Unit 9 Flashcards by daria behrens

Hydrogen Bonding

water is highly attracted to itself (cohesion), due to the hydrogen atom being attracted to the oxygen atom of other water molecules.

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Surface Tension

the property of the surface of a liquid that allows it to resist an external force fur to the cohesive nature (attraction to itself) of its molecules

water has a strong surface tension that allows it to form almost completely spherical droplets

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Boiling Point (Heat of Vaporization)

water requires more energy to break its hydrogen bonds before it can boil and reach its heat of vaporization

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Boiling point of water

100°C

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Vaporization

the point when a liquid changed to a gas

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Cohesion

like molecules attract each other, stick to each other (intermolecular forces)

water molecules are very cohesive because of the molecule’s polarity

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Adhesion

the attraction of water to other materials

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Capillary Action

the movement of water within the spaces of a porous material due to the forces of adhesion, cohesion, and surface tension

occurs because water is “sticky”, thanks to the forces of cohesion (water stays together) and adhesion (water is attracted and stick to other substances)

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Properties of Water

-Hydrogen Bonding
-Surface Tension
-Boiling Point and Heat of Vaporization
-Cohesion and Adhesion
-Capillary Action

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Electrolyte

a compound that conducts an electric current when it is dissolved in water or melted

has freely moving ions when dissolved

all soluble ionic compounds are electrolytes

when ionic compounds dissolve, they break apart into ions, which are then able to conduct a current

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Strong Electrolyte

a solution in which almost all of the dissolved solute exists as ions

-strong acids (7)
-strong bases (8)
-soluble salts

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Strong acids

HCl
HSO4
HI
HNO3
HBrO3
HBr
HClO4
HClO3

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Strong bases

LiOH
NaOH
KOH
RbOH
CsOH
Ba(OH)2
Sr(OH)2
Ca(OH)2

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Weak Electrolyte

a solution in which only a small fraction of the dissolved solute exists as ions

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Most common weak base

Ammonia

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Weak acids

Acetic acid
CH3COOH

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Non-electrolyte

a compounds that does not conduct an electric current in either aqueous solution

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Common non-electrolytes

Sugar
Ethanol

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What does water do to IONIC compounds?

water will separate the compound into its positive and negative ions (cations and ions)

dissociation

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Dissociation

a chemical reaction where a compound breaks into two or more components

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Solvation

the process in which water surrounds ions to dissociate them

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Like Dissolves Like

Polar solvents dissolve polar solutes
Non-polar solvents dissolve non-polar solutes

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Polar Structures

A-symmetrical

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Non-Polar Structures

Symmetrical

Electronegativity

the ability of an atom to hold its electrons and to attract electrons to form ionic or covalent bonds increases bottom-top, left to right on the periodic table as atomic radius increases, more space between electrons and other atoms who want those electrons, making them more safe, increasing electronegativity

Fluorine

most electronegative element

Polar Covalent Bond

created when the shared electrons between atoms are not equally shared when one atom has a higher electronegativity than the atom it is sharing with atom with higher electronegativity will have a stronger pull for electrons shared electrons will be closer to the more electronegative atom dipole moment is created, net dipole points in the direction of more electronegative atom

Non-Polar Covalent Bond

created when atoms share their electrons equally usually occurs when two atoms have similar or the same electron affinity NO DIPOLE MOMENT NET DIPOLE OF ZERO

Dipole Moment

represents the polarity of a molecule, indicating how much positive and negative charge is present on different parts of the molecule

Net Dipole

when there is an overall partial positive charge on one end of the molecule and a partial negative charge on the other end of the molecule

Lewis Structures

structures that use a line to show the bond and link formed between atoms in the compound

Drawing Lewis Structures

-count total valence electrons -identify central atoms -connect atoms with single bonds -place remaining electrons as lone pairs -check for octets and adjust if necessary

Central atom rules

-Atom with lowest subscript, and can form most bonds -C is ALWAYS central atom -H is NEVER central atom

Soluble Compounds

-Compounds containing alkali metal ions and ammonium -Nitrates -Bicarbonates -Chlorates -Halides (except when paired with Ag, Hg, and Pb) -Sulfates (except when paired with Ag, Ca, Sr, Ba, Hg, and Pb)

Insoluble Compounds

-Carbonates -Phosphates -Chromates -Sulfides -Hydroxides (except when paired with Ba) Exceptions: -Compounds containing alkali metal and ammonium

Soluble Compounds rhyme thing

C (chlorates) A (acetates) S (sulfates) H (Halides) N (Nitrates) G1 (G1 metals) A (Ammonium) Exceptions: -Sir Angel Campos Peanut Butter Hugger (Sr, Ag, Ca, Pb, Ba, Hg with a sulfate is insoluble) -HAPpy Halides (Hg, Ag, Pb with a halide is insoluble)

Insoluble Compounds rhyme thing

C (Chromates) C (Carbonates) O (Hydroxides) P (Phosphates) S (Sulfides) Exceptions: -G1 metals, ammonium -Barium with hydroxide is soluble

Molarity Equation

M = n/v

Dilution Equation

M1V1 = M2V2

a solution that has a large amount of solute compared to it's solvent (too sweet lemonade)

Concentrated

states that gases under pressure remain dissolved in solution better than those not under pressure

Henry's LAW

the inability of a liquid solute to dissolve in a liquid solvent (oil + water)

Immiscible

a solution that has a very small amount of solute compared to solvent (watered-down lemonade)

Diluted

a homogenous mixture made of two or more metals (copper + zinc)

Alloy

the ability of a liquid solute to dissolve in a liquid solvent (ethanol + water)

Miscible

concentration of a solution expressed in the number of moles per liter of solution M = n/L

Molarity

the inability of any solute (no matter its state of matter) to dissolve in a solvent

Insoluble

the ability of any solute (no matter its state of matter) to dissolve in a solvent

Soluble

the amount of solute that will dissolve in 100g of water at a specific temperature

Solubility

water is known as this because of the large number of solutes that can be dissolved in it

Universal Solvent

the substance that dissolves in the solvent and exists in smaller quantities

Solute

another name used to describe the concentrated solution used when diluting

Stock Solution

a solution that is no longer able to dissolve more solute because it already has the maximum amount of solute

Saturated

a solution that can still dissolve more solute in its solvent

Unsaturated

the substance that causes the solute to dissolve and exists in a larger quantity

Solvent

a solution that specifically uses water as its solvent

Aqueous Solution

the process of surrounding solute particles with solvent particles to form a solution

Solvation

a chemical reaction where a compound breaks up into two or more components

Dissociation