Science 25 LAB

Non-polar substances

-Toluene -Benzene

Polar solvent examples

-Water -Alcohol

Water surrounding dialysis bag

-barium ion present -positive for chloride ion -Starch present Conclusion small ions such barium 2+ and chloride ions easily travel through semi permeable membrane. And colloidal such as starch solution 1% does not cause its larger

Content of dialysis bag

-barium ion present -positive for starch -positive chloride ion

Silver Nitrate to test for Chloride Ion

-forms AglCl percipitate -white solid precipitated -suspension solution

Inside Dialysis Bag

-mixure of collidal solution: starch 1% -true solution: Barium Chloride, barium 2+ion and chloride CL-ion -Homogeneous mixture

Cu + 2AgNO³➡️2Ag + Cu(NO³)²

-single replacement -silver Nitrate being dissolved -copper source of electrons that will turn silver ions into silver electrons. -aqueous -does not react as fast -bluish color liquid -Pure silver solid is form -Product silver and Copper to Nitrate

moles of HCl

0.02095

2CO2 (gas)

2 carbon dioxide molecules

3O2 (gas)

3 Oxygen molecules

3H2O (liquid)

3 water molecules

Procedure to see how many moles of hcl react with tablet.

50ml of HCl -bubbles developed -5mL sodium hydroxide -boil tablets for 2 mins to get rid of all the co2 -add penaphile and then add sodium hydroxide to change color purple.

Molarity

A common measure of solute concentration, referring to the number of moles of solute per liter of solution.

Solid

A form of matter that has a definite shape and volume

Solvent

A liquid substance capable of dissolving other substances

Potential of Hydrogen (ph)

A measure of the acidity or alkalinity of a solution

Heterogeneous Mixture

A mixture in which different materials can be distinguished easily

homogeneous mixture

A mixture in which substances are evenly distributed throughout the mixture

Solution

A mixture of a solute in a solvent.

Endothermic reaction

A reaction in which energy is absorbed. -takes in heat colder outside

Exothermic Reaction

A reaction that releases energy in the form of heat -release heat colder inside than outside. example freezing and condensation

Titration

A solution of known concentration is used to determine the concentration of another solution.

liquid

A state of matter that has no definite shape but has a definite volume.

Gas

A state of matter with no definite shape or volume

Compound

A substance made up of atoms of two or more different elements joined by chemical bonds

Single Replacement reaction

A+BC➡️AC+B a chemical change in which one element replaces a second element in a compound

Alkanes

Alkanes have no functional groups.

2NH4SCN (s)

Ammonia Thiocyanate

Universal indicator

An indicator with a different colour for each pH value.

Hoffman meter

Apparatus used in lab to separate out the H2 and O2 gases from water

Suspensions

Are mixtures of finely divided substances in a suspending medium.

Frequency +light

Blue light has a higher frequency than red light.

Light+energy

Blue light has more energy than red light

Ca(O2C2H3)² (aqueous, saturated)

Calcium acetate

Ca2

Calcium ion (aq)

2H2O2 + KI ➡️ O2 + 2H2O

Catalyst reaction -catalyst potassium iodine - more production of oxygen -bubbles - faster reaction

clues that a chemical reaction has taken place

Color Change. Production of an odor. Change of Temperature. Evolution of a gas (formation of bubbles) Precipitate (formation of a solid)

CH3CH2OH + 3O2 ➡️ 2CO2 + 3H2O

Combustion reaction -creates heat and light when spark -produces CO2 and H2O

True Solutions

Contains small molecules and ions -Homogeneous mixture

Cu

Copper -good conductor

2Cl (aq)

DICHLOROPHENYL)ACETIC ACID

2PbO2 ➡️ 2PbO +O2

Decomposition reaction -releases oxygen- flame reignites. - color changed from black to orange.

