energy (ATP + heat) sugar glucose + oxygen --> break down to carbon dioxide + water + Energy such as ATP + heat is produce Another explanation: When glucose is oxidized, carbon dioxide, water and energy are produced. The food that is consumed by most organisms is basically glucose. The other carbohydrates consumed are ultimately reduced to glucose during digestion. Glucose acts as a fuel and a source of energy for the organism's activities. The energy in glucose is released during respiration. During respiration, the oxygen taken in is used to oxidise glucose. The glucose molecule is broken down to produce carbon dioxide and water. This process releases a lot of energy. This energy is used in formation of ATP molecules. These ATP molecules thus become storehouses of energy. The numbers in the equation represent the proportions in which the ingredients react and the proportion in which the products are formed. It is clear that, to oxidize every molecule of glucose, you need 6 molecules of oxygen. After the process is complete, you are left with 6 moles of CO2 and 6 moles of water along with some energy.

cellular respiration vs. photosynthesis

C6H12O6 + 6O2 --> 6CO2 + 6H2O + Energy (ATP + heat) vs. 6CO2 + 6H2O + light energy ---> C6H12O6 + 6O2

CF₄ + Br₂ → CBr₄ + F₂

CF₄ + 2Br₂ → CBr₄ + 2F₂

example of weak acidic compounds ionising

CH₃COOH ⇌ CH₃COO- + H+

CH₄ + O₂ → CO₂ + H₂O

CH₄ + 2O₂ → CO₂ + 2H₂O

CO₂ → C + O₂

Ca + H₂O → Ca(OH)₂ + H₂

Ca + 2H₂O → Ca(OH)₂ + H₂

Ca(NO₃)₂ + Na₂CO₃ → CaCO₃ + NaNO₃

Ca(NO₃)₂ + Na₂CO₃ → CaCO₃ + 2NaNO₃

Formula for Calcium hydroxide

Ca(OH)₂

Ca(OH)₂ + HCl → CaCl₂ + H₂O

Ca(OH)₂ + 2HCl → CaCl₂ + 2H₂O

CaCO₃ + HNO₃ → Ca(NO₃)₂ + H₂O + CO₂

CaCO₃ + 2HNO₃ → Ca(NO₃)₂ + H₂O + CO₂

2 factors of acne

Can blood supply perform any rehealing, or will pathogenic bacteria spread

CO3 (-2 charge)

Carbonate

Electric current

Causes a chemical reaction that breaks down the ionic compound.

Ca₃(PO₄)₂ + H₂SO₄ → CaSO₄ + Ca(H₂PO₄)₂

Ca₃(PO₄)₂ + 2 H₂SO₄ → 2 CaSO₄ + Ca(H₂PO₄)₂

Ca₃(PO₄)₂ + SiO₂ + C → CaSiO₃ + CO + P

Ca₃(PO₄)₂ + 3SiO₂ + 5C → 3CaSiO₃ + 5CO + 2P

FSH

Changed testosterone to estrogen

Changes testosterone to progesterone

What is the redox reaction, aka Oxidation and Reduction reaction?

Chemical reactions that transfer electrons between reactants The transfer of electrons during chemical reactions releases energy stored in organic molecules

ClO3 (-1 charge)

Chlorate

The conjugate base of the acid HCl (what ion?)

Chloride ion

Electrolysis of brine produces...

Chlorine, hydrogen, sodium hydroxide.

ClO2 (-1 charge)

Chlorite

CrO4 (-2 charge)

Chromate

Cr (+3 charge)

Chromium (III)

Conjugate base of HCl (formula)

Cl-

Co (+3 charge)

Cobalt (III)

Archard-theirs syndrome

Combination of cushings and virilism disease. Woman who have beards

Brine

Concentrated aqueous solution of sodium chloride, obtained from seams of rock salt underground.

what is brine

Concentrated sodium chloride solution

Difference between strength of an acid and concentration

Concentration = the measure of how much acid there is in a litre (1dm3) of water Strength = the proportion of the acid molecules ionised in water

Vocabulary: The particle formed when a base gains a hydrogen ion

Conjugate acid

Consists of two substances related by the loss or gain of a single hydrogen ion.

Conjugate acid-base pair

The particle that remains when an acid has donated a hydrogen ion

Conjugate base

Cu (+1 charge)

Copper (I) Cuprous

Cu (+2 charge)

Copper (II) Cupric

Consider the half reaction below. Cu2+(aq)+2e--->Cu(s) Which statement best describes what is taking place?

Copper is being reduced.

How does iron corrode?

Corrodes by being oxidized to ions of iron by oxygen.

Which half-reaction correctly describes an oxidation?

Cr(s)-->Cr3+(aq)+3e-

Why is a mixture of aluminium oxide and cryolite used, rather than aluminium oxide alone?

Cryolite lowers the melting point and reduces some of the energy costs involved in extracting aluminium oxide.

