the force of attraction or repulsion between two charged particles is directly proportional to the product of the charges and inversely proportional to the distance between them. F = (kq1q2)/dˆ2
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As an electron moves away from the nucleus it's potential energy...
..increases
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what is special about transition metal ions?
they lose electrons from the s sublevel before d
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isometric
same electron configuration (K+, Cl-, S2-, Ar)
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periodic groups are...
...columns, # of electrons in outer shell
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periodic periods are...
...rows, # of shells
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transition element properties
conductive, malleable, for ions with variety of positive charges, act as good catalysts, often form colored compounds, form variety of alloys
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valence electrons
outermost electron ring (highest energy level)
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core electrons
\n all non valence electrons
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effective strength formula
proton # - # core electrons = strength of + on valence e-
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electronegativity/electron affinity
how much an element will attract electrons. increases (+ charge increases) across the periodic table, and decreases (greater atomic radii) descending
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ionization energy (IE)
energy required to remove an electron. increases across (+ charge increases) and decreases descending periodic table (more barriers)
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Evaporation is endothermic or exothermic
endothermic, need to GIVE it heat
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cation
positive, metal
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anion
negative, non-metal
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Order of IMFs (least to greatest)
Disperson, dipole-dipole, hydrogen
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Trigonal pyramidal
4 e- pairs, 3 bonds, 1 lone pair
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Tetrahedral
4 e- pairs, all bonds
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Octahedral
6 e- pairs, all bonds, x,y,z
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Trigonal planar
3 e- pairs, all bonds, flat
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Linear
2 e- pairs, all bonds, a line
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Bent
4 e- pairs, 2 bonds, 2 lone pairs, angle
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Water's normal boiling point is 100˚C, why can water evaporate at 20˚C?
Because of random velocities of water molecules causing some to have a high enough kinetic energy to escape from the surface.
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What havens to water vapor pressure in a container with ice melting at room temp?
Increases rapidly, then more slowly until reaching equilibrium
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What happens to the rate of condensation?
Increases until it equals the rate of evaporation and then remains constant.
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What are the affects of temp, IMFs, and molar mass on the vapor pressure of a substance?
Vapor pressure increases with an increase in temp and a decrease in strength of IMFs and molar mass.
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When, in general, does a liquid begin to boil?
\n When the vapor pressure equals the outside pressure
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Why does ice have a lower density than water>
**than water>**
**Because of the crystal structure formed by hydrogen bonds and its open structure.**
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hydrogen bonds occur when hydrogen is bonded to which elements
F, O, N
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kinetic molecular theory
gas molecules are in constant random motion, when they collide energy is not lost, do not attract each other, far apart, same temp, same average kinetic energy
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kinetic energy formula
KE=1/2mvˆ 2
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pressure and force formula
p=f/a
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Formula for pressure, volume, and temp
pv/t = pv/t
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Dalton's law of partial pressures
Since gas pressure depends on # of molecules not their mass or size, it is easy to see that each gas in a mixture contributes pressure according to the number of molecules present.
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Graham's Law
small particles diffuse faster
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˚ C to K
\+273
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atm to mmHg
atm x 760
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How do gasses exert pressure?
Tiny molecules colliding with every pinhead-sized area of any surface. # of collisions is identical, forces add up for exert a force on the whole surface, creating a uniform "pressure".
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Which is larger: proportional more collisions or harder collisions
samsies
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mole to liter (for gasses)
1 mol = 22.4L
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molar mass
g/mol
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particles / mol
6\.02x10ˆ 23
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Relative atomic mass
average atomic mass of all isotopes based on how common they are: (mass(%)+mass(%))/100
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percent composition by mass
mass/total mass
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density=
m/v
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molarity
mass of solute per solution: moles of solute/liters
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Flashcard (96)