2H² + O²➡️2H²O

Dihydrogen Monoxide -combination reaction -when combined with hydrogen gas from the balloon; hydrogen gas is a great source of energy, it forms a new substance water H2O when a little jolt of energy is added (heat.) -fire explosion -aqueous -loud noise -

AgNO3 + NaCl ➡️ AgCl + NaNO3K

Double Replacement reaction - Silver Nitrate and Sodium Chloride -silver Nitrate reacting with sodium Chloride. -2 cations AG+ and Na+ exchanged anions -produces AgCL(silver Chloride) (white percipitate.) and sodium Nitrate. -sodium Nitrate is soluble in water thats why you do not see it. -solid

2AgNO3 + K2CrO4 ➡️ Ag2CrO4 + 2KNO3

Double Replacement reaction -Produces silver chromate and potassium Nitrate -percipitate red color -solid - potassium Nitrate dissolved in water because its a soluble substance.

2 NaHCO3 + H2SO4 ➡️ Na2SO4 + 2H2CO3 ⬇️ H2O + CO2

Double replacement reaction -double displacement reaction because sodium changes places with hydrogen ion and forms a sodium sulphate, and carbonic acid. Which is unstable so as a result decomposes right into water and CO2 gas. -

Heat + Ba(OH)2 + 2NH4SCN ➡️ 2NH4OH + Ba(SCN)2

Endothermic Reaction -takes energy from surrounding -droplet got frozen -heat sucked in droplet got frozen as a result

CaCl2 (s) ➡️ Ca2 + 2Cl

Exothermic Reaction

Ca(O2C2H3)² + CH3CH2OH> sterno (flammable)

Gel formation (not a reaction, its a physical change) -creates gel -gel use to make sterno - burns slowly - flammable

Carbon-in the form of Charcoal change Carbon dioxide.

Glow Amber -like a fire cracker

noble gases

Helium, Neon, Argon, Krypton, Xenon, Radon

2H²

Hydrogen Peroxide

2NH4OH (aq)

Hydroxide

Water and Chloroform

Immiscible

Dialysis process

In the dialysis process solution particles are separated from colloidal particles by means of a selectively permeable membrane. -colloidal particles do not pass through a membrane. - The principle of dialysis is very important in hemodialysis in an artificial kidney machine, where certain body wastes that are dissolved in the blood are removed. -simple filtration method -semi permeable membrane

Galvanometer

Instrument used for measuring very small electrical currents

Geiger Counter

Instrument used to detect the emitted beta particles.

Iodine+Solutions

Iodine passes through the bag's semi-permeable membrane and turns Starch blue-black.

Ionic+polar substances

Ionic or polar substances dissolve in polar solvents.

Solute

Is the substance that is dissolved or goes into solutions.

2PbO2 (s, black)

Lead dioxide

2PbO (solid, orange, ppt)

Lead monoxide lead(II) Oxide

2Mg+O²➡️2MgO

MAGNESIUM OXIDE combination reaction -forms a white powder -example of an oxidation reaction reduction. -example of combination reaction. -forms a bright white/UV light -shiny turns white solid ​

2Mg

Magnesium Ion

metals+oxygen

Many Metals react with Oxygen to form compounds call oxides. example: iron reacts with oxygen to form iron(III) OXIDE (RUST)

Metalloids

Metalloids will also react with oxygen. Silicon forms silicon dioxide, the main component of sand, when reacts with oxygen.

Metals and No Metals with Oxygen

Metals are Basic Non- metals are acidic.

Alcohol and Chloroform

Miscible

water and ethanol/alcohol

Miscible

Why do we use Antacids

Neutalize Hydrochloric Acid in Stomach -active ingredient is CaCo3(s) Calcium carbonate. CaCO3 + CaCl2➡️ CaVl2 + H2O + CO2

Non polar+covalent

Non polar covalent substances dissolve in non polar solvent

Phosphorus ph

Orange 5

Downward displacement of water

Oxygen is collected by a method of downward displacement of water.