Cr₂(SO₄)₃ + NaOH → Cr(OH)₃ + Na₂SO₄

Cr₂(SO₄)₃ + 6NaOH → 2Cr(OH)₃ + 3Na₂SO₄

C₂H₄O₂ + O₂ → CO₂ + H₂O

C₂H₄O₂ + 2O₂ → 2CO₂ + 2H₂O

C₆H₁₂O₆ + O₂ → CO₂ + H₂O

C₆H₁₂O₆ + 6O₂ → 6CO₂ + 6H₂O

C₆H₆ → C + H₂

C₆H₆ → 6C + 3H₂

C₉H₂₀ + O₂ → CO₂ + H₂O

C₉H₂₀ + 14O₂ → 9CO₂ + 10H₂O

49. Each of the following can act as both a Brönsted acid and a Brönsted base EXCEPT... (A) HCO3− (B) H2PO4− (C) NH4+ (D) H2O (E) HS−

Acid Acid Dissociation Constant, Ka H3PO4 7 x 10−3 H2PO4− 8 x 10−8 HPO42− 5 x 10−13 On the basis of the information above, a buffer with a pH = 9 can best be made by using... (A) pure NaH2PO4 (B) H3PO4 + H2PO4− (C) H2PO4− + PO43− (D) H2PO4− + HPO42− (E) HPO42− + PO43−

The graph below shows the titration curve that results when 100. mL of 0.0250 M acetic acid is titrated with 0.100 M NaOH. Which of the following indicators is the best choice for this titration? pH Range of Color Change (A) Methyl orange 3.2 - 4.4 (B) Methyl red 4.8 - 6.0 (C) Bromthymol blue 6.1 - 7.6 (D) Phenolphthalein 8.2 - 10.0

The pH of 0.1-molar ammonia is approximately... (A) 1 (B) 4 (C) 7 (D) 11 (E) 14

The safest and most effective emergency procedure to treat an acid splash on skin is to do which of the following immediately? (A) Dry the affected area with paper towels (B) Sprinkle the affected area with powdered Na2SO4(s) (C) Flush the affected area with water and then with a dilute NaOH solution (D) Flush the affected area with water and then with a dilute NaHCO3 solution (E) Flush the affected area with water and then with a dilute vinegar solution

Use these answers for questions 8 - 10. (A) a solution with a pH less than 7 that is not a buffer solution (B) a buffer solution with a pH between 4 and 7 (C) a buffer solution with a pH between 7 and 10 (D) a solution with a pH greater than 7 that is not a buffer solution (E) a solution with a pH of 7 Ionization Constants CH3COOH = 1.8 x 10−5 NH3 = 1.8 x 10−5 H2CO3; K1 = 4 x 10−7 H2CO3; K2 = 4 x 10−11 9. A solution prepared to be initially 1 M in Na2CO3 and 1 M in CH3COONa

What is the H+(aq) concentration in 0.05 M HCN(aq) ? (The Ka for HCN is 5.0 x 10−10) (A) 2.5 x 10−11 (B) 2.5 x 10−10 (C) 5.0 x 10−10 (D) 5.0 x 10−6 (E) 5.0 x 10−4

What is the pH of a 1.0 x 10−2-molar solution of HCN? (Ka = 4.0 x 10 −10 ) (A) 10 (B) Between 7 and 10 (C) 7 (D) Between 4 and 7 (E) 4

Insulin

Decreases sugar in the blood

Cr2O7 (-2 charge)

Dichromate

Drugs that caused hair growth

Dilatin, loestrin, minoxidil, prednisone, Premarin

Reducing agent

Donates electrons and becomes oxidized.

What happens when an electron continuously gets passed between oxidation agents and reducing agents?

During each pass, it will lose energy. Eventually, the electrons will have no energy/use left

. Which of the following ions is the strongest Lewis acid? (A) Na+ (B) Cl− (C) CH3COO− (D) Mg2+ (E) Al3+

22. HSO4− + H2O ⇄ H3O+ + SO42− In the equilibrium represented above, the species that act as bases include which of the following? I. HSO4− II. H2O III. SO42− (A) II only (B) III only (C) I and II (D) I and III (E) II and III

As the number of oxygen atoms increases in any series of oxygen acids, such as HXO, HXO2, HXO3, ...., which of the following is generally true? (A) The acid strength varies unpredictably. (B) The acid strength decreases only if X is a nonmetal. (C) The acid strength decreases only if X is a metal. (D) The acid strength decreases whether X is a nonmetal or a metal. (E) The acid strength increases.

Ascorbic acid H2C6H6O6(s), is a diprotic acid with K1 = 7.9 × 10−5 and K2 = 1.6 × 10−12. In a 0.005 M aqueous solution of ascorbic acid, which of the following species is present in the lowest concentration? (A) H2O(l) (B) H3O+(aq) (C) H2C6H6O6(aq) (D) HC6H6O6−(aq) (E) C6H6O62−(aq)

If the acid dissociation constant, Ka, for an acid HA is 8 x 10−4 at 25 °C, what percent of the acid is dissociated in a 0.50-molar solution of HA at 25 °C? (A) 0.08% (B) 0.2% (C) 1% (D) 2% (E) 4%

The net ionic equation for the reaction that occurs during the titration of nitrous acid with sodium hydroxide is... (A) HNO2 + Na+ + OH− NaNO2 + H2O (B) HNO2 + NaOH Na+ + NO2− + H2O (C) H+ + OH− H2O (D) HNO2 + H2O NO2− + H3O+ (E) HNO2 + OH− NO2− + H2O

Which of the following acids can be oxidized to form a stronger acid? (A) H3PO4 (B) HNO3 (C) H2CO3 (D) H3BO3 (E) H2SO3

Which of the following reactions does NOT proceed significantly to the right in aqueous solutions? (A) H3O+ + OH− 2 H2O (B) HCN + OH− H2O + CN− (C) Cu(H2O)42+ + 4 NH3 Cu(NH3)42+ + 4H2O (D) H2SO4 + H2O H3O+ + HSO4− (E) H2O + HSO4− H2SO4 + OH−

Cushing syndrome

Enlarged face, muscle weakness. is caused from *to much cortisol

Oxidation of number of a monatomic ion is...?

