Unit 5 Key Terms, Concepts, and Solubility Flashcards by Brashe Webster

Solutes

Spread evenly throughout the solution
Cannot be separated from the solvent by filtration
Can be separated by evaporation
Are not visible, but can give a color to the solution

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The angle between the H’s in H2) is

104.5 degrees

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crystal lattice

An orderly 3-D arrangement of positive and negatice ions

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insolubility

When the pull of water molecules is not strong enough to overcome the attractions among the ions, the ionic compound will not dissolve.

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Solubility

When the pull of water molecules is strong enough to overcome the attractions among the ions, water can start to pull the crystal apart. The compound will dissolve.

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strong electrolytes

Dissociate in water resulting in separate positive and negative ions in the solution

Conduct an electric current in water

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Nonelectrolytes

Dissove as intact molecules in water
Do not produce ions in water
form solutions that do not conduct an electric current

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like dissolves like

polar solvents (water, low fw alcohols) dissolve polar compounds and often ionic compounds
Nonpolar solvents (hydrocarbons) dissolve nonpolar compounds
Oil(nonpolar) and water (polar) don't mix

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metathesis reactions

double-replacement reactions
involve a trading of ion partners
Are driven by:
--The formation of precipitates
--The formation of a molecular liquid(usually water)
--The formation of a molecular gas

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Precipitation reactions

Metathesis reactions that result in the formation of an insoluble solid(precipitate) in the reaction

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solibility

a physical property describing how readily a substance will dissolve in a given solvent

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soluble compounds

Nitrate salts
acetate salts
chlorate and perchlorate
chloride, bromide, and iodide salts (except those containing silver, Lead II, or Mercury I Ions(Hg2^2+)
Sulfate Salts-(except those containing calcium, strontium, barium, mercury I, or Lead II Ions.

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Insoluble Compounds

Carbonate (CO3) salts (except those containing alkali metal or ammonium Ions)
Phosphate salts – except those containing alkali metal or ammonium ions
Sulfide salts – except those containing ammonium, alkali metal, calcium, strontium, or barium ions
Hydroxides  except those containing ammonium, alkali metal, calcium, strontium, or barium ions

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Gas-Forming Compounds

Carbonic acid and sulfurous acid are unstable. If a metathesis reaction produces one of these acids, the acid quickly decomposes.
H2CO3(aq)  H2O(l) + CO2(g)

H2SO3(aq)  H2O(l) + SO2(g)  Na2CO3(aq) + 2 HCl(aq)  2 NaCl(aq) + H2O(l) + CO2(g) not  Na2CO3(aq) + 2 HCl(aq)  2 NaCl(aq) + H2CO3(aq)

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When given two reactants and no products for a possible precipitation reaction, you have to ;

Determine the formulas of the products
Use the solubility rules to predict the states of the products
Balance the equation if a reaction occurs
Write Nrxn if both products are water soluble

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What writing product formulas, always show the ___ in the formulas first

Cations

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Molecular Equation

When cations and anions of ionic compounds are shown together forming neutral units

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Ionic Equations (Total Ionic Equations or Complete Ionic Equations)

WHen an Ionic compound dissolves, and the individual ions will be separated from each other and be surrounded by water molecules. They show soluble ionic compounds and strong acids separated into the ions they contain

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Spectator Ions

Ions not involved in making new products

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Net Ionic Equation

When spectator Ions are taken out of an equation

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When a compound starts with H, it’s an _____ when dissolved in water.

Acid

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The number of Hydrogens in an acid equals the negative charge on the _____

Anion

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HCl

Hydrocholoric Acid

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HBr

Hydrobromic Acid

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Hydroiodic Acid

HNO3

Nitric Acid

H2SO4

Sulfuric Acid

HClO4

Perchloric Acid

HClO3

Chloric Acid

Ca(OH)2

Calcium Hydroxide

Sr(OH)2

Strontium Hydroxide

Ba(oh)2

Barium Hydroxide

Acids and bases neutralize each other to produce a

Salt (any ionic compound that is not a hydroxide or oxide)

All bases must have

an atom that has at least one nonbonding pair of electrons. | The nonbonding pair of electrons is used to form the new bond with H+

HCl (Name, Acid/Base, Strong/Weak)

Hydrochloric Acid | Strong Acid

HBr (Name, Acid/Base, Strong/Weak)

Hydrobromic Acid | Strong Acid

HI (Name, Acid/Base, Strong/Weak)

Hydroiodic Acid | Strong Acid

HClO3 (Name, Acid/Base, Strong/Weak)

Chloric Acid | Strong Acid

HClO4 (Name, Acid/Base, Strong/Weak)

Perchloric Acid | Strong Electrolyte

HNO3 (Name, Acid/Base, Strong/Weak)

Nitric Acid | Strong Acid

H2SO4 (Name, Acid/Base, Strong/Weak)

Sulfuric Acid | Strong Acid

HF(aq) (Name, Acid/Base, Strong/Weak)

Hydrofluoric Acid | Weak Acid

H3PO4 (Name, Acid/Base, Strong/Weak)

Phosphoric Acid | Weak Acid

HC2H3O2 (Name, Acid/Base, Strong/Weak)

