Test 2 content Flashcards by Andrea Pedraza-Heakin

solids in which the atoms, ions, or molecules are arranged in a definite repeating pattern

crystalline solids

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a liquid that freezes before its molecules become arranged in an orderly pattern ( noncrystalline solid)

amorphous solids

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_________ solids lack internal structure and are randomly arranged

amorphouse

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_______ solids: positive and negative ions that are held together by electrostatic attractions

ionic

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What are the characteristics of Ionic solids

1.) high mp/ bp
2.) hard but brittle
3.) solids do not conduct electricity

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_____ solids: uniform distribution of atomic nuclei within a “sea” of delocalized electrons

metallic

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What are the characteristics of metallic solids?

1.) high thermal and electrical conductivity
2.) metallic luster
3.) malleability
4.) mp and bp vary

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______ ______ solid: the atoms are held together by a network of covalent bonds

covalent network

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What are characteristics of covalent network solids?

1.) hard
2.) strong
3.) high melting points

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_____ solids: are composed of neutral molecules

molecular

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What are the three crystal defects?

1.) vacancies
2.) interstial sites
3.) doping

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______: defects that occur when positions that should have atoms or ions are vacant

vacancies

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_______: defect where atoms and ions occuring in irregular space in lattice structure

interstitial sites

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______: defect where atoms and ions substitute other ions/ atoms in the lattice structure

doping

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_______: homogenous mixtures of 2 or more substances

solution

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________: the component in a mixture with greater concentration

solvent

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_______: the component in the mixture with the lesser component

solutes

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______: a solid solution of one metal dissolved in another

alloy

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What are the characteristics of a solution?

1.) homogenous
2.) physical state of solution same as solvent
3.) components of a solution are dispersed on a molecular scale
4.) dissolves solute in a solution will not separate from the solvent
5.) the composition of a solution can be varied continuously

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________: occurs without input of energy

spontaneous process

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What two things can make a process spontaneous process?

1.) a decrease in the internal energy of the system
2.) an increased dispersal of matter in the system

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______ solution: solution is formed with no accompany energy

ideal

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What are the three types of intermolecular attractive forces?

1.) solute-solute
2.)solvent- solvent
3.) solute- solvent

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________: stepwise process in which energy is consumed to overcome solute-solute and solvent-solvent attracting and released which solute-solvent attractions are established

solvation

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________: substance that when dissolved in water yeild ions in solutions

electrolytes

_______: substance that when dissolved do not yield ions

nonelectrolytes

T or F: as ion concentration increase, electrical conductivity increases

True

__________ attraction: the electrostatic attraction between an ion and a molecule with a dipole

ion-dipole

_____: the process of when ionic compounds dissolve in water, the ions the solid separate and disperse uniformly throughout the solution because water molecules surround and solvate the ions, reducing the strong electrostatic forces between

dissociation

______ _______: conduct electricity because the solute molecules react chemically with the solvent to produce

covalent electrolytes

______: the maximum concentration that may be achieved under given conditions when the dissolution process is at equilibrium

solubility

______: solute's concentration equals its solubility

saturated

________: solute's concentration is less than solubility

unsaturated

______: solute concentration exceeds its solubility

supersaturated

With solutions of gases in liquids, how does temperature affect solubility?

When temperature increases the gas solubility decreases

With solutions of gases in liquids, how does partial affect solubility?

When partial pressure is high, gas solubility is high

What is the equation for gas solubility in relation to pressure of the gas?

Cg= kPg

What is Henry's law?

the quantity of an ideal gas that dissolves in a definite volume of liquid is directly proportional to the pressure of the gas

When does Henry's law have deviations?

When a chemical reaction takes place between the gaseous solute and the solvent

_______: mixed in any proportions to yield solutions

miscible

______: two liquids that do not mix to appreciable extent

immisicible

What is the equation for molality (m)?

mol solute/ kg solvent

What is the equation mole fraction?

Xa = mol A/ total mol of all components

What is the equation for molarity?

mol solute/ L solution

What two equations are not dependent on temperature?

molality and mole fraction

What are the colligative properties?

1.) vapor pressure 2.) boiling point elevation 3.) freezing point depression 4.) osmotic pressure

When a nonvolatile substance is dissolved into a volatile liquid the _______ _________ decreases because surface area decreases so evaporation decreases

vapor pressure

What is the law that is with vapor pressure lowering?

Raoult's law

What is Raoult's law?

the partial pressure exerted by any components of an ideal solutions to equal to the vapor pressure of the pure component multiplied by its mole fraction in the solution

What is the equation of Raoult's law?

Pa = XaP*a

_______: occurs when gases have significantltly different vapor pressures

distillation

When a nonvolatile substance is dissolved into a volatile liquid the ________ _______ increases because it requires more kinetic energy to evaporate

boiling point

_______ pressure is the pressure required to stop the movement of solvent molecules across a semipermeable membrane due to osmosis

osmotic pressure

What is the equation for osmotic pressure?

n (pie)= MRT

______ _____ factor: the ratio of solute particles to the number of formula units dissolved

van't Hoff factor

__________ bond between molecules (physical properties)

intermolecular

_________ _______: interactions between nonpolar molecules

london dipersion

T or F: in london dispersion IMFs larger molecules are favorable because there are more electrons

True

____-_______ ______: an atomic ion interacting with a nonpolar molecule

Ion-induced dipole

Why do Ion-induced dipole interactions occur?

the electric field of the ion distorts the electron cloud of the nearby nonpolar molecule, temporarily inducing a dipole

____-_____ dipole interaction is where a polar and nonpolar molecule interact

dipole- induced

Why does a dipole-induced dipole interaction occur?

The polar molecule, which a permanent dipole, interacts with a nonpolar molecule, causing the electron cloud to shift and create a temporary dipole

______-______ interaction is where two polar molecules interact.

dipole-dipole

_____-_____ interaction is where a polar molecule and ion interact

ion-dipole

What does the strength of an IMF depend on?

the distance between molecules and the magnitude of the dipole

true or false: larger ions have weaker IMFs

true

If IMFs increase, vapor pressure ______

decreases

If IMFs increase, boiling point and melting point _______-

increase

if IMFs increase, surface tension _______

increase

What is surface tension?

the energy required to increase the surface area of a liquid due to cohesive forces between its molecules

______ forces are the intermolecular forces that attract like molecules to each other.

cohesive

what is the equation for density?

p= m/v

What is viscosity?

a measure of a liquid's resistance to flow or how thick and sticky it is.

What interactions hold ionic solids together?

the electrostatic attractions between oppositely charged ions

What type of interactions are in the molecular solids?

London dispersion

What are the interactions between covalent network solids?

covalent bonds

_________: interact strongly w/ solvent

lyophilic

________: interact weakly with solvent

lyophobic

What are the four different types of surfactants?

1.) anionic 2.) cationic 3.) nonionic 4.) amohoteric

What are the strong acids?

HCl, HBr, HI, HNO3, H2SO4, HClO4, HClO3,

What are the strong bases?

NaOH, KOH, Ca(OH)2, Ba(OH)2, Sr(OH)2

solid in a solid is

solid sol

solid in a liquid is a

sol

gas in a solid is a

solid aerosol

liquid in a solid is a?

gel

liquid in a liquid is a

emulsion

gas in a liquid is a

liquid aerosol

gas in solid is a

solid foam

gas in liquid is a

foam