Oxygen

Oxygen is the most abundant element on the Earth's surface. -Earth's Atmosphere contains 21 Percent by volume of Oxygen -water bodies contains about 89% by weight of Oxygen -Earth's crust predominantly made of silica (silicone dioxide)

silicone dioxide (SiO2).

PHYSICAL PROPERTIES Main component of sand when react with oxygen brown grainy/granule Solid -when heated no color change - Sand did not change physical or chemical change

Sodium Nitrat (NaNo3)

PHYSICAL PROPERTIES -white -granule/solid -when under flames it turns liquid -liquid bubbles into gas -wooden splint reignites so there is oxygen being released

Lead Oxide (IV) PbO2

PHYSICAL PROPERTIES Black powder color changed from black to orange or a red- brown - there is oxygen being released -solid

Magnesium Oxide (MgO)

PHYSICAL PROPERTIES White powder use to make brick NO PHYSICAL CHANGE

Potassium Chlorate (KCIO3)

PHYSICAL PROPERTIES white powder -change to liquid when heated. - releases oxygen -creates like a little rocket

2KNO3 (aqueous)

Potassium Nitrate

Red Phosphorus

React with Oxygen change to P4O10 - small solid forms - bright flame

Wavelength+light

Red light has longer wavelength than blue light.

2AgNo3 (aqueous)

Silver Nitrate

2AgNO³

Silver Nitrate -colourless

2 NaHCO3 (aqueous)

Sodium Bicarbonate

Solutions+temperature

Solutions boil at a temperature that is higher than the normal boiling point of the pure solvent, and freeze at a temperature that is lower than the freezing point of the pure solvent.

Solute

Substance being dissolved

Product

The chemical composition of the result of the reaction.

Solute+temperature of solvent

The present of a solute affects the boiling point and freezing point of the solvent.

Visible Light(Tyndall Effect)

True Solutions-no light path Colloidal- red light beam

Phenolphtalein Indicator

Turn pink if the environment is basic -clear if acidic

Trough

Water bath

Test to see if iodine goes through semi permeable membrane

Yes iodine as a molecule travel though semi permeable membrane -the boiling water surrounding the dialysis bag prove that none of the starch came out because it did not turn blue.

Everytime use molarity

You have to use LITERS. ​

Zn

Zinc

combination reaction

a chemical change in which two or more substances react to form a single new substance. A+B➡️AB ​

combustion reaction

a chemical reaction that occurs when a substance reacts with oxygen, releasing energy in the form of heat and light 2H2(g) + O2(g) ➡️ 2H2O(g) ​

decomposition reaction

a reaction in which a single compound breaks down to form two or more simpler substances AB ➡️ A + B

oxidation-reduction reaction

a reaction in which electrons are transferred from one reactant to another

double replacement reaction

a reaction in which the positive and negative ions of two ionic compounds exchange places to form two new compounds. AB + CD➡️ AD + CB

synthesis reaction

a reaction in which two or more substances combine to form a new compound

Simple filtration

a simple technique used to separate solid particles from suspension in a liquid solution.

suspension solution

a solution in which particles settle (sediment) -heterogeneous mixture -Usually precipitate

aqueous solution

a solution in which water is the solvent

saturated solution

a solution that cannot dissolve any more solute under the given conditions

supersaturated solution

a solution that holds more dissolved solute than is required to reach equilibrium at a given temperature

dioxide

an oxide containing two atoms of oxygen in the molecule

relative proprotions

balance equations indicates the relative proportion of each reactant and product.

