Unit 3: Ch 8, 10, 11 - Definitions & Equations Flashcards
covalent bonds are _ + _
nonmetals + nonmetals
covalent bonds in molecules are the sharing of
electrons between 2 ATOMS
A single bond is the sharing of
Length and strength:
2 bonding electrons; (1 pair)
longest and weakest
A double bond is the sharing of
Length and strength:
4 bonding elections; (2 pairs)
medium
A triple bond is the sharing of
Length and strength:
6 bonding elections; (3 pairs)
shortest and strongest
Intramolecular interactions are
inside molecules
Intermolecular interactions are
rhyme; inter-vene
between molecules
Electronegativity is the
The highest is
ability of an atom to attract electrons to itself
F!!!
An ionic interaction is the
Transfer of electrons
A polar covalent bond is the
Unequal-sharing of electrons
A nonpolar covalent bond is the
Equal-sharing of electrons
Bond polarity is found by the
difference between the 2 electronegativity values
Nonpolar molecules shapes are
slide 41
Symmetrical shape (NO lone pairs on central atoms with the exterior atoms all the SAME)
Polar molecules shapes are
slide 41
- Symmetrical geometry (NO lone pairs) with different exterior atoms all the SAME
- ANY combination of atoms with a NONsymmetrical geometry (lone pairs)
Dipole-Dipole Forces are present in (polar/nonpolar) molecules
polar
ionic compounds are _ + _
metal + nonmetal
Hydrogen bonding is (strength)
Present ONLY between molecules with _, _ and _ bonds
VERY STRONG
N-H, O-H, H-F bonds
London Forces are present in
Everything
Heat of Fusion is the
amount of heat needed to melt or freeze 1 g of a substance
Heat of Vaporization is the
amount of heat needed to boil/condense 1 g of a substance
Heat of Sublimation is the
same for sublimation and deposition
Equation for Heat of Fusion
Q = m•Hf
Equation for Heat of Vaporization
Q = m•HV
For the heating curve Q1 is Q2 is Q3 is Q4 is Q5 is
Q1 - ice melting Q2 - ice melting into water Q3 - water heating Q4 - water boiling into steam Q5 - steam heating
For the heating curve the equations for: Q1 = Q2 = Q3 = Q4 = Q5 =
Q1 = mCpΔT Q2 = mΔHfus Q3 = mCpΔT Q4 = mΔHvap Q5 = mCpΔT
Dilute concentration is
solution that contains a small amount of solute
Concentrated concentration is
solution contain a lot of solute
Concentration is
the amount of solute present in a given amount of solvent or solution
Percent by Mass =
% by mass = mass solute/mass solution • 100%
Volume Percentage =
volume % = volume solute/mass solution • 100%
Molarity =
Molarity = moles solute/moles solution
M=n/v
Equation for dilution of solutions
C1V1=C2V2
Ion-dipole forces
the interactions between ions and the dipoles of a polar molecule (like H2O)
Ionic compound dissolving:
O (δ-) attracted to [charge] ions
H (δ+) attracted to [charge] ions
O (δ-) attracted to + ions
H (δ+) attracted to - ions
MISCIBLE mixtures of 2 molecular (covalent) liquids are
two liquids that mix (solute and solvent)
e.g. alcohol and water
IMMISCIBLE mixtures are
two liquids that DO NOT mix
e.g. oil and water
Solubility is
maximum amt of solute that dissolves in a certain amount of solvent at a specific temperature
Polar compounds (dissolve/dissolve poorly) in water Nonpolar compounds (dissolve/dissolve poorly) in water
Polar compounds dissolve in water (because of dipole-dipole attractions)
Nonpolar compounds dissolve POORLY in water
Solubility of solids/liquids
(increase/decrease) with (increasing/decreasing) temperature
Solubility of solids/liquids
increase with increasing temperature
Solubility of solids/liquids
are (affected/unaffected) by pressure
Solubility of solids/liquids
are unaffected by pressure
Solubility of gases
(increases/decreases) with (increasing/decreasing) temperature
Solubility of gases
decreases with increasing temperature
Solubility of gases
(increases/decreases) with (increasing/decreasing) pressure
Solubility of gases
increases with increasing pressure
Ionization is
dissolving SOLUBLE ionic compounds in WATER
Electrolyte is a
compound that when dissolved causes the solution to conduct electricity
A strong electrolytes conductivity is _
(High/low) # ions when dissolved
(High/low) concentration (#M) of ion
A strong electrolytes conductivity is good
High # ions when dissolved
High concentration (#M) of ion
A weak electrolytes conductivity is _
(High/moderate/low) # ions when dissolved
(High/moderate/low) concentration (#M) of ions
A weak electrolytes conductivity is good
Moderate # ions when dissolved
Moderate concentration (#M) of ions
A nonelectrolytes conductivity is _ #_ ions when dissolved
Insignificant
NO IONS WHEN DISSOLVED
Colligative property is a
These properties are only for
Property that depends on the amount of particles in a solution (solute particles)
These properties are only for SOLUTIONS
Adding a solute (increases/decreases) the vapor pressure
Higher # solute particles or higher #M = (higher/lower) vapor pressure
Adding a solute decreases the vapor pressure
Higher # solute particles or higher #M = lower v.p. (less escaping)
The higher # solute particles or higher #M = (higher/lower) Boiling Point
Higher # solute particles or higher #M = higher b.p.
e.g. salt added to water for pasta
The higher # solute particles or higher #M = (higher/lower) Freezing Point
Higher # solute particles or higher #M = higher f.p.
e.g. salting the roads
Osmotic pressure (Π) is
Water flows from the _ to _ side
if pure water and dissolution are separated by a semipermeable membrane
Water flows from the solvent to solution side
Higher # solute particles or higher #M = (higher/lower) Π
Higher # solute particles or higher #M = higher Π
Isotonic solutions are
solutions with the SAME Π as another solution
Hypotonic solutions have
lower Π than a particular solution
Hypertonic solutions have
higher Π than a particular solution
Collision theory is
the assumption that chemical reactions are caused by the collisions of molecules
Collisions with: High temperature = _ reactions High concentration = _ reactions Large particles = _ surface area More surface area = _ reactive Larger the particles = _ reaction
High temperature = faster reaction High concentration = faster reactions Large particles = small surface area More surface area = more reactive Larger the particles = slower reaction will proceed
A reversible reaction is
Generally take place in _ phase
a reaction where both the forward (forming products) and backward (reforming reactants) rxns are possible
Generally take place in the SAME phase
Increase pressure, shift to _ moles of gas
Increase pressure, shift to FEWER moles of gas
Decrease pressure, shift to _ moles of gas
Decrease pressure, shift to MORE moles of gas
Rxns that have a change in temperature are _ and _ is a product
Exothermic and HEAT is a product
Equilibrium constant Keq =
Keq =
[C]c[D]d/
[A]a[B]b