Equal to the charge of the ion

The sum of the individual oxidation numbers of all atoms in the formula for a polyatomic ion is...?

Equal to the charge of the ion

During cellular respiration, the fuel (such as glucose) is oxidized and oxygen is reduced:

Every time we pull off a hydrogen, the sugar glucose becomes oxidize ..

Pre treatment and post Electrolysis

FDA 70% alcohol, minimum 30% alcohol= antiseptic

True or False Not all oxidation reactions are accompanied by reduction reactions

False

True or False: All compounds that contain hydrogen are acids

False

True or False The presence of salts and acids halts the process of corrosion.

False, the presence of salts and acids speed of the process of corrosion.

True or False The oxidation numbers of elements in a compound are not written per atom.

False, they are written per atom.

FeCl₃ + NaOH → Fe(OH)₃ + NaCl

FeCl₃ + 3NaOH → Fe(OH)₃ + 3NaCl

Fe₂(C₂O₄)₃ → FeC₂O₄ + CO₂

Fe₂(C₂O₄)₃ → 2 FeC₂O₄ + 2 CO₂

Fe₂O₃ + H₂ → Fe + H₂O

Fe₂O₃ + 3H₂ → 2Fe + 3H₂O

Fe₂O₃ + H₂O → Fe(OH)₃

Fe₂O₃ + 3H₂O → 2Fe(OH)₃

The process of photosynthesis

First you would need energy. Not ATP but energy from the sun..Then it needs water and C02 to release oxygen and make some glucose or other organic molecules 6CO2 + 6H2O + light energy >>> C6H12O6 + 6O2

Positive ions

Form at the cathode.

Diabetes symptoms

Frequent thirst; polydipsia, fragile blood vessels=bruising, HBP, cardio problems, obesity, neuropathy

GaF₃ + Cs → CsF + Ga

GaF₃ + 3Cs → 3CsF + Ga

Define reduction?

Gain of electrons

Glycogen is broken into?

Glucose

what happens at the cathode during the electrolysis of a solution

H+ ions and metal ions are present - hydrogen gas will be produced if the metal is more reactive than hydrogen, a layer of pure metal will be produced if the metal is less reactive than hydrogen

Oxygen -1

H2O2

Conjugate acid of HSO₄⁻

H2SO4

Sulfuric Acid

H2SO4 (Strong Acid)

what virus in the Heps family can survive in dry blood for 7 days

HBV

Gastric acid is also known as

HCl

Example of monoprotic acids (formula)

HNO3

HNO₃ + NaHCO₃ → NaNO₃ + H₂O + CO₂

Conjugate base of H₂SO₄

HSO₄⁻

HAV

Hepatitis A: most innocent of heps family

HSO3 (-1 charge)

Hydrogen Sulfite

OH (-1 charge)

Hydroxide

ClO (-1 charge)

Hypochlorite

Conjugate acid of OH-

H₂O

H₂SO₃ → H₂O + SO₂

Example of diprotic acid (formula)

H₂SO₄

H₂SO₄ + NaNO₂ → HNO₂ + Na₂SO₄

H₂SO₄ + 2NaNO₂ → 2HNO₂ + Na₂SO₄

example of strong acidic compounds ionising

H₂SO₄ ---> 2H+ (aq) + SO₄2- - sulfuric acid --> hydrogen + sulphate

Example of triprotic acids (formula)

H₃PO₄

H₃PO₄ + KOH → K₃PO₄ + H₂O

H₃PO₄ + 3KOH → K₃PO₄ + 3H₂O

Why do we have to do the tumble and go through the ETC? Why don't we want to do a combustion reaction (explosive reaction) or do everything in one giant step?

If we did one giant step, we would release all of the heat/light energy at once. That would cause us to explode.

Explain why oxidation cannot occur without reduction, and vice versa.

In a redox reaction one element has a complete or partial loss of electrons (oxidation) therefore another element must have a complete or partial gain of electrons (reduction).

Diabetes type 1

Insulin dependent, childhood onset, not producing enough insulin

Half-equations

Ionic equations that only show what is happening at only one of the electrodes.

Why do ionic compounds only conduct when molten or aqueous?

Ions are fixed when ionic compounds are solid, meaning they can't move so can't conduct electricity. When the compounds are molten or in aqueous solution, the ions (that are electrically charged) are able to move and carry charge.

Fe (+2 charge)

Iron (II) Ferrous

Fe (+3 charge)

Iron (III) Ferric

Consider the half reaction below. Fe--->Fe2+ +2e- Which statement best describes what is taking place in this half reaction?

Iron is being oxidized.

Hydrogen

Is +1 except in hydrides where it is -1

Oxygen

Is -2 except in peroxdes where it is -1

How does temperature affect an enzyme?

It affects the shape and rate at which an enzyme will react

What happens when ATP release energy/loses its 3 phosphate group?

It becomes ADP ATP + H2O--> ADP + Pi ATP goes through hydrolysis by breaking bonds using water.. it turns to ADP. ADP is adenosine diphosphate. Pi is inorganic phosphate

Which statement is true of the following reaction? H2+O2-->2H+ +O2-

It is not balanced for charge or for number of atoms.

What is the final electron acceptor?

It is oxygen. Oxygen's only role is to be the final acceptor of electrons that is being passed by NADH

Oxidation number of nitrogen is 0 in

Its free state of N2

K + MgBr → KBr + Mg

potassium dichromate

K2Cr2O7. A strong oxidizing agent.