Ba(OH)2 (s)

barium hydroxide

Ba(SCN)2 (aq)

barium thiocyanate

Magnesium

bluish purple

Boiling water 100 degrees celcius

boiling point of water elevated to 103.5 after adding sodium Chloride

pure solven

by50mL salt (sodium Chloride)solution used to depress the freezer point. was 1.5 now negative 1

CaCl2 (s)

calcium chloride

Reagents

chemical substances known to react in specific ways; used to detect or synthesize other substances in chemical reactions

Immiscible liquids

combinations of liquids that are incapable of mixing with, or dissolving in, each other

Diatomic

consisting of two atoms

super saturated solution

contains more dissolved solute than a saturated solution at the same temperature

O²

dioxygen

Negative beta particle

electron

CH3CH2OH (ethanol)

ethanol

CH3CH2OH (liquid)

ethanol (ethyl alcohol)

PROPERTIES OF OXYGEN

gas (colorless, odorless, tasteless), slightly heavier than air, slightly soluble in water, does not burn but will support combustion. Oxygen is a highly reactive element.

Noble Metals

gold, silver, platinum -they don't like to react

Soulution

homogeneous mixture in which one substance is evenly mixed with another substance

H2 (gas)

hydrogen gas

2H2O2 (liquid)

hydrogen peroxide

Sulfuric Acid to test for Barium ion

if barium ion is present it will form barium suphate SOLID. -white precipitation

water and toluene

immiscible

Acidic pH

less than 7 -colors: red,orange,yellow.

Miscible liquids

liquids that dissolve freely in one another in any proportion

Conservation of mass

mass cannot be created or destroyed

Triangle in Reaction

means that heat applied

Alcohol and Toluene

miscible

Chloroform and toulene

miscible

Colloidal Dispersions

mixtures containing particles larger than normal solutes but small enough to remain suspended in the dispersing medium. -Colloids do not settle out on standing.

Molarity formula

moles of solute/liters of solution

Alkaline pH/Basic

more than 7 colors:green, blue, purple

Iron ph

neutral

Ph 7 is neutral

neutral

Carbon ph

neutral 7 Sea green

percipitation reaction

occur when cations and anions in aqueous solution combine to form an insoluble ionic solid called a precipitate.

Particle of light

photon

K2CrO4 (aqueous, yellow)

potassium chromate

KI (s, white)

potassium iodide

Sulfur

react with oxygen -forms SO2 and SO3 gases -sulfur loves oxygen, bright flame when react with oxygen

Iron-steel wool

react with oxygen. -burns bright

Sulfur ph

red

AgCl

silver chloride

Ag2CrO4 (solid, red)

silver chromate

AgNO3

silver nitrate

Zn + H²SO⁴➡️ZnSO⁴ + H²

single replacement reaction (zinc sulphate) -bubbles (could be hydrogen gas, could be oxygen gas or Co2 gas.) -produce Hydrogen gas. Made a pop sound. If it was oxygen splint would be reignite. If it was Co² gas it would extinguish the flame which is one reason why Co² is in fire extinguishers. ​

Saturated clear solution saturated solution of sodium Acetate crystals make it supersaturated

sodium Acetate crystals added fast growth of crystals

NaCl

sodium chloride (salt)

NaNO3

sodium nitrate

Na2SO4 (aqueous)

sodium sulfate

colloidal solution

solution containing larger molecules, but not as large as suspension. -Homeogenus mixture

catalyst reaction

speed up a reaction by reducing the activation energy or changing the reaction mechanism ​

H2SO4 (aqueous)

sulfuric acid

H²SO⁴

sulfuric acid

Gel Formation

the formation of a gel with cooling of a gelatinized starch paste

Organic chemistry

the molecules that are predominantly made of carbon and hydrogen -occasionally oxygen, nitrogen, sulfur.

Reactants

the number and kinds of the interacting substances

chemical reaction

the process by which one or more substances change to produce one or more different substances

Oxide

the product of the reaction of oxygen with a non metal is an oxide.

instantaneous speed

the speed of an object at one instant of time. -Speedometer shows instantaneous speed.

Solvent

the substance in which the solute dissolves

oxidize

to combine with oxygen; to rust

Iodine test for starch

turns blue/black

Molecule

two or more atoms held together by covalent bonds

stoichiometric coefficients

types of numbers written infront of atoms, ion and molecules in a chemical reaction to balance them.