- london dispersion forces - dipole-dipole interactions - hydrogen bonding

- resistance of liquid to flow - increases with stronger IMF and decreases with higher temperature

Exam 1 Flashcards by Paloma Loera

kinetic energy increases as the temp _______

increases

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condensed phases are which states of matter

solid and liquid

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INTRAmolecular forces

covalent bonds (strong)
H — O for example

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INTERmolecular forces

IM attraction (weaker)

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this is much weaker than chemical bonds (intra)

intermolecular forces
Example:
evap. of water, I.F. breaks but intramolecular O-H bond (covalent) remains

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van der waals forces

london dispersion forces
dipole-dipole interactions
hydrogen bonding

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london dispersion forces

present in all molecules primarily NONPOLAR molecules
due to polarziability (e- cloud distorting – electrostatic attraction)

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factors that affect LDF

molecular weight (larger molecule = stronger dispersion)
larger electron cloud atoms
molecule shape

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long skinny molecules have _____ dispersion forces than short fat ones

stronger

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dipole-dipole interactions are

molecules w/ permanent dipoles attracted
opposite charges attract
important only when molecules are close together

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d-d forces increase with ____

increasing polarity

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(d-d forces) the more polar the molecule (similar size) the _____ its boiling point

higher !

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hydrogen bonds happen when hydrogen covalently bonds to what…

(F.O.N.) electroneg. atoms
- fluorine
- oxygen
- nitrogen

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ion-dipole interactions responsible for what

dissolution of ionic substance in polar solvent/solvation

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ion-dipole interactions important in solutions with ____

ions

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no ions present
no polar molecules present
Which IMF?

LDF

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no ions present
polar molecules ARE present
no H atom to F.O.N. bonds

dipole-dipole forces

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no ions present
polar molecules ARE present
H atom covalently bonded to F.O.N.

hydrogen bonding

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ion (cation/anion) and polar molecule
NaCl dissolving in H2O

ion-dipole forces

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if 2 molecules are similar in size/shape… ______ will be dominating forces

dipole-dipole forces

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if 1 molecule is much larger than another molecule ____ will be dominating

LDF

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rank lowest to highest boiling point (polar, nonpolar, ionic, h-bonding)

lowest
- nonpolar
- polar
- h-bonding
- ionic
highest

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viscosity

resistance of liquid to flow
increases with stronger IMF and decreases with higher temperature

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viscosity: more _____ (bonds)= more resistance

hydrogen bonds

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exothermic phase changes:

- condensation - freezing

endothermic phase changes:

- vaporization - melting/fusion - sublimation (solid to gas)

heat of fusion

solid to liquid

heat of vaporization

liquid to gas

heat of sublimation

solid to gas

at a given temp, the weaker the IMF in the liquid, the _____ the vapor pressure is

HIGHER

types of solids

- metallic - ionic - covalent-network - molecular

crystalline solids

atoms are arranged in a very regular pattern

amorphous solids

lack of order in the arrangement of atoms EX: glass, rubber

crystal lattices:

- primitive cubic lattice - body-centered cubic lattice - face-centered lattice

primitive cubic lattice

- lattice points at 8 corners (1/8) - 1 atom per unit cell

body-centered cubic lattice

- lattice points at 8 corners PLUS 1 atom at center - total: 2 atoms per unit cell

face-centered cubic lattice

- lattice points @ 8 corners (1/8), 6 faces (1/2) - total: 4 atoms per unit cell

what are alloys, majority are?...

combo of two or more elements, majority are metals

examples of alloys

- yellow brass - bronze - stainless steel - sterling silver

substitutional alloys

second element takes place of a metal ion

interstitial alloy

second element fills space in lattice of metal atoms (steel FeC)

example of substitutional alloy

Au (gold) + Ag (silver!!!) = STRONGER GOLD

interstitial alloy example

C (carbon!!!) + Fe (iron) = STRONGER

elemental samples of nonmetals and metalloids bonding: what type of bond?

covalently

metals have a ____ __ _____ electrons, this allows them to form ____ groups of atoms that _____ electrons among themselves

- dearth of valence - large - share

metals having dearth of valence electrons allows them to be better ________

conductors

ionic solids facts

- high melting and boiling point - hard and brittle - poor !!! conductors

metallic solids facts

- low to very high melting point - soft to hard - excellent !!! conductors

molecular solids facts

- low to mod. melting point - soft - poor !!! conductors

covalent network solids facts

- very high melting point - very hard - often ... poor !!! conductors

amorphous solids facts

- no sharp melting point - soft to hard depending on temperature - poor !!! conductors

covalent ntwk solids are what?

- bonding to multiple neighboring atoms - crystalline solid where atoms bond in continuous network of covalent bonds

solution is ...

homogenous mixture of solvent and solute

a solute can be separated by ____

evaporation

solute cannot be separated from solution by ___

filtration

an aqueous solute will not ___ ___ to a solution

give color

Molarity M= ______

moles of solute/L of solution

Molality m= ______

moles of solute/kg of solvent

mass % = _____

(mass of component in soln/total mass of soln) x 100

ppm or ppb= ____

(mass of component in soln/total mass of comp.) x 10^6 ppm or 10^9 ppb

mole fraction of component= ____

moles of comp/total moles of ALL comps

how does a solution form?

the solvent pulls solute particles apart and surrounds (solvates) them

endothermic:

- takes heat ^H+

exothermic:

- releases heat ^H-

separation! of solute particles is ....

endothermic

separation! of solvent particles is...

endothermic

new! interactions between solute and solvent are...

exothermic

solubility of alcohol in water

each has one O-H bond, however the more CH bonds you add, the less soluble in water (soluble in water: methanol, ethanol, propanol)

solubility of alcohol in hexane (C6H14)

same as solubility in water except reversed, methanol is not as soluble in hexane for having the least CH

ionic comp. endo: solubility _____ with temperature

increases, this is most all ionic compounds

ionic comp. exo: solubility _____ with temperature

decreases

gases in solution/temp do what? (solubility) decrease or increase with temp…

decreases with temperature

Henrys Law !!!

C (small A) = k P (small A)

Finding P (1 or 2) Calsius equation

ln(P2/P1) = e^ (-Hvap/R)(1/T2-1/T1)

Finding T (1 or 2): Calsius equation

T2: [1/T1 - ( R•ln(p2-p1) / Hvap )]^ -1

Finding Hvap: calsius equation

Hvap= -R • ln(p2/p1) / (1/T2 - 1/T1)

Exam 1 Flashcards

(76 cards)