Formula for potassium hydroxide

KOH

Acid dissociation constant

Base dissociation constant

Give 2 uses for chlorine

Kills harmful bacteria in swimming pools To sterelise the domestic water supply To manafacture PVC

The ion-product constant for water

Pb (+2 charge)

Lead (II)

Pb (+4 charge)

Lead (IV)

To which electrodes do the lead and bromide ions go during the electrolysis of PbBr2

Lead is positively charged and moves to the negative electrode (cathode). Bromine is negatively charged and move to the positive electrode (anode).

Hypopigmentation

Less melanocytes = white

Who proposed an base donates a pair of electrons during a reaction?

Lewis

Who proposed that an acid accepts a pair of electrons during a reaction?

Lewis

Overview:

Living cells require energy from outside sources •Some animals, such as the giant panda, obtain energy by eating plants; others feed on organisms that eat plants •Energy flows into an ecosystem as sunlight and leaves as heat •Photosynthesis generates oxygen and organic molecules, which are used in cellular respiration •Cells use chemical energy stored in organic molecules to regenerate ATP, which powers work

Define oxidation?

Loss of electrons

Dilute acid

Lots of water, small amount of acid

Hg2 (+2 charge)

Mercury (I) Mercurous

Hg (+2 charge)

Mercury (II) Mercuric

Formula for Magnesium hydroxide

Mg(OH)₂

Magnesium Oxide Oxidation Number

Mg:+2,O:-2

MgF₂ + Li₂CO₃ → MgCO₃ + LiF

MgF₂ + Li₂CO₃ → MgCO₃ + 2LiF

Mg₃N₂ + H₂O → NH₃ + Mg(OH)₂

Mg₃N₂ + 6H₂O → 2NH₃ + 3Mg(OH)₂

Mn(NO₂)₂ + BeCl₂ → Be(NO₂)₂ + MnCl₂

calculating moles (1)

Moles = mass/Mr

Acids that contain one ionizable hydrogen

Monoprotic

Hyper-pigmentation

More active melanocytes= brown

Addison's disease

Muscle weakness, low bp, hyperpigment on face and arms, *not enough cortisol

The role of NAD in cellular respiration

NAD is a co-enzyme.. this means its going to be continuously reused and help carry out another reaction in cellular respiration NAD is going to carry electrons from the glucose molecule to use them in a different type of reaction

When NAD accepts electron and changes from an oxidize to reduce state, it beomes

NADH

What is NADH?

NADH is NAD's reduced form because it is now carrying the hydrogens and electrons

An electron transport chain...

NADH passes the electrons to the electron transport chain. Electron transport chain passes electrons in a series of steps.. Each time the electrons get transferred it is LOOSING energy.

Reversible reaction - alkaline

NH3 + H2O ⇌ NH4+ + OH-

Conjugate base of NH₄⁺

NH₃

NH₄NO₃ → N₂O + H₂O

NH₄NO₃ → N₂O + 2H₂O

Sodium chloride oxidation number

Na:+1,Cl=-1

examples of alkaline compounds ionising

NaOH(aq) --> Na+(aq) + OH-

Na₃PO₄ + KOH → NaOH + K₃PO₄

Na₃PO₄ + 3KOH → 3NaOH + K₃PO₄

The cathode is the .......

Negative electrode

Cathode

Negative electrode.

Anions

Negative ions.

What is NAD called?

Nicotinamide

NO3 (-1 charge)

Nitrate

NO2 (-1 charge)

Nitrite

When we harvest energy out of a molecule, are we using all of the molecule's energy?

No, because we are very inefficient at it. We do not use all of the energy to make ATP, we release some in the form of heat

Are double-replacement reactions redox reactions?

No, never.

Does ADP have a high energy bond?

No. It was broken off and used during its transformation of ATP to ADP.

Diabetes type 2

Non insulin dependent, adulthood, *insulin resistant patients

N₂ + H₂ → NH₃

N₂ + 3H₂ → 2NH₃

Acronym that helps us understand redox reaction...

O.I.L.R.I.G Oil - oxidation I loose [electrons, or other elements caring electrons] Rig - reduction I gain [electrons, or other elements carrying electrons]

Conjugate base of H₂O

OH-

Acidified potassium dichromate colour change

Orange to green

PCOS = Polycystic ovarian syndrome

Ovaries contain cysts

Oxidation or Reduction Shift of electrons away from an atom in a covalent bond (Increase in oxidation number)

Oxidation

Loss of electrons from an atom or ion Gain of oxygen Example?

Oxidation Burning

OIL

Oxidation is loss of electrons

OILRIG

Oxidation is loss, Reduction is gain.

Rule 2 for oxidation number

Oxidation number of elements that exist as simple ions in ionic compounds is the same as the charge on the ion

Does oxidation occur at the anode or cathode?

Oxidation occurs at the anode. Oxidation is the loss of electrons.

Rule 1 for oxidation numbers

Oxidation state of atoms of an element in its free state is zero

What is oxygen's role?

Oxygen pulls electrons down the chain in an energy-yielding tumble .. Oxygen is used at the very END •The energy yielded is used to regenerate ATP

Pb(OH)₂ + HCl → H₂O + PbCl₂

Pb(OH)₂ + 2HCl → 2H₂O + PbCl₂

ClO4 (-1 charge)

Perchlorate

MnO4 (-1 charge)

Permanganate

O2 (-2 charge)

Peroxide

PO4 (-3 charge)

Phosphate

3 types of visible scars

Pitted scars, Dermal contraction, keloid

what is the test for chlorine

Placing a piece of damp litmus paper into a test tube containing a gas and seeing if it turns from blue to white

Cations

Positive ions.

what is the anode

Positively charged electrode where oxidation takes place

reactivity series

Potassium Sodium Lithium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Hydrogen Copper Silver Gold

KMnO4

Potassium permanganate

what is the test for hydrogen

Put a lit splint where the gas is and if there's a squeaky pop, hydrogen is present.

what is the test for oxygen

Putting a glowing splint into a test tube containing a gas and if it relights oxygen is present

P₄O₁₀ + H₂O → H₃PO₄

P₄O₁₀ + 6H₂O → 4H₃PO₄

Pseudofolliculitis barbe

Razor bumps, Ingrown hairs

Reduction

Reaction with gain of electrons.

Oxidation

Reaction with loss of electrons.

oxidizing agent

Reduced

Gain of electrons by atoms or ions Loss of oxygen

Reduction

Oxidation or Reduction Shift of electrons toward an atom in a covalent bond (Gain of hydrogen)

Reduction

Does reduction occur at the anode or cathode?

Reduction occurs at the cathode. Reduction is the gain of electrons.

Delta A

Regulates the activity of £ & B

Electrodes

Rods that carry electric current to and from the electrolyte.

Why during the extraction of aluminium from aluminium oxide, do the anodes need to be replaced during ?

Since the positive electrodes are made of carbon they get corroded by the oxygen forming carbon dioxide and so must be replaced every few weeks

Concentrated acid

Small amount of water, lots of acid

Are acid-base reactions redox reactions?

Sometimes, they can be.

Are single-replacement reactions redox reactions?

Sometimes, they can be.

Ex redox reaction

Start out with a molecule name josh. he has some electrons that he's going to give to tran.. he just lost an electron and became *oxidized tran gained an electron so she became *reduced This situation allowed them to transfer energy by transferring electrons.. some energy did get lost in the transfer could be used in the cells to do other reactions now tran is going to give the electrons to daisy.. she became oxidized and daisy just got electrons so she just became reduced.. once again, in the transfer.. energy was lost so the energy could be used to do some type of work such as generate ATP or heat

If a substance gains electrons readily it is known as a...?

Strong oxidizing agent

Glycogen

Sugar stored in the muscle & liver converted to glucose (source of energy)

SO4 (-2 charge)

Sulfate

S₈ + O₂ → SO₃

S₈ + 12O₂ → 8SO₃

How do you turn ADP back to ATP?

Take the energy released in the reactions, from the electrons in the Redox reaction to use its molecules and reattach phosphate back into ADP and turn it back into ATP.. use the same energy that was broken off and through cellular respiration, turn it back into ATP The process of cellular respiration

What does cell respiration mean?

The cell is exchanging gases. It takes in oxygen from air and release C02 To do cellular respiration, we are going to oxidize glucose, break off all of the hydrogen and use it to generate ATP

Electrolyte

The compound that conducts electricity when molten and breaks down during electrolysis.

In compounds, the oxidation number corresponds with what?

The element's position in the periodic table.

Why can molten ionic compounds be electrolysed?

The ions can move freely and conduct electricity

What is phosphorylation

The process of adding phosphate back onto ADP to turn it into ATP

What is electrolysis?

The process of splitting up a chemical compound into its elements by the passage of an electric current.

Rule 4 for oxidation number

The sum of all the oxidation numbers of the elememts in a radical is equal to the charge on the ion

Rule 3 for oxidation number

The sum of all the oxidation numbers of the elements in a compound is zero

Our body heat that we generate on a daily basis ultimately comes from?

The sun

Titration

The use of volume measurements to solve for concentrations, often of unknown substances.

Sn (+4 charge)

Tin (IV)

SnCl4

Tin (IV) Chloride

Acids that contain three ionizable hydrogens

Triprotic

True or False Oxidation reactions are the principal source of energy on Earth

True

True or False Some atoms have several possible oxidation numbers.

True

Inert conductor

Unreactive conductor that won't interfere with the electrolysis.

Give 2 uses for sodium hydroxide

Used to make soap Manufacture bleach (with chlorine)

How much NAD we have at one time?

Very limited amount. because it is a co enzyme, it needs to get regenerated. While a NADH is carrying a hydrogen, it cannot pick up another one. It needs to get rid of it to restart the process

smallest living organisms, contains dna structures and requires a target host for reproduction

Virus

V₂O₅ + CaS → CaO + V₂S₅

V₂O₅ + 5CaS → 5CaO + V₂S₅

Why do we have to harvest energy in a metabolic pathway

We cannot produce it because our bodies would have to go through a combustion reaction.. we are unable to do that because it would make us burn up. We have to harvest our energy instead in a metabolic pathway

Why are humans called an aerobic organism instead of an anrobic organism?

We need oxygen to do metabolic pathway Anrobic can do the pathway without the need of oxygen

how are aqueous solutions formed

When solutes are dissolved in the solvent water

How does ATP release energy?

When the third phosphate group of ATP is removed by hydrolysis, a substantial amount of free energy is released.

When do we use ADP vs ATP?

When we don't need as much energy for a reaction

Iron(III) salts colour change

Yellow to pale green

Is the corrosion of metal a redox reaction?

Yes

Can ADP be used as an energy molecule?

Yes. you can break off the next phosphate and turn it into AMP Adenosine monophosphate

What happens when NADH pass the electron through electron transport chain?

You started out as NADH because you were reduced, once you passed the electron to another you became NAD again (oxidized)

The sum of individual oxidation numbers of all the atoms in a formula must equal...?

Zero

Zn + HCl → ZnCl₂ + H₂

Zn + 2 HCl → ZnCl₂ + H₂

Consider the half reactions below for a chemical reaction. Zn--->Zn2+(aq)+2e- Cu2+(aq)+2e---->Cu(s) What is the overall equation for this chemical reaction?

Zn(s)+Cu2+(aq)--->Zn2+(aq)+Cu(s)

Consider the redox reaction below. Zn(s)+2HCl(aq)--->ZnCl2(aq)+H2(g) Which half reaction correctly describes the oxidation that is taking place?

Zn(s)---->Zn2+(aq)+2e-

ZnSO₄ + Li₂CO₃ → ZnCO₃ + Li₂SO₄

Oxidizing agents

[organic redox] agents that have high affinity for electrons (O2, O3, Cl2) or unusually high electron states (Mn7+, Cr6+)

nitrogen dioxide

a highly poisonous brown gas (NO2)

what forms at the anode

a non metal other than hydrogen

The molecule that functions as the reducing agent in a redox reaction will...

a reducing agent is the donor (oxidation i lose --giving electrons away).. this makes it loses electrons and loses potential energy

titrant

a solution of known concentration and volume

analyte/titrand

a substance that has a known volume but an unknown concentration

In cellular respiration, the C02 carbon dioxide released is considered what?

a waste we exhale

According to Bronsted-Lowry, a base is an H+ _____

acceptor

According to Lewis, an acid is an electron-pair_____

acceptor

According to Lewis, an acid (accepts/donates) a pair of electrons during a reaction

accepts

A solution with a pOH >7

acidic

Below 7

acidic

Strong acid + Weak base = _________ solution

acidic

Type of solution in which [H+] is greater than [OH-]

acidic

2 stages of bacteria life..

active phase: vegetable, reproductive, and dormant phase: non vegetable, non-reproductive

how to calculate the titre

add the values of the volume of acid added to the burette (excluding the rough volume) and divide by the number of readings taken

Basic solutions are also known as ______ solutions

alkaline

Over 7

alkaline

This acid is associated with protein

amino acid

Name the buffer system involving amm-

ammonium ion-ammonia

A substance can act as both an acid and a base is said to be ___________

amphoteric

NAD is

an electron acceptor or electron carrier As we're stripping the electrons off the molecules such as glucose, NAD is going to carry it

The process in which you take the CO2+H20 and used its energy to build organic molecules is what type of process?

anabolic (taking smaller molecules, used some energy to build larger molecules)

A salt consists of an ____ of an acid and a ____ of a base

anion, cation

which electrode does oxidation take place

anode

in electrolysis which direction do the electrons travel

anode ➔ cathode

where is the reading taken

at the bottom of the meniscus

__C + __O₂ --> __CO₂

balanced

__CaO + __H₂O --> __Ca(OH)₂

balanced

__Cu +__Cl₂ --> __CuCl₂

balanced

A solution with a pOH < 7

basic

Type of solution in which [H+] is less than [OH-]

basic

Weak acid + Strong base = ________ solution

basic

Why do anodes need to be replaced regularly?

because they are made of graphite (carbon) and this reacts with the oxygen to produces carbon dioxide

What are the high energy bonds in ATP

bond between the second and third (last bond) phosphates is commonly described as a "high-energy" bond and is depicted in the figure by a wavy red line

The amount of acid or base that can be added to a puffer solution before a significant change in pH occurs

buffer capacity

How do Catabolic pathways yield energy?

by oxidizing (combined chemically with oxygen) organic fuels .. "catabolic pathways yield energy by oxidizing organic fuels" because transferring electrons from an organic molecule to an oxygen molecule is commonly termed "oxidizing" process is catabolic/destructive and yields storage energy

Name the buffer system involving ca--

carbonic acid-hydrogen carbonate ion

The process of cellular respiration is what type of process?

catabolic process .. takes the large organic molecules and some oxygen.. breaks them down to release energy and waste products

which electrode does reduction take place

cathode

Cellular respiration is what type of process? Photosynthesis is what type of process?

cellular respiration is the catabolic process photosynthesis is the anabolic process

electrolysis of calcium chloride is performed: what is formed at the anode

chlorine

what are the 4 ions that are present in a copper sulphate solution

copper ions, sulphate ions, hydrogen ions and hydroxide ions

what would happen during the electrolysis of copper sulphate solution

copper will be produced at the cathode and oxygen will be produced at the anode from the hydroxide ions (seen by bubbling)

Some redox reactions do not transfer electrons but change the electron sharing in

covalent bonds. An example is the reaction between methane and O2

things that affect treatment

dermatitis/ eczema, cold sores, moles, or anything raised dont treat

Which is an important step in the alternate method for balancing equations in redox reactions?

determining the half reactions of chemical equations

Name the buffer system involving dihy--

dihydrogen phosphate ion-hydrogenphosphate ion,

what is spread through bacteria

dipheria and typhoid

According to Lewis, an base (accepts/donates) a pair of electrons during a reaction

donates

According to Bronsted-Lowry, an acid is an H⁺______

donor

According to Lewis, a base is an electron pair _______

donor

In cellular respiration, we are transferring?

electron-- which is energy

When we are harvesting energy out of a molecule, we are pulling apart that molecule's?

electrons (electrons hold energy therefore when you're harvesting energy, you're pulling apart the electrons)

The point of neutralization is the _____ point of the titration

end

The point at which the indicator changes color is the ______ _______ of the titration

end point

The moving of an electron from oxidation to reduction is transferring..

energy. This released energy is ultimately used to synthesize ATP

When an acid and base are mixed, the ____________ _________ is when the number of moles of hydrogen ions equals the number of moles of hydroxide ions

equivalence point

The break down of organic molecules is?

exergonic, this means that energy is being released

If it is a reduction, I will..

gain an electron (negative charge) and reducing the positive charges

Reduction

gain of electrons

reduction

gain of electrons

Which of the following statements describes the results of this reaction? C6H12O6 (Glucose) + 6O2 --> 6CO2 + 6 H2O + Energy

glucose is oxidized and oxygen is reduced When glucose is oxidized, carbon dioxide, water and energy are produced.

why are electrodes made from graphite (3)

graphite is insoluble in water, has high melting and boiling points and can conduct electricity

In a respiration reaction, what are the 2 key components?

he oxidation of glucose. this means glucose (sugar) is combined with oxygen to produce carbon dioxide, water and energy

Viral infection is

herps= cold sores, flat warts

Basic solutions have a pH ____ than

higher

shallow insertion causes

higher % of over treatment, HF blow out and % of re growth increases

HCO3 (-1 charge)

hydrogen carbonate (bicarbonate)

HPO4 (-2 charge)

hydrogen phosphate

HSO4 (-1 charge)

hydrogen sulfate (bisulfate)

When we break down glucose to get its energy.. we essentially want its?

hydrogens

Aside of carry electrons, NAD will also carry?

hydrogens .. ex: in glucose C6H12O6 .. NAD can carry 12 H

A water molecule that gains a hydrogen ion becomes a positively charged _________

hydronium ion

Conjugate acid of the base water (what ion?)

hydronium ion

A base is a source of ______________ ions

hydroxide

The number of moles of hydrogen ions provided by an acid are equivalent to the number of _________ ions provided by the base

hydroxide

Equations can be balanced by using the half-reaction method. Which step should be completed immediately after finding the oxidation states of atoms?

identifying the half reactions

what happens at the anode during the electrolysis of solutions

if OH‐ ions and halide ions are present, molecules of chlorine, bromine or iodine form if no halide ions are present the hydroxide ions are discharged and oxygen will be formed

A valuable tool for measuring pH because its acid form and base have different colors in solution

indicator

An acid or a base that undergoes dissociation in a known pH range

indicator

The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the (long name)

ion-product constant for water

Acids are classified as strong or weak depending on the degree to which they ___ in water

ionize

what ions are present in an aqueous solution

ions from the ionic compound, hydrogen ions and hydroxide ions

ionise

ions in a compound split up when in water

electrometallic phenomenon

is a chemical injury belongs to blend and galvanic electrolysis

bacteria: prokaryoctic

is a single celled, vegetable in nature, grow by the thousands to form a mass called a colony

What can the energy that is lost during a redox reaction be used as ?

it can be used in the cell to do other reaction such as generate ATP, or as heat

what is a disadvantage of using electrolysis to extract a metal from its ore

it's expensive as lots of energy is required to heat the ionic compound

During electrolysis what do you understand by the term 'discharge'?

lose its charge, become neutral

Oxidation

loss of electrons

why is cryolite used in the electrolysis of aluminium oxide

lower melting point

bacterial: Non-pathogenic

majority, useful, helpful, necessary

pH scale

measurement system used to indicate the concentration of hydrogen ions (H+) and hydroxide ions in a solution; ranging from 0 to 14

Define molten?

melted by heat

Neutralisation of dilute acids with bases - metal oxide (3rd acid equation)

metal oxide + acid --> metal salt + water CuO + H2SO4 --> CuSO4 + H2O

For precise and continuous measurements, what sort of device would you use to measure the pH of a substance?

meter

bacteria: pathogenic

minority, 100% disease, harmful

concentration of solution units

mol/dm-3

what happens to the negative ions during electrolysis and where does it happen

move towards the anode and lose electrons so they are oxidized

what does MSS stand for

muscular skeletal symptoms

An electron donor, otherwise known as the reducing agent is giving away..

negative (electrons) if he is giving someone a negative, he is reducing them.. this makes him the reducing agent

What type of salt produces a basic solution? One that contains ________ ____ _____ _______ ____________ _____ __________

negative ions that attract protons from water

Salts that produce basic solutions contain (negative/positive) ions that attract (neutrons, protons, electrons)

negative, protons

In a reduction, you are gaining an electron.. this actually means you are gaining..

negativity.. Why? because electrons are negatively charged.. In a negative charge, it reduces a positively charged molecule. *You are gaining an electron that reduces positive charged molecules.

Strong acid + Strong base = ______ solution

neutral

Any aqueous solution in which [H+] and [OH-] are equal is described as a _______ ________

neutral solution

You can determine the concentration of acid (or base) in a solution by performing a __________________ reaction

neutralization

Reactions in which an acid and a base react in an aqueous solution to produce a salt and water are called

neutralization reactions

Nitric acid forms

nitrate salts

Example of monoprotic acid (name)

nitric acid

Does plants produce more than one organic molecule?

no- it can produce glucose, lipids, proteins, oils

In cellular respiration, does glucose get turned into ATP?

no. energy stored in glucose is used to REGENERATE ATP.. glucose does not turn into atp, we only use the energy to turn it into ATP

Type of acid in DNA and RNA

nucleic acid

the complete or partial loss of electrons or the gain of oxygen

oxidation

a positive or negative number assigned to an atom according to a set of arbitrary rules

oxidation number

the balancing of a redox reaction by comparing the increases and decreases in oxidation numbers

oxidation-number-change method

the chemical changes that occur when electrons are transferred between reactants

oxidation-reduction reactions

substance in a redox reaction that gains electrons Contains the atoms that are reduced

oxidizing agent

NAD+ functions as an_____during cellular respiration.

oxidizing agent, also an electron acceptor

The electron acceptor in a redox reaction is called the ____________? During the course of the reaction it becomes ____________.

oxidizing agent; reduced

Cellular respiration consumes___ and yields ____

oxygen and organic molecules ATP

-log[H+] =

The __ of a solution is the negative logarithm of the hydrogen-ion concentration

-log[OH-] = ___

pOH

The ____ of a solution equals the negative logarithm of the hydroxide-ion concentration

pOH

____ = 14 - pH

pOH

pH = 14 - ___

pOH

Example of triprotic acid (name)

phosphoric acid

What is the opposite of a respiration?

photosynthesis-- the reverse process of respiration, combing carbon dioxide and water to make sugar 6CO2 + 6H2O + light energy >>> C6H12O6 + 6O2

Salts that produce acidic solutions contain ________ ions that release protons to water

positive

What type of type of salt produces an acidic solution? One that contains ________ ____ _____ _______ ____________ _____ __________

positive ions that release protons to water

According to Arrhenius, a base is an OH- _____

producer

According to Arrhenius, an acid is an H⁺________

producer

what are the three types of scabs

pus crust, blood crust, honey crust=lymph crust=eschar

bacterial: Boil

pus pocket

pseudofolliculitis barbe

razor bumps, ingrown hairs

another name for an oxidation-reduction reaction

redox reactions

the electron donor?

reducing agent

the substance in a redox reaction that gives up electrons Contains the atoms oxidized

reducing agent

The electron donor in a redox reaction is called the ____________? During the course of the reaction it becomes ____________.

reducing agent; oxizidized.

the complete or partial gain of electrons or the loss of oxygen

reduction

NADH

represents stored energy that is "trapped" to synthesize ATP

fungal infection is

ringworm and candida

Compounds consisting of an anion from an acid and a cation from a base

salt

In general, the reaction of an acid with a base produces and ______

salt

In this process, the cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water

salt hydrolysis

The reaction in which water molecules produce ions is called

self-ionization

miss pone

sharp pain and bleeding, higher % of infection, petechiae

what is another name for Herpes zoster

shingles, chicken pox, small pox, cow pox

Weak acids have ____ Ka values

small

K2SO4 (potassium sulfate)

soluble

these ions do not change oxidation number or composition during a reaction

spectator ions

bacterial: folliculitis

staph and pustules

bacterial: impetigo

staph and strep

___ bases dissociate completely into metal ions and hydroxide ions in aqueous solution

strong

Our waste products are the plant's The plant's waste products are our

substrate substrate

Fermentation is a partial degradation (break down) of?

sugars that occurs without oxygen

edema

swelling, blood serum, blood vessels widen

which electrode do the negatively charged ions move towards

the anode

which electrode does the positive ion go towards

the cathode (negative electron)

what is the cathode

the electrode at which reduction occurs

heparin and heparoids aid in what

the healing process, bleeding, and bruising

why can't a solid ionic compound be electrolysed

the ions are fixed in position and are not free to move, therefore can't carry charge

Which cation (metal or hydrogen) gets discharged during electrolysis of an aqueous solution?

the least reactive

The entire reaction of cellular respiration is...

the oxidation of glucose in order to form carbon dioxide and water (loses an hydrogen during oxidation..) oxidation refers to i lose an electron electrons in this case are associated with hydrogens Electrons are basically pulling all of the hydrogens off

what is electrolysis

the splitting up of an ionic compound using electricity

How to decide which solution is more concentrated in a titration

the substance that requires less volume to neutralise the other substance is more concentrated

what happens when ions gain or lose electrons at the electrode

they are discharged and form neutral atoms

what happens to the positive ions during electrolysis and where does it happen

they gain electrons so they are reduced at the cathode

Where does NADH pass the electrons?

through the electron transport chain

The process of adding a known amount of solution of known concentration to determine the concentration of another solution is called

titration

why is a trial run taken during a titration

to get a rough estimate of what volume is required o

What is the purpose of finding oxidation states in the half-reaction method for balancing equations?

to identify the half reactions for the equation

True or false: A buffer solution is better able to resist drastic changes in pH than is purse water

true

True or false: not all solution are neutral

true

Most heat resistant bacteria in the world

tuberculosis TB

how are viruses observed

under an electronic microscope

O oxidation number

usually -2, -1 in peroxide (H2O2)

Which anion (OH- or halide) gets discharged during electrolysis of an aqueous solution?

usually the halide ion (unless very dilute)

___ acids ionize only slightly in aqueous solution

weak

____ bases react with water to form the hydroxide ion and the conjugate acid of the base

weak

A buffer is a solution of a ____ acid and on of its salts, or a solution of a ____ base and one of its salts

Quizlet Chemistry Comp, Electrolysis (IGCSE), Electrolysis - IGCSE, Chemistry - Electrolysis, Electrolysis, Oxidation, Oxidation Numbers, Balancing oxidation-reduction equations, Redox Reactions, Redox Reaction, Balancing Chemical Equations, Balancin...

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ap classroom questions unit 1

ch. 3

ACCT Chapter 12

Chapter 2 review (Fundamentals of Nursing)

Dsom 6 adaptive prac.

CHAPTER 17 MICRO

Evolution MC