Acetic Acid | Weak Acid

Alkali Metal (1A) Hydroxides

Strong Bases

LiOH (Name, Acid/Base, Strong/Weak)

Strong Base | Lithium Hydroxide

NaOH (Name, Acid/Base, Strong/Weak)

Sodium Hydroxide | Strong Base

KOH (Name, Acid/Base, Strong/Weak)

Potassium Hydroxide | Strong Base

RbOH (Name, Acid/Base, Strong/Weak)

Rubidium Hydroxide | Strong Base

CsOH (Name, Acid/Base, Strong/Weak)

Cesium Hydroxide | Strong Base

Ca(OH)2 (Name, Acid/Base, Strong/Weak)

Calcium Hydroxide | Strong Base

Sr(OH)2 (Name, Acid/Base, Strong/Weak)

Strontium Hydroxide | Strong Base

Ba(OH)2 (Name, Acid/Base, Strong/Weak)

Barium Hydroxide | Strong Base

NH3 (Name, Acid/Base, Strong/Weak)

Ammonia | Weak Base

NaHCO3

Sodium Hydroxide Baking Soda Weak Base

Reactions between acids and bases are called

Neutralization Reactions

Salt

any ionic compound whose cation comes from a base and whose anion comes from an acid

General Formula for a Salt

acid + metal hydroxide →a salt + water

Neutralization reactions are a type of

Metathesis reaction

What is the net Ionic equation for any strong acid and a strong base?

H+(aq)+ OH-(aq)→H2O (l)

Bases that do not contain hydroxide which react with acids to form gases

Na2S NaCN NaHCO3

When H2CO3 is listed as a product of a reaction, it is further broken down into

H2O(l) and CO2 (g)

Oxidation-Reduction (re-dox reaction)

Electrons are transferred from an element in one reactant to an element in another reactant

Example of a redox reaction

Corrosion of your car battery terminal is caused by a reaction between the metal terminal, oxygen, and the battery acid, H2SO4.

Oxidation

The loss of electrons (chemical Species becomes more positively charged) or has an increased oxidation #

Reduction

The gain of electrons (Chemical Species becomes more negatively charged) through the loss of oxygen or a decrease in oxidation #

Oxidation #s are used

to keep track of electrons gained and lost during redox reactions.

Oxidation Number

hypothetical number assigned to an individual atom present in a compound using a set of rules. May be positive, negative, or zero

Oxidation numbers are always reported as

individualatoms or ions not groups of atoms or ions!!!!!!!!!!! 

For an atom in its elemental form, the oxidation number is always

Zero

H2 Oxidation Number

For a monatomic Ion, the Oxidation number is the same as the

Charge

K+ Oxidation#

Cl- Oxidation #

-1

S2- Oxidation#

-2

Group 1A Cations' Oxidation Numbers are always

Group 2A Cations' Oxidation Numbers are always

Hydrogen's Oxidation# when Bonded to a nonmetal

Hydrogen's Oxidation# when bonded to a metal or B

-1

Oxygen's Oxidation # in a peroxide

-1

Oxygen's Oxidation# in all compounds except peroxides?

-2

Fluorine's Oxidation# in a compound is always

-1

The sum of the oxidation numbers of all atoms in any chemical species (ion or neutral compound) is equal to

the charge on that chemical species

A forest fire is an example of what type of reaction

Redox | combustion

Corrosion of iron is an example of what type of reaction

Redox

A Charcoal grill is an example of what type of reaction?

Combustion | Redox

Natural gas burning is an example of what type of reaction

Redox | Combustion

Batteries are an example of what type of reaction?

Redox

Metabolic Processes are an example of what type of reaction

Redox

displacement reaction

The reaction between a metal and an acid or between a metal and a metal salt

Mg(s)+ 2HCl (aq)→MgCl2(aq)+ H2(g) | What type of reaction?

Displacement reaction

How to determine if a Redox reaction has occurred

If the oxidation number changes, then a redox reaction has occurred

Oxidizing Agent

The reactant that causes another reactant to be oxidized | The reactant that contains the element that was reduced

Reducing Agent

The reactant that causes another reactant to be reduced | The reactant that contains the element that was oxidized.

Metals differ in the ease with which they are

Oxidized

Activity Series

A list of metals arranged in order of decreasing ease of oxidation Used to predict whether a metal will react with an acid or with a metal salt

Concentration

the amount of solute dissolved in a given quantity of solvent or solution

Concentration Units

(%, ppm, g/L, etc)

Concentration is often expressed as

Molarity

the number of moles of solute per liter of solution

Units of Molarity

Moles/L

Steps involved in preparing solutions from pure solid

Calculate the amount of solid required Weigh out the solid Place in an appropriate volumetric flask Fill flask about half full with water and mix. Fill to the mark with water and invert to mix.

Dilution Equation

M1x V1= M2x V2

Steps involved in preparing a dilute solution from a more concentrated stock solution.

Calculate the volume of stock solution needed. Pipet the required amount of stock solution into an appropriate volumetric flask. Dilute to the mark with DI water. Mix well.

Concentration of an acid can be determined using a process called

titration

Titration

reacting a known volume of the acid with a known volume of a standard base solution (i.e. a base whose concentration is known)

Unit 5 Key Terms, Concepts, and Solubility Flashcards

(106